Chemical Bonding Types

Chemical Bonding

Types of Chemical Bonds

• Ionic Bonds: formed by the transfer of electrons between atoms, resulting in the formation of ions with opposite charges.
  • Typically formed between metals and non-metals.
  • Examples: NaCl (sodium chloride), CaCO3 (calcium carbonate).
• Covalent Bonds: formed by the sharing of electrons between atoms.
  • Typically formed between non-metals.
  • Examples: H2 (hydrogen gas), CO2 (carbon dioxide).

Bonding Theories

• Electron Sea Model: assumes that electrons are delocalized and free to move throughout the metal lattice.
• Molecular Orbital Theory: describes the arrangement of electrons in molecules in terms of molecular orbitals.
• Valence Shell Electron Pair Repulsion (VSEPR) Theory: predicts the shape of molecules based on the arrangement of electron pairs around the central atom.

Polarity of Molecules

• Polar Molecules: have a permanent electric dipole moment due to unequal sharing of electrons.
  • Examples: H2O (water), CO (carbon monoxide).
• Nonpolar Molecules: have a symmetric shape and equal sharing of electrons.
  • Examples: O2 (oxygen gas), N2 (nitrogen gas).

Bond Strength and Length

• Bond Strength: the energy required to break a chemical bond.
• Bond Length: the average distance between the nuclei of two bonded atoms.
  • Factors affecting bond length: atomic size, electronegativity, and bond order.

Chemical Bonding

Types of Chemical Bonds

• Ionic bonds are formed by the transfer of electrons between atoms, resulting in the formation of ions with opposite charges, typically between metals and non-metals.
• Examples of ionic bonds include NaCl (sodium chloride) and CaCO3 (calcium carbonate).
• Covalent bonds are formed by the sharing of electrons between atoms, typically between non-metals.
• Examples of covalent bonds include H2 (hydrogen gas) and CO2 (carbon dioxide).

Bonding Theories

• The Electron Sea Model assumes that electrons are delocalized and free to move throughout the metal lattice.
• Molecular Orbital Theory describes the arrangement of electrons in molecules in terms of molecular orbitals.
• VSEPR Theory predicts the shape of molecules based on the arrangement of electron pairs around the central atom.

Polarity of Molecules

• Polar molecules have a permanent electric dipole moment due to unequal sharing of electrons, such as H2O (water) and CO (carbon monoxide).
• Nonpolar molecules have a symmetric shape and equal sharing of electrons, such as O2 (oxygen gas) and N2 (nitrogen gas).

Bond Strength and Length

• Bond strength is the energy required to break a chemical bond.
• Bond length is the average distance between the nuclei of two bonded atoms, affected by factors such as atomic size, electronegativity, and bond order.