polyatomic ions / ch 2

chem1a ch2

NH₄⁺

Ammonium (cation)

HSO₃⁻

bisulfite (hydrogen sulfite, anion)

HSO₄⁻

bisulfate

HCO₃⁻

Bicarbonate

SO₃²⁻

Sulfite

SO4⁻²

Sulfate

S₂O3²⁻

S2O32-

Thiosulfate

CO₃²⁻

Carbonate

H₂PO₄⁻

dihydrogen phosphate

HPO₄⁻²

monohydrogen phosphate

PO33-

Phosphite

PO₄³⁻

Phosphate

CN⁻

Cyanide

CrO₄²⁻

Chromate

SCN⁻

Thiocyanate

NO₂⁻

Nitrite

NO₃⁻

Nitrate

Cr₂O₇²⁻

Dichromate

HPO₄²⁻

monohydrogen phosphate

ClO⁻

Hypochlorite

ClO₄⁻

Perchlorate

MnO₄⁻

permanginate

OH⁻

hydroxide

C₂H₃O₂⁻

acetate

O₂²⁻

peroxide

C₂O₄²⁻

oxalate

-ate

Larger # of oxygen

-ite

Smaller # of oxygen

per-

LARGEST # of oxy (pur)

bi-

+ Hydrogen and +1 charge

hypo-

Smallest # of oxygen

Anion

Electron gained (- charge)

Cation

Electron lost (+ charge)

Metals lose or gain electrons?

Lose electrons

Non-metals lose or gain electrons?

Gain electrons

Diatomic molecules

HOFBriNCl

Electron Discovery

JJ Thomson, beam deflected

Nucleus Discovery

Ernest Rutherford, gold foil

Nucleus charge on indv. drops

Robert Millikan, oil drop

Ionic compound properties (think table salt)

high melting + boiling pts, nonconducive in solid form, conducive when molten, crystal-like

ionic compound charge

neutral

metal + non-metal =

ionic bond (electron transfer)

how to find ion's charge?

protons - electrons

calculate atomic mass?

(fractional abundance in nature x mass)

gives an atom its identity?

atomic #

find neutrons?

mass number (A) - protons (Z) = neutrons

molecular compound

2 nonmetals bond

ionic compound

metal + nonmetal bond