Chemistry-Bonds

linear angle?

180

trigonal planar angle?

120

tetrahedral angle?

109\.5

trigonal pyramidal angle?

107\.3

bent angle?

104\.5

linear hybrid orbital?

sp

trigonal planar hybrid orbital?

sp^2

tetrahedral hybrid orbital?

sp^3

trigonal pyramidal hybrid orbital?

sp^3

bent hybrid orbital?

sp^3

Stability is achieved through?

sharing electrons, forming bonds

Covalent bonds occur between?

non-metals

Ionic bonds form between?

metals and nonmetals

Ionic characteristics?

strong, high melting/boiling points, solid, conduct electricity, electrons transfer, attraction between oppositely charged ions

Covalent characteristics?

weak, low melting/boiling points, liquid/gas, non conductors, electrons shared, attraction between v/e and nucleus

What bond requires one electron from each atom?

covalent

Sigma bond?

single covalent bonds

Pi bond?

multiple bonds; occurs when orbitals are parallel and share electrons

Shorter length of bond?

greater strength (stronger bond)

Forming a bond?

releases energy

Breaking a bond?

requires energy

How to name covalent compounds?

first element + second element with -ide, add prefixes when needed

Two types of acids?

binary; oxyacid

What are binary acids?

hydrogen + one other element; first word is hydro + root of other element + ic acid

What are oxyacids?

acid with hydrogen + polyatomic ion containing O

VSEPR model?

valence shell electron pair repulsion model; based on arrangement that minimizes electron repulsion

What causes fixed angles?

electron clouds repelling one another

What is hybridization?

atomic orbitals mix and form new identical hybrid orbitals

What is electronegativity?

relative ability of an atom to attract electrons in a chemical bond

How to find bond character?

find the difference of 2 elements

Polar covalent bonds?

electrons are pulled toward one atom more than the other

More electronegative end attracts what?

electrons

Nonpolar covalent bonds?

electrons are shared equally

Bonds between atoms of the same element are always?

nonpolar

Polar’s lone pairs make it what?

asymmetrical

Nonpolar models?

symmetrical; they cancel out

What are intermolecular forces?

forces between different molecules weaker than bonds in a molecule or ionic compound

Dispersion force?

not strong (nonpolar molecules)

Dipole-dipole effect

strong (polar molecules)

Hydrogen bond?

very strong

Properties of covalent compounds

low melting points, gases

Soluble in polar substances?

polar and ionic molecules

Soluble in nonpolar?

nonpolar molecules

Covalent network solids result in?

hard, non-conductive, brittle, solid, w/ high melting pt