2.2.2 Bonding and structure

• what is average bond enthalpy?

  The average energy required to break a bond, used as a measurement of the strength of a covalent bond.
• what is a bonding pair?

  A pair of electrons shared between two atoms in a covalent bond.
• what is a covalent bond?

  A strong bond formed between 2 atoms due to the electrostatic attraction between a shared pair of electrons and the atomic nuclei.
• What is a dative covalent bond?

  a type of covalent bond in which both of the electrons in the shared pair come from one atom.
• what is electronegativity?

  the ability of an atom to attract bonding electrons in a covalent bond. This is often quantified using Pauling’s electronegativity values. Electronegativity increases towards F in the periodic table.
• What is the electron pair repulsion theory?

  Theory that states that electron pairs in the valence shell of an atom repel each other and arrange themselves in a way that minimizes repulsion.
• what is hydrogen bonding?

  Attraction between a hydrogen atom and an electronegative atom.
• What are intermolecular bonding?

  Intermolecular bonding refers to the forces of attraction between molecules.
• What is an ionic bond?

  The electrostatic attraction between oppositely charged ions
• what is an ionic compund?

  a compound made up of oppositely charged ions
• what is an ionic lattice?

  a giant structure in which oppositely charged ions are strongly attracted in all

  directions
• what is meant by linear?

  he shape of a molecule in which the central atom has 2 bonding pairs.
• what are london dispersion forces?

  induced dipole-dipole interactions caused when the random movement of electrons creates a temporary dipole in one molecule which then induces a dipole in a neighbouring molecule.
• what is a lone pair?

  a pair of outer-shell electrons not involved in bonding