5 Written questions
5 Matching questions
- Lattice Energy
- Electronegativity and Polarity
- Lewis Structure
- EDG Tetrahedral
- a MG Tetrahedral
MG Trigonal pyramidal
- b The greater the electronegativity difference between two atoms the more polar the bond.
- c (∆ H lattice) is the energy required to completely separate a mole of a solid ionic compound into its gaseous ions. Ionic compounds tend to have high lattice energies, which tend to make ionic compounds hard and brittle with relatively high melting points.
- d For covalent molecules often show shared pairs of electrons (bonding pairs) as lines and unshared electron pairs (nonbonding pairs) as lines or dots.
- e Refers to the arrangement of a molecule's atoms in three-dimensional space.
5 Multiple choice questions
- Results from sharing electrons between two atoms, usually nonmetal atoms.
- A model that is based on the natural repulsive forces that electron pairs exhibit within a molecule.
- MG Linear
- A bond in which the electrons are shared equally between two atoms.
- The energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
5 True/False questions
6 ED → Orbital Hybridization sp
Ionization Energy → The energy required to remove an electron from an atom or ion in the gaseous state. Increases from left to right and from bottom to top on the Periodic Table.
EDG Trigonal Planar → MG Trigonal Planar
Ionic → >2.0
Ionic Bond → An attractive force between ions of opposite charges, often a metal cation and a nonmetal anion.