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chem > chapter 3/4 review > Flashcards

chapter 3/4 review Flashcards

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1
Q

chemical equilibruim

A

reached when a chemical reaction reaches a state where the reactants and products stop undergoing any change
the chemical reaction is still going on, but without any change

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2
Q

all chemical reactions try to

A

reach equilibrium

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3
Q

solutions

A

homogeneous mixtures involving solvent (does the dissolving) and solute (thing that is dissolved)

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4
Q

when an ionic compound goes into an aqueous solution…

A

it is hydrated and breaks up into individual ions

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5
Q

electrolytes

A

ionic solutions that are good conductors of electricity

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6
Q

strong electrolytes

A

soluble and dissolve

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7
Q

weak electrolytes

A

insoluble and don’t really dissolve

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8
Q

non electrolytes

A

solutions of molecular/covalent compounds and do not conduct electricity

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9
Q

does insoluble mean that you will never dissolve

A

no, it creates a solid (precipitate)

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10
Q

salts containing _________ are soluble (no exceptions)

A

Na+, NH4+, NO3-, ClO3-, ClO4-. CH3CO2-

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11
Q

almost all salts of ____ are soluble EXCEPT WITH

A

Cl-, Br-, I- (aq)
Ag+, Hg2 2+, Pb 2+ (exceptions=insoluble)

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12
Q

almost all salts containing __ are soluble (aq)

A

F- (aq)
exceptions= Mg2+, Ca2+, Sr2+. Ba2+, Pb2+

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13
Q

almost all salts containing SO4 2- are soluble except with

A

exceptions= Ca2+, Sr2+, Ba2+, Pb2+, Ag+

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14
Q

most salts with _______ are INSOLUBLE except with

A

CO3 2-, PO4 3-, C2O4 2-, CrO4 2-, S2-
exceptions (aq)= NH4+, group 1 metals, BaS

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15
Q

most metal hydroxides and oxides are insoluble except with

A

exceptions (aq)= group 1 hydroxides, Ba(OH)2 and Sr(OH)2

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16
Q

precipitation reaction (double displacement)

A

the cation and anion pairs swap to make new ionic compounds
the insoluble compound precipitates out (s)

17
Q

Arrhenius def of an acid and base

A

acid= a substance that when dissolved in water produces H+
base= a substance that when dissolved in water produces OH-

18
Q

bronsted-lowry definition of an acid and a base

A

acids= H+ donor
base- H+ acceptor

19
Q

strong acids

A

HCl, HI, HBr, H2SO4, HClO3, HClO4, HNO3

20
Q

weak acids

A

carboxylic acids (-COOH) and oxyacid’s NOT on the strong list

21
Q

strong base pneumonic

A

Larry Never Kicked Can Straight Beautifully

22
Q

strong bases

A

LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

23
Q

weak bases

A

any bases not on the strong list and often include an NH bond

24
Q

strong base and strong acid=

A

strong electrolyte

25
Q

weak base and a weak acid=

A

weak electrolyte

26
Q

acid-base reactions (neutralization reactions)

A

Acid + Base —> H2O + Salt

27
Q

redox reactions

A

involve atoms that change their oxidation states

28
Q

oxidation rule 1

A

atoms in their elemental form have oxidation state of zero

29
Q

oxidation rule 2

A

a monoatomic ion has the same oxidation as its charge

30
Q

oxidation rule 3

A

fluorine has a -1 oxidation state

31
Q

oxidation rule 4

A

oxygen has a -2 oxidation state (except for H2O2 which has a -1 oxidation state)

32
Q

oxidation rule 5

A

hydrogen has a +1 oxidation state

33
Q

oxidation rule 6

A

halogens other than fluorine have a -1 oxidation state

34
Q

reduction

A

is GAINING an electron
it is the oxidizing agent

35
Q

oxidation

A

is LOSING an electron
is the reducing agent

36
Q

combustion reactions are usually

A

redox reactions

37
Q

percent yeild

A

actual (g)/ theoretical (g) times 100

38
Q

concentration/ molarity (M)

A

mole of solute/ liters of solution

39
Q

dilution eq

A

M1V1 = M2V2

chem (14 decks)

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