IB CHEM EXAM

Ammonium

1+ & NH₄ ⁺

Hydroxide

1- & OH^-

Nitrate

1- & NO₃ ^-

Hydrogencarbonate

1- & HCO₃^-

Carbonate

CO32-

Sulfate

SO₄ ^2-

Phosphate

3- & PO₄^3-

Tetrahedral, Tetrahedral

4 e^- , 4 bonding pairs, 0 lone pairs, 109.5^o

Tetrahedral, Trigonal Pyramidal

4 e^- , 3 bonding pairs, 1 lone pairs, 107^o

Tetrahedral bent

4e^-, 2 bonding pairs, 2 lone pairs, 105^o

Trigonal Planar, Trigonal Planar

3e^-, 3 bonding pairs, 0 lone pairs, 120^o

Trigonal Planar, V-shaped

3e^-, 2 bonding pair, 1 lone pair, 117^o

Linear, Linear

2e^-, 2 bonding pair, 0 lone pairs, 180^o.

London Disperson Forces

Formed btw induced dipoles. Can exist btw: 2 nonpolar molecules, 2 polar molecules (nonpolar “ends”), or a nonpolar and a polar molecule (nonpolar end). Weak

Covalent bonds

sharing electrons & low and high electronegativity

Polar covalent bonds ( polar bonds)

unequal sharing of electrons low & high electronegativity,(difference of 0.4)

Dipole-Induced Dipole

Forms btw dipole and a nonpolar species. Dipole causes the movement of elecrons in a neutral speices to shift to one side, thus the formation of an induced-dipole

Dipole-Dipole Forces

Forms btw 2 polar molecules. Dipole describes the permenant separation of positive & negative charge in a molecule.

Hydrogen Bond

Special version of dipole-dipole bond. 2 molecules must be a polar & 1 must contsin sn available hydrogen (i.e. polar bond) & other molecules must have N,O,F (PT).

Conducts Electricity

Ability of an electron/ion to flow freely in a substance

Malleable

able to be hammered /pressed permanently out of shape w/out breaking or cracking.

Metals conduct electricity

Due to delocalized electrons

Metals are malleable

Due to non-directional bond (btw electron & positive nucleus).

Lattice strength is infleuced by atomic radius & ionic charge

smaller atomic radius = larger attractive force & greater ionic charge = larger attractive force

Ionic Bond

attraction btw oppositvely charged ions & high & low electronegatively.