Which of the following molecule has odd ?

Question

Accepted Answer

To determine which molecule has an odd number of electrons, we need to calculate the total number of valence electrons for each molecule.

Step 1: Calculate total valence electrons for each option.

A) $Cl O_{2}$
Chlorine (Cl) is in Group 17, so it has 7 valence electrons.
Oxygen (O) is in Group 16, so it has 6 valence electrons.
Total valence electrons = $7 + (2 \times 6) = 7 + 12 = 19$ electrons.
Since 19 is an odd number, $Cl O_{2}$ has an odd number of electrons.
B) $OC l_{2}$
Oxygen (O) has 6 valence electrons.
Chlorine (Cl) has 7 valence electrons.
Total valence electrons = $6 + (2 \times 7) = 6 + 14 = 20$ electrons.
Since 20 is an even number, $OC l_{2}$ does not have an odd number of electrons.
C) $O (Si H_{3})_{2}$
Oxygen (O) has 6 valence electrons.
Silicon (Si) is in Group 14, so it has 4 valence electrons.
Hydrogen (H) has 1 valence electron.
Total valence electrons = $6 + 2 \times (4 + 3 \times 1) = 6 + 2 \times (4 + 3) = 6 + 2 \times 7 = 6 + 14 = 20$ electrons.
Since 20 is an even number, $O (Si H_{3})_{2}$ does not have an odd number of electrons.
D) $SC l_{2}$
Sulfur (S) is in Group 16, so it has 6 valence electrons.
Chlorine (Cl) has 7 valence electrons.
Total valence electrons = $6 + (2 \times 7) = 6 + 14 = 20$ electrons.
Since 20 is an even number, $SC l_{2}$ does not have an odd number of electrons.

Step 2: Identify the molecule with an odd number of electrons.

Based on the calculations, only $Cl O_{2}$ has an odd number of valence electrons (19).

Correct Answer: (A)