Which of the following elements (shown as Bohr models) would have the lowest ionization energy?
Element A
Element B
Element a
Element D
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A
Element A
B
Element B
С
Element C
D
Element D

Element D would have the lowest ionization.

(D) is correct option

Explanation:

Given that,

Number of electron in element A = 17

Number of electron in element B = 3

Number of electron in element C = 18

Number of electron in element D = 11

We know that,

The name of element A is chlorine which have 17 electron.

The name of element B is lithium which have 3 electron.

The name of element C is argon which have 18 electron.

The name of element D is sodium which have 11 electron.

We know that,

The ionization energy of the element decreases from up to down in group and increases from left to right in a period.

We need to find the element would have the lowest ionization

Using periodic table

According to periodic table the lowest Ionization energy of sodium.

Hence, Element D would have the lowest ionization.

(D) is correct option

2b2t

explanation:

2b2t