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Final Exam Review Questions
Balancing Equations:
1. Write the name:
a. Fe(ClO3)3
b. H2SO4
c. CH4
2. Write the formula:
a. Ammonium Sulfate
b. Tungsten(VI) Carbonate
c. Methanol
3. Balance the Equation w/ symbols of state
a. Zinc + Oxygen 
b. Hydrogen + Nitrogen 
1. Balance the Equation w/ symbols of state
a. Potassium Chlorate 
b. Cupric Carbonate 
2. Confirm that a reaction occurs, and balance
a. Calcium + Silver Nitrate 
b. Chromium + Sodium Chloride 
c. Zinc + Stannic Acetate 
3. Balance, and determine precipitate
a. Lithium Chloride+Silver Nitrate
b. Magnesium Bromide + Potassium
Hydroxide 
4. Write the net ionic and tell what was oxidized and reduced in 2a above
5. Write the net ionic equations for 3b above.
Stoichiometry:
1. If you have 13.0 mol of chlorine gas added to sodium bromide, what mass of bromine
will form?
2. If you produce 9.8mol of product, how many moles of aluminum will react with
excess oxygen?
3. What mass of solid product would form in the decomposition of 113.7g of ferric
carbonate?
Solutions, Acids and Bases:
1. What is the Arrhenius Definition of Acids and Bases?
2. What is the Molarity of 39.0grams of Hydrogen Chloride is 3000 mL of water?
3. How many grams of Sodium Hydroxide were dissolved to form 350 mL of a 0.24 M
solution?
4. What volume of 3.0 M HNO3 would be needed to make 300 mL of 0.2 M HNO3?
5. What is the mass percent of Sugar when 34 grams of C12H22O11 are dissolved in 766
grams of water?
6. What is the mole fraction of 218g of silver nitrate in 3000.0g of water?
7. What is the freezing and boiling point of 16g of calcium chloride in 350mL water? (
Kfp = 1.85 oC/m Kbp = 0.515 oC/m)
6. What is the Bronsted-Lowry Definition of Acids and Bases?
7. What is the pH if the [H1+] = 1x10-4 ?
8. What is the pH if the [OH1-]= 1x10-12 ?
9. Nitric Acid is neutralized with Calcium Hydroxide.
a. Write the balanced equation
b. Given 50.0 mL of 0.50 M Nitric Acid, how many mL of 0.10 Calcium Hydroxide are
required to neutralize?
10. Name four properties each of acids and bases.
11. If a solution has a pH = 4.50, what is the [H1+]?
12. If a solution has a pH = 11.00, what is the [OH1-]?
13. Phosphoric Acid is neutralized by Potassium Hydroxide.
a. Write the balanced eq.
b. Given 50.0 mL of 0.50 M Phosphoric, what is the molarity of the Hydroxide if
it took 300 mL to reach the end-point?
Gases
1. What causes pressure?
What causes temperature?
2. A gas-filled syringe has a volume of 3 mL, and a pressure of 1.5 atm. If the pressure
is reduced to 1.0 atm, what is the new volume? (other factors constant)
3. A balloon has a volume of 230 dm3 and a temperature of 40 C. If the balloon is
cooled to 20 C, what is the new volume?
4. A piston has a pressure of 101.3 kPa and a temp. of 25 C. If the pressure increases to
202.6 kPa, what is the new temp?
5. What is STP?
What is vapor pressure?
6. A sample of gas has a pressure of 1.3 atm, a volume of 500. mL, and a temp of 22 C.
What will be the volume of the gas at STP?
7. A 3.5 moles of a gas is at STP. What is its volume?
8. Iron reacts with Oxygen to form Ferric Oxide.
a. write the balanced eq.
b. 20,000. mL of Oxygen, at 10C and 800 mm Hg reacts with an excess of Iron. How
many grams of Ferric Oxide are formed?
9. What are the components of the Kinetic Theory of Gases?
10. A sample of gas is at 25C, 1.25 atm, and occupies 3200 mL of volume. How many
moles are in the sample?
11. A Solution of Rubidium Bromide reacts with gaseous Fluorine.
a. write the balanced eq.
b. If 25,000. mL of Fluorine at 25 C and 110.1 kPa is provided, what is the maximum
mass of Rubidium Bromide that would react?
12. 75.0 grams of Methane combusts.
a. write the balanced eq.
b. Determine the mass of oxygen needed for complete combustion.
c. At STP, what would be the volume of the Oxygen?
13. Krypton effuses 1.38 times faster than what diatomic gas?
Electron Configuration
1. What is the electron configuration for:
C
K
Cr
Fe3+
2. List the 4 sublevels and how many electrons in each
3. How many valence electrons in these elements:
N
I
Ba
B
Sc
Cd
4. Name and describe the four quantum numbers.
5. What is the aufbau rule?
6. What is Hund’s rule? Give an example of its application.
7. What is the Pauli Exclusion Principle?
How is it used in electron configuration or Orbital notation problems?
Periodic Trends
1. What is the trend for atomic radius?
Put in order from large to small:
Li Rb K
P
Cl
Na
2. What is the trend for ionic radius?
Put in order from large to small
Ca
Ca2+
N3N
3. What is the trend for reactivity?
4. What is the trend for ionization energy?
5. What is electron affinity?
Quantum Problems
1. What is the dual nature of light?
2. Write the colors of the visible spectrum in order from long to short wavelength
3. Label the electromagnetic spectrum in terms of frequency, (low to high)
4. Label the electromagnetic spectrum in terms of energy, (low to high)
5. What is the dual nature of matter?
6. A photon of light has a frequency of 7.5x10 14 Hz.
What is its energy?
7. A beam of light has a wavelength of 6.25x106 m.
What is its frequency?
8. A particle has a mass of 2.55x10-30 kg. Its velocity is 75% of the speed of light.
What is its wavelength?
Heat
1. How much heat is required to raise the temperature of 854g of water from 23.5oC to
85.0oC? (Cp = 4.184J/goC)
2. If a piece of aluminum with a mass of 3.90g and a temperature of 99.3oC is dropped
into 10.0cm3 of water at 22.6oC, what will the final temperature be of the system?
(specific heat Al = 0.9025 J/goC)
3. Compute the heat of reaction for the formation of 193g of ammonium bromide from
the following equation:
NH3 + HBr  NH4Br + 188.32kJ
4. Calculate the amount of heat in joules required to raise 180.0g of water at 10.0oC to
steam at 105.0oC. (Heat of vaporization = 2.26kJ/mol, Cp(g) = 2.03J/goC)