Understanding Bonding in Solids

What is ionic bonding and how does it occur in solids?

• Ionic bonding involves the sharing of electrons between atoms in a liquid state.

• Ionic bonding is the attraction between two neutral atoms without any charge.

• Ionic bonding is the electrostatic attraction between cations and anions formed through the transfer of electrons, resulting in a stable ionic lattice in solids.

• Ionic bonding occurs only in gases and does not form a solid structure.

Describe the characteristics of ionic solids.

• Ionic solids conduct electricity in solid form.

• Ionic solids have low melting points and do not form crystals.

• Ionic solids are soft and malleable.

• Ionic solids are hard, brittle, have high melting and boiling points, form crystalline structures, and conduct electricity when melted or dissolved.

What are the common properties of covalent network solids?

• High melting and boiling points, poor electrical conductivity, insolubility in solvents, and a rigid structure.

• Soluble in most solvents

• High electrical conductivity

• Low melting and boiling points

How do covalent bonds differ from ionic bonds in solids?

• Covalent bonds involve shared electrons, while ionic bonds involve transferred electrons and electrostatic attraction.

• Covalent bonds are formed by metallic interactions, while ionic bonds are formed by covalent sharing.

• Ionic bonds involve shared electrons, while covalent bonds involve a mixture of ionic and metallic bonds.

• Covalent bonds are weaker than ionic bonds due to the lack of electron sharing.

Explain the significance of lattice energy in ionic solids.

• Lattice energy is significant as it determines the stability, melting point, and solubility of ionic solids.

• Lattice energy is solely determined by the size of the ions involved.

• Lattice energy only affects the color of ionic solids.

• Lattice energy is irrelevant to the properties of ionic solids.

What are some examples of covalent network solids?

• Sodium chloride

• Calcium carbonate

• Diamond, silicon carbide, graphite

• Iron oxide

Describe the characteristics of metallic bonding.

• Metallic bonding involves a sea of delocalized electrons, strong electrostatic attraction between positive ions, and results in properties like conductivity, malleability, and ductility.

• Metallic bonding involves isolated atoms with no electron sharing.

• Metallic bonding leads to properties like brittleness and poor conductivity.

• Metallic bonding is characterized by fixed electrons and weak attractions between atoms.

How does metallic bonding contribute to the properties of metals?

• Metallic bonding causes metals to be non-malleable.

• Metallic bonding prevents electrical conductivity in metals.

• Metallic bonding makes metals brittle and weak.

• Metallic bonding contributes to the conductivity, malleability, and strength of metals.

What is the role of delocalized electrons in metallic bonding?

• Delocalized electrons create strong covalent bonds in metals.

• Delocalized electrons prevent electrical conductivity in metals.

• Delocalized electrons are responsible for the color of metals.

• Delocalized electrons allow for electrical conductivity, malleability, and ductility in metals.

Compare the electrical conductivity of ionic, covalent, and metallic solids.

• Ionic solids conduct when dissolved or molten, covalent solids do not conduct, and metallic solids conduct well.

• Ionic solids conduct in all states, covalent solids conduct when heated, and metallic solids do not conduct.

• Covalent solids conduct when dissolved in water, ionic solids do not conduct, and metallic solids conduct poorly.

• Metallic solids do not conduct, ionic solids conduct only as gases, and covalent solids conduct well.