Question

Sort the characteristics of ionic and covalent compounds into the correct categories:

Ionic Compounds:
A) High melting point
B) Conduct electricity in molten state
C) Shared electron pairs
D) Strong electrostatic attraction

Covalent Compounds:
A) Low melting point
B) Do not conduct electricity
C) Transfer of electrons
D) Weak electrostatic attraction

Answer 1

Ionic compounds have high melting points, can conduct electricity when melted, and are held together by strong electrostatic attractions. Covalent compounds have low melting points, do not conduct electricity, and are held together by weak intermolecular forces.

Step-by-step explanation:

Ionic Compounds:

1. High melting point: Ionic compounds generally have high melting points due to the strong electrostatic attraction between the positively and negatively charged ions.
2. Conduct electricity in molten state: Ionic compounds do not conduct electricity in the solid state, but they can conduct electricity when melted because the ions are free to move and carry charge.
3. Strong electrostatic attraction: Ionic compounds are held together by strong electrostatic attractions between oppositely charged ions.
4. Shared electron pairs: Shared electron pairs are a characteristic of covalent compounds, not ionic compounds.

Covalent Compounds:

1. Low melting point: Covalent compounds generally have low melting points compared to ionic compounds.
2. Do not conduct electricity: Covalent compounds do not conduct electricity in any state since they are composed of neutral molecules.
3. Weak electrostatic attraction: Covalent compounds are held together by weak intermolecular forces between molecules, resulting in a weak electrostatic attraction.
4. Transfer of electrons: Transfer of electrons is a characteristic of ionic compounds, not covalent compounds.