Question

An oxide of chlorine which is an odd electron molecule is:
1 ClO2
2 Cl2O6
3 Cl2O7
4 Cl2O

Answer 1

No. of electrons in
ClO₂ = 33
Cl₂O₆ = 82
Cl₂O₇ = 90
Cl₂O = 40

∴ Odd electron molecule is ClO₂
(1) is the correct option.

Answer 2

Among the given oxides of Chlorine, the oxide of chlorine given in the option 1 - $ClO_2$ has odd number of electrons.

Explanation:

• To identify the oxide with odd electrons, the number of electrons present in all the four given oxides of chlorine must be identified.
• To calculate it the atomic number of constituent elements present in the compound is needed.
• As the given compounds are oxides of chlorine, they are composed of Oxygen and chlorine. The atomic number of Oxygen is 6 and chlorine is 17.
• With help of it the number of electrons present in each oxide are calculated as shown:

1. Number of electrons in $ClO_2$

$ClO_2$

= 1(Cl)+2(O)

= 1(17)+2(8)

= 17+16

=33

2. Number of electrons in $Cl_2O_6$

$Cl_2O_6$

= 2(Cl)+6(O)

= 2(17)+6(8)

= 34+48

= 82

3. Number of electrons in $Cl_2O_7$

$Cl_2O_7$

= 2(Cl)+7(O)

= 2(17)+7(8)

= 34+56

= 90

4. Number of electrons in $Cl_2O$

$Cl_2O$

= 2(Cl)+1(O)

= 2(17)+1(8)

= 34+8

= 42

• From the above calculation the following data is obtained:

1. $ClO_2$ has 33 electrons (odd)
2. $Cl_2O_6$ has 82 electrons (even)
3. $Cl_2O_7$ has 90 electrons (even)
4. $Cl_2O$ has 42 electrons (even)

• Thus it is inferred that the oxide of chlorine given in the option 1 - $ClO_2$ has odd number of electrons.

Learn more about such concept

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