5 Written questions
5 Matching questions
- Octet Rule
- Electron Affinity
- Hydrogen and Lewis Structures
- Ionization Energy
- Dipole Moment
- a 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.
- b H is never the central atom.
- c A quantitative measure of the magnitude of a dipole. The higher the dipole moment, the more polar is the molecule.
- d 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.
- e States that representative elements tend to gain, lose, or share electrons until they are surrounded by eight valence electrons (an octet).
5 Multiple choice questions
- Hydrogen provides an exception to the octet rule because it requires only two electrons to attain a noble gas configuration.
- Two or more Lewis structures that are equally good representations of the bonding in a molecule or ion. Usually differ only in the positions of multiple bonds or single, unpaired electrons.
- (∆ 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.
- A molecule with one end having a slight positive charge and the other end having a slight negative charge due to differences in electronegativity. Arrow points towards the more electronegative element.
- Orbital Hybridization sp2
5 True/False questions
Sextet Rule Elements → H
2 ED → Orbital Hybridization sp
Ions → Form when electrons transfer from an atom of low ionization energy (usually a metal) to an atom of high electron affinity (usually a nonmetal). The electrostatic attraction between two oppositely charged ions constitutes this bond.
Covalent Bond → Results from sharing electrons between two atoms, usually nonmetal atoms.
Polar Covalent → 0.4-1.0