Covalent Bond vs Ionic Bond

Q. Ionic compounds have high melting and boiling points because:

1. Ionic compounds can conduct electricity in molten and solid state.
2. In an ionic compound, cations and anions are held together in the lattice by covalent bonds
3. In an ionic compound, cations and anions are held together in the lattice by strong electrostatic forces of attraction
4. None of the above

Q. Select the member(s) of group $14$ that
(i) forms the most acidic dioxide
(ii) is commonly found in $+2$ oxidation state
(iii) is used as semiconductor.

Q. In which of the following molecules the central atom has more than 8 electrons in outermost orbit?

1. $S{O}_3$
2. $S{O}_2$
3. $P_2{O}_5$
4. All of these

Q. Why is $ICl$ more reactive than $I_2$ ?

Q. What is back bonding?

Q.

Why does carbon not form C_{​​​​​​2} atom with 4 covalent bonds ?
When it form 3 covalent bonds then why not 4 bonds.

Q. which d-block element has highest heat of atomisation and why explain in detail

Q.

Is NaCl Polar or Non-polar?

Q. Among the following, which compound will show the highest lattice energy?

1. CsF
2. RbF
3. KF
4. NaF

Q. Which of the following compounds has the minimum cation to anion size ratio?

1. $CsF$
2. $LiI$
3. $LiF$
4. $CsI$

Q. Electron precise hydride among the following is:

1. $C{H}_4$
2. $N{H}_3$
3. $B_2{H}_6$
4. $H_{2}O$

Q.

How does the co-ordinate covalent bond between BF3 and NH3 form?

Q. The formation of an ionic bond depends on:

1. Ionization energy
2. Electron gain enthalpy
3. Lattice energy
4. All of the above

Q.

why helium do not form molecule explain by VBT and MOT

Q. Which amongst the following is an example of a non-polar covalent compound?​

1. $\text{HCl}$
2. $\text{NaCl}$
3. ${\text{Cl}}_2$
4. $\text{KCl}$

Q.

How bonding and antibonding orbital are formed according to lcao

Q.

Is Ion Dipole interaction stronger than Hydrogen bonding?

Q. Which compound possesses the greatest lattice energy?

1. $LiBr$
2. $LiCl$
3. $LiI$
4. $LiF$

Q.

Choose the incorrect statement from the following -

1. In bonding molecular orbital, electron density is low in the region between the nuclei of bonded atoms.
2. The energy of antibonding molecular orbital is higher than that of atomic orbitals from it is formed.
3. Every electron in bonding molecular orbital contribute towards the stability of molecules.
4. Antibonding takes place when lobes of atomic orbitals have different signs.

Q. Dissolution of a solute is an exothermic process, if:

1. Hydration Energy > Lattice energy
2. All of the above
3. Lattice Energy > Hydration Energy
4. Hydration Energy = Lattice Energy

Q.

Among $Ca{H}_2,N{H}_3,NaHand{B}_2{H}_6$ which are covalent hydride

1. NH₃ and B₂H₆

2. NaH and CaH₂

3. NaH and NH₃

4. CaH₂ and B₂H₆

Q. If $N{a}^{+}$ is larger than $M{g}^{2+}$ ion and $S^{2-}$ ion is larger than $C{l}^{-}$ ion, which of the following will be the least soluble in water?

1. $NaCl$
2. $MgC{l}_2$
3. $MgS$
4. $N{a}_{2}S$

Q. In which of the following species are the bonds non-directional?

1. $NC{l}_3$
2. $RbCl$
3. $BeC{l}_2$
4. $BC{l}_3$

Q. Out of the following pairs of electrons, identify the pairs of electrons present in degenerate orbitals.

1. (a)$n=4,l=1,m_l=1,m_s=\frac{+1}{2}$
   (b)$n=3,l=2,m_l=1,m_s=\frac{+1}{2}$
2. (a) $n=3,l=1,m_l=-1,m_s=\frac{+1}{2}$
   (b)$n=3,l=2,m_l=1,m_s=\frac{+1}{2}$
3. (a)$n=3,l=2,m_l=+2,m_s=\frac{-1}{2}$
   (b)$n=3,l=2,m_l=+2,m_s=\frac{+1}{2}$
4. (a) $n=3,l=2,m_l=-2,m_s=\frac{-1}{2}$
   (b) $n=3,l=2,m_l=-1,m_s=\frac{-1}{2}$

Q. The most favourable conditions for electrovalent bonding are:

1. Low ionisation enthalpy of one atom and high electron affinity of the other atom
2. High ionisation potential and high electron affinity of both the atoms
3. Low ionisation enthalpy and low electron affinity of both the atoms
4. High ionisation enthalpy of one atom and low electron affinity of the other atom

Q. An element A has a valence electronic configuration $3s^{2}3p^5$ and the other element B has a valence electronic configuration $3s^1$. The bond formed between them is:

1. Covalent
2. Ionic
3. Coordinate covalent
4. Cannot predict

Q. An element A crystallises in FCC lattice with an edge length of 362 pm. The radius of smallest atom that can fit into the octahedral void without disturbing the crystal structure?

Q. Which of the following reaction(s) is/are exothermic for the formation of $NaF\left(s\right)$?
I. $N{a}_{\left(g\right)}\to N{a}_{\left(g\right)}^{+}+e^{-}$
II. $F_{\left(g\right)}+e^{-}\to F_{\left(g\right)}^{-}$
III. $N{a}_{\left(g\right)}^{+}+F_{\left(g\right)}^{-}\to Na{F}_{\left(s\right)}$

1. I only
2. II only
3. I and III only
4. II and III only

Q.

Effect of temperature and pressure on crystal structure

Q. Spin only magnetic moment of an octahedral complex of $F{e}^{2+}$ in the presence of a strong field ligand in $BM$ is

1. 2.82
2. 0
3. 4.89
4. 3.46