Semester II Review

• Name the compounds• H2SO3 Sulfurous Acid

• H2S Hydrosulfuric acid

• H3PO4 Phosphoric acid• HCN Hydrocyanic acid• H3P Hydrophosphoric acid• HBr Hydrobromic acid• HClO Hypochlorous acid

SM II Review

• Give the formula for the following compounds• hydrofluoric acid HF

• hydroselenic acid H2Se

• carbonic acid H2CO3

• nitrous acid HNO2

• sulfuric acid H2SO4

• hydrobromic acid HBr

• Chlorous acid HClO2

SM II Review

• Antimony tribromide SbBr3

• Silicon difluoride SiF2

• Tetracarbon octahydride C4H8

• Dinitrogen monoxide N2O

• Pentaphosphorous decoxide P5O10

• Sulfur hexachloride SF6

SM II Review

• P2O5 Diphosphorous pentoxide

• SO2 Sulfur dioxide

• NO2 Nitrogen dioxide

• AsCl3 Arsenic trichloride

• P4H8 Tetraphosphorous octahydride

SM II Review

Semester II Review

• For the following compound, draw its Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces.

• SO2 e tally = 2BA 1LP, Hybrid = sp2, Shape = Bent, Polar, IMF= Dipole

Semester II Review• For the following compound, draw its

Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces.

• NH3 e tally = 3BA 1LP, Hybrid = sp3, Shape = Trigonal Pyrmidal, Polar, IMF= H-Bonds

Semester II Review• For the following compound, draw its

Lewis structure, give the electron tally, hybridization, name of shape, determine if it is polar or not, and identify the Intermolecular Forces.

• SO42- e tally = 4BA 0LP, Hybrid = sp3,

Shape = Tetrahedral, Nonpolar, IMF(Ion)

• Balance and classify the reactions

• _2_ C8H18 + _25_ O2 _16_ CO2 + _18_ H2O

• ____ FeCl3 + _3__ NaOH ____ Fe(OH)3 + _3__NaCl

• _4__ P + __5_O2 _2__P2O5

• _2__ Na + _2__ H2O __2_ NaOH + ____H2

• _2__ Ag2O _4__ Ag + ____O2

• ____ S8 + _12_ O2 _8__ SO3

Semester I Review

SM II Review• Complete, Balance, and Classify each Rxn

1. 2Al + 3S Al2S3 Synthesis

2. NaCl + AgNO3 AgCl + NaNO3 D.R.

3. C3H8 + 5O2 3CO2 + 4H2O Combustion

4. 2H2O 2H2 + O2 Decomposition

5. 2Li + Na2CO3 2Na + Li2CO3 S.R.

• In every chemical reaction, what item(s) is/are conserved? Mass and Atoms

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.

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 %

– Calculate the amount of grams of excess reactant leftover at the end of the reaction 25.8 g N2 Leftover

• 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

SM II Review

SM II Review

• Calculate the specific heat of an unknown metal, given that 25.0g of the metal lost 3570 J of energy during a temperature change from 100.0oC to 25.0oC

• c = -3570J / (25.0g)x(-75.0oC)

• c = 1.90 J/goC

SM II Review

• Identify each of the letters on the graph and explain what is occurring.

• C = solid warming/cooling• D = Phase change solid to

liquid or vice versa• E = liquid warming/cooling• F = phase change liquid to

gas or vice versa• G = gas warming/cooling C

D

E

F

G

SM II Review

• Label the solid, liquid, and gas regions on the graph.

• Label the triple point and critical point

• At 600oC and 90 atm, what phase is yummygum in? Liquid

solid

liquid

gas

Triple point

Critical point

SM II Review

• Calculate the amount of heat released if 25.0g of steam is cooled from 150.0 oC to (-15.0 oC)

• Phase 1 = -2537.5 J• Phase change = -56500 J• Phase 2 = -10460 J• Phase change = -8350 J• Phase 3 = -753.75 J• Total Energy = -78600 J

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

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.

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

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

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