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Chemistry > Group 7 > Flashcards

Group 7 Flashcards

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1
Q

Properties of Fluorine

A

pale yellow gas, highly reactive

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2
Q

Properties of Chlorine

A

green has, poisonous

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3
Q

What happens to the melting point as you go down the group?

A

Increase

molecules size increases so larger Vanderwalls forces between molecules. This means that more energy is required to break IMF

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4
Q

What happens to oxidising strength of group 7

A

Decrease as you go down

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5
Q

Reaction between chlorine and bromide ions

A

Cl2 (aq) + 2Br– (aq) —–> 2Cl– (aq) + Br2 (aq)

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6
Q

What is the role of nitric acid when testing halide ions?

A

React carbonate to prevent formation of Ag2CO3

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7
Q

Reaction between nitric acid and sodium carbonate

A

2HNO3 + Na2CO3 —> 2NaNO3 + H2O + CO2

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8
Q

Equation and observation: Silver ion and Chloride ion

A

Ag+ (aq) + Cl- (aq) —-> AgCl(s)

white precipitate

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9
Q

Equation and observation: Silver ion and bromide ion

A

Ag+ (aq) + Br- (aq) —-> AgBr(s)

cream precipitate

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10
Q

Equation and observation: Silver ion and iodide ion

A

Ag+ (aq) + I- (aq) —-> AgI(s)

pale yellow precipitate

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11
Q

How to distinguish the silver nitrate reaction?

A

Add dilute ammonia for AgCl —-> for dissolve
Add concentrated ammonia for AgBr —-> for dissolve

AgI is insoluble

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12
Q

What is reducing agent?

A

donate electrons

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13
Q

What happens to reducing agent as you go down the group?

A

Increases

Greater tendency to donate electrons as the ions get bigger so easier to lose electrons

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14
Q

Reaction between sodium fluoride and sulfuric acid + observation

A

NaF(s) + H2SO4(l) —> NaHSO4(s) + HF(g)

white steamy fumers of HF

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15
Q

Reaction between sodium chloride and sulfuric acid + observation

A

NaCl(s) + H2SO4(l) —> NaHSO4(s) + HCl(g)

white steamy fumes of HCl

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16
Q

What does H2SO4 acts as?

A

acid (proton donor)

17
Q

What is the overall sodium bromide and sulfuric acid

A

2NaBr + 3H2SO4 —> 2NaHSO4 + SO2 + Br2 + 2H2O

18
Q

Observation for NaBr and H2SO4

A

white steamy fume of HBr

19
Q

What is disproportionation?

A

Element simultaneously oxidises and reduces

20
Q

Reaction with water + Chlorine in sunlight (

A

2Cl2 + 2H2O —> 4H+ + 4Cl- + O2

21
Q

Chlorine is used in water to….

A

kill bacteria

22
Q

Chlorine with water (ONLY) reversible

A

Cl2(g) + H2O (l) ⇌ HClO (aq) + HCl (aq)

23
Q

Reaction between chlorine and cold dilute NaOH

A

Cl2(aq) + 2NaOH (aq) —> NaCl (aq) + NaClO (aq) + H2O (l)

Chemistry (15 decks)

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