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Module 8 - Chemical Synthesis and Design HSC

Total questions: 70

Worksheet time: 55mins

Name
Class
Date
1.

What is the best way to identify whether a solution contains barium ions or calcium ions?

a)

Add chloride ions to the solution: barium will precipitate but calcium will not.

b)

Add carbonate ions to the solution: barium will precipitate but calcium will not

c)

Do a flame test: barium produces a scarlet flame and calcium a blue/green flame

d)

Do a flame test: barium produces a pale green flame and calcium a brick red flame

2.

It is suspected that a stream is contaminated with metal ions. A sample of water from the stream was analysed.

The results of some tests on the sample are recorded in the table.

What is the most likely contaminant in the water?

a)

Ba2+

b)

Ca2+

c)

Cu2+

d)

Fe3+

3.

A diagram of an atomic absorption spectrophotometer is shown. What is the purpose of the hollow cathode lamp?

a)

To excite the sample

b)

To atomise the sample

c)

To produce white light

d)

To produce light of specific wavelengths

4.

A section of the emission spectrum of a mercury lamp is shown. Light at 623.4 nm and 615.2 nm from the mercury lamp was passed through a sample of water containing mercury, and the intensities were then measured by a detector.


I (x nm) = Intensity of light at a wavelength of x nm from the lamp

Id (x nm) = Intensity of light at a wavelength of x nm at the detector


Which of the following pairs of intensities can be used in the determination of the amount of mercury in the water sample using atomic absorption spectroscopy (AAS)?

a)

I (615.2 nm) and Id (615.2 nm)

b)

I (615.2 nm) and Id (623.4 nm)

c)

I (615.2 nm) and I (623.4 nm)

d)

Id (615.2 nm) and Id (623.4 nm)

5.

All the lead ions present in a 50.0 mL solution were precipitated by reaction with excess chloride ions. The mass of the dried precipitate was 0.595 g.


What was the concentration of lead in the original solution?

a)

8.87 g L–1

b)

10.2 g L–1

c)

11.9 g L–1

d)

16.0 g L–1

6.

The diagram shows the infrared spectrum of a compound.


Which compound was analysed?

a)

Butane

b)

Propanol

c)

Propanal

d)

Butanoic Acid

7.

A colorimeter was used to calculate the percentage of iron in a 0.200 gram tablet. The tablet was dissolved and oxidised, then reacted with thiosulfate according to the equation: Fe3+(aq) + SCN–(aq) --> [FeSCN]2+(aq) .


The resulting solution was made up to 200 mL with distilled water. The absorbance of the final solution was measured to be 0.6105 .


The calibration curve shows the absorbance of various concentrations of Fe3+.


How much iron was in the tablet?

a)

1.10 × 10–5 g

b)

5.50 × 10–5 g

c)

6.14 × 10–4 g

d)

3.07 × 10–3 g

8.
Which of the following type of electromagnetic radiation affects the bonds,vibrating ,stretching rocking...
a)
infrared
b)
ultraviolet
c)
microwaves
d)
radiowaves
9.
Which of the following type of electromagnetic radiation affects spin of the nucleons
a)
infrared
b)
ultraviolet
c)
microwaves
d)
radiowaves
10.
The number of peaks in 13C NMR  for CH3 CH2 CH3 is
a)
0
b)
1
c)
2
d)
3
11.
The number of peaks in 1H NMR  for CH3 CH2 CH3 is
a)
0
b)
1
c)
2
d)
3
12.
The splitting pattern for the Hydrogen on the middle carbon in high resolution 1H NMR  for CH3 CH2 CH3 is
a)
a sextet
b)
a heptet
c)
a triplet
d)
a quartet
13.
The splitting pattern for the Hydrogen on the carbon at the end in high resolution 1H NMR  for CH3 CH2 CH3  
a)
a sextet
b)
a heptet
c)
a triplet
d)
isa quartet
14.
Which of the following would be different  for 1-butanol and
 2-butanol
a)
The number of peaks on low res H NMR
b)
the molar mas
c)
the number of peaks in C NMR
d)
the finger print region of the infrared spectrum
15.
NMR is used to determine
a)
the function groups present in inorganic molecules
b)
the molar mass of the compound
c)
the structure of the molecule
d)
the number of different carbon or hydrogen enviroments in the molecule
16.

What is the molecular weight of this compound?

a)

29

b)

87

c)

54

d)

15

17.

The infrared spectrum of an organic compound is shown.


Which compound produces this spectrum?

a)

butanone

b)

ethanol

c)

pent-2-ene

d)

propanoic acid

18.

Which compound gives this infrared spectrum?

a)

1-bromobutane

b)

butan-1-ol

c)

butanal

d)

butanoic acid

19.

Which of these infrared spectra could represent a carboxylic acid?

a)
b)
c)
d)
20.

This question is about the reaction between propanone and an excess of ethane-1,2-diol, the equation for which is given.


In a typical procedure, a mixture of 1.00 g of propanone, 5.00 g of ethane-1,2-diol and 0.100 g of benzenesulphonic acid, C6H5SO3H, is heated under reflux in an inert solvent. Benzenesulphonic acid is a strong acid.


The products would not have an absorption in the infra-red at

a)

1050 cm−1

b)

1720 cm−1

c)

2950 cm−1

d)

3400 cm−1

21.

Which one of the following statements about but-2-enal, CH3CH=CHCHO, is not true?

a)

It has stereoisomers.

b)

It shows a strong absorption in the infra-red at about 1700 cm−1.

c)

It will turn an acidified solution of potassium dichromate(VI) green.

d)

It can be dehydrated by concentrated sulphuric acid.

22.
A molecule absorbs IR at a wavenumber of 1720 cm-1.  Which functional group could account for this absorption.
I. aldehydes
II. esters
III. ethers
a)
I only
b)
I and II 
c)
I, II and III 
d)
none of the above
23.
Identify the bonds which will produce strong absorptions in the IR region of the electromagnetic spectrum.
I. C-O bond
II. C=C bond
III. C=O bond
a)
I and II only
b)
I and III only
c)
II and III only
d)
I, II and III
24.
The finger print region is 
a)
different for each organic compound
b)
 from 600 - 1400 cm-1
c)
both the above
25.
Stronger bonds absorb  IR at 
a)
higher wave numbers
b)
lower wave numbers
c)
in the finger print region
d)
600cm-1
26.
 Mass of attached atoms affect the absorbance of the bond
a)
True
b)
False
27.
A molecule has a broadband at 3200cm-1 and sharp band at 1711cm-1. the molecule is most likely an
a)
amide
b)
ester
c)
alkanol
d)
carboxylic acid
28.
A molecule has a band at 3500cm-1 and sharp band at 1711cm-1. the molecule is most likely an
a)
amide
b)
ester
c)
alkanol
d)
carboxylic acid
29.
 molecule than has a broard band at 3400 cm-1 and no sharp peak at around 1680 cm-1
a)
amide
b)
ester
c)
alkanol
d)
carboxylic acid
30.

How many carbon environments?

a)

1

b)

2

c)

3

d)

4

31.

How many carbon environments?

a)

1

b)

2

c)

3

d)

4

32.

How many carbon environments?

a)

1

b)

2

c)

3

d)

4

33.

How do you test for carbonate ions?

a)

Add dilute hydrochloric acid and look for bubbles

b)

Add silver nitrate and look for a white precipitate

c)

Add sodium hydroxide and look for a white precipitate

d)

Add lime water and look for bubbles

34.

Which halide ions would produce a white precipitate when tested with silver nitrate?

a)

Cl-

b)

Br-

c)

I-

d)

F-

35.

Why is nitric acid added to a solution before testing for halide ions?

a)

To remove any carbonate ions that might also produce a precipitate

b)

To remove any metal ions that might also produce a precipitate

c)

To remove any fluoride ions in the solution

d)

To remove any halide ions in the solution

36.

Which metal ion would produce a blue precipitate when tested with sodium hydroxide?

a)

Fe2+

b)

Fe3+

c)

Cu2+

d)

Ca2+

e)

Al3+

37.

Which metal ion would produce a brown precipitate when tested with sodium hydroxide?

a)

Fe2+

b)

Fe3+

c)

Cu2+

d)

Ca2+

e)

Al3+

38.

Which metal ion would produce a green precipitate when tested with sodium hydroxide?

a)

Fe2+

b)

Fe3+

c)

Cu2+

d)

Ca2+

e)

Al3+

39.

Which metal ion is identified by a blue-green flame test colour?

a)

Ca2+

b)

Na+

c)

Li+

d)

Cu2+

40.

Which metal ion is identified by a orange-red flame test colour?

a)

Ca2+

b)

Na+

c)

K+

d)

Cu2+

41.

Which metal ion is identified by a lilac flame test colour?

a)

Ca2+

b)

Na+

c)

K+

d)

Cu2+

42.

triglyceride + sodium hydroxide

a)

esterification

b)

saponification

43.

alkene + Br2

a)

no reaction

b)

colourless to brown

c)

brown to colourless

d)

bubbles

44.

alkane + Br2

a)

bubbles

b)

brown to colourless

c)

colourless to brown

d)

no reaction

45.

carboxylic acid + sodium bicarbonate

a)

bubbles of carbon dioxide

b)

colour change

c)

temperature change

d)

bubbles of hydrogen gas

46.

alcohol + sodium metal

a)

bubbles of carbon dioxide

b)

bubbles of hydrogen gas

c)

bubbles of oxygen

d)

no bubbles

47.

primary alcohol + zinc chloride/HCl mixture (Lucas reagent)

a)

cloudy immediately

b)

cloudy after an hour

c)

no reaction

48.

secondary alcohol + zinc chloride/HCl mixture (Lucas reagent)

a)

cloudy immediately

b)

cloudy after an hour

c)

no reaction

49.

tertiary alcohol + zinc chloride/HCl mixture (Lucas reagent)

a)

cloudy immediately

b)

cloudy after an hour

c)

no reaction

50.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

51.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
52.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
53.

Green chemistry is regarded as a reduction process. Which of the following aspects are the targets of reduction?

(1) Cost of production

(2) Use of catalyst

(3) Risk and hazard

a)

(1) and (2) only

b)

(1) and (3) only

c)

(2) and (3) only

d)

(1), (2) and (3)

54.

Which of the following types of reaction has the greatest value of atom economy?

a)

Substitution

b)

Addition

c)

Elimination

d)

Condensation

55.

Which of the following substances is NOT a volatile organic compound?

a)

Benzene

b)

Trichloromethane

c)

Carbon dioxide

d)

Methanal

56.

Which of the following are sources of biomass to replace natural gas as the feedstock of many industrial processes?

(1) Seaweed from large-scale farming

(2) Waste paper from schools and offices

(3) Methane gas from landfill sites

a)

(1) and (2) only

b)

(1) and (3) only

c)

(2) and (3) only

d)

(1), (2) and (3)

57.

Which of the following are the benefits of using catalysts in industrial processes?

(1) Obtaining a higher yield per reaction cycle

(2) Lowering the operating temperature

(3) Getting more product in a relatively shorter period of

time

a)

(1) and (2) only

b)

(1) and (3) only

c)

(2) and (3) only

d)

(1), (2) and (3)

58.

What is green chemistry?

a)

the utilization of a set of guidelines that increases or adds the use or generation of hazardous substances in the design, manufacture and application of chemical products.

b)

the utilization of a set of principles that reduces or eliminates the use or generation of hazardous substances in the design, manufacture and application of chemical products.

c)

a form of chemistry that focuses on how the color green was chemically formed and its components

59.

T/ F: It is best to use the most energy-intensive chemical route.

a)

True

b)

False

60.

Why is transportation an issue for the textile industry?

a)

the industry prefers to keep the textiles in refrigerated transportation

b)

excessive consumption of non-renewable fuel

c)

Textile production units is generally close to the the consumer point

d)

none of the above

61.

What are some alternatives to greener chemistry in the textile industry?

a)

Bio-polymers

b)

recycle textiles

c)

modifications of dyeing process

d)

all of the above

62.

Which of the following is the correct equation for BeerLambert law?

a)

E = A / LC

b)

C = E / AL

c)

A = ELC

d)

L = ACE

63.

Before AAS can be carried out, all the wavelengths of light must be scanned so that the correct wavelength which is absorbed most strongly by the coloured sample can be selected

a)

true

b)

false

64.

Colorimetry is more precise than AAS

a)

true

b)

false

65.

What is AAS used for?

a)

detecting trace amounts of non metal anions

b)

detecting organic molecules

c)

detecting trace amounts of metal cations

66.

What scale does AAS measure to?

a)

ppb

b)

ppm

c)

ppt

67.

Which cation gives a green precipitate with NaOH?

a)

Fe+2

b)

Al+3

c)

Ca+2

d)

Cu+2

e)

Fe+3

68.
All of the following salts are soluble except...
a)
Lead(II) nitrate
b)
Sodium carbonate
c)
Magnesium chloride
d)
Barium sulphate
69.
How do you test for carbon dioxide gas?
a)
Turns limewater milky
b)
Relights a glowing splint
c)
Makes a squeaky pop with a splint
d)
Bleaches damp litmus paper
70.

Colourimetry tells us the concentration of metal ions in a coloured solution based on the fact that:

a)

concentration is proportional to the wavelength

b)

concentration is proportional to the absorption

c)

absorption is proportional to the wavelength

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