5 Written questions
5 Matching questions
- Resonance Structures
- Octet Rule
- Metallic Bond
- Ionization Energy
- 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 Occurs when the nuclei of a collection of metal atoms simultaneously attract their collective electrons.
- c States that representative elements tend to gain, lose, or share electrons until they are surrounded by eight valence electrons (an octet).
- d 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.
- e 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.
5 Multiple choice questions
- (∆ 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.
- Refers to the arrangement of a molecule's atoms in three-dimensional space.
- Al, B
- The arrangement of electron domains around the central atom of a molecule.
- Results from sharing electrons between two atoms, usually nonmetal atoms.
5 True/False questions
Molecular Geometry → Refers to the arrangement of a molecule's atoms in three-dimensional space.
Electronegativity and Polarity → The greater the electronegativity difference between two atoms the more polar the bond.
Isoelectric → When an atom gains or loses electrons to attain an octet of valence electrons, it does not become a noble gas. Chloride ion, Cl-, has the same electron configuration as argon, but it is not argon. Chloride ion has the same number of electrons (term) with argon but chloride has one fewer proton.
Lattice → A stable, ordered, solid three-dimensional array of ions associated with ionic compounds.
Ionic → >2.0