Inorganic Chemistry - Periodicity Practice Questions
A-Levels · A-Level Chemistry · 130 free MCQs with instant results and detailed explanations.
130
Total
33
Easy
69
Medium
28
Hard
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Sample Questions from Inorganic Chemistry - Periodicity
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Q1
Easy
As you move from left to right across a period in the periodic table, how does atomic radius typically change?
A.
Increases
B.
Decreases
C.
Remains constant
D.
Increases then decreases
Show Answer & Explanation
Correct Answer: B
As you move from left to right across a period, the atomic radius decreases due to the increase in nuclear charge which pulls the electrons closer to the nucleus.
Q2
Easy
Which of the following elements has the smallest first ionization energy?
A.
Sodium
B.
Aluminium
C.
Phosphorus
D.
Magnesium
Show Answer & Explanation
Correct Answer: A
Sodium has the smallest first ionization energy among the options because it is located in Group 1, where elements have lower ionization energies compared to those in other groups.
Q3
Easy
Which of the following trends is observed in the atomic radius as you move down a group in the periodic table?
A.
The atomic radius decreases.
B.
The atomic radius increases.
C.
The atomic radius remains constant.
D.
The atomic radius fluctuates.
Show Answer & Explanation
Correct Answer: B
As you move down a group, additional electron shells are added, which increases the distance between the nucleus and the outermost electrons, leading to a larger atomic radius.
Q4
Medium
Which of the following elements exhibits the highest ionization energy in the third period of the periodic table?
A.
Sodium (Na)
B.
Magnesium (Mg)
C.
Chlorine (Cl)
D.
Silicon (Si)
Show Answer & Explanation
Correct Answer: C
Chlorine has the highest ionization energy due to its small atomic size and high effective nuclear charge, leading to a stronger attraction between the nucleus and the outer electrons compared to the other elements listed.
Q5
Medium
What trend is observed in the electronegativity of elements as you move across a period from left to right?
A.
Electronegativity decreases
B.
Electronegativity increases
C.
Electronegativity remains constant
D.
Electronegativity varies randomly
Show Answer & Explanation
Correct Answer: B
Electronegativity tends to increase across a period due to the increasing nuclear charge, which attracts the bonding electrons more strongly as the atomic radius decreases.
Q6
Medium
Which of the following oxides would most likely form a basic solution when dissolved in water?
A.
SiO2
B.
Na2O
C.
Cl2O7
D.
MgO
Show Answer & Explanation
Correct Answer: D
Magnesium oxide (MgO) is a basic oxide that reacts with water to form magnesium hydroxide, which is alkaline, thereby resulting in a basic solution.
Q7
Medium
As you move down Group 17, the halogens, which of the following trends is observed?
A.
Decreasing atomic radius
B.
Increasing melting point
C.
Decreasing reactivity
D.
Increasing ionization energy
Show Answer & Explanation
Correct Answer: B
The melting point of halogens increases down the group due to increasing molecular size and van der Waals forces, leading to stronger intermolecular attractions.
Q8
Hard
Consider the trend in atomic radius across Period 3. Which of the following statements is true?
A.
The atomic radius increases from sodium to chlorine.
B.
The atomic radius decreases from sodium to chlorine.
C.
The atomic radius remains constant across Period 3.
D.
The atomic radius first increases and then decreases across Period 3.
Show Answer & Explanation
Correct Answer: B
Across Period 3, the atomic radius decreases from sodium to chlorine due to the increase in nuclear charge, which pulls the electrons closer to the nucleus, resulting in a smaller atomic size.
Q9
Hard
Which of the following elements exhibits the highest ionization energy in its respective group in the periodic table?
A.
Fluorine (F)
B.
Chlorine (Cl)
C.
Bromine (Br)
D.
Iodine (I)
Show Answer & Explanation
Correct Answer: A
Fluorine has the highest ionization energy among its group due to its small atomic size and high effective nuclear charge, which makes it more difficult to remove an electron compared to the other halogens.
Q10
Hard
In the context of periodicity, which of the following elements would you expect to have the largest atomic radius?
A.
Na (Sodium)
B.
K (Potassium)
C.
Li (Lithium)
D.
Rb (Rubidium)
Show Answer & Explanation
Correct Answer: D
Rubidium has the largest atomic radius among the given options because atomic radius increases down a group due to the addition of electron shells, which outweighs the increase in nuclear charge.
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Inorganic Chemistry - Periodicity — A-Levels A-Level Chemistry Practice Questions Online
This page contains 130 practice MCQs for the chapter Inorganic Chemistry - Periodicity in A-Levels A-Level Chemistry. The questions are organized by difficulty — 33 easy, 69 medium, 28 hard — so you can choose the right level for your preparation.
Every question includes a detailed explanation to help you understand the concept, not just memorize answers. Take a timed quiz to simulate exam conditions, or practice at your own pace with no time limit.