Chemistry Pre Test - Before Starting Yr 12

8/9/2019 Chemistry Pre Test - Before Starting Yr 12

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Before you start Year 12

Chemistry

Introduction Why study chemistry?

What do Chemists do?

What do

chemists do?

In most jobs a chemist would

plan experiments

use a range of equipment to analyse materials and samples

devise new tests and experiments as new products aredeveloped

learn from what other chemists have done, and are doing

What sort of jobs need chemistry training?

Sources: http://www.chem.ubc.ca/undergraduate/brochure/wherechem.shtml http://www.ltu.edu/arts_sciences/chemistry/what_do_chemists_do.asp

Many industries require people with all levels of chemical training,

from technician to Ph.D. Here are some examples.

Environmental

chemist

Determines what substances are present in an environmental

sample and how they got there.

Clinical chemist Works with medical personnel to analyse body tissues and fluids to

provide medical doctors with useful diagnostic information.

Quality control

chemist

Analyses raw materials and intermediates as products of an

industrial process. This provides information about whether a

batch meets specifications and what went wrong in the plant if that

batch failed the tests.

Chemical

technician

Develops practical processes for the large-scale manufacture of

products, as well as improving the existing manufacturing

processes.

Technical

salesperson

Needs a good background in chemistry to sell chemical products to

potential customers.

As background

for other careers

Chemistry provides background knowledge for doctors, metallurgists,

patent attorneys, and technical writers.

Chemistry is a practical subject.

It can lead to many different types of careers, or provide

the background needed for other careers.

http://www.chem.ubc.ca/undergraduate/brochure/wherechem.shtmlhttp://www.chem.ubc.ca/undergraduate/brochure/wherechem.shtmlhttp://www.chem.ubc.ca/undergraduate/brochure/wherechem.shtmlhttp://www.ltu.edu/arts_sciences/chemistry/what_do_chemists_do.asphttp://www.ltu.edu/arts_sciences/chemistry/what_do_chemists_do.asphttp://www.ltu.edu/arts_sciences/chemistry/what_do_chemists_do.asphttp://www.chem.ubc.ca/undergraduate/brochure/wherechem.shtml


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Before you start Page 2

The

chemistry

pre-test

To help you understand what is expected in Year 12 Chemistry, we would like you

to do the pre-test on pages 7 to 9.

Do the pre-test. (You can refer to chemistry notes and texts, but thetest should not take more than about an hour).

Time how long it takes.

Correct your answers and work out your score.

See what we recommend below.

Fill in the questionnaire over the page, and send it in to your teacher.

Your pre- test result… What we recommend …

If you got less than half the pre-test right you will most

likely need a lot of time and support to make a success of

Year 12 Chemistry. Past experience has shown that

students scoring less than 20 out of 40 are not able to

continue with this subject because they find it too

difficult. We strongly recommend that you contact the

Chemistry teachers to discuss your options.

If your score was less than20

40

If you scored between 20 and 30 you will most

likely need revision support throughout the year todevelop the skills expected. This means making

extra time available for your studies, and perhaps

finding a tutor to help you. We suggest that you

consider realistically whether you will be able to

make the extra study time available. Contact the

Chemistry teachers to discuss your options.

If your score was between20

40 and

30

40

If you scored between 30 and 40 you should be able

to cope with most of the skills expected. However,

you will also need to make regular study time a part

of your weekly schedule. If you have any concerns,contact the DECV, and speak to the Chemistry

teachers.

If your score was between 30

40 and

40

40

It’s only fair to warn you…

If you found the pre-test difficult and/or you have enrolled late you will probably find

this subject very challenging.

To have the best chance of making this year a success, you may wish to consider other

options.

The quickest way of finding out more is to ring the DECV, and speak to the Year 12

student manager. Phone: (03) 8480 0000, or toll free (in Victoria) 1800 133 511

Is Year 12 Chemistry the right choice for you?

Before going any further, do the pre-test.


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SEND Why study Year 12 Chemistry?

Your name:____________________________________

Your student number:_________

Your pre-test

1. How did you go in the pre-test? My pre-test score was40

2. How long did it take? The pre-test took me ……………… minutes

3. Which of the following best applies to you?

My pre-test score was good and I feel confident about studying Year 12Chemistry

I found the pre-test challenging but I wish to continue with Year 12 Chemistry.I realise that I will need to spend extra study time each week to revise the

necessary skills.

I found the pre-test difficult and I would like to discuss other options.My contact phone is…………………………………………………………………………………………

The best time to call is……………………………………………………………………………………

The quickest way to find out more about your options is to ring the DECV,

and speak to the Year 12 student manager.

Phone: (03) 8480 0000, or toll free (in Victoria) 1800 133 511


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SEND Why study Year 12 Chemistry?

A bit about you

1. I want to study Chemistry with the DECV because:

………………………………………………………………………………………………………………………………………………………

………………………………………………………………………………………………………………………………………………………

2. Have you studied chemistry before? Tick which best applies to you.

I have studied Year 11 chemistry previously.

I know a bit of chemistry from general science.

I have never studied chemistry before.

3. Have you had a break from study? Tick which best applies to you.

I am still at school.

I am returning to study after a number of months.

I am returning to study after a number of years.

Something different to the above

………………………………………………………………………………………………………………………………………………………

4. What it takes to succeed.

About a third of the students who enrol in Distance Ed Chemistry drop out. To help you

plan ahead it’s important that you realise what is expected before you start. There are

three key questions you should ask yourself about your Chemistry studies.

1st. Time: Do you have approximately 6 hours each week,

more when there is an assessment task due? Yes No

2nd. Can you schedule study periods for chemistry each

week? Yes No

3rd. Lab experiments: Can you attend the DECV for lab work,

or inquire locally for lab pracs (for example, at your own

school or TAFE)?

Yes No

If you answered no to any of the above, your chances of success in this subject may be

affected.

Please contact your chemistry teacher at the DECV to discuss possible options.

Phone: (03) 8480 0000, or toll free (in Victoria) 1800 133 511


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CHEM ISTRY UNITS 3 and 4

PRETEST DATA PAGE

Use the data tables below and the periodic table over the page to help you

answer the pre-test questions.

Table 1: Formulae and charge of selected ions:

Cations Anions

Na+ sodium OH hydroxide

NH4+ ammonium Cl chloride

Ag+ silver NO3 nitrate

Mg2+ magnesium O2 oxide

Zn2+

zinc SO42

sulfate

Cu2+ copper CO32 carbonate

Pb2+ lead PO43 phosphate

Table 2: Solubility of ions in water:

Ions that are soluble in water

Compounds with the following ions

are always soluble in water

Ammonium NH4+

Sodium Na+

Potassium K +

Nitrate NO3


are mostly soluble in waterChloride Cl except with silver, Ag+, or lead, Pb2+

Sulfate SO42 except with silver, Ag+, or lead, Pb2+

Ions that are not soluble in water


are mostly not soluble in water

Hydroxide OH

Sulfide S2

Carbonate CO32

Phosphate PO43

except with

Ammonium NH4+

Sodium Na+

Potassium K +

Table 3: Molar mass of selected elements:

Element H C O Ne Na Cl Pb

Molar mass

(g per mol)1.0 12.0 16.0 20.1 23.0 35.5 207.2

Table 4: Molar mass of gases

STP standard temperature and pressure

temperature 0°C, pressure 101.3 kPa

SLC standard laboratory conditions

temperature 25°C, pressure 101.3 kPa

One mol of any gas occupies22.4 litres at STP

One mol of any gas occupies24.5 litres at SLC


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CHEMISTRY UNITS 3 and 4

PRETEST QUESTIONS

1. Use the Periodic Table given on the previous page to help you answer the following

questions.

(a) What is the atomic number of the following elements

(i) silver (ii) radon (iii) radium

½ + ½ + ½ = 1½ marks

(b) What is the chemical symbol of the following elements

(i) gold (ii) silicon (iii) sodium (iv) antimony

½ + ½ + ½ + ½ = 2 marks

(c) Identify the element with 13 protons and 13 neutrons.1 mark

2. Butane, C4H10 is commonly used in LPG and lighter fluid. It’s melting and boiling points

are shown below.

melting point/ freezing (solidification) point 138 ºC

boiling (evaporation) point/ condensation point 0.5 ºC

Circle the physical state of butane

at room temperature, 25 C solid liquid gas

at fridge temperature, 4 C solid liquid gas

at 5 C solid liquid gas

½ + ½ + ½ = 1½ marks

Use the table of ions (Table 1) on the data page to help you answer questions 3 and 4.

3. Identify the ions present in the following ionic compounds and name the compound.

(a) MgCl2 (b) Na3PO4 (c) Ag2S

3 marks

4. Work out the chemical formula of the following compounds.

(a) Silver hydroxide (b) Magnesium carbonate (c) Zinc nitrate

3 marks

5. Balance the following chemical equations.

(a) Mg(s) + N2(g) Mg3 N2(s) (b) Ca(S) + O2(g) CaO(s)

(c) H2(g) + O2(g) H2O(l) (d) Al (s) + I2 (l) Al2I6(s)

4 marks


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Pre-test questions continued…

6. Use the solubility table (Table 2) on the data page to determine which of the following

ionic compound are soluble.

(a) lead sulfate (b) silver chloride

(c) ammonium chloride (d) zinc carbonate

½ + ½ + ½ + ½ = 2 marks

7. The compound Cu(NO3)2 dissolves in water by dissociation of ions

(a) Identify the ions in the compound.

(b) Write the ionic equation of the dissociation reaction. Show the state of each

compound or ion.

1 + 2 = 3 marks

Refer to the molar mass of elements (Table 3) on the data page to help you answer questions 8,

9 and 10.

8. Find the molar mass of the following compounds

(a) H2O (b) NaCl

2 marks

9. Find the mass of 1.3 mol of CH4

1 mark

10. Calculate the number of mol contained in the following samples, rounded to three decimal places.

(a) 50 g of lead (b) 62 g of NaCl

2 marks

Refer to the molar volume of gases (Table 4) on the data page to help you answer the following

question.

11. (a) Work out the volume of 1.4 mol of chlorine (Cl2) at STP

(b) Work out the mass of 2.8 L of neon (Ne) gas at SLC

1 + 1 = 2 marks

The table below summarises the different types of acid reactions:

Reactions of acids The chemical formulae of selected compounds. 1. acid + metal salt + hydrogen

This reaction does not occur with Cu, Hg, or Ag.

2. acid + metal carbonate

salt + water + carbon dioxide

3. acid + metal oxide salt + water

4. acid + metal hydroxide salt + water

HCl (aq)

Na2CO3 (aq)

NaCl (aq)

H2O (l)

CO2 (g)

CuO (s)

CuCl2 (aq)

H2O (l)

H2SO4 (aq)

NaOH (aq)

Na2SO4 (aq)

Carbonates contain the CO32

ion


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Pre-test questions continued…

12. Use the summary of acid reactions shown above to predict the products of the followingreactions:

(a) HCl (aq) + Mg (s)

(b)HCl (aq) + Na2CO3 (aq)

(c) HCl (aq) + CuO (s)

(d) H2SO4 (aq) + NaOH (aq)

1 + 1 + 1 + 1 = 4 marks

13. Are the following reactions oxidation or reduction reactions?

(a) Cl2(g) + 2e 2Cl (aq)

(b) Pb (s) Pb2+ (aq) + 2e

½ + ½ = 1 mark

14. The reaction Zn(s) + S(s) ZnS (aq) can be written as two half reactions:

Zn(s) Zn2+(aq) + 2e and S(s) + 2e S2 (aq)

(a) Identify the oxidant in this redox reaction

(d) Identify the reductant in this redox reaction

½ + ½ = 1 mark

15. Iron reacts with hydrochloric acid according to the ionic equation

Fe(s) + 2H+(aq) Fe2+(aq) + H2(g)

(a) What has been oxidised in this reaction?

(b) Write a half equation for the oxidation reaction.

(d) What has been reduced in this reaction?

(e) Write a half equation for the reduction reaction.

½ + 1 + ½ + 1 = 3 marks

16. Hydrogen gas and oxygen gas react to form water according to the reaction

2H2 ( g ) + O2 ( g ) 2H2O (l )

10 g of oxygen is reacted in excess hydrogen.

(a) How many mol of oxygen was reacted?

(b) How many mole of hydrogen is required?

(c) Work out the mass of hydrogen reacted.

1 + 1 + 1 = 3 marks

END OF PRE-TEST

Chemistry Pre Test - Before Starting Yr 12

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