Chem Exam 2 Review

aufbau principle

1. lower energy orbitals fill first

2. orbitals hold 2 electrons w/ opposite spins

3. if degenerate orbitals → ½ fill each orbital w/ the same spin before

valence shells

outermost shell/largest n-value

valence electrons

the electrons in the valence shell

core electrons

inner shell electrons (remaining electrons)

anomaly Cr

[Ar] 4s1 3d5

anomaly Mo

[Kr] 5s1 4d5

anomaly Cu

[Ar] 4s1 3d10

anomaly Ag

[Kr] 5s1 4d10

anomaly Pd

[Kr] 4d10

increasing Zeff

strong pull to the nucleus

decreasing Zeff

weak pull to the nucleus

metals

low ionization energies/tend to form cations

malleable, ductile, good conductors

nonmetals

large negative electron affinities/tend to form anions

poor conductors

metalloids

intermediate prop/good semiconductors

alkali

1A → form +1, most reactive metals

alkaline earth

2A → forms +2, reactive

chalcogens

6A → forms -2

halogens

7A → forms -1, most reactive nonmetals

noble gases

8A → inert. (no charge)

covalent bonds

sharing of e-, nonmetal + nonmetal, metalloids + nonmetal

ionic bonds

transfer of e-, metal + nonmetal, cation + anion

cations

parent + roman numeral charge + ion

anions

parent - ending + ide + ion

Hg₂²⁺

Mercury

NH₄⁺

Ammonium

NO₂^-

Nitrite

NO₃^-

Nitrate

SO₃^2-

Sulfite

SO₄^2-

Sulfate

HSO₄^-

Hydrogen Sulfate

OH^-

Hydroxide

CN^-

Cyanide

PO₄^3-

Phosphate

HPO₄^2-

Hydrogen Phosphate

H₂PO₄^-

Dihydrogen Phosphate

NCS^-

Thiocynate

CO₃^2-

Carbonate

HCO₃^-

Hydrogen Carbonate

ClO^-

Hypochlorite

ClO₂^-

Chlorite

ClO₃^-

Chlorate

ClO₄^-

Perchlorate

C₂H₃O₂^-

Acetate

MnO₄^-

Permanganate

Cr₂O₇^2-

Dichromate

CrO₄^2-

Chromate

O₂^2-

Peroxide

C₂O₄^-

Oxalate

S₂O₃^2-

Thiosulfate

linear

sp

trigonal planar

sp2

tetrahedral

sp3

trigonal bipyramidal

sp3d

octahedral

sp3d2

ionic bonding

a metal and non-metal bonding

polar covalent bond

2 nonmetals w a dipole present

non polar covalent

2 nonmetal w similar EN pulls