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Chemistry > 3.2.4 - Period 3 and their oxides > Flashcards

3.2.4 - Period 3 and their oxides Flashcards

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1
Q

Give the equation for the reaction between Al2O3 and NaOH.

A

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

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2
Q

How do you prove experimentally that a compound contains ions?

A

Melt the solids and show they conduct electricity.

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3
Q

What are the observations for when Mg reacts with steam?

A

Bright white flame and white solid/powder.

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4
Q

How does Aluminum oxide react with water?

A

AlO2 is amphoteric, acting as both an acid and a base. Aluminum oxide has both ionic and covalent nature, resulting in it being insoluble in water.

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5
Q

Does electronegativity increase across period 3?

A

Yes, electronegativity increases across a period because the number of charges on the nucleus increases, attracting the bonding pair of electrons more strongly.

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6
Q

Type of bonding between Phosphorus?

A

Covalent.

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7
Q

Bonding between sodium?

A

Ionic.

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8
Q

What are the 2 basic metal oxides?

A

Sodium and Magnesium.

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9
Q

How do you test for H2 gas?

A

Test with a lighted splint; a squeaky pop proves the presence of H2 gas.

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10
Q

Why does MgO have a higher boiling point than Al2O3 and Na2O?

A

MgO has a 2+ charge, while Na has only a +1 charge, leading to greater charge density and stronger attraction to oxygen. Al2O3 has 3+ ions that distort the electron cloud of oxygen, containing some covalent character, requiring less energy to break bonds.

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11
Q

What do Ionic oxides (Na and Mg) form when they are added to water?

A

They form hydroxides.

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12
Q

Explain how Sodium burns with oxygen and what it forms.

A

Sodium burns with a yellow flame to produce a white solid.

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13
Q

State how Mg, Al, Si, and P burn with oxygen.

A

They burn with a white flame to give white solid smoke.

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14
Q

How does S react with oxygen?

A

S burns with a blue flame to form an acidic choking gas.

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15
Q

Explain how period 3 elements react with a Bunsen burner.

A

Sodium burns with a yellow flame to produce a white solid. Mg, Al, Si, and P burn with a white flame to produce white solid smoke. S burns with a blue flame to produce an acidic choking gas.

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16
Q

Write an equation for the reaction of excess magnesium oxide with phosphoric acid.

A

MgO + H3PO4 -> Mg3(PO4)2 + H2O

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17
Q

Reactions of non-metal oxides.

A

Non-metal oxides react with water to form acids.

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18
Q

Bonding of simple molecular oxides.

A

Simple molecular oxides have covalent bonds.

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19
Q

Bonding of SiO2.

A

SiO2 has a giant covalent structure.

20
Q

How is the aluminum metal ion protected from corrosion?

A

Aluminum forms a protective oxide layer.

21
Q

Explain how metal ionic oxide (Na2O) reacts with water to form hydroxides which are alkaline.

A

Na2O + H2O -> 2NaOH

22
Q

Why is MgO better than NaOH for treating acidity?

A

MgO is sparingly soluble and weakly alkaline, preventing excessive alkalinity in water.

23
Q

How do simple molecular covalent oxides (P4O10) react with water?

A

P4O10 + 6H2O -> 4H3PO4

24
Q

How do simple molecular covalent oxides (SO2) react with water?

A

SO2 + H2O -> H2SO3

25
Q

Draw the displayed formula for the acids: H2SO4, H2SO3, H3PO4.

A

H2SO4, H2SO3, H3PO4

26
Q

Explain how the basic oxides react with acids.

A

Basic oxides react with acids to form salts and water.

27
Q

Aluminum acting as an amphoteric oxide ionically.

A

Al2O3 + 6HCl -> 2AlCl3 + 3H2O

28
Q

Ionic equations of Period 3 elements reacting to form a salt.

A

Na2O + 2HCl -> 2NaCl + H2O

29
Q

Explain the bonding of Al2O3.

A

Al2O3 is ionic but shows some covalent character.

30
Q

Describe the reaction of sodium with water, including the chemical equation.

A

Sodium reacts vigorously with cold water, forming sodium hydroxide and hydrogen gas. The equation is 2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g).

31
Q

Compare magnesium’s reaction with cold water and with steam.

A

Magnesium reacts slowly with cold water to form magnesium hydroxide, while it reacts readily with steam to produce magnesium oxide and hydrogen gas. The equation for steam is Mg(s) + H2O(g) -> MgO(s) + H2(g).

32
Q

How do Period 3 elements react with oxygen?

A

Period 3 elements react with oxygen to form oxides, characterized by bright flames and the production of white solids or gases.

33
Q

How do the basic oxides of Period 3 react with acids?

A

Basic oxides like Na2O and MgO react with acids to form salts and water.

34
Q

Explain the amphoteric behavior of aluminum oxide.

A

Al2O3 can act as both a base and an acid, reacting with acids and bases.

35
Q

What happens when silicon dioxide reacts with sodium hydroxide?

A

SiO2 + 2NaOH -> Na2SiO3 + H2O

36
Q

Differentiate between the properties of metal and non-metal oxides in Period 3.

A

Metal oxides are ionic, basic, and have high melting points. Non-metal oxides are covalent, acidic, and have lower melting points.

37
Q

Describe the structures of ionic and macromolecular oxides in Period 3.

A

Ionic oxides have giant ionic lattice structures, while macromolecular oxides have giant covalent structures.

38
Q

How can you experimentally demonstrate that certain Period 3 oxides contain ions?

A

By melting the solids and demonstrating that they conduct electricity in the molten state.

39
Q

How does magnesium oxide react with hydrochloric acid?

A

MgO + 2HCl -> MgCl2 + H2O

40
Q

Provide the equations for aluminum oxide acting as both a base and an acid.

A

As a base: Al2O3 + 6HCl -> 2AlCl3 + 3H2O. As an acid: Al2O3 + 2NaOH + 3H2O -> 2NaAl(OH)4.

41
Q

Describe the trend in oxide acidity and basicity across Period 3.

A

Oxides transition from basic to acidic across Period 3. Sodium and magnesium oxides are basic, while phosphorus pentoxide and sulfur trioxide are acidic.

42
Q

Why is magnesium oxide preferred over sodium hydroxide for treating acidification in environments?

A

Magnesium oxide is sparingly soluble and weakly alkaline, preventing excessive alkalinity in water.

43
Q

What are the reactions of non-metal oxides like SO2 and P4O10 with water?

A

SO2 + H2O -> H2SO3 and P4O10 + 6H2O -> 4H3PO4.

44
Q

What is the reaction for sulfur dioxide?

A

l) → H2S + O3 (aq)

This illustrates the behavior of sulfur dioxide as an acidic oxide.

45
Q

What is the reaction for phosphorus pentoxide?

A

P4O10 (s) + 6 H2O (l) → 4 H3PO4 (aq)

This illustrates the behavior of phosphorus pentoxide as an acidic oxide.

Chemistry (18 decks)

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