Lewis Kossel Structure

Q. According to vsper theory why multiple bond are treated as a single electron pair ??

Q.

Valence bond theory explains:

1. Resonance

2. Directional properties of bonds in molecules

3. Polarity of bonds

4. Formal charge on the atoms in molecules

Q.

Give an example of ionic compound formation.

Q.

Among the following compounds the maximum number of lone pair is present on the central atom of:

1. ClO₃^-

2. SF₄

3. I₃^-

4. XeF₄

Q. The correct order of the number of unpaired electrons in the ions, ${\text{Cu}}^{2+},{\text{Ni}}^{2+},{\text{Fe}}^{3+}\text{and}{\text{Cr}}^{3+}$ is

1. ${\text{Cu}}^{2+}>{\text{Ni}}^{2+}>{\text{Cr}}^{3+}>{\text{Fe}}^{3+}$
2. ${\text{Fe}}^{3+}>{\text{Cr}}^{3+}>{\text{Cu}}^{2+}>{\text{Ni}}^{2+}$
3. ${\text{Cr}}^{3+}>{\text{Fe}}^{3+}>{\text{Ni}}^{2+}>{\text{Cu}}^{2+}$
4. ${\text{Fe}}^{3+}>{\text{Cr}}^{3+}>{\text{Ni}}^{2+}>{\text{Cu}}^{2+}$

Q. The hydroxides and carbonates of sodium and potassium are easily soluble in water while the corresponding salts of magnesium and calcium are sparingly soluble in water. Explain.

Q.

Boric acid has a layer structure in which planar BO₃ units are joined by:

1. O-bonds

2. H-bonds

3. N-bonds

4. Na-bonds

Q. the atom with lowest atomic no. that has a ground state electronic configuration of(n-1)d6 ns2 is

Q.

An ionic bond is present in which of the following species:

1. Sodium Bromide

2. Sulfur Trioxide

3. Hydrogen Chloride

4. Carbon Monoxide

Q. Why modern periodic table is called Bohrs Table while it was made by Henry Moseley?

Q. The covalency of sulphur in sulphuric acid $\left(H_{2}S{O}_4\right)$ is:

Q. 35.Which series has the highest energy in hydrogen spectra 1) Balmer 2) bracket 3) pfund 4) lyman

Q. The correct electron-dot formulation for hydrogen cyanide shows:

1. 2 double bonds and two lone pairs of electrons on the N atom.
2. 1 C-H bond, 1 C = N bond, 1 lone pair of electrons on the C atom and 1 lone pair of electrons on the N atom.
3. 1 C-H bond, 1 C-N bond, 2 lone pairs of electrons on the C atom and 3 lone pairs of electrons on the N atom.
4. 1 triple bond between C and N, 1 C-H bond and 1 lone pair of electrons on the N atom.

Q. AB CRYSTALLIZES IN A BODY CENTERED CUBIC LATTICE WITH EDGE LENTH a EQUAL TO 387 PM.THE DISTANCE BETWEEN TWO OPPOSITIVELY CHARGED IONS IN THE LATTICE IS?

Q. 50. Which has stronger intermolecular hydrogen bonding and why ? : HF or H2O

Q.

In LiF, the structure of $F^{-}$ is

1. 

2. 

3. 

4. 

Q. For which of the following compounds a valid Lewis structure cannot be drawn without violating the octet rule?

1. $P{O}_4^{3-}$
2. $Si{F}_4$
3. $C{F}_4$
4. $Se{F}_4$

Q. In what ways lithium shows similarities to magnesium in its chemical behaviour?

Q. The formal charge on $N$ in $N{O}_2^{-}$ is:

1. \N
2. 1
3. -1
4. +$\frac{1}{2}$

Q. what is the total number of sigma and pi bonds in C₂H₂molecule

Q. The enolic form of ethyl acetoacetate as given below has :

1. 9 sigma bonds and 1 pi-bond
2. 18 sigma bonds and 2 pi-bond
3. 16 sigma bonds and 1 pi-bond
4. 9 sigma bonds and 2 pi-bonds

Q. For which of the following compounds a valid Lewis structure cannot be drawn without violating the octet rule?

1. $P{O}_4^{3-}$
2. $Si{F}_4$
3. $C{F}_4$
4. $Se{F}_4$

Q.

In LiF, the structure of $F^{-}$ is

1. 

2. 

3. 

4. None of these

Q.

Distinguish b/w Molecular Bond & Valence Bond Theory

Q. What is solvation of halide ion with proton of protic solvent

Q.

Apart from tetrahedral geometry, another possible geometry for CH₄ is square planar with the four H atoms at the corners of the square and the C atom at its centre. Explain why CH₄ is not square planar?

Q.

Explain BeCl2 has 0 dipole moment although the Be-Cl bonds are polar?

Q. In which of the following N is in the $sp$ hybridisation state ?

1. $(C{H}_3{)}_{3}N$
2. $C{H}_{3}CON{H}_2$
3. $N{O}_2^{+}$
4. None of the above

Q. Which of the following does not have eight valence electrons?

1. $C{a}^{+}$
2. $R{b}^{+}$
3. $Xe$
4. $B{r}^{-}$

Q. Identify the correct sequence of the increasing order of $\pi$- bonds in the following molecules:
(I) $H_2{S}_2{O}_6$
(II) $H_{2}S{O}_3$
(III) $H_2{S}_2{O}_5$

1. I < II < III
2. II < III < I
3. II < I < III
4. I < III < II