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Chemistry🧪 > IO1: Inorganic > Flashcards

IO1: Inorganic Flashcards

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1
Q

In terms of the periodic table, where are the blocks found?

A

s- left
d- middle
p- right
f- bottom

(outer electrons in these orbitals)

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2
Q

Do groups or periods have similar chemical properties?

A

Groups

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3
Q

Periods are arranged…

A

Periodically, as they have repeating patterns or periodic trends

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4
Q

In terms of the periodic table, where are metals and non-metals?

A

Metals- left and middle until the…
Metalloids- diagonal B, Si, As, Te, At, separates metals and non-metals
Non-metals- right

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5
Q

What is a metalloid?

A

Show some chemical properties of a metal, but is not a metal.

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6
Q

What is the trend in atomic radius of group 2?

A

Increases down

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7
Q

What is the trend in 1st ionisation energy of group 2?

A

Decreases down

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8
Q

How do the group 2, alkaline earth metals bond?

A

Metallically

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9
Q

What state are the group 2 metals at room temp?

A

Solid

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10
Q

What is the trend in melting point of group 2 metals?

A

Decreases down

-Metallic bonds get weaker
-Apart from Magnesium, which is lower than all group 2 metals

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11
Q

How do the group 2 metals react with water?

A

Going down, each reacts more vigourously.

-This is because 1st IE decreases down the group, so easier to lose electrons (decrease activation energy)

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12
Q

Which group 2 metal does not react with water?

A

Be

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13
Q

How does Mg react with water?

A

Only slightly, but does rapidly react with steam and gives off a bright light.

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14
Q

Group 2 + water =?

A

Metal Hydroxide

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15
Q

Magnesium can be used to extract Ti from its ore, explain how.

A
  1. TiO2 is heated with carbon and chlorine to form titanium chloride
  2. Reduced by Mg where Mg donates its electrons to Ti, making Ti and magnesium chloride.

Mg= reducing agent

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16
Q

How is calcium used to prevent acid rain?

A

Burning fossil fuels gives off SO2 which causes acid rain.

-Spraying ‘slurry’ of calcium carbonate, or calcium oxide over sulfur dioxide gas, and collects the calcium sulfide that forms.

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17
Q

What is the solubility of Group 2 Hydroxides?

A

Increases down the group

Magnesium hydroxide is hardly soluble, so is a white precipitate

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18
Q

What group 2 hydroxide can be used to cure heartburn and why?

A

Magnesium Hydroxide- Mg(OH)2

-Base is strong enough to neutralise the pH of stomach
-Low solubility means it is not strong enough to damage body.

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19
Q

What group 2 hydroxide neutralises soil?

A

Calcium hydroxide - Ca(OH)2

-‘slaked lime’
-strong base to neutralises pH

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20
Q

Hydroxide solubility increases, sulfate solubility…

A

Decreases

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21
Q

What is Barium sulfate used for and why?

A

(Barium Meal)

Consumed before an X-ray as it insoluble but dense.

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22
Q

What is Barium Chloride used for?

A

To test for sulfate ions.

-When acid is added to removes carbonate, forms a white precipitate.

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23
Q

Are group 7 Halogens reactive?

A

Very

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24
Q

Halogen + metal =?

A

Salts

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25
What is a halide?
When halogens gain an electron and become ions e.g chloride, fluoride
26
What is fluorine at room temp?
Pale yellow gas
27
What is chlorine at room temp?
Green gas
28
What is bromine at room temp?
Red/brown liquid
29
What is iodine at room temp?
Black or dark grey solid
30
What is astatine at room temp?
Black or dark grey solid
31
All halogens form ______ molecules
Diatomic
32
What is the trend in electronegativity of group 7 and why?
Decreases down -More full shells, increases shielding, increases atomic radius, electron pair is further away from nucleus -This outweighs increase in nuclear charge.
33
What is the trend in boiling point of group 7?
Increases down -More mass, electrons, size, surface area -Stronger VDW forces -More energy needed to overcome forces
34
Describe the oxidising ability of halogens
Decreases down, fluorine being the best -tend to gain an electron (halides) -oxidising agents in redox, become 1- ions. -in a displacement reaction, fluorine will always displace another halogen.
35
Describe the reducing ability of Halides
Increases down the group, iodide the best
36
Discuss the reducing ability of NaBr with sulphuric acid
Acid-base reaction= HBr, a steamy gas Redox reaction= Br2, a brown steamy gas
37
Discuss the reducing ability of NaI with sulphuric acid
Acid-base reaction= HI, steamy fumes Redox reaction= H2S, yellow solid or rotten eggs smell, or I2, dark grey solid
38
What would you use to identify halides?
Silver nitrate
39
What happens to the halides when silver nitrate is added to them dissolved in water?
F- = no ppt (soluble) Cl- = white ppt Br- = cream ppt I- = pale yellow ppt become silver fluoride...
40
If the halide has impurities, what can you react it with?
Dilute nitric acid -gets rid of carbonates and forms CO2 and H2O
41
What are the further tests to adding silver nitrate to halides, that help us identify?
Dilute ammonia: Cl- = colourless Br- = cream I- = pale yellow Concentrated ammonia: Cl- = colourless Br- = colourless I- = pale yellow
42
Cl2 + water =?
Dissociates to form Cl- ions, forming either: HCl (hydrochloric acid) HClO ( chloric 1 acid) -a disproportionation reaction
43
What does HClO dissociate to and how is it useful?
H+ and ClO- ClO- (chlorate ion) is an oxidising agent that is toxic and will kill bacteria (used in chlorination).
44
What are the pros and cons of chlorination?
+Kept at harmless concs +Saved millions of lives -Toxic -Wasteful (only 1% of water we drink)
45
Write the chemical equation for the disproportionation of chlorine and water
Cl2 + H2O <> HCl + HClO <>= reversible reaction
46
What happens when sunlight is a factor in the chlorine + water reaction?
Produces HCl + O2 There is no HClO to kill bacteria, a problem in pools
47
Bleach is an oxidising agent, how is it formed?
Chlorine + cold, dilute sodium hydroxide forms NaClO
48
What happens to the atomic radius across period 3 and why?
Decreases More protons in the nucleus, an electrostatic attraction to electrons, pulling them in, decreasing size.
49
Describe the trend in First ionisation energy across period 3.
Increases across, due to increase in nuclear charge. Dip between Mg and Al: electrons start to fill the p-sub shell in Al, so a small increase in shielding, less energy to remove an electron. Dip between P and S: in group 5, each p sub unit has one electron in it but in group 6 there is 2, so spin pair repulsion occurs, already repel each other making it easy to remove.
50
What is the bonding of the period 3 elements?
Na, Mg, Al: metallic Si: Giant covalent lattice (metalloid) P, S, Cl: covalent
51
Describe the trend in melting points for metals of period 3
Melting point increases going across as the metal cations have a higher charge, so number of delocalised electrons increases, more electrostatic attraction, higher temps needed.
52
Describe the covalent bonding in silicon
-Can bond to any number of other silicon atoms, so can make a giant covalent lattice -A macromolecule
53
What molecule does phosphorus go around as?
P4
54
Describe the trend in melting points of the non-metals in the period 3 elements
Highest: Silicon- giant covalent lattice, strong bonds Sulphur- simple molecule, more VDW due to size Phosphorus- less VDW Chlorine- even less VDW Argon- no molecules Lowest
55
What molecule does sulphur go around as?
S8
56
What trend can we/ can not generalise to other periods?
Can: -Atomic radius -1st IE Cannot: -Melting points
57
What reaction proves group 7s oxidising ability?
Displacement More reactive halogen (better oxidising agent) takes the place of a less reactive halide ion (better reducing agent)
58
Explain how to do the displacement reactions to prove group 7s oxidising ablilities
Chlorine water with... NaCl - colourless NaBr- orange/yellow NaI- Brown
59
How do you prove the reducing abilities of group 7?
React with sulphuric acid (H2SO4)
60
Explain how to do the reaction with group 7 and sulphuric acid to prove reducing ability
Conc H2SO4 with... NaCl - misty white fumes NaBr- misty white, or orange fumes NaI- misty white, or grey solid/ rotten eggs smell

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