why is CCl4 more stable than CCl. At the top of Group 4, the most stable oxidation state shown by the elements is +4. This is the oxidation state shown by carbon and silicon in CCl4 and SiCl4. These therefore have no tendency to split up to give dichlorides.
In this post
Which is more stable GeCl2 or GeCl4?
GeCl4 is more stable than GeCl2 while PbCl2 is more stable than PbCl4.
Why is sicl4 stable?
Stability. At the top of Group 4, the most stable oxidation state is +4. This is the oxidation state of carbon and silicon in CCl4 and SiCl4. These compounds have no tendency to break down into dichlorides.
Which is more stable Sn2+ or Sn4+?
a) The Sn2+ ions convert to Sn4+ ions because the tin(IV) oxidation state is more stable than tin(II). This means the loss of two more electrons from the tin(II) ions, and these have to be given to something else, which gains them. Gain of electrons is reduction, and so tin(II) ions are reducing agents.
Why PbX2 is more stable than PbX4?
Due to inert pair effect +2 oxidation state of Pb is more stable than its +4 oxidation state. Consequently PbX2 in which the oxidation state of Pb is +2 is more stable than PbX4 in which the oxidation state of Pb is +4.
Which of the following has highest thermal stability CCl4 SiCl4 sncl4 pbcl4?
Thus, the correct order for the boiling point is CCl4>SiCl4.
Which of the following has highest thermal stability CCl4?
As the number of oxygen atoms in hypochlorous acid increases the thermal stability increases so HClO4 is the most stable thermally.
Why is the reaction between CCl4 and SiCl4 different?
CCl4 also reacts with water but slower than SiCl4. The difference is mostly due to the atomic size of C and Si4 is easier to attack.
Which is more stable Pb2+ and Pb4+?
Pb4+ is less stable than Pb2+.
Which of the following is most stable sn2 plus?
Solution : Due to inert pair effect which increases on moving down the group, `Pb^(2+)` is the most stable.
Why is sn2 more stable?
Out of Sn^(2+) and Sn^(4+), which one is more stable? Solution : `Sn^(2+)` ion is more stable due to inert pair effect.
Which is more stable pbx2 and pbx4?
PbX 2 is more stable than PbX 4.
Why is +2 more stable than +4?
Normally, 6p electrons become availbale for the bond formation while 6s electrons because of greater penetraton in the nucleus remain quite inert (iner pair effect). They become available only under vigorous conditions. Thus +2 oxidation state is more stable tan +4 oxidation state.
Why gex4 is stable than gex2?
and in case of GeX4 the more two electrons are removed from 4s shell because it has low energy than d shell and the rest configuration remains same . Now according to the question GeX4 is more stable because it does not have a full valence so it is unfilled valance so GeX4 is more stable than GeX2.
Why is CCl4 more stable?
why is CCl4 more stable than CCl. At the top of Group 4, the most stable oxidation state shown by the elements is +4. This is the oxidation state shown by carbon and silicon in CCl4 and SiCl4. These therefore have no tendency to split up to give dichlorides.
Why is CCl4 more stable than PbCl4?
Q. Assertion :CCl4 is stable while PbCl4 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.
Which is more stable CCl4 or SiCl4?
CCl4 is stable or do not undergo hydrolysis but SiCl4 undergoes hydrolysis.
Which is the highest thermal stability?
Hence, among the given alkali metal halides, NaCl is highest thermal stability.
Is CCl4 thermally stable?
635 oC for CCl4. Chloroform was thermally less stable than CCl4 at fairly low temperatures (< 570 oC), due to the low activation energy of the three-center HCl elimi- nation reaction of chloroform.
Which is more stable CCl4 or cf4?
The compound that is most stable in the given list is (C) CCl4.
Why is SiCl4 not stable?
SiCl4 is easily hydrolysed by water whereas CCl4 is stable towards hydrolysis in water because silicon has vacant 3d orbital available for further co-ordination with water whereas carbon has no d orbital for bonding.