Properties of Ionic, Covalent, and Metallic Compounds

Properties of Ionic, Covalent, and Metallic Compounds & Intermolecular Forces

Bonding

• Ionic Compounds:

  • Nonmetal + Metal

  • Bond Strength: Strongest among the three types.

• Covalent Compounds:

  • Nonmetal + Nonmetal

  • Bond Strength: Strong, but usually weaker than ionic and metallic.

• Metallic Compounds:

  • Metal + Metal

  • Bond Strength: Strong, but usually weaker than ionic.

State at Room Temperature

• Ionic Compounds: Solid

• Covalent Compounds: Usually Liquid or Gas

• Metallic Compounds: Solid

Bonds Formed

• Ionic Compounds:

  • Electrons are transferred from one atom to another.

  • Ions are formed through this transfer.

• Covalent Compounds:

  • Electrons are shared between two atoms, usually in pairs.

• Metallic Compounds:

  • Outer electrons are donated to create a delocalized sea of electrons.

Structure

• Ionic Compounds:

  • Arrange in an ionic lattice structure.

  • Lattice Structure: Regular arrangement of alternating positive and negative ions.

  • Held together by strong electrostatic attraction between oppositely charged ions.

• Covalent Compounds:

  • Arrange in a regular covalent lattice structure.

  • Lattice Structure: Made up of individual molecules held together by weak intermolecular forces (Van der Waals forces).

  • Intramolecular forces within covalent molecules are stronger than intermolecular forces between the molecules.

  • Attraction between separate covalently bonded molecules is much weaker than electrostatic attraction in ionic and metallic lattices.

• Metallic Compounds:

  • Arrange in a metallic lattice structure.

  • Lattice Structure: Structure of cations in a sea of delocalized electrons.

  • Held together by strong electrostatic attraction between positively charged cations and delocalized electrons.

Volatility

• Volatility: How easily a substance evaporates into a gas.

• Ionic Compounds:

  • Usually not volatile; do not evaporate easily.

  • Due to strong electrostatic attraction, making it difficult for individual ions to evaporate.

• Covalent Compounds:

  • Usually volatile; easily evaporate.

  • Due to weak intermolecular forces (Van der Waals forces), making it relatively easy for individual molecules to evaporate.

• Metallic Compounds:

  • Usually not volatile; do not evaporate easily.

  • Due to strong electrostatic attraction, making it difficult for individual ions to evaporate.

Solubility in Water

• Ionic Compounds: Usually soluble in water.

• Covalent Compounds: Usually not soluble in water.

• Metallic Compounds: Usually not soluble in water.

Melting and Boiling Points

• Ionic Compounds:

  • Have high melting and boiling points.

  • Due to strong electrostatic attraction, making it difficult for individual ions to break away from the lattice to turn into a liquid or gas.

• Covalent Compounds:

  • Have low melting and boiling points.

  • Due to weak intermolecular forces (Van der Waals forces), making it relatively easy for individual molecules to break away to form a liquid or gas.

• Metallic Compounds:

  • Have high melting and boiling points.

  • Due to strong electrostatic attraction, making it difficult for individual ions to break away from the lattice to turn into a liquid or gas.

Electrical Conductivity

• Ionic Compounds:

  • Conduct electricity when melted or dissolved (aqueous state), but not in the solid state.

  • Electricity flow requires movement of charged particles.

  • In solid state, ions are stuck in the lattice.

  • In aqueous or liquid state, charged ions are free to move, allowing electrical conductivity.

• Covalent Compounds:

  • Do not conduct electricity.

  • Covalent compounds involve sharing electrons; atoms remain neutral.

  • No charged particles mean no conduction of electricity.

• Metallic Compounds:

  • Conduct electricity as a solid or when melted.

  • Delocalized electrons (negative charges) are free to move, even in the liquid state.

  • Allows electricity to flow easily through the lattice.

Brittleness vs. Malleability

• Ionic Compounds:

  • Brittle.

  • Ionic lattice is extremely rigid.

  • Applying force disrupts the organization of cations and anions, causing a break in the lattice.

• Covalent Compounds:

  • Soft.

  • Held together by weak intermolecular forces.

  • Can be pushed around; intermolecular forces release and reattach, but will not keep its shape.

• Metallic Compounds:

  • Malleable.

  • Layers of atoms in the structure can slide or slip over each other when a force is applied.

  • Delocalized electrons can move with the cations and reform their structure.

  • Most metals are also ductile (can be drawn into wires).

  • EXTRA INFORMATION> explain to me like im a 5 why ionic compounds have high melting and boiling pt but does it not have a strong electrostatic attraction - Ionic compounds have high melting and boiling points because they are made of ions, which are like tiny magnets that stick together very tightly. These ions are held together by something called electrostatic attraction, which means that positive and negative charges pull on each other really strong. When you try to heat them up to melt or boil them, you need a lot of energy to break those tiny magnets apart, so they don't melt or boil easily. That's why they need a lot of heat to change from solid to liquid or from liquid to gas. So, in a way, the strong pull between the ions is what makes it hard to melt or boil them