Question

Give reasons for the following:-
_______________________
1. The size of a CI- ion is greater than the size of a CI atom.
2. Argon atom is bigger than chlorine atom.
3. Ionisation potential of the element increases across a period.
4. Alkali metals are good reducing agents.
_______________________

Don't spam
No copied answer​

Answer 1

Explanation:

1. (1) It is because cl- ions gain one electron to achieve stable configuration and hence is bigger than cl atom. (2) Argon atom is bigger than chlorine atom because argon atom has one more electron than chlorine.
2. Argon atom is bigger than chlorine atom because,Chlorine atom has 3 outermost shells revolving around it and it has seven valence electrons and its valency is 1. But Argon has 4 outermost shells and has the Octet structure. Hence it is stable. So due to addition of a shell argon atom is bigger than chlorine atom.
3. The ionisation potential of the element increases across a period. Atomic size decreases and nuclear charges increases as we move from left to right in a period so the energy required to remove one electron from the valence shell increases from left to right thus ionisation potential increases.
4. Due to low ionization potential and having the smallest nuclear charge they can easily lose an electron. Hence, alkali metals are considered as a powerful reducing agent.

Answer 2

${\underbrace{\mathbb{\orange{answer - }}}}$

• (1) It is because cl- ions gain one electron to achieve stable configuration and hence is bigger than cl atom.
• Argon atom is bigger than chlorine atom because argon atom has one more electron than chlorine.

• 2) Argon atom is bigger than chlorine atom because,Chlorine atom has 3 outermost shells revolving around it and it has seven valence electrons and its valency is 1. But Argon has 4 outermost shells and has the Octet structure. ... So due to addition of a shell argon atom is bigger than chlorine atom.

• 3) The ionisation potential of the element increases across a period. Atomic size decreases and nuclear charges increases as we move from left to right in a period so the energy required to remove one electron from the valence shell increases from left to right thus ionisation potential increases.

• 4) Alkali metals are known as good reducing agents because they have their only one valence electron in their outermost shell. ... Thus, they lose electrons and get oxidized themselves, hence reducing other compounds. Lesser the number of electrons in the valence shell, stronger will be the reducing agent.

______________________

${\underbrace{\mathbb{\orange{i \: hope \: itz \: help \: to \: u}}}}$