Chemistry 2026/2027 Exam Test Bank:
Periodic Trends, Atomic Structure, Quantum
Numbers & Electron Configurations | 105
Practice Questions with Answers
Description:
Master chemistry periodic trends and atomic structure with this comprehensive 2026/2027
examination test bank featuring 105 exam-style questions covering ionization energy,
electronegativity, atomic radius, electron configurations, quantum numbers, VSEPR
theory, and isotope calculations. This university-level study guide includes multiple-choice,
true/false, matching, short-answer, and calculation problems with detailed explanations for every
answer. Aligned with 2026/2027 academic standards, this resource is ideal for exam preparation,
study guides, and digital learning platforms. Whether you are reviewing for final exams or
building foundational chemistry knowledge, this test bank delivers targeted practice.
Download now and boost your exam confidence with this essential chemistry revision tool for
2026/2027.
, Chemistry Periodic Trends Exam Bank 2026/2027
SECTION A: PERIODIC TABLE ORGANIZATION AND FAMILIES
Question 1
What is the group number of the alkaline earth metals?
A. 1
B. 2
C. 17
D. 18
Answer: B
Explanation: The alkaline earth metals are located in Group 2 of the periodic table. This group
includes beryllium, magnesium, calcium, strontium, barium, and radium. These elements are
characterized by having two valence electrons and forming +2 ions.
Question 2
The family name for elements in Group 17 is:
A. Alkali metals
B. Noble gases
C. Halogens
D. Chalcogens
Answer: C
Explanation: Group 17 elements are known as halogens. This family includes fluorine, chlorine,
bromine, iodine, and astatine. The term "halogen" derives from Greek roots meaning "salt-
forming," reflecting their tendency to react with metals to form salts.
Question 3
Which of the following correctly describes the noble gas family?
A. High boiling points and highly reactive
B. Low boiling points and highly reactive
,C. High boiling points and unreactive
D. Low boiling points and unreactive
Answer: D
Explanation: Noble gases are characterised by low boiling points due to weak London
dispersion forces between their atoms. They are chemically unreactive because their valence
electron shells are completely filled, resulting in high ionization energies and negligible electron
affinity.
Question 4
Which statement correctly describes the arrangement of elements A, B, and C in the periodic
table? Element A bursts into pink flames when it dissolves in water. Element B sizzles slightly
when it dissolves in water. Element C sizzles and sometimes burns when it dissolves in water.
A. A is highest, B is lowest, C is in between
B. B is highest, A is lowest, C is in between
C. C is highest, A is lowest, B is in between
D. A is highest, C is lowest, B is in between
Answer: B
Explanation: The reactivity with water indicates these are alkali metals. Reactivity increases
down the group as atomic radius increases and ionization energy decreases. The least reactive
(B) would be highest in the group, the most reactive (A) would be lowest, with C in the middle
position.
SECTION B: PERIODIC TRENDS AND PROPERTIES
Question 5
Electronegativity is defined as:
A. The energy required to remove an electron from an atom
B. The energy released when an atom accepts an electron
C. The ability of an atom to attract electrons towards itself in a chemical bond
D. The tendency of an atom to lose electrons during chemical reactions
, Answer: C
Explanation: Electronegativity quantifies an atom's ability to attract shared electrons in a
chemical bond. This property, first systematised by Linus Pauling, influences bond polarity and
molecular behaviour. Higher electronegativity values indicate stronger electron-attracting
capability.
Question 6
Which of the following best describes the general trend in ionization energy from left to right
across a period?
A. Decreases due to increasing atomic radius
B. Increases due to decreasing atomic radius
C. Remains constant due to constant nuclear charge
D. Fluctuates randomly due to electron shielding
Answer: B
Explanation: Ionization energy increases from left to right across a period because atomic
radius decreases. This occurs because nuclear charge increases while the number of principal
energy levels remains constant, strengthening the nucleus's hold on valence electrons.
Question 7
The difference between ionization energy and electron affinity is that:
A. Ionization energy involves electron gain while electron affinity involves electron loss
B. Ionization energy is always positive while electron affinity is always negative
C. Ionization energy is the energy required to remove an electron, while electron affinity is the
energy change when an atom accepts an electron
D. Ionization energy decreases across a period while electron affinity increases
Answer: C
Explanation: Ionization energy measures the energy needed to remove an electron from a
gaseous atom. Electron affinity measures the energy change (usually released) when a gaseous
Periodic Trends, Atomic Structure, Quantum
Numbers & Electron Configurations | 105
Practice Questions with Answers
Description:
Master chemistry periodic trends and atomic structure with this comprehensive 2026/2027
examination test bank featuring 105 exam-style questions covering ionization energy,
electronegativity, atomic radius, electron configurations, quantum numbers, VSEPR
theory, and isotope calculations. This university-level study guide includes multiple-choice,
true/false, matching, short-answer, and calculation problems with detailed explanations for every
answer. Aligned with 2026/2027 academic standards, this resource is ideal for exam preparation,
study guides, and digital learning platforms. Whether you are reviewing for final exams or
building foundational chemistry knowledge, this test bank delivers targeted practice.
Download now and boost your exam confidence with this essential chemistry revision tool for
2026/2027.
, Chemistry Periodic Trends Exam Bank 2026/2027
SECTION A: PERIODIC TABLE ORGANIZATION AND FAMILIES
Question 1
What is the group number of the alkaline earth metals?
A. 1
B. 2
C. 17
D. 18
Answer: B
Explanation: The alkaline earth metals are located in Group 2 of the periodic table. This group
includes beryllium, magnesium, calcium, strontium, barium, and radium. These elements are
characterized by having two valence electrons and forming +2 ions.
Question 2
The family name for elements in Group 17 is:
A. Alkali metals
B. Noble gases
C. Halogens
D. Chalcogens
Answer: C
Explanation: Group 17 elements are known as halogens. This family includes fluorine, chlorine,
bromine, iodine, and astatine. The term "halogen" derives from Greek roots meaning "salt-
forming," reflecting their tendency to react with metals to form salts.
Question 3
Which of the following correctly describes the noble gas family?
A. High boiling points and highly reactive
B. Low boiling points and highly reactive
,C. High boiling points and unreactive
D. Low boiling points and unreactive
Answer: D
Explanation: Noble gases are characterised by low boiling points due to weak London
dispersion forces between their atoms. They are chemically unreactive because their valence
electron shells are completely filled, resulting in high ionization energies and negligible electron
affinity.
Question 4
Which statement correctly describes the arrangement of elements A, B, and C in the periodic
table? Element A bursts into pink flames when it dissolves in water. Element B sizzles slightly
when it dissolves in water. Element C sizzles and sometimes burns when it dissolves in water.
A. A is highest, B is lowest, C is in between
B. B is highest, A is lowest, C is in between
C. C is highest, A is lowest, B is in between
D. A is highest, C is lowest, B is in between
Answer: B
Explanation: The reactivity with water indicates these are alkali metals. Reactivity increases
down the group as atomic radius increases and ionization energy decreases. The least reactive
(B) would be highest in the group, the most reactive (A) would be lowest, with C in the middle
position.
SECTION B: PERIODIC TRENDS AND PROPERTIES
Question 5
Electronegativity is defined as:
A. The energy required to remove an electron from an atom
B. The energy released when an atom accepts an electron
C. The ability of an atom to attract electrons towards itself in a chemical bond
D. The tendency of an atom to lose electrons during chemical reactions
, Answer: C
Explanation: Electronegativity quantifies an atom's ability to attract shared electrons in a
chemical bond. This property, first systematised by Linus Pauling, influences bond polarity and
molecular behaviour. Higher electronegativity values indicate stronger electron-attracting
capability.
Question 6
Which of the following best describes the general trend in ionization energy from left to right
across a period?
A. Decreases due to increasing atomic radius
B. Increases due to decreasing atomic radius
C. Remains constant due to constant nuclear charge
D. Fluctuates randomly due to electron shielding
Answer: B
Explanation: Ionization energy increases from left to right across a period because atomic
radius decreases. This occurs because nuclear charge increases while the number of principal
energy levels remains constant, strengthening the nucleus's hold on valence electrons.
Question 7
The difference between ionization energy and electron affinity is that:
A. Ionization energy involves electron gain while electron affinity involves electron loss
B. Ionization energy is always positive while electron affinity is always negative
C. Ionization energy is the energy required to remove an electron, while electron affinity is the
energy change when an atom accepts an electron
D. Ionization energy decreases across a period while electron affinity increases
Answer: C
Explanation: Ionization energy measures the energy needed to remove an electron from a
gaseous atom. Electron affinity measures the energy change (usually released) when a gaseous
