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auer mod 2.1 mols Flashcards

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1
Q

what is Avogadro’s number (definition)

A

the number of particles/ atoms/ molecules in one mole of any substance

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2
Q

what is Avogadro’s number (number)

A

6.02x10^23

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3
Q

what’s Ar

A

the relative atomic mass of an element “neutron + proton”

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4
Q

what’s Mr

A

the sum of all the Ar’s of all the atoms present in the substance. Its the relative molecular mass

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5
Q

what’s percentage yield

A

the mass or moles of product obtained expressed as a percentage of what should be produced.

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6
Q

what’s atom economy

A

a measure of the proportion of reactants that become useful

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7
Q

what’s percentage yield equation

A

actual yield
_____________ x 100
theoretical yield

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8
Q

what’s atom economy equation

A

mass of desired products
____________________ x 100
total mass of reactants

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9
Q

what are 5 reasons why percentage yield is not normally 100%

A
  1. reactants or products may be left behind in apparatus.
  2. separation and purification may result in loss of some of the product
  3. the reaction may be at equilibrium and not go to completion
  4. The reactions may not be pure
  5. side reactions may occur leading to side products
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10
Q

what numbers from equations are used in atom economy

A

large numbers as well as the small numbers

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11
Q

what is a standard solution

A

a solution of known concentration. It can be prepared by dissolving a known mass of a solid in solvent and making it up to an exact volume.

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12
Q

what is the limiting reactant

A

the reactant that is not in excess

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13
Q

what is pressure proportional to

A

temperature

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14
Q

what is volume proportional to

A

temperature

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15
Q

what is pressure inversely proportional to

A

volume

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16
Q

what is the ideal gas equation…

A

pV=nRT

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17
Q

ideal gas equation: p and what its measured it

A

p=Pressure (Pa)

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18
Q

ideal gas equation: V and measurement

A

V= Volume (m^3)

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19
Q

ideal gas equation: n and measurement

A

n= amount of substance (mol)

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20
Q

ideal gas equation: R and measurement

A

R= ideal gas constant (8.314Jk^-1mol^-1

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21
Q

ideal gas equation: T and measurement

A

T=temperature (K=kelvin)

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22
Q

how do you get from dm^3 to m^3

A

divide by 1000

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23
Q

how do you get from cm^3 to m^3

A

divide by 1000000

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24
Q

how do you get from dm^3 to cm^3

A

multiply by 1000

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25
Q

how do you get from K to C

A

subtract 273

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26
Q

what does the molecular formula tell us

A

the molecular formula tells us the number and type of atoms of each element in a molecule

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27
Q

what does the empirical formula tell us

A

the simplest whole number ratio of atoms in a molecule

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28
Q

the molecular formula for butene is C4H8, what’s the empirical formula

A

CH2

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29
Q

How do you find concentration from mass and volume

A

conc= mass/vol

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30
Q

what does an oxidation reaction involve

A

the loss of electrons

31
Q

what does a redox reaction involve

A

oxidation and reduction occurring at the same time

32
Q

what’s a redox reaction

A

where oxidation and reduction occur simultaneously in a reaction because one species lose electrons which are the donated and gained by another species.

33
Q

if the oxidation number increases, is it reduced or oxidised?

A

oxidised (loss of electrons)

34
Q

formula for hydrochloric acid

A

HCL

35
Q

formula for nitric acid

A

HNO3

36
Q

formula for sulfuric acid

A

H2SO4

37
Q

3 strong bases?

A

lithium hydroxide
sodium hydroxide
potassium hydroxide

38
Q

what does water of crystallisation mean

A

when ionic compounds form, they often have molecules of water stuck in them.

39
Q

formula for ethanoic acid

A

CH3COOH

40
Q

what is an acid

A

a species able to donate protons ( H+ (hydrogen) ions)

41
Q

what is a base

A

a species able to accept protons ( via a lone pair)

42
Q

what are all alkalis

A

bases

43
Q

what are alkalis in terms of bases

A

water soluble bases ( metal hydroxides and NH3)

44
Q

what is a standard solution and what is it used to do

A

a standard solution has a known concentration, its used in a titration to find the concentration of another substance

45
Q

what happens when an acid is added to water ( what does the acid release)

A

the acid releases H+ ions into solution

46
Q

what are the two common bases and what’s another base

A
  • metal oxides
  • metal hydroxides
  • ammonia
47
Q

what happens to alkalis when dissolved in water

A

they release OH- (aq) ions when dissolved in water

48
Q

what are the 3 common alkalis

A

NaOH
KOH
NH3

49
Q

acid+ carbonate??

A

=salt + carbon dioxide +water

50
Q

acid+ metal oxide??

A

=salt+ water

51
Q

acid + alkali??

A

= salt+ water

52
Q

acid + metal??

A

= salt + hydrogen

53
Q

what does hydrated mean

A

the crystalline form containing water

54
Q

what does anhydrous mean

A

the form containing no water

55
Q

reduction=________ in oxidation number?

A

decrease

56
Q

oxidation=________ in oxidation number?

A

increase

57
Q

123FHOC - what do these all mean in terms of oxidation state

A

oxidation sates:

  1. group 1= 1+
  2. group 2= 2+
  3. group 3= 3+
  4. flourine= -1
  5. hydrogen= +1
  6. oxygen= -2
  7. chlorine nearly always=-1 (except when bonded to oxygen)
58
Q

if something is in its elemental state, what’s its oxidation state

A

0

59
Q

what are the 7 solubility rules

A
  1. all salts of group 1 and ammonium are soluble
  2. all salts of nitrates, chlorates and acetates are soluble
  3. all salts of halides are soluble except silver(I),copper(I), lead (II) sulfate and strontium sulfate
  4. All salts of sulphate are soluble except for barium sulfate, lead(II) sulfate, and strontium sulfate
  5. All salts of carbonate, phosphate and sulphite are incsoluble, except those from point 1.
  6. All oxides and hydroxides are insoluble except those from group 1, calcium, strontium and barium
  7. all salts of sulfides are insoluble except those from group 1 and 2** elements and of ammonium.
60
Q

salts are _____, _____ and _____

A

sulfates, chlorides and nitrates

61
Q

what is the definition of relative atomic mass

A

the weighted mean mass of an atom of an element compared with one twelfth of the mass of an atom of carbon-12

62
Q

what id relative isotopic mass

A

the mass of an atom of an isotope compared with one twelfth of the mass of an atom of carbon-12

63
Q

what is a mole

A

the amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope

64
Q

what does the avogadro constant represent

A

the number of atoms per mole of the carbon 12 isotope.

65
Q

what is mass number the same as

A

relative atomic mass

66
Q

what type of reaction has the greatest atom economy

A

addition

67
Q

how do you calculate mols of ions

A

same as how you would calculate mols of atoms (using Avogadro’s constant)

68
Q

state the similarities and differences between the atomic structures of isotopes

A
  • same amount of protons and electrons

- different number of neutrons

69
Q

how could you reduce percentage error when weighing something

A

use a balance weighing more decimal places

70
Q

how do you calculate percentage error

A

uncertainty( +- (you may have to x by 2 eg if weighed twice)/ measurement from apparatus x100

71
Q

EXPLAIN one advantage of a high atom economy

A

more sustainable/ less waste product

72
Q

explain one advantage of a high percentage yield

A

less waste of reactants

73
Q

3 reasons for a need for a high atom economy

A
  • reduces production of unwanted product
  • makes this process more sustainable
  • in this reaction, water is the only unwanted process so green

chem (14 decks)

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