Chemical Bonding and Molecular Structure

Ionic Bonds

1. Ionic bonds are formed by the complete transfer of electrons from one atom to another.
2. These bonds occur between a metal and a non-metal.
3. The atom that loses electrons becomes a cation, and the atom that gains electrons becomes an anion.
4. The bond is held together by strong electrostatic forces of attraction between oppositely charged ions.
5. Common examples include sodium chloride (NaCl) and magnesium oxide (MgO

Overview of Gas Laws

1. Gas laws describe the behavior of gases under various conditions of pressure, temperature, and volume.
2. These laws are based on the kinetic theory of gases, which assumes that gas molecules are in constant random motion.
3. The major gas laws include Boyle’s law, Charles’s law, and Avogadro’s law.
4. The combined gas laws form the foundation for the ideal gas equation, PV = nRT.

Boyle’s Law

Overview of Intermolecular Forces

1. Intermolecular forces are forces of attraction or repulsion between neighboring molecules.
2. They are weaker than intramolecular forces (such as covalent or ionic bonds).
3. These forces determine physical properties like boiling points, melting points, and solubility.
4. The three main types of intermolecular forces are dipole-dipole interactions, London dispersion forces, and hydrogen bonding.

VSEPR Theory

1. VSEPR Theory stands for Valence Shell Electron Pair Repulsion Theory.
2. It is used to predict the shape of molecules based on electron pair repulsion.
3. The theory states that electron pairs around a central atom arrange themselves to minimize repulsion.
4. Both bonding pairs and lone pairs of electrons influence molecular geometry.
5. Lone pairs occupy more space than bonding pairs due to greater repulsion.
6. The molecu

Valence Bond Theory (VBT)

1. Valence Bond Theory (VBT) explains the formation of chemical bonds through the overlap of atomic orbitals.
2. In VBT, atoms combine by overlapping their valence orbitals to form bonds.
3. The overlapping orbitals contain unpaired electrons, which pair up to form a covalent bond.
4. Bond strength depends on the extent of overlap; greater overlap results in stronger bonds.
5. VBT distinguishes between sigma (σ) and pi (π) bonds based