- Which of the following has the lowest ionization energy?
a) Fluorine (F)
b) Nitrogen (N)
c) Oxygen (O)
d) Phosphorus (P)
Answer: d) Phosphorus (P)
Explanation: Ionization energy generally decreases down a group and increases across a period. Phosphorus has the lowest ionization energy among the elements listed because it is farther down in Group 15.
- Which of the following has the highest electron affinity?
a) Phosphorus (P)
b) Sulfur (S)
c) Oxygen (O)
d) Nitrogen (N)
Answer: b) Sulfur (S)
Explanation: Sulfur has a higher electron affinity compared to nitrogen and phosphorus because it is more electronegative and is more likely to gain an electron. Oxygen’s smaller size increases electron-electron repulsion, reducing its electron affinity.
- Which of the following halogens has the lowest melting point?
a) Fluorine (F)
b) Chlorine (Cl)
c) Bromine (Br)
d) Iodine (I)
Answer: a) Fluorine (F)
Explanation: Fluorine, being the smallest halogen and a diatomic gas at room temperature, has the lowest melting point compared to chlorine, bromine, and iodine, which are found as gases, liquids, and solids, respectively, at room temperature.
- Which of the following elements has the highest metallic character?
a) Carbon (C)
b) Silicon (Si)
c) Tin (Sn)
d) Lead (Pb)
Answer: d) Lead (Pb)
Explanation: Metallic character increases down a group. Lead, being the farthest down in Group 14, has the highest metallic character among the elements listed.
- Which of the following has the highest electronegativity?
a) Boron (B)
b) Carbon (C)
c) Nitrogen (N)
d) Oxygen (O)
Answer: d) Oxygen (O)
Explanation: Electronegativity increases across a period. Oxygen, being the farthest to the right, has the highest electronegativity of the elements listed.
- Which of the following elements has the smallest atomic size?
a) Lithium (Li)
b) Sodium (Na)
c) Potassium (K)
d) Cesium (Cs)
Answer: a) Lithium (Li)
Explanation: Atomic size increases down the group in alkali metals. Lithium, at the top of Group 1, has the smallest atomic size.
- Which of the following elements has the lowest first ionization energy?
a) Hydrogen (H)
b) Sodium (Na)
c) Potassium (K)
d) Rubidium (Rb)
Answer: d) Rubidium (Rb)
Explanation: Ionization energy decreases down a group. Rubidium, being the farthest down in Group 1 among the listed elements, has the lowest first ionization energy.
- Which of the following elements has the highest first ionization energy?
a) Helium (He)
b) Neon (Ne)
c) Argon (Ar)
d) Krypton (Kr)
Answer: a) Helium (He)
Explanation: Helium has the highest first ionization energy in the periodic table due to its small size and high effective nuclear charge, which tightly holds its electrons.
- Which of the following elements forms an acidic oxide?
a) Magnesium (Mg)
b) Sodium (Na)
c) Phosphorus (P)
d) Calcium (Ca)
Answer: c) Phosphorus (P)
Explanation: Phosphorus forms acidic oxides like P₄O₁₀, which react with water to produce phosphoric acid. Magnesium, sodium, and calcium form basic oxides.
- Which of the following halogens has the highest boiling point?
a) Fluorine (F)
b) Chlorine (Cl)
c) Bromine (Br)
d) Iodine (I)
Answer: d) Iodine (I)
Explanation: Iodine, being a solid at room temperature, has the highest boiling point compared to fluorine, chlorine, and bromine, which are gases or liquids at room temperature.
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