G11 ASSESSMENT 4 JUNE 2020

Last updated about 1 year ago

23 questions

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G11 ASSESSMENT 4 JUNE 2020

Last updated about 1 year ago

23 questions

Bonding and IMFs Assessment          [50 Marks]
You have one hour to complete this assessment. At 9:30 the assessment will automatically close.
If you are experiencing any difficulties, message me in Formative, at the relevant question.

SECTION A: Short questions (25 Marks)

1

6

1

8

Draggable item		Corresponding Item

1

Section B: Longer Questions (25 Marks)

Question 1     (9 marks)
Surface tension can be used as an indication of the strength of the intermolecular forces in a substance. Watch the video illustrating an experiment to determine which substance (A, B or C) has the strongest intermolecular forces, and answer the questions that follow:
If you are unable to view the video: copy this link and watch it in separate window: https://drive.google.com/open?id=1Q-wqRmwSCm6v1DILa2huP7dTN58RvCFR 

1

1.1 What is the independent variable in this experiment? [Link for video https://drive.google.com/open?id=1PwV0P8vsYTWPz-eOt_ZjDE44_EJDH0xK]

1

1.2 What is the dependent variable in this experiment?

3

1.3 Complete the table of results for the experiment shown in the video (using the text tool instead of the pen tool may be easier, the size of the text is adjusted using the pen thickness button):

3

Draggable item		Corresponding Item

1

1.5 Suggest ONE controlled variable for this experiment.

Question 2   (16 marks)
Consider the boiling points of the substances in the table and answer the questions that follow:

1

6

2.3 Draw TWO hydrogen sulphide molecules, indicating and labelling the following:
- the elements
- the partial charges
- intramolecular forces (name them)
- intermolecular forces (name them)
(Consider using the circle shape to represent atoms, remember you have an eraser too )

4

2.4 Why is the hydrogen sulphide molecule 'bent" in shape?

1

2.5 What determines bond polarity?

4

2.6 Carbon monoxide and hydrogen fluoride have vastly different boiling points. Use your knowledge of intermolecular forces to explain why their boiling points differ so greatly. Type each point on a new line!

THE END OF THE ASSESSMENT. CHECK YOUR ANSWERS, SUBMIT AND GO GRAB A HOT CHOCOLATE !

Bonding and IMFs Assessment          [50 Marks]
You have one hour to complete this assessment. At 9:30 the assessment will automatically close.
If you are experiencing any difficulties, message me in Formative, at the relevant question.

SECTION A: Short questions (25 Marks)

Which of the following compounds has the lowest boiling point?

hydrogen chloride

ammonia

bromine

neon

Which of the following contain polar covalent bonds, but experience no net dipole?

ammonia

oxygen

water

carbon dioxide

Identify the best explanation for differences in boiling points in each set of examples, by dragging them to appropriate explanation.

noble gases
butan-2-ol and butane-1,2-diol
hexane and methane
2-bromopentane and 2-bromo-2-methylbutane
halogens
NH3 and PH3

Differences in intermolecular forces strength
Differences in electron number and therefore the strength of the temporary dipole
Differences in opportunities for London forces
Differences in number of hydrogen bonds formed

Which answer correctly arranges these compounds in order of DECREASING boiling point?

DCAB

CADB

ABCD

BACD

Which substance has the lowest boiling point?

A

B

C

Impossible to say

Which option correctly arranges the substances in order of INCREASING boiling point?

Consider substances X, Y and Z, which all have a molar mass of 60 g.mol-1:

Which one of the following is the most likely boiling point of Y?

24

40

90

118

Match the following substances with the statement that best describes it.

Draggable item		Corresponding Item
bromine		A substance with a giant network structure in which the atoms are held together by covalent bonds
carbon dioxide		A substance with hydrogen bonding forces
graphite		A substance with a high melting point due to strong electrostatic attraction between cations and anions in the crystal lattice.
barium oxide		A substance which has London forces between atoms in liquid or solid state
hydrogen bromide		A molecular substance with non-polar covalent bonds
sodium		A molecular substance which has dipole-dipole intermolecular forces
ammonia		A substance that can conduct electricity in both the solid and liquid phase
helium		A linear molecular substance with polar covalent bonds

A molecule of hexane is considered to be non-polar. Which one of the statements best describes the reason why the molecule is non-polar?

Hexane is a hydrocarbon with single bonds only between carbons

The charge distribution of electrons within the hexane molecule is symmetrical

The electronegativity difference between C and H atoms is so small as to be considered polar

Hexane is linear molecule and hence considered to be non-polar

The table below lists three properties of solids.
Which one of the solids (A-D) has its particular properties listed correctly?

A

B

C

D

A scientist investigates a factor that influences the boiling points of alkanes. He determines the boiling points of the first six straight chain alkanes. Which one of these is the independent variable in this investigation?

Boiling point

Functional group

Degree of branching

Chain length

Which of these hypothetical substances will be a liquid at room temperature?

A

B

C

D

Which of the following exists as a solid in a molecular crystal lattice with dipole-dipole forces between particles/subunits?

chloromethane

methane

chlorine

calcium chloride

Section B: Longer Questions (25 Marks)

Question 1     (9 marks)
Surface tension can be used as an indication of the strength of the intermolecular forces in a substance. Watch the video illustrating an experiment to determine which substance (A, B or C) has the strongest intermolecular forces, and answer the questions that follow:
If you are unable to view the video: copy this link and watch it in separate window: https://drive.google.com/open?id=1Q-wqRmwSCm6v1DILa2huP7dTN58RvCFR 

1.1 What is the independent variable in this experiment? [Link for video https://drive.google.com/open?id=1PwV0P8vsYTWPz-eOt_ZjDE44_EJDH0xK]

1.2 What is the dependent variable in this experiment?

1.3 Complete the table of results for the experiment shown in the video (using the text tool instead of the pen tool may be easier, the size of the text is adjusted using the pen thickness button):

1.4 Match each of these substances to the IMF that is most likely present based on these results.

Draggable item		Corresponding Item
B		hydrogen bonding
C		London forces
A		dipole-dipole forces

1.5 Suggest ONE controlled variable for this experiment.

Question 2   (16 marks)
Consider the boiling points of the substances in the table and answer the questions that follow:

2.1 The boiling point of methane is greater than that of oxygen because ....

a molecule of methane has a smaller mass than a molecule of oxygen

molecules of methane have stronger intermolecular forces than those of
oxygen

the molecule of methane is polar and oxygen is non-polar

molecules of methane form hydrogen bonds, but those of oxygen do not

2.3 Draw TWO hydrogen sulphide molecules, indicating and labelling the following:
- the elements
- the partial charges
- intramolecular forces (name them)
- intermolecular forces (name them)
(Consider using the circle shape to represent atoms, remember you have an eraser too )

2.4 Why is the hydrogen sulphide molecule 'bent" in shape?

2.5 What determines bond polarity?

2.6 Carbon monoxide and hydrogen fluoride have vastly different boiling points. Use your knowledge of intermolecular forces to explain why their boiling points differ so greatly. Type each point on a new line!

THE END OF THE ASSESSMENT. CHECK YOUR ANSWERS, SUBMIT AND GO GRAB A HOT CHOCOLATE !

Which of the following compounds has the lowest boiling point?

hydrogen chloride

ammonia

bromine

neon

Which of the following contain polar covalent bonds, but experience no net dipole?

ammonia

oxygen

water

carbon dioxide

Identify the best explanation for differences in boiling points in each set of examples, by dragging them to appropriate explanation.

noble gases

butan-2-ol and butane-1,2-diol

hexane and methane

2-bromopentane and 2-bromo-2-methylbutane

halogens

NH3 and PH3

Differences in intermolecular forces strength

Differences in electron number and therefore the strength of the temporary dipole

Differences in opportunities for London forces

Differences in number of hydrogen bonds formed

Which answer correctly arranges these compounds in order of DECREASING boiling point?

DCAB

CADB

ABCD

BACD

Which substance has the lowest boiling point?

A

B

C

Impossible to say

Which option correctly arranges the substances in order of INCREASING boiling point?

CBA

ACB

CAB

ABC

BCA

Consider substances X, Y and Z, which all have a molar mass of 60 g.mol-1:

Which one of the following is the most likely boiling point of Y?

24

40

90

118

Match the following substances with the statement that best describes it.

bromine

A substance with a giant network structure in which the atoms are held together by covalent bonds 

carbon dioxide

A substance with hydrogen bonding forces

graphite

A substance with a high melting point due to strong electrostatic attraction between cations and anions in the crystal lattice.

barium oxide

A substance which has London forces between atoms in liquid or solid state

hydrogen bromide

A molecular substance with non-polar covalent bonds

sodium

A molecular substance which has dipole-dipole intermolecular forces

ammonia

A substance that can conduct electricity in both the solid and liquid phase

helium

A linear molecular substance with polar covalent bonds

A molecule of hexane is considered to be non-polar. Which one of the statements best describes the reason why the molecule is non-polar?

Hexane is a hydrocarbon with single bonds only between carbons

The charge distribution of electrons within the hexane molecule is symmetrical

The electronegativity difference between C and H atoms is so small as to be considered polar

Hexane is linear molecule and hence considered to be non-polar

The table below lists three properties of solids. 
Which one of the solids (A-D) has its particular properties listed correctly?

A

B

C

D

A scientist investigates a factor that influences the boiling points of alkanes. He determines the boiling points of the first six straight chain alkanes. Which one of these is the independent variable in this investigation?

Boiling point

Functional group

Degree of branching

Chain length

Which of these hypothetical substances will be a liquid at room temperature?

A

B

C

D

Which of the following exists as a solid in a molecular crystal lattice with dipole-dipole forces between particles/subunits?

chloromethane

methane

chlorine

calcium chloride

1.4  Match each of these substances to the IMF that is most likely present based on these results.

B

hydrogen bonding

C

London forces

A

dipole-dipole forces

2.1  The boiling point of methane is greater than that of oxygen because ....

a molecule of methane has a smaller mass than a molecule of oxygen

molecules of methane have stronger intermolecular forces than those of
oxygen

the molecule of methane is polar and oxygen is non-polar

molecules of methane form hydrogen bonds, but those of oxygen do not

G11 ASSESSMENT 4 JUNE 2020

G11 ASSESSMENT 4 JUNE 2020

Bonding and IMFs Assessment [50 Marks]

SECTION A: Short questions (25 Marks)

Section B: Longer Questions (25 Marks)

1.1 What is the independent variable in this experiment? [Link for video https://drive.google.com/open?id=1PwV0P8vsYTWPz-eOt_ZjDE44_EJDH0xK]

1.2 What is the dependent variable in this experiment?

1.3 Complete the table of results for the experiment shown in the video (using the text tool instead of the pen tool may be easier, the size of the text is adjusted using the pen thickness button):

1.5 Suggest ONE controlled variable for this experiment.

2.3 Draw TWO hydrogen sulphide molecules, indicating and labelling the following: - the elements - the partial charges - intramolecular forces (name them) - intermolecular forces (name them)(Consider using the circle shape to represent atoms, remember you have an eraser too )

2.4 Why is the hydrogen sulphide molecule 'bent" in shape?

2.5 What determines bond polarity?

2.6 Carbon monoxide and hydrogen fluoride have vastly different boiling points. Use your knowledge of intermolecular forces to explain why their boiling points differ so greatly. Type each point on a new line!

Bonding and IMFs Assessment [50 Marks]

SECTION A: Short questions (25 Marks)

Which of the following compounds has the lowest boiling point?

Which of the following contain polar covalent bonds, but experience no net dipole?

Identify the best explanation for differences in boiling points in each set of examples, by dragging them to appropriate explanation.

Which answer correctly arranges these compounds in order of DECREASING boiling point?

Which substance has the lowest boiling point?

Which option correctly arranges the substances in order of INCREASING boiling point?

Consider substances X, Y and Z, which all have a molar mass of 60 g.mol-1:Which one of the following is the most likely boiling point of Y?

Match the following substances with the statement that best describes it.

A molecule of hexane is considered to be non-polar. Which one of the statements best describes the reason why the molecule is non-polar?

The table below lists three properties of solids. Which one of the solids (A-D) has its particular properties listed correctly?

A scientist investigates a factor that influences the boiling points of alkanes. He determines the boiling points of the first six straight chain alkanes. Which one of these is the independent variable in this investigation?

Which of these hypothetical substances will be a liquid at room temperature?

Which of the following exists as a solid in a molecular crystal lattice with dipole-dipole forces between particles/subunits?

Section B: Longer Questions (25 Marks)

1.1 What is the independent variable in this experiment? [Link for video https://drive.google.com/open?id=1PwV0P8vsYTWPz-eOt_ZjDE44_EJDH0xK]

1.2 What is the dependent variable in this experiment?

1.3 Complete the table of results for the experiment shown in the video (using the text tool instead of the pen tool may be easier, the size of the text is adjusted using the pen thickness button):

1.4 Match each of these substances to the IMF that is most likely present based on these results.

1.5 Suggest ONE controlled variable for this experiment.

2.1 The boiling point of methane is greater than that of oxygen because ....

2.3 Draw TWO hydrogen sulphide molecules, indicating and labelling the following: - the elements - the partial charges - intramolecular forces (name them) - intermolecular forces (name them)(Consider using the circle shape to represent atoms, remember you have an eraser too )

2.4 Why is the hydrogen sulphide molecule 'bent" in shape?

2.5 What determines bond polarity?

2.6 Carbon monoxide and hydrogen fluoride have vastly different boiling points. Use your knowledge of intermolecular forces to explain why their boiling points differ so greatly. Type each point on a new line!

2.3 Draw TWO hydrogen sulphide molecules, indicating and labelling the following:
- the elements
- the partial charges
- intramolecular forces (name them)
- intermolecular forces (name them)
(Consider using the circle shape to represent atoms, remember you have an eraser too )

Consider substances X, Y and Z, which all have a molar mass of 60 g.mol-1:

Which one of the following is the most likely boiling point of Y?

The table below lists three properties of solids.
Which one of the solids (A-D) has its particular properties listed correctly?

2.3 Draw TWO hydrogen sulphide molecules, indicating and labelling the following:
- the elements
- the partial charges
- intramolecular forces (name them)
- intermolecular forces (name them)
(Consider using the circle shape to represent atoms, remember you have an eraser too )