Covalent Bonding

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noble gas

Group 18: Nonreactive family of nonmetals; 8 valence e- (full octet). All are gases at room temp.

diatomic elements

H2, N2, O2, F2, Cl2, Br2, I2 (Use the 7-up shortcut to help you!)

octet rule

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons

trigonal planer

The shape of a molecule with three bonded atoms and no lone pairs

nonpolar covalent bond

a bond formed when the atoms in a molecule are alike and the bonding electrons are shared equally

polar covalent bond

a bond formed when the atoms in a molecule are different and the bonding electrons are shared unequally

polar bond

a bond formed when two different atoms are joined by a covalent bond and the bonding electrons are shared unequally

single covalent bond

a bond in which two atoms share a pair of electrons

polar molecule

a molecule, like water, in which one or more atoms is slightly negative and one or more is slightly positive, unless molecular geometry causes the polarities to cancel each other out

hydrogen bond

a relatively strong intermolecular force in which a hydrogen atom that is covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom in the same molecule or one nearby

linear structure

all atoms in a line O=C=O

triple covalent bonds

bonds that involve three shared pairs of electrons

double covalent bonds

bonds that involve two shared pairs of electrons

structural formulas

chemical formulas that show the arrangement of atoms in molecules and polyatomic ions; each "-" indicates one pair of shared electrons

octa-

eight

Bond energy

energy required to break a bond

penta-

five

Lewis Structures

formulas 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

tetra-

four

nona-

nine

mono-

one

unshared pairs

pairs of valence electrons that are not shared between atoms; aka lone pairs or nonbonding pairs

octahedral

rule breaker

hepta-

seven

hexa-

six

resonance structures

structures that occur when it is possible to write two or more valid electron dot formulas that have the same number of electron pairs for a molecule or ion

deca-

ten

tri-

three

di-

two

VSEPR theory

valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence-electron pairs are as far apart as possible

ALL HALOGENS AND HYDROGEN

1 bond ONLY

bent

2 atoms bonded to central atom 1 lone pair of electrons or 2 atoms bonded to central atom 2 lone pair of electrons

oxygen

2 bonds 2 lone pairs of electrons (element)

nitrogen

3 bonds 1 lone pair of electrons (element)

trigonal pyramidal

3 bonds, 1 lone pair

Group 14

4 Valence Electrons....needs 4 more to reach 8 4 Bonds no lone pair of electrons

carbon

4 bonds 0 lone pair of electrons (element)

trigonal bipyramidal

5 bonded atoms, 0 lone pairs

Group 15

5 valence electrons.......needs 3 more to reach 8 3 Bonds one lone pair of electrons

Group 16

6 valence electrons.......needs 2 more to reach 8 2 Bonds 2 lone pairs of electrons

Group 17

7 valence electrons.......needs 1 more to reach 8 1 Bond

electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

Bond

An attractive force acting between atoms


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