CHEMISTRY EXAM PREP
CHEM 103 FINAL EXAM
GENERAL CHEMISTRY I W/ LAB
2026/2027 ACTUAL EXAM TEST BANK A+
WITH REAL EXAM QUESTIONS AND
100% CORRECT VERIFIED ANSWERS
(GUARANTEED PASS!!)
Aligned to Portage Learning CHEM 103 General Chemistry I Objectives • College-Level Chemistry
A+ QUESTIONS 5 SECTIONS 100%
VERIFIED COMPLETE RATIONALES
CATEGORIES
SECTION 1 — Atomic Structure, Periodicity & Electron Configuration
SECTION 2 — Chemical Bonding, Lewis Structures & Molecular Geometry
SECTION 3 — Stoichiometry, Chemical Reactions & Solutions
SECTION 4 — Gases, Thermochemistry & Equilibrium
SECTION 5 — Acids/Bases, Electrochemistry & Laboratory Concepts
Difficulty Level: Intermediate College Chemistry (Application / Analysis)
Question Format: Multiple Choice (A–D) | 1 Mark each
Passing Score: 80% | Total Marks: 50
Aligned to Portage Learning CHEM 103 General Chemistry I W/ Lab
All questions original | Answer key with rationales included
STUVIAACTUALEXAM
CHEM 103 Final Exam General Chemistry I W/ Lab 2026/2027
, CHEM 103 Final Exam: General Chemistry I W/ Lab 2026/2027 STUVIAACTUALEXAM
SECTION 1: Atomic Structure, Periodicity & Electron Configuration
Q1. A student is determining the number of protons, neutrons, and electrons in an atom of ^{35}Cl. The atom has a neutral charge. The
correct composition is:
A. 17 protons, 18 neutrons, 17 electrons
B. 17 protons, 35 neutrons, 17 electrons
C. 18 protons, 17 neutrons, 18 electrons
D. 35 protons, 17 neutrons, 35 electrons
Correct Answer: A
Rationale: Atomic number of Cl is 17, so 17 protons and (for a neutral atom) 17 electrons. Mass number 35 means 35 − 17 = 18 neutrons.
Q2. Two atoms have the same number of protons but different numbers of neutrons. These atoms are best described as:
A. Isotopes of the same element
B. Ions of different elements
C. Allotropes of the same element
D. Molecules with different formulas
Correct Answer: A
Rationale: Isotopes are atoms of the same element (same atomic number/protons) that differ in neutron number and therefore mass number.
Q3. A student writes the electron configuration for a neutral oxygen atom (Z = 8). The correct ground-state configuration is:
A. 1s^{2} 2s^{2} 2p^{4}
B. 1s^{2} 2s^{2} 2p^{6}
C. 1s^{2} 2s^{2} 2p^{3}
D. 1s^{2} 2s^{1} 2p^{5}
Correct Answer: A
Rationale: Oxygen has 8 electrons. Filling order gives 1s^{2} 2s^{2} 2p^{4}. The 2p subshell holds four of the six possible electrons.
Q4. Across a period from left to right, atomic radius generally decreases. The primary reason for this trend is:
A. Increasing effective nuclear charge pulling electrons closer
B. Increasing number of electron shells
C. Decreasing nuclear charge
D. Increasing shielding by core electrons only
Correct Answer: A
Rationale: As protons are added across a period, effective nuclear charge increases while the principal energy level stays the same, drawing the electron
cloud inward.
Q5. A student compares the first ionization energies of Na and Cl. Chlorine has the higher ionization energy primarily because:
A. Chlorine has more electron shells than sodium
B. Sodium has a full valence shell
C. Chlorine has a higher effective nuclear charge and a smaller atomic radius, holding its valence electrons more tightly
D. Chlorine is a metal
Correct Answer: C
Rationale: Chlorine is farther right in the same period; higher Z_eff and smaller size make removal of an electron more difficult than for sodium.
Q6. The electron configuration of a ground-state Fe^{2+} ion is obtained by removing electrons from neutral Fe (Z = 26). The electrons are
removed first from:
A. The 3d orbitals only
B. The 4s orbital, then if needed from 3d
C. The 3p orbitals
D. The 1s orbital
Correct Answer: B
Rationale: For transition-metal cations, the 4s electrons are removed before the 3d electrons. Fe is [Ar] 4s^{2} 3d^{6}; Fe^{2+} is [Ar] 3d^{6}.
Q7. A student is asked why noble gases are generally unreactive. The best explanation is that noble gases:
A. Have the highest atomic masses
B. Possess completely filled valence shells, making them energetically stable
C. Have the lowest ionization energies
D. Exist only as ions in nature
Correct Answer: B
Rationale: A full valence shell (ns^{2} np^{6} for most noble gases) confers high stability, so noble gases have little tendency to gain, lose, or share
electrons.
Page 2
CHEM 103 FINAL EXAM
GENERAL CHEMISTRY I W/ LAB
2026/2027 ACTUAL EXAM TEST BANK A+
WITH REAL EXAM QUESTIONS AND
100% CORRECT VERIFIED ANSWERS
(GUARANTEED PASS!!)
Aligned to Portage Learning CHEM 103 General Chemistry I Objectives • College-Level Chemistry
A+ QUESTIONS 5 SECTIONS 100%
VERIFIED COMPLETE RATIONALES
CATEGORIES
SECTION 1 — Atomic Structure, Periodicity & Electron Configuration
SECTION 2 — Chemical Bonding, Lewis Structures & Molecular Geometry
SECTION 3 — Stoichiometry, Chemical Reactions & Solutions
SECTION 4 — Gases, Thermochemistry & Equilibrium
SECTION 5 — Acids/Bases, Electrochemistry & Laboratory Concepts
Difficulty Level: Intermediate College Chemistry (Application / Analysis)
Question Format: Multiple Choice (A–D) | 1 Mark each
Passing Score: 80% | Total Marks: 50
Aligned to Portage Learning CHEM 103 General Chemistry I W/ Lab
All questions original | Answer key with rationales included
STUVIAACTUALEXAM
CHEM 103 Final Exam General Chemistry I W/ Lab 2026/2027
, CHEM 103 Final Exam: General Chemistry I W/ Lab 2026/2027 STUVIAACTUALEXAM
SECTION 1: Atomic Structure, Periodicity & Electron Configuration
Q1. A student is determining the number of protons, neutrons, and electrons in an atom of ^{35}Cl. The atom has a neutral charge. The
correct composition is:
A. 17 protons, 18 neutrons, 17 electrons
B. 17 protons, 35 neutrons, 17 electrons
C. 18 protons, 17 neutrons, 18 electrons
D. 35 protons, 17 neutrons, 35 electrons
Correct Answer: A
Rationale: Atomic number of Cl is 17, so 17 protons and (for a neutral atom) 17 electrons. Mass number 35 means 35 − 17 = 18 neutrons.
Q2. Two atoms have the same number of protons but different numbers of neutrons. These atoms are best described as:
A. Isotopes of the same element
B. Ions of different elements
C. Allotropes of the same element
D. Molecules with different formulas
Correct Answer: A
Rationale: Isotopes are atoms of the same element (same atomic number/protons) that differ in neutron number and therefore mass number.
Q3. A student writes the electron configuration for a neutral oxygen atom (Z = 8). The correct ground-state configuration is:
A. 1s^{2} 2s^{2} 2p^{4}
B. 1s^{2} 2s^{2} 2p^{6}
C. 1s^{2} 2s^{2} 2p^{3}
D. 1s^{2} 2s^{1} 2p^{5}
Correct Answer: A
Rationale: Oxygen has 8 electrons. Filling order gives 1s^{2} 2s^{2} 2p^{4}. The 2p subshell holds four of the six possible electrons.
Q4. Across a period from left to right, atomic radius generally decreases. The primary reason for this trend is:
A. Increasing effective nuclear charge pulling electrons closer
B. Increasing number of electron shells
C. Decreasing nuclear charge
D. Increasing shielding by core electrons only
Correct Answer: A
Rationale: As protons are added across a period, effective nuclear charge increases while the principal energy level stays the same, drawing the electron
cloud inward.
Q5. A student compares the first ionization energies of Na and Cl. Chlorine has the higher ionization energy primarily because:
A. Chlorine has more electron shells than sodium
B. Sodium has a full valence shell
C. Chlorine has a higher effective nuclear charge and a smaller atomic radius, holding its valence electrons more tightly
D. Chlorine is a metal
Correct Answer: C
Rationale: Chlorine is farther right in the same period; higher Z_eff and smaller size make removal of an electron more difficult than for sodium.
Q6. The electron configuration of a ground-state Fe^{2+} ion is obtained by removing electrons from neutral Fe (Z = 26). The electrons are
removed first from:
A. The 3d orbitals only
B. The 4s orbital, then if needed from 3d
C. The 3p orbitals
D. The 1s orbital
Correct Answer: B
Rationale: For transition-metal cations, the 4s electrons are removed before the 3d electrons. Fe is [Ar] 4s^{2} 3d^{6}; Fe^{2+} is [Ar] 3d^{6}.
Q7. A student is asked why noble gases are generally unreactive. The best explanation is that noble gases:
A. Have the highest atomic masses
B. Possess completely filled valence shells, making them energetically stable
C. Have the lowest ionization energies
D. Exist only as ions in nature
Correct Answer: B
Rationale: A full valence shell (ns^{2} np^{6} for most noble gases) confers high stability, so noble gases have little tendency to gain, lose, or share
electrons.
Page 2
