Inorganic Chemistry Flashcards
1
Q
Sodium + water -
A
Sodium hydroxide + hydrogen
2
Q
What are Halogens?
A
Elements in group 7
3
Q
What colour of Chlorine at room temperature?
A
Green gas
4
Q
What is the colour/state change of Bromine at room temperature?
A
Red/brown liquid - orange vapour
5
Q
What is the colour/state change of Iodine when heated?
A
Dark grey crystalline solid - purple vapour
6
Q
How does the atomic number of halogens increasing affect the elements?
A
Elements have darker colour and higher boiling point
7
Q
What is a Displacement reaction?
A
- More reactive element pushes out (displaces) a less reactive element from a compound
- Reduction and Oxidation happens simultaneously
8
Q
Give an Example of a Displacement Reaction using Chlorine Iodine:
A
- Chlorine more reactive than iodine
- Add chlorine water to potassium iodide solution
- Chlorine react with potassium to form potassium chloride
- Iodine displaces from salt and left in sodium, turning it brown
9
Q
How much Nitrogen is in the air?
A
78%
10
Q
How much Oxygen is in the air?
A
21%
11
Q
How much Carbon Dioxide is in the air?
A
0.04%
12
Q
How much Argon is in the air?
A
Nearly 1%
13
Q
How can you determine the percentage of Oxygen on air?
A
- Phosphorus in tube, attach glass syringe at either end
- 1 syringe with air, other empty
- Heat phosphorus - react with oxygen in air to make phosphorus oxide
- Reacts=amount of air in syringes decreases
- Measure starting & final volume of air using scale on syringes
- Calculate percentage of O2 in air = difference in volume / start volume * 100
14
Q
How do you form Magnesium Oxide?
A
Magnesium burns with bright white flame in air and white powder
15
Q
What is the test for Hydrogen Gas?
A
Squeaky pop when burnt
16
Q
How do you make Sulfur Dioxide?
A
Sulfur burns in air or oxygen with pale blue flame
17
Q
What is an Example of Thermal Decomposition of Metal Carbonates?
A
- Heat metal carbonate, get carbon dioxide & metal oxide
- Copper(II)carbonate is green powder, decompose to form carbon dioxide and copper(II)oxide when heated
- CuCO3 - CuO + CO2
18
Q
What is Thermal Decomposition?
A
When substance breaks down into simpler substance when heated
19
Q
How does Deforestation affect amount of Carbon Dioxide in atmosphere?
A
Fewer trees means less CO2 is removed from atmosphere via photosynthesis
20
Q
How does Burning Fossil Fuels affect amount of Carbon Dioxide in atmosphere?
A
Carbon that was locked up in these fuels is being released as CO2
21
Q
How is Increasing Carbon Dioxide linked to Climate Change?
A
- Extra CO2 caused average temp of Earth to increase
* Global warming-climate change - cause flooding, change in rainfall patterns, rising sea levels
22
Q
Acid + Metal -
A
Salt + Hydrogen
23
Q
Metal + Water -
A
Metal Hydroxide + Hydrogen
24
Q
How can you Test for how Reactive Metals are using Acid?
A
- Reactions of different metals with dilute acids
- More reactive = faster reaction
- Very reactive metals (e.g. sodium) react explosively
25
How can you Test for how Reactive Metals are using Water?
* Very reactive metals (e.g. potassium, sodium, lithium) react vigorously with water
* Less reactive metals (e.g. zinc, magnesium, iron) won’t react much with cold water, react with steam
* Copper doesn’t react with water or steam
26
What is the Reactivity series?
| Please Send Lions Cats Monkeys And Crazy Zebras In To Lovely Hot Country’s Signed General Penguin
```
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum
```
27
How do you Prevent Rusting of Iron?
* Painting/coating with plastic
* Oiling/Greasing
* Coating of zinc - zinc oxidised instead of iron
28
Iron + Oxygen + Water -
Hydrated Iron(III)oxide (rust)
29
What is Rusting in Iron?
* Iron In contact with oxygen and water
* Iron corrodes and becomes flakey & soft
* Form hydrated iron(III)oxide
30
What does Copper Oxide form when reduced and what is the Equation?
* Form copper using carbon
| * 2CuO + C - 2Cu + CO2
31
What is a Metal Ore?
* Compound contains enough of metal to make it worthwhile extracting
* Mote reactive metal = harder to extract from compound
32
What are the Common Properties of Iron, Aluminium and Copper?
* Dense, lustrous, high melting points
* Strong and hard to break
* Malleable
* Good conductors of electricity and heat energy
33
What is Iron Used for and its Main Problem?
* Make gates and railings
| * Corrodes easily so rusts
34
What is Aluminium used for?
* Bicycle frames
| * Aeroplanes
35
What is Copper used for?
* Electrical compounds and wiring - has low resistance so efficient at transferring electricity
* Heating systems (underfloor heating) - speedy transfer of heat to surroundings
36
How are Alloys made?
* Adding other elements to the metal (metals or carbon)
| * Harder than pure metals - new atoms distort layers of metal ions - difficult for them to slide over each other
37
What is the pH for Acids and colour (universal indicator)?
* pH 0-7
| * Red - orange
38
What is pH for a neutral substance and colour (universal indicator)?
* pH 7
| * Green
39
What is pH for Alkaline’s and colour (universal indicator)?
* pH 8-14
| * Blue - purple
40
What colour is Acid if Methyl Orange Indicator is added?
Red
41
What colour is Alkaline if Methyl Orange Indicator is added?
Yellow / orange
42
What colour is Acid if Litmus paper is added?
Red
43
What colour is Alkaline if Litmus paper is added?
Blue
44
What colour is Neutral substance if Litmus paper is added?
Purple
45
What colour is Acid if Phenolphthalein is added?
Colourless
46
What colour is Alkaline if Phenolphthalein is added?
Bright pink
47
What is an Acid?
* Source of Hydrogen ions (H^+)
| * Proton donors
48
What is a Base?
* Substance that can neutralise an acid
| * Proton acceptors
49
What is an Alkali?
* Source of hydroxide ions (OH^-)
| * Soluble bases
50
What is Neutralisation and its Formula?
* Reaction between acid and base (alkali)
| * H^+ + OH^- - H20
51
Acid + Base -
Salt + Water
52
Acid + Ammonia-
Ammonium Salt
53
Acid + Metal Carbonate -
Salt + Water + Carbon Dioxide
54
Acid + Metal Hydroxide-
Salt + Water
55
Acid + Metal Oxide -
Salt + Water
56
What is Titration used for?
Find out exactly how much acid is needed to neutralise a quantity of alkali (vice versa)
57
How do you do a Titration?
* Pipette alkali into conical flask
* Add few drops of indicator
* Put Acid onto burette
* Measure volume - initial reading
* Add acid to alkali from burette
* Indicator changes colour when all alkali is neutralised (e.g. phenolphthalein - pink to colourless)
* Record volume of acid to neutralise alkali
* Repeat until concordant results
58
How do you make Insoluble Salts and give and example?
* Use precipitation reaction
* Pick 2 soluble salts and react together to get insoluble salt
* E.g. lead nitrate + magnesium sulfate = lead sulfate (insoluble)
59
What Substances are Soluble?
* Nitrates
* Common Salts of sodium, potassium, ammonium
* Common Chlorides (not silver/lead chloride)
* Common Sulfates (not lead, barium, calcium sulfate)
60
What Substances are Insoluble?
* Common Carbonates (not sodium,potassium,ammonium)
| * Common Hydroxides (not sodium,potassium,calcium)
61
Flame test for Lithium (Li^+):
Bright red flame
62
Flame test for Sodium (Na^+):
Orange flame
63
Flame test for Potassium (K^+):
Lilac flame
64
Flame test for Calcium (Ca^2+):
Brick red flame
65
Flame test for Magnesium (Mg^2+):
No colour
66
Flame test for Copper (Cu^2+):
Green flame
67
How do you do the Flame Tests?
* Platinum wire loop dipped in dilute HCl, hold in flame
| * Dip it In sample you want to test then place in Bunsen burner
68
What are Metal Hydroxides:
* Insoluble
| * Precipitate forms out of solution
69
How can you Test for Ammonia Gas?
* Damp red litmus paper
| * Ammonia present = paper turn blue
70
What Colour Precipitate does Chloride Ion give?
White precipitate
71
What Colour Precipitate does Bromide Ion give?
Cream precipitate
72
What Colour Precipitate does Iodide Ion give?
Yellow precipitate
73
What do you use to Test for Halides?
Cl^-/Br^-/I^- with Nitric Acid and Silver Nitrate
74
What is the Test for Carbonates?
* Add dilute hydrochloric acid (HCl)
| * If carbonates present = CO2 released
75
What is the Test for Sulfates?
* Add dilute hydrochloric acid (HCl) with barium chloride solution (BaCl2)
* White precipitate of barium sulfate = original compound was sulfate
76
What is Test for Chlorine?
Bleaches damp blue litmus paper, turning white
77
What is Test for Oxygen?
Relights a glowing splint
78
What is Test for Carbon Dioxide?
Turns limewater cloudy
79
What is the Test for Hydrogen?
Makes a squeaky pop with lighted splint
80
What is the Test to see if Water is Present?
* Add anhydrous copper(II)sulfate
| * If white powder turn blue - water present
81
How do you make Lead Sulfate?
* Add 1 spatula of lead nitrate to test tube, add water to dissolve
* Add 1 spatula of magnesium sulfate to another test tube, add water to dissolve
* Put both solutions into beaker, stir, lead sulfate precipitate out
* Pour contents into filter paper, rinse contents so all magnesium nitrate gone
* Scrape lead sulfate onto paper, dry in oven
82
How do you make Soluble Salts?
* Reacting acid (contains 1 ion you want in salt) with insoluble base (contains other ion you need)-usually metal oxide/hydroxide
* Reacting acid with an alkali - titration using indicator
83
How do you Make Soluble Salts using Acid and Insoluble Base?
* Heat acid in water bath
* Add base, produces soluble salt and water
* Filter excess solid to get solution with salt and water
* Heat solution gently, evaporate some water, cool and salt crystallises
* Filter off solid and leave to dry
84
How do you make Soluble Salts using Acid/Alkali Reactions?
* Measure out acid using pipette
* Add few drops of indicator
* Add alkali
