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1
Q

macro vs micro

A

big vs small

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2
Q

empirical knowledge

A

observation

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3
Q

theoretical knowledge

A

ideas to explain empirical knowledge

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4
Q

atomic theory: greeks

A

matter can be divided into indivisible atoms

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5
Q

atomic theory: democritus

A

atoms vary in size, constant motion, empty space around them

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6
Q

atomic theory: aristotle

A

matter made of earth, air, wind, fire

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7
Q

daltons atomic theory

A
  • matter: indivisible atoms
  • element atoms are identical
  • law of constant proportion
  • law of conservation of mass
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8
Q

atomic theory: jj thompson

A

plum pudding model of electrons

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9
Q

atomic theory: rutherford

A

alpha particles, nucleus, protons

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10
Q

atomic theory: chadwick

A

confirmed neutrons

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11
Q

atomic theory: bohr

A

electrons release light + orbit nucleus, planetary model

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12
Q

radioisotopes: alpha

A

blocked by paper, 2+

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13
Q

radioisotopes decay to emit

A

nuclear radiation + break apart easily

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14
Q

radioisotopes: beta

A

blocked by aluminum, negative charge

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15
Q

radioisotopes: gamma

A

penetrates most, no mass, speed of light

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16
Q

nuclear reaction =

A

change in nucleus (presence of radioisotopes)

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17
Q

metals: majority of

A

known elements

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18
Q

non metals are

A

non conductors, brittle solids (or gases)

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19
Q

metalloids are along the

A

staircase line, properties of metals and non metals

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20
Q

group 1

A

alkali metals

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21
Q

group 2

A

alkaline earth metals

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22
Q

group 17

A

halogens

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23
Q

group 18

A

noble gases

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24
Q

groups 3-13

A

transition metals

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25
Q

who published the first periodic law

A

mendeleev (properties = functions of atomic mass)

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26
Q

atomic radius is the only trend to

A

decrease across a period and increase down a group (other than metallic properties)

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27
Q

define ionization energy

A

energy required to remove an electron

28
Q

define electron affinity

A

energy released in gaining an electron

29
Q

define electronegativity

A

ability to attract electrons

30
Q

who proposed electronegativity

A

pauling

31
Q

ions are held together by

A

electrostatic forces

32
Q

lewis structure vs symbol

A

molecular vs ionic (sharing vs giving e)

33
Q

what if electronegativity is exactly 1.7

A

polar covalent

34
Q

if electronegativity is polar, it’s bc of

A

unequal sharing between dipoles

35
Q

define polarity

A

distribution of electrical charge over bonded atoms

36
Q

geometric molecule =

A

non polar

37
Q

molecule can have polar covalent bonds but be non polar if

A

not symmetrical

38
Q

define intermolecular forces

A

between molecules

39
Q

types of intermolecular forces

A
  • van der waals
  • dipole dipole
  • london dispersion
  • hydrogen bonding
40
Q

hydrogen bonds are stronger than

A

dipole dipole

41
Q

define intramolecular forces

A

within single molecules (ionic or covalent bonds)

42
Q

there are no intermolecular forces in

A

ionic compounds

43
Q

hydrogen bonds: hydrogen must be bonded to

A

N, O, F (highly electronegative)

44
Q

water has unusually

A
  • high melting boiling points
  • low density
  • high surface tension
  • high specific heat capacity
45
Q

evidence of chemical reaction

A
  • colour change
  • energy is released/absorbed (sparks)
  • gas produced
  • precipitate
46
Q

law of conservation of mass

A

reactants mass = products mass

47
Q

catalyst:

A

speeds up a reaction

48
Q

acid + sulfate

A

H2S + salt

49
Q

acid + carbonate

A

water + CO2 + salt

50
Q

acid + sulfite

A

water, SO2, salt

51
Q

metal oxanion —>

A

ionic compound and gas

52
Q

metal carbonate —>

A

metal oxide and carbon dioxide

53
Q

N
A

A

avogadros constant

54
Q

avogadros constant is the number of atoms in

A

12 g of carbon-12

55
Q

why could it not yield 100%

A
  • competing reverse reaction
  • measurements/spills/purifications
  • impurities
  • side reactions
56
Q

air and water are usually

A

excess reagents

57
Q

why is it important to use LR

A
  • saves money and resources
  • environment (less resources)
  • uses undesired
  • improves efficiency
58
Q

transparent gases and liquids are

A

solutions (entities too small to block light)

59
Q

translucent: opaque gases or liquids:

A

heterogenous (entities block light, like blood)

60
Q

ionic compounds dissolve in

A

water

61
Q

like dissolves like:

A

polar and polar, non polar and non polar

62
Q

charles law

A

v/t

gas volume is proportional to its temperature in kelvins

63
Q

boyles law

A

pv

gas volume is inversely proportional to pressure

64
Q

gay lussacs law

A

pt

gas pressure is directly proportional to temperature

65
Q

combined gas law

A

pv/t

product of pressure and volume divided by temperature is constant

chem (7 decks)

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