Chapter 10 - Group 7 Flashcards

1
Q

why are halogens diatomic

A

because when they are monoatomic, they are highly unstable because they have one unpaired electron

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2
Q

why are halide ionicc compounds more stable than halogens

A

because in ionic compounds the halogen has an electron to fill up its outer shell and make it fully stable, while in a halogen, the halide has to share its electron

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3
Q

whats the difference between halide and halogen

A

halide is an ion, all halides have charge of -1
halogen is the name for the diatomic molecule that all g7 elements form

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4
Q

why are halogens reactive

A

they have only one electron that they need to gain to obtain a full outer shell, so it is much easier for them to become compounds

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5
Q

what is the trend in reactivity down group 7 and why

A

reactivity decreases down the group because the shielding increases so the atomic radius increases so the outermost shell is further from the nucleus so it experiences a weaker attraction so for the element to gain an electron on a further shell it requires more energy

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6
Q

what is the trend in electronegativity down group 7 and why

A

decreases because the shielding increases so atomic radius increases so shared electrons are further from the nucleus so they experience a smaller attraction to the nucleus and are pulled less towards it

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7
Q

what is th emost electronegative elemtn

A

fluorine

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8
Q

how does boiling point (and melting point) change down group 7 and why

A

increases because the sheulding increases so number of eletcons increases so greater surface area so greater van der waals forces

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9
Q

what intermolecular forces do halogens experience

A

only van der waals forces because they are non-polar molecuoles with no ability to form hydrogen bonds

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10
Q

what does F2 look like

A

it is a pale yellow gas

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11
Q

what does Cl2 look like

A

pale green gas

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12
Q

what does Br2 look like

A

Oorange/brown liquid

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13
Q

what does I2 look like

A

black / purple solid

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14
Q

how does oxising power of halogens change down the group

A

it decreases

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15
Q

how does reducing power of halides change down the group

A

it increases

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16
Q

why are chloride ions bad reducing agents

A

because thier atomic radius is so small that they struggle to lose electrons since they experience so much attraction to the nucleus

17
Q

give a general equation for the reaction of a halogen salt with sulfuric acid
what are the observation foir tyhis reaction

A

NaX + H2SO4 —-> HX + NaHSO4
streamy fumes forming

18
Q

give the equation between hydrogen vbromide and sulfuric acid
what rre the observations

A

2H+ + 2Br- + H2SO4 —-> SO2 + 2H2O + Br2
colourless choking gas and brown fumes

19
Q

what is reduced and what is oxidised, and to what, in the reaction between hydrogen bromide and sulfuric acid

A

brinmide ions are reduced to bromine
sulfuric acid is reduced to sulfur dioxide

20
Q

how can you tell that iodide ions are the strongest reducing agesnt

A

sulfur gets reduced from its oxidation state of +6 ibn sulfuric aduic to an oxidation state of -2 in hjydrogen sulfide

21
Q

Give the reaction that takes place between chlorine and water in bright sunlight.

A

2Cl2 + 2H2O —->

22
Q

Why is
HClO
more useful than
HCl
for sterilising pools?

A

The bacteria in the water are killed by oxidation using
HClO

23
Q

Why do outdoor pools require more chlorine to sterilise them than indoor pools?

A

In the presence of sunlight, chlorine reacts with water to form hydrochloric acid and oxygen, in an irreversible reaction. In outdoor pools, there is brighter sunlight, so this reaction happens more rapidly. This causes chlorine to be lost from the pool, meaning less chlorine is available to react with water to form chloric (I) acid, which is the oxidising agent needed to kill bacteria. Therefore outdoor pools require more chlorine to sterilise them than indoor pools.

24
Q

in what conditions will chlorine react with sodium hydroxide to give sodium chlorate (I)

A

it must react with cold and dilute sodium hydroxide

25
Q

give the equation for the reaction between sodium hydroxide and chlorine to give sodium chlorate

A

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