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Chem Mr D > Group 7 & Redox > Flashcards

Group 7 & Redox Flashcards

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1
Q

Fluorine f2

A

Yellow gas

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2
Q

Chlorine Cl2

A

Green gas

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3
Q

Bromine Br2

A

Orange liquid

  • often used in solution in water
  • easily forms orange vapour
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4
Q

Iodine i2

A

Grey crystalline solid

  • often used in a (sort of) solution in water
  • easily forms purple vapour
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5
Q

Atomic radius down group

A
  • increases

- more shells of electrons so bigger atom

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6
Q

Electronegativity down group

A
  • decreases
  • more shells/ shielding
  • so weaker attraction between nucleus + pair of electrons in covalent bond
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7
Q

Electronegativity definition

A

Power of an atom to attract the 2 electrons in the covalent bond

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8
Q

Melting and boiling points down group

A
  • increases
  • due to stronger van der Waals forces between molecules
  • due to molecules having more electrons
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9
Q

Ionisation energy down group 7

A
  • decreases
  • more shells/ shielding
  • atoms get bigger
  • so weaker attraction between nucleus + outer electron
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10
Q

What is broken when states are changed?

A

Van der Waals forces not covalent bonds

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11
Q

Halides

A

Fluoride
Chloride
Bromide
Iodide

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12
Q

Halides charge?

A
  • 1
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13
Q

Halogens and halides reaction table

A 
F- Cl- Br- I-
F2    X.  Y.   Y.  Y 
Cl2.  X.  X.  Y.  Y
Br2.  X.  X.  X. Y
I2      X.  X. X.  X
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14
Q

What happens in halogen and halide reaction?

A

The halogen steals electron from the halide

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15
Q

What happens when Bromide and Chlorine react?

A

Yellow solution

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16
Q

What happens when iodide and chlorine react?

A

Brown solution

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17
Q

What happens when iodide and bromine react?

A

Brown solution

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18
Q

Halide and halogen overall reaction equation?

A

Halogen + 2 halide -> 2 new halide + new halogen
E.g Cl2 + 2I- -> 2 Cl- + I2
Use 2 to balance

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19
Q

Oxidising power of halogens explainaiton

A
  • halogen atom gains an electron when it oxidises the halide ion
  • the small the halogen atom, the earlier it is to gain an electron as it is smaller and has less shielding
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20
Q

Oxidising power strongest - weakest

A

Chlorine
Bromide
Iodine

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21
Q

Oxidation states definition

A

A number representing how many electrons have either been lost or gained

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22
Q

Oxidation number/ state of a single element

A

0

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23
Q

Oxidation state of oxygen

A

-2

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24
Q

Writing half equations steps

A

1) calculate oxidation states
2) balance equation
3) sort out electrons
4) for every O gained/lost, add/remove H2O
5) for every H gained/lost, ass remove one H+
6) check if total electric charge on left equals that in right

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25
Q

Combining half equations

A

Put two equations together then balance

Should be no electrons in final equation

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26
Q

Strongest to weakest reducing power of halogens

A

Iodide I-
Bromide Br-
Chloride Cl-
Fluoride F-

27
Q

Reducing power of halogens explanations

A
  • halide ion loses ion when it reduces the H2SO4 (sulfuric acid)
  • bigger halide ion, easier to lose electron because not shielding
28
Q

What does HCL produce?

A

Steamy fumes

29
Q

What acid is involved in reducing power of halides?

A

Concentrated sulfuric acid (H2SO4)

30
Q

Does chlorine want to gain or lose electron?

A

Gain

31
Q

Where are electrons on reduction?

A

Left

32
Q

Where are electrons in oxidation?

A

Right

33
Q

What is chlorine used for?

A
  • swimming pools
  • water
  • kills bacteria
34
Q

What is H2SO4?

A

Sulfuric acid

35
Q

What is NAOH?

A

Sodium hydroxide

36
Q

What is NaCl?

A

Sodium chloride

  • table salt
  • roads
37
Q

What is NaClO?

A

Sodium chlorate

-bleach

38
Q

Most to learn soluble ions (H2SO4)

A

Mg 2+ (mgso4)
Ca 2+ (caso4)
Sr 2+ (srso4)
Ba 2+ (baso4)

39
Q

Which H2SO4 ions are liquids?

A

MgSO4

CaSO4

40
Q

Which H2SO4 ions are solids/white precipitates?

A

SrSO4

BaSO4

41
Q

What is BaSO4 used for?

A

X-rays to light up insides as it is insoluble

42
Q

What are the 4 hydroxide ions? (NaOH)

A

Mg(OH)2
Ca (OH)2
Sr (OH)2
Ba (OH)2

43
Q

Which hydroxide ions are solids?

A

Mg (OH)2

Ca (OH)2

44
Q

Which hydroxide ions are liquids?

A

Sr (OH)2

Ba (OH)2

45
Q

What is the ammonia gas test?

A
  • red litmus paper
  • damp
  • turns blue to detect ammonia
46
Q

What is NH4OH?

A

Ammonium hydroxide

47
Q

What are the 4 silver nitrate ions? (AgNO3)

A

AgF
AgCl
AgBr
AgI

48
Q

What AgNO3 ions are solids?

A

AgCl
AgBr
AgI

49
Q

What AgNO3 ion is a liquid?

A

AgF

50
Q

What does AgF look like?

A

Colourless solution

51
Q

What does AgCl look like?

A

White precipitate

52
Q

What does AgBr look like?

A

Cream precipitate

53
Q

What does AgI look like?

A

Yellow precipitate

54
Q

What happens when AgCl/ AgF / AgI reacts with dilute NH3?

A

Nothing

55
Q

What happens when AgCl reacts with NH3?

A

Dissolve (colourless solution)

56
Q

What is NH3?

A

Ammonia

57
Q

What happens when AgI/ AgF reacts with concentrated NH3?

A

Nothinf

58
Q

Why don’t we react AgCl with concentrated NH3?

A

Because it already dissolved with dilute NH3

59
Q

What happens with AgBr reacts with concentrated NH3?

A

Dissolve (colourless solution)

60
Q

What is a text for hydroxide?

A

Add magnesium + vice versa

61
Q

What can be used to check for Br-?

A

Dilute NH3

62
Q

What can be used to text for Barium?

A

Sulfate (vice versa)

63
Q

What contains H+ ions?

A

Acid

Chem Mr D (8 decks)

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