Chemistry Exam

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Ionic

Back 1

Held together by electrostatic attraction
1 cation and 1 anion

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covalent

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held together by sharing of electrons

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empirical formula

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simplest whole # ratios for atoms in a compound

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molecular formula:

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represents the # and type of atoms in a molecule, provides little structural information

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acetate

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C2H3O2-

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carbonate

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Co3-2

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hydrogen carbonate

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HCO3-1

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Hydroxide

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OH-

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Nitrate

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NO3-

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Nitrite

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NO2-

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Chromate

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CrO4-2

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Dichromate

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Cr2O7-2

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Phosphate

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PO4-3

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Hydrogen Phosphate

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HPO4-2

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Ammonium

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NH4+

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Hydrogen Sulfite

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HSO3-

Front 17

Hydrogen Sulfate

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HSO4-

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Peroxide

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O2-2

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Hypochlorite

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ClO-

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Chlorite

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ClO2-

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Chlorate

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ClO3-

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Perchlorate

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ClO4-

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Permanganate

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MnO4-

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Sulfate

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SO4-2

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Sulfite

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SO3-2

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Cyanide

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CN-

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electronegativity

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

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Mole

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# atoms present in exactly 12 g of C12

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% Comp

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Fraction of the total mass of a given compound that is made due to a single element

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Chemical Reaction Evidence:

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1) color change
2) formation of a solid
3) emission of light
4) emission of heat

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Homogenous

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completely dissolved

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Heterogenous

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not entirely dissolved

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Electrolytes

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compounds whose solutions conduct electricity

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Always Soluble:

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Li+, Na+, K+, NH4+, NO3-, C2H3O2-

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Soluble unless paired with Ag+, Hg2+2, Pb+2

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Cl-, Br-, I-

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SO4-2 always soluble unless paired with

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Sr+2, Ba+2, Pb+2, Ca+2

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OH- always insoluble unless paired with

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Li+, Na+, K+, NH4+

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S-2 always insoluble unless paired with:

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Li+, Na+, K+, NH4+, Ca+2, Sr+2, Ba+2

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Co3-2, PO4-3 always insoluble unless paired withL

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Li+, K+, Na+, NH4+

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Spectator Ions:

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Do not undergo a change in a chemical reaction

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Acid:

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substance that causes an increase in H+ concentration

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Base

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Substance that causes an increase in OH- concentration

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Strong Acids:

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HCl, HBr, HI, HNO3, HClO4, H2SO4, LiOH, NaOH, KOH

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Weak Acids:

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CH3COOH

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Strong Bases:

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Alkaline Metals (ex. NaOH)

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Diatomic Molecules:

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H2, O2, N2, F2, Br2, I2

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Oxidation:

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Process of losing an electron