Electronic Configuration

Q.

What is inert pair effect? Explain with an example.

Q.

The noble gas that does not have a closed octet in its outer shell is:

1. He

2. Ne

3. Ar

4. Kr

Q.

Which of the following electronic configuration (a or b) is more stable and why?

(a) 3d⁴4s²

(b) 3d⁵ 4s¹

Q. Which of these is/are negatively charged ligand(s)?

1. $C{l}^{-}$
2. $O{H}^{-}$
3. $C{N}^{-}$
4. All of the above.

Q. The spin only magnetic moment of a divalent ion in aqueous solution (atomic number 29) is (nearest integer)

JEE MAINS 2021

Q. Identify the least stable ion amongst the following:

1. $L{i}^{–}$
2. $B{e}^{-}$
3. $B^{-}$
4. $C^{–}$

Q. What is the hybridization of $Xe$ in $Xe{F}_6$?

1. $s{p}^3{d}^3$
2. $s{p}^{2}d$
3. $s{p}^3{d}^2$
4. $s{p}^3$

Q. Find the value of $\frac{y.z}{x}$, if the following molecules undergo dimerization:
I. $Cl{O}_3$
II. $O{F}_2$
III. $Ga{H}_3$
IV. $AlC{l}_3$
V. $IC{l}_3$
VI. $Be{H}_2$
VII. $N{O}_2$
$x$: Number of molecules which are hypervalent in dimeric form
$y$: Number of molecules with a complete octet in dimeric form
$z$: Number of molecules which are hypovalent in dimeric form

Q. A neutral atom has $2K$ electrons, $8L$ electrons and $6M$ electrons. Predict total number of $d-$ electrons

1. 4
2. 2
3. \N
4. 10

Q.

The electronic configuration of a dipositive metal $M^{2+}$ is 2, 8, 14 and its atomic weight is 56 a.m.u. The number of neutrons in its nuclei would be

1. 30

2. 32

3. 34

4. 42

Q. An ion has electronic configuration $\left[Kr\right]4d^4$ placed in group 6 in the modern periodic table. The ion is:

1. $C{r}^{2+}$
2. $M{n}^{3+}$
3. $M{o}^{2+}$
4. $T{c}^{3+}$

Q.

Where would you locate the element with electronic configuration 2, 8 in the Modern Periodic Table?

1. Group 8

2. Group 2

3. Group 18

4. Group 10

Q. $Xe{F}_6,I_3^{-},SnC{l}_2,C{O}_2$
The sum of the number of lone pairs on the central atom of the given compounds is

Q. A neutral atom has $2K$ electrons, $8L$ electrons and $6M$ electrons. Predict its atomic number

1. 10
2. 12
3. 14
4. 16

Q. What is the increasing order of equivalent weights of the following oxidising agents?
(i) $KMn{O}_4⟶M{n}^{2+}$
(ii) $K_{2}C{r}_2{O}_7⟶C{r}^{3+}$
(iii) $KCl{O}_3⟶C{l}^{-}$
[Atomic wt.:
$K=39,Cr=52,Mn=55,Cl=35.5,O=16$]

1. $KCl{O}_3<KMn{O}_4<K_{2}C{r}_2{O}_7$
2. $K_{2}C{r}_2{O}_7<KMn{O}_4<KCl{O}_3$
3. $KMn{O}_4<K_{2}C{r}_2{O}_7<KCl{O}_3$
4. $KCl{O}_3<K_{2}C{r}_2{O}_7<KMn{O}_4$

Q. Which one of the following is correct order of the size of iodine species?

1. $I>I^{–}>I^{+}$
2. $I^{+}>I^{–}>I$
3. $I>I^{+}>I^{-}$
4. $I^{–}>I>I^{+}$

Q. <!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> An example of a disproportionation reaction is:

JEE MAIN 2019

1. $2KMn{O}_4\to K_{2}Mn{O}_4+Mn{O}_2+O_2$
2. $2NaBr+C{l}_2\to 2NaCl+B{r}_2$
3. $2CuBr\to CuB{r}_2+Cu$
4. $2Mn{O}_4^{-}+10I^{-}+16H^{+}\to 2M{n}^{2+}+5I_2+8H_{2}O$

Q. A neutral atom has $2K$ electrons, $8L$ electrons and $6M$ electrons. Predict total number of $p-$ electrons

1. 4
2. 6
3. 8
4. 10

Q. A neutral atom has $2K$ electrons, $8L$ electrons and $6M$ electrons. Predict total number of $p-$ electrons

1. 4
2. 6
3. 8
4. 10

Q. What is the general formula for oxide of element $M$ with atomic number 87?

1. $M_{2}O$
2. $MO$
3. $M_2{O}_3$
4. $M{O}_2$

Q. Assertion: Fluorine is a stronger oxidising agent than iodine.
Reason: Fluorine has greater electronegativity than iodine.

<!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> AIIMS 2012

Q.

Which has most stable +2 oxidation state?

1. Sn

2. Pb

3. Fe

4. Ag

Q. Which one of the following is correct order of the size of iodine species?

1. $I^{+}>I^{–}>I$
2. $I>I^{+}>I^{-}$
3. $I^{–}>I>I^{+}$
4. $I>I^{–}>I^{+}$

Q.

The general electronic configuration of halogens is?

1. $n{s}^{2}n{p}^6$

2. $n{s}^{2}n{p}^3$

3. $n{s}^{2}n{p}^5$

4. $n{s}^2$

Q. What is the increasing order of equivalent weights of the following oxidising agents?
(i) $KMn{O}_4⟶M{n}^{2+}$
(ii) $K_{2}C{r}_2{O}_7⟶C{r}^{3+}$
(iii) $KCl{O}_3⟶C{l}^{-}$
[Atomic wt.:
$K=39,Cr=52,Mn=55,Cl=35.5,O=16$]

1. $KCl{O}_3<KMn{O}_4<K_{2}C{r}_2{O}_7$
2. $K_{2}C{r}_2{O}_7<KMn{O}_4<KCl{O}_3$
3. $KMn{O}_4<K_{2}C{r}_2{O}_7<KCl{O}_3$
4. $KCl{O}_3<K_{2}C{r}_2{O}_7<KMn{O}_4$

Q. In the transformation: $Na\left(s\right)\to N{a}^{+}\left(g\right)$, the energies involved are

1. Ionization energy
2. Sublimation energy
3. Ionization energy and sublimation energy
4. Bond dissociation energy