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Inorganic Chemistry > Unit 2: Section 3- Period 3 Elements (2.4) > Flashcards

Unit 2: Section 3- Period 3 Elements (2.4) Flashcards

1
Q

What subshell is the outer electron in in Mg and Na?

A

s subshell

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2
Q

What are the different reactions between magnesium and sodium with water?

A

sodium more reactive, more readily ionises
magnesium reacts slowly with cold water

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3
Q

State the reaction between sodium and cold water

A

2Na + 2H2O → 2NaOH + H2

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4
Q

State the reaction between magnesium and cold water

A

Mg + 2H2O → Mg(OH)2 + H2

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5
Q

State the reaction between magnesium and steam

A

Mg (s) + H2O (g) → MgO (s) + H2 (g)

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6
Q

How do the period 3 elements react with oxygen?

A

they all form oxides (except argon) that take up their highest oxidation state

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7
Q

What is the exception for sulphur in oxidation states when reacting with oxygen?

A

sulphur forms an oxide where the oxidation state of sulphur is +4

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8
Q

What is the oxidation state of the period 3 element in an oxide?

A

+3 (except sulphur)

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9
Q

What visible changes can you see when sodium reacts with oxygen?

A
  • white solid formed
  • yellow flame
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10
Q

State the equation of sodium reacting with oxygen

A

4Na (s) + O2 (g) → 2Na2O (s)

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11
Q

What colour flame do magnesium, aluminium, silicon and phosphorous burn with?

A

white flame

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12
Q

What colour flame does sulphur burn with?

A

blue flame

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13
Q

State the equation between sulphur and oxygen

A

S (s) + O2 (g) → SO2 (g)

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14
Q

State the equation for magnesium reacting with oxygen

A

2Mg (s) + O2 (g) → 2MgO (s)

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15
Q

State the equation for aluminium reacting with oxygen

A

4Al (s) + 3O2 (g) → 2Al2O3 (s)

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16
Q

State the equation for silicon reacting with oxygen

A

Si (s) + O2 (g) → SiO2 (s)

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17
Q

State the equation for phosphorous reacting with oxygen

A

4P (s) + 5O2 (g) → P4O10 (s)

18
Q

What are properties of sulphur dioxide (SO2)

A

acidic, choking gas

19
Q

What are the three giant ionic lattice structures of period 3 oxides?

A

Na2O, MgO, Al2O3

20
Q

Describe the structure of SiO2

A

macromolecular, giant covalent oxide

21
Q

Name the structure of P4O10 and SO2

A

simple molecular structures

22
Q

How do the structures of period 3 metal oxides effect the melting points?

A

these different structures lead to period 3 metal oxides having different melting points

23
Q

What type of melting point do ionic metal oxides have?

24
Q

Explain the trend in melting point from Na2O to Al2O3

A

melting point increases due to the increased charge of the cation, which makes the electrostatic forces even stronger

25
Q

What happens to the trend in melting point after Al2O3?

A

there is an increase, as SiO2 is macromolecular, with very strong covalent bonds, and a very high MP

26
Q

What type of melting point does SiO2 have?

A

very high, strong covalent bonds, high energy needed to break

27
Q

What happens to the trend in melting point after SiO2?

28
Q

What type of melting point does P4010 and SO2 have?

A

lower melting point because they are simple molecular oxides
P4O10 has higher than SO2 because of more electrons, so larger van der waals.

29
Q

What do metal ionic oxides form when they react with water?

A

hydroxides which are alkaline

30
Q

State the reaction between Na2O and water, and the pH of the product

A

Na2O + H2O → 2NaOH

pH of 13

31
Q

State the reaction between MgO and water, and the pH of the product

A

MgO (s) + H2O (l) → Mg(OH)2 (s)

pH of 9

32
Q

Explain why the pH of Mg(OH)2 is lower than 2NaOH

A

because Mg(OH)2 is only slightly soluble, so it only slightly dissociates
difference in solubility due to Mg ion being smaller, so it has a stronger lattice, so fewer OH- ions produced

33
Q

State the reaction between phosphorous oxide and water, and give the pH of the product

A

P4O10 (s) + 6 H2O (l) → 4H3PO4 (aq)

pH of 0

34
Q

State the reaction between SO2 and water, and give the pH of the product

A

SO2(g) + H2O (l) → H2SO3 (aq)

pH of 3

35
Q

State the reaction between SO3 and water, and give the pH of the product

A

SO3 (g) + H2O (l) → H2SO4 (aq)

pH of 0

36
Q

What are the three types of oxides?

A

acidic
basic
amphoteric

37
Q

What period 3 oxides are examples of basic oxides?

38
Q

What period 3 oxides are examples of acidic oxides?

A

P4O10
SO2
SO3

39
Q

What period 3 oxides are examples of amphoteric oxides?

40
Q

What happens to period 3 basic oxides in reactions?

A

react with acids to form a salt and water

41
Q

What happens to period 3 acidic oxides in reactions?

A

react with bases to form salts

42
Q

What happens to period 3 amphoteric oxides in reactions?

A

react with acids or bases

they can act as both an acid an an alkali

Inorganic Chemistry (5 decks)

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