ACS CHEMISTRY GENERAL EXAM
110+ (Fully Updated 2026) Exam Questions + Verified & Rationalized
Answers | A+ Graded
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📋 DOCUMENT OVERVIEW 113 Qs
This document, the ACS Chemistry General Exam, contains 113 questions with detailed explanations
covering various topics in general chemistry. Specifically, it covers atomic structure, electron
configuration, isotope properties, atomic number, nuclear particles, atomic models, hybridization,
covalent bonds, and energy requirements in chemical reactions. The document provides a
comprehensive review resource, offering correct answers and detailed rationales for each question,
allowing students to study, review, and understand key chemistry concepts for exam preparation.
✓ Verified Answers ✓ Exam Ready ✓ Study Guide
Trusted by thousands of students and professionals worldwide
EXAM QUESTIONS
QUESTION 1
What is the electron configuration of an element with a specific number of protons that defines its
position in the periodic table?
A) 1s² 2s² 2p⁶
B) 2s² 2p⁶ 3s² 3p⁶
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
D) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁷
CORRECT ANSWER
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
RATIONALE: The electron configuration provided in option C is characteristic of an element with a certain number of
protons, which defines its position in the periodic table. Options A and B are electron configurations for elements with a
lower number of protons. Option D is an electron configuration for an element with a different number of protons,
resulting in an incorrect atomic structure.
QUESTION 2
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, A chemist should identify that the numerical value representing the total amount of protons and
neutrons in an atom's nucleus is determined by the following equation: ______.
A) # of electrons + neutrons
B) # of protons + electrons
C) # of neutrons + electrons
D) # of protons + neutrons
CORRECT ANSWER
D) # of protons + neutrons
RATIONALE: The mass number, or total amount of protons and neutrons in an atom's nucleus, is calculated by adding
the number of protons to the number of neutrons. Options A, B, and C include electrons in the calculation, which is
incorrect.
QUESTION 3
What is the difference in mass between a neon isotope with a mass number of 20 and its atomic
number?
A) 1 amu
B) 2 amu
C) 4 amu
D) 6 amu
CORRECT ANSWER
B) 2 amu
RATIONALE: The atomic number represents the number of protons in an atom. The difference in mass is found by
subtracting the atomic number from the mass number. In this case, 20 - 18 = 2 amu.
QUESTION 4
Which of the following is a characteristic of atoms having the same number of protons but varying
numbers of neutrons?
A) Different electron configurations
B) Isotopes
C) Different atomic numbers
D) Ionic compounds
CORRECT ANSWER
B) Isotopes
RATIONALE: Isotopes are atoms of the same element with the same number of protons (atomic number) but differing
numbers of neutrons, which results in varying atomic masses. This characteristic is distinct from atomic number,
electron configuration, and ionic compound formation.
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, QUESTION 5
What is the impact on an atom's atomic number when a particular particle is lost from the nucleus?
A) The atomic number remains unchanged.
B) The atomic number increases by 1.
C) The atomic number decreases by 1.
D) The atomic number remains the same as the preceding element in the periodic table.
CORRECT ANSWER
A) The atomic number remains unchanged.
RATIONALE: The atomic number of an atom is determined by the number of protons in its nucleus. Since a neutron has
no charge, losing one does not alter the atomic number, making option A the correct choice. Options B and C are
incorrect because they imply a change in the number of protons, while option D is incorrect as the atomic number is not
directly related to the preceding element in the periodic table.
QUESTION 6
Which model of the atom is supported by the experimental evidence from alpha particle scattering,
which revealed most particles passing through a metal foil target with minimal deflection?
A) The lattice model, where atoms are arranged in a rigid structure
B) The planetary model, where atoms have a small, dense nucleus surrounded by electrons
C) The particle-in-a-box model, where electrons occupy specific energy levels within an atom
D) The sea of electrons model, where electrons are distributed throughout the atom
CORRECT ANSWER
B) The planetary model, where atoms have a small, dense nucleus surrounded by electrons
RATIONALE: The experimental evidence from alpha particle scattering supports the planetary model of the atom, which
includes a small, dense nucleus surrounded by electrons. This model explains the minimal deflection of alpha particles
as they passed through the metal foil target, suggesting that most particles interacted with the sparse, low-mass
electrons rather than the dense, positively charged nucleus.
QUESTION 7
A student calculates the valence shell configuration of an atom and should conclude that it belongs to
which main group of elements in the periodic table?
A) IIA - alkaline earth metals
B) IA - alkali metals
C) VIIA - halogens
D) VIIB - transition metals
CORRECT ANSWER
B) IA - alkali metals
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, RATIONALE: The correct answer is IA - alkali metals because the given valence shell configuration, 1s1, indicates a
single electron in the outermost energy level, characteristic of the alkali metals. The incorrect options are IIA - alkaline
earth metals (too many electrons), VIIA - halogens (correct number but wrong type), and VIIB - transition metals
(incorrect number of electrons).
QUESTION 8
What is the pH of a solution containing a particular wavelength of light, and how would this
wavelength affect the concentration of hydrogen ions?
A) The pH would be neutral, and the wavelength would have no effect on hydrogen ion concentration.
B) The pH would decrease as the wavelength of light increases.
C) The pH would increase as the wavelength of light decreases.
D) The pH would remain unchanged, regardless of the wavelength of light.
CORRECT ANSWER
C) The pH would increase as the wavelength of light decreases.
RATIONALE: The correct answer is C) The pH would increase as the wavelength of light decreases. This is because the
energy of a photon is inversely proportional to its wavelength. A lower wavelength corresponds to a higher energy
photon, which can lead to increased ionization of water molecules (H2O) and, subsequently, an increase in hydrogen ion
concentration. This would decrease the pH of the solution.
QUESTION 9
In which of the following does an increase in photon frequency occur, resulting in a change to its
associated property?
A) The photon's momentum increases while its energy remains constant
B) The photon's wavelength becomes longer while its energy remains unchanged
C) A shift to a lower-energy state is observed in the photon
D) The photon's wavelength is inversely proportional to its frequency
CORRECT ANSWER
D) The photon's wavelength is inversely proportional to its frequency
RATIONALE: An increase in photon frequency is directly related to a decrease in its wavelength. According to the wave-
particle duality principle, the energy (E) of a photon is directly proportional to its frequency (f): E = hf, where h is
Planck's constant. Since energy and frequency are directly related, an increase in frequency results in an increase in
energy.
QUESTION 10
Which element has the highest energy released when transitioning from the ground state to the first
excited state?
A) Hydrogen (H)
B) Helium (He)
Trusted by thousands of students and professionals worldwide Page 4 of 43
110+ (Fully Updated 2026) Exam Questions + Verified & Rationalized
Answers | A+ Graded
100% Guarantee Pass
📋 DOCUMENT OVERVIEW 113 Qs
This document, the ACS Chemistry General Exam, contains 113 questions with detailed explanations
covering various topics in general chemistry. Specifically, it covers atomic structure, electron
configuration, isotope properties, atomic number, nuclear particles, atomic models, hybridization,
covalent bonds, and energy requirements in chemical reactions. The document provides a
comprehensive review resource, offering correct answers and detailed rationales for each question,
allowing students to study, review, and understand key chemistry concepts for exam preparation.
✓ Verified Answers ✓ Exam Ready ✓ Study Guide
Trusted by thousands of students and professionals worldwide
EXAM QUESTIONS
QUESTION 1
What is the electron configuration of an element with a specific number of protons that defines its
position in the periodic table?
A) 1s² 2s² 2p⁶
B) 2s² 2p⁶ 3s² 3p⁶
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
D) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁷
CORRECT ANSWER
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
RATIONALE: The electron configuration provided in option C is characteristic of an element with a certain number of
protons, which defines its position in the periodic table. Options A and B are electron configurations for elements with a
lower number of protons. Option D is an electron configuration for an element with a different number of protons,
resulting in an incorrect atomic structure.
QUESTION 2
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, A chemist should identify that the numerical value representing the total amount of protons and
neutrons in an atom's nucleus is determined by the following equation: ______.
A) # of electrons + neutrons
B) # of protons + electrons
C) # of neutrons + electrons
D) # of protons + neutrons
CORRECT ANSWER
D) # of protons + neutrons
RATIONALE: The mass number, or total amount of protons and neutrons in an atom's nucleus, is calculated by adding
the number of protons to the number of neutrons. Options A, B, and C include electrons in the calculation, which is
incorrect.
QUESTION 3
What is the difference in mass between a neon isotope with a mass number of 20 and its atomic
number?
A) 1 amu
B) 2 amu
C) 4 amu
D) 6 amu
CORRECT ANSWER
B) 2 amu
RATIONALE: The atomic number represents the number of protons in an atom. The difference in mass is found by
subtracting the atomic number from the mass number. In this case, 20 - 18 = 2 amu.
QUESTION 4
Which of the following is a characteristic of atoms having the same number of protons but varying
numbers of neutrons?
A) Different electron configurations
B) Isotopes
C) Different atomic numbers
D) Ionic compounds
CORRECT ANSWER
B) Isotopes
RATIONALE: Isotopes are atoms of the same element with the same number of protons (atomic number) but differing
numbers of neutrons, which results in varying atomic masses. This characteristic is distinct from atomic number,
electron configuration, and ionic compound formation.
Trusted by thousands of students and professionals worldwide Page 2 of 43
, QUESTION 5
What is the impact on an atom's atomic number when a particular particle is lost from the nucleus?
A) The atomic number remains unchanged.
B) The atomic number increases by 1.
C) The atomic number decreases by 1.
D) The atomic number remains the same as the preceding element in the periodic table.
CORRECT ANSWER
A) The atomic number remains unchanged.
RATIONALE: The atomic number of an atom is determined by the number of protons in its nucleus. Since a neutron has
no charge, losing one does not alter the atomic number, making option A the correct choice. Options B and C are
incorrect because they imply a change in the number of protons, while option D is incorrect as the atomic number is not
directly related to the preceding element in the periodic table.
QUESTION 6
Which model of the atom is supported by the experimental evidence from alpha particle scattering,
which revealed most particles passing through a metal foil target with minimal deflection?
A) The lattice model, where atoms are arranged in a rigid structure
B) The planetary model, where atoms have a small, dense nucleus surrounded by electrons
C) The particle-in-a-box model, where electrons occupy specific energy levels within an atom
D) The sea of electrons model, where electrons are distributed throughout the atom
CORRECT ANSWER
B) The planetary model, where atoms have a small, dense nucleus surrounded by electrons
RATIONALE: The experimental evidence from alpha particle scattering supports the planetary model of the atom, which
includes a small, dense nucleus surrounded by electrons. This model explains the minimal deflection of alpha particles
as they passed through the metal foil target, suggesting that most particles interacted with the sparse, low-mass
electrons rather than the dense, positively charged nucleus.
QUESTION 7
A student calculates the valence shell configuration of an atom and should conclude that it belongs to
which main group of elements in the periodic table?
A) IIA - alkaline earth metals
B) IA - alkali metals
C) VIIA - halogens
D) VIIB - transition metals
CORRECT ANSWER
B) IA - alkali metals
Trusted by thousands of students and professionals worldwide Page 3 of 43
, RATIONALE: The correct answer is IA - alkali metals because the given valence shell configuration, 1s1, indicates a
single electron in the outermost energy level, characteristic of the alkali metals. The incorrect options are IIA - alkaline
earth metals (too many electrons), VIIA - halogens (correct number but wrong type), and VIIB - transition metals
(incorrect number of electrons).
QUESTION 8
What is the pH of a solution containing a particular wavelength of light, and how would this
wavelength affect the concentration of hydrogen ions?
A) The pH would be neutral, and the wavelength would have no effect on hydrogen ion concentration.
B) The pH would decrease as the wavelength of light increases.
C) The pH would increase as the wavelength of light decreases.
D) The pH would remain unchanged, regardless of the wavelength of light.
CORRECT ANSWER
C) The pH would increase as the wavelength of light decreases.
RATIONALE: The correct answer is C) The pH would increase as the wavelength of light decreases. This is because the
energy of a photon is inversely proportional to its wavelength. A lower wavelength corresponds to a higher energy
photon, which can lead to increased ionization of water molecules (H2O) and, subsequently, an increase in hydrogen ion
concentration. This would decrease the pH of the solution.
QUESTION 9
In which of the following does an increase in photon frequency occur, resulting in a change to its
associated property?
A) The photon's momentum increases while its energy remains constant
B) The photon's wavelength becomes longer while its energy remains unchanged
C) A shift to a lower-energy state is observed in the photon
D) The photon's wavelength is inversely proportional to its frequency
CORRECT ANSWER
D) The photon's wavelength is inversely proportional to its frequency
RATIONALE: An increase in photon frequency is directly related to a decrease in its wavelength. According to the wave-
particle duality principle, the energy (E) of a photon is directly proportional to its frequency (f): E = hf, where h is
Planck's constant. Since energy and frequency are directly related, an increase in frequency results in an increase in
energy.
QUESTION 10
Which element has the highest energy released when transitioning from the ground state to the first
excited state?
A) Hydrogen (H)
B) Helium (He)
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