Chapter 6- Bonding Flashcards
A formula in which atomic symbols represent nuclei and inner shell electrons, dot pairs, or dashes between two atomic symbols represent electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent unshared electrons.
Lewis structure
A chemical bond resulting from the sharing of an electron pair between two atoms
Covalent Bonding
A Formula that indicates the relative numbers of atoms of each card in a chemical compound by using atomic symbols and numerical subscripts
Chemical formula
A covalent bond in which the bonding electrons are shared equally by the bonded atoms resulting in a balanced just distribution of electrical charge
Nonpolar covalent bond
A formula showing the types and numbers of atoms combined in a single molecule of a molecular compound
Molecular Formula
A chemical compound whose simplest units are molecules
Molecular compound
A formula that indicates the number and types of atoms present in the molecule and also shows the bonding arrangement of the atoms; A formula that indicates the kind of numbers errands and lines but not that unsure electron pairs of the atoms and molecule
Structural formula
Electronic configuration medication which only the valence electrons of an atom of a particular element are shown, indicated by the dot placed around elements symbol
Electron dot notation
And molecule containing only two atoms
Diatomic molecule
The distance between two bonded atoms at their minimum potential energy that is the average distance between two bonded atoms.
Bond length
Having an uneven distribution of charge
Polar
The energy required to break a chemical bond and form neutral isolated atoms
Bond energy
Chemical compounds tend to form so that each atom by gaining or losing or sharing electrons has an octet of electrons in its highest occupied energy level
Octet rule
A double or triple bond
Multiple bond
Repulsion between that valence level electrons surrounding an atom causes these sets to be oriented as far apart as possible
VSEPR theory
