Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry Paper 2 > Topic 8 Chemical Analysis > Flashcards

Topic 8 Chemical Analysis Flashcards

1
Q

What is a pure substance?

A

Single element/compound, not mixed with any other substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What will a chemically pure substance melt and boil at?

A

Specific temperatures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How can you test the purity of a sample?

A

Measuring melting or boiling point, compare with melting or boiling point of pure substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What will impurities in a sample do to the melting point?

A

Lower, increase melting range

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What will impurities in a sample do to the boiling point?

A

Increase, sample may boil at range of temperatures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is a formulation?

A

Mixture designed as a useful product

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How are formulations made?

A

Mixing components in carefully measured quantities to ensure product has required properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are 7 examples of formulations?

A

Foods
Cleaning agents
Paints
Medicines
Alloys
Fertilisers
Fuels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the mobile phase in chromatography?

A

Molecules can move, liquid or gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the stationary phase in chromatography?

A

Molecules can’t move, solid or really thick liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the stationary phase in paper chromatography?

A

Chromatography paper

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the mobile phase in paper chromatography?

A

Solvent (ethanol/water)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What 2 things does the amount of time the molecules spend in each phase in paper chromatography depend on?

A

How soluble they are in solvent
How attracted they are to paper

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What will happen to molecules with higher solubility in solvent and less attracted to paper in paper chromatography?

A

Spend more time in mobile phase, carried further up paper

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the test for hydrogen?

A

Hold lit splint at open end of test tube of gas, hydrogen burns rapidly with pop sound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the test for oxygen?

A

Insert glowing splint into test tube of gas, splint relights in oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the test for carbon dioxide?

A

Bubbling co2 through/shaking co2 with aqueous solution of calcium hydroxide (limewater), turns cloudy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is the test for chlorine?

A

Damp litmus paper put into chlorine gas, litmus paper bleached and turns white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are cations?

A

Positive (metal) ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What are the 2 ways we can test for cations?

A

Flame tests
Sodium hydroxide solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Which 5 metal compounds produce distinctive colours in flame tests?

A

Lithium
Sodium
Potassium
Calcium
Copper

22
Q

What colour flame will copper ions produce?

23
Q

What colour flame will sodium ions produce?

24
Q

What colour flame will calcium ions produce?

A

Orange-red

25
What **colour flame** will **lithium ions produce**?
**Crimson**
26
What **colour flame** will **potassium ions produce**?
**Lilac**
27
What **reagent** can we use to **identify some metal ions (cations)**?
**Sodium hydroxide solution NaOH**
28
What **colour precipitate** will **copper ions produce**?
**Blue**
29
What **colour precipitate** will **magnesium ions produce**?
**White**
30
What **colour precipitate** will **calcium ions produce**?
**White**
31
What **colour precipitate** will **aluminium ions produce**?
**White**, then **dissolves in excess NaOH** to **form colourless solution**
32
What **colour precipitate** will **iron 2+ ions produce**?
**Green**
33
What **colour precipitate** will **iron 3+ ions produce**?
**Brown**
34
How can we **test for sulphate ions**?
**Barium chloride solution** in presence of **dilute hydrochloric acid**
35
What is the **formula** for a **sulphate ion**?
**SO4 2-**
36
What **colour precipitate** will **sulphate ions make** with **acidified barium chloride**?
**White**
37
What is an **anion**?
**Negative ion**
38
How can we **test for carbonates**?
**React with dilute acid** to form **CO2, CO2 identified with limewater**
39
How can we **test for halides**?
**Silver nitrate solution** in presence of **dilute nitric acid**
40
Which **3 halide ions produce precipitates** with **acidified silver nitrate**?
Chloride Bromide Iodide
41
What **colour precipitate** do **chloride Cl- ions make** with **acidified silver nitrate**?
**White**
42
What **colour precipitate** do **bromide Br- ions make** with **acidified silver nitrate**?
**Cream**
43
What **colour precipitate** do **iodide I- ions make** with **acidified silver nitrate**?
**Yellow**
44
What is the **equation to calculate the Rf value**?
**Rf= distance travelled by solvent (B)/ distance travelled by solvent (A)**
45
What is **flame emission spectroscopy an example of**?
**Instrumental method**
46
What can **chemists use to detect and identify elements instead of conducting tests**?
**Instrumental methods (tests that use machines)**
47
What are **3 advantages of using instrumental methods (machines)**?
**Accurate** **sensitive** **Rapid**
48
What can **flame emission spectroscopy be used to identify**?
**Different metal ions in solutions**
49
What are the **5 steps in flame emission spectroscopy**?
1. **Sample** put in **flame** 2. **Ions heat up, electrons excited, electrons** drop back to **original energy levels** 3. **Transfer energy as light** 4. **Light passed through spectroscope** 5. **Detects different wavelengths of light**, produce **line spectrum**
50
Why does **each ion produce a different pattern of wavelengths** and has a **different line spectrum** in **flame emission spectroscopy**?
**Ions** have **different charges** and **electron arrangements, different ions emit different wavelengths of light**
51
What does the **intensity** of the **line spectrum indicate in flame emission spectroscopy**?
**Concentration of ion**
52
What **2 things** can **line spectrums be used to identify in flame emission spectroscopy**?
**Ions in solution** **Calculate concentrations**

Chemistry Paper 2 (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions