1 an Introduction to Chemistry

1 An Introduction to Chemistry

1. What is chemistry the study of?

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2. What was an alchemist?

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3. What links does modern chemistry have with alchemy?

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4. List the four goals of alchemy?

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5. Complete the following table on alchemist regions.

Alchemy Region / Purpose / General Information / Contribution to modern chemistry
China
India and Tibet
Egypt

6. What were the four elements that all materials were made from according to alchemists?

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7. Discuss the fall of alchemy and then its rise in western science?

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8. What is aether?

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9. How does the definition of an element to alchemists differ to modern classification?

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10. Explain the origin of the term atom.

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11. Outline the process of scientific method? What are the benefits of using this method?

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12. Why were scientists sceptical of the element theory?

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13. What contributions did French couple Antoine and Marie Lavoisier give to modern chemistry?

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14. Complete the following table

Law / Description / Example
Conservation of mass
Constant proportions

15. Complete the following table

Substance / Definition / Example
Element
Compound
Mixture

17. Discuss John Dalton’s model of the atom?

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18. Summarise Dalton’s atomic theory?

Unit 1 & 2 PowerPoints Supplementary Notes

VCE Chemistry – Horsham College

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Unit 1 & 2 PowerPoints Supplementary Notes

VCE Chemistry – Horsham College

Unit 1 & 2 PowerPoints Supplementary Notes

VCE Chemistry – Horsham College

2 The Structure of the Atom

1. What was the purpose and findings from Crooke’s Tube?

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2. Summarise J.J Thomson’s cathode ray experiment findings

Experiment / Findings

3. What was J.J Thomson’s plum pudding model of the atom?

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4. Explain Rutherford’s famous alpha-particle scattering experiment using the diagram below as a guide.

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5. What was Rutherford’s model of the atom and how was it different to Dalton’s model?

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6. What was the major problem with Rutherford’s model of the atom?

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7. How did Niels Bohr prove Rutherford wrong?

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8. Explain Bohr’s model of the atom

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9. Complete the following table on Bohr’s energy shells

Shell / Letter / Number of Electrons
1
2
3
4
n

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10. How does flame testing demonstrate?

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11. What is meant by a substance’s electron configuration?

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12. What are spectral lines? How can they be calculated?

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13. What is an element’s atomic number (z)?

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14. List some problems with Bohr’s model of the atom.

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15. What is the Scrödinger model?

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16. Complete the following table on Scrödinger’s model.

Electron Shell / n / Sub shells / Names of subshells / Max number of electrons in the subshell / Max number of electrons in the shell
K
L
M
N

17. What is an atomic orbital?

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18. Complete the following table on atomic orbitals.

Type of subshell / Type of orbit / Number of orbits / Max number of electrons in the subshell
s
p
d
f
g

19. Explain, using the diagram below, how electrons fill the subshells.

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3 The Masses of Atoms

1. What is accuracy important in chemistry?

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2. What is meant by a relative scale for measurement?

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3. What was the contribution of Jons Berzelius to modern chemistry?

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4. Discuss the difference between the terms mass and weight.

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5. What is an isotope?

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6. What was the significance of the invention of a mass spectrograph?

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7. Describe was a mass spectrum reading indicates.

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8. How were neutrons discovered?

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9. How is an element’s mass number (A) determined?

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10. Why is carbon-12 used as the comparative isotope on the relative mass scale?

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11. What are the units for the relative mass scale?

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12. What is the trend on the periodic table between atomic and mass numbers as you increasing through the table?

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13. How is the RMM of molecules calculated?

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14. How is the percentage composition of a substance calculated?

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4 The Modern Periodic Table

1. What is the periodic table and why is it commonly displayed in science classrooms?

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2. Why is the periodic table only a recent addition to the field of chemistry? ______

3. How were elements originally sorted?

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4. What is meant by the term periodic law?

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5. What were the four groups that Antoine Lavoisier classified elements into called?

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6. What were Johann Döbereiner’s triads? Give an example.

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7. Explain how Alexandre de Chancourtois’ cylinder of the elements worked.

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8. What was John Newlands’ law of octives table?

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9. What were the major flaws of Newland’s table?

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10. Who is the ‘father’ of the modern periodic table? Discuss your answer.

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11. Discuss Dmitri Mendeleev’s formation of the periodic table.

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12. Why wasn’t Julius von Meyer credited for developing the modern periodic table?

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13. What similarities and differences occur in Mendeleev/Meyer’s periodic table to today’s modern table?

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14. What was the major contribution that Henry Moseley made to the modern periodic table?

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15. What was the major contribution that Glenn Seaborg made to the modern periodic table?

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16. On, the periodic table, what does the group and period number signify in terms of electron configuration?

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17. Complete the following table

Block / s / p / d
Holding capacity of subshell
Number of groups
Metal Classification
(Main series / transition)
Example

18. What makes group 18 elements special?

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19. How did Henry Cavendish discover one of these elements?

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20. How did the work of Lord Rayleigh and William Ramsay change the periodic table?

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21. Name the six noble gases.

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22. Why were there missing elements? What were the four missing elements called?

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5 Trends of the Periodic Table

1. What characteristics can elements be classified as?

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2. Complete the following table of metallic elemental properties

Property / Description
Lustre
Conductivity – Heat
Conductivity - Electricity
Malleability
Ductility

3. What are metalloids and where are the found on the periodic table?

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4. Hydrogen is considered a ‘special case’ on the periodic table? Explain why.

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5. What is a compound?

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6. What is a binary compound? What are oxides?

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7. Complete the following table

Compound / Bonding / Oxide (Acid or Base)
Metal
Non-metal

8. What is the most reactive non-metal element on the periodic table? What compounds does it form?

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9. What is the most reactive metal? What is the least reactive metal?

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10. What is the trend of reactivity on the periodic table?

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11. What is meant by the term ‘first ionisation energy’ of an uncharged element? How does this effect its reactivity?

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12. What is the trend of first ionisation energy on the periodic table?

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13. How does the atomic radius of an element affect its reactivity?

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14. What is meant by the term ‘electronegativity’? What is the trend of electronegativity on the periodic table?

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6 Measurement in Chemistry

1. Why was the system of atomic weights originally used?

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2. What does the term mole mean in Chemistry?

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3. What is the relationship between the mole and Avogadro’s number?

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Formulas;

4. The mole is an SI unit – what does this mean?

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5. Many substances are found in molecule or compound form. Discuss how to calculate the total number of particles in ‘packaged’ substances.

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6. Water has a molar mass of 18.0gmol-1. What does this figure mean?

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7. Explain how to calculate the percentage composition of sodium in sodium chloride (NaCl).

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8. What is the relationship between number of moles and mass?

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Formulas;

9. What is the empirical formula of a substance?

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10. What is meant by a hydrated salt? What does anhydrous mean?

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7 Metals

1. Historically, why have metals been very important to humans?

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2. Why do most metals need to be ‘extracted’?

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3. What is an alloy? What was the first alloy made?

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4. Outline the properties of metals

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5. Why are particular metals used for specific uses? Eg. Copper in wiring, Iron in construction etc..

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6. What is the internal structure of metals?

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7. Explain how metallic bonding works.

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8. Use the metallic model to explain the properties of metals.

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9. Explain the other properties of metals based on metallic bonding.

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10. What are some limitations to the metallic model?

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11. Why is copper one of the most commonly used metals?

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12. Why do metals differ in their reactivity levels?

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13. What do the terms reductant and oxidant mean?

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14. How can the rate of corrosion be slowed down in metal surfaces?

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15. What are the metals used in the following alloys; steel, sterling silver and carat gold?

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16. What is the relationship between crystals and the structure of metals?

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17. Complete the following table on the heat treatment of metals

Treatment / Process / Properties

8 Ionic Compounds

1. What are salts?

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2. What are some properties of salts?

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3. What are cations and anions?

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4. Explain why the following ions have the given charges.

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5. Discuss chemically how sodium chloride forms.

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6. What is an ionic lattice? Use the model to explain the properties of salts.

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7. What are some limitations of the ionic model?

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8. What is meant by the coordination number of a salt?

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9. What determines the boiling and melting point of a salt?

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10. Briefly explain how to name ionic compounds.

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11. What is a polyatomic ion?

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12. How do you write ionic formulas? Pick five different cations and anions and write their formulas.

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13. How are hydrates named?

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9 Non Metals

1. What some properties of non-metals?

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2. Hydrogen forms a diatomic molecule. What does this mean?

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3. What is a discrete substance?

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4. What is a covalent bond?

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5. What does the term intramolecular bonding mean?

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6. Discuss how the fluorine molecule is formed. Why does fluorine have lone pairs? What is a single bond?

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7. Discuss how the oxygen molecule is formed. What is a double bond?

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8. Discuss how the sulphur molecule is formed. Why is it often called the sulphur ring molecule?

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9. What do graphite and diamond have in common? What is an allotrope?

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10. List three major differences between non-metals.

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11. What is intermolecular bonding? What is a dispersion force?

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12. Why does diamond form a giant lattice?

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13. Why does graphite form a layer lattice?

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14. What is a buckeyball?

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15. What is nanotechnology? How small is a nanometre?

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10 Molecular Compounds

1. What is a molecular compound?

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2. Discuss the formation of hydrogen fluoride. What type of intramolecular bonding is occurring? What shape is the molecule?

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3. Why is water essential to life on earth?

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4. Discuss the main features of the water molecule.

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5. State three facts about ammonia.

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6. What shape is the ammonia molecule? Explain why it is that shape.

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7. State three facts about methane.

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8. What shape is the methane molecule? Explain why it is that shape.

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9. What shape is the carbon dioxide molecule? Explain why it is that shape.

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10. What are some general properties of molecular compounds?

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11. What is a polar substance? What makes a molecule non-polar?

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12. What is dipole-dipole attraction?

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13. Outline the main differences between a polar and a non-polar substance.

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14. Why is hydrogen bonding a stronger form of intermolecular bonding?

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15. Why is water unique?

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16. What is surface chemistry?

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17. How do soaps make water ‘wet’ better?

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11 Organic Compounds

1. Why is carbon special?

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2. Why are carbon compounds the most common type of compound?

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3. State the difference between organic and inorganic compounds.

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4. Complete the following table of prefixes.

1 / 2 / 3 / 4 / 5 / 6 / 7 / 8 / 9 / 10

5. What is a functional group?

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6. List seven families of organic compounds.

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7. What is a hydrocarbon? What is the difference between a saturated and unsaturated hydrocarbon?

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8. What is an alkane? What is the formula for an alkane family member?

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9. What are some properties of alkanes?

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10. Write a worded combustion reaction for an alkane.

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11. What is a structural isomer? Give an example.

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12. List the key steps in naming hydrocarbons.

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13. What is a semi-structural formula?

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14. What is an alkene? What is the formula for the alkene family?

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15. What is an addition reaction?

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16. What is a polymer? What is a polymerisation reaction?

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17. What is an alkyne? What is the formula for the alkyne family?

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18. What is a cyclic hydrocarbon?