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CHEM 104 COMPREHENSIVE FINAL EXAM 2026/2027 |
GENERAL CHEMISTRY – PORTAGE LEARNING | EXPERT
VERIFIED | 150 VERIFIED Q&A | DETAILED RATIONALES |
NGN-ALIGNED | PASS GUARANTEED - A+ GRADED
SECTION A: MULTIPLE CHOICE (Questions 1-100)
Instructions: Select the single best answer for each question.
1. Which type of bond is formed by the transfer of electrons between atoms?
• A) Covalent bond
• B) Ionic bond
• C) Metallic bond
• D) Hydrogen bond
Answer: B) Ionic bond
Rationale: An ionic bond is formed by the transfer of electrons from one atom to another, resulting
in the formation of cations and anions. Covalent bonds involve sharing of electrons, metallic bonds
involve a "sea of electrons," and hydrogen bonds are intermolecular forces.
Teaching Point: Ionic bonds typically form between metals and nonmetals. Covalent bonds form
between nonmetals.
2. What is the molecular geometry of methane (CH₄)?
• A) Linear
• B) Trigonal planar
• C) Tetrahedral
• D) Bent
Answer: C) Tetrahedral
Rationale: Methane (CH₄) has a tetrahedral molecular geometry with bond angles of 109.5°. The
central carbon atom has four bonding pairs and no lone pairs.
Teaching Point: VSEPR theory predicts molecular geometry based on the number of bonding and
lone pairs around the central atom.
3. What is the pH of a solution with [H⁺] = 1 × 10⁻⁴ M?
• A) 2
,2
• B) 3
• C) 4
• D) 5
Answer: C) 4
Rationale: pH = -log[H⁺] = -log(1 × 10⁻⁴) = 4.
Teaching Point: pH is a measure of acidity. Lower pH means higher acidity.
4. Which of the following is a strong acid?
• A) HCl
• B) CH₃COOH
• C) H₂CO₃
• D) HF
Answer: A) HCl
Rationale: HCl (hydrochloric acid) is a strong acid that completely dissociates in water. CH₃COOH,
H₂CO₃, and HF are weak acids.
Teaching Point: The six common strong acids are HCl, HBr, HI, HNO₃, H₂SO₄, and HClO₄.
5. What is the oxidation number of oxygen in most compounds?
• A) -1
• B) -2
• C) 0
• D) +2
Answer: B) -2
Rationale: Oxygen typically has an oxidation number of -2 in most compounds (except in peroxides
where it is -1 and in OF₂ where it is +2).
Teaching Point: Oxidation numbers are assigned based on a set of rules.
6. What is the equilibrium constant expression for the reaction aA + bB ⇌ cC + dD?
• A) Keq = [A]^a[B]^b / [C]^c[D]^d
• B) Keq = [C]^c[D]^d / [A]^a[B]^b
• C) Keq = [A][B] / [C][D]
• D) Keq = [C][D] / [A][B]
,3
Answer: B) Keq = [C]^c[D]^d / [A]^a[B]^b
Rationale: The equilibrium constant expression is the ratio of the concentrations of products raised
to their stoichiometric coefficients divided by the concentrations of reactants raised to their
stoichiometric coefficients.
Teaching Point: Pure solids and liquids are not included in the equilibrium constant expression.
7. What is the effect of increasing temperature on the rate of a reaction?
• A) Increases reaction rate
• B) Decreases reaction rate
• C) No effect
• D) Depends on the reaction
Answer: A) Increases reaction rate
Rationale: Increasing temperature increases the kinetic energy of molecules, leading to more
frequent and more energetic collisions, which increases the reaction rate.
Teaching Point: Increasing temperature by 10°C approximately doubles the reaction rate.
8. What is the Arrhenius equation?
• A) k = A e^(-Ea/RT)
• B) k = A e^(Ea/RT)
• C) k = RT e^(-Ea/A)
• D) k = A RT e^(-Ea)
Answer: A) k = A e^(-Ea/RT)
Rationale: The Arrhenius equation relates the rate constant (k) to temperature (T), activation energy
(Ea), and the frequency factor (A).
Teaching Point: The Arrhenius equation shows that k increases with temperature and decreases
with activation energy.
9. What is the pH of a 0.01 M NaOH solution?
• A) 2
• B) 7
• C) 10
• D) 12
Answer: D) 12
, 4
Rationale: NaOH is a strong base, so [OH⁻] = 0.01 M. pOH = -log(0.01) = 2. pH = 14 - 2 = 12.
Teaching Point: Strong bases completely dissociate in water.
10. What is the oxidation number of hydrogen in most compounds?
• A) -1
• B) 0
• C) +1
• D) +2
Answer: C) +1
Rationale: Hydrogen typically has an oxidation number of +1 in most compounds (except in metal
hydrides where it is -1).
Teaching Point: In metal hydrides (e.g., NaH), hydrogen has an oxidation number of -1.
11. Which of the following is a strong base?
• A) NH₃
• B) NaOH
• C) CH₃NH₂
• D) NaHCO₃
Answer: B) NaOH
Rationale: NaOH (sodium hydroxide) is a strong base that completely dissociates in water. NH₃,
CH₃NH₂, and NaHCO₃ are weak bases.
Teaching Point: Strong bases include NaOH, KOH, and Ca(OH)₂.
12. What is the effect of a catalyst on the activation energy?
• A) Lowers activation energy
• B) Raises activation energy
• C) No effect
• D) Changes the equilibrium
Answer: A) Lowers activation energy
Rationale: A catalyst lowers the activation energy by providing an alternative pathway for the
reaction. This increases the reaction rate.
Teaching Point: Catalysts are not consumed in the reaction and are regenerated.
CHEM 104 COMPREHENSIVE FINAL EXAM 2026/2027 |
GENERAL CHEMISTRY – PORTAGE LEARNING | EXPERT
VERIFIED | 150 VERIFIED Q&A | DETAILED RATIONALES |
NGN-ALIGNED | PASS GUARANTEED - A+ GRADED
SECTION A: MULTIPLE CHOICE (Questions 1-100)
Instructions: Select the single best answer for each question.
1. Which type of bond is formed by the transfer of electrons between atoms?
• A) Covalent bond
• B) Ionic bond
• C) Metallic bond
• D) Hydrogen bond
Answer: B) Ionic bond
Rationale: An ionic bond is formed by the transfer of electrons from one atom to another, resulting
in the formation of cations and anions. Covalent bonds involve sharing of electrons, metallic bonds
involve a "sea of electrons," and hydrogen bonds are intermolecular forces.
Teaching Point: Ionic bonds typically form between metals and nonmetals. Covalent bonds form
between nonmetals.
2. What is the molecular geometry of methane (CH₄)?
• A) Linear
• B) Trigonal planar
• C) Tetrahedral
• D) Bent
Answer: C) Tetrahedral
Rationale: Methane (CH₄) has a tetrahedral molecular geometry with bond angles of 109.5°. The
central carbon atom has four bonding pairs and no lone pairs.
Teaching Point: VSEPR theory predicts molecular geometry based on the number of bonding and
lone pairs around the central atom.
3. What is the pH of a solution with [H⁺] = 1 × 10⁻⁴ M?
• A) 2
,2
• B) 3
• C) 4
• D) 5
Answer: C) 4
Rationale: pH = -log[H⁺] = -log(1 × 10⁻⁴) = 4.
Teaching Point: pH is a measure of acidity. Lower pH means higher acidity.
4. Which of the following is a strong acid?
• A) HCl
• B) CH₃COOH
• C) H₂CO₃
• D) HF
Answer: A) HCl
Rationale: HCl (hydrochloric acid) is a strong acid that completely dissociates in water. CH₃COOH,
H₂CO₃, and HF are weak acids.
Teaching Point: The six common strong acids are HCl, HBr, HI, HNO₃, H₂SO₄, and HClO₄.
5. What is the oxidation number of oxygen in most compounds?
• A) -1
• B) -2
• C) 0
• D) +2
Answer: B) -2
Rationale: Oxygen typically has an oxidation number of -2 in most compounds (except in peroxides
where it is -1 and in OF₂ where it is +2).
Teaching Point: Oxidation numbers are assigned based on a set of rules.
6. What is the equilibrium constant expression for the reaction aA + bB ⇌ cC + dD?
• A) Keq = [A]^a[B]^b / [C]^c[D]^d
• B) Keq = [C]^c[D]^d / [A]^a[B]^b
• C) Keq = [A][B] / [C][D]
• D) Keq = [C][D] / [A][B]
,3
Answer: B) Keq = [C]^c[D]^d / [A]^a[B]^b
Rationale: The equilibrium constant expression is the ratio of the concentrations of products raised
to their stoichiometric coefficients divided by the concentrations of reactants raised to their
stoichiometric coefficients.
Teaching Point: Pure solids and liquids are not included in the equilibrium constant expression.
7. What is the effect of increasing temperature on the rate of a reaction?
• A) Increases reaction rate
• B) Decreases reaction rate
• C) No effect
• D) Depends on the reaction
Answer: A) Increases reaction rate
Rationale: Increasing temperature increases the kinetic energy of molecules, leading to more
frequent and more energetic collisions, which increases the reaction rate.
Teaching Point: Increasing temperature by 10°C approximately doubles the reaction rate.
8. What is the Arrhenius equation?
• A) k = A e^(-Ea/RT)
• B) k = A e^(Ea/RT)
• C) k = RT e^(-Ea/A)
• D) k = A RT e^(-Ea)
Answer: A) k = A e^(-Ea/RT)
Rationale: The Arrhenius equation relates the rate constant (k) to temperature (T), activation energy
(Ea), and the frequency factor (A).
Teaching Point: The Arrhenius equation shows that k increases with temperature and decreases
with activation energy.
9. What is the pH of a 0.01 M NaOH solution?
• A) 2
• B) 7
• C) 10
• D) 12
Answer: D) 12
, 4
Rationale: NaOH is a strong base, so [OH⁻] = 0.01 M. pOH = -log(0.01) = 2. pH = 14 - 2 = 12.
Teaching Point: Strong bases completely dissociate in water.
10. What is the oxidation number of hydrogen in most compounds?
• A) -1
• B) 0
• C) +1
• D) +2
Answer: C) +1
Rationale: Hydrogen typically has an oxidation number of +1 in most compounds (except in metal
hydrides where it is -1).
Teaching Point: In metal hydrides (e.g., NaH), hydrogen has an oxidation number of -1.
11. Which of the following is a strong base?
• A) NH₃
• B) NaOH
• C) CH₃NH₂
• D) NaHCO₃
Answer: B) NaOH
Rationale: NaOH (sodium hydroxide) is a strong base that completely dissociates in water. NH₃,
CH₃NH₂, and NaHCO₃ are weak bases.
Teaching Point: Strong bases include NaOH, KOH, and Ca(OH)₂.
12. What is the effect of a catalyst on the activation energy?
• A) Lowers activation energy
• B) Raises activation energy
• C) No effect
• D) Changes the equilibrium
Answer: A) Lowers activation energy
Rationale: A catalyst lowers the activation energy by providing an alternative pathway for the
reaction. This increases the reaction rate.
Teaching Point: Catalysts are not consumed in the reaction and are regenerated.
