Bonding and Molecular Geometry

Ionic bond

involves a transfer of electrons- metal and nonmetal (more brittle, higher melting and boiling points, can conduct electricity)

Covalent bond

involves a sharing of electrons- two nonmetals, (form non-reactive gases, low melting/boiling point, polarity)

Metallic bond

involves delocalized electrons- two metals

luster

the electrons allow the light to be reflected off the surface of a metal

linear bond

two atoms attached to a central atom, 0 lone pairs, bond angle of 180 (CO2)

trigonal planar

trigonal planar- 3 atoms attached to one center atom, 0 lone pairs, bond angle of 120 (BF3)

bent (one lone pair)

bent-2 atoms attached to center atom, 1 lone pair, <120 (NO2-)

bent (two lone pairs)

2 atoms attached to center atom, 2 lone pairs, 104.5 (H20)

trigonal pyramidal

3 atoms attached to center atom, 1 lone pair, 107 (NH3)

tetrahedral bond

tetrahedral- 4 atoms attached to one center atom, 0 lone pairs, bond angle is 109.5 (CH4)

Octahedral

6 atoms attached to central atom, 0 lone pairs, bond angle is 90 (SF6)

nonpolar covalent polarity

two same nonmetals or all outer atoms are identical and central atom has no lone pairs

polar covalent polarity

two different nonmetals, outer atoms aren't identical, central atom has lone pairs

polar bonds

form when a high electronegativity atom bonds with a low electronegativity atom

molecular geometry

Includes the lone pairs (if there's 3 bonds, 1 lone pairs it's trigonal pyramidal)

electron domain geometry

does not include lone pairs (if there's 3 bond, 1 lone pair it's tetrahedral)

sea of electrons

metallic

shortest bond

3 bonds

weakest bond

1 bond

sharing of 2 electrons

1 bond

most reactive metals

halogens

isotopes

change in # of neutrons

ions

lost or gained an electron to form a cation or anion

speed of light

c = 3.00 x 10^8

how to find speed

c=λv

photon

quantum of light

higher to lower wavelength

energy is released/emitted

lower to higher wavelength

energy is absorbed

effective nuclear charge

highest towards the right

atomic radius

largest on bottom left

ionization energy and electronegativity, nonmetallic c/r

highest on top right

metallic character/reactivity

highest bottom left

strength of forces; strongest to weakest

ion-ion, H bonding, dipole-dipole, LDF

stronger the force the higher the

melting point, boiling point, viscosity, surface tension

dipole-dipole

attractions between oppositely charged regions of polar molecules

h bonding

occurs when H bonds with F, O, N

ion-dipole

ion and polar molecule, force is strong enough that ionic substances can dissolve in polar substances

LDF

for ALL nonpolar