Download Learning Outcomes for CHEM1001 in 2015

Learning Outcomes for CHEM1001
Generic attributes and learning outcomes for each topic of the course are given below. They describe the skills and
knowledge you should be able to demonstrate through successful participation in the learning activities in this unit of
study.
Generic Attributes
1. apply scientific knowledge and critical thinking to identify, define and analyse problems, create solutions, evaluate
opinions, innovate and improve current practices
2. gather, evaluate and deploy information relevant to a scientific problem
3. disseminate new knowledge and engage in debate about scientific issues
4. recognize the rapid and sometimes major changes in scientific knowledge and technology, and to value the
importance of continual growth in knowledge and skills
5. use a range of computer software packages in the process of gathering, processing and disseminating scientific
knowledge
6. make value judgements about the reliability and relevance of information in a scientific context
7. evaluate your own performance and development, to recognize gaps in knowledge and acquire new knowledge
independently
8. set achievable and realistic goals and monitor and evaluate progress towards these goals
9. appreciate sustainability and the impact of science within the broader economic, environmental and socio-cultural
context
10. present and interpret data or other scientific information using graphs, tables, figures and symbols
11. work independently and as part of a team and to take individual responsibility with a group for developing and
achieving goals
12. actively seek, identify and create effective contacts with others in a professional and social context, and maintain
those contacts for mutual benefit
13. recognize the importance of safety and risk management and compliance with safety procedures
14. manipulative equations and measurements with due regard for significant figures and unit conventions
Laboratory Skills
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perform careful and safe experiments
accurately report scientific observations
work as a professional scientist with due regard for personal safety and for the safety of those around you
interpret observations in terms of chemical models with appropriate use of chemical equations and calculations
perform calculations containing concentrations, moles and masses
choose and use appropriate glassware for a given task
choose and use balances accurately and appropriately
present and interpret data or other scientific information using graphs, tables, figures and symbols
work as a member of a team and to take individual responsibility within a group for developing and achieving
group goals
10. actively seek, identify and create effective contacts with others in a professional and social context, and maintain
those contacts for mutual benefit
Elements and Atoms
1. explain what an element is
2. appreciate that elements may be metals or non-metals and may be solids, liquids or gases and what these terms
mean
3. recognize that elements are labelled using their chemical symbol
4. explain the differences between elements, compounds and mixtures
5. explain the difference between allotropes and the physical state of an element
6. explain what atoms are and how they combine to form compounds
7. appreciate the difference between physical and chemical properties
8. list the particles that make up atoms, their symbols and their relative masses and charges
9. read and write the atomic symbol containing the mass number and atomic number
10. explain what isotopes are and work out the number of neutrons an isotope contains from its atomic symbol
11. explain how elements can change into another by radioactive decay
12. explain what light is and how its energy is related to its frequency and wavelength
13. draw the shell structure of atoms with up to 18 electrons
Molecules and Ions
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work out the number of electrons an ion has from its symbol
recognize that most ions have a Noble gas configuration
predict whether an element will form a cation or an anion
explain the characteristics of ionic bonding
read and write the chemical formula of ionic compounds
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read and write the chemical formula of ionic compounds
name simple binary ionic compounds according to IUPAC nomenclature
explain how covalent molecules are bonded together and how they differ from ionic compounds
draw simple Lewis dot and line diagrams showing single, double and triple bonds and lone pairs
read and write the chemical formula of covalent compounds
use molecular formula, empirical formula and structural formula
name simple covalent compounds using IUPAC nomenclature
predict the polarity of the bonds in molecules
list the properties of metallic, ionic and covalent solids
Chemical Equations
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explain what chemical reactions are and why they occur
identify reactions as being combination, precipitation, decomposition, replacement or acid/base
write balanced chemical equations for reactions of neutral species, including physical states
write balanced chemical equations for reactions involving charged species, including physical states
write balanced ionic equations for reactions without spectator ions, including physical states
list the characteristics of acids including their reactions
Stoichiometry
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work out atomic mass as a weighted average of isotope masses
work out the molecular mass of a covalent compound from its chemical formula
work out the formula mass of an ionic compound from its chemical formula
relate the mass of a substance to the number of particles it contains using Avogadro's constant
appreciate what a mole of substance is
convert between mass and moles and between moles and mass
work out which reactant is the limiting reagent in a reaction and use it to predict how much product can form
work out the percentage yield in a chemical reaction by identifying the limiting reagent and the theoretical yield
use experimentally determined percentage composition to work out the empirical formula
identify the solvent, solute and solution for a reaction in a solution
interconvert between moles, concentration and volume given two of these quantities
The Periodic Table
1. recognize the relationships between elements in the same periods and in the same groups
2. predict the properties of an element from its position, including its metallic, semi-metallic or non-metallic
properties and the acid, basic or amphoteric properties of its oxide
Atomic Energy Levels
1. identify the number of sub-shells available for each shell and the number of electrons that can fit in each of these
2. write down electron configurations for atoms and ions
Lewis Model of Bonding
1. draw Lewis structures for molecules containing single and multiple bonds and with lone pairs
2. draw resonance structures for molecules where more than one Lewis structure is possible
3. recognize that molecules with resonance structures have bonds which are intermediate between single and double
bonds
VSEPR
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work out the number of bonding and non-bonding pairs from the Lewis structure of a molecule
predict the distribution of these pairs around an atom
place any lone pairs in appropriate positions to minimize the overall electron pair repulsion
predict and describe the molecular shape
Gas Laws
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use the ideal gas law to relate the number of moles, pressure, volume and temperature of a gas
relate gas density and molar mass
convert between the common units of pressure (atm, Pa and mmHg
use the appropriate value of the gas constant, R
Thermochemistry
1. explain the difference between heat and temperature
2. appreciate that heat is mostly associated with changes kinetic energy and chemical reactions are mostly associated
with changes in potential energy
First Law of Thermodynamics
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explain the difference between heat and temperature
identify a process as endothermic or exothermic from the temperature change
relate temperature and heat change using specific and molar heat capacities
calculate internal energy changes using the bomb calorimeter
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define the difference between internal energy and enthalpy
obtain the enthalpy change using a coffee-cup calorimeter
use Hess's Law
estimate reaction enthalpies from bond energies
define standard states
combine enthalpies of formation to work out the enthalpy change for chemical reactions
combine enthalpies of reactions to work out the enthalpies of formation
explain the advantages and disadvantages of solid, petroleum, hypergolic and cryogenic (hydrogen) fuels
work out the efficiency of fuels
Types of Intermolecular Forces
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describe the different kinds of intermolecular forces that exist
identify which intermolecular forces are present and which are more important between different molecules
relate variations in melting and boiling points in related compounds to their intermolecular forces
describe the subunits of synthetic and natural polymers
outline the role of intramolecular and intermolecular forces on the primary, secondary, quaternary and tertiary
structure of synthetic and natural polymers
Oxidation Numbers
1. assign formal oxidation numbers to each atom in a compound
Nitrogen Chemistry and Compounds
1. work out the oxidation number of nitrogen in its compounds
2. work out the shapes and the number of unpaired electrons on nitrogen oxides and halides
3. explain the difference between a fuel and an explosive
Nitrogen in the Atmosphere
1. discuss the NOx cycle in the atmosphere
Chemical Equilibrium
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explain the dynamic nature of equilibrium processes
write the equilibrium constant for any reaction or process
use initial, change, equilibrium (ICE) tables and the small 'x' approach to work out equilibrium concentations
use Le Chatelier's principle to predict the response of a system at equilibrium to changes in temperature, pressure
and composition
5. explain the difference between the equilibrium constant, K, and the reaction quotient, Q
6. write down the reaction quotient and use it to predict the direction of change
7. explain how catalysts effect chemical reactions without changing the equilibrium concentrations
Equilibrium and Thermochemistry in Industrial Processes
1. explain the main processes used industrially to extract metals from their ores
2. use Ellingham diagrams to predict which metals can be extracted using coke at different temperatures
3. outline the thermodynamic principles behind the industrially optimized routes to sulfuric acid and ammonia
Electrochemistry
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relate the sign of the electrode potential to the direction of spontaneous change
combine half cells to produce balanced redox reactions and to calculate cell potentials
identify the species which are being oxidzied and those being reduced in a redox reaction
write down the cell notation for a Galvanic cell including ones involving inert electrodes
use the Nernst equation to calculate the effect of concentration on the cell potential
relate the electrode potential and the reaction quotient
relate the standard electrode potential and the equilibrium constant
Electrolytic Cells
1. identify the processes and species formed at the anode and cathode of Galvanic and electrolytic cells
2. identify the direction of electron flow in Galvanic and electrolytic cells
3. identify what can be electroysed and the role of over-potential in the electrolysis of water and in the production of
NaOH and Cl 2
4. use Faraday's Laws of Electrolysis to relate the amount of product to the electric current applied
Electrochemistry (Batteries and Corrosion)
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explain the difference between primary and secondary batteries
identify the chemical reactions in common batteries
explain how fuel cells work
explain how corrosion occurs and can be reduced