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Chemistry > 2 - Atoms, ions and compounds > Flashcards

2 - Atoms, ions and compounds Flashcards

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1
Q

mass within atoms

A

mass of proton = mass of neutron
electron gas negligible mass

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2
Q

charges within atoms

A

electron is negative
proton is positive
neutrons has no charge

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3
Q

atoms

A

protons = electrons
most neutrons = protons

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4
Q

identity of an element

A

different elements have atoms with the different number of neutrons

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5
Q

what does the atomic number show

A

number of neutrons in an atoms
-> as well as electron

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6
Q

isotopes

A

atoms of the same element with different numbers of protons and therefore different atomic masses
- most elements are made of a mixture of isotopes

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7
Q

isotopes and chemical reactions

A
  • different isotopes of the same element have the same number of e-
  • the number of neutrons have no effect on the reactions of that element
  • so different isotopes of the same element react in the same way chemically
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8
Q

ions

A

a charged atom, where the number of e- is different to neutron number

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9
Q

what is the atomic mass unit u

A

the standard mass for atomic mass is 1 u, the mass of 1/12 th of the mass of a carbon atom
- approximately the mass of a proton or electron

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10
Q

relative atomic mass

A

the weighted mean mass of an atom of an element relative to 1/12th of the mass of carbon-12

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11
Q

relative atomic mass equation

A

sum (isotopes mass x relative abundance)/ total abundance

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12
Q

copper ions

A

CU+
Cu2+

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13
Q

Iron ions

A

Fe 2+
Fe 3+

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14
Q

binary compounds

A

contains only two elements

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15
Q

ammonium

A

NH4 +

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16
Q

Hydroxide

A

OH-

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17
Q

Nitrate

A

NO3 -

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18
Q

Nitrite

A

NO2 -

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19
Q

Hydrogencarbonate

A

HCO3 -

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20
Q

Manganate (VII)

A

MnO4 -

21
Q

carbonate

A

CO3 2-

22
Q

sulfate

A

SO4 2-

23
Q

sulfite

A

SO3 2-

24
Q

dichromate (VI)

A

Cr2O7 2-

25
Q

phosphate

A

PO4 3-

26
Q

amount of substance -n

A

the number of particles in a substance

27
Q

how many particles does one mole of a substance contain

A

avogadro constant 6.02 x 10 ^23

28
Q

mass of one mole of any atom is

A

relative atomic mass

29
Q

equation linking mass mr and moles

A

n=mass/mr

30
Q

molecular formula

A

is the number of atoms of each element in a molecule

31
Q

empirical formula

A

simplest whole number ratrio of atoms of each element in a compound

32
Q

relative molecular mass

A

the weighted mean mass of a molecule of a compound compared with 1/12 th of the mass of an atom of carbon-12

33
Q

relative formula mass

A

the weighted mean mass of the formula unit of a compound compared with 1/12 th of the mass of an atom of carbon-12

34
Q

two assumptions when finding out the formula of a hydrated salts through experiment

A

1) all the water has been lost
2) no further decomposition

35
Q

1dm ^3 =

A

1000 cm3 = 1000ml = 1litre

36
Q

moles = of solution

A

c x V

37
Q

standard solution

A

a solution of a known concentration

38
Q

molar gas volume

A

volume per mole of gas molecules at stated temp and pressure

39
Q

what is RTP

A

20 ‘c and 101kPa

40
Q

at RTP 1 mole of gas has

A

volume 24 dm^3

41
Q

mole of a gas

A

volume / molar gas volume Vm
must be of same units
if V = dm3 than Vm is 24
if V is cm3 than Vm is 24000

42
Q

ideal gas equation and units

A

pV=nRT

p= Pa (kPa -> Pa x10^3)
V= m^3 (cm3 -> m3 x10^-6) or (dm3 -> m3 x10^-3)
T= K (‘C -> K +273)

43
Q

theoretical yield
why is this not always possible

A

maximum possible amount of product
- reaction may not have gone to completion
- other reactions may have taken place (side reactions)
- purification of the product may result in los of the product

44
Q

percentage yield

A

=actual yield / theoretical yield x 100

45
Q

limiting reagent

A

the reactant that is not in excess
it is completely used up

46
Q

atom economy

A
  • how well the atoms have been utilised
    = (sum of molar mass of desired products)/sum of molar mass of all products x 100
47
Q

reactions with high atom economies

A
  • produce a large proportion of desired products and few unwanted waste products
    -make best use of natural resources
48
Q

why is atom economy not always the best way to see if a reaction is sustainable

A
  • may use reactants that are sourced wrongly
  • other reactions can have a poor percentage yield but high atom economy

Chemistry (30 decks)

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