Semester II Review
SM II Review
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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
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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
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Antimony tribromide
Silicon difluoride
Tetracarbon octahydride
Dinitrogen monoxide
Pentaphosphorous decoxide
Sulfur hexachloride
SbBr3
SiF2
C 4H 8
N 2O
P5O10
SF6
SM II Review
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P2O5
SO2
NO2
AsCl3
P4H8
Diphosphorous pentoxide
Sulfur dioxide
Nitrogen dioxide
Arsenic trichloride
Tetraphosphorous octahydride
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)
Semester I Review
• Balance and classify the reactions
• _2_ C8H18 + _25_ O2  _16_ CO2 + _18_ H2O
• ____ FeCl3 + _3__ NaOH  ____ Fe(OH)3 + _3__NaCl
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_4__ P + __5_O2  _2__P2O5
_2__ Na + _2__ H2O  __2_ NaOH + ____H2
_2__ Ag2O  _4__ Ag + ____O2
____ S8 + _12_ O2  _8__ SO3
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SM II Review
Complete, Balance, and Classify each Rxn
2Al + 3S  Al2S3 Synthesis
NaCl + AgNO3  AgCl + NaNO3 D.R.
C3H8 + 5O2  3CO2 + 4H2O Combustion
2H2O  2H2 + O2
Decomposition
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
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
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
G
F
E
D
C
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
liquid
solid
Triple point
gas
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