Among the following solids, which one shows the strongest bonding?

a)
Metallic solids

b)
Ionic solids

c)
Covalent solids

d)
Molecular solids

Correct answer is option 'B'. Can you explain this answer?

Question

Among the following solids, which one shows the strongest bonding?a)Metallic solidsb)Ionic solidsc)Covalentsolidsd)Molecular solidsCorrect answer is option 'B'. Can you explain this answer?

Answer

1. Covalent (or network) solids are extended-lattice compounds, in which each atom is covalently bonded to its nearest neighbors. Because there are no delocalized electrons, covalent solids do not conduct electricity.

2. The rearranging or breaking of covalent bonds requires large amounts of energy; therefore, covalent solids have high melting points.

3. Covalent bonds are extremely strong, so covalent solids are very hard. Generally, covalent solids are insoluble due to the difficulty of solvating very large molecules.

4. Diamond is the hardest material known, while cubic boron nitride (BN) is the second-hardest. Silicon carbide (SiC) is very structurally complex and has at least 70 crystalline forms.

Answer

C since ionic bond is much stronger than covalent bond

Answer

Less the electronegativity difference more is the covalent character and more is the electronegativity difference more is the ionic character.

More electronegativity difference means there would be more attraction ,so according to this ionic bond is stronger and also the attractive force is electrostatic.

please reply if u got this wrong.

Answer

C is the write answer because ionic bond is stronger than covalent bond

Answer

Iionic solids show strongest bonding.... But in ncert textbook ans is given as covalent solids...

Answer

Option C is correct because
bond strength order:
covalent solid - ionic solid- metallic solid-molecular solid
here - means greater than

Answer

Ionic bond is the strongest Bond because they have latttice structure in which there cation and anion are strongly held at the lattice point in the lattice structure by strong electrovalent bond

Answer

Covalent solids show weak bonding

Answer

1. Covalent (or network) solids are extended-lattice compounds, in which each atom is covalently bonded to its nearest neighbors. Because there are no delocalized electrons, covalent solids do not conduct electricity.
2. The rearranging or breaking of covalent bonds requires large amounts of energy; therefore, covalent solids have high melting points.
3. Covalent bonds are extremely strong, so covalent solids are very hard. Generally, covalent solids are insoluble due to the difficulty of solvating very large molecules.
4. Diamond is the hardest material known, while cubic boron nitride (BN) is the second-hardest. Silicon carbide (SiC) is very structurally complex and has at least 70 crystalline forms@@

Answer

A single covalent bond is not strongest buy because of large network of covalent bonds , covalent solids become stronger than other solids

Answer

Ionic bond is twenty times stronger than covalent bond

Answer

Covalent solids content of covalent bonds

Answer

Ionic solids because there is a lattice energy in between them.

Answer

Yup! covalent solids do shows the strongest bonding as the atoms r bonded with each other with 'strong london force of attraction' or 'Vander walls force of attraction' which r very difficult to break. hope uh got that point :)

Answer

Covalent bonding is strongest due to multiple bonding of carbon

Answer

According to new era book
binding energy is...
ionic- 400-40000 unit
covalent- 150-500 unit
molecular- 5-25 unit
metallic- 70-1000 unit

Answer

Because ionic solids are held in lattice due to electrostatic force of attraction between cations and anions...

Answer

Explanation:

Ionic solids exhibit the strongest bonding among the given options. This can be attributed to the nature of the bonding present in these solids.

What are Ionic Solids?
Ionic solids are formed by the combination of positively and negatively charged ions held together by electrostatic forces of attraction. These solids are typically composed of a metal cation and a non-metal anion. Examples of ionic solids include sodium chloride (NaCl) and calcium carbonate (CaCO3).

Strong Electrostatic Forces:
Ionic solids possess strong ionic bonds due to the electrostatic attraction between oppositely charged ions. The positive metal ions are attracted to the negative non-metal ions, resulting in a strong bond. These electrostatic forces are stronger than the forces present in other types of solids.

High Melting and Boiling Points:
The strong bonding in ionic solids leads to high melting and boiling points. To break the strong ionic bonds, a considerable amount of energy is required, resulting in high melting and boiling points. This is because the ionic bonds need to be overcome in order to convert the solid into a liquid or gas state.

Rigid and Brittle Structure:
Ionic solids have a rigid crystal lattice structure due to the strong electrostatic forces between ions. The ions are arranged in a repeating pattern in three dimensions. However, this rigid structure also makes ionic solids brittle. When a force is applied, the ions shift and like charges come into proximity, causing repulsion and resulting in the fracture of the crystal lattice.

Conductivity:
Ionic solids are poor conductors of electricity in the solid state because the ions are held in fixed positions and cannot move freely. However, when melted or dissolved in a solution, the ions become mobile and can conduct electricity.

Summary:
In summary, ionic solids exhibit the strongest bonding among the given options due to the strong electrostatic forces of attraction between oppositely charged ions. This results in high melting and boiling points, a rigid crystal lattice structure, brittleness, and poor conductivity in the solid state.

Top Courses for JEEView all

Physics for JEE Main & Advanced

Chapter-wise Tests for JEE Main & Advanced

Mock Tests for JEE Main and Advanced 2026

Chemistry for JEE Main & Advanced

Mathematics (Maths) for JEE Main & Advanced

Top Courses for JEE

Top Courses for JEE

Related Content

JEE Courses

Mock Test Series

Past Year Papers

Additional Courses

Company