you should hand in the task at your first lesson in september ...13. barium metal can be extracted...

Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL Telephone: 01484 652341 email: [email protected] www.huddnewcoll.ac.uk

Pre-enrolment task for 2014 entry

Chemistry

Why do I need to complete a pre-enrolment task?

This task is so we can assess your skills before starting the course

You should hand in the task at your first lesson in September 2014.

How will I be given feedback on how well I have done?

You will receive feedback from your teacher at the end of the second teaching week.

Task In Detail

1. Draw out a table showing the charge, mass and location of the sub-atomic particles

protons, neutrons and electrons.

When should I hand it in?


2. Complete the following table. The first few have been done for you

element symbol atomic

number

mass

number

number

of

protons

number

of

neutrons

number

of

electrons

electron

arrangement

hydrogen H 1 1 1 0 1 1

helium He 2 4 2 2 2 2

lithium Li 3 7 3 4 3 2,1

beryllium 9

boron 11

carbon 12

nitrogen 14

oxygen 16

fluorine 19

neon 20

sodium 23

magnesium 24

aluminium 27

silicon 28

phosphorus 31

sulphur 32

chlorine 35

argon 40

potassium 39

calcium 40


3. Neatly draw diagrams to show the electron arrangement of an atom for the

following elements.

a. nitrogen

b. carbon

c. potassium

d. phosphorus

e. argon


Ionic bonding and properties of ionic compounds

4. Draw a dot and cross diagram that shows the ionic bonding in lithium fluoride.

5. Draw a dot and cross diagram that shows the ionic bonding in calcium oxide.

6. Draw a dot and cross diagram that shows the ionic bonding in aluminium oxide.


7. Using the Periodic Table, write the symbol for the ion formed (including its charge)

from each of the following elements:

element symbol of ion

formed

element symbol of ion

formed

lithium fluorine

rubidium iodine

calcium astatine

strontium selenium

gallium phosphorus

8. Fill in the table to show the electron arrangements for the following ions:

ion electron

arrangement

ion electron

arrangement

K+ F-

S2- Mg2+

Al3+ N3-


9. Formulae: Using the table of common ions provided complete the following table by

writing in the symbols for all the ions, positive (cations) and negative (anions), which are

part of the named compounds. Hence work out the formulae of the compounds. You are

permitted to use a Periodic Table.

Name of Compound Symbol for

positive ion

(cation)

Symbol for

negative ion

(anion)

Formula of

Compound

potassium iodide

rubidium oxide

sodium nitride

beryllium fluoride

magnesium oxide

aluminium oxide

sodium nitrate

magnesium hydroxide

magnesium nitrate

calcium phosphate

ammonium sulphate

copper(II) carbonate

iron(II) sulphate

sodium hydrogencarbonate


Covalent bonding and properties of covalent compounds

10. Draw ‘dot and cross’ diagrams showing all the electrons in the following molecules:

Fluorine (F2) Phosphine (PH3)

Hydrogen sulphide (H2S) Nitrogen (N2)

Carbon dioxide (CO2)


11. Balancing Equations.

1. Balance the following equations:

C2H6(g) + O2 (g) → CO2 (g) + H2O(l)

Fe(s) + O2(g) → Fe2O3(s)

Na(s) + H2O(l) → NaOH(aq) + H2(g)

KI(aq) + Pb(NO3)2(aq) → PbI2(s) + KNO3(aq)

CaCO3(s) + HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)


Question 12, 13, and 14 involve chemical calculations

12. Rubidium forms an ionic compound with silver and iodine. This compound has a

potential use in miniaturised batteries because of its high electrical

conductivity.

The empirical formula of this ionic compound can be calculated from its

percentage composition by mass: Rb, 7.42%; Ag, 37.48%; I, 55.10%.

(i) Define the term empirical formula.

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

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

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

(ii) Calculate the empirical formula of the compound showing your working

clearly.


13. Barium metal can be extracted from barium oxide, BaO, by reduction with

aluminium.

6BaO + 2Al 3Ba + Ba3Al2O6

Calculate the mass of barium metal that could be produced from reduction of

500 g of barium oxide using this method.

Answer = ............................... g

14 (i) Balance the following equation.

CaCO3 + HNO3 Ca(NO3)2 + CO2 + H2O

(ii) What mass of calcium nitrate would be obtained from 40grams of calcium

carbonate in the above reaction.


15. Structures formed by carbon atoms

Carbon forms giant covalent structures

Diamond

In the structure each carbon is joined to _________

other carbon atoms by ___________________ bonds

consisting of _____________________ electrons.

The arrangement around each carbon is

__________________________and the C-C-C bond

angles are all _______ degrees.

http://www.hull.ac.uk/chemistry/intro_inorganic/Diamond.htm

Explain why diamond has a high melting temperature

Explain why diamond does not conduct electricity


Graphite

http://facweb.bhc.edu/academics/science/harwoodr/GEOL101/study/minerals.htm

Each carbon atom is bonded to __________________ other carbon atoms by

_______________ bonds, forming hexagonal rings. The fourth outer electron of each

carbon atom is delocalised between the sheets of hexagons. The interactions between the

layers of hexagons are _________________ so the layers can slip over each other.

Explain why graphite has a high melting temperature

Explain why graphite conducts electricity

http://facweb.bhc.edu/academics/science/harwoodr/GEOL101/study/minerals.htm

OCR AS Chemistry Bridging course

Table of common ions

+1 +2 +3 -3 -2 -1

lithium Li+ beryllium Be2+ aluminium Al3+ nitride N3- oxide O2- fluoride F-

sodium Na+ magnesium Mg2+ iron(III) Fe3+ phosphide P3- sulphide S2- chloride Cl-

potassium K+ calcium Ca2+ phosphate PO43- carbonate CO3

2- bromide Br-

rubidium Rb+ strontium Sr2+ sulphate SO42- iodide I-

caesium Cs+ barium Ba2+ hydroxide OH-

silver Ag+ iron(II) Fe2+ nitrate NO3-

copper(I) Cu+ zinc Zn2+ hydrogencarbonate HCO3-

hydrogen H+ Copper(II) Cu2+ hydrogensulphate HSO4-

ammonium NH4+

you should hand in the task at your first lesson in september ...13. barium metal can be extracted...

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