Free Periodic Properties and Trends MCQs with Answers
606 Periodic Properties and Trends MCQs from Chemistry, each with the correct answer and a written explanation of why it is correct. Free and unlimited, with no account needed.
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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606 questions · page 15 of 31
- A. F
- B. Cl
- C. Br
- D. I
Explanation: F has maximum non-metallic character among the given non-metals.
Correct answer: F- A. F, S and Li
- B. Cl, S and Li
- C. Cl, Se and Na
- D. F, Se and Na
Explanation: In the periodic table, electron affinity generally increases across a period and decreases down a group.
Correct answer: Cl, S and Li- A. Increase in atomic mass
- B. Increase in shielding effect of the intervening electrons
- C. Increase in proton number
- D. Decrease in atomic size
Explanation: Ionization energy is the energy required to remove an electron from the outermost shell of the atom.
Correct answer: Increase in shielding effect of the intervening electrons- A. Atomic radius
- B. Ionization energy
- C. Ionic radius
- D. Hydration energy
Explanation: Polarizability usually refers to the tendency of matter, when subjected to an electric field, to acquire an electric dipole moment in…
Correct answer: Atomic radius- A. Down the Group
- B. Across the Period
- C. Along the d-block
- D. All of these
Explanation: The covalent character 'decreases in groups' as we go from top to bottom.
Correct answer: Down the Group- A. Nuclear charge
- B. Number of electrons
- C. Atomic number
- D. All of these
Explanation: In general, ionization energy increases across a period and decreases down a group.
Correct answer: Nuclear charge- A. 3.4
- B. 4.0
- C. 1.2
- D. 2.6
Explanation: Of the main group elements, fluorine has the highest electronegativity (EN = 4.0), and cesium has the lowest electronegativity (EN =…
Correct answer: 4.0- A. Nitrogen and Phosphorus
- B. Neon and Argon
- C. Lithium and Sodium
- D. Carbon and Silicon
Explanation: So in periods two and three, the highest melting point elements tend to be the metal elements with the most delocalized electrons.In…
Correct answer: Carbon and Silicon- A. Acidity of metal
- B. Polarization power
- C. Basicity of metal
- D. None of these options is correct
Explanation: Metals in lower oxidation states form more ionic and hence more basic oxides/hydroxides,while metals in higher oxidation states form more…
Correct answer: Basicity of metal- A. Group 2A
- B. Group 5A
- C. Both A & B
- D. None of these
Explanation: Correct option is C. Elements in group 2 of the periodic table do not have a high electron affinity.
Correct answer: Both A & B- A. Nuclear charge
- B. Proton number and nuclear charge
- C. Proton number
- D. None of the above
Explanation: Down the group, ionization energy decreases. Even though an increase in nuclear charge should cause an increase in ionization energy, an…
Correct answer: Proton number and nuclear charge- A. Mg²⁺
- B. Na
- C. Al³⁺
- D. Na⁺
Explanation: The size of an ion depends on two factors: its parent atomic size and the charge on the ion.
Correct answer: Al³⁺- A. Divalent cations
- B. Trivalent anions
- C. Divalent anions
- D. Trivalent cations
Explanation: A cation is smaller than the parent atom while an anion is bigger than the parent anion.
Correct answer: Trivalent cations- A. Effective nuclear charge
- B. Shells
- C. Electrons
- D. Screening effect
Explanation: As we move down the group, the screening effect, the number of electrons and the number of shells increase.
Correct answer: Effective nuclear charge- A. 40 pm
- B. 53 pm
- C. 37 pm
- D. 120 pm
Explanation: The atomic radius is a measure of the size of an atom. It is the distance from the nucleus to the outermost shell.
Correct answer: 53 pm- A. 152
- B. 153
- C. 154
- D. 155
Explanation: Option A 152 isotopes have not even atomic and mass numbers. Option B It is also wrong because 153 isotopes have not even atomic and mass…
Correct answer: 154- A. Option A
- B. Option B
- C. Option C
- D. Option D
Explanation: Oxidising power of halogens decreases down the group. Iodine has the least oxidising power, followed by Br2, Cl2 and then F2.
Correct answer: Option B- A. Atomic radius
- B. Melting point
- C. Number of shells (orbits)
- D. Electrical conductivity
Explanation: Across a period, the atomic number increases, which means the number of protons increases in the nucleus.
Correct answer: Number of shells (orbits)- A. More the electropositivity
- B. More the reducing power
- C. Less the metallic character
- D. Bigger the atomic radius
Explanation: Ionization energy is the energy required to remove an electron from a neutral gaseous atom, and it is a measure of the tendency of an…
Correct answer: Less the metallic character- A. 1
- B. 2
- C. 4
- D. 3
Explanation: Carbon has the highest melting point, due to it having 4 strong covalent bonds which require a lot of energy to break.
Correct answer: 3