Chapter 6-7 Covalent Bonding Flashcards
The normally weak forces of attraction that exist between molecules.
Intermolecular forces
What is the formula for the compound carbon tetraiodide?
CI4
States that chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has 8 valence electrons.
Octet rule
The energy required to break a chemical bond and form neutral, isolated atoms.
Bond (dissociation) energy
A molecule that has a partial positive end and a partial negative end.
A dipole
A particularly strong dipole-dipole interaction that results from the attraction between a hydrogen atom bonded to fluorine, oxygen, or nitrogen and another F, O, or N atom
Hydrogen bonding
Indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts.
Chemical formula
Draw the Lewis structure and predict the molecular for geometry for the compound SeF6.
Intermolecular attractive force that results from the constant motion of electrons and the creation of instantaneous dipoles
London (Dispersion) forces
Draw the Lewis structure for the azide ion, N3-1. What is the predicted shape of the ion?
A covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge. The electronegativity difference between the atoms is between 0 and 0.3.
Non-polar covalent bond
Uranium(VI) fluoride is a compound used in the uranium enrichment process that produces fuel for nuclear reactors and nuclear weapons. Calculate the percent composition to one decimal place for each element.
Refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure.
Resonance structures
What is the name of the compound SO3?
Sulfur trioxide
What is the formula for the compound dinitrogen trioxide?
N2O3
What is the name of the compound ICl3?
Iodine trichloride