Chemistry Terms ЁЯФм
Electron dot structures
Diagrams that show valence electrons as dots
Lone pairs
Electrons unused in bonding bonding
Alloy
Mixtures composed of two or more elements, at least one of which is a metal.
Dipole interactions
Occur when polar molecules are attracted to one another
Polar molecule
One end of the molecule is slightly negative and the other end is slightly positive
Chemical formula
Shows the kinds and numbers of atoms in the smallest representative unit of a substance
Resonance structure
A structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
Polyatomic ion
A tightly bound group of atoms that has a positive or negative charge and behaves as a unit
Octet rule
An octet is a group of eight electrons; in forming compounds atoms want to achieve the electron configuration of a noble gas.
Hydrogen bonds
Attractive forces in which hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom.
Single bond
Two atoms held together by sharing a pair of electrons
No polar covalent bonds
When the atoms in the bond pull equally, the bonding electrons are shared unequally.
Molecule
A neutral group of atoms joined together by covalent bonds
Coordinate covalent bond
A covalent bond in which one atom contributes both bonding electrons
Duet rule
A duet is a pair of electrons; this rule is followed by hydrogen, which only needs on more electron to be content.
Diatomic molecule
A molecule consisting of two atoms
Dipole
A molecule that has two poles
Ionic compounds
Compounds composed cations and anions
Metallic bonds
Consists of attraction of the free floating valence electrons for the positively charged metal ions.
Triple bond
Formed by the sharing of three pairs of electrons
Double bond
Involves two shared pairs of electrons
Covalent bond
The atoms held together by sharing electrons
Valence electrons
The electrons in the highest occupied energy level of an element's atoms
Ionic bond
The electrostatic forces that hold ions together in ionic compounds
VSPER theory
The idea that the repulsion between electron pairs causes molecular shapes to adjust so that the valence electron pairs stay far apart
Formula unit
The lowest whole number ratio of ions in an ionic compound
Coordination number
The number of ions of opposing charge that surround the ion in a crystal.
Dispersion forces
The weakest of all molecular interactions, are caused by the motion of electrons
