Which of the following elements has maximum metallic character ?
Li
N
Na
P
Which of the following elements has maximum metallic character ?
Li
N
Na
P
The correct option is C Na
Metallic character
The tendency of an element to remove an electron in its neutral state is called its metallic character. Therefore, elements that remove electrons easily are more metallic. The metallic character of the elements decreases across a period because the effective nuclear charge of the atom decreases. As the nuclear charge increases, the electrons are more bound to the nucleus thus becoming more difficult for removal.
The metallic character decreases down a group because of the decrease in the effective nuclear charge due to the increase in number shells.
Therefore, alkali metals will have the highest metallic character in their respective period and the metallic character decreases down the group.
Explanation for wrong answers
(A) Lithium (Li) belongs to the alkali metal group. But it is belongs to the second group and therefore, the metallic character will be less than Sodium (Na). Therefore, option (A) is incorrect.
(B) Nitrogen belongs to the 15th group. Its electronic configuration is 2,5. It belongs to the second group and it accepts three electrons to obtain stable electronic configuration. There, Nitrogen is a non-metal ad its metallic character is very low. Option (B) is incorrect.
(D) Phosphorus (P) is a non- metal belonging to the third period and 15th group. Similar to Nitrogen, it accepts three electrons to get octet configuration. Therefore, it is difficult to remove electrons from Phosphorus. Option (D) is wrong.
Explanation for correct answer
(C) Sodium is an alkali metal. Therefore, it has high metallic character. Since the metallic character increases down a group, Sodium in the third group will have higher electronegativity than Lithium in the second group. Therefore, the metallic character among is highest for Sodium among the given elements.
The correct answer is (C) Na
Na
Metallic character
The tendency of an element to remove an electron in its neutral state is called its metallic character. Therefore, elements that remove electrons easily are more metallic. The metallic character of the elements decreases across a period because the effective nuclear charge of the atom decreases. As the nuclear charge increases, the electrons are more bound to the nucleus thus becoming more difficult for removal.
The metallic character decreases down a group because of the decrease in the effective nuclear charge due to the increase in number shells.
Therefore, alkali metals will have the highest metallic character in their respective period and the metallic character decreases down the group.
Explanation for wrong answers
(A) Lithium (Li) belongs to the alkali metal group. But it is belongs to the second group and therefore, the metallic character will be less than Sodium (Na). Therefore, option (A) is incorrect.
(B) Nitrogen belongs to the 15th group. Its electronic configuration is 2,5. It belongs to the second group and it accepts three electrons to obtain stable electronic configuration. There, Nitrogen is a non-metal ad its metallic character is very low. Option (B) is incorrect.
(D) Phosphorus (P) is a non- metal belonging to the third period and 15th group. Similar to Nitrogen, it accepts three electrons to get octet configuration. Therefore, it is difficult to remove electrons from Phosphorus. Option (D) is wrong.
Explanation for correct answer
(C) Sodium is an alkali metal. Therefore, it has high metallic character. Since the metallic character increases down a group, Sodium in the third group will have higher electronegativity than Lithium in the second group. Therefore, the metallic character among is highest for Sodium among the given elements.
The correct answer is (C) Na
