Chem 1601 Final Things to Know

tera

10^12

exceptions to octet rule

B - 6 electrons, Be - 2 electrons, H - 2 electron

molecular geometries that tend to be polar

bent, trigonal pyramidal

molecular geometries that tend to be nonpolar

trigonal planar, linear, tetrahedral (when same element around)

density of gas

g/L = (P)(MM)/RT

giga

10^9

mega

10^6

kilo

10^3

deci

10^-1

centi

10^-2

milli

10^-3

micro

10^-6

nano

10^-9

pico

10^-12

femto

10^-15

atomic mass

A; protons + neutrons

atomic number

Z; protons

wavelength spectrum (in order of increasing energy)

radio waves
microwave
infrared
visible (ROYGBIV)
Ultraviolet
X Ray
Gamma Ray

polyatomic ion pattern

1- HYPO__ITE, 2-___ITE, 3-___ATE, 4-PER___ATE

naming acids

ide- hydro_______ ic
ate - ic
ite- ous

oxalate

C2O4 2-

sulfate

SO4 2-

hydrogen sulfate

HSO4-

Ammonium

NH4+

binary acid

H+element

acetate

C2H3O2-

cyanide

CN-

cyanate

OCN-

thiocyanate

SCN-

hydrogen carbonate

HCO3-

carbonate

CO3 2-

hypochlorite

ClO-

chlorite

ClO2-

chlorate

ClO3-

perchlorate

ClO4-

chromate

CrO4 2-

dichromate

Cr2O7 2-

permanganate

MnO4-

nitrite

NO2-

nitrate

NO3-

hydroxide

OH-

peroxide

O2 2-

Dihydrogen Phosphate

H2PO4-

hydrogen phosphate

HPO4 2-

phosphate

PO4 3-

sulfite

SO3 2-

oxoacid

H+polyatomic ion

Zn charge

2+

Ag charge

1+

Cd charge

2+

Sc charge

3+

number of electrons in orbitals

2n^2

number of orbitals

n^2

exceptions to electron configuration rules

Cr, Mo, Cu, Ag

total number of nodes

n-1

radial nodes

n-l-1

angular/planar nodes

l

number of degenerate orbitals

2l+1

non polar covalent bond EN

0-0.4

polar covalent bond EN

0.4-2.0

ionic bond EN

2.0+

3 bond, 0 lone pair

trigonal planar, 120

2 bond, 1 lone pair

bent, <120

4 bond, 0 lone pair

tetrahedral, 109.5

3 bond, 1 lone pair

trigonal pyramidal, <109.5

2 bond, 2 lone pair

bent, <109.5

5 bond, 0 lone pair

trigonal bipyramidal, 90, 120

4 bond, 1 lone pair

Seesaw <90, <120

3 bond, 2 lone pair

t shaped, <90

2 bond, 3 lone pair

linear, 180

6 bond, 0 lone pair

octahedral, 90

5 bond, 1 lone pair

square pyramidal, <90

4 bond, 2 lone pair

square planar, 90

3 bond, 3 lone pair

t shaped, <90

2 bond, 4 lone pair

linear, 180

alkane

C(single)C

alkene

C(double)C

alkyne

C(triple)C

alcohol

O-H

ether

O-R

aldehyde

O(double)C-H

ketone

O(double)C

carboxylic acid

O(double)C-O-H

ester

O(double)C-O

amine

H-N-H

amide

O(double)C-N-H-R

aryl/aromatic ring/arene

ring with three C(double)C

solute

what dissolves

solvent

what its dissolved in

molecular acids that ionize

HCl, HBr, HI, HF, HNO3, H2SO4

strong common acids

HClO4, H2SO4, HI, HBr, HCl, HNO3

weak common acids

H3PO4, HF, HNO2, HCOOH, CH3CO2H

strong common bases

Group 1 and 2 cations, NaOH, KOH, BaOH2, LiOH

weak common bases

NH3, RNH2

gas evolution reactions: direct

sulfides (H2S), ammonium (NH3-intermediate product: NH4OH)

gas evolutions reaction: indirect

carbonates and bicarbonates (CO2-intermediate product: H2CO3), sulfites and bisulfites (SO2-intermediate product: H2SO3)

oxidation rules for compounds

group 1 element: +1, group 2 elements: 2+, halogens: -1, H: +1 with nonmetals, -1 with metals; O:-2 or -1

oxidation rules for elements

free element with no EN: 0, monatomic ion: charge of ion

1 calorie

4.184 joules

1000 calorie

1 Calorie