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Chemistry > Conversions/Equation > Flashcards

Conversions/Equation Flashcards

1
Q

Converting Celsius to Kelvins

A

273 + Celsius = K

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2
Q

Converting Kelvin to Celsius

A

K - 273 = C

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3
Q

Converting to different units

A

King Henry Died By drinking chocolate milk
K H D B d c m

B= grams, meters, liters
B is the base
ex) 1056 cm -> ? m
You start at c and then you need to go to B in order to do this you move the decimal point to the left 2 places...
meaning 1056cm = 10.56 m
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4
Q

Percent Error

A

Experiement value - accepted value
—————————————————— x 100
accepted value

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5
Q

Determine rounding when dividing or multiplying numbers

A 
LEAST SIG FIGS
ex) 0.00000016/ 74.3
             ^2               ^3
Answer must be in 2 sig figs
= 2.2 x 10^-9
(10 doesn't count)
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6
Q

Determining rounding when adding or subtracting

A

LEAST Decimal Places
ex) 17 - 3.88
^0 ^2

Answer must have ZERO decimal places
=13

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7
Q

1 mol = ________ molecules

AVOGRADOS NUMBER

A

6.02 x 10^23 molecules

lets convert from grams to atomic mass

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8
Q

Grams

A

AMU x Mol

atomic mass

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9
Q

AMU

A

g/mol

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10
Q

cation

A

pos charge

SMALLEST IONIC RADIUS

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11
Q

anion

A

neg charge (ion)

LARGEST IONIC RADIUS

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12
Q

Atomic Mass

A

(% x mass) + (% x mass) + ….
note: % should be in decimals
use when given multiple amu and dif percents

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13
Q

% composition

A

use atmoic mass formula but replace % with x

ex) atomic mass (63.546) = ( y x mass [62.9296]) + ( {1 - x} x mass [64.9278])

to find 2nd % composition must subtract original answer by 1
ex) 1-0.6915

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14
Q

Empirical Formula Steps

A

1) change % to grams (same value)
2) convert grams to mols with molar mass
3) divide by smallest number of mols
4) multiply the values found to get a whole #
- 0.5 x 2
- 0.33 and 0.66 x 3
- 0.25 and .75 x 4

ex) Cr1O1.5 -> Cr2O3

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15
Q

Molecular Formula Steps

A

1) Find Empirical Formula
2) Change % to grams
3) grams to mols (note molar mass is atomic mass)
4) divide by smallest # of moles
5) Write empirical formula
6) Find molar mass of empirical formula
7) divide molecular formula molar mass by empirical formula molar mass
8) multiple whole # found above to the subscript of empirical formula

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16
Q

Charges where found in periodic table

A

Skipping transition metals left to right

+1, +2, +3, +4, -3, -2, -1, 0

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17
Q

Balancing ionic compounds with transition metal NAMING

A

-name of transition metal
- roman numeral (charge)
ex Iron [III] = Fe 3+
-nonmetal ending in ide

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18
Q

Ammonium

A

NH4+

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19
Q

Cyandide

A

CN-

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20
Q

Hydroxide

A

OH-

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21
Q

Acetate

A

C2H3O2-

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22
Q

Perchlorate

A

ClO4-

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23
Q

Chlorite

A

ClO2-

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24
Q

Chlorate

A

ClO3-

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25
Q

ate and ite rule

A

-ate always has 1 more oxygen than -ite

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26
Q

Hypochlorite

A

ClO-

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27
Q

Nitrate

A

NO3-

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28
Q

Nitrite

A

NO2-

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29
Q

Carbonate

30
Q

Chromate

31
Q

Sulfate

32
Q

Sulfite

33
Q

Phosphate

34
Q

Phosphite

35
Q

Bromate

36
Q

Iodate

37
Q

Dichromate

38
Q

Covalent Prefixes

1, 2, 3, 4, 5

A 
1 mono
2 Di
3 Tri
4 Trenta
5 Penta
39
Q

Covalent Prefixes

6,7,8,9,10

A 
6 Hexa
7 Hepta
8 Octa
9 Nona
10 Deca
40
Q

Combustion Reaction

A

CxHy + O2 –> CO2 + H2O

41
Q

Actual yield

A

givens in problem (actual)

42
Q

Theoretical yield

A

whatever our limiting reactant produces

must use conversions to get from one element to another

43
Q

Percent Yield

A

actual yield
————————– x100
theoretical yield

44
Q

Molarity

A

liters of solution

45
Q

1 L = ____mL

46
Q

1kg = ____g

47
Q

Gas Law given pressure and volume

A

P1V1 = P2V2

48
Q

Gas Law given volume and temp

A

TEMP MUST BE IN KELVIN

V1/T1 = V2/T2

49
Q

Gas law given pressure volume and temp

A

KELVINS

P1V1/T1 = P2V2/T2

50
Q

Gas Law given pressure and temp

A

KELVIN

P1/T1 = P2/T2

51
Q

Gas law given volume and mols

A

V1/n1 = V2/n2

52
Q

Ideal Gas Law (no 2nd values)

A

PV =nRT

R= 0.0821

53
Q

Calorimetry

A

q= mC△T

q=heat kJ or J
m= mass in g
Cs = specific heat capaticity J/g°C
△T= change in temp CELCIUS
FINAL - INTIAL
54
Q

Exceptions to Octet Rule

A

-groups that do not have 4 electrons (always incomplete)
ex B and Be
-an expanded octet has 8+ electrons on central atom 3RD ROW AND BELOW

55
Q

Formal Charge

A

FC= valence E - (Bonding electrons (touching) + Individual lone pair)
CENTRAL ATOM MUST = ZERO FOR LEWIS DIAGRAM TO BE CORRECT

56
Q

S

A

1 orbital, 2 electrons

57
Q

P

A

3 oribitals, 6 electrons

58
Q

d

A

5 orbitals, 10 electrons (5 x 2)

needs to be in 5-10 range to be stable

59
Q

f

A

7 orbitals, 14 electrons

60
Q

electron configuaration exceptions s,p,d,f

A

Cr : [Ar] 4s1 3d5
Cu : [Ar] 4s1 3d10

because d wants to be full/half full
so we take 1 from 4s to fulfill

61
Q

Atmoic Radius increases

A

leftward, downward

62
Q

Ionization energy increases

A

rightward, upward

63
Q

ionization energy exceptions

A

2a and 3a (2a larger)

5a and 6a (5a IE bigger)

64
Q

pH

65
Q

pH and pOH equation

A

pH + pOH = 14

66
Q

OH-

A

10^-pOH

units in molarity

67
Q

H+

68
Q

H and OH equation

A

[H+] x [OH-] = 1 x 10^-14

69
Q

pOH

70
Q

propane

71
Q

Methane

Chemistry (4 decks)

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