1. IONIC BOND: Metal-NonMetal
1.1. Ions created by electron transfer from Metal to Non-metal to comply the octet rule.
1.2. Electrostatic forces between Cation-Anion.
1.3. Ions are in fixed positions forming a 3D lattice.
1.4. Properties of Ionic crystals due to a strong bond:
1.4.1. Hard and rigid.
1.4.2. Brittle.
1.4.3. Solid at normal temperature.
1.4.4. High melting and boiling points.
1.4.5. Soluble in water.
1.4.6. In solid state they do not conduct electricity but, they do it melted or in dissolved in water.
2. METALLIC BOND: Metal-Metal
2.1. Between atoms of the same metal.
2.2. Atoms are fixed in a 3D lattice.
2.3. Electrons of the valence shell are shared collectively and they can move freely.
2.4. Properties of metallic crystal due to a strong bond:
2.4.1. Hard but not rigid.
2.4.2. Flexible, ductile and malleable.
2.4.3. Solid at normal temperature, unless mercury.
2.4.4. High melting and boiling points.
2.4.5. Insoluble.
2.4.6. Good conductors of electricity and heat.
3. COVALENT BOND: NonMetal-NonMetal
3.1. Molecules
3.1.1. Atoms share electrons in each bond to comply the octet rule.
3.1.2. Due to molecular forces substances can be:
3.1.2.1. Extremely weak - Gases
3.1.2.2. Relatively strong - Liquids
3.1.2.3. Strong - Molecular solids.
3.1.3. Properties of molecular compounds due to the forces between molecules:
3.1.3.1. Solids, liquids or gases.
3.1.3.2. Low melting and boiling points.
3.1.3.3. Solids are malleable.
3.1.3.4. Insoluble in water but they can dissolve in some polar solvents.
3.1.3.5. They do not conduct electricity.
3.2. covalent crystals
3.2.1. Atoms share electrons in each bond to comply the octet rule.
3.2.2. Atoms are fixed in a 3D lattice but electrons are fixed in each covalent bond.
3.2.3. Properties of covalent crystals due to a strong bond:
3.2.3.1. Hard and rigid.
3.2.3.2. Brittle.
3.2.3.3. Solid at normal temperature.
3.2.3.4. High melting and boiling points.
3.2.3.5. Insoluble.
3.2.3.6. They do not conduct electricity.