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Semester II Review

Semester II Review. Semester II Review. Which of the following elements has the smallest first ionization energy: potassium or calcium? Which of the following has the smallest atomic radius: O or S?

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Semester II Review

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  1. Semester II Review

  2. Semester II Review • Which of the following elements has the smallest first ionization energy: potassium or calcium? • Which of the following has the smallest atomic radius: O or S? • The energy required to remove an electron from a gaseous atom is called the Ionization energy.

  3. Semester II Review • Atomic size generally decreases as you move left to right in a period. • How does atomic radius change down a group in the periodic table?Increases • How does ionization energy change as you move up and to right on the periodic table? Decreases up and increases to the right

  4. Semester II Review • Sheilding will increase as you go down a group. • Sheilding will remain constant as you move left to right across a period. • Electronegativity will decrease as you move down and to the left. • Columns on the periodic table are known as groups or families. • Rows on the table are known as periods.

  5. Semester II Review • Name the following compounds: • HBr Hydrobromicacid (bromide) • NaOH Sodium Hydroxide • FeO Iron (II) Oxide • HNO3 NitricAcid (nitrate) • SO3 Sulfur Trioxide (molecule all nonmetals) • Li3PO4 Lithium Phosphate

  6. Semester II Review • Give the formula for the following compounds. • Carbonic acid H2CO3 • Manganese (II) chloride MnCl2 • Calcium nitride Ca3N2 • Hydrochloric acid HCl • Dinitrogen Tetroxide N2O4

  7. Semester II Review • For the following compound, draw its lewis structure, give the electron tally, hybridization, name of shape, bond angles, and determine if it is polar or not. • SO2

  8. Semester II Review • For the following compound, draw its lewis structure, give the electron tally, hybridization, name of shape, bond angles, and determine if it is polar or not. • NH3

  9. Semester II Review • For the following compound, draw its lewis structure, give the electron tally, hybridization, name of shape, bond angles, and determine if it is polar or not. • SO42-

  10. SM II Review • Complete, Balance, and Classify each Rxn • 2Al + 3S  Al2S3 • NaCl + AgNO3 AgCl + NaNO3 • C3H8 + 5O2 3CO2 + 4H2O • 2H2O  2H2 + O2 • 2Li + Na2CO3 2Na + Li2CO3 • In every chemical reaction, what item(s) is/are conserved? Mass and Atoms

  11. SM II Review • For a given chemical reaction, the theoretical yield is generally more than the actual yield • The first step in most stoichiometry problems is to balance the equation.

  12. SM II Review • Hydrogen gas reacts with nitrogen gas to form ammonia gas. • Write and balance the equation • 3H2 + N2  2NH3 • Determine the Limiting reactant if 3.50 g of hydrogen reacts with 42.0 g of nitrogen. • What is the theoretical yield of the above problem? 39.4 g NH3 • What is the % yield if the reaction produced 15.3 g of ammonia. 38.8 %

  13. SM II Review • What is the empirical formula of a compound that is 32.37 % Na, 22.58 % S, and 45.05 % O. Na2SO4 • If the molecular formula molar mass is 284.10, what is the molecular formula of the above compound. Na4S2O8 • What is the percent composition of FeO? 77.73% Fe and 22.27% O

  14. SM II Review • If the volume of a container holding a gas is reduced, what will happen to the pressure within the container? Increase • What happens to the temperature of a gas when it is compressed? Increases • What happens to the pressure of a gas inside a container, if the temperature of the gas is lowered? Decreases • The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change? Decreases by 2 times

  15. SM II Review • Boyle’s law states that PV = K, inverse proportion. • Charles’ law states that V/T = K, direct proportion. • Gay-Lussac’s law states that P/T = K, direct proportion. • Avogadro’s law states that V/n = K, direct proportion. • Dalton's Law states that sum of all the pressures = the total pressure. • Graham's law states that gases with smaller masses with effuse and diffuse faster than gases with larger masses.

  16. Semester II Review • How many grams of CO2 are produced when 34.6 L of CH4 combusts with oxygen at a pressure of 1.78 atm and a temperature of 28oC. • Balance the equation first. (combustion of hydrocarbon) • CH4 + 2O2 CO2 + 2H2O • 2.49 mol CH4 will produce 110. g CO2

  17. SM II Review • A gas confined in a 305 mL container exerts a pressure of 1.07 atm at 38.6°C. At what Celsius temperature will it exert a pressure of 2.75 atm if it is placed into a 644 mL container? • 1506 K - 273 = 1233 °C

  18. SM II Review • What is the pressure inside a 3.0 L flask if 30.5 g of Carbon Monoxide is held at a temperature of 105.2 oC? • 11 atm or 1100 kPa

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