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A Level Chemistry > 3.2.4 Period 3 Elements > Flashcards

3.2.4 Period 3 Elements Flashcards

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1
Q

State how and under what conditions, sodium and magnesium react with water

A

Sodium- reacts with cold water vigorously
Floats on water, fizzes, melts
2Na + 2H2O —> 2NaOH + H2
Magnesium- reacts with steam/slowly with water
Steam: Mg + H2O —> MgO + H2
Water: Mg + 2H2O —> Mg(OH)2 + H2 sparingly soluble

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2
Q

State how the group 3 elements react with oxygen?

A

Na: burns with yellow-orange flame to produce white powder
Mg,Al,Si: burns with white flame to produce white powder
P4: burns with very bright white flame to produce white powder
S8: burns with blue flame + gives off choking gas
Cl2: No reaction
4Na + O2 —> 2Na2O / 2Na + O2 —> Na2O2
2Mg + O2 —> 2MgO
4Al + 3O2 —> 2Al2O3
Si + O2 —> SiO2
P4 + 5O2 —> P4O10 / P4 + 3O2 —> P4O6
S + O2 —> SO2

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3
Q

Structure, bonding, melting point of Na2O, MgO, Al2O3

A

All ionic-lattice structure, high boiling points (solid)
Bp order: MgO, Al2O3, Na2O
MgO + Al2O3 > Na2O as Mg2+ ions are smaller + more charged
MgO > Al2O3 as Al2O3 has some covalent character due to polarising nature of Al3+

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4
Q

Structure, bonding, melting point of SiO2

A

Giant covalent (solid)
High boiling point

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5
Q

Structure, bonding, melting point of P4O10

A

Simple molecular
Relatively high boiling point (solid)
Large molecule-strong IMF

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6
Q

Structure, bonding, melting point of SO2 + SO3

A

Simple molecular
Low boiling points
Bp- SO3 is larger molecule than SO2 so higher- more IMF
SO2- gas
SO3- liquid

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7
Q

Group 2 oxide reaction with water trend + how the structures explain their reactions

A

General increase in solubility
Na2O- dissolves + reacts with water to form solution
Na2O + H2O —> 2NaOH(aq)
MgO- slightly soluble- some dissolves + reacts with water to form solution
MgO + H2O —> Mg(OH)2(aq)
Al2O3- insoluble - high lattice enthalpy
SiO2- insoluble - high lattice enthalpy due to covalent bonds
P4O10- violent reaction
P4O10 + 6H2O —> 4H3PO4
SO2- dissolves + reacts with water to form solution
SO2 + H2O —> H2SO3
SO3- violent reaction
SO3 + H2O —> H2SO4
Na+/Mg2+ and O2- ions dissolve in water
O2- + H2O —> 2OH- (ionic)
P/S are partially positive so attach to H2O molecules to produce H+ ions from water molecules (simple molecular)

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8
Q

Describe how the period 3 oxides react with acids

A

Metals react with acids (Na2O,MgO,Al2O3) to produce metal cations and water
Na2O + 2H+ —> 2Na+ + H2O
MgO + 2H+ —> Mg2+ + H2O
Al2O3 + 6H+ —> 2Al3+ + 6H2O
Basic oxides

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9
Q

Describe how the period 3 oxides react with bases

A

Al2O3,SiO2,P4O10,SO2,SO3 react with bases to form negative ions
Al2O3 + 2OH- + 3H2O —> 2Al(OH)4-
SiO2 + 2OH- —> SiO32- +H2O (hot, conc NaOH)
P4O10 + 12OH- —> 4PO43- + 6H2O
SO2 + 2OH- —> SO32- + H2O
SO3 + 2OH- —>SO42- + H2O

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10
Q

Which metal oxide is amphoteric + define

A

Al2O3
Acts as acid or base

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11
Q

pH of
NaOH
Mg(OH)2
4H3PO4
H2SO3
H2SO4
SO2
SO3

A

14
10
1-2
3
0
2-3
0-1

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12
Q

Explain why sodium oxide forms an alkaline solution when it reacts with water

A

Na2O contains O^2- ions
Ions react with water to form OH^-

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13
Q

Silicone melting point

A

Very high
Very strong covalent structure
Lots of energy required to break strong covalent bonds

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14
Q

Melting point of phosphorus to chlorine

A

Simple covalent held together by weak van der Waals
Less energy required to overcome

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15
Q

Why does Argon have lower melting point than chlorine

A

Noble gas
Individual atoms with full outer shell electrons
Stable with weak Van der Waals
Less energy required to overcome

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16
Q

Appearance and physical properties of sodium

A

Metallic, shiny, conducts electricity

17
Q

Appearance and physical properties of magnesium

A

Metallic, shiny, conducts electricity

18
Q

Appearance and physical properties of aluminum

A

Metallic, shiny, conducts electricity

19
Q

Reaction of Al with cold water

A

No reaction

20
Q

Why is aluminium considered unreactive even though the metal itself is reactive

A

Covered by Al2O3 from oxidation
If Al2O3 scratched off, Al reacts rapidly with air to form new coat

21
Q

Appearance and physical properties of silicon

A

Semimetal, semiconductor of electricity

22
Q

Appearance and physical properties of phosphorus

A

Non-metal, low melting + boiling point, doesn’t conduct electricity
Red has crystal structure
White as P4

23
Q

Reaction of phosphorus in limited oxygen

A

Incomplete combustion
4P + 3O2 —> P4O6

24
Q

Appearance and physical properties of sulphur

A

Non-metal, low melting + boiling point, doesn’t conduct electricity

25
Q

Which period 3 oxides are basic

A

Na2O and MgO, Al2O3

26
Q

Is aluminium oxide soluble

A

Not in water

27
Q

Reaction of aluminium oxide with NaOH

A

Al2O3 + 2NaOH + 3H2O —> 2NaAl(OH)4
Sodium aluminate

28
Q

Is silicon dioxide soluble in water

A

No

29
Q

In what conditions will silicon dioxide act as an acid

A

Reacts as weak acid with strong base

30
Q

Reaction of silicon dioxide with hot conc NaOH

A

SiO2 + 2NaOH —> H2O + Na2SiO3
Sodium silicate

31
Q

How is silicon dioxide used in the production of Fe

A

SiO2 + CaO —> CaSiO3
Calcium silicate

32
Q

Reaction of P4O10 with NaOH

A

3NaOH + H3PO4 —> Na3PO4 + 3H2O

33
Q

Reaction of SO2/SO3 with water

A

SO2 + H2O —> H2SO3
SO3 + H2O —> H2SO4

34
Q

Reaction of SO2 with NaOH (2 reactions)

A

SO2 + NaOH —> NaHSO3
NaHSO3 + NaOH —> Na2SO3 + H2O

35
Q

Structure, bonding and shape in PO4^3-/SO4^2-

A

Electrons delocalise to give tetrahedral structure
Each P-O/S-O bond same length
109.5°

36
Q

Structure, bonding and shape of SO3^2-

A

Trigonal pyramid shape
Each S-O bond the same
S has one lone pair of electrons
107° bond angle

37
Q

Uses of MgO

A

Additive to cattle feed

38
Q

Uses of SO2

A

Reactant in contact process making H2SO4

A Level Chemistry (36 decks)

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