Question

Which of these is/are correct order(s) for group $14$ elements?

• A. Order of stability:
  $C{X}_2<Si{X}_2<Ge{X}_2<Sn{X}_2$
• B. Order of acidic character:
  $C{O}_2>Si{O}_2>Ge{O}_2$
• C. Tendency for catenation:
  $C>Si>Ge\approx Sn>Pb$
• D. Order of I.E.:
  $C>Si>Ge>Sn>Pb$

Answer 1

Answer: (A), (B), (C)

Tendency for catenation:

$C>Si>Ge\approx Sn>Pb$
(a) $C$ and $Si$ do not form any stable dihalides as $Ge,Pb$ or $Sn.$
Due to inert pair effect, the stability of $+2$ oxidation state as we move down the group increases.

(b) As we move down the group, electronegativity decreases.
Acidic character $\alpha$ electronegativity
So, down the group, acidic character decreases.

(c) As we move down the group, catenation tendency decreases due to decrease in bond dissociation energy which is due to increase in atomic size.

(d) As we move down the group, the I.E. decreases due to increase in atomic size, thereby, increasing the distance of $e^{-}$ from nucleus. The $1^{st}$ I.E. of lead is slightly higher than tin due to lanthanide contractions.