Unit 3 Honors Chemistry

ionic bond

when nonmetals and metals bond together to create a charge

covalent bond

when two or more nonmetals SHARE electrons between each other ex. Fluorine 7 and fluorine 7

metallic bonding

metals lose electrons or they roam freely throughout metals in order to create a cation

Octet rule

an atom must have 8 valence electrons to be completely stable like the noble gases

Lewis Dot Symbol

a diagram the shows the amount of electrons in an atom and helps in explaining bonds between atoms

atom

in all matter and made up of subatomic particles (neutrons, protons, electrons) and either have a positive, negative, or neutral charge

element

made up of many different atoms, everything is made up of elements. Each posses certain characteristics and are organized as metals, metalloids, or nonmetals on the periodic table

compound

two different elements chemically or physically combined to perform a function ex. NaCl

electronegativity

the tendency for an atom to attract electrons to itself; increases across a period and decreases going down

ion

a form of an element with a positive or negative charge after gaining or losing electrons

cation

a positive ion generally on the left side of the periodic table

anion

a negatively charged ion generally on the right side of the periodic table

ionic compound

a compound composed of negative and positive ions ex. NaCl

covalent compound

a bond shared by the sharing of electrons between atoms ex. Two fluorine atoms

single bond

a bond formed when two atomic orbitals combine and form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei

double (covalent) bond

a bond when two atoms share two pairs of electrons

triple (covalent) bond

a covalent bond in which three pairs of electrons are shared by two atoms

VSEPR theory

Valence-Shell Electron-Pair Repulsion theory; because electron pair repel, molecules adjust their shapes so that the valence electron pairs are as far apart as possible

electron domain

the number of lone pairs or bond locations surrounding an atom or molecule

trigonol planar

the shape of an atom when there is an atom at the end of each orbital (3)

tetrahedral (angle)

a bond angle of 105.9 degrees that result when a central atom forms four bonds directed towards the center of a regular tetrahedron

trigonal pyramid

a molecular shape when there is three bonds on one lone pair on the central atom of a molecule

lone pair

2 electrons not bonded together with another pair of electrons

polar covalent bond

a covalent bond between atoms in which the electrons are shared unequally

nonpolar covalent bond

a covalent bond in which the electrons are shared equally between the two atoms

electrolyte

a compound that carries an electrical charge

nonelectrolyte

a compound that does not conduct an electric current in aqueous solution or in molten state

Dipole moment

measure of net molecular polarity, which is the magnitude of a charge (Q) at either end of the molecular dipole times the distance (r) between the charges

polar molecule

a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive

polyatomic ion

a tightly bound group of atoms that behaves as a unit and has a positive or negative charge

resonance structure

one of the two or more equally valid electron dot structures of a molecule or polyatomic ion