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chemistry 141 > Exam 2 Cards (Aqueous solutions, Strong/Weak Electrolytes, Enthalpy..) > Flashcards

Exam 2 Cards (Aqueous solutions, Strong/Weak Electrolytes, Enthalpy..) Flashcards

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1
Q

NH4+

A

Ammonium

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2
Q

Charge on Ag

A

Ag+

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3
Q

Carbonate

A

CO3(2-)

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4
Q

Phosphate

A

PO4(3-)

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5
Q

Phosphoric acid

A

H3PO4

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6
Q

Oxidation Rule 1: Sum of oxidation numbers for a neutral compound?

A

The sum of oxidation numbers for a neutral is ZERO

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7
Q

Oxidation Rule 2: Sum of oxidation numbers for a polyatomic ion?

A

The sum will be the same as the charge of the polyatomic ion

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8
Q

Oxidation Number of an atom in its elemental state

A

0

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9
Q

Oxidation Number of a monatomic ion

A

same as the charge on the ion

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10
Q

Oxidation Number of F

A

ALWAYS -1

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11
Q

Oxidation Number of Group 1A?

A

Always +1

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12
Q

Oxidation Number of Group 2A

A

Always +2

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13
Q

Oxidation Number of Aluminum

A

Always +3

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14
Q

Oxidation Number of Hydrogen

A

if in a compound with NONMETALS: +1

if in a compound with METALS: -1

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15
Q

Oxidation Number of Oxygen

A

Usually -2

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16
Q

Units of ΔHfO

A

kJ/mol

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17
Q

Determination of ΔH from ΔHfO values

A

Summation of (a)(ΔHfO) [products] - Summation of (b)ΔHfO[reactants]

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18
Q

micro

A

10^-6

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19
Q

pico

A

10^-12

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20
Q

oxidation numbers of: Cl, Br,I

A

usually -1

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21
Q

cal

A

calorie: 1 cal = 4.184 J exactly

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22
Q

milli

A

10^-3

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23
Q

centi-

A

10^-2

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24
Q

deci-

A

10^-1

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25
Q

giga

A

10^9

26
Q

mega

A

10^6

27
Q

kilo

A

10^3

28
Q

Polyatomic molecules

A

P4, S8

29
Q

ΔH is dependent on these 4 properties

A
  1. temp 2. pressure 3. concentration 4. physical state of matter
30
Q

Diatomic molecules

A

Br2, Cl2, F2, O2, N2, I2, H2

31
Q

nano

A

10^-9

32
Q

C to K

A

C + 273= K

33
Q

Hess’ Law

A

rearrange the given equations to match the desired equation- be sure to manipulate the ΔH as necessary

34
Q

kcal

A

kilocalorie 1kcal= 1000 cal, 1 CAL = 1 food calorie

35
Q

standard enthalpy of formation

A

1 MOL ΔH = ΔHfO

36
Q

q

A

heat

37
Q

if q

A

exothermic (energy is being released)

38
Q

if q>0

A

endothermic (energy is being absorbed)

39
Q

Bomb calorimetry

A

qrxn= CcalΔT + cH2OMH2OΔT **THIS IS ENDOTHERMIC

40
Q

kJ

A

1000J

41
Q

Common Strong Bases (4)

A

M*OH (M = metal group 1A)
Ca(OH)2
Sr(OH)2
Ba(OH)2

42
Q

Hydrogen Displacement reaction

A

M + HX–> MX + H2 (g)
M> H2 on activity scale for a reaction
M= cation
X= anion

43
Q

Metal Hydroxide Bases (Acid-Base neutralization Reactions)

A

acid + base–> salt + H2O

salt formation: the cation is from the base and the anion is from the acid

44
Q

Metathesis Reactions Rule

A

AB + CD–> AD + CB

A & C = cations
B & D= anions

45
Q

Common weak acids

A

if not listed as strong, then weak

46
Q

common weak bases

A

NH3

47
Q

Salts

A

any compound where the anion is NOT OH-

48
Q

Common Strong Acids

A 
HCl
HBr
HI
HNO3
H2SO4
HClO4
49
Q

Precipitate Reactions

A

AB + CD–> AD + CB
A/C= cations
B/D= anions
either AD or CB MUST be insoluble for a reaction to occur

50
Q

c

A

specific heat (J/gxC)

51
Q

NH3 as a weak base in acid-base neutralization

A

acid + NH3–> SaltNH+
the cation is NH3, the anion come from the acid
the saltNH4+ is ALWAYS soluble

52
Q

Gas formation reaction

A

metal carbonate + acid –> salt + CO2 (g) + H2O (l)
salt formation: anion from acid, cation from carbonate

metal carbonate M(CO3(2-))

53
Q

metal displacement reaction

A

M + M’X –> M’ + MX
X= anion (goes unchanged)
M’= cation
M>M’ on activity series for a reaction to occur

54
Q

C

A

heat capacity

C= cm

55
Q

Dilution of a solution

A

M1V1= M2V2

56
Q

M (molarity)

A

mol/L

57
Q

Calorimetry equation

A

q= cmΔT or q= CΔT

58
Q

% yield equation

A

experimental/theoretical x 100

59
Q

ΔHO–> ΔHOf

A

elements –> 1 MOL substance

60
Q

ΔT

A

temperature change (Tfinal-Tinitial)

chemistry 141 (5 decks)

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