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Chemistry Paper 1 > Key concepts > Flashcards

Key concepts Flashcards

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1
Q

how are ions formed?

A

when atoms gain or lose electrons

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2
Q

what is the plum pudding model?

A

that an atom was positively charged and contained negatively charged electrons

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3
Q

how was the plum pudding model wrong?

A

because alpha particles passed straight through, deflected more than expected or even deflected backwards

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4
Q

what is the nuclear atom?

A

an atom has a positive nucleus surrounded by negative electrons with empty space

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5
Q

what is the bohr model?

A

shows that electrons can only exist in a fixed shell orbit with fixed energy

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6
Q

what charge are protons?

A

positive

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7
Q

what charge are neutrons?

A

neutral

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8
Q

what charge are electrons?

A

negative

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9
Q

what is the mass of a proton?

A

1

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10
Q

what is the mass of a neutron?

A

1

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11
Q

what is the mass of a electron?

A

negligible

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12
Q

what charge does a nucleus have?

A

positive

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13
Q

what does the nucleus contain?

A

protons and neutrons

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14
Q

what charge to atoms have?

A

neutral - no charge

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15
Q

why does an atom have no charge?

A

because they have the same number of protons as electrons

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16
Q

why do ions have a charge?

A

because there isn’t the same number of protons and electrons

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17
Q

what does the atomic number tell you?

A

how many protons an atom has

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18
Q

what does the mass number tell you?

A

the total number of protons and neutrons

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19
Q

which is bigger the mass or atomic number?

A

the mass number

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20
Q

what are isotopes?

A

different forms of elements with the same number of protons and a different number of neutrons

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21
Q

what is the relationship with the atomic and mass number of isotopes?

A

they have the same atomic number but different mass numbers

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22
Q

what is relative atomic mass?

A

the average mass of one atom of the element compared to 1/12 of the mass of one atom of carbon12

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23
Q

what happens if an element has one isotope?

A

it’s relative atomic mass with be the same as its mass number

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24
Q

how to work out relative atomic mass from isotopic abundances

A

multiply each relative isotopic mass but it’s abundance and add up results
divide by the sum of abundances

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25
Q

how did Mendeleev sort the elements originally?

A

through their properties

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26
Q

what did he realise by doing this?

A

by putting the elements in order of atomic mass he could put the elements with similar chemical properties in columns

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27
Q

How did Mendeleev fill in the gaps?

A

used properties of other elements in the columns to predict undiscovered elements properties

28
Q

what do groups show?

A

the number of electrons it has on its outer shell

29
Q

what do periods show?

A

how many full shells an element has

30
Q

how do negative ions form?

A

when atoms gain electrons

31
Q

do negative ions have more or less electrons than protons?

A

more

32
Q

how are positive ions formed?

A

when an atom loses electrons

33
Q

does a positive ion have more or less electrons than protons?

A

less

34
Q

what links electrons and charge?

A

the number of electrons lost or gained is the charge number

35
Q

what are ionic compounds made of?

A

a positively charged part and a negatively charged part

36
Q

what is the overall charge of an ionic compound?

A

zero

37
Q

what does it mean if an ion ends in ‘ate’?

A

they are negative ions containing oxygen and one other element

38
Q

what does it mean if an ion ends in ‘ide’?

A

negative ions containing only one element

39
Q

which ion is an acceptable to the rule when an ion ends in ‘ide’?

A

hydroxide ions as they are OH minus

40
Q

How is an ionic bond formed?

A

when a metal and non metal react together

41
Q

does a metal lose or gain electrons and what does it form?

A

loses electrons to form positive ion

42
Q

does a non metal gain or lose electrons and what does it form?

A

gains electrons to form a negative ion

43
Q

what is the structure of ionic compounds?

A

giant ionic lattice structures

44
Q

properties of ionic compounds

A

strong electrostatic forces
high m and b points
don’t conduct if a solid
dissolve in water

45
Q

why does an ionic compound carry a current when a liquid or gas?

A

because the ions are free to move

46
Q

how are covalent bonds formed?

A

when two non metals share electrons between atoms

47
Q

What substance has covalent bonds?

A

simple molecular substances

48
Q

simple molecular substances properties

A 
very strong covalent bonds 
weak intermolecular forces 
low m and b points 
don’t conduct 
some soluble some aren’t
49
Q

why do simple molecular substances not conduct?

A

because they don’t contain any free electrons

50
Q

what state of matter are molecular substances at room temp?

A

gas or liquid

51
Q

how do melting and boiling points increase?

A

if the molecule gets bigger, the strength of intermolecular forces increase so more energy is needed to break them

52
Q

what are polymers?

A

molecules made up of long chains of covalently bonded carbon atoms

53
Q

how do polymers form?

A

when lots of small monomers join together

54
Q

Giant covalent structure properties

A

strong covalent bonds
high m and b points
don’t conduct
aren’t soluble

55
Q

why don’t giant covalent structures conduct?

A

because they don’t contain any charged particles

56
Q

Diamonds properties

A 
has 4 covalent bonds 
high m and b point 
strong covalent bonds 
hard structure 
no delocalised electrons
57
Q

Graphite properties

A

forms three covalent bonds
high melting and boiling point
has one delocalised electron
conducts electricity

58
Q

why is graphite a good lubricant?

A

because it’s layers can slide over each other as there are no covalent bonds between layers

59
Q

Fullerene properties

A

shaped like hollow balls or closed tubes
carbon atoms in shape of hexagon
huge surface area
conduct electricity

60
Q

what are fullerenes used for?

A

drug delivery

61
Q

why is it good that fullerenes have a large surface area?

A

help make great industrial catalysts

62
Q

how are metallic bonds formed?

A

when two metals react together

63
Q

Metallic bond properties

A 
electrostatic forces very strong 
high m and b points 
aren’t soluble 
can conduct 
delocalised electrons
64
Q

why are metals more dense?

A

the ions are packed closer together

65
Q

how are metals malleable?

A

layers can slide over each other

66
Q

properties of non metals

A 
dull 
more brittle 
low density 
don’t conduct 
low m and b points 
gain electrons for full outer shell

Chemistry Paper 1 (7 decks)

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