Question 1

A student mixes aqueous solutions of silver nitrate (AgNO$$_3) $$and sodium chloride (NaCl). A white precipitate forms. Which of the following best represents the net ionic equation for this reaction?

Accepted Answer

$$\mathrm{Ag^+ (aq) + Cl^- (aq) \rightarrow AgCl (s)}$$

Question 2

Which of the following statements about the periodic trend in atomic radius is correct?

Accepted Answer

Atomic radius decreases across a period due to increasing nuclear charge.

Question 3

A sample of gas occupies 4.00 L at 1.00 atm and 300 K. What will be its volume at 2.00 atm and 300 K, assuming ideal behavior?

Accepted Answer

$$2.00\ \mathrm{L}$$

Question 4

Which of the following compounds is expected to have the highest boiling point?

Accepted Answer

H$$_2O$$

Question 5

A 10.0 g sample of a compound contains 2.0 g hydrogen and 8.0 g oxygen. What is the empirical formula of the compound?

Accepted Answer

H$$_2O$$

Question 6

Which of the following best describes the difference between a physical and a chemical change?

Accepted Answer

A physical change does not alter the chemical identity, while a chemical change produces new substances.

Question 7

Which of the following quantum number sets is NOT allowed for an electron in an atom?

Accepted Answer

$$n=2,\ l=2,\ m_l=0,\ m_s=+\frac{1}{2}$$

Question 8

A solution is prepared by dissolving 0.50 mol NaCl in enough water to make 1.0 L of solution. What is the molarity of the solution?

Accepted Answer

$$0.50\ \mathrm{M}$$

Question 9

Which of the following best explains why water (H$$_2O) $$has a much higher boiling point than methane (CH$$_4$$)?

Accepted Answer

Water forms hydrogen bonds, which are much stronger than the London dispersion forces in methane.

Question 10

A reaction has a theoretical yield of 10.0 g and an actual yield of 8.0 g. What is the percent yield?

Accepted Answer

$$80\%$$

Question 11

Which of the following is a strong electrolyte?

Accepted Answer

NaOH (aq)

Question 12

Which of the following best describes the molecular geometry of SF$$_6$$?

Accepted Answer

Octahedral

Question 13

Which of the following statements about the Pauli Exclusion Principle is correct?

Accepted Answer

No two electrons in the same atom can have the same set of four quantum numbers.

Question 14

A sample of hydrogen gas is collected over water at 25$$^\circC $$and 1.00 atm total pressure. The vapor pressure of water at 25$$^\circC is 0.0313 $$atm. What is the partial pressure of hydrogen gas?

Accepted Answer

$$0.969\ \mathrm{atm}$$

Question 15

Which of the following best describes the effect of increasing temperature on the root mean square speed ($$u_{rms}) of a $$gas?

Accepted Answer

$$u_{rms}$$ increases as temperature increases.

Question 16

Which of the following is the correct electron configuration for a ground-state phosphorus atom (Z = 15)?

Accepted Answer

$$1s^2\ 2s^2\ 2p^6\ 3s^2\ 3p^3$$

Question 17

Which of the following laboratory errors would most likely cause the calculated concentration of a titrated solution to be too high?

Accepted Answer

Overshooting the endpoint during titration

Question 18

Which of the following molecules is nonpolar, despite having polar bonds?

Accepted Answer

CO$$_2$$

Question 19

Which of the following best describes the process occurring at the flat region of a heating curve for water at 100$$^\circC$$?

Accepted Answer

Vaporization (liquid to gas) at constant temperature

Question 20

Which of the following best explains why the ionization energy of nitrogen is higher than that of oxygen, contrary to the general trend?

Accepted Answer

Nitrogen has a half-filled p subshell, which is especially stable.

General Chemistry I: Comprehensive Study Notes (Chapters 1–11)

Study Guide - Practice Questions

Study Guide - Flashcards