Elements & the Periodic Table

Transcription

1 Elements & the Periodic Table Learning Guide Visit for Online Learning Resources. Copyright NewPath Learning

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3 Table of Contents Lesson 1 - Introduction to Elements... Pause & Review - Parts of an Atom... 7 Lesson - Classes of Elements... 8 Pause & Review - Classes of Elements... 1 Lesson - The Periodic Table of Elements Pause & Review - The Periodic Table of Elements Lesson - Groups on the Periodic Table... 0 Pause & Review - Groups on the Periodic Table... 8 Lab Investigation - Flame Test... 9 Key Vocabulary Terms... Vocabulary Review... Assessment Review... 6 Assessment... 9 Assessment Key... 1 NGSS Correlations... Phone: Fax: NewPath Learning Products are developed by teachers using research-based principles and are classroom tested. The company s product line consists of an array of proprietary curriculum review games, workbooks, charts, posters, visual learning guides, interactive whiteboard software and other teaching resources. All products are supplemented with web-based activities, assessments and content to provide an engaging means of educating students on key, curriculum-based topics correlated to applicable state and national education standards. Copyright MMXIII NewPath Learning. All Rights Reserved. ISBN Printed in the United States of America. 1

4 Lesson 1 Introduction to Elements Elements An element is a pure substance that cannot be separated into simpler substances. This means an element is a substance made entirely of one type of atom. For example, every atom in a piece of copper is the same. Gold Silver Sulfur Carbon (coal) Iron Copper Copper atom Scientists have identified 90 elements that occur naturally in our universe. Some elements you might recognize include oxygen, iron, and calcium. H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Sc 1 Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium Periodic Table of the Elements state at room temperature solid gas liquid not found in nature V Vanadium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Cr Chromium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium Mn 5 Manganese Tc Technetium Re 75 Rhenium Bh 107 Bohrium Fe 6 Iron Ru Ruthenium Os 76 Osmium Hs 108 Hassium Co 7 Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds Cu 9 Copper Ag 7 Silver Au 79 Gold 111 Rg Zn 0 Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 16 S Sulfur Se Selenium Te 5 Tellurium 8 8 Bi Bismuth Po Polonium 116 Lv Livermorium F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Ce 58 Cerium 90 Th Thorium 59 Pr Praseodymium Neodymium 91 Pa Protactinium Nd 60 9 U Uranium Pm 61 Promethium 9 Np Neptunium Sm 6 Samarium 9 Pu Plutonium Eu 6 Europium 95 Am Americium Gd 6 Gadolinium 96 Cm Curium Tb 65 Terbium 97 Bk Berkelium Dy 66 Dysprosium 98 Cf Californium Ho 67 Holmium 99 Es Einsteinium 68 Er Erbium 100 Fm Fermium Tm 69 Thulium 101 Md Mendelevium Yb 70 Ytterbium 10 No Nobelium Lu 71 Lutetium 10 Lr Lawrencium Copyright NewPath Learning

5 There are also over 0 man-made elements, such as einsteinium. H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Sc 1 Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium state at room temperature solid gas liquid Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium Periodic Table of the Elements V Vanadium Nb 1 Niobium Ta 7 Tantalum 105 Db Cr Chromium Mo Molybdenum W 7 Tungstun 106 Sg Dubnium Seaborgium not found in nature Mn 5 Manganese Tc Technetium Re 75 Rhenium 107 Bh Bohrium Fe 6 Iron Ru Ruthenium Os 76 Osmium 108 Hs Hassium Co 7 Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds Cu 9 Copper 7 Ag Silver Au 79 Gold 111 Rg Zn 0 Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Meitnerium Darmstadtium Roentgenium Copernicium B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 8 8 Bi Bismuth 16 S Sulfur Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Ce 58 Cerium 90 Th Thorium 59 Pr Praseodymium Neodymium Promethium 91 Pa Protactinium Nd 60 9 U Uranium 61 Pm 9 Np Neptunium Sm 6 Samarium 9 Pu Eu 6 Europium 95 Am Plutonium Americium Gd 6 Gadolinium 96 Cm Curium Tb 65 Terbium 97 Bk Berkelium 66 Dy Dysprosium 98 Cf Ho 67 Holmium 99 Es Californium Einsteinium 68 Er Erbium 100 Fm Fermium Tm 69 Thulium 101 Md Yb 70 Ytterbium 10 No Mendelevium Nobelium Lu 71 Lutetium 10 Lr Lawrencium Np-7 (Neptunium) alpha particle Am-1 (Americium) Man-made elements are radioactive and unstable and decay over time into lighter elements. Compounds Most living and nonliving things are made up of a combination of elements. Elements chemically combine in a variety of ways to form compounds. A compound is made of two or more different elements bonded together in an exact ratio according to their masses. Pure Cane SUGAR NaCl C 1 H O 11 H O Copyright NewPath Learning

6 Introduction to Elements For example, water is a compound made of hydrogen and oxygen with a mass ratio of 1 to 8. However, if the mass ratio of hydrogen to oxygen is 1 to 16, the compound formed would be hydrogen peroxide. While water and hydrogen peroxide are both made of hydrogen and oxygen, they are different compounds with distinct properties. H Hydrogen (H = 1 amu) atomic mass = O 1:8 H 1 Oxygen (O = 16 amu) atomic mass = 16 mass ratio water H O O H Hydrogen Oxygen (H = 1 amu) (O = 16 amu) atomic atomic mass = mass = Copyright NewPath Learning H hydrogen 1:16 peroxide mass ratio H O Atomic Number Although atoms are amazingly small, scientists have discovered they are made up of even smaller particles - protons, neutrons and electrons. The nucleus of the atom contains neutrons and positively charged protons. Neutrons have no charge, but are thought to help to keep the nucleus together. The number of protons in the nucleus of an atom is the atomic number of that atom. All atoms of an element have the same atomic number. For example, all atoms of the element oxygen have 8 protons in their nucleus. Therefore, oxygen has an atomic number of 8. The atomic number represents the most important property of an element. nucleus O electron Oxygen atom neutron proton O 8 Oxygen atomic number symbol element name

7 Isotopes Each element has a limited number of naturally occurring isotopes. Isotopes are different forms of the same atom. An isotope of an element has the same number of protons but different numbers of neutrons. Because atomic mass is determined by the number of protons and neutrons in an atom, isotopes of the same element have different masses. For example, while the most common isotope of oxygen has 8 neutrons, other isotopes of oxygen have 9 or 10 neutrons. While some Oxygen isotopes isotopes are stable, others are radioactive and unstable. They decay to form other isotopes by releasing radiation in the form of particles or electromagnetic waves. Atomic Mass Scientists express the mass of an atom in atomic mass units (amu). The mass of a proton, the positively charged particle in the nucleus, is about 1 amu. The mass of a neutron, although a bit more massive than a proton is still considered to be 1amu. The mass of an electron is so small that it is not used in calculating # of protons (atomic number) # of neutrons Atomic protons 8 protons 8 protons 8 neutrons 9 neutrons 10 neutrons atomic mass units = amu proton (+) ~ 1 amu neutron ~ 1 amu 8 8 8mass 9 number 8 = protons + neutrons 10 mass (protons + neutrons) O 8 Oxygen amu amu amu atomic mass Copyright NewPath Learning nucleus amu amu amu neutron O 8 Oxygen electron proton electron (-) ~ 1 amu 1,86 atomic mass. Oxygen atom Oxygen-16 Oxygen-17 Oxygen-18 Each isotope of an element is identified 8 neutrons by its mass number. 9 neutrons The mass number 10 neutrons is the sum of the number of protons and neutrons in an atom. Because most elements contain a mixture of two or more isotopes, the atomic mass of an element is the weighted average of the masses of all the naturally occurring isotopes of that element. Oxygen isotopes 5

8 Introduction to Elements Electron Configuration The specific way the electrons are arranged in an atom is called the electron configuration. Electrons play an important role in how elements interact with each other and form compounds. Electrons are negatively charged particles that surround the nucleus in the form of a cloud. The atomic number of an atom, which is equivalent to its number of protons, also represents the number of electrons in that atom. The electrons electron valence electron are distributed among orbital shells or energy levels (1,, and so on) that are different distances from the nucleus. The larger the number of the energy level, the farther it is from the nucleus. Electrons that are in the highest or outmost energy level are called valence electrons. The valence electrons are the ones that are lost, gained or shared during chemical bonding. In the electron configuration for oxygen which has a total of 8 electrons, the first orbital or energy level closest to the nucleus is filled with two electrons. The second energy level can hold up to eight electrons. It begins to fill with the remaining six electrons when the first level is full. Electrons and Bonding Oxygen s valence shell has six electrons but it can hold up to eight electrons. Therefore, oxygen will often combine with other elements that allow it to share or lose two electrons. Atoms with four or more electrons in the valence shell like to gain electrons to fill the shell. 8 electron cloud 7 nucleus 6 1 orbital shell 1 orbital shell atomic number = 8 5 protons = 8 Oxygen atom (neutral) electrons = 8 valence shell 1 valence shell 1 6 nucleus 7 6 nucleus Hydrogen atom Hydrogen atom 8 5 Oxygen atom 5 Atoms with three or less electrons in their valence shell like to lose electrons to reveal the full inner shell. Atoms with full valence shells will not combine with other elements. 6 Copyright NewPath Learning

9 Label the parts of the atom. Pause and Review Complete the graphic organizer. Write one similarity and one difference between the pairs of terms. Similarities Differences Protons and Neutrons Protons and Electrons Atomic number and Atomic mass Copyright NewPath Learning 7

10 Lesson Classes of Elements Many elements have similar properties. Scientists find it useful to group elements with similar properties into classes. The classes of elements are metals, nonmetals, and metalloids. The elements within each class have similar physical properties such as appearance, density, and state of matter. They also have similar chemical properties such as the number of electrons in their metals nonmetals metalloids outermost orbital, which determines an element s reactivity, or how likely the element is to react with other elements. Metals The largest class of elements in the periodic table is metals. Examples of metals include calcium, iron, gold, silver and mercury H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Sc Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium Tc Technetium Re 75 Rhenium Bh 107 Bohrium Ru Ruthenium Os 76 Osmium Hs 108 Hassium Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium Pd 6 Palladium 78 Pt Platinum Copyright NewPath Learning Ds Ag 7 Silver Au 79 Gold 111 Rg Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium 1 cup 1 Periodic Table of the Elements Background Color metal nonmetal metalloid V Vanadium Cr Chromium Lanthanoids Ce 58 Cerium 59 Pr Actinids Th Pa 5 Mn Manganese Nd 60 Praseodymium Neodymium 9 U 6 Fe Iron Pm 61 Promethium 9 Np Symbol Color solid gas liquid 7 Co Cobalt Sm 6 Samarium 9 Pu 8 Ni Nickel Eu 6 Europium 95 Am unknown 9 Cu Copper Gd 6 Gadolinium 96 Cm 0 Zn Zinc Tb 65 Terbium 97 Bk Arsenic B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium Dy 66 Dysprosium 98 Cf C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium Ho 67 Holmium 99 Es N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 16 S Sulfur 8 8 Bi Bismuth 68 Er Erbium 100 Fm Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium Tm 69 Thulium 101 Md F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine Yb 70 Ytterbium 10 No 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 10 Lr

11 Metals have some distinct Properties of Metals: properties. Due to their high melting points, most high melting points metals are solid at room temperature, with the solid at room temperature exception of mercury which (except mercury) is a liquid. Most metals are malleable and ductile. malleable & ductile Malleability is the ability of a metal to be hammered shiny into shapes. Ductility is the ability of a metal to good conductors of heat be stretched into wire. and electricity Metals are often shiny in appearance and are good conductors of heat and electricity. Atoms of most metals have 1- electrons in the outer shell and easily lose valence electrons. Metals combine with other metals, and select nonmetals, to form a vast number of alloys that enhance the properties of metals in specific applications. For example combining iron, nickel and chromium produces a series of stainless steel alloys that are commonly used. Metals are often found combined with nonmetals as salts. Table salt is produced when the metal sodium combines with the nonmetal chlorine. aluminum calcium Chemical properties: 1- valence electrons lose electrons easily react with metals and some nonmetals valence electrons sodium chlorine Copyright NewPath Learning 9

12 Classes of Elements Nonmetals Nonmetals make up another class of elements. Some examples of nonmetals include oxygen, nitrogen, and fluorine. 1 H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Sc Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium Periodic Table of the Elements Background Color metal nonmetal metalloid V Vanadium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Cr Chromium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium Lanthanoids 58 Ce Cerium Actinids 90 Th 59 Pr 91 Pa 5 Mn Manganese Tc Technetium Re 75 Rhenium Bh 107 Bohrium Nd 60 Praseodymium Neodymium 9 U 6 Fe Iron Ru Ruthenium Os 76 Osmium Hs 108 Hassium Pm 61 Promethium 9 Np Symbol Color solid gas liquid 7 Co Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium Sm 6 Samarium 9 Pu 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds Ag 7 Silver Au 79 Gold 111 Rg Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium Eu 6 Europium 95 Am unknown 9 Cu Copper Gd 6 Gadolinium 96 Cm 0 Zn Zinc Tb 65 Terbium 97 Bk B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium Dy 66 Dysprosium 98 Cf C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium Ho 67 Holmium 99 Es N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 8 8 Bi Bismuth 68 Er Erbium 100 Fm 16 S Sulfur Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium Tm 69 Thulium 101 Md F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine Yb 70 Ytterbium 10 No 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 10 Lr Due to their low melting points, most nonmetals are gases at room temperature. Some nonmetals are solids and one element, bromine, is a liquid at room temperature. Unlike metals, nonmetals have low densities, are brittle, and do not conduct heat and electricity. Physical properties: low melting points most are gases at room temperature low densities brittle do not conduct heat and electricity bromine helium carbon 10 Copyright NewPath Learning

13 1 Chemical properties: do not give up or lose Nonmetals do not conduct electricity because their atoms are not likely to give up or lose electrons valence electrons. Nonmetals usually have four to eight electrons in their outer orbital and most of them readily gain or share valence electrons. Although nonmetals can form compounds -8 valence with metals, electrons they can also form compounds with other nonmetals. 1 carbon argon 7 Chemical gain or properties: share valence do electrons not give up easily or lose do electrons not give up or lose electrons react with metals and -8 nonmetals valence electrons -8 valence electrons gain or share valence gain electrons or share easily valence electrons react with easily metals and nonmetals react with metals and nonmetals For example, oxygen combines with sulfur to form sulfur dioxide. SO carbon oxygen 6 sulfur 5 argon oxygen oxygen SO Carbon is a very important nonmetal because it is part of all compounds found in living things. DNA SO CH OH O H H OH H OH oxygen H sugar OH H OH sulfur Helium helium oxygen A A G amino acid chain A U A U U CU G C G A A G C U A U A U U U C H H O H + N C C O - H CH CH H C CH amino acid neon Neon Some nonmetals such as neon and helium are called inert or nonreactive because their valence shell is full so they do not react with other elements to form compounds. Copyright NewPath Learning 11

14 Classes of Elements Metalloids The smallest class of elements has properties of both metals and nonmetals. These elements are called metalloids. Examples of metalloids include silicon, germanium, and boron. 1 H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Sc Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium Periodic Table of the Elements Background Color metal nonmetal metalloid V Vanadium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Cr Chromium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium Lanthanoids Ce Cerium Actinids Th Physical properties: Pr 5 Mn Manganese Tc Technetium Re 75 Rhenium Bh 107 Bohrium Praseodymium Neodymium Pa solid at room temperature shiny or dull Nd 60 9 U 6 Fe Iron Ru Ruthenium Os 76 Osmium Hs 108 Hassium Pm 61 Promethium 9 Np Symbol Color solid gas liquid 7 Co Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium Sm 6 Samarium 9 Pu 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds 9 Cu Copper Ag 7 Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium Eu 6 Europium Sb Am unknown Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium Dy 66 Dysprosium 98 Cf C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium Ho 67 Holmium 99 Es N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 8 8 Bi Bismuth 68 Er Erbium 100 Fm 16 S Sulfur Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium Tm 69 Thulium 101 Md F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine Yb 70 Ytterbium 10 No 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Antimony All metalloids are solids and can be shiny or dull in appearance. Some metalloids are malleable but some are brittle. Metalloids conduct heat and electricity, but not as well as metals. Semiconductors, made of such metalloids as silicon, can conduct electricity under certain conditions. Semiconductors are used to make electronic components like computer chips. 10 Lr malleable or brittle conductors of heat and electricity 1 Si Silicon 1 Copyright NewPath Learning

15 Metalloids have -7 electrons in their outer shell and can form bonds in similar ways as metals and nonmetals. They are also useful when combined with metals to form alloys. Pewter is an alloy that contains the metalloid antimony. Chemical properties: -7 valence electrons forms alloys with metals Sb 51 Antimony Copyright NewPath Learning 1

16 Fill in the table below. Pause and Review Class Physical property Chemical property Example Metal Nonmetal Metalloid Circle the best answer. Some may have more than one correct answer. 1) Which classes of elements are shiny? ) Which class of elements contains sodium? ) Which class of elements does not conduct electricity? ) Which class has the largest number of elements? 5) Which class of elements is found in semiconductors? 6) Which classes of elements form salts? 7) Which class contains the element found in all living things? 8) Which class of elements can be formed into sheets and wires? 9) Which class of elements is dull in appearance? 10) Which class of elements has 1- valence electrons? metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid metal nonmetal metalloid 1 Copyright NewPath Learning

17 Lesson The Periodic Table of Elements Arranging the Elements In 1869, a scientist named Dmitri Mendeleev developed a periodic table to help organize information about the 6 elements known at that time. He arranged the elements in order of increasing atomic mass. In doing so, he noticed that those that had similar properties such as Periodic Table of the Elements 1869 I H 1.01 Li 6.9 Na.0 K 9.1 Cu 6.5 Rb 85.5 Ag 108 Cs 1 Au 197 II III IV V VI VII B 10.8 Al 7.0 Be 9.01 Mg. Ca 0.1 Zn 65. Sr 87.6 Cd 11 Ba 17 Hg 01 Y 88.9 In 115 La 19 Tl 0 C 1.0 Si 8.1 Ti 7.9 Zr 91. Sn 119 Pb 07 Th N 1.0 P 1.0 V 50.9 As 7.9 Nb 9.9 Sb 1 Ta 181 Bi 09 increasing atomic mass O 16.0 S.1 Cr 5.0 Se 79.0 Mo 95.9 Te 18 W 18 U 8 F 19.0 Cl 5.5 Mn 5.9 Br 79.9 I 17 Fe 55.9 Ru 101 Os 19 VIII Co 58.9 Rh 10 Ir 19 Ni 58.7 Pd 106 Pt 195 density, appearance and melting point occurred in a repeating or periodic pattern. He found that these properties of elements Dmitri Mendeleev repeated every seven elements. Because of this pattern his table became known as the periodic table of the elements. His first attempt at arranging the known elements left some gaps in the pattern of his periodic table. Mendeleev made a prediction that elements yet to be discovered would fill these gaps. When scientists discovered these missing elements they found many of Mendeleev s predictions were correct. Henry Moseley Changing the Arrangement of the Periodic Table In 191, Henry Moseley, a British scientist discovered how to determine the number of protons in an atom. Moseley s discovery of the atomic number (number of protons) resulted in a more accurate arrangement of elements in the Periodic Table. It became apparent that atomic mass was not the significant player in the periodic law as Mendeleev had proposed, but rather, the properties of the elements varied periodically with atomic number. When atoms were arranged according to increasing atomic number, the few problems with Mendeleev s periodic table disappeared. Because of Moseley s work, the modern periodic table is based on the atomic numbers of the elements. nucleus O 8 Oxygen 16 atomic number atomic mass Oxygen atom 8 protons Copyright NewPath Learning 15

18 The Periodic Table of Elements The Modern Periodic Table There are over 110 elements in the modern periodic table arranged by increasing atomic number and similarities. These similarities are found in the rows and columns. The 18 vertical columns are called groups. The seven horizontal rows are called periods. In order to make the table more compact, two rows of elements are displayed below the main part of the table instead of in rows six and seven. When the elements are organized by period and group, elements in the same class are grouped together. Metallic elements range from the far right, across the middle and onto the left side. Metalloids form stair steps, starting at Group 1. The far right hand elements are nonmetals. Most of the radioactive elements are in the bottom rows. 1 Modern Periodic Table of the Elements H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium increasing atomic number Sc Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium V Vanadium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium metal metalloid Cr Chromium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium Lanthanoids Ce Cerium Th Pr Actinids Pa 5 Mn Manganese Tc Technetium Re 75 Rhenium Bh 107 Bohrium Nd 60 Praseodymium Neodymium 9 U Ru Ruthenium Os 76 Osmium Hs 108 Hassium Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium Pd 6 Palladium 78 Pt Platinum Copyright NewPath Learning 6 Fe Iron Pm 61 Promethium 9 Np nonmetal 7 Co Cobalt Sm 6 Samarium 9 Pu 8 Ni Nickel Ds 9 Cu Copper Ag 7 Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium Eu 6 Europium 95 Am Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 16 S Sulfur 8 8 Bi Bismuth Se Selenium Te 5 Tellurium Po Polonium 116 F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Fl Lv Flerovium Livermorium increasing atomic number Dy 66 Dysprosium Element Key Each square in the periodic table represents an element. The square may display information about the element s symbol, atomic number, atomic mass, state of matter, and class of element. The symbol is a short hand way to represent each element. The first letter of the symbol is always uppercase. If the symbol has a second letter, it is always lowercase. Some symbols are easy to remember, such as O for oxygen or C for carbon. While other symbols, such as Fe for iron, do not share any common letters. O 8 Oxygen Fe 6 Iron Cf Ho 67 Holmium 99 Es 68 Er Erbium 100 Fm C 6 Carbon Tm 69 Thulium 101 Md Yb 70 Ytterbium 10 No Ferrum (Latin term for Iron) Lu 71 Lutetium 10 Lr 17 Cl Chlorine

19 Some periodic tables display the symbols in different colors depending on their state of matter - solid, liquid, or gas at room temperature. The color of the square may also be used to show whether the element is a metal, nonmetal, or metalloid. Periods of the Periodic Table O 8 Oxygen B 5 Cl Chlorine Boron C 6 Carbon Fe 6 Iron Symbol Color solid gas liquid unknown Background Color metal nonmetal metalloid The rows of the periodic table are called periods. The periods are numbered one through seven on the left-hand side of the table. The elements in a period increase in atomic number from left to right. Elements in the same period also have the same number of orbitals. For example, all the elements in Period have two orbitals while all the elements in Period have four orbitals. At this time, the maximum number of electron orbitals or electron shells for any element is seven. The physical and chemical properties of elements in the same period are not all that similar but they follow a repeated pattern as you move across a period. For example, properties such as conductivity and reactivity steadily change from left to right in each period H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 7 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium 88 Ra Radium Modern Periodic Table of the Elements Sc Scandium Y 9 Yttrium La 57 Lanthanum 89 Ac Actinium Background Color metal metalloid Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf V Vanadium Nb 1 Niobium Ta 7 Tantalum 105 Db Cr Chromium Mo Molybdenum W 7 Tungstun 106 Sg Rutherfordium Dubnium Seaborgium Lanthanoids Ce Cerium Actinids Th nonmetal Pr Pa 5 Mn Manganese Tc Technetium Re 75 Rhenium 107 Bh Bohrium Nd 60 Praseodymium Neodymium 9 U 6 Fe Iron Ru Ruthenium Os 76 Osmium 108 Hs Hassium Pm 61 Promethium 9 Np Symbol Color solid liquid 7 Co Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds 9 Cu Copper 7 Ag Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Meitnerium Darmstadtium Roentgenium Copernicium Sm 6 Samarium 9 Pu Eu 6 Europium 95 Am gas unknown Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium 66 Dy Dysprosium 98 Cf C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium Ho 67 Holmium 99 Es N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 16 S Sulfur 8 8 Bi Bismuth 68 Er Erbium 100 Fm Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium Tm 69 Thulium 101 Md F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine Yb 70 Ytterbium 10 No 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon period Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 10 Lr Francium 7 orbitals Copyright NewPath Learning 17

20 Groups of the Periodic Table The vertical columns on the periodic table are called groups. Elements in a group have similar properties, because the atoms of the elements have the same number of valence electrons in their outer shell. For example, atoms in Group 1 have one valence electron while atoms in Group have two valence electrons. 1 1 H 1 Be Berylium 1 Mg Magnesium Ca 0 CalciumC 8 SrS Strontium Ba 56 Raa Radium Sc Y 9 Yttrium Symbol Color La Cs Hf Ta Re Os 76 Lanthanum 89 AcA Actinium Ti Zr 0 Zirconium B 5 10 Hafnium Boron 1 Rf Al Rutherfordium V Vanadium Nb 1 Niobium C Tantalum Carbon 1 Db Dubnium Si Cr Mo Molybdenum W 7 Tungstun N Nitrogen Sg 15 P Seaborgium 5 Mn Scandium Titanium Chromium Manganese dic Table 5 of the Elements solid liquid7 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cesium 87 Fr Francium e Iron u thenium 76 s smium 108 s assium The Periodic Table of Elements 7 Co Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium 8group Ni Cu 9 Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds gas Barium unknown 88 Copper Ag 7 Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium Modern Periodic Table of the Elements Background Color metal nonmetal metalloid Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium Silicon Lanthanoids Ge Ce 58 Cerium Sn 50 Tin90 Th Pb 8 Germanium Actinids Lead 11 Fl Flerovium Phosphorus 59 As Arsenic Pr Sb 51 Antimony 91 Pa Bi Tc Technetium O Oxygen Rhenium Bh 16 Bohrium S Se Nd 60 e Selenium Te 5 Tellurium 9 8 U PoP 6 Fe Iron Ru Ruthenium F Fluorine Osmium Hs 17 Hassium Cl Br Pm 61 Bromine 5 I Iodine 9 85 Np At Praseodymium Neodymium Promethium 8 Bismuth Sulfur Polonium 116 Lv Livermorium Chlorine 5 Astatine Symbol Color solid gas liquid 7 Co Cobalt 18 5 Rh Rhodium He Helium Ir 77 Iridium Ne Neon Mt 18 Ar 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds 9 Cu Copper Ag 7 Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Meitnerium Darmstadtium Roentgenium Copernicium Argon 6 Kr Sm 6 Krypton Samarium Xe 5 Xenon 9 Pu Rn 86 Radon 1 valence electron Eu 6 Europium 95 Am unknown Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium 66 Dy Dysprosium 98 Cf C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium 67 Ho Holmiumm 99 Es N 7 Nitrogen 15 P Phosphorus As Arsenic Bi O 8 Oxygen 16 S Sulfur Sb 51 5 Te Antimony Te 8 8 Bismuth 68 Er Erbium 100 Fm See Selenium ellurium PoP Polonium 116 Lv Livermorium Tm 69 Thulium 101 Md 17 F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine Yb 70 Ytterbium 10 No 7 valence electrons 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Lu 71 Lutetium 10 Lr 61 m methium Sm 6 Samarium Eu 6 Europium Gd 6 Gadolinium Tb 65 Terbium 66 Dy Dysprosium 67 Ho Holmiumm 68 Er Erbium Tm 69 Thulium Yb 70 Ytterbium Lu 71 Lutetium 9 p 9 Pu 95 Am Sodium Cm Bk Cf 99 Es 100 Fm 101 Md 10 No 10 Lr Chlorine 1 valence Valence electrons are often involved in chemical electron 7 valence bonding, making certain groups electrons more likely to react with other elements. The valence electrons also determine the ratio of elements in a compound. An element from Group 1 will combine with an element from Group 17 in a one to one Chlorine ratio. For instance, sodium (Na) combined with chlorine (Cl) forms sodium chloride, NaCl. NaCl 18 Copyright NewPath Learning

21 Pause and Review Use the Periodic Table to answer the following questions H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Periodic Table of the Elements Sc Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Background Color metal nonmetal metalloid Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium V Vanadium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Cr Chromium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium 5 Mn Manganese Tc Technetium Re 75 Rhenium Bh 107 Bohrium 6 Fe Iron Ru Ruthenium Os 76 Osmium Hs 108 Hassium Symbol Color solid gas liquid 7 Co Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds unknown 9 Cu Copper Ag 7 Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 16 S Sulfur 8 8 Bi Bismuth Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Lanthanoids 58 Ce Cerium Actinids 90 Th 59 Pr Praseodymium Neodymium 91 Pa Nd 60 9 U Pm 61 Promethium 9 Np Sm 6 Samarium 9 Pu Eu 6 Europium 95 Am Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk Dy 66 Dysprosium 98 Cf Ho 67 Holmium 99 Es 68 Er Erbium 100 Fm Tm 69 Thulium 101 Md Yb 70 Ytterbium 10 No Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 10 Lr 1) How many groups are on the periodic table? ) How many periods are on the periodic table? ) What period and group is Na in? ) What period and group is C in? 5) Which element has an atomic number of 8? 6) List three elements in group 1. 7) Which element has the symbol Si? 8) How many metalloids are there? 9) List three elements in period. 10) List two gases. Copyright NewPath Learning 19

22 s y e ive Lesson Groups on the Periodic Table Li Li Lithium 11 Lithium 11 Na Sodium Na Sodium K 19 Potassium K 19 7 Potassium Rb Rubidium Rb 7 Cs 55 Cesium 87 Cs 55 Cesium Fr87 Francium Rubidium Francium Group 1- Alkali Metals Group 1 elements, which include lithium, sodium, potassium, rubidium, cesium and francium, are alkali metals. The metals in this group are so soft that they can be cut with a knife. They are also shiny, and have low density. Alkali metals are the most reactive metals and are never found in elemental form. They are only found combined with other elements. In pure form these metals will explode when they come in contact with water and need to be stored in oil. stored in oil stored in oil easy to cut easy to cut water water highly reactive highly reactive Alkali metals are very reactive because they can easily give away or lose their single valence electron. Some important compounds formed with alkali metals include sodium chloride (table salt), borax (sodium tetraborate), potash (potassium carbonate), and washing soda (sodium carbonate) among others. single valence electron Sodium atom potash (in fertilizers) table salt washing soda (in cleaning products) 0 Copyright NewPath Learning

23 Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Group - Alkaline-Earth Metals Group elements, which include beryllium, magnesium, calcium, strontium, barium, and radium, are called alkaline-earth metals. These metals are fairly hard, shiny, and good conductors of electricity. beryl (berylium) beryl (berylium) Calcium atom valence electron calcite (calcium) Chlorine atom (halogen) barium Although alkaline-earth metals are not as reactive as alkali metals, they are still not found in elemental form, but only in compound form. They have two electrons in their valence shell and like alkali metals react readily with halogens to form salts, such as calcium chloride. CaCl Calcium Chloride Copyright NewPath Learning 1

24 Groups on the Periodic Table Groups to 1 - Transition Metals The 8 elements in Groups through 1 of the periodic table are called transition metals. Iron, copper, zinc, silver, and gold are all transition metals. As with all metals, transition metals are ductile and malleable, shiny and good conductors of heat and electricity. Because the atoms of transition metals do not give away their electrons as easily as atoms of Group 1 and, they are less reactive than alkali metals and alkaline-earth metals H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Periodic Table of the Elements Sc Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Background Color metal nonmetal metalloid Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium V Vanadium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Cr Chromium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium 5 Mn Manganese Tc Technetium Re 75 Rhenium Bh 107 Bohrium 6 Fe Iron Ru Ruthenium Os 76 Osmium Hs 108 Hassium Symbol Color solid gas liquid 7 Co Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds unknown 9 Cu Copper Ag 7 Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 16 S Sulfur 8 8 Bi Bismuth Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon groups -1 transition metals Lanthanoids 58 Ce Cerium Actinids 90 Th 59 Pr Praseodymium Neodymium 91 Pa Nd 60 9 U Pm 61 Promethium 9 Np Sm 6 Samarium 9 Pu Eu 6 Europium 95 Am Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk Dy 66 Dysprosium 98 Cf Ho 67 Holmium 99 Es 68 Er Erbium 100 Fm Tm 69 Thulium 101 Md Yb 70 Ytterbium 10 No Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 10 Lr The transition metals are unique in that their valence electrons are present in more than one shell. Also, unlike other elements, they don t always use the same number of valence electrons in chemical reactions. Iron (Fe), for example, sometimes likes to give away two electrons, and sometimes three, forming different compounds. Iron atom valence electrons Copyright NewPath Learning

25 Transition metals can be mixed with other metals to form alloys such as steel, or with calcium to form compounds found in cement or chalk. iron + nickel + chromium iron + aluminum + calcium Transition Metals - Lanthanides and Actinides The lanthanides and actinides, the two rows below the main part of the periodic table, are part of the transition metals group. The first row includes the lanthanides. At one time, the lanthanides were called the rare-earth elements, although they are not particularly rare Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium Tc Technetium Re 75 Rhenium Bh 107 Bohrium Ru Ruthenium Os 76 Osmium Hs 108 Hassium Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium Pd 6 Palladium 78 Pt Platinum 110 Ds Ag 7 Silver Au 79 Gold 111 Rg Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium In 9 Indium 81 Tl Thallium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium Sb 51 Antimony 8 8 Bi Bismuth Te 5 Tellurium Po Polonium 116 Lv Livermorium 5 I Iodine 85 At Astatine Xe 5 Xenon Rn 86 Radon La 57 Lanthanum transition metals Lanthanoids Ce Cerium Actinids Th Pr Praseodymium Neodymium Pa The lanthanides Lanthanides Lanthanides include the metal neodymium Rare used Rare Earth Earth as Metals a component Metals to make high-strength, powerful Ce Pr Nd 60 Pm 61 Sm 6 Eu 6 Gd 6 Tb 65 Dy 66 Ho 67 Pr Nd 60 Pm 61 Sm 6 Eu 6 Gd 6 Tb 65 Dy 66 Ho Er Tm 69 Cerium Praseodymium Praseodymium Neodymium Neodymium Promethium Promethium Samarium Samarium Europium Gadolinium Europium Gadolinium Terbium Dysprosium Terbium Holmium DysprosiumErbium HolmiumThulium neodymium magnets. 58 Ce Cerium Nd 60 9 U Pm 61 Promethium 9 Np Sm 6 Samarium 9 Pu Eu 6 Europium 95 Am Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk Dy 66 Dysprosium Th- U-8 (Thorium) (Uranium) The elements in the second row are radioactive or unstable and are called actinides. Only two of the actinides, thorium and uranium, occur in nature, the others are man-made. Copyright NewPath Learning 98 Cf Ho 67 Holmium 99 Es 68 Er Erbium 100 Fm Tm 69 Thulium 101 Md Yb 70 Ytterbium 10 No Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 68 Er Erbium Yb 70 YtterbiumThulium Lutetium Ytterbium YbTmLu Lu 71 Lutetium alpha particle 10 Lr

26 Groups on the Periodic Table Group 1- Boron Group The Boron Group, which includes boron, aluminum, gallium, indium, and thallium, is the first group of mixed elements. The group contains one metalloid (boron) and four metals. The elements in this group have three electrons in the valence shell and are very reactive. Aluminum is the most important metal in the Boron Group. It is used to make light weight alloys used in automotive Aluminum parts, - light foil, weight cans alloys and other products. Aluminum Foil B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium metalloid valence electron metals The metalloid boron is used to make the compound boric acid. Boric acid is used as a cleaning agent and is also added to Pyrex glass to make it heat resistant. C 6 Carbon Carbon C 6 group 1 Si Silicon Ge 11 ls 11 Fl nium Fl- etals ioactive Carbon 1 properties Group 1- vary Carbon Group Sigreatly Silicon Ge Tin & Lead - behave Sn 50 C 6 as metals Silicon & Germanium - Carbon Tin behave Pb 8 1 as nonmetals Flerovium Si - radioactive Germanium Germanium 50 Sn Tin 8 Pb Lead Lead Flerovium Flerovium 1 The Carbon Group includes carbon, silicon, germanium, tin, lead and flerovium (temporary name ununquadium). The properties Si of the Carbon Group vary greatly. Silicon Tin and lead behave entirely as metals. In their elemental solid state, Group 1 metalloids, silicon and germanium, act as electrical semiconductors, although silicon is mainly non-metallic. Tin and lead are metals, while flerovium, also known as Element 11, is radioactive. Ge Silicon Ge Germanium 50 Copyright NewPath Learning Sn silicon & germanium C 6 Carbon Germanium Sn 50 Tin Pb 8 Lead 11 tin & lead

27 ons s Carbon, the fourth most abundant element on Earth, is a very important nonmetal that forms compounds in a variety of ways. When combined with oxygen, hydrogen, and trace amounts of other elements, carbon forms all the organic compounds that make up living organisms. 7 N Nitrogen 15 P Phosphorus carbon Group 15- Nitrogen Group The Nitrogen Group includes two nonmetals: nitrogen and phosphorous; two metalloids: arsenic and antimony; and one metal: bismuth. The elements in this group have five valence electrons and generally gain three electrons when bonding with other elements. As Arsenic 51 Sb Antimony PH 8 Bi Phosphorus hydride Bismuth Nitrogen is a gas that makes up 80% of Earth s atmosphere. Natural sources of nitrogen can be found in animal and plant proteins and in fossilized remains of ancient plant life. Nitrogen from the atmosphere can be combined with hydrogen to form ammonia, used in fertilizer production. found in fossils sulfur coating found in animal & plant proteins phosphorous compound MATCHES returned to soil by decomposers Unlike nitrogen, phosphorus is extremely reactive and only found in compounds with other elements. Copyright NewPath Learning 5

28 Groups on the Periodic Table 8 O Oxygen 16 S Sulfur Se Group 16- Oxygen Group The Oxygen Group includes three nonmetals: oxygen, sulfur, and selenium; and two metalloids: tellurium, and polonium. These can be found in nature in both free and combined states. All elements of the Oxygen Group have six electrons in their outermost shell which makes this group reactive. Oxygen is the most abundant element on Earth, found in the atmosphere and dissolved in water. It is essential for the survival of most living organisms. Selenium 8 O5 Te Oxygen 16 S8 Tellurium Sulfur Po Se Polonium Selenium ns Te Lv Tellurium HO Livermorium 8 s rons Po Polonium 116 Lv Livermorium 9 F Fluorine e, 17 Cl Chlorine 5 Br ons HO water Group 17- Halogens valence The Halogen Group includes electronfour nonmetals: fluorine, chlorine, bromine, and iodine; and one metalloid: astatine. The elements in this group have seven valence electrons and are very reactive because they only need to gain one more electron to complete their outer shell. In their pure form, halogens form diatomic molecules, such as chlorine (Cl). Halogens combine with metals to form salts. Most halogens, such as chlorine or iodine, can be used as disinfectants. Feet Bromine valence electron 5 5 Feet 7 Feet I Cl Iodine 85 At Clorine atom diatomic molecule Astatine Cl diatomic molecule diatomic molecule atom 6 Copyright NewPath Learning Chlorine Tablets disinfectants disinfectants

29 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Group 18- Noble Gases Group 18, which includes elements helium, neon, argon, krypton, xenon, and radon, are all colorless, odorless gases at room temperature. These gases are inert, or nonreactive and do not react with other elements to form compounds because their valence shell is full. These elements can be used in gaseous form. Neon is used to make lighted signs. Helium, because it s less dense than air, is used to make blimps and weather balloons float. neon Neon Helium helium H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium group 1 Hydrogen Hydrogen is a special element because it is not like any other group of elements. It is placed above Group 1 in the periodic table because it has one electron in its valence shell but does not belong in the alkali metals group. Hydrogen is found in stars and it is the most abundant element in the universe. However, it only makes up one percent of the Earth s mass. On Earth, most hydrogen is combined with oxygen in the form of water. H O H O H H Copyright NewPath Learning 7

30 Pause and Review Use the Periodic Table to answer the questions below H 1 Hydrogen Li Lithium 11 Na Sodium K 19 Potassium Rb 7 Rubidium Cs 55 Cesium 87 Fr Francium Be Berylium 1 Mg Magnesium Ca 0 Calcium 8 Sr Strontium Ba 56 Barium Ra 88 Radium Periodic Table of the Elements Sc Scandium Y 9 Yttrium La 57 Lanthanum Ac 89 Actinium Background Color metal nonmetal metalloid Ti Titanium 0 Zr Zirconium 7 Hf Hafnium 10 Rf Rutherfordium V Vanadium Nb 1 Niobium Ta 7 Tantalum Db 105 Dubnium Cr Chromium Mo Molybdenum W 7 Tungstun Sg 106 Seaborgium 5 Mn Manganese Tc Technetium Re 75 Rhenium Bh 107 Bohrium 6 Fe Iron Ru Ruthenium Os 76 Osmium Hs 108 Hassium Symbol Color solid gas liquid 7 Co Cobalt Rh 5 Rhodium Ir 77 Iridium 109 Mt Meitnerium 8 Ni Nickel Pd 6 Palladium 78 Pt Platinum 110 Ds unknown 9 Cu Copper Ag 7 Silver Au 79 Gold 111 Rg 0 Zn Zinc Cd 8 Cadmium 80 Hg Mercury 11 Cn Darmstadtium Roentgenium Copernicium B 5 Boron 1 Al Aluminum Ga 1 Gallium In 9 Indium 81 Tl Thallium C 6 Carbon 1 Si Silicon Ge Germanium Sn 50 Tin Pb 8 Lead 11 Fl Flerovium N 7 Nitrogen 15 P Phosphorus As Arsenic Sb 51 Antimony O 8 Oxygen 16 S Sulfur 8 8 Bi Bismuth Se Selenium Te 5 Tellurium Po Polonium 116 Lv Livermorium F 9 Fluorine 17 Cl Chlorine 5 Br Bromine 5 I Iodine 85 At Astatine 18 He Helium Ne 10 Neon 18 Ar Argon 6 Kr Krypton Xe 5 Xenon Rn 86 Radon Lanthanoids 58 Ce Cerium Actinids 90 Th 59 Pr Praseodymium Neodymium 91 Pa Nd 60 9 U Pm 61 Promethium 8 Copyright NewPath Learning 9 Np Sm 6 Samarium 9 Pu Eu 6 Europium 95 Am Gd 6 Gadolinium 96 Cm Tb 65 Terbium 97 Bk Dy 66 Dysprosium 98 Cf Ho 67 Holmium 99 Es 68 Er Erbium 100 Fm Tm 69 Thulium 101 Md Yb 70 Ytterbium 10 No Lu 71 Lutetium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 1) What happens to the reactivity of metals as you move from group 1 to 15? Are there any other differences across the table? ) What is one similarity between metalloids? What is one difference? ) Outline the nonmetals on the periodic table. What happens to the reactivity of nonmetals as you move from group 1 to 18? Are there any other differences between the nonmetal elements? 10 Lr

31 Lab Investigation - Flame Test How are elements identified by using a flame test? A metal salt is a compound of a metal and a nonmetal. When dissolved in water, the metal and nonmetal atoms separate into charged particles called ions. As the metal ions are heated by a flame, the electrons gain energy and move to outer orbitals. When the metal ions cool, the electrons go back to their original orbitals and release energy in the form of light. Are these colors a characteristic of the metal? In this virtual investigation, you will observe the results of burning small amounts of various metal salt solutions and record the color of the flames. From your results, you will draw conclusions about the colors released from heated metal ions. You will also observe an unknown metal salt and determine which metal is present. Procedure Several metal salt solutions have been prepared. A wire loop is dipped in each solution and then inserted into a flame. Observe the color of the flame and record the colors in the data table. Note: The wire loop is cleaned between each test. Copyright NewPath Learning 9

32 Lab Investigation - Flame Test Data and Observations Record the flame color for each solution in the data table. Solution Lithium Chloride: LiCl Calcium Chloride: CaCl Potassium Chloride: KCl Flame color Copper(II) Chloride: CuCl Strontium Chloride: SrCl Barium Chloride: BaCl Barium Carbonate:BaCO Sodium Chloride: NaCl Unknown 0 Copyright NewPath Learning

33 Conclude & Apply 1. Is the color from the flame test a characteristic of the metal? Explain your answer.. How do you know the chlorine in the solution did not cause the color of the flame?. What was the purpose of performing the flame test on barium chloride and barium carbonate?. What metal is present in the unknown? Explain your answer. 5. Why is it necessary to clean the wire before each test? 6. What do you think would happen if the solution contained a mixture of two metal compounds? 7. What experiment could you do to prove the flame test color was not caused by the wire? Copyright NewPath Learning 1

34 Key Vocabulary Terms atom the building blocks of all matter; atoms are composed of protons, neutrons, and electrons electron neutron proton electron the negatively charged particle of an atom found outside the nucleus in specific areas called orbitals; electrons are very small compared to protons and neutrons atomic mass the weighted average of the masses of all naturally occurring isotopes of that element O 8 Oxygen element a substance that can t be broken down into other substances; there are over 100 known elements, examples include oxygen and copper Gold Carbon (coal) Sulfur Copper atomic number the number of protons in the atom of an element; atomic number is a property of an element O 8 Oxygen group a column on the periodic table; elements in a column share chemical and physical properties, for example the number of electrons in the valence shell compound the chemical combination of two or more elements such as table salt, a compound of the elements sodium and chlorine Cl- Na+ isotope different forms of the same element; isotopes of an element have the same number of protons but different number of neutrons 8 protons 9 neutrons 8 protons 8 neutrons 8 protons 10 neutrons Copyright NewPath Learning

35 metal a class of elements that have similar chemical and physical properties; they are shiny, good conductors of electricity and heat, and malleable; iron is an example of a metal nucleus the center of the atom; made of protons and neutrons neutron proton metalloid a class of elements that have some properties of metals and nonmetals; boron is an example of a metalloid period a row on the periodic table; elements in a period have the same number of orbitals, and their atomic number increases from left to right neutron the neutral particle found in the nucleus of an atom; the number of neutrons is not a property of an element, but helps keep the nucleus stable proton the positively charged particle in the nucleus of an atom; the number of protons is a property of an element nonmetal a class of elements that have similar chemical and physical properties; they are dull, poor conductors of heat and electricity, and brittle; oxygen is an example of a nonmetal valence shell the outermost shell of an atom; usually involved in the chemical combination of elements Copyright NewPath Learning

36 Vocabulary Review atom atomic mass atomic number compound electron element group isotope metal Copyright NewPath Learning

37 metalloid neutron nonmetal nucleus period proton valence shell Copyright NewPath Learning 5

38 Assessment Review 1. Two oxygen atoms are often bonded together as O. Is O a compound? Explain your reasoning.. How many protons, neutrons, and electrons does a neutral atom of nitrogen have? How many electrons need to be gained to fill the valence shell? N 7 Nitrogen What is the atomic mass of an element with 19 protons and 0 neutrons? What is the element? What happens if the element gains neutrons? Explain your answer.. Why is atomic mass often not a whole number? 5. Using your knowledge of metals, nonmetals, and metalloids, which class of materials would be used to make a frying pan, a pot holder, and electrical wires. Explain your reasoning. 6. After repeated pounding metals become brittle. How could you make these metals malleable again? 6 Copyright NewPath Learning

39 7. Look at the models of the elements below. Does each model represent a metal, nonmetal or metalloid? 8. Fill in the chart to describe each class of elements. Class # valence electrons Conducts electricity? Properties metal metalloid nonmetal 9. Why are alkali earth metals not found in pure form? 10. Which element: K, Cu, Si, or Cl is the best conductor of electricity? Explain your reasoning. Copyright NewPath Learning 7

40 Assessment Review 11. Predict which element: K, Fe, As or Kr is most reactive. Which element is least reactive? Explain your reasoning. 1. Fill in the chart to describe the properties of the element groups. Group alkali # valence electrons Reac tivity Properties transition noble gas 1. Groups and periods on the periodic table share similar properties. Explain which particle of the atom: proton, neutron, or electron, is most likely responsible for these similarities. 1. Why is hydrogen in a group by itself? 8 Copyright NewPath Learning

41 Assessment Copyright NewPath Learning 9

42 Assessment Copyright NewPath Learning