Name Date ID. Chemistry (2) Interim Assessment Third Grading Period

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1 Name Date ID Chemistry (2) Interim Assessment Third Grading Period 1. As you examine the elements in period four, going from left to right, you notice atomic size generally decreases. This is best explained by the fact that protons are being added to each element which makes them have more mass, resulting in a smaller atom. the nucleus becomes denser and so the atoms of an element become much smaller than the atoms of the element before it. as the number of protons in the nucleus increase, the outer electrons are pulled in closer which decreases the overall size of the atom. metals, being harder than nonmetal, will aways have atoms that are larger than nonmetals. 2. Ionization energy, simply stated, is the energy needed to remove an electron from an atom. Which of the following elements has the highest ionization energy? Nitrogen Magnesium Copper Lithium 3. A new element is discovered and given the symbol Sa. It has an electron configuration that ends in 4s 2 4p 3 and is placed in group 5A (15). The electron dot diagram for Sa should be Chemistry (2) Interim Assessment (3) Page 1

2 4. Metal atoms become metal ions by gaining electrons losing electrons gaining protons losing protons 5. Which of the following, when combined, will form an ionic bond? Pb and Cr S and O Li and F N and N 6. Which of the following is a property of ionic compounds? Most are hard and have a metallic appearance. They are often found as liquids at room temperature. When dissolved in water they conduct an electrical current. Generally they have rather low melting points. 7. Metals are conductors of electrical current. This is explained by the fact that electrons in metals are mobile and can drift freely. metals have more electrons than nonmetals. metals can be melted and formed into long strands. magnetic force lines push electrons out of metallic atoms. Chemistry (2) Interim Assessment (3) Page 2

3 8. Which of the following structures is an example of covalent bonding? 9. Gasoline will dissolve a greasy spot on a cotton shirt, but it cannot dissolve sugar. Ordinary water can dissolve sugar but not greasy spots. Water and gasoline do not mix. Gasoline is described as having a non-polar structure while water is described as being polar. Which of the following substances can you infer will dissolve in gasoline? salt detergent powder milk flakes butter 10. What is the major factor that determines if a substance is a solid, liquid, or gas at room temperature? The type of bonding it displays. The mass of the molecular structure. The position of its elements on the periodic table. The mass to density ratio of its components. 11. Which of the following compounds is composed of formula units? He O 2 MgF 2 CC1 4 Chemistry (2) Interim Assessment (3) Page 3

4 12. Which of the following polyatomic ions contains the most oxygen atoms? Ammonium Nitride Sulfite Phosphate 13. Which of the following is classified as a binary molecular compound? CaS NO 2 KOH H The name of a compound contains a prefix. This indicates the compound is binary molecular. is binary ionic. contains a polyatomic ion. must contain oxygen atoms. 15. Iodine is in group 7A(17). When it becomes an ion, how many electrons does it gain? The correct name for the chemical compound A1F 3 is Aluminum Tri-Fluorine Aluminum Fluoride Aluminum Fluorate Aluminum Fluorite Chemistry (2) Interim Assessment (3) Page 4

5 17. When Methane (CH 4 ) is completely burned in the presence of Oxygen (O 2 ), what are the products that are formed? Carbon and hydroxide Ozone Carbon and water Water and carbon dioxide 18. Identify the correct formula for Copper(II) Nitride CuN 2 CuN Cu 3 N 2 Cu 2 N Use the chemical equation below to the question. A1(NO 3 ) 3 + CaS A1 2 S 3 + Ca(NO 3 ) 2 Which sequence of coefficients are in the correct order to correctly balance the chemical reaction? 6, 1, 5, 5 2, 3, 1, 3 3, 2, 2, 3 1, 4, 2, Use the chemical equation below to answer the question. HC1 + NaOH HOH + NaC1 This chemical equation is an example of a reaction. Double replacement Synthesis Combustion Displacement Chemistry (2) Interim Assessment (3) Page 5

6 21. In a balanced chemical equation you are given one mole of Ni(OH) 2. Use information contained in the periodic table to calculate how many grams of the compound you have A balanced chemical reaction produced one hundred twenty five (125) grams of Gold (Au). This amount is equivalent to moles of Gold The following is a word equation for a chemical reaction: Gasoline is combined with oxygen to produce carbon dioxide, water vapor, heat and light. What must happen for this reaction to occur? Heat must be added to start the reaction. The liquid must be in a sealed metal container. There must be more gasoline molecules than oxygen molecules. The air must be free of moisture. Use the periodic table to answer question Based on their placement on the periodic table, which element listed below is not expected to take place in chemical reactions? Hydrogen Helium Aluminum Iodine Chemistry (2) Interim Assessment (3) Page 6

7 Name Date ID Chemistry (2) Interim Assessment Third Grading Period Answer Document

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9 Ion Chart For use on IPC and Chemistry Interim Assessments Common Monatomic Ions Li Ba Al Pb N O F Na Mg Fe Sn P S Cl K Ca Cr As Se Br Rb Sr Mn I Cs Cu Co Cu Ag Fe Be Hg Sn Co Mn Cr Pb Ni Zn Common Polyatomic Ions -1 Charge -2 Charge -3 Charge Formula Name Formula Name Formula Name C 2 H 3 O 2 Acetate HPO 4 Hydrogen PO 3 Phosphite Phosphate HCO 3 Hydrogen SO 3 Sulfite PO 4 Phosphate Carbonate HSO 4 Hydrogen Sulfate SO 4 Sulfate NO 2 Nitrite CO 3 Carbonate +1 Charge NO 3 Nitrate CrO 4 Chromate NH 4 Ammonium CN Cyanide Cr 2 O 7 Dichromate OH Hydroxide SiO 3 Silicate MnO 4 Permanganate ClO 2 Chlorite ClO 3 Chlorate

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11 Density = heat gained or ( ) = mass in change in specific lost by water ( grams )( temperature )( heat ) distance Speed = time final velocity initial velocity Acceleration = change in time Momentum = mass velocity Force = mass acceleration Work = force distance work Power = time work output % efficiency = 100 work input 1 Kinetic energy = 2 (mass velocity 2 ) Gravitational potential energy = mass acceleration due to gravity height Energy = mass (speed of light) 2 Velocity of a wave = frequency wavelength Current = mass volume voltage resistance Electrical power = voltage current Electrical energy = power time FORMULA CHART for Grades Science Assessment Constants/Conversions g = acceleration due to gravity = 9.8 m/s 2 c = speed of light = m/s speed of sound = 343 m/s at 20 C 1 cm 3 = 1 ml 1 wave/second = 1 hertz (Hz) 1 calorie (cal) = 4.18 joules 1000 calories (cal) = 1 Calorie (Cal) = 1 kilocalorie (kcal) newton (N) = kgm/s 2 joule (J) = Nm watt (W) = J/s = Nm/s volt (V) ampere (A) ohm (Ω) D = Q = (m)( T)(Cp) s = a = p = mv F = ma W = Fd P = % = 100 KE = GPE = mgh E = mc 2 v = f λ I = m v W O W I V R P= VI E = Pt d t v f v i t W t mv 2 2 Centimeters

12 Periodic Table of the Elements Group 1 IA 1 H Hydrogen 2 IIA 3 4 Li Be Lithium Beryllium Na Mg Sodium Magnesium K Ca IIIB IVB VB VIB VIIB VIII Sc Ti V Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Cr Mn Rb Sr Y Zr Nb Mo Tc Ru (98) Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Cs Ba La Hf Ta W Re Os Cesium Barium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Fr Ra Ac Rf Db Sg Bh Hs Mt (223) (261) (262) (263) (262) (265) (266) Francium Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Fe Co Rh Ir Lanthanide Series Actinide Series 58 Ce Th Pr Pa Nd U Pm Np Sm (145) Cerium Praseodymium Neodymium Promethium Samarium Pu (244) Thorium Protactinium Uranium Neptunium Plutonium IB 28 Ni Pd Pt Atomic number Symbol Atomic mass 29 Cu Ag Au 12 IIB 30 Zn Cd Hg 14 Si Silicon 13 IIIA Ga Tl 14 IVA Ge Pb Name 15 VA As 16 VIA In Sn Sb Te I Bi Se Po 17 VIIA Br At 18 VIIIA He Helium B C N O F Ne Boron Carbon Nitrogen Oxygen Fluorine Neon Al Si P S Cl Ar Aluminum Silicon Phosphorus Sulfur Chlorine Argon Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon (209) (210) (222) Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon 110 Mass numbers in parentheses are those of the most stable or most common isotope. (269) 2 Kr Xe Rn 63 Eu Am 64 Gd Cm 65 Tb Bk 66 Dy Cf 67 Ho Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Es (243) (247) (247) (251) (252) (257) (258) (259) (262) Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium 68 Er 100 Fm 69 Tm 101 Md 70 Yb 102 No 71 Lu 103 Lr Revised October 15,