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Revision > Chemistry-2 (Elements of Life) > Flashcards

Chemistry-2 (Elements of Life) Flashcards

1
Q

Colour change of phenolphthalein from acid to alkali

A

Red/ pink to clear

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2
Q

Colour change of methyl orange from acid to alkali

A

Yellow to red

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3
Q

What shape is the s orbital?

A

Spherical

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4
Q

What shape is the p orbital?

A

Dumbbell

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5
Q

What is a dative covalent bond?

A

When the electrons come from the same atom

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6
Q

2 special cases of covalent bonding

A

BF3 boron only has 6 outer electrons not 8

SF6 sulfur has 12 outer electrons not 8

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7
Q

Angle size of tetrahedral molecule

A

109.5

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8
Q

Angle size of water

A

<109.5

104.5 due to lone pairs

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9
Q

Draw a standard first ionisation enthalpy equation

A

X(g) —> x+(g) + e-

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10
Q

Relationship of first ionisation enthalpy down group 1 and 2

A

Decreases

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11
Q

First ionisation enthalpy trend across periods

A

Increases

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12
Q

First ionisation enthalpy of group 1 high or low

A

Low

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13
Q

How to detect carbonates?

A

Dilute HCl and carbonates will fizz and produce CO2

Then test for CO2 with lime water which will turn cloudy if present

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14
Q

How to test for sulfates?

A

Add dilute HCl follow by Barium Chloride
If it forms a white precipitate of barium sulfate
( HCl added to get rid of traces of carbonate ions)

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15
Q

Test for ammonium compounds

A

Ammonia gas is like an alkaline so can be checked using a damp piece of red litmus paper and will turn blue if present

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16
Q

How to test for hydroxides?

A

Litmus paper

Red litmus paper will turn blue

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17
Q

Test for halides

A

Add silver nitrate
Cl- Chlorine will form white precipitate
Br- Bromine will form cream precipitate
I- Iodine will form yellow precipitate

18
Q

How is energy related to frequency

A

E= hv
Plancks constant x freq

E= hc/ w
Plancks constant x speed of light/ wavelength

19
Q

Define elimination reaction

A

When a molecule is removed. Product becomes unsaturated. Double bond formed.

20
Q

Flame test for lithium

A

Crimson

21
Q

Flame test for sodium

A

Yellow

22
Q

Flame test for potassium

A

Lilac

23
Q

Flame test for calcium

A

Red

24
Q

Flame test for barium

A

Green

25
Q

Flame test for copper

A

Blue- Green

26
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Silver Ag 2+

A

Brown

27
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Calcium Ca2+

A

White

28
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Copper (II) Cu 2+

A

Blue

29
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Lead (III) Pb 2+

A

White

30
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Iron (II) Fe 2+

A

Green

31
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Iron (III) Fe 3+

A

Brown

32
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Zinc Zn 2+

A

White, in excess of NaOH is colourless

33
Q

Coloured precipitate by adding sodium hydroxide (NaOH) to Aluminium Al 3+

A

White, in excess of NaOH will turn colourless

34
Q

Describe metallic bonding

A 
Between metals
Sea of delicalised electrons
Conduct 
Insoluble 
High MP 2+ higher than 1+
35
Q

Describe ionic bonding

A 
Metal and non metal
Electrons transferred
High MP
Soluble 
Conduct when molten
35
Q

Describe ionic bonding

A 
Metal and non metal
Electrons transferred
High MP
Soluble 
Conduct when molten
36
Q

Describe simple covalent bonding

A 
Between non metals
Share electrons
Low MP
Don't conduct 
Insoluble
37
Q

Describe giant ionic lattices

A

Eg NaCl
Very high MP
Many ionic bonds

38
Q

Describe giant covalent bonding

A 
Mainly carbon and silicon
Don't conduct except graphite 
High MP
Thermal conductors
Insoluble
39
Q

How to calculate percentage composition?

A

Mass of element/ total mass of compound x100

40
Q

How to calculate empirical formula from percentage composition

A

Percentage, pretend it’s in 100g,

1) Divide percent by Mr of element.
2) Divide by smallest number

Revision (30 decks)

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