nomenclature + polyatomics + gas laws formulas

-ate

normal ending

-ite

one less oxygen

per-

one more oxygen

hypo-ite

two less oxygen

acetate ion

CH₃COO^-

chlorate ion

ClO₃^-

Iodate ion

IO₃^-

bromate ion

BrO₃^-

florate ion

FO₃^-

cyanide ion

CN^-

hydroxide ion

OH^-

nitrate ion

NO₃^-

permangatate ion

MnO₄^-

carbonate ion

CO₃^2-

bicarbonate ion

HCO₃^-

peroxide ion

O₂²⁻

sulfate ion

SO₄^2-

phosphate

PO₄^3-

ammonium

NH₄⁺

ammonia

NH₃ (neutral)

arsine

AsH₃ (neutral)

stibine

SbH₃ (neutral)

water

H₂O (neutral)

ozone

O₃ (neutral)

phosphine

PH₃ (neutral)

borane

BH₃ (neutral)

two oxidation states: endings

• -ic = higher oxidation state

• -ous = lower oxidation states

two oxidation states: latin naming Fe2+ and Fe3+

• Fe²⁺ = ferrous

• Fe³⁺ = ferric

two oxidation states: latin naming Sn2+ and Sn4+

• Sn²⁺ = stannous

• Sn⁴⁺ = stannic

two oxidation states: latin naming Cu+ and Cu2+

• Cu⁺ = cuprous

• Cu²⁺ = cupric

two oxidation states: latin naming Au+ and Au3+

• Au⁺ = auros

• Au³⁺ auric

two oxidation states: latin naming Hg+ and Hg2+

• Hg⁺ = mercurous

• Hg²⁺ = mercuric

two oxidation states: latin naming Pb2+ and Pb4+

• Pb²⁺ = plumbous

• Pb⁴⁺ = plumbic

naming polyatomic oxyacids (contain oxygen, hydrogen, and smth else)

• hypo-ite = hypo-ous acid

• -ite = -ous acid

• -ate = -ic acid

• per-ate = per-ic acid

bi-

one hydrogen, reduces charge by +1

molar volume formula

mV = V/n

Density of an ideal gas

D_gas = mm/mV, this ONLY works for gasses

how to convert g/L to g/mL

divide by 1000 since the conversion is happening in the denominator

universal gas constant

R = 8.314 kPaL/Kmol (kilopascal litres/ Kelvin mol)

ideal gas law

R = PV / nT or PV = nRT

use ideal gas law to find molar volume

• PV = nRT

• V = nRT/P

• V/n = RT/P

• since V/n is molar volume, mV = RT / P

use ideal gas law to find density

• D = m/V

• V = m/D

• substitute V = m/D into PV = nRT

• Pm/d = nRT

• Pm = nRTD

• D = Pm/nRT

• since m/n is mm, D = mmP/RT

• since P/RT is mV, this is the same as D = mm/mV

use ideal gas law to find mm

• substitute n = m/mm into PV = nRT

• PV = mRT/mm

• mmPV = mRT

• mm = mRT/PV

boyle’s law

• Volume is inversely proportional to pressure at constant T and n

• P₁V₁ = P₂V₂

charles’ law

• volume is directly proportional to temperature in Kelvin at constant P and n (moles per mass)

• V₁/V₂ = T₁/T₂

Gay-Lussac’s law

• pressure is directly proportional to temperature at constant n/m and Volume 

• P₁/P₂ = T₁/T₂

combined gas law

P₁V₁/T₁ = P₂V₂/T₂ at constant n/m and T in kelvin

Avagadro’s law/hypothesis

• number of moles of gas is directly proportional to volume at constant T and P

• n₁/n₂ = V₁/V₂

Density of a gas

D_gas = mm/mV at specific T and P

Density

D = m/v

use ideal gas law to find density

• D = m/V

• V = m/D

• substitute V = m/D into PV = nRT

• Pm/d = nRT

• Pm = nRTD

• D = Pm/nRT

• since m/n is mm, D = mmP/RT

• since P/RT is mV, this is the same as D = mm/mV

use ideal gas law to find molar volume

• PV = nRT

• V = nRT/P

• V/n = RT/P

• since V/n is molar volume, mV = RT / P

use ideal gas law to find mm

• substitute n = m/mm into PV = nRT

• PV = mRT/mm

• mmPV = mRT

• mm = mRT/PV

standard conditions

• P_STP = 101.3 kPa

• T_STP = 0.00000 degrees C or 273.15 K

• mV_STP = 22.4 L/mol

Standard Ambient Temperature and Pressure

• P_SATP = 100.0 kPa

• T_SATP = 25.00 degrees C = 298.15 kPa

• mV_SATP = 24.8 L/mol

universal gas constant

R = 8.314 kPaL/Kmol

Density of water at STP

1.00 g/mL

conversions of pressure

101.3 kPa = 1.00 atm = 760 mmHg or 760 torr