Similarities) and contrast (differences) ionic and covalent bonding.

Full Answer Section

• Covalent Bonding: Electrons are shared between atoms, forming pairs that occupy the orbitals of both atoms and create a molecule.

Electronegativity:

• Ionic Bonding: Significant difference in electronegativity between metal (low) and non-metal (high) drives the complete electron transfer.
• Covalent Bonding: Electronegativity difference can be small or large.
  • Polar covalent bond: Unequal sharing of electrons occurs when one atom has higher electronegativity and pulls the shared pair closer to itself.
  • Nonpolar covalent bond: Electrons are shared equally when atoms have similar electronegativity.

Examples:

• Ionic Molecule: Sodium chloride (NaCl), IUPAC name: Sodium chloride
• Covalent Molecule: Methane (CH4), IUPAC name: Methane

Additional Examples:

• Ionic: Magnesium oxide (MgO)
• Covalent: Ammonia (NH3)

Remember, these are just representative examples, and numerous other molecules exist for each type of bonding. Identifying which type of bonding a molecule has involves analyzing the electronegativity difference and electron placement.

Sample Solution

Comparing and Contrasting Ionic and Covalent Bonding:

Similarities:

• Both involve sharing or transferring electrons to achieve a stable configuration with eight electrons in their outermost shell (the octet rule).
• Both create molecules with strong attractive forces between atoms, holding them together.
• Both are fundamental forces responsible for building a vast array of chemical compounds.

Differences:

Electron Involvement:

• Ionic Bonding: Electrons are completely transferred from one atom (usually a metal) to another (usually a non-metal), creating charged ions that attract electrostatically.