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CL4 Definition


Electronegativity the ability of an atom in an element to attract electrons in an compound
Valence electrons the electrons in the highest occupies level of an elements atoms
Electron dot structures Diagrams that show valence electrons in the atoms of an element as dots.
Ions an atom or molecule with a net charge due to the loss or gain of one or more electrons
molecule a neutral group of atoms joined together by covalent bonds
The octet rule states that in forming compounds, atoms tend to achieve the electron configuration of a noble gas
Halide ion a halogen atom bearing a negative charge
Ionic compound a compound composed of cations and anions. Electrically neutral.
Ionic bond The electrostatic forces that hold ions together in ionic compounds
Chemical formula Shows the number of atoms in each element in the smallest representative unit of a substance.
formula unit the lowest whole-number ratio of ions in an ionic compound
The coordination number of an ion the number of ions of opposite charges that surround the ion in a crystal.
Metallic bond the forces of attraction between the free-floating valence electrons and the positively charged (cations) metal ions.
Alloys mixtures of two or more elements, at least one in which is a metal.
covalent bonds atoms that are held together by sharing electrons are joined by this
diatomic molecule a molecule that contains two atoms
molecular compound a compound composed of molecules
molecular formula the chemical formula of a molecular compound
single covalent formed two atoms held together by sharing one pair of electrons are joined by this
structural formula represents the covalent bonds as dashes and shows the arrangement of covalently bonded atoms.
unshared pair A pair of valence electrons that is not shared between atoms
double covalent bond a bond that involves two shared pairs of electrons
triple covalent bond a bond formed by sharing three pairs of electrons
coordinate covalent bond a covalent bond in which one atom contributes boht bonding electrons
polyatomic ion a tightly bound group of atoms that has a positive or negative charge and behaves as a unit
bond dissociation energy the energy required to break the bond between two covalently bonded atoms
nonpolar covalent bond when the atoms in the bond pull equally, the bonding electrons are shared equally and each bond formed is this
polar covalent bond a covalent bond between atoms in which the electrons are shared equally
polar molecule one end of the molecule is slightly negative and the other end is slightly positive
dipole a molecule that has two poles is called a dipolar molecule or this
van der Waales forces the two weakest attractions between two molecules are collectively called this named after the dutch chemist.
dipole interaction this occurs when polar molecules are attracted to one another
dispersion force the weakest of all molecular interactions are caused by electrons
hydrogen bonds are attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom
network solid solids in which all of the atoms are covalently bonded to each other.
Created by: TJ365