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Chemistry by Thaidz > Chemistry of the Elements > Flashcards

Chemistry of the Elements Flashcards

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1
Q

Describe group 0

A

noble gases are inert, colourless gases

have a full outer shell so no need to react

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2
Q

Describe what happens when group 1 elements with water

A

react vigorously, producing a metal hydroxide solution
the solution is alkaline, and also produces hydrogen
Group 1 + water —– Group 1 hydroxide + hydrogen

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3
Q

Describe what happens when Lithium reacts with water

A

fizzes slightly for 30s

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4
Q

Describe what happens when Sodium reacts with water

A

fizzes for 20s may ignite

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5
Q

Describe what happens when Potassium reacts with water

A

lilac flame for 5s sometimes explodes

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6
Q

Why do atoms in group 1 react easier as you go down the group ?

A

only 1 electron in their outer shell - want to react
going down, outer electron gets further from nucleus
attraction from outer electron and nucleus decrease

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7
Q

Describe halogens as you go up / down the group

A

Group 7
as you go down: darker colour and higher boiling point
as you go up: more reactive as missing electron is nearer to nucleus so electrostatic force is greater

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8
Q

Chlorine :
colour -
physical state (RT) -
boiling point -

A

Chlorine :
colour : green
physical state (RT) : gas
boiling point : -34

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9
Q

Bromine :
colour -
physical state (RT) -
boiling point -

A

Bromine :
colour - red / brown
physical state (RT) - liquid
boiling point - 59

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10
Q

Iodine :
colour -
physical state (RT) -
boiling point -

A

Iodine :
colour - dark grey
physical state (RT) - solid
boiling point - 185

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11
Q

Describe dissociation

A

Hydrogen Chloride (HCl) is a gas and dissociates in water, splitting into H+ and Cl- ions, this is dissociation
the solution formed is hydrochloric acid (acid)
testing the solution with litmus paper will make it red

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12
Q

Describe dissociation in methylbenzene

A

HCl does not dissociate in methylbenzene
no H+ ions means it is not acidic
testing the solution with litmus paper will stay blue

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13
Q

what is a displacement reaction ?

A

more reactive element displaces (pushes out) a less reactive element from a compound
involves transfer of electrons

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14
Q

Describe halogen displacement reactions

A

Halogens take part in displacement reactions
higher up in group 7 - more reactive
this will sometimes change the colour of solution

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15
Q

Give an example of a halogen displacement reaction

A

chlorine is more reactive than iodine
chlorine water + potassium iodide solution
chlorine react with potassium to form potassium chloride, iodine left over changing solution brown

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16
Q

Give an experiment for halogen displacement

A

add a few drops of halogen solution to salt solution

look for colour change

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17
Q

what is the name for loss of electrons ?

A

oxidation

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18
Q

what is the name for gain of electrons ?

A

reduction

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19
Q

what is an oxidising agent ?

A

receives electrons (gain) and gets reduced

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20
Q

what is a reducing agent ?

A

gives electrons (loss) and gets oxidises

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21
Q

what is a redox reaction ?

A

reaction with both oxidation and reduction recurring

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22
Q

acid + metal —

A

salt + hydrogen

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23
Q

Metal + Water —

A

Metal Hydroxide + Hydrogen

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24
Q

(less reactive metal + steam —

A

Metal oxide + Hydrogen)

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25
Q

Describe some metals reacting with water

A

sodium, lithium and potassium react vigorously
magnesium, zinc and iron won’t react with water, but will react with steam
Copper won’t react with water or steam

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26
Q

state the reactivity series

A

Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Zinc, Iron, Copper, Silver, Gold

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27
Q

how does rust occur ?

what type of reaction is this?

A

iron rusts when it is in contact with oxygen and water

oxidation reaction as iron gains oxygen (iron oxide)

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28
Q

state the equation for rust

A

iron + oxygen + water — hydrated iron(III) oxide

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29
Q

what are the 2 main ways of preventing rust

A

barrier method

sacrificial method

30
Q

describe the barrier method for rust

A

paint/coat with plastic - ideal for structures

oil/grease - used on moving parts like bike chains

31
Q

describe the sacrificial method for rust

A

place a more reactive metal with iron so water/oxygen get sacrificial metal instead
zinc is often used, spraying a coat of zinc is called galvanising, or big blocks can be bolted to the iron

32
Q

What are the gas percentages in the air ?

A

78% nitrogen
21% oxygen
1% argon
0.04% carbon dioxide

33
Q

what happens when an element burns in the air ?

A

it reacts with the oxygen to form an oxide

these oxides can either have acid or base character

34
Q

Describe magnesium burnt in air

what is formed?

A

burns bright white flame
white powder formed (magnesium oxide)
magnesium oxide slightly alkaline dissolved in water

35
Q

Describe Carbon burnt in air

what is formed?

A

will burn in air if very strongly heated
orange/yellow flame and produces carbon dioxide
carbon dioxide is slightly acidic dissolved in water

36
Q

Describe sulfur burnt in air

what is formed?

A

pale blue flame
produces sulfur dioxide
sulfur dioxide is acidic when dissolved in water

37
Q

when do you use upward delivery ?

A

collect gasses light that air

38
Q

when do you use downward delivery ?

A

collect gasses heavier than air

39
Q

Describe the use for carbon dioxide in fizzy drinks

A

CO² is slightly soluble in water and dissolves into drink under pressure,as CO² is acidic (slightly) it creates a carbonic acid
bubbles in fizzy drinks are CO² escaping

40
Q

Describe the use for carbon dioxide in fire extinguishers

A

CO² is denser than air so sinks onto flames and stops oxygen getting to it (suffocates)
CO² fire extinguishers used when water isn’t safe (electrical fires)

41
Q

Why is Carbon dioxide a problem in the atmosphere?

A

gases in atmosphere like CO² and methane act as an insulating layer, absorbing the heat radiated back from earth, and radiates it back
more CO² is being released than removed

42
Q

How is human activity affecting CO² concentration in the atmosphere ?

A

deforestation - fewer trees means less CO² removed via photosynthesis
burning fossil fuels - carbon in fossil fuels released as CO²

43
Q

How is carbon dioxide linked to global warming ?

A

correlation between temperature of earth and concentration of CO²
global warming is a type of climate change
causes flooding due to ice caps melting

44
Q

Describe the sodium flame test

A

yellow-orange flame

45
Q

Describe the potassium flame test

A

lilac flame

46
Q

Describe the calcium flame test

A

brick-red flame

47
Q

How do you test for a cation?

A

clean a platinum wire loop in dilute HCl and hold in flame, once it burns without any colour then dip in sample and put in flame, observing colour

48
Q

are (most) metal hydroxides soluble or insoluble?

A

metal hydroxides are insoluble

49
Q

Copper (II) + Sodium hydroxide (NaOH)

Colour of precipitate:

A

Copper (II) + Sodium hydroxide (NaOH)

Colour of precipitate: blue

50
Q

Iron (II) + Sodium hydroxide (NaOH)

Colour of precipitate:

A

Copper (III) + Sodium hydroxide (NaOH)

Colour of precipitate: green

51
Q

Iron (III) + Sodium hydroxide (NaOH)

Colour of precipitate:

A

Iron (III) + Sodium hydroxide (NaOH)

Colour of precipitate: reddish brown

52
Q

Ammonium + Sodium hydroxide (NaOH)

A

produces ammonia gas, gives off pungent smell

ammonium is colourless

53
Q

state the test for ammonia gas

A

use damp piece of red litmus paper
if turns blue, ammonia is present
ammonia gives off pungent smell

54
Q

How do you test if substance contains ammonium ions ?

A

add some sodium hydroxide (NaOH) to substance
If ammonia gas given off, ammonium ions present
(damp red litmus paper turns blue)

55
Q

what is anion ?

A

a negatively charged ion

56
Q

state the test for carbonates

A

add dilute HCl to test sample

If carbonates present, CO² given off

57
Q

state the test for sulfates

A

sulfate ions produce a white precipitate
add HCl followed by barium chloride, white precipitate of barium sulfate means original compound was a sulfate (HCl added to rid any traces of carbonate or sulfite ions as these would produce a precipitate)

58
Q

state the test for Halides (Cl, Br, I)

A

add dilute nitric acid, followed by silver nitrate solution
(acid used to rid carbonate or sulfite ions)
observe colour

59
Q

Describe the halide test for Chlorine + silver nitrate

A

gives white precipitate of silver chloride

60
Q

Describe the halide test for Bromine + silver nitrate

A

gives a cream precipitate of silver bromide

61
Q

Describe the halide test for Iodine + silver nitrate

A

gives a yellow precipitate of silver iodide

62
Q

State the test for chlorine

A

bleaches (turns white) damp litmus paper

63
Q

State the test for oxygen

A

place glowing splint by test tube, splint will relight if oxygen present

64
Q

State the test for CO²

A

CO² turns lime water cloudy - bubble gas through a test tube of time water

65
Q

State the test for hydrogen

A

hydrogen makes a squeaky pop with a lit splint

noise is hydrogen burning with oxygen in air to form H²O

66
Q

State the test for water

A 
Anhydrous Copper (II) sulfate is white 
Hydrated Copper(II) sulfate is blue 
add anhydrous copper (II) sulfate to sample, will turn blue if water is present
67
Q

State the test for pure water

A

pure water will always : boil at 100°C

freeze at 0°C

68
Q

Flame test for Lithium

A

Crimson red flame

69
Q

Calorimetry example (not combustion)

A

Add acid to polystyrene cup, record temp
add base to measuring cylinder, record temp
add base to acid and stir
record temp every 30s and find highest temp
(surround cup with cotton wool and put lid)

70
Q

Calorimetry example (combustion)

A

50g of water in metal (copper) can and record temp
weigh spirit burner and lid
light and hold under can until 50 degrees
measure final temp (water)
weigh spirit burner and lid
(use draught excluder)

Chemistry by Thaidz (5 decks)

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