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ΔHrxn =
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Exercise 9.25
Part A
How do you determine the number of electrons that go into the Lewis structure of a molecule?
ANSWER:
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Part B
How do you determine the number of electrons that go into the Lewis structure of a polyatomic ion?
ANSWER:
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Exercise 9.38
Exercise 8.18
Part A
What are valence electrons?
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Part B
Why are they important?
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Exercise 8.22
Exercise 8.52
Part A
Name an element in the third period (row) of the periodic table with three valence electrons.
Express your answer as a chemical symbol.
ANSWER:
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Exercise 8.44
Exercise 10.82
Part A
Use the drawing of energy diagram for HCl to predict the bond order.
Express your answer using two significant figures.
ANSWER:
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bond order =
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Exercise 10.54
The valence electron configurations of several atoms are shown. How many bonds can each atom make without hybridization?
Part A
B2s22p1
ANSWER:
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Part B
Why is polarity important?
ANSWER:
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Exercise 10.48
Exercise 10.15
In Lewis theory, the two bonds in a double bond look identical. However, valence bond theory shows that they are not.
Part A
Describe a double bond according to valence bond theory.
ANSWER:
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Part B
Explain why rotation is restricted about a double bond, but not about a single bond.
ANSWER:
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Exercise 10.34
The following figures show several molecular geometries.
Part A
Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (a) geometry.
Express your answers as integers separated by commas.
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Ntotal, Nbonding, Nlone =
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Exercise 11.48
Part A
Explain how doping can increase the conductivity of a semiconductor. What is the difference between an n-type semiconductor and a p-type semiconductor?
ANSWER:
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Exercise 11.98
Determine the coordination number for each of the following structures.
Part A
Gold
ANSWER:
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Coordination number =
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Score Summary:
Exercise 11.90
The high-pressure phase diagram of ice is shown at the top of the next column. Notice that, under high pressure, ice can exist in several different solid forms .
Part A
What three forms of ice are present at the triple point marked O?
ANSWER:
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Part C
Explain your answers.
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Exercise 11.80
Part A
Calculate the amount of heat required to completely sublime 99.0g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.
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Exercise 11.72
A 65.0mL sample of water is heated to its boiling point.
Part A
How much heat (in kJ) is required to vaporize it? (Assume a density of 1.00 g/mL.)
ANSWER:
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Exercise 11.68
Exercise 11.24
Part A
How is vapor pressure related to temperature? What happens to the vapor pressure of a substance when the temperature is increased? Decreased?
Check all that apply.
ANSWER:
Check all that apply.
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Exercise 11.19
Part A
Why is vaporization endothermic? Why is condensation exothermic?
ANSWER:
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Exercise 11.17
Part A
What is capillary action? How does it depend on the relative strengths of adhesive and cohesive forces?
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Exercise 11.62
Water (a) “wets” some surfaces and beads up on others. Mercury (b), in contrast, beads up on almost all surfaces.
Part A
Explain this difference.
ANSWER:
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Exercise 11.63
Part E
For the following pair of compounds, pick the one with the higher vapor pressure at a given temperature: CH3OH or H2CO.
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Exercise 11.54
Arrange the following in order of increasing boiling point.
Part A
H2S, H2Se, H2O
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Exercise 11.58
Part A
For the following pair of compounds, pick the one with the higher vapor pressure at a given temperature: CH4 or CH3Cl.
ANSWER:
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Part C
For the following pair of compounds, pick the one with the higher vapor pressure at a given temperature: CH3CH2CH2OH or CH3OH.
ANSWER:
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Part E
Exercise 11.9
Part A
Why are intermolecular forces generally much weaker than bonding forces?
ANSWER:
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Exercise 6.8
Part A
What is a state function?
ANSWER:
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Part B
List some examples of state functions.
Check all that apply.
ANSWER:
Check all that apply.
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Exercise 6.42
A system absorbs 198kJ of heat and the surroundings do 110kJ of work on the system.
Part A
What is the change in internal energy of the system?
ANSWER:
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ΔE =
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Part B
Why does the reaction mixture undergo a decrease in temperature even though energy is absorbed?
ANSWER:
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Exercise 6.74
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction:
NH4NO3(s)→NH+4(aq)+NO−3(aq)
In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 ∘C and the final temperature (after the solid dissolves) is 21.9 ∘C.
Part A
Calculate the change in enthalpy for the reaction in kilojoules per mole. (Use 1.0g/mL as the density of the solution and 4.18J/g⋅∘C as the specific heat capacity.)
Express your answer to two significant figures and include the appropriate units.
ANSWER:
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ΔHrxn =
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Exercise 7.8
Part A
What determines the color of a colored object?
ANSWER:
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Part B
This question will be shown after you complete previous question(s).
Exercise 7.12
Part A
Describe the photoelectric effect.
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Exercise 7.42
Calculate the wavelength of each of the following frequencies of electromagnetic radiation.
Part A
104.8MHz (typical frequency for FM radio broadcasting)
Express your answer using four significant figures.
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λ1 =
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Part B
What forces air into your lungs?
ANSWER:
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Exercise 5.30
The pressure on top of Mt. Everest averages about 235 mmHg.
Part A
Convert this pressure to torr.
ANSWER:
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P =
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Part B
How is the root mean square velocity of a gas related to its molar mass?
ANSWER:
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Exercise 5.22
Part A
Describe how the molecules in a perfume bottle travel from the bottle to your nose.
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Part B
What is mean free path?
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Exercise 5.23
Part A
Explain the difference between diffusion and effusion.
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Part B
How is the effusion rate of a gas related to its molar mass?
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Exercise 5.84
Exercise 5.90
A sample of N2O effuses from a container in 47 seconds.
Part A
How long would it take the same amount of gaseous I2 to effuse from the same container under identical conditions?
Express your answer using two significant figures.
ANSWER:
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t =
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Exercise 5.94
Part A
Which postulate of the kinetic molecular theory breaks down under conditions of low temperature?
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Exercise 5.146
Part A
Which of the following gases would you expect to deviate most from ideal behavior under conditions of low temperature: F2, Cl2, Br2?
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