Consider the following elements A, B, C and D and their outer electronic configurations are and respectively. Element also has same outer electronic configuration like but shows only single oxidation

Question

Consider the following elements A, B, C and D and their outer electronic configurations are $ns^2np^1, ns^2np^3, ns^2np^4$ and $ns^2np^5$ respectively. Element $E$ also has same outer electronic configuration like $D$ but shows only single oxidation state ($-1$). If element A, B, C and D belong to same period as that of sodium. Consider the following compounds.
(i) $CE_4$
(ii) $BD_2E_3$
(iii) $DE_3$
(iv) $CE_2$
(v) $BD_3E_2$
(vi) $C_2E_2$
(vii) $DE$
(viii) $A_2D_6$
Then calculate the value of "$x \div y$", (where $x$ and $y$ are total number of polar and non-polar compounds).

Prashant Kotian · Accepted Answer

Correct answer: 3

**SOLUTION:** ELEMENTS $A = AL, B = P, C = S, D = CL, E = F$.
POLAR COMPOUNDS ($X=6$): $SF_4, PCL_2F_3, CLF_3, SF_2, S_2F_2, CLF$.
NON-POLAR COMPOUNDS ($Y=2$): $PCL_3F_2, AL_2CL_6$.
$X/Y = 6/2 = 3$.. Step 1: Calculate the total number of valence electrons for each oxide of nitrogen: N2O has 16 electrons (even, all paired); NO has 11 electrons (odd, contains one unpaired electron); NO2 has 17 electrons (odd, contains one unpaired electron). Step 2: Any molecule with an odd number of total valence electrons must have at least one unpaired electron. Step 3: Therefore, NO and NO2 are odd-electron molecules containing unpaired electrons, matching option (b).

💡 Solution & Explanation

Practice 22,000+ questions like this