General Chemistry
Semester 1 Exam Objectives, December 2008
Atomic Structure
1. Distinguish between mass number (A), atomic number (Z) and isotopes of an element.
2. Deduce the symbol for an isotope given its mass number and atomic number using the
notation AZX.
3. Calculate the number of protons, neutrons and electrons in atoms and ions form their mass
number and atomic number.
4. Draw a labeled diagram to show the emission spectrum of hydrogen. Label the relative
wavelength, frequency and energy.
5. Explain how electron transitions produce the characteristic line spectrum of hydrogen.
6. Write electron configurations using s,p,d,f notation for the first 20 elements.
7. Determine the frequency and wavelength of visible light using c =  x f
Periodic Table
1. Describe the arrangement of elements on the periodic table in terms of increasing atomic
number, groups and periods, metals and non-metals.
2. Number the groups and periods and know the original names for groups 1,2,7 and 8.
3. Describe and explain the trends in ionization energy and atomic radii on the periodic table.
4. Describe the trends in the number of outer shell electrons and number of electron shells on
the periodic table.
Measurement
1. Express answers using scientific notation.
2. Correctly apply significant figure, decimal place and rounding rules for calculations involving
addition, subtraction, multiplication and division.
3. Correctly indicate the precision of a measurement recorded from a laboratory measuring
device.
4. Interpret data presented in graphs and tables.
5. Plot graphs from provided data. Graphs should be drawn with a sharp pencil; have correctly
plotted points joined with a line of best fit; have an appropriate scale; labeled axes –
variable and unit of measurement in brackets; be an appropriate size; have a concise yet
descriptive title that relates the variables plotted on the x and y axes.
Bonding
1. Describe an ionic bond as the intramolecular electrostatic attraction between two
oppositely charged ions.
2. Deduce the charges on the ions formed when elements in groups 1, 2 and 3 lose electrons
and when elements in groups 5 and 6 gain electrons.
3. Using an ion chart deduce the formulas and names of ionic compounds between monatomic
and polyatomic ions.
4. Use roman numeral notation to name ionic compounds containing transition metals. E.g.
copper (II) chloride.
5. Describe a covalent bond as the intramolecular electrostatic attraction between pairs of
electrons and positively charged nuclei.
6. Deduce the formula and name of common covalent molecules.
7. Draw Lewis (electron dot) structures of simple covalent molecules that obey the octet rule.
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8. Predict the shape (linear, bent, trigonal pyramid, tetrahedral) and bond angles for simple
covalent molecules using the VSEPR theory.
9. Predict whether a compound would be more likely to contain ionic or covalent bonds from
the position of its elements on the periodic table, or from their electronegativity values.
10. Predict whether a covalent molecule is polar or non-polar from its molecular shape.
11. Distinguish between the differences between the three type of intermolecular forces
between covalent molecules (hydrogen bond, permanent dipole attractions and temporary
dipoles/Van Der Waals).
12. Compare the relative strength of intramolecular and intermolecular forces.
13. Identify trends and patterns in the physical properties of ionic, covalent and metallic
substances.
14. Explain in terms of the intermolecular and intramolecular forces of attraction the reason for
the differences in the melting points, boiling points and electrical conductivity of ionic and
simple covalent compounds.
Chemical Reactions
1. Distinguish between chemical and physical changes
2. Understand the law of conservation of mass.
3. Identify chemical reaction as being either: synthesis, combustion, decomposition, singlereplacement (or single displacement) or double replacement (displacement).
4. Write word and balanced chemical reactions for the different types of reactions and be able
to predict the products of a reaction. Use state symbols when appropriate.
Quantitative Chemistry
1. Define an isotope
2. Use the mole concept to determine the number and amount (mole) of all kinds of particles:
atoms, molecules, ions. Convert between the moles of substance and the number of atoms,
ions and molecules. (N = n x 6.02 x 1023)
3. Distinguish between and be able to calculate relative molecular mass (Mr) and molar mass
(M).
4. Solve problems involving the relationship between the moles, mass and molar mass.
(n = m  M)
5. Solve problems involving the relationship between density, mass and volume. (d = m  v)
6. Distinguish between solute, solvent, solution, concentration and liquid.
7. Solve problems involving concentration, amount of solute and volume of solution. (c= n  v
and civi = cfvf)
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