Tetrahalides of group 4 which do not behave as oxidizing agents are:

P b C l_{4}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

S n C l_{4}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

C C l_{4}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

G e C l_{4}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct options are
B $S n C l_{4}$
C $C C l_{4}$
D $G e C l_{4}$
Carbon shows only $+ 4$ oxidation state. Ge and Sn show $+ 2$ oxidation states because of inert pair effect, but $+ 4$ state is more stable than $+ 2$ state and hence do not show oxidizing property.

Suggest Corrections

Similar questions

Stability order for CCl₄_>SiCl4 >GeCl₄ >SnCl₄ >PbCl_{4 bt we know that carbon have no vacant d-orbital than how it form bond with 4Chlorine stom and bocomes most stable ?}

Q. Assertion :

C C l_{4}

is stable while

P b C l_{4}

is powerful oxidizing agent. Reason: Due to the inert pair affect the stability of the

+ 2

state increases on moving down the group from carbon to lead.

Q. Which of the following behaves as both oxidizing and reducing agents ?

Q. Assertion :

P b C l_{2}

is more stable than

P b C l_{4}

. Reason:

P b C l_{4}

is powerful oxidizing agent.

H_{2} C_{2} O_{4}

and

N a H C_{2} O_{4}

behave as acids as well as reducing agents. Which are correct statements?

Join BYJU'S Learning Program

Tetrahalides of group 4 which do not behave as oxidizing agents are:

The correct options are B SnCl4 C CCl4 D GeCl4Carbon shows only +4 oxidation state. Ge and Sn show +2 oxidation states because of inert pair effect, but +4 state is more stable than +2 state and hence do not show oxidizing property.

The correct options are
B $S n C l_{4}$
C $C C l_{4}$
D $G e C l_{4}$
Carbon shows only $+ 4$ oxidation state. Ge and Sn show $+ 2$ oxidation states because of inert pair effect, but $+ 4$ state is more stable than $+ 2$ state and hence do not show oxidizing property.