Periodic Table, Bonding and Organic

8/10/2019 Periodic Table, Bonding and Organic

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C Three

D Four

(Total 1 mark)

5. The sketch graph below shows the trend in first ionization energies for some elements in Periods

two and three.

Select, from the elements A to D, the one that

(a) has atoms with five p electrons.

A

B

C

D

(1)

(b) is a member of Group 3.

A

B

C

D

(1)

(c) is likely to be very unreactive.


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A

B

C

D

(1)

(d) normally forms four covalent bonds per atom.

A

B

C

D

(1)

(Total 4 marks)

6. Which of these ions has the greatest ability to polarize an anion?

A Ba2+

B Ca

2+

C Cs+

D K+

(Total 1 mark)

7. Which of these electron density maps best represents the bonding in the compound lithium iodide,

LiI?


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(Total 1 mark)

8. Which of the following compounds shows hydrogen bonding in the liquid state?

A Hydrogen bromide, HBr

B Hydrogen sulfide, H2S

C Silane, SiH4

D Ammonia, NH3

(Total 1 mark)

9. Which of the following molecules is polar?

A Carbon dioxide, CO2

B Beryllium chloride, BeCl2

C Ammonia, NH3

D Boron trifluoride, BF3

(Total 1 mark)

10. The electronegativities of four pairs of elements are given below. Which pair would form the

compound with the greatest ionic character?

A 0.7 and 4.0

B 0.7 and 3.5


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C 1.0 and 4.0

D 0.8 and 2.8

(Total 1 mark)

11. Which of the following successive ionization energies (values in kJ mol1) could have come from atransition element?

A 496 4563 6913 9544 13352 16611 20115 25941

B 590 1145 4912 6474 8144 10496 12320 14207

C 717 1509 3249 4940 6985 9200 11508 18956

D 2081 3952 6122 9370 12177 15239 19999 23069

(Total 1 mark)

12. The mechanism of the reaction represented by the equation

C2H4+ Br2 CH2BrCH2Br

is an example of

A Free radical substitution

B Free radical addition

C Electrophilic substitution

D Electrophilic addition

(Total 1 mark)

13. Which of the following successive ionization energies (values in kJ mol1) could have come from a

transition element?

A 496 4563 6913 9544 13352 16611 20115 25941

B 590 1145 4912 6474 8144 10496 12320 14207

C 717 1509 3249 4940 6985 9200 11508 18956

D 2081 3952 6122 9370 12177 15239 19999 23069

(Total 1 mark)

14. The first ionization energies, in kJ mol1, of four elements with consecutive atomic numbers are

shown below.

A 1680

B 2080

C 496


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D 738

(a) Which element could be an inert gas?

A

B

C

D

(1)

(b) Which element could be X in a covalent compound with formula HX?

A

B

C

D

(1)

(c) Which element could be Y in an ionic compound with formula YH2?

A

B

C

D

(1)

(Total 3 marks)

15. The graph below shows the secondionization energy of a series of elements with consecutive

atomic numbers.


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Which element could be lithium?

A

B

C

D(Total 1 mark)

16. Going across Group 1 from sodium to aluminium

A the melting temperature increases.

B the radius of the atom increases.

C the radius of the metal ion increases.

D the bonding in the element changes from metallic to covalent.

(Total 1 mark)

Section - B

1. Consider the following data for the hydrides of the Group 4 elements.

element formula of

hydride

boiling

temperature

/K

relative

molecular

mass

carbon CH4 109 16

silicon SiH4 161 32


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germanium GeH4 185 77

tin SnH4 221 123

lead PbH4

(a) Represent the trend in the boiling temperature with relative molecular mass for these

hydrides.

(2)

(b) (i) Account for the increase in boiling temperature as the relative molecular mass

increases.

............................................................................................................................

Boilingtemperature/K

350

300

250

200

150

100

50

00 50 100 150 200 250

Relative molecular mass


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............................................................................................................................

(2)

(ii) Use your diagram in (a) to suggest a likely value for the boiling temperature of PbH4.

............................................................................................................................(1)

(iii) PbH4 is actually thermally unstable and unlikely to have the boiling temperature you

have suggested. Suggest why PbH4is thermally unstable

............................................................................................................................

............................................................................................................................

(2)

(c) Predict the shape of a molecule of SiH4and justify your prediction.

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................

(3)

(d) (i) Define the termfirst ionisation energy.

............................................................................................................................

............................................................................................................................

(2)


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(ii) The successive ionisation energies of silicon are given in the table below.

number of ionisation ionisation energy/kJ mol-

1

1 789

2 1580

3 3230

4 4360

5 16100

6 19800

7 23800

8 292009 33900

10 38800

11 45900

12 505000

13 235000

14 258000

Use these data to deduce the electronic structure of silicon.

............................................................................................................................

............................................................................................................................

............................................................................................................................

(2)

(Total 14 marks)

2. (a) (i) Define the terms:

atomic number ...............................................................................................

......................................................................................................................

mass number .................................................................................................

......................................................................................................................

(2)


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(ii) Identify the particle which contains 11 protons, 12 neutrons and 10 electrons.

......................................................................................................................

(1)

(b) Bromine consists of two isotopes, mass numbers 79 and 81. A sample of bromine gas, Br2,

was examined in a mass spectrometer. The mass spectrum showing the molecular ions is

given below.

(i) Identify the species responsible for the peak at m/e= 160.

......................................................................................................................

(1)

(ii) Deduce the relative abundances of the two isotopes,

(2)

(c) Define the term first electron affinity for bromine atoms, illustrating your answer with an

equation.

................................................................................................................................

100

50

Relativeintensity

158 160 162

m/e


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................................................................................................................................

................................................................................................................................

................................................................................................................................

(3)

(d) The graph showing the variation of the first ionisation energies of the elements neon to

potassium is given below.

(i) Define the term first ionisation energy with reference to neon.

......................................................................................................................

......................................................................................................................

......................................................................................................................(2)

(ii) Explain the general trend in the first ionisation energies of the elements sodium to

argon.

......................................................................................................................

......................................................................................................................

......................................................................................................................

(2)

(iii) Explain why the first ionisation energy of neon is greater than the first ionisation

energy of argon.

......................................................................................................................

......................................................................................................................

......................................................................................................................

2500

2000

1500

1000

500

0

Firstionisationenergy/kJ mol

1

Ne Na Mg Al Si P S Cl Ar K


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(2)

(Total 15 marks)

3. (a) Define the term covalent bond.

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................

(2)

(b) Nitrogen forms an oxide called nitrous oxide, N2O. The bonding in nitrous oxide can be

represented as:

N N O

Complete the diagram below for the N2O molecule using dots or crosses to represent

electrons. Just show all of the outer shell electrons.

4. (a) (i) Complete the electronic configuration of the magnesium atom.

1s2......................................................................................................................(1)

(ii) Complete the electronic configuration of the chlorine atom.

1s2......................................................................................................................

(1)

(b) (i) Write the equation, including state symbols, for the reaction of magnesium with

chlorine.(2)


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(ii) Name the type of bonding present in magnesium chloride.

...........................................................................................................................

(1)

(iii) Draw a diagram (using dots or crosses) to show the bonding in magnesium chloride.Include ALLthe electrons in each species and the charges present.

(3)

(c) State the type of bonding that exists in solid magnesium.

Type.............................................................................................................................

(1)

(d) Explain fully why the melting temperature of magnesium is higher than that of sodium.

.....................................................................................................................................

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.....................................................................................................................................

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.....................................................................................................................................

.....................................................................................................................................

(3)

(Total 12 marks)

5. (a) The molecule isoprene has the displayed formula

C C C C

H C HH

H

H

H

H

H


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(i) Give the systematic name of isoprene.

...........................................................................................................................

(2)

(ii) What colour change occurs when aqueous bromine solution is added to isoprene?

From ..................................................... to .......................................................

(1)

(iii) State the type and mechanism of this reaction.

Type ................................................ Mechanism .............................................

(2)

(iv) Suggest the displayed formula of the product formed when excess bromine reacts with

isoprene in the dark.

(1)

(b) Compound Q, an isomer of isoprene, has the structural formula

CH2 =CHCH2CH=CH2.

(i) Give the name of the intermolecular force present in both isomers.

...........................................................................................................................

(1)

(ii) Which isomer would you expect to have the higher boiling point? Justify your answer.

...........................................................................................................................

...........................................................................................................................

...........................................................................................................................

(2)

(Total 9 marks)


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6. (a) (i) State TWO features that members of a homologous series have in common.

...........................................................................................................................

...........................................................................................................................

...........................................................................................................................

...........................................................................................................................

(2)

(ii) Name the homologous series to which propene belongs.

...........................................................................................................................(1)

(iii) Propene can be converted into a mixture of 2-chloropropane (as the major product) and

1-chloropropane.

Classify the reaction involved and identify the reagent required.

Classification ....................................................................................................

Reagent .............................................................................................................

(2)

(b) Define the term structural isomers.

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................(2)

(c) 1-chloropropane and 1-bromopropane both react with ammonia to give 1-propylamine.

State and explain, in terms of bonding and kinetics, which of 1-chloropropane and 1-

bromopropane would react faster with ammonia.

.....................................................................................................................................

.....................................................................................................................................


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.....................................................................................................................................

.....................................................................................................................................

(3)

(d) 1-chloropropene, CH3CH CHCl, can be polymerised to form poly(1-chloropropene).

Draw the repeat unit of poly(1-chloropropene).

(2)

(e) Explain why 1-chloropropene exists as two different geometric isomers, but propene does not.

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................

.....................................................................................................................................

(2)

(Total 14 marks)

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Periodic Table, Bonding and Organic