Chem Chapter 4

Front 1

electrolyte

Back 1

a substance that, when dissolved in water, results in a solution that can conduct electricity

Front 2

nonelectrolye

Back 2

does not conduct electricity when dissolved in water

Front 3

strong vs weak electrolytes

Back 3

a strong electrolyte is assumed to be 100% dissociated into ions in a solution

Front 4

hydration

Back 4

the process in which an ion is surrounded by water molecules arranged in a specific manner

Front 5

chemical equilibrium

Back 5

a chemical state, in which no net change can be observed

Front 6

precipitation reaction

Back 6

results in the formation of an insoluable product or precipitate

Front 7

solubility

Back 7

the maximum amount of solute that will dissolve in a given quantity of solvent at specific temperature.

Front 8

S/I?

Compounds containing alkali metal ions

(Li+, Na+, K+ Rb+, and the ammonium ion NH4+)

Back 8

Soluble

Front 9

S/I?

Nitrates (NO3-)

bicarbonates (HCO-3)

Chlorates (ClO3-)

Back 9

Soluble

Front 10

S/I?

Sulfates (SO4 ^2-)

Back 10

soluable except Ag+, Ca2+, Sr2+, Ba2+, Hg2+ Pb2+

Front 11

S/I?

Carbonates (CO2-,3

Phosphates (PO-3,5)

Chromates(CrO-2,4)

Sulfides (SO-2,4)

Back 11

insoluable excpet alkali

Front 12

S/I?

Hyrdoxides (OH-)

Back 12

insoluble

Front 13

Molecular formula

Back 13

formulas of compounds written as though all species exist as molecules or whole units. It identifies reagents.

Front 14

ionic equation

Back 14

shows dissolved species as free ions.

Front 15

spectator ions

Back 15

ions that are not invoved in the overall reaction`

Front 16

net ionic equation

Back 16

shows only the species that actually take paet in the reaction

Front 17

procedure for writing ionic and net ionic equations?

Back 17

1.) Write a balanced molecular equation for the reaction using for correct formulas from reactant and product. Check solubility and label percipitate

2.) Write ionic equation for the reaction. The compound that does not appear as the percipitate should be shown as free ions.

3.) Identify and cancel the spectator ions on both sides

4.) Check that the chargers and number of atoms balance in the net ionic equation.

Front 18

Acids

Back 18

-sour taste

-color changes in plant dyes

-will react with metals to produce hydrogen gas

-react with carbonates bicarbonates to produce CO2

Front 19

Bases

Back 19

-have bitter taste

-feel slippery

-Aqueous base solutions conduct electricity

Front 20

acid base reactions

Back 20

proton transfer processes

Front 21

Redox reaction

Back 21

electron transfer reactions

Front 22

half reaction

Back 22

explicitly shows the electrons involved in a redox reaction

Front 23

Oxidation reaction

Back 23

refers to the half reaction that involves the loss of electrons.

Front 24

Reduction reaction

Back 24

is the half reaction in a redox that refers to the gain of electrons which are negative

Front 25

reducing agent

Back 25

guy doing the electron donations

Front 26

oxidizing agent

Back 26

guy accepting electron dontation

Front 27

Oxidation Number or state

Back 27

signifies the number of charges that an atom would have in a molecule or ionic compound if electrons were transferred completely

Front 28

Oxidation number rulez

Back 28

1.) Free elements (uncombined) each atom has an oxidation number of zero

2.) Ions composed of 1 atom, the oxi number is equal to the charge of the ion.

3.) O is usually -2

4.) Hydrogen usually +1 except with metals in binary compounds

5.) Alkalis, +1, A earth +2

6.) Flourine is ALWAYS -1

Front 29

Decomposition reactions

Back 29

the breakdown of a compound into two or more components.

Front 30

Combustion reaction:

Back 30

a reaction in which a substance reacts with oxygen, usually with the release of heat and ligh to produce a flame.

Front 31

concentration of a solution

Back 31

is the amount of solute present in a given amount of solution.

Aka Molarity (M)

molarity = (moles of the solute) / liters of solution

Front 32

classifying for electrolyte

Back 32

Step 1Is it one of the seven strong acids?

Step 2Is it of the form Metal(OH)n? Then it's a strong base.

Step 3Is it of the form Metal(X)n? Then it's a salt.

Step 4Does it's formula start with 'H'? It's probably a weak acid.

Step 5Does it have a nitrogen atom? It may be a weak base.

Step 6None of those? Call it a nonelectrolyte.