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Chemistry Y13 > Period 3 elements > Flashcards

Period 3 elements Flashcards

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1
Q

PERIOD 3 - Trends in Period 3

A
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2
Q

What is Periodicity?

A

Periodicity is a pattern, in chemical or physical properties across a row of elements (a period) which repeat across the next row of elements

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3
Q

Describe the trend as we go across period 3?

A
  • Atomic radii decreases
  • Due to increasing nuclear charge
  • (more protons) and there is similar shielding
  • Therefore the nucleus attracts the outer electrons more strongly
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4
Q

Describe Trend in Electronegativity as we go across period 3?

A
  • Electronegativity increases as we go across a period
  • Due to increasing nuclear charge
  • And there is similar shielding
  • Therefore more able to withdraw electron density from a covalent bond
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5
Q

Describe trend in First Ionisation energy for period 3?

A

Generally across a period
- There is increasing nuclear charge
- And there is similar shielding
- Therefore the outer electron is attracted more strongly to the nucleus

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6
Q

What are some exceptions when it comes to period 3 elements first ionisation energy?

A
  1. 1st I.E of Al is less than Mg as Al’s Outer electron is in a higher 3p Orbital, Whereas Mg’s outer electron is in a 3s orbital
  2. 1st 1.E of S is less than P’s , as S has a pair of electrons in the same 3P orbital which repel.
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7
Q

Which Period 3 metals undergo metallic bonding?
Describe their their melting and boiling points?

A
  • Na, Mg, Al - Metal Lattices
  • Metallic bonding is the attraction between positively charged ions and delocalised outer shells electrons
  • m.p and b.p increases from Na<Mg<Al
  • Due to stronger metallic bonding
  • Smaller ionic radii
  • More delocalised electrons
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8
Q

What element in Period 3 has the highest melting and boiling point?

A
  • Silicon has the highest melting point
  • As it has strong covalent bonds between all atoms
  • Macromolecular lattice
  • Lots of energy is required to break the bonds
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9
Q

Which elements from period 3 have low melting points?

A
  • Phosphorus, Sulphur and Chlorine have low melting points
  • Due to weak Van Der Waals Forces
  • Between covalent molecules
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10
Q

Why is the melting and boiling point of sulphur greater than Phosphorus?

A
  • Sulphur has a larger molecule
  • Which are more polarisable
  • Has stronger Van Der Waals Forces Between Its Molecules
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11
Q

What element in Period 3 Has the lowest Melting and boiling Point?

A

Argon - Has the lowest melting and boiling point
- Made up of single atoms - Monotomic
- Has weakest Van Der Waals forces between it’s atoms.

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12
Q

REACTIONS OF PERIOD 3 WITH WATER

A
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13
Q

Describe the reaction between Sodium metal and Cold water?
What observations could be seen?

A

Reacts very vigorously with cold water
- Sodium reacts very vigorously
- sodium floats
- Bubbles/Fizzes vigorously
- Colourless solution is formed
- Solution is strongly alkaline (pH = 13/14) when a universal indicator is added

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14
Q

Write an equation to show this reaction?

A

2Na (s) + 2H2O (l) –> 2Na+ (aq) + 2OH- (aq) + H2 (g)

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15
Q

Describe the reaction between magnesium and steam, state the observations that would be seen?

A
  • Magnesium reacts with stea to form magnesium oxide and hydrogen gas
  • White solid is formed
  • Magnesium glows orange as it reacts
  • gas is given off (H2)
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16
Q

Draw an equation to show this reaction?

A
17
Q

Describe the reaction when magnesium reacts with cold water?

A
18
Q

Draw an equation to show this reaction?

A
19
Q

PERIOD 3 ELEMENTS AND OXYGEN

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20
Q

Describe the reaction between the following period 3 elements and oxygen, what colour flame is produced:
1. Sodium
2. Magnesium
3. Aluminium
4. Silicon
5. Phosphorous
6. Sulphur

A
  1. reacts vigorously with oxygen and Yellow flame
  2. Magnesium reacts vigorously with oxygen and a white flame is produced
  3. Aluminium reacts slowly in oxygen and produces a white flame
  4. Silicon reacts very slowly to produce a white flame
  5. Phosphorous spontaneously combusts with oxygen and a white flame is produced
  6. Sulphur burns steadily in oxygena dn a blue flame is produced
21
Q

What products do period 3 elements form when reacted with oxygen?

A

They all form Metal oxides - and white solids except Sulphur

22
Q

Write equations for each of the following period 3 elements with oxygen:
1. sodium
2. Magnesium
3. Aluminium
4. Silicon
5. Phosphorus
6. Sulphur

A
  1. 4Na + O2 –> 2Na2O
  2. 2Mg + O2 —-> 2MgO
  3. 2Al + 3/2 O2 —> Al2O3
  4. Si+ O2 –> SiO2
  5. P4 + 5o2 –> P4O10
  6. S + O2 —> SO2 ( Misty fumes, choking smell, colourless gas)
23
Q

REACTIONS OF PERIOD 3 OXIDES

A
24
Q

What can the trend in melting point of period 3 oxides be explained by? DRAW A GRAPH TO SHOW TREND!

A

The trend in meting point across the period can be explained by the structure and bonding of period 3 oxides

25
Q

What type of bonding occurs between sodium oxide and magnesium oxide? What structure is formed?

A

Ion bonding and an ionic lattice is formed

26
Q

Why do these structures have a high melting point?

A

High melting point is due to strong electrostatic forces of attraction between oppositely charged ions. MgO has a higher m.p than Na2O as Mg2+ ions have a greater charge/more protons and a smaller ionic radii

27
Q

What bonding occurs in aluminium oxide?

A

Al2O3 (s) - forms an ionic bond with a covalent character, and has an ionic lattice

28
Q

Why does Aluminium form an ionic bonds with a covalent character?

A

O2- ions are non-spherical as have been polarised by Al3+ ions, as Al3+ have high charge/size ration. High m.p as strong electrostatic forces of attraction between Al3+ and O2-

29
Q

Describe bonding and structure when Silicon, Phosphorus and Sulphur react with oxygen? And state why they either has a low or high melting point?

A
  • SIO2 - Forms a macromolecular - covalent structure -= therefore has a high melting point as lot’s of energy is required to break strong covalent bonds
  • P4O10 and SO2 are simple molecular covalent substances - therefore little energy is required to break weak intermolecular forces between molecules
  • P4O10 > SO2 as P4O10 is a larger molecule, so more polarisable, stronger van Der Waals forces
30
Q

PERIOD 3 OXIDES WITH WATER

A
31
Q

What type of oxides do metal oxides and Non-metal oxides form? And what does each of these particular oxides react with?

A
  1. Metal oxides have ionic bonding and for BASIC oxides (Na2O and MgO), Basic metal oxides react with Acids
  2. Non-metal oxides have covalent bonding and for ACIDIC oxides (P4O10, SO2, SIO2) , Acidic non-metal oxides react with bases

(so across the period table, bonding goes from ionic to covalent and oxides turn from basic to acidic)

32
Q

Describe what is formed when Period 3 Oxides react with water. Write equations to show these reactions. And Give the approximate pH for the resulting solution.

A
  1. Na2O + H2O —> 2Na+ (aq) + 2OH- (aq) pH = 13/14
  2. MgO + H2O –> Mg(OH)2 (s) pH = 9/10
  3. Al2O3 + H2O —> insoluble pH= 7
  4. SiO2 + H2O –> Insoluble pH = 7
  5. P4O10 + 6H2O –> 4H3PO4 pH = 0
  6. SO2 + H2O ⇌ H+ + HSO3- pH = 3
  7. SO3 + H2O –> 2H+ + SO42- pH = 0/1
33
Q

PERIOD 3 OXIDES WITH ACIDS AND ALKALIS

A
34
Q

What acids do metal oxides react wiht?

A
  1. Na2O reacts with HCL
  2. MgO reacts with sulphuric acid
35
Q

What alkali’s do non-metal oxides react with?

A

All non-metal oxides react with Sodium hydroxide (NaOH)

36
Q

Draw equations to show the reaction of Period 3 metal oxides with Acids

A
  1. Na2O (s) + 2HCl (aq) –> 2NaCl (aq) + H2O (l)
  2. MgO (s) + H2SO4 (aq) –> MgSO4 (aq) + H2O (l)
37
Q

Write equations to show how non-metal period 3 oxides react with an alkali (such as NaOH)

A
  1. SiO2 (s) + 2NaOH (aq) —> Na2SiO3 (aq) + H2O (l)
  2. P4O10 (S) + 12NaOH (aq) —> 4Na3PO4 (aq) + 6H20 (l)
  3. SO2 + 2NaOH (aq) —> Na2SO3 (aq) + H2O (l)
  4. SO3 + 2NaOH (aq) —> Na2SO4 (aq) + H2O (l)
38
Q

DONE!

A

Chemistry Y13 (13 decks)

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