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Chemistry > TOPIC 4: INORGANIC CHEMISTRY & THE PERIODIC TABLE > Flashcards

TOPIC 4: INORGANIC CHEMISTRY & THE PERIODIC TABLE Flashcards

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1
Q

Describe the Trend in ionisation energy of Group 2

A

As you go down group 2, number of shells increase means increased shielding.There is a lower attraction between the outer electron and nucleus so ionisation energy decreases

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2
Q

Describe the Trend in reactivity down Group 2

A

The reactivity increases as you go down the group as outer electrons are more easily lost

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3
Q

Equation of GROUP 2 element reacting with water

A

Metal (solid)+ 2Water (liquid)- Metal Hydroxide (aqueous)+ Hydrogen (gas)

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4
Q

Equation of GROUP 2 element reacting with oxygen

A

Metal (solid)+ Oxygen (gas) -2Metal Oxide (solid)

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5
Q

Equation of GROUP 2 element reacting with chlorine

A

Metal (solid)+ Chlorine (gas)- Metal Chloride( solid)

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6
Q

Exceptions on solubility

A
  1. Beryllium oxide- does not react with water and beryllium hydroxide isn’t very soluble.
  2. Magnesium oxide-reacts slowly and magnesium hydroxide is not very soluble.
  3. Barium sulfate is insoluble
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7
Q

Trends in solubility down Group 2 hydroxides + sulfates

A
  1. Singly charged metal hydroxides increase in solubility down the group.
  2. Doubly charged metal sulfates decrease in solubility down the group.
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8
Q

Equation for metal oxide + water

A

metal oxide (solid)+ Water (liquid)-Metal hydroxide (aqueous)

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9
Q

Equation for metal hydroxide with water

A

Metal hydroxide (solid)+Water (liquid)- Metal hydroxide (aqueous)

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10
Q

Equation for metal oxide with dilute hydrochloric acid

A

Metal oxide (solid)+2 HCL (aqueous)-Metal chloride (aqueous)+ Water (liquid)

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11
Q

Equation for metal hydroxide with dilute hydrochloric acid

A

Metal hydroxide (aqueous)+ 2HCl (aqueous) - Metal chloride (aqueous)+ 2Water (liquid)

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12
Q

Thermal decomposition

A

When a substance breaks down when heated

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13
Q

Which ion polarises which ion?

A

The cation polarises the anion distorting it

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14
Q

Difference in thermal stability between group 1 and group 2 carbonates/nitrates

A

Group 2 compounds are less stable than group 1 as they have a higher charge density

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15
Q

Relationship between charge density of a cation and thermal stability

A

The greater the charge density the more the anion is polarised (distorted) the less thermally stable the compound

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16
Q

Thermal decomposition of Group 1 carbonates

A

Group 1 carbonates do not thermally decompose under a bunsen flame

an exception is lithium carbonate(solid)- Lithium oxide (solid)+ carbon dioxide (gas)

17
Q

Thermal decomposition of Group 1 nitrates

A

Group 1 nitrates thermally decompose to form a nitrite and oxygen

General formula: Metal nitrate (solid) - 2Metal nitrite (solid)+ Oxygen (gas)

18
Q

What is the exception for the thermal decomposition of the Group 1 nitrates

A

Lithium nitrate(solid)- Lithium oxide (solid)+ Nitrogen oxide (gas)+ Oxygen (gas)

19
Q

Thermal decomposition of Group 2 carbonates

A

Group 2 carbonates thermally decompose to form the oxide and carbon dioxide

General formula: Metal carbonate (solid)- Metal oxide (solid)+ Carbon dioxide (gas)

20
Q

Thermal decomposition of Group 2 nitrates

A

Group 2 nitrates thermally decompose to form the metal oxide, nitrogen dioxide and oxygen

General formula: 2Metal nitrate (solid)- 2Metal oxide (solid)+ 4Nitrogen dioxide (gas)+ Oxygen (gas)

21
Q

How to test for carbonates

A
  1. See if carbon dioxide is produced

2. Lime water(calcium hydroxide) turns cloudy if carbon dioxide present

22
Q

How to test for nitrates

A
  1. See if oxygen is produced
  2. If glowing splint is relit oxygen is present
  3. Nitrogen oxide is a brown gas and is toxic so has to be done in a fume cupboard
23
Q

Lithium flame colour

A

red

24
Q

Sodium flame colour

A

Orange/yellow

25
Q

Pottasium flame colour

A

Lilac

26
Q

Rubidium flame colour

A

red

27
Q

Caesium flame colour

A

blue

28
Q

Calcium flame colour

A

Brick red

29
Q

Strontium flame colour

A

Crimson red

30
Q

Barium flame colour

A

green

31
Q

How to do a flame test

A
  1. Mix a small amount of the compound with a few drops of hydrochloric acid.
  2. Heat a nichrome wire in a bunsen flame to sterilise it.
  3. Dip the wire in the compound and hold it in the hot flame and observe colour produced.

Chemistry (20 decks)

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