CH 101 piece of shit class

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

resonance structure

same sequence, diff bond and lone pair placement

best resonance structures have:

full octets

minimized formal charge diffs

formal charges add up to total chg

- formal charge is on most EN atom

e delocalization throughout = stability

more res structure = more stabile

valence bond theory

predicts overlap of valence electrons

VSEPR - valence shell electron pair repulsion

explain discrepancies in bond angles and geo hybridsixzation, how e config

sp² hybrid orbital :

1s+2p=sp²

1 p left unbonded

surround unhybrid p in center

33%s, 66% p

sp hybrid orbital

s+p=sp

2 unhybridized p orbital

sp³ hybrid orbital

25% s 75% p

s+3p=sp³

AX4 = 4 atom bond, tetra

AX3E, 3 atom, tri py

AX2E2, 2 atom, bent

AXE3, 1 atom, lin

morphine mocks what

endorphins (shape received by receptors)

octet exceptions

odd elec/free radical

incomplete octet

expanded octet

odd elec: ex Cl, NO2, NO

incomplete: B and Al 6/8, H 2/8, Be 4/8

expanded: elements in period 3+ ( low lying d orb accomadates extra electrons)

spdf are wave functions, so

new waves =

absence of waves =

new = bonding molc orb

absence = nodes/anti molc orb

rotation : pi and sigma

pi restricted (double bond rotation breaks pi orb interaction), sigma free (internuc axis)

isomers

const:

stereo:

same molc form, diff struct form

const: same molc form, diff sequence

stereo: same molc form, seq, diff spatial arc

• cis - same side of double bond

• trans - opposite sides

perturbation theory

complex system = simple system that is sl;ighty altered

greater orbital overlap =

lower e, stronger bond , typically hybrid

more likely to be hybridized

central and interior (more bonds formed)

MO theory “trial function”

best possible orbital = lowest energy orbital (more stable)

bonding orbital has intrinsic ….

electron density

diatomic homonucelar mo diagram

diatomic homonuclear mo diagram

diatoimic hetero nuclear mo diagram

diatomic hetero nuclear mo diagram

NH₄⁺

ammonium

CN^-

cyanide

CH₃CO₂^-

acetate

CO3²^-

carbonate

HCO₃^-

hydrocarbonate/bicarbonate

NO₂^-

nitrite

NO₃^-

nitrate

PO₄^3-

phosphate

HPO₄^2-

hydrogen phosphate

H₂PO₄^-

dihydrogen phosphate

OH_-

hydroxide

SO₃^2-

sulfite

SO₄^2-

sulfate

HSO₄^-

hydrogen sulfate/bisulfate

ClO_-

hypochlorite

ClO₂^-

chlorite

ClO₃^-

chlorate

ClO₄^-

perchlorate

Cr₄O^2-

chromate

Cr₂O₇^2-

dichromate

MnO₄^-

permanganate

methane

CH₄

ethane

C₂H₆

propane

C₃H₈

butane

C₄H₁₀

salient chem prop is

tendency to undergo oxidation/lose e

tendency to undergo reduction/gain e

potential energy is attrib to ?

low = ?

high = ?

sys pos, comp, state

low = stable

high = unstable

only predictible trans metals

Zn

Ag

Cd

Zn²⁺

Ag⁺

Cd²⁺

ex. [cation] (x) [anion]

higher x =

lower x =

higher x: -ic

lower x: -ous

S^2-, Br^- , PO₄^3-are always charged liek this

S^2-, Br^- , PO₄^3-are always charged liek this

nomenclature of main group ionic comps

[cation] [anion]-ide (no prefixes)

nomenclature of binary ionic comp

[cation] ([cation charge]) [anion]-ide

(find cation charge by cx+d*([anion charge])=0)

nomenclature for poly atomics: oxoanions

exclusions

XO₄^n- per…ate

XO₃^n- …ate

XO₂^n- …ite

XO^n- hypo…ite

exc: Cr As P S

XO₄^n- …ate

XO₃^n- …ite

acid nomenclature (anion endings)

ate → ic

ite → ous

ide → hydro…ic

acid nomenclature

HnXO4 per…ic acid

HnXO₃ …ic acid

HnXO₂ …ous acid

HXO hypo…ous acid

HX hydro…ic acid

Hydrate nomenclature

[[ionic name]] [# prefix]-hydrate

hydrate prefixes (#)

1 mon

2 di

3 tri

4 tetr

5 pent

6 hex

7 hepta

8 oct

9 non

10 dec

molecular comp nomenclature rules

element with lower group # is always listed 1st

same group - higher period # listed 1st

[lower group #] (prefix)[higher group#]-ide

mol to atom

multiply by avogardro

atom to mol

divide by avogadro

organic compounds are made of CHNOPS

key element?

simplest form?

compose common what?

carbon ( can form 4 bonds)

hydrocarbons

fuels

common hydrocarbons

methane CH (natural gas)

propane C3H8 (LP gas/grills gas)

n-butane C4H10 (lighter fuel)

n-pentane C5H12 (gasoline)

ethene C2H4 (fruit ripening agent)

ethlyne C2H2 (fuel for wielding sm sm)

n= straight chain

degenerate orbitals

orbitals of same n value

hydrogen energy state depends solely on

n value

multielectron atoms

energy levels split into subshells with own energy

as n inc, some sublevels overlap as energy levels come closer together

aufbaus

fill lowest energy orbital first

hunds rule

electrons must be added singly, and all singly/unpaired orbitals are same spin to maximize spin

pauli exclusion

orbital can have a max of 2 e with opposite spins +/-

Z (at num) guides # of electron being addes

f and d are diff by what numbers

f = row # - 2

d = row # - 1

steps to find config

write row #

write letter of corres. subshell

count across until filled

trans metal exceptions for stability

Cr & Mo:

Cu & Ag & Au:

Pd:

how?

Cr & Mo: ns¹(n-1)d⁵ (partially filled)

Cu & Ag & Au: ns¹(n-1)d¹⁰ (completely filled)

Pd: (n-2)d¹⁰(completely filled)

They steal the nearest electrons (lowest level)

cation monatomic

pos charge, e deficient

typically metal

subtract 1 electron from valence shell per positive charge

anion monatomic

neg charge, e gain

typically nm

add 1 electron to valence shell per negative charge

special case of transition metal cations

comp form involve e of highest energy

after Z=20 energy of 4s orbital exceeds energy of 3d, e in s orb is more likely to change than d

innner/core electrons are represented by what

nearest noble gas

complete trans series d¹⁰ and f¹⁴

outer electrons are rep by

highest n values in atom

furthest from nuc

valence electrons are rep by

bonding

main group group #

periodic law (mendeleeve and meyer)

properties recur periodically if organized by mass number

mendeleeve accounted for blank spaces

alkali traits

loiw melting point

high molar vol

+1 state

moseley x ray spectra

inner ejected, outer drop down to fill

energies depend on nuc charge and xray freq = v

v=A(Z-b)²

periodic patterns

metallic left and down

radius left and down

IE, EA, and EN right and up

if sheild is constant,

z inc, and z_eff inc

ionization energy exclusions

IE_Al<IE_Mg

IE_P>IE_S

newtons second law

force = m(kg) * a (m/s²)

1 newton =

1 kg m/s²

density

mass/volume

volume

mass/density

F to C

(F-32)/1.8

C to K

C + 273.15

percent mass

mass/comp mass

work

force*distance (in J)