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OCR GCSE C4-C6 > C4.1 - predicting chemical reactions > Flashcards

C4.1 - predicting chemical reactions Flashcards

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1
Q

what is another name for Group 1 elements? (and why)

A

alkali metals, because they react with water to form alkaline solutions

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2
Q

state 4 properties of group 1 elements

A
  • solid at room temperature
  • can be cut with a knife (soft)
  • shiny when freshly cut
  • good conductor of electricity
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3
Q

how is softness affected as you go down the group 1 elements?

A

increases

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4
Q

what is the trend of density in group 1 elements?

A

increases (while going down list)

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5
Q

what is the trend for melting points of Group 1 elements?

A

decreases

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6
Q

how does reactivity change as you go down the Group 1 elements?

A

increases

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7
Q

how does lithium react with water?

A

fizzes steadily then slowly disappears

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8
Q

how does sodium react with water? (3)

A
  • melts to form a silver ball
  • fizzes vigorously
  • quickly disappears
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9
Q

how does potassium react with water? (2)

A
  • ignites immediately
  • lilac flame
  • quickly disappears
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10
Q

state the word equation of the reaction between Group 1 elements and water

A

metal + water -> metal hydroxide + hydrogen

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11
Q

give the balanced chemical formula (with state symbols) of when sodium reacts with water

A

2Na (s) + 2H20 (l) -> 2NaOH (aq) + H2 (g)

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12
Q

explain the trend of reactivity in Group 1 elements

A
  • reactivity increases
  • atoms become larger, and so harder for positive nucleus to attract outer electron (so easier to lose, and therefore react)
  • outer electron’s distance from nucleus increases
  • shielding (other electrons get in the way)
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13
Q

are halogens:

  • nonmetals/metals
  • brittle/solid
  • conduct elecricity well/or not
  • exist as mono-atomic/diatomic
  • strong intermolecular forces/weak
A
  • nonmetals
  • brittle (solid)
  • poor conductors of electricity
  • exist as diatomic molecules
  • weak im forces
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14
Q

describe The colour of fluorine at room temperature

A

pale yellow gas

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15
Q

describe chlorine at room temperature

A

green gas

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16
Q

describe bromine at room temperature

A

orange-brown liquid (vaporises easily)

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17
Q

describe iodine at room temperature

A

grey-back solid (sublimes to purple gas)

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18
Q

trend of density of group 7 elements?

A

increases

19
Q

trend of melting/boiling points of Group 7 elements?

A

increases

20
Q

what is another name for group 7 elements?

A

halogens

21
Q

trend of reactivity of halogen elements?

A

decreases

22
Q

do group 7 elements react with group 1 elements?

A

yes, vigorously

23
Q

how do you explain the trend in reactivity of group 7 elements?

A
  • decreases
  • atoms become larger, and so harder for positive nucleus to attract other electrons electron (so harder to gain, and therefore react)
  • outer electron’s distance from nucleus increases (so harder to gain electrons)
  • shielding (other electrons get in the way) - amplified effect
24
Q

what determines how reactive an element is?

A

how easily it loses/gains electrons

25
Q

what is a halide?

A

a compound containing a group 7 element with one other element (hydrogen/metal)
a group 7 ion would be a halide ion

26
Q

how do you determine whether a halogen would displace another halide?

A

whether it is more reactive or not (or higher on the periodic table)

27
Q

would chlorine displace bromine from bromides?

A

yes

28
Q

where are the noble gases?

A

Group 0 (IUPAC group 18)

29
Q

why are noble gases unreactive?

A

because they have full outer shells (little tendency to lose or gain electrons)

30
Q

state 3 features of noble gases

A
  • conduct electricity
  • odorless
  • gases at room temperature
31
Q

trend of boiling point of noble gases? (and why)

A

increases (atoms get larger, im attractive forces become stronger) - GENERALLY VERY LOW

32
Q

trend of density of noble gases (why)?

A

increases, larger atoms take up more space in set volume

GENERALLY VERY LOW - in gas state

33
Q

state 4 properties of transition metals

A
  • shiny (when freshly cut)
  • good conductor of electricity
  • strong
  • malleable
  • high density
  • hard
34
Q

how do transition metals compare to Group 1 metals (alkali metals)

A
  • stronger + harder
  • higher density
  • higher melting point
35
Q

are the transition metals reactive?

A

not really, react very slowly (if at all)

36
Q

what do gold, platinum and iridium have in common?

A

do not react with water or oxygen at all

37
Q

are alkali metals coloured in ionic compounds?

A

(no) colourless

38
Q

are transition metals coloured in ionic compounds?

A

(yes) coloured

39
Q

are transition metals good catalysts?

A

yes

40
Q

give an example of uses for platinum, rhodium and palladium

A

catalytic converters

convert harmful gases in vehicle exhaust fumes into less harmful ones

41
Q

what is produced when a metal reacts with water?

A

metal hydroxide + hydrogen

42
Q

what is produced when a metal reacts with a dilute acid?

A

salt (ie. sodium chloride) + hydrogen

43
Q

what experiment do you do to put metals into order of reactivity?

A
  • place metal in water/dilute acid

- compared amount of bubbles/hydrogen produced

44
Q

how would reactive non-metals react (what bonds do they form)?

A

form covalent bonds with each other

OCR GCSE C4-C6 (12 decks)

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