Chem 1211 elc quiz + final chapters

Degenerate

Single electron atom (H): only n needs to be the same

Multi-electron atoms: same n and l make it degenerate

Effective nuclear charge (Z_eff)

Increases across the periodic table

Cab be approx. with (atomic # - # of core electrons)

Shell filling order exceptions

Chromium (Cr) , Molybdenum (Mo), Copper (Cu), Silver (Ag), Gold (Ag)

Excited states

An electron missing from a lower energy subshell moves to a higher subshell but the # of electrons stay the same

Losing electrons

Electrons are removed from the highest energy subshell first

Paramagnetic / Diamagnetic

paramagnetic: element has unpaired electrons; is magnetic

diamagnetic: element has no unpaired electrons; not magnetic

Ionization energy

Increases to the right and up the periodic table

Exceptions: groups 2←→13, 15←→16

x(g) → x⁺ (g) + e^-

Second Ionization energy

e^- is removed from an element that has already lost one electron

Electron attachment enthalpy

Increase to the up and to the right on the periodic table

Exceptions: groups 14←→15, 1←→2, rows 2←→3

x(g) + e^- → x^- (g)

typically exothermic

Atomic radius

Increases down and to the left of the periodic table

Ions with a more (-) charge (anions) are bigger than cations

isoelectronic = same # of e^-

When comparing isoelectronic atoms/ions the higher # protons = a smaller compound

Polarizability

Increases down and to the left of the periodic table

A higher atomic radius = higher polarizability

cations⁺ are smaller than anions^-

Electronegativity

Increases up and to the right of the periodic table

An atoms ability to attract electrons to itself

Noble gases are excluded

Number of bonds

8 - # v.e^- = # of bonds

Lattice energy

Lattice energy increases as charge increases and atomic radius decreases

Octet rule exceptions

H only needs 2 e^-

B only needs 6 e^- or 3 bonds

Period 3 and higher can exceed 8 electrons

Formal charge

v.e^- - lines - dots = charge

negative charges go on most electronegative element

positive charges go on least electronegative charges

best structures contribute the most

Resonance structures

Can have more than 1 equal structure

Usually have double or triple bonds

Reactivity

Compounds with odd # of e^- are more reactive

VESPR: 2 electron groups

E: linear

0 lone pairs

M: linear

Angle: 180

VESPR: 3 electron groups

E: trigonal planar , 0 lone pairs = M: trigonal planar , angle; 120

E: trigonal planar, 1 lone pair = M: bent , angle: <120

VESPR: 4 electron groups

E: tetrahedral, 0 lone pairs = M: tetrahedral, angle: 109.5

E: tetrahedral, 1 lone pair = M trigonal pyramidal, angle: <109.5

E: tetrahedral, 2 lone pairs = M: bent, angle: <109.5

VESPR: 5 electron groups

E: trigonal bypyramidal, 0 lone pairs = M: trigonal bypyramidal, angle: 120, 90

E: trigonal bypyramidal, 1 lone pair = M: seesaw, angle: <120, 90

E: trigonal bypyramidal, 2 lone pairs = M: t-shaped, angle: 180, 90

E: trigonal bypyramidal, 3 lone pairs = M: linear, angle: 180

VESPR: 6 electron groups

E: octahedral, 0 lone pairs = M: octahedral, angle: 90

E: octahedral, 1 lone pair = M: square pyramidal, angle: 90

E: octahedral, 2 lone pairs = M: square planar, angle: 90