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Chemistry > 3.2 Inorganic Chemistry > Flashcards

3.2 Inorganic Chemistry Flashcards

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1
Q

Why does melting point decrease down group 2?

A

•metal ions will get bigger but 2e- delocalised
•larger ionic radius, further the e- are from the +ve nuclei so less attraction
•less energy needed to break metallic bonds

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2
Q

What forms when group 2 metals react with water? (+reactivity)

A

M(OH)2 + H2
Reactivity increases down the group as ionisation energy decreases so e- lost easily

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3
Q

What happens to the solubility of group 2 with sulfates?

A

Solubility decreases down the group, where BaSO4 is insoluble

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4
Q

What happens to the solubility of group 2 with hydroxide?

A

Increase solubility down the group, where Mg(OH)2 is sparingly soluble (least soluble)

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5
Q

What are Ca(OH)2 and Mg(OH)2 used for?

A

•Ca(OH)2 is used in agriculture to neutralise acid soils
•Mg(OH)2 is used as antacids that neutralise excess stomach acid

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6
Q

What is BaSO4 used for and how is it tested?

A

•Barium meals= coats tissues, and show up on X-rays so organ structures can be seen. (Diagnose problems)
•add HCl to remove carbonate impurities and then add BaCl2 = white precipitate of BaSO4 forms

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7
Q

How is Mg used in the extraction of Ti from TiCl4?

A

Reduced by Mg in a furnace at around 1000•C
TiCl4 + 2Mg = Ti + 2MgCl2

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8
Q

What are the uses of CaO and CaCO3?

A

•slurry formed by mixing them with water
•sprayed onto flue gas= SO2 reacts with alkaline slurry and makes CaSO3 (calcium sulfite)

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9
Q

What happens to the boiling point down group 7?

A

Increases as they become larger molecules (more e-) so more stronger van der waals

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10
Q

What happens to electronegativity down group 7?

A

Decrease as more shielding and so less attraction between the nucleus and the shared pair of electrons in the covalent bond

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11
Q

How are halides tested for? (AgNO3)

A

•add nitric acid to remove ions (OH-/CO3 -2) that give ppt
•add silver nitrate
= AgCl: white precipitate
AgBr: cream
AgI: yellow

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12
Q

How are halides tested for? (NH3 solution)

A

•Cl- dissolves in dilute + conc. NH3
•Br- dissolves in conc. NH3 only
•I- is insoluble in conc. NH3

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13
Q

What happens to the oxidising power down group 7?

A

Ability to gain e- is reduced as more shielding so less attraction between nucleus and outer shell. Hence they are less reactive and can be displaced by halogens above.

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14
Q

What happens to the reducing power (of halides) down group 7?

A

•to reduce something they must lose an e-
•more shielding and bigger ions so e- is lost more easily as less attraction between nucleus and outer e-

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15
Q

What forms when sodium (fluoride/chloride) is added to conc. H2SO4? (Reducing power)

A

•HF/HCl (misty fumes)
•NaHSO4

*weak reducing agents
*not redox

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16
Q

What forms when NaBr is added to conc. H2SO4? (Reducing power)

A

1) •NaHSO4 + HBr
2) 2NaBr + 2HSO4 = Na2SO4 + Br2 + SO2 + 2H2O
Br2 = orange fumes

*stronger reducing agent
*redox reaction occurs

17
Q

What forms when NaI is added to conc. H2SO4? (Reducing power)

A

1) NaHSO4 + HI
2) 2HI + HSO4 = I2 + SO2 + H2O
3) 8HI + H2SO4 = H2S + 4I2 + 4H2O
H2S: toxic gas

*strongest reducing agent
*solid I2 made

18
Q

What is the reaction between chlorine and water that forms chlorate(I) ions? (+type of reaction)

A

Cl2 + H20 = HClO + HCl
ClO- : kills bacteria, prevents algae growth

•disproportionation: Cl2 is both oxidised and reduced

19
Q

How does the reaction between chlorine and water that forms oxygen occur?

A

2Cl2 + 2H20 = 4H+ + 4Cl- + O2

In the presence of sunlight

20
Q

What are the risks of adding Cl2 to water and why is it still added?

A

• Cl2 has irritates respiratory system when breathed in
• liquid Cl2 can cause chemical burns to skin/eyes
•Cl2 can react with compounds to form chlorinated hydrocarbons = many are carcinogens

BUT benefits outweigh the risks

21
Q

How is bleach made and what does the NaOH reactant have to be?

A

2NaOH + Cl2 = NaClO + NaCl + H2O
ClO- kills bacteria
• NaOH = cold, dilute and (aq)

22
Q

How is a flame test carried out?

A

•dip nichrome wire loop in conc. HCl
•dip loop in solution
•hold loop in blue flame of Bunsen burner

Na: yellow
Ba: pale green
Sr: red
Ca: brick red

23
Q

What is the ppt. Made when cations are tested with NaOH?

A

Mg: white ppt
Ca: slight white ppt
Sr: slight white ppt.
Ba: no change

24
Q

How do you test for ammonium ions?

A

Warm compound with NaOH, which forms NH3 gas. Damp, red litmus paper will turn red

25
Q

What are the reactions of period 3 metals and water?

A

• 2Na + 2H2O = 2NaOH + H2
Na reacts vigorously with cold water
•Mg + H2O = Mg(OH)2 + H2
Mg reacts very slowly with cold water

26
Q

What is the reaction between Mg and steam (H20 (g))?

A

Mg + H2O (g) = MgO (s) + H2

27
Q

What are the reactions of period 3 elements with oxygen and what is observed?

A

•4Na + O2 = 2Na2O (s) *yellow flame, white solid
•2Mg + O2 = 2MgO (s) *bright white light, white solid
•4Al + 3O2 = 2Al2O3 (s) *bright white light, white powdery solid= Al2O3 is corrosion resistant
•Si + O2 = SiO2 (s) *bright white light only at very high •C
•P4 + 5O2 = P4O10 (s) *bright white light, white solid
•sulfur burns in oxygen and produces blue flame

28
Q

What is the trend in melting point of period 3 oxides?

A

•Na2O < MgO = both ionic but Mg2+ is small + highly charged
•Al2O3 has both ionic + covalent which reduces m.p =Al3+ are able to distort the charge cloud of O2-
•SiO2 is a giant covalent molecule
•P4O10>SO3>SO2 = they are simple molecules with weak van der waals between molecules

29
Q

Which period 3 oxides are insoluble and why?

A

Al2O3 and SiO2 as bonding in them are too strong and ions cannot be separated

30
Q

Why are Na2O and MgO basic and which one is stronger?

A

They are both soluble in water and can release OH-. As NaOH is more soluble it can release more OH- so higher Ph
•act as Bronsted Lowry bases= proton acceptors

31
Q

Give the reactions of the acidic period 3 oxides when dissolved in water

A

•P4O10 (s) + 6H2O = 4H3PO4 (aq)
•SO2 (g) + H2O = H2SO3 (aq)
•SO3 (g) + H2O = H2SO4 (aq)

32
Q

Why is SiO2 classified as an acidic oxide even though it is insoluble?

A

•will react with very concentrated alkali
•SiO2 (s) + 2NaOH (aq) = Na2SiO3 (aq) + H2O (l)

33
Q

Show Al2O3 being amphoteric

A

•acts as a base
Al2O3 (s) + 6H+(aq) = 2Al3+ (aq) + 3H2O (l)
•acts as an acid
Al2O3 (s) + 2NaOH (aq) = 2NaAl(OH)4 + 3H2O (l)

Chemistry (3 decks)

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