Question 1

Which of the following best describes the difference between ionic and covalent bonds?

Accepted Answer

Ionic bonds involve the transfer of electrons from one atom to another, resulting in oppositely charged ions, while covalent bonds involve the sharing of electrons between atoms.

Question 2

A student mixes 50.0 mL of 1.0 M HCl with 50.0 mL of 1.0 M NaOH in a coffee-cup calorimeter. The temperature of the solution increases by 6.0 °C. If the specific heat capacity of the solution is $$4.18 \ \mathrm{J} / (\mathrm{g} \cdot \mathrm{K})$$ and the density is $$1.00 \ \mathrm{g} / \mathrm{mL}$$, what is the enthalpy change ($$\Delta H) $$for the reaction per mole of water formed?

Accepted Answer

$$-50.2 \ \mathrm{kJ} / \mathrm{mol}$$

Question 3

Which of the following statements about the periodic table is correct?

Accepted Answer

Elements in the same group have the same number of valence electrons.

Question 4

A sample of gas occupies $$2.00 \ \mathrm{L} at$$ $$1.00 \ \mathrm{atm}$$ and $$300 \ \mathrm{K}. If $$the pressure is increased to $$2.00 \ \mathrm{atm}$$ and the temperature is increased to $$400 \ \mathrm{K}$$, what is the new volume of the gas?

Accepted Answer

$$2.67 \ \mathrm{L}$$

Question 5

Which of the following best explains why water has a higher boiling point than methane ($$\mathrm{CH}_4$$)?

Accepted Answer

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

Question 6

Which of the following is the correct electron configuration for a neutral atom of phosphorus ($$Z = 15$$)?

Accepted Answer

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

Question 7

A 10.0 g sample of an unknown metal is heated to $$100.0 \ ^\circ \mathrm{C}$$ and then placed in 50.0 g of water at $$20.0 \ ^\circ \mathrm{C}. $$The final temperature of the system is $$22.0 \ ^\circ \mathrm{C}. $$What is the specific heat capacity of the metal? (Assume no heat loss to the surroundings. $$c_{\mathrm{water}} = 4.18 \ \mathrm{J} / (\mathrm{g} \cdot \mathrm{K}))$$

Accepted Answer

$$0.42 \ \mathrm{J} / (\mathrm{g} \cdot \mathrm{K})$$

Question 8

Which of the following best describes the concept of electronegativity?

Accepted Answer

The ability of an atom to attract electrons in a chemical bond.

Question 9

A solution is prepared by dissolving $$10.0 \ \mathrm{g} of $$NaCl in enough water to make $$500.0 \ \mathrm{mL} of $$solution. What is the molarity of the solution? ($$\mathrm{Molar\ mass\ of\ NaCl} = 58.44 \ \mathrm{g} / \mathrm{mol})$$

Accepted Answer

$$0.342 \ \mathrm{M}$$

Question 10

Which of the following is a correct statement about oxidation and reduction in a redox reaction?

Accepted Answer

Oxidation is the loss of electrons, and reduction is the gain of electrons.

Question 11

A balloon filled with helium has a volume of $$2.50 \ \mathrm{L} at$$ $$25.0 \ ^\circ \mathrm{C}$$ and $$1.00 \ \mathrm{atm}. If $$the balloon rises to an altitude where the temperature is $$-15.0 \ ^\circ \mathrm{C}$$ and the pressure is $$0.800 \ \mathrm{atm}$$, what is the new volume of the balloon?

Accepted Answer

$$2.86 \ \mathrm{L}$$

Question 12

Which of the following best explains why ice floats on liquid water?

Accepted Answer

Ice is less dense than liquid water because hydrogen bonding causes the molecules to arrange in an open hexagonal structure.

Question 13

Which of the following is the correct net ionic equation for the reaction between aqueous solutions of silver nitrate and sodium chloride?

Accepted Answer

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

Question 14

A 0.500 mol sample of an ideal gas is confined in a 10.0 L container at 300 K. What is the pressure of the gas? ($$R = 0.0821 \ \mathrm{L} \cdot \mathrm{atm} / (\mathrm{mol} \cdot \mathrm{K}))$$

Accepted Answer

$$1.23 \ \mathrm{atm}$$

Question 15

Which of the following best describes a buffer solution?

Accepted Answer

A solution that resists changes in pH when small amounts of acid or base are added.

Question 16

Which of the following is the correct balanced equation for the combustion of propane ($$\mathrm{C}_3\mathrm{H}_8$$)?

Accepted Answer

$$\mathrm{C}_3\mathrm{H}_8 + 5 \mathrm{O}_2 \rightarrow 3 \mathrm{CO}_2 + 4 \mathrm{H}_2\mathrm{O}$$

Question 17

A patient receives an intravenous solution containing $$0.90\%$$ NaCl by mass. If the patient receives $$500 \ \mathrm{mL} of $$this solution, how many grams of NaCl does the patient receive?

Accepted Answer

$$4.5 \ \mathrm{g}$$

Question 18

Which of the following best explains why noble gases are generally unreactive?

Accepted Answer

They have a full complement of valence electrons, making them stable.

Question 19

Which of the following is the correct Lewis structure for carbon dioxide ($$\mathrm{CO}_2$$)?

Accepted Answer

O=C=O, with each oxygen atom having two lone pairs.

General Chemistry I: Course Schedule and Key Topics Overview

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