DAT General Chemistry

Hydroxide

OH^-

Nitrate

NO₃^-

Carbonate

CO₃^2-

Sulfate

SO₄^2-

Phosphate

PO₄^3-

Ammonium

NH₄⁺

Methane

CH₄

Ammonia

NH₃

Hydrogen Peroxide

H₂O₂

accuracy

closeness of data value to literature value

precision

consistency of all data values

log 2

0.3

log 3

0.48

1 Liter = ? mL and ? cm³

1000 mL and 1000 cm³

t (K) =

t (C) + 273.15 (K)

Pressure: 1 atm = ? torr / mmHg, ? kPa, and ? bar

760 torr / mmHg, 101.3 kPa, and 1.013 bar

Standard Temp and Pressure (STP)

1 bar and 0 C or 273.15 K

Boiling Point of water

100 C

Freezing Point of water

0 C

Amount of substance

mole (mol)

thermodynamic temperature

kelvin (K)

mass

kilogram (kg)

length

meter (m)

time

second (s)

giga-

G = 10⁹

mega

M = 10⁶

kilo

k = 10³

hecto

h = 10²

deca

da = 10¹

deci

d = 10^-1

centi

c = 10^-2

milli

m = 10^-3

micro

u = 10^-6

nano

n = 10^-9

Have No Fear Of Ice Cold Beer

Diatomic gases: H2, N2, F2, O2, I2, Cl2, Br2

Metal Properties: (6)

• Malleable and lustrous

• Form basic oxides

• High melting and boiling points

• Lose electrons to form cations

• Good conductors of electricity 

• Solid at room temperature (exception: mercury)

Non-metal Properties: (6)

• Brittle and dull

• Form acidic oxides

• Low melting and boiling points

• Gain electrons to form anions

• Poor conductors of electricity and heat 

• Gas or solid at room temperature (exception: bromine) 

Atomic radius

½ the bond length between identical atoms;

increases to the left and down the periodic table

Effective Nuclear Charge

Z_eff = Z (proton #) - S (# of shielding electrons)

= the amount of positive charge experience by an electron;

increasing to the right and down the periodic table

isoelectronic series

atoms/ions with the same number of electrons but different proton numbers; anions have larger atomic radius, cations have smaller atomic radius

ionization energy/potential

the energy needed to remove an electron from a gaseous, neutral atom… = change in enthalpy (delta H)

increases to the right and up (1st ionization energy)

• 2nd ionization energy: after 1st electron is removed, the 2nd ionization is harder and higher energy; easier for 1st group and smaller elements than group 2, but still a high energy;

• alkaline earth metals have a higher than usual 1st ionization energy because of p orbital valence electrons;

• group 15 higher energy than group 16 because of half filled orbitals

• group 2 have higher energy than group 13 because of group 2 filled orbital

electron affinity

the amount of energy released/required when an electron is added to a gas-phase atom

increase to the right and up; becomes more negative

• noble gases have low affinity (they have all of their valence electrons);

• if an element can perfectly half fill their orbital with the electron, it will have a higher affinity than an adjacent element with an already half-filled orbital (group 4 > group 5)

electronegativity

the ability of an atom to attract electrons to itself in a covalent bond

increase to the right and up

• noble gases are negligible