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Chemistry > 22.Periodicity > Flashcards

22.Periodicity Flashcards

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1
Q

Na, Mg and Al…

A
  • are metallic
  • shiny when exposed to air
  • conduct electricity
  • react with dilute acids to give hydrogen and salts
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2
Q

Si…

A
  • is a metalloid

- conducts electricity to some extent

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3
Q

P, S and Cl

A
  • are non metals
  • do not conduct electricity
  • low melting and boiling points
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4
Q

What are the only metal elements in period 3 that react with cold water

A
  • sodium

- magnesium

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5
Q

What is the only non metal that reacts with water

A

Chlorine

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6
Q

Describe the reaction between water and sodium

A
  • vigorous
  • sodium floats on the surface of the water
  • fizzes rapidly
  • melting because of the heat released in the reaction
  • strong alkaline solution of sodium hydroxide is formed
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7
Q

What is the equation of the reaction between sodium and water

A

2Na (s) + 2H2O (l) —> 2 NaOH (aq) + H2 (g)

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8
Q

Describe the reaction of magnesium and water

A
  • very slow at room temperature
  • only few bubbles of H2 formed after a few days
  • resulting solution less alkaline as magnesium hydroxide is only sparingly soluble
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9
Q

Write the equation of the reaction between magnesium and water

A

Mg (s) + 2H2O (l) —-> Mg(OH)2 (aq) + H2 (g)

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10
Q

Write the equation of the reaction between magnesium and steam

A

Mg (s) + H2O (g) —> MgO (s) + H2 (g)

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11
Q

How fast is the reaction between Mg and steam relative to Mg and water

A

Much faster

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12
Q

What type of reactions is the reaction between Na/Mg and water

A

Redox reaction

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13
Q

How can the oxides of elements in group 3 be prepared

A

By a direct reaction of the element with oxygen

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14
Q

Write the equation of the reaction for when sodium burns completely in air

A

2Na (s) + 1/2 O2 (g) —-> Na2O (s)

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15
Q

What colour is sodium oxide

A

White

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16
Q

Write the equation of the reaction for when magnesium burns completely in air

A

2Mg (s) + O2 (g) —-> 2MgO (s)

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17
Q

What colour is magnesium oxide

A

White

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18
Q

What colour are the flames of Na and Mg when burned

A 
Na= yellow
Mg= white
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19
Q

Write the equation of the reaction for when aluminium burns completely in air

A

4Al (s) + 3O2 (g) —> 2AlO3 (s)

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20
Q

What colour is aluminium oxide

A

White

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21
Q

Why is aluminium a reactive metal but appears to be unreactive

A
  • it is always coated with a strongly bonded surface layer of oxide
  • preventing it from further reaction
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22
Q

Write the equation of the reaction for when silicon burns completely in air

A

Si (s) + O2 (g) —> SiO2 (s)

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23
Q

Write the equation of the reaction for when phosphorus burns completely in air

A

4P (s) + 5O2 (g) —> P4O10 (s)

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24
Q

What is the difference between red and white phosphorus when reacting with oxygen

A
  • red must be heated before it will react

- white spontaneously ignites in air and white smoke of phosphorus pentoxide is given up

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25
Q

In a limited supply of oxygen what is formed in the reaction of P and O2

A

P2O3

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26
Q

What colour is sulfur when it burns

A

Blue flame

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27
Q

Write the equation of the reaction for when sulfur burns completely in air

A

S (s) + O2 (g) —> SO2 (g)

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28
Q

Why do Na Mg and Al oxides have high boiling points

A

They are giant ionic lattices where the bonding extends throughout the compound. Strong electrostatic forces

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29
Q

What metal oxide shows covalent character

A
  • Aluminium oxide

- Al high charge density can approach closely to O2- and distort electron cloud

30
Q

Why does silicon oxide have a high melting point

A
  • Giant covalent structure

- bonding extends throughout throughout the structure

31
Q

What do phosphorus and sulfur oxides exist as

A

Separate covalently bonded molecules

32
Q

Why do phosphorus and sulfur oxides have a low boiling point

A

-intermolecular forces are weak van der Waals and dipole dipole forces

33
Q

What is the trend in melting points with SO3 P4O10 and SO2

A

P4O10 > SO3 > SO2

34
Q

What are sodium and magnesium oxides

A

Bases

35
Q

Describe the reaction between sodium oxide and water

A
  • gives sodium hydroxides

- a strongly alkaline solution

36
Q

Write the equation of the reaction for when sodium oxide reacts with water

A

Na2O (s) + H2O (l) —-> 2Na+ (aq) + 2OH- (aq)

37
Q

Describe the reaction between magnesium oxide and water

A
  • gives magnesium hydroxide
  • which is sparingly soluble
  • produces a somewhat alkaline solution
38
Q

Write the equation of the reaction for when magnesium oxide reacts with water

A

MgO (s) + H2O (l) —> Mg2+ (aq) + 2OH- (aq)

39
Q

What two oxides are insoluble in water

A

Aluminium oxide

Silicon dioxide

40
Q

Describe the trend in melting points in period 3 oxides

A

MgO > Al2O3 > SiO2 > Na2O > P4O10 > SO3 > SO2

41
Q

Why does MgO have a higher boiling point then Al2O3

A

Due to packing

42
Q

Non-metals oxides typically form what with water

A

An acidic solution

43
Q

Write the equation of the reaction for when phosphorus oxide reacts with water

A

P4O10 (s) + 6H2O (l) —-> 4H3PO4 (aq)

44
Q

Describe the reaction between phosphorus oxide and water

A
  • reacts violently with water

- to produce acidic solution of phosphoric (V) acid

45
Q

Write an equation for the first stage of ionisation of phosphoric (V) acid in water

A

H3PO4 (aq) H+ (aq) + H2PO4- (aq)

46
Q

Describe the reaction between sulfur dioxide and water

A
  • sulfur dioxide is fairly soluble in water

- reacts with water to give acidic solultion of sulfuric (IV) acidic

47
Q

Write the equation of the reaction for when sulfur dioxide reacts with water

A

SO2 (g) + H2O (l) —> H2SO3 (aq)

48
Q

Write an equation for the ionisation of sulfuric (IV) acid in water

A

H2SO3 (aq) H+ (aq) + HSO3- (aq)

49
Q

Describe the reaction between sulfur trioxide and water

A
  • reacts violently

- to produce sulfuric (VI) acid

50
Q

Write the equation of the reaction for when sulfur trioxide reacts with water

A

SO3 (g) + H2O (l) —> H2SO4 (aq)

51
Q

Write an equation for the ionisation of sulfuric (VI) acid in water

A

H2SO4 (aq) —> H+ (aq) + HSO4 - (aq)

52
Q

Using bonding and structure explain why sodium oxide reacts with water

A
  • sodium oxide contains oxide ion O2- which is a very strong base
  • so readily reacts with water to produce hydroxide ions
53
Q

Using bonding and structure explain why magnesium oxide reacts with water

A
  • magnesium oxide contains oxide ion which is a very strong base
  • however its reaction with water produces a less alkaline solution than sodium oxide
  • because it is less soluble than sodium oxide
54
Q

Using bonding and structure explain why aluminium oxide doesn’t reacts with water

A
  • aluminium oxide is ionic
  • but because of the addition covalent character
  • and strong metallic bonds (al has high charge density)
  • bonding is too strong for the ions to be separated
55
Q

Using bonding and structure explain why silicon dioxide doesn’t reacts with water

A
  • silicon dioxide is giant macromolecular

- water does not affect this type of structure

56
Q

Using bonding and structure explain why phosphorus and sulfur oxides reacts with water

A
  • are covalent molecules

- are react with water to form acidic solutions

57
Q

What is the general trend of solutions of oxides of period 3 elements

A

Go from alkaline to acidic across the period

58
Q

Sodium and magnesium oxide react with acids to give

A
  • salt

- water

59
Q

Give the equation of the reaction between sodium oxide and sulfuric acid

A

Na2O (s) + H2SO4 (aq) —> Na2SO4 (aq) + H2O (l)

60
Q

Give the equation of the reaction between magnesium oxide and hydrochloric acid

A

MgO (s) + 2HCl (aq) —> MgCl2 (aq) + H2O (l)

61
Q

What property does aluminium oxide have

A
  • it is amphoteric

- reacts with both acids and alkalis

62
Q

Give the equation of the reaction between aluminium oxide and hydrochloric acid

A

Al2O3 (s) + 6HCl (s) —-> 2AlCl3 (aq) + 3H2O (l)

63
Q

Give the equation of the reaction between aluminium oxide and sodium hydroxide

A

Al2O3 (s) + 2NaOH (aq) + 3H2O —> 2NaAl(OH)4 (aq)

64
Q

What are the conditions of the reaction between aluminium oxide and sodium hydroxide

A
  • hot ,
  • concentrated,
  • sodium hydroxide
65
Q

What can silicon dioxide act as

A

A weak acid with strong bases

66
Q

Give the equation of the reaction between silicon dioxide and sodium hydroxide

A

SiO (s) + 2NaOH (aq) —> Na2SiO3 (aq) + H2O (l)

67
Q

What are the conditions of the reaction between silicon dioxide and sodium hydroxide

A
  • hot
  • concentrated
  • sodium hydroxide
68
Q

Give the overall equation of the reaction between H3PO4 and sodium hydroxide

A

3NaOH (aq) + H3PO4 (aq) —-> Na3PO4 (aq) + 3H2O (l)

69
Q

Why is the reaction of phosphorus pentoxide and NaOH basically the reaction of H3PO4 and sodium hydroxide

A

H3PO4 is formed when P4O10 reacts with water

70
Q

Give the 3 equation of the reaction between H3PO4 and sodium hydroxide

A

H3PO4 (aq) + NaOH (aq) —> NaH2PO4 (aq) + H2O (l)
NaH2PO4 (aq) + NaOH (aq) —> Na2HPO4 (aq) + H2O (l)
Na2HPO4 (aq) + NaOH (aq) —> Na3PO4 (aq) + H2O (l)

71
Q

Give the equations of the reaction between sodium hydroxide and sulfur dioxide

A

SO2 (aq) + NaOH (aq) —> NaHSO3 (aq)

NaHSO3 (aq) + NaOH (aq) —-> Na2SO3 (aq) + H2O (l)

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