Element Families. By: Olivia Litrun Physical Science Pd. 4

Transcription

1 Element Families By: Olivia Litrun Physical Science Pd. 4

2 Hydrogen ~It has one valence electron and the type of ion formed is a Cation. Its atomic number is 1 and the symbol is H. ~Hydrogen is the lightest element ~It s monotonic form is the most abundant chemical substance in the world ~The discoverer was Henry Cavendish ~It s melting point is F

3 Alkali Metals - Group 1 ~Alkali Metals contain one valence electron and it has one Cation ion. ~This group includes soft and shiny metals that react violently with water.

4 Potassium ~Potassium is in the Alkali Metals group because it reacts vigorously to air and water, but the reactivity of the Alkali Metals increases down the group. ~It has an atomic number of 19 and it s symbol is K. ~Pure Potassium is a lightweight silvery metal that is soft enough to cut with a knife. ~Potassium compounds emit a lilac or violet flame color when burned. ~It was discovered in 1807 by Humphry Davy, who isolated it from caustic potash. ~It was the first metal isolated by electrolysis.

5 Alkaline-Earth Metal- Group 2 ~ It contains 2 valence electrons and has +2 cations. ~Magnesium is used to build some airplanes, it is also found in Epsom salts, and milk of Magnesium.

6 Strontium ~Strontium is in this group because it reacts with water to produce hydrogen gas and the metal hydroxide, although somewhat less vigorously than the alkali metals. ~The atomic number of Strontium is 38 and it s symbol is Sr. ~This element was discovered in 1790 by Adair Crawford. ~Freshly cut strontium has a silvery appearance but it rapidly turns yellowish with the formation of oxide. If finely divided, it ignites spontaneously in the air. ~Strontium can be used for cardiac imaging by using it in a PET.( Positron Emission Tomography) ~It has an extremely high refractive index.

7 Transition Metals- Group 3-12 ~The amount of valence electrons cannot be determined. ~Much less reactive than groups one and two, and can lose electrons to form positive. ~Silver, gold, and platinum are often used in jewelry because they are shiny and like all metals can be stretched and pounded into different shapes. Copper is used in electrical wiring or plumbing, and tungsten is used in light bulb filaments.

8 Gold ~As with all metals, the transition elements are both ductile and malleable, and conduct electricity and heat. ~The atomic number of Gold is79 and its symbol is Au. ~Gold has been used to make jewelry since at least 4,000 BC ~Two-thirds of the world s gold is mined in South Africa, and 78% of the world s early supply is used to make jewelry, the rest goes to electronics and dental/medical uses. ~Astronaut helmets have a thin layer of gold that blocks harmful ultraviolet rays from the sun. ~Because gold is so soft it is combined with other metals to give it strength.

9 Boron Family- Group 13 ~Elements in this family have three valence electrons and they may react with other elements to form +3 cations. ~Aluminum is the most common metal in the earth s outer layer, and it is also found in cans, foil, and siding.

10 Aluminum ~It is used in lightweight alloys and is an active metal. ~Aluminum is the most important metal in the Boron family, with the chemical symbol Ai and atomic number 13. Facts ~Its discoverer is Hans Christian Orsted. ~It is a silvery white, soft, nonmagnetic, ductile metal. ~This element is the second-most abundant metallic element in the earth s crust after Silicon. ~It is very lightweight and easy to mold, fold, and recycle. ~This metal oxidizes, or loses electrons, easily, the same type of reaction that causes iron to rust.

11 Carbon Family- Group 14 ~This group does not form ionic bonds because it contains four valence electrons. ~Carbon is found in all living substances and in many synthetic. Silicon ~Silicon is metalloid, readily either donating or sharing its four outer electrons. ~This element has the symbol Si and atomic number 14. ~Its discoverer is Jons Jacob Berzelius. ~It is the second most abundant element in the earth s outer layer. ~It is a tetravalent metalloid, more reactive than germanium. ~It is a solid sitting at room temperature but it has extremely high melting points.

12 Nitrogen Family- Group 15 ~Elements in this family contain 5 valence electrons and they may react with other elements to form an anion with -3 charge. ~Pure nitrogen exists as a gas. It combines with carbon, oxygen, and hydrogen to form explosive compounds such as TNT. It s compounds are found in most fertilizers. Nitrogen is found in amino acids and nucleic acids. (DNA, RNA)

13 Phosphorus ~It is in this group because it is a non-metal, forming -3 charge anions, and it is a solid. ~It s atomic number is 15 and the symbol is P. ~Hennig Brand accidentally discovered this element while processing urine in search of a compound that would turn ordinary metals into gold. ~The world phosphorus comes from a Greek word meaning "bearer of light," and this element delivers on that promise. ~Phosphorus is waxy and gives off a slight glow in air. ~It's capable of self-igniting in air once the temperature reaches about 86 F (30 C); the only safe storage is under water.

14 Oxygen Family- Group 16 ~This family has 6 valence electrons and they may react with other elements to gain 2 electrons to form an anion with -2 charge. ~Sulfur is a yellow solid and is used to make matches and rubber tires.

15 Tellurium ~Tellurium is a metalloid which looks similar to tin, it is chemically related to selenium and sulfur. It is occasionally found in native form, as elemental crystals. ~Its atomic number is 52 and its symbol is Te. ~Tellurium was discovered in the Habsburg Empire, in 1782 by Franz-Joseph Muller von Reichenstein in a mineral containing tellurium and gold. ~It is an extremely rare element, and is most commonly found as a telluride of gold. ~It s not toxic or carcinogenic; however, when humans are exposed to too much of it they develop a garlic-like smell on their breaths. ~It is used in solar panels and memory chips for computer

16 Halogen Family- Group 17 ~This family contains 7 valence electrons and they may react with other elements to gain an electron to form a -1 anion. ~Fluorine compounds are used in toothpastes, insecticides, and in the preparation of some plastics; Bromine is used in drugs, photographic film, and in gasoline to prevent engine knocking.

17 Chlorine ~It is a non-metallic element and it has 7 electrons in its outer shell, giving it an oxidation number of -1. ~It s symbol is Ci and the atomic number is 17. ~Chlorine s discoverer is Carl Wilhelm Scheele ~It is used to make drinking water sterile and to disinfect swimming pools, and it is used in the manufacturing of a number of commonly used products, such as paper, textiles, medicines, paints, and plastic. ~But when chlorine is in a gas form it can be very harmful to human health; it is a respiratory irritant and inhaling it may cause pulmonary (buildup of fluid in the lungs), skin irritation, or even severe burns and ulcerations. ~Chlorine is a very sociable element, meaning it likes to bond with other elements rather than occur on its own.

18 Noble Gases- Group 18 ~This group contains 8 valence electrons in the outermost shell; all elements in this family are gases. ~All elements in this family are stable or inert and do not interact with other elements, this is because their outer energy level is full of electrons. Noble has elements do not lose or gain electrons to form ions. ~Helium is the second most abundant element and the lightest noble gas in the universe.

19 Radon ~All isotopes of radon are radioactive. ~Radon s atomic number is 86 and it s symbol is Rn. ~This element was discovered in 1900 by Friedrich Eritnest dorn. ~It is a radioactive, colorless, odorless, tasteless noble gas, occurring naturally as an indirect decay product of uranium, or thorium. ~Whenever it is below the freezing point it glows yellow, and when its at the temperature of liquid air it glows an orange-red color. ~This element is responsible for causing about lung cancer deaths in a air because it is very harmful to your health.

20 Lanthanides ~You are not able to predict the valence electrons or type of ion formed because of its position on the periodic table. ~Some lanthanides are used in the production of steel and glass.

21 Praseodymium ~This element reacts the same way as all of the other elements in this group. ~The atomic number of this element is 59 and the symbol is Pr. ~ Swedish chemist Carl Gustav Mosander in 1841 discovered this element. ~Although praseodymium is more resistant to corrosion in air than some other rare-earth metals, it can develop a green oxide coating when exposed to air. ~It is used as an alloying agent to create high-strength metals used in aircraft engines, It s also a component of mischmetal, a material that is used to make flints for lighters, and in carbon arc lights. It is also used in the motion picture for studio lighting and projector lights. ~This element s salts can give glasses and enamels a bright, true yellow color.

22 Actinides ~The number of valence electrons and ions formed are not able to be predicted because of the position they are in on the element table. ~All of the actinides are radioactive; they give off high energy particles.

23 Uranium ~It has a high diversity in oxidation numbers and it is radioactive. It s the most common and known element, and it s used as nuclear fuel when it s converted into plutonium, through a nuclear reaction. ~The atomic number of Uranium is 92 and it s symbol is U. ~This element was discovered by Marin H. Klaproth. ~Uranium is named after the planet Uranus, which was newly discovered when the element was identified in ~Pure uranium metal is malleable, ductile, slightly paramagnetic, and strongly electropositive. Uranium reacts with almost all nonmetallic elements in their compounds, and reactivity increases with temperature. When finely divided, uranium is pyrophoric and can react with cold water.