Group 1 and 7 Flashcards

1
Q

what are the similarities of the physical properties of Alkali metals?

A

the melting point is low and it gets lower as you go down the group. The density tends to increase as you go down the group (not regularly). Li, Na, K are all less dense than water. THey are all very soft, getting softer as you go down. THey are shiny when freshly cut but tarnish quickly in air

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2
Q

why does Li, Na, K float on water

A

because they are less dense than water

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3
Q

how do you prevent any reactions form taking place with Na, Li, K and other alkali metals

A

by storing them under oil

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4
Q

What happens when alkali metals are put into water?​ write out the chemical reaction. What changes the speed of the reaction?

A

They react rapidly and form strong alkaline solutions of metal hydroxides.
2M + 2H2O -> 2MOH + H2 (M being an alkali metal)
As you go down the group, the reaction occurs more rapidly as metals are more reactiv
so if you have enough sweat on your hands a corrosive metal hydroxide will form

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5
Q

what are the similar chemical properties of group 1 metals?

A

they all react with water to form a hydroxide (with formula MOH), they react with oxygen to form an oxide (with formula M2O), they form with halogens to form compounds with the formula MX e.g., LiCl, they form ionic compounds which contain an M+ ion e.g, Na+

m represents an alkali metal

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6
Q

what do chemical properties depend on?

A

no. electrons in outer shells

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7
Q

name the main observations that would take place when sodium is put into water

A

sodium floats (less dense than water),
sodium melts into a ball because it has a low melting point and lots of heat is produced by the reaction,
effervescence/ fizzing (hydrogen gas produced), sodium moves around on the surface of the water because the hydrogen isn’t given off symmetrically,
the piece of sodium gets smaller and eventually disappears (as it is used up),
if you ted the solution with universal indicator it goes blue because an alkaline solution has been formed (metal hydroxide so it contains OH- ions)

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8
Q

what is the difference between the reaction between lithium and sodium

A

the reaction with lithium is slower because it has a higher melting point, and the heat isn’t produced as quickly so the lithium doesn’t melt

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9
Q

what is the equation of the reaction with water and K, Na, and Li?

A

2 Na ( s ) + 2 H 2 O ( l ) → 2 NaOH ( aq ) + H2 ( g )
2 K ( s ) + 2 H 2 O ( l ) → 2 KOH ( aq ) + H 2 ( g )
Li(s) + 2H2O(l) → 2LiOH(aq) + H2(g).

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10
Q

what happens when lithiums reacts with water?

A

reaction is slower than sodium’s ​
- lithium has a higher melting point​
- lithium doesn’t melt​
– effervesces more slowly​
- takes longer to disappear​
- floats and moves around on the water (same reasons as sodium)​

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11
Q

what happens when potassium reacts with water?

A

the fastest reaction overall ​
- enough heat is produced to ignite the hydrogen, which burns with a lilac flame​
- reaction often ends with potassium spitting around and exploding​
-effervesces​
- moves around the water and floats​
fizzes MORE vigorously than sodium, moves around and disappears quicker

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12
Q

what is the reaction with rubidium or caesium and water?

A

dangerous and explosive

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13
Q

describe the trend of reactivity in group 1

A

as you go down the group, the ELECTROSTATIC ATTRACTION between the nucleus and outer shells gets weaker (as the distance between the nucleus and outer shell increases aka radius) so it is easier for the atom to lose its electron on its outer shell. Therefore, rwactivity increases as you go down group 1. Shielding also increases as you go down the group which dampens the electrostatic reaction

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14
Q

what happens with a group 1 element in air

A

it tarnishes, the more reactive, the quicker it tarnishes. It tarnishes to form an oxide with the formula M2O (M being an alkali metal)

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15
Q

what happens if you heat an alkali metal in air using a bunsen burner?

A

you get a much more vigorous reaction and it is more difficult to tell the reactivity of the metals as the reactions are so rapid.

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16
Q

what happens when Li is heated using a bunsen burner in air?

A

Li burns with a red flame to form Lithium oxide

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17
Q

what happens when Na is heated using a bunsen burner in air?

A

Sodium burns in a yellow flame to form sodium oxide

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18
Q

what happens when K is heated using a bunsen burner in air?

A

it burns with a lilac flame to form potassium oxide?

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19
Q

what is the reaction for a metal alkali reaction in air? what is produced?

A

4M (g) + O2(g) -> 2M2O (s) (M is an alkali metal)
A WHITE POWDER, AN ALKALI METAL OXIDE, IS PRODUCED

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20
Q

what colour are group 1 metal ions? what does this mean?

A

colourless, meaning that their compounds will be colourless or white unless they are combined with a coloured negative ion like orange Potassium dichomate (VI)

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21
Q

what are group 1 compounds?

A

typical ionic solids and mostly soluble in water

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22
Q

if most group 1 compounds are white/colourless, what colour will they dissolve to be?

A

colorless solutions

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23
Q

what can you predict about francium, given what you know about other group 1 elements?

A
  • it is very soft
  • melting point around room temp
  • density of around 2g/cm3
  • silvery metal which will almost instantly tarnish in air
  • react more violently in water to give francium hydroxide and hydrogen
  • more reactive than caesium
  • will create a strongly alkaline solution which is soluble in water (FrOH)
  • will form compounds what are white or colourless and dissolve in water to give colourless solutions
24
Q

what is another name for group 7?

A

halogen

25
Q

​What is the physical state and colour (at room temp.) of F2

A

gas-yellow

26
Q

​What is the physical state and colour (at room temp.) of Cl2?

A

gas - green

27
Q

​What is the physical state and colour (at room temp.) of Br2?

A

liquid-red-brown liquid, orange/brown vapour

28
Q

​What is the physical state and colour (at room temp.) of I2?

A

solid-grey solid, purple vapour

29
Q

What happens to halogens as you go down group 7? (melting and boiling point)

A
  • melting and boiling points increase as you go down the group​
  • the halogens are all covalent molecular substances and the melting point increases as the relative molecular mass increases and the intermolecular forces of attraction become stronger and requires more energy to overcome the stronger forces of attraction
    remember no covalent bonds broken when melted/boiled
30
Q

what is the trend for reactivity group 7?

A

as you go down group 7 reactivity decreases. as distance (atomic radius) increases and number of outer shells increase, reactivity decreases because the forces of ELECTROSTATIC ATTRACTION get weaker. this makes it harder for the tom to attract an electron to complete its outer shell. (the incoming electron is less attracted to the nucleus). therefore, making it less reactive

31
Q

are halogens safe?

A

no all halogens have extremely acidic, poisonous vapours and have to be handled in a fume cupboard. Liquid bromine is also corrosive

32
Q

what happens when halogens react with hydrogen? what is the equation?

A

they from hydrogen halides e.g., hydrogen fluoride
H2(g) + Br2(g) -> 2HBr (g)

33
Q

are halogens soluble in water?

A

yes, very e.g., HCl (g) - HCl (aq)

34
Q

what happens when halogens react with alkali metals?

A

they form salts e.g., 2Na (s) + Cl(g) -> 2NaCl (s).
this is an ionic solid

35
Q

can you use halogens in displacement reactions?

A

yes

36
Q

what is the difference between dilute and pure bromine?

A

dilute- orange
pure- red-brown

37
Q

what happens if you add chlorine solution to colourless potassium bromide? why does this happen? what is this called? what is the equation for this reaction

A

the solution becomes orange as bromine is formed. This is because chlorine is more reactive than bromine and has displaced bromine from the solution
2KBr (aq) + Cl2 (aq) -> 2KCl (aq) + Br2 (aq)

38
Q

why is it, the more reactive the element the more it can displace (rlly badly worded but ygm)

A

the more reactive an element, the greater tendency it has to form a compound. something that is less reactive is more likely to go back to being the element

39
Q

what happens when chlorine solution is added to potassium iodide solution? what is the equation?

A

a brown or orange (if it is very dilute) solution of iodine. 2KI (aq) + Cl2 (aq) -> 2KCl (aq) + I2 (aq)

40
Q

what happens if a bromine solution is added to colourless potassium iodide? what is the equation?

A

a brown solution of iodine is created
2KI (aq) + Br2 (aq) -> 2KBr (aq) + I2 (aq)

41
Q

what happens when bromine solution is added to potassium chloride? what is the equation?

A

nothing. bromine is less reactive than chlorine, therefore it is not displaced.

42
Q

what happens when iodine solution is added to potassium chloride? what is the equation?

A

nothing. iodine is less reactive than chlorine, therefore it is not displaced.

43
Q

what happens when iodine solution is added to potassium bromide? what is the equation?

A

nothing. iodine is less reactive than bromine, therefore it is not displaced.

44
Q

what is a halide ion?

A

A halide ion is a halogen atom with a negative charge

45
Q

how can displacement reactions involving halogens and halides provide evidence for the trend of G7 reactivity?

A

Displacement reactions involving halogens and halides can be used to show the trend in reactivity of Group 7 elements (halogens) because they demonstrate that more reactive elements displace less reactive elements.

This is clear as the trend in reactivity can be seen by adding halogens to solutions of other halogens and observing any color changes. For example, if you add bromine to a solution of sodium iodide, the bromine will displace the iodine because bromine is more reactive. Iodine is less reactive than bromine and cannot displace it, so no color change will occur.

therefore, As you move up Group 7, the elements become more reactive. For example, fluorine is the most reactive halogen, while astatine is the least reactive.

46
Q

what is a spectator ion? give an example of one.

A

A spectator ion is an ion that is present in a chemical reaction but does not participate in it. e.g. in a displacement reaction with halogens and halides, it doesn’t matter what metal is used so…
potassium in potassium iodide is a spectator ion

47
Q

what does an ionic equation include?

A

everything but the spectator ions

48
Q

write out the ionic equation for potassium bromide reacting with chlorine

A

2Br - (aq) + Сl2 (aq) -> 2Cl - (aq) + Br2 (aq)

49
Q

what is oxidation?

A

loss of electrons

50
Q

what is reduction?

A

gain of electrons

51
Q

what is an oxidising agent?

A

it is something that oxidises something else by taking electrons away from it. Oxidising agents accept electrons and are therefore the thing being reduced in a reaction

52
Q

what is a reducing agent?

A

it is something that reduces something else by giving electrons to it. Reducing agents give away electrons and are therefore the thing being oxidised in a reaction

53
Q

in a reaction between potassium bromide and chlorine, what is being reduced/oxidised?

A

bromide ion is being oxidised because if goes to bromine and loses an electron.
chlorine is being reduced because it becomes a chloride ion and loses an electron

54
Q

what are the main features of G7 elements?

A
  • have diatomic molecules
  • go from gases to liquid to solid as you move down the group
  • melting points and bp increase down the group
  • have coloured poisonous vapours. colours get darker down the group
  • from compounds of HX (x being g7 element) when reacted with hydrogen and these dissolve into water to form acids
  • form ionic salts with metals and covalent compounds with non-metals
  • become less reactive toward the bottom of group
  • will displace elements lower down the group from their salts
55
Q

what can we predict about Astatine, which is the element below iodine in Group 7?

A

-will be darker than iondine
- very dark grey/black
- will be solid at room temp and have a higher melting point than iodine
- will be diatomic and contain At2 molecules
- will react with hydrogen to form HAt, which will dissolve in water to form an acid
- will form salt NaAt with sodium or KAt with potassium
- will contian the astatide ion in its ionic salts
- less reactive than iodine
- will be displaced from solution by iodine

56
Q

describe the trend of reactivity with the halogens.

A

reactivity decreases as you go down
as distance (atomic radius) increases and number of outer shells increases, reactivity decreases because the forces of electrostatic attraction get weaker.
this makes it harder for the atom to attract an electron to complete its outer shell, therefore making it less reactive

57
Q
A