Ionic Bonding

Explain the process of formation of ionic bonds.

• Ionic bonds form through the sharing of electrons between atoms.

• Ionic bonds form through the attraction of similarly charged ions.

• Ionic bonds form through the repulsion of like-charged ions.

• Ionic bonds form through the transfer of electrons between atoms, leading to the attraction of oppositely charged ions.

What are the key properties of ionic compounds?

• High melting and boiling points, non-conductivity, and liquid state structure

• Low melting and boiling points, insulating properties, and amorphous structure

• High melting and boiling points, conductivity in molten or aqueous state, and crystalline structure

• Moderate melting and boiling points, conductivity in solid state, and crystalline structure

How does ionic bonding occur in salts?

• Ionic bonding occurs through covalent sharing of electrons between metal and non-metal atoms.

• Metal atoms transfer electrons to non-metal atoms, forming oppositely charged ions that are held together by electrostatic forces.

• Non-metal atoms transfer electrons to metal atoms, forming oppositely charged ions.

• Ionic bonding is a result of the repulsion between metal and non-metal atoms.

Describe the crystal lattice structure of ionic compounds.

• Positively and negatively charged ions are arranged in a repeating pattern to form a three-dimensional crystal lattice structure.

• The crystal lattice structure of ionic compounds is amorphous

• The crystal lattice structure of ionic compounds is one-dimensional

• Ions are randomly distributed in the crystal lattice structure

Why do ionic compounds have high melting and boiling points?

• Strong electrostatic forces of attraction between ions

• Presence of covalent bonds between ions

• Weak electrostatic forces of attraction between ions

• Lack of electrostatic forces between ions

What is the role of electronegativity in ionic bonding?

• Electronegativity has no impact on ionic bonding

• Electronegativity determines the size of the ions formed in ionic bonding

• Electronegativity influences the transfer of electrons in ionic bonding by determining which atom will attract the shared electrons more strongly.

• Electronegativity causes the atoms to share electrons equally in ionic bonding

How do ionic compounds conduct electricity in molten or aqueous state?

• Ionic compounds do not conduct electricity in any state.

• Ions are free to move and carry electric charge when the ionic bonds are broken in the molten or aqueous state.

• Ions are stationary and do not move in the molten or aqueous state.

• The ionic bonds become stronger in the molten or aqueous state, preventing conductivity.

Discuss the relationship between the size of ions and the strength of ionic bonds.

• The size of ions has no impact on the strength of ionic bonds.

• The strength of ionic bonds decreases as the size of ions increases.

• Ionic bonds are not affected by the size of ions.

• The strength of ionic bonds increases as the size of ions increases.

Explain the concept of lattice energy in the context of ionic bonding.

• Lattice energy is the energy released when gaseous ions come together to form a solid ionic compound.

• Lattice energy is the energy released when covalent bonds are formed between atoms.

• Lattice energy is the energy absorbed when gaseous ions come together to form a solid ionic compound.

• Lattice energy is the energy released when metallic bonds are formed between atoms.

What are some common examples of ionic compounds found in everyday life?

• Hydrogen peroxide (H2O2)

• Table salt (sodium chloride - NaCl), baking soda (sodium bicarbonate - NaHCO3), calcium carbonate (CaCO3)

• Sugar (sucrose)

• Vinegar (acetic acid)