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Chemistry 12 > UDM chemistry Placement > Flashcards

UDM chemistry Placement Flashcards

1
Q

base SI unit for length

A

Meteres

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2
Q

base SI unit for mass

A

KG

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3
Q

base SI unit for time

A

s

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4
Q

base SI unit for electric current

A

amperes

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5
Q

base SI unit for temperature

A

kelvin

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6
Q

base SI unit for amount of substance

A

mole

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7
Q

base SI unit for luminous intensity

A

candela

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8
Q

kelvin to celsius equation

A

Tk= Tc +273.15

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9
Q

tera-

A

symbol: T
size: 10^12

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10
Q

giga-

A

symbol: G
size: 10^9

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11
Q

mega

A

symbol: M
size: 10^6

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12
Q

kilo

A

symbol: K
size: 10^3

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13
Q

deci

A

symbol: d
size: 10^-1`

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14
Q

centi-

A

symbol: c
size: 10^-2

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15
Q

milli

A

symbol: 10^-3
size: m

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16
Q

micro

A

symbol: mu
size: 10^-6

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17
Q

nano

A

symbol: n
size: 10^-9

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18
Q

pico

A

symbol: p
size: 10^-12

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19
Q

femto

A

symbol: f
size: 10^-15

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20
Q

element

A

pure substance that can’t be separated

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21
Q

compound

A

pure substance that can be separated

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22
Q

isotope

A

different # of neutrons

Mass #
element

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23
Q

mass #

A

protons + neutrons

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24
Q

periodic trends

A

go do the grade 11 flashcards

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25
Q

ionic bond

A

1.8 and above en difference means that there is an exchange of electrons and a crystal lattice is created. held together by electrostatic forces [ppp]+ [pppp]-

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26
Q

polar covalent bond

A

0,4-1.8 there is unequal sharing of e- H-O-H

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27
Q

non polar covalent bond

A

equal sharing 0-0.4

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28
Q

1 mole =

A

6.02 x 10^23 molecules

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29
Q

moles

A

go do some practice in the grade 11 textbook

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30
Q

balancing equations

A

practice some in the grade 11 textbook

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31
Q

chemical reactions

A

do the grade 11 unit 2 brains cape cards

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32
Q

stoichiometry

A

do the grade 11 practice in text

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33
Q

states of matter

A

see imp flashcards in “chemistry”

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34
Q

ideal gas laws

A

do practice in textbook gr 11

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35
Q

solubility and solutions

A

do practice in gr 11 texts and the flashcards in unit 3/4

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36
Q

go review some naming of compounds

A

online and a few flashcards in gr 11

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37
Q

TAKE A VERY IN DEPTH REVIEW OF STOICHIOMETRY AND MOLARITY

A

DO THE GRADE 11 MASS PERCENTAGE PROBLEMS

38
Q

do some mass percentage problems man

39
Q

do some density problems with moles

A

gr 11 text

40
Q

REVIEW ALL GRADE 12 NOTES

41
Q

states of matter of elements

A

noble gases: gas

bromine, mercury: liquid

HOFNCl: gas

Iodine: solid

42
Q

ion charge and solubility

A

more charge is less soluble

43
Q

ion size and solubility

A

more size is more solubility

44
Q

hydrogen ion and solubility

A

nearly everything

45
Q

ammonium ion and solubility

A

nearly everything

46
Q

group 1 ion and solubility

A

nearly everything

47
Q

nitrate ion and solubility

A

nearly everything

48
Q

acetate ion and solubility

A

nearly everything

49
Q

cl ,br and I ion and solubility

A

silver, pb, hg, cu ad thallium group 11 stuff

50
Q

f ion and solubility

A

low with mg, ca, ba and pb (group 2 stuff)

51
Q

percent concentration (m/v) units

A

grams solute / ml solution times 100

52
Q

percent m/m

A

grams solute/ grams TOTAL times 100

53
Q

planck’s quantum theory

A

the amount of a single quantum is this:

delta e= hv
h= 6.6 x 10^-34 js

54
Q

when you are calculating the excited atom’s energy, z is always

A

1 for hydrgen

55
Q

go do some quantum theory practice on brains cape (it is unit 1)

56
Q

m in calorimetry is always in (units)

57
Q

enthalpy of formation is

A

reactants -p

58
Q

bond energy is

59
Q

how to write rate law

A

it is r=k[a}order[b]order etc.

60
Q

when to use integrated rate law

A

when you need to find the concentration after a certain time

61
Q

writing the equilibrium expression (k)

A

first write the products to their coefficients/ reactants to their coefficients and only aq solutions are included

62
Q

do some quantum practice

A

like the numbers

63
Q

practice some hf and some bond energy stuff

64
Q

conjugate acid goes to

A

BASE by loosing an h

65
Q

conjugate base goes to

A

acid by adding an h

66
Q

name the strong acids

A

cl, br, i, h2so4, hno3

67
Q

weak acid

A

ch3cooh, hf

68
Q

how large will a strong acid’s ka be?

69
Q

a weak acid equation

A

weak acid + water – equilibrium– hydronuim and a-

70
Q

strong base

A

group 1 and 2 metal OH

71
Q

weak base equatio

A

B+water–equilibrium–

72
Q

basic ion

A

conjugate base of weak acid

73
Q

acidic ion

A

conjugate acid

74
Q

in any acid base problem

A

start with the chemical eon, then puzzle out an ice table, then write a k

75
Q

oxidation numbers

A

oxygen is –2, except when it is r2o2 (then -1)
hydrogen is =1
all halogens have -1

76
Q

cell potential

A

the half cell with the MORE POSITIVE e red will be reduced (the other will switch signs)

77
Q

how to balance redox

A 
split into half reactions
balance atoms not o and h
balance o by adding water
balance h by adding H+
add electrons to the more +ve side
cancel the electrons
78
Q

high vp means

79
Q

hydrogen bonding

80
Q

plasma

A

noble gases + electricity

81
Q

bose einstein

A

near absolute zero and becomes one “super particle”

82
Q

what is the combined gas law

83
Q

what is the ideal gas law

84
Q

go do the gas laws gr 11 practice cards

A

memorize the laws

85
Q

when given separate gases with pressures and you mix them,

A

the pressures add up

86
Q

what is stp

A

273.15 K (0 °C, 32 °F) and an absolute pressure of exactly 105 Pa (100 kPa, 1 bar).

87
Q

density units

88
Q

quantum number things

A

n= 1,2,3 and is the energy level

l=0-(n-1) and s=0, p=1 etc. and s can have 1 orbital, p can have 3, d can have 5 etc.

ml= -l..l number of orientations
ms= +or -1/2 is spin
89
Q

how do you name a 4 oxygen

90
Q

how to name a 1 oxygen

91
Q

how to name a basic acid

A

hydro-ic acid

92
Q

mass percent is always using

A

molar mass and grams NOT MOLES

Chemistry 12 (6 decks)

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