Polar Covalent Bond

Q.

The basicity of sulphuric acid is :

1. 1

2. 1.5

3. 2

4. 2.5

Q.

Nature of the bond in HCl is

1. Electrovalent

2. Ionic

3. Polar covalent

4. Non-polar covalent

Q.

Give the reason why ${\mathrm{NH}}_3$has a higher boiling point than ${\mathrm{PH}}_3$.

Q. The basicity of HCl is ___

1. 1
2. 0
3. 2
4. 4

Q.

A bond formed between two atom is covalent if the reacting atom have nearly the same electronegativities. Give reason

Q. (b) Methane molecule is non-polar molecule. Explain.

Q.

Why covalent bond attracted to each other ever they don't have ions

Q.

Write the name given to be bases that are highly soluble in water. Give an example.

Q.

Select the correct statement regarding covalent bond:

1. It involves transfer of electrons between atoms

2. It involves formation of positive and negative ions

3. It involves sharing of electrons between atoms

4. It is usually formed between a metal and a non-metal

Q.

What is the reason for the formation of polar covalent bond in HCl?

1. It reacts with water.

2. The difference in the atomic mass of H and Cl.

3. Chlorine is more electronegative than hydrogen.

4. Hydrogen is more electronegative than Chlorine.

Q.

Which of the following is a polar covalent molecule?

1. O₂

2. H₂

3. Cl₂

4. HCl

Q.

On comparison with water, which of these is true about sulphuric acid?

1. Water has higher boiling point than sulphuric acid.

2. The melting point of sulphuric acid is higher than water.

3. Both water and sulphuric acid are liquid at room temperature.

4. The density of water is lower than that of sulphuric acid.

Q.

The basicity of HCl is ___

Q. Identify Arrhenius acids and bases among the following:
$$\begin{array}{cc}1.NaCl& 2.HCl\\ 3.Cu{\left(OH\right)}_2& 4.NaOH\\ 5.H_{2}S{O}_4& 6.HN{O}_3\\ 7.KOH& \end{array}$$

1. 1, 2 and 5 are acids and 3, 4 and 7 are bases
2. 2, 3 and 5 are acids and 1, 4 and 6 are bases
3. 4, 6 and 7 are acids and the rest are bases
4. 2, 5 and 6 are acids and 3, 4 and 7 are bases

Q.

1. What is the difference between moleule and Covalent bond if there's not a difference then Give similarities between them ?

2. How CO2 gas is an acidic ?

Please give in detailed solution....

Q. Hydrogen and Chlorine in $HCl$ is bonded by a bond.

1. hydrogen
2. polar covalent
3. coordinate

Q.

Which of the following compounds are a poor conductors of electricity?

1. Distilled water

2. HCl

3. $C{H}_4$

4. $H_{2}S{O}_4$

Q.

Sulphuric acid is dense, oily like liquid.

Q.

Explain monobasic acids with examples.

Q.

$HCl$ acid is

1. Monobasic

2. Tribasic

3. All the above

4. Dibasic

Q. Amongest LiF and LiI which has more covalent character?

Q. Which of the following can change the colour of red litmus to blue?

1. Lemon juice
2. Sodium hydroxide
3. Sulphuric acid
4. Vinegar

Q.

What colour do the following indicators turn when added to a base or alkali (such as sodium hydroxide)?

(b) litmus

Q.

Which one of the following statement is correct?

1. HCl gas is highly soluble in water

2. HCl gas is insoluble in water

3. Hydrochloric acid ionizes partially in water

4. Hydrochloric acid turns red litmus solution to blue

Q.

$HCl$ acid is

1. Monobasic

2. Dibasic

3. Tribasic

4. All the above

Q. $BC{l}_3$ in aqueous solution exists as $B^{3+}$ and $Cl$.

1. True
2. False

Q. Write the electron-dot structures for the following molecules?
(i) NaCl
(ii) Cl₂

Q. Statement I: Equal volumes of 0.3 M $H_{2}S{O}_4$ solution and 0.2 M $H_{3}P{O}_4$ solution will require the same volume of the same $NaOH$ solution for complete neutralization.
Statement II: $H_{2}S{O}_4$ is a dibasic and $H_{3}P{O}_4$ is a tribasic acid.

1. Statement I is CORRECT, but Statement II is INCORRECT.
2. Both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.
3. Both statements are CORRECT, and Statement II is NOT the CORRECT explanation of Statement I.
4. Statement I is INCORRECT, but Statement II is CORRECT.

Q.

why H-bonding does not exist in HCL , though chlorine is electronegative?

Q.

Nature of the bond in HCl is

1. Electrovalent

2. Polar covalent

3. Non-polar covalent

4. Ionic