Neon and Heteronuclear Diatomic Molecules

Q. Draw the electron dot diagram and structure of (a) nitrogen molecule​

Q. The value of the 'spin only ' magnetic moment for one of the following configurations is 2.84 BM. The correct one is

1. $d^4\text{(in strong ligand field)}$
2. $d^4\text{(in weak ligand field)}$
3. $d^3\text{(in weak as well as in strong fields)}$
4. $d^5\text{(in strong ligand field)}$

Q. In isolated condition $C-C$ bond length of $C_2{H}_4$ is x, then the bond length of $C-C$ bond of $C_2{H}_4$ in Zeise's salt is :

1. greater than x
2. Less than x
3. Equal to x
4. None of these

Q.

Classify the following molecule as a polar and non-polar molecule. Give a reason for your classification.

1. ${\mathrm{H}}_2$
2. ${\mathrm{O}}_2$
3. ${\mathrm{H}}_2\mathrm{O}$
4. ${\mathrm{CCl}}_4$
5. ${\mathrm{NH}}_3$
6. ${\mathrm{Cl}}_2$
7. $\mathrm{HCl}$

Q.

Q3-(1)- Metals form ________ Chlorides.

Q.

________ is the combining capacity of an element.

Q.

Which of the following are iso-electronic and iso-structural?

$N{O}_3^{-}$, $C{O}_3^{2-}$, $Cl{O}_3^{-}$, $S{O}_3$

1. CO, SO

2. CO, ClO

3. NO, SO

4. NO, CO

Q. In which of the following ionisation processes has the bond order increased and the magnetic behaviour changed?

1. $C_2\to C_2^{+}$
2. $NO\to N{O}^{+}$
3. $N_2\to N_2^{+}$
4. $O_2\to O_2^{+}$

Q.

Which of the following atoms will have the same number of electrons, protons and neutrons?

1. ${}_6{}^{12}\mathrm{C}$

2. ${}_{11}{}^{23}\mathrm{Na}$

3. ${}_{15}{}^{31}\mathrm{P}$

4. ${}_{17}{}^{35}\mathrm{Cl}$

Q.

Which of the following is iso-electronic?

1. ${CN}^{-},CO$

2. $N{O}_2,C{O}_2$

3. ${N{O}_2}^{-},C{O}_2$

4. $S{O}_2,C{O}_2$

Q. 4. Calculate the no of electrons require to deposit 40.5g of Al?

Q.

chemistry how to calculate dipole moment

Q.

Which of the following have same bond order?

1. $C{N}^{-}$

2. ${O_2}^{-}$

3. $N{O}^{+}$

4. $C{N}^{+}$

Q.

Elements with higher electronegativity are good oxidizing agents. Give reasons.

Q.

Which of the following is iso-electronic?

1. 

2. 

3. 

4. 

Q. Which of the following are isoelectronic species i.e. those having the same number of electron $C{a}^{+2},S^{-2}$?

Q. Which of the following does not contain isoelectronic species?

1. $P{O}_4^{3-}$, $S{O}_4^{2-}$, $Cl{O}_4^{-}$
2. $C{N}^{-}$, $N_2$, $C_2^{2-}$
3. $S{O}_3^{2-}$, $C{O}_3^{2-}$, $N{O}_3^{-}$
4. $B{O}_3^{3-}$, $C{O}_3^{2-}$, $N{O}_3^{-}$

Q. The common features of the species $N_2^{2-},O_2$ and $N{O}^{-}$ are:

1. bond order is three and are isoelectronic
2. bond order is two and are isoelectronic
3. bond order is three but are not isoelectronic
4. bond order is two but are not isoelectronic

Q. Which of the following are iso-electronic species ?

1. $C{O}_2,N{O}_2$
2. $N{O}_2^{-},C{O}_2$
3. $C{N}^{-},CO$
4. $S{O}_2,C{O}_2$

Q. Calculate the number of electrons required to deposit 40.5 g of Al.

Q.

The common features among the species $C{N}^{-},COandN{O}^{+}$ are

1. Bond order three and isoelectronic

2. Bond order three and weak field ligands

3. Bond order two and -acceptors

4. Isoelectronic and weak field ligands

Q.

Which of the following is not isoelectronic?

1. 

2. 

3. 

4. 

Q. The electronegativity difference between N and F is greater than N and H, yet the dipole moment of $N{H}_3$ (1.5 D) is greater than that of $N{F}_3$ (0.2 D). This is because:

1. In $N{H}_3$ as well as $N{F}_3$, the overall molecular dipole and bond dipoles are in the opposite direction
2. In $N{H}_3$, the overall molecular dipole and bond dipoles are in the opposite direction, whereas in $N{F}_3$, these are in the same direction.
3. In $N{H}_3$ as well as in $N{F}_3$ the overall molecular dipole and bond dipoles are in the same direction
4. In $N{H}_3$, the overall molecular dipole and bond dipoles are in the same direction, whereas in $N{F}_3$ these are in the opposite direction