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Chemistry A level Module 3 > Chapter 7-8 - Periodicity&Reactivity Trends > Flashcards

Chapter 7-8 - Periodicity&Reactivity Trends Flashcards

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1
Q

The repeating…

Define Periodicity

A

The repeating pattern of trends in physical and chemical properties which occurs across different periods in the periodic table.

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2
Q

nuclear attraction? ionisation energy?

Trends across a period

A

Nuclear charge - Increases
Shielding - Stays roughly the same
Atomic Radius - Decreases

= Nuclear Attraction - Increases

= Ionisation energy increases

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3
Q

Trends down a group

A

Nuclear Charge - Increases
Shielding - Increases
Atomic Radius - Increases

= Nuclear Attraction decreases because atomic charge and shielding cancel out

= Ionisation energy decreases

= Reactivity increases

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4
Q

The energy required to…

Define First Ionisation Energy

A

The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.

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5
Q

Give an equation to represent the First Ionisation Energy

A

X(g) ——> X+(g) + e-

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6
Q

State the factors that affect Ionisation Energy

A

Nuclear Charge
Atomic Radius
Electron Shielding

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7
Q

when an element is…

Define Disproportionation

A

When an element is simultaneously oxidised and reduced to form 2 different products

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8
Q

Metal + Oxygen

A

= Metal Oxide

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9
Q

Metal + Water

A

= Metal Hydroxide + Hydrogen

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10
Q

Metal Oxide + Water

A

= Metal Hydroxide

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11
Q

Metal + Acid

A

= Salt + Hydrogen

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12
Q

What compound can be used to neutralise acids soils?

A

Calcium Hydroxide

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13
Q

Which 2 compounds can be used to treat indigestion?

A

Magnesium Hydroxide and Calcium Carbonate

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14
Q

2 facts about of Chlorine

A

Kills Bacteria and is toxic

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15
Q

Colour of fluorine as an element

A

Pale Yellow Gas

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16
Q

Colour of Chlorine as an element

A

Pale Green Gas

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17
Q

Colour of Chlorine in water

A

Pale Green

18
Q

Colour of Chlorine in hexane (an organic solvent)

A

Pale Green

19
Q

Colour of Bromine as an element

A

Red-Brown Liquid

20
Q

Colour of Bromine in water

A

Orange (yellow-orange)

21
Q

Colour of Bromine in hexane (an organic solvent)

A

Orange (orange-red)

22
Q

Colour of Iodine as an element

A

Grey Crystals (purple vapour)

23
Q

Colour of Iodine in water

A

Brown

24
Q

Colour of Iodine in hexane (an organic solvent)

A

Violet

25
Q

Why do the boiling points increase down group 7?

A

Due to the increased london forces between molecules that require more kinetic energy to overcome

26
Q

Why does reactivity decrease down group 7?

A

It becomes harder to gain electrons to form 1- ions.

27
Q

Cl2 + H2O

A

= HClO + HCl

28
Q

Chlorine + cold, dilute, aqueous sodium hydroxide

A

= NaClO (bleach) + NaCl + Water

29
Q

State the 3 steps to test for Halide ions

A
  • add dilute nitric acid
  • add silver nitrate solution
  • add ammonium solution
30
Q

Chloride positive result

A

White precipate formed
soluble in all conc. ammonia

31
Q

Bromide positive result

A

Cream precipitate formed
soluble only in concentrated ammonia

32
Q

Iodide positive result

A

Yellow precipitate formed
Insoluble in ammonia

33
Q

Test for carbonate ions

A
  • add dilute acid
  • bubble through limewater
    PR- turns cloudy (CO2 formed)
34
Q

Test for sulphate ions

A
  • add dilute HCl
  • add barium chloride sol.
    PR- white precipitate forms (barium sulphate)
35
Q

Test for Ammonium ions

A
  • add sodium hydroxide
  • warm gently
    PR- ammonia gas turns red litmus paper blue
36
Q

Cl2 + NaOH (aq)

chlorine + cold, dilute sodium hydroxide

A

NaClO + NaCl + H2O

bleach + sodium chloride + water

37
Q

when asked about boiling points talk about…

A
  • london forces etc..
38
Q

when asked about reactivity talk about…

A
  • shells/ electrons
39
Q

Br2 + Cl- ion

A

no reaction as Chlorine is more reactive than Bromine so solution remains orange in cyclohexane

40
Q

halogen reactivity

A

Cl2 > Br2 > I2

41
Q

displacement reaction to confirm order of halogen reactivity

A

addition of Br2 (aq) to I- (aq) ions

Chemistry A level Module 3 (2 decks)

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