Chapter 5
Chapter 9
Chapter 10
Chapter 11
Random
100
What is Dalton's Law of Partial Pressure?
The total pressure is the summation of all contributing pressures.
100
What is a resonance structure?
A contributing structure to the overall structure of the molecule. "Movement of electrons"
100
What is VSEPR theory?
Valence-Shell Electron-Pair Repulsion predicts the molecular and electronic shape of a molecule based on the number of ligands and lone pairs.
100
What are the four Intermolecular forces? Order from least to greatest strength.
Van der Waals (London Dispersion), Dipole-Dipole, Hydrogen Bonding, and Ionic Bonding.
100
A direct over lap of orbitals that share electrons is called what?
sigma bond
200
A sample of gas has an initial volume of 5.6 L at a pressure of 735 mmHg. If the volume of the gas is increased to 9.4 L, what is its pressure? What simple gas law are we using?
438 mmHg or 0.576 atm. Boyle's Law (constant temperature)
200
What is the equation to calculate formal charge?
# Valence electrons - (1/2 # bonding electrons+ #lone electrons)
200
According to Valence Bond Theory what type of orbital can create a bond?
A paramagnetic or 1 electron filled orbital
200
If intermolecular force of a solution increases in strength what happens to the vapor pressure and boiling point?
The vapor pressure decreases and the boiling point increases
200
Which the following would have the smallest average velocity at a constant temperature of 25 °C: H2, CH4, N2, O2, or Cl2?
Cl2 (g) =1/2 mv^2 and =3/2RT
300
At standard temperature and pressure (STP) what is the volume of 1 mole of propane gas?
At STP an ideal gas has a volume of 22.44 L
300
Draw the lewis structure for CH3COOH.
300
What is the electronic geometry of SF4?
Octahedral
300
Does the temperature change when water in converted from a liquid to a gas (before all liquid water is a gas)?
No, heat of vaporization is the conversion of liquid to a gas once this process is done the temperature can finally change.
300
Which of the following compounds would have the greatest ionic bonding (most negative lattice energy): NaI, NaBr, NaCl, or NaF?
NaF, Coulomb's Law with relative force acting on the charges.
400
Consider the chemical reaction: 2 H2O(l) --> 2 H2(g) + O2(g) What mass of H2O is required to form 1.4 L of O2 at a temperature of 315 K and a pressure of 0.957 atm?
1.87g
400
Draw to Lewis structure of phosphate (PO4)^(-3). Create all resonance structures of phosphate?
400
What is the molecular geometry of ClF3?
T-shape
400
Calculate the amount of heat required to completely sublime 50.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol
36.7 kJ
400
Explain boiling point.
Occurs when the vapor pressure is equivalent to the external pressure.
500
A gas mixture contains each of the following gases at the indicated partial pressures: N2(g) , 215 torr; O2(g) , 102 torr; and He(g), 117 torr. What is the total pressure of the mixture? What mass of each gas is present in a 1.35 L sample of this mixture at 25.0 °C?
Total pressure: 439 torr or 0.578 atm Mass: N2 - 0.437g O2 - 0.249g He - 0.0340g
500
A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the compound.
HCCH, acetylene
500
What is the hybridization of carbon in carbon dioxide (CO2) and acetylene (C2H2)?
sp
500
How much heat (in kJ) is required to warm 10.0 g of ice, initially at -150.0 °C , to liquid at 75.0 °C ? The Heat capacity of ice is 2.09 J/g°C , Heat capacity of steam is 2.01 J/g°C, Heat capacity of water: 4.179 J/g°C, Heat of Vaporization: 40.65 kJ/mol, and Heat of Fusion: 6.0 kJ/mol
9.6 kJ
500
A scuba diver creates a spherical bubble with a radius of 2.5 cm at a depth of 30.0 m where the total pressure (including atmospheric pressure) is 4.00 atm. What is the radius of the bubble when it reaches the surface of the water? (Assume that the atmospheric pressure is 1.00 atm and the temperature is 298 K.) Volume of sphere= 4/3πr^3 and 1cm^3=1mL
3.97 cm
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