Chemical Bonding: A Comprehensive Guide for High School Chemistry, Study notes of Chemistry

Download Chemical Bonding: A Comprehensive Guide for High School Chemistry and more Study notes Chemistry in PDF only on Docsity!

CHEMICAL BONDING

Chemical Bonding

― defined as any arrangement of electron in two atoms that generates a force, causing the atoms to be bound to each other, forming a molecule

Valence Electrons

➢ electron in the outermost orbital shell ➢ electron that can be gained or lost ➢ Noble gases , complete valence

• most stable

Octet Rule

➢ all atom must have eight electrons ➢ atoms form bonds to have 8 valence electrons ➢ compounds containing 8 valence electrons are stable ➢ does not apply with hydrogen

Lewis Structure

➢ strictly follows the octet rule ➢ illustrations of electrons in an element ➢ dots surrounding elements represents valence electron(s)

Ionic Bonding

― or elctrovalent bond involves the transfer of electrons from one atom to another, usually between a metal and a non-metal, forming electrically charged atoms of ions ― the strong electrostatic attraction between the cation and the anion hold them together, to form an ionic compound

Ionic Compounds

➢ hard and brittle ➢ form crystal lattices rather than amorphous solids ➢ have high melting and boiling point ➢ conduct electricity when dissolved in water ➢ good insulators in solid state

Covalent Bonding

― formed when two electrons are shared between two or more atoms resulting in the formation of a molecule ― the shared pair of electrons is simultaneously being attracted by the nuclei of the two atoms, thus holding them together ― generally formed between non-metals

Covalent Bonding

Covalency number

― number of covalent bonds that an atom can form within a molecule ― number of unpaired electrons indicates the number of covalent bonds

Types of Covalent Bonds

Normal Covalent bond ― formed when both atoms donate to form the shared pair Coordinate covalent bonds ― formed when the electrons that constitute the shared electron pair comes from only one of the participating atoms

Bond Polarity

➢ bonding between unlike atoms results in unequal sharing of the electrons ➢ one atom pulls the electrons in the bond closer to its side and one end of the bond has larger electron density than the other ➢ the end with the larger electron density gets a partial negative charge and the end that is electron deficient gets a partial positive charge H Cl

d+ d-