Valency and Oxidation States

Q.

The electronic configuration of four elements are given below.

Which elements does not belong to same family as others?

1. $\left[xe\right]4f^{14}5d^{10}6s^2$
2. $\left[kr\right]4d^{10}5s^2$
3. $\left[Ne\right]3s^{2}3p^5$
4. $\left[Ar\right]3d^{10}4s^2$

Q. The number of valence electrons in the elements A and B are 4 and 6 respectively. The most probable compound formed from A and B is:

1. $A_2{B}_3$
2. $A{B}_3$
3. $A{B}_2$
4. $A_{2}B$

Q. The species that contains 24 protons, 26 neutrons and 22 electrons would be represented by the symbol:

1. ${}^{50}{V}^{3+}$
2. ${}^{26}C{r}^{2+}$
3. ${}^{50}C{r}^{2+}$
4. ${}^{26}M{n}^{2+}$

Q. Which of the following halides is the least stable?

1. $CC{l}_4$
2. $Ge{I}_4$
3. $Sn{I}_4$
4. $Pb{I}_4$

Q. If an element A shows two oxidation states $+2$ and $+3$. A forms oxides in such a way that they have a ratio 1 : 3 in a compound, the formula of the compound will be

1. $A_8{O}_{11}$
2. $A_4{O}_{11}$
3. $A_9{O}_{11}$
4. $A_5{O}_{11}$

Q. Select the correct option for the below statements:
Statement I: $P{b}^{4+}$ compounds are stronger oxidizing agents than $S{n}^{4+}$compounds.
Statement II: The higher oxidation states for the group $14$ elements are more stable for the heavier members of the group due to the ‘inert pair effect’.

1. Statement I is true; Statement II is true; Statement II is the correct explanation of Statement I.
2. Statement I is true; Statement II is true; Statement II is not the correct explanation of Statement I.
3. Statement I is true; Statement II is false.
4. Statement I is false; Statement II is true.

Q. If an element A shows two oxidation states $+2$ and $+3$. A forms oxides in such a way that they have a ratio 1 : 3 in a compound, the formula of the compound will be

1. $A_8{O}_{11}$
2. $A_4{O}_{11}$
3. $A_9{O}_{11}$
4. $A_5{O}_{11}$