Course title

Pre-requisite

Course description

IB Chemistry Standard Level is designed to expand on the knowledge and experimental skills obtained in Chemistry and to prepare the student for further study of pure and applied sciences in higher education. It will also help the student to develop the ability to analyze scientific literature critically and to develop manipulative and experimental skills necessary to perform college level scientific investigations. Topics include stoichiometry; atomic theory; periodicity; bonding; states of matter; energetics; kinetics; equilibrium; acids and bases; oxidation and reduction; and organic chemistry. This course is part of the IB Diploma Programme. Prerequisite: Integrated Science; and/or Biology. Fee required. Scientific calculator required.

IB Chemistry SL/ HL Syllabus

I. Course description and aims

Chemistry is an experimental science that combines academic study with the acquisition of practical and investigational skills. Chemical principles underpin both the physical environment in which we live and all biological systems. Chemistry is often a prerequisite for many other courses in higher education; such as medicine; biological science and environmental science.
Both theory and practical work should be undertaken by all students as they complement one another naturally; both in school and in the wider scientific community. The DP chemistry course allows students to develop a wide range of practical skills and to increase facility in the use of mathematics. It also allows students to develop interpersonal and information technology skills; which are essential to life in the 21st century.
By studying chemistry students should become aware of how scientists work and communicate with each other. While the scientific method may take on a wide variety of forms; it is the emphasis on a practical approach through experimental work that characterizes the subject.
Teachers provide students with opportunities to develop manipulative skills; design investigations; collect data; analyse results and evaluate and communicate their findings.
Through the overarching theme of the nature of science; the aims of the DP chemistry course are to enable students to: 1. appreciate scientific study and creativity within a global context through stimulating and challenging opportunities 2. acquire a body of knowledge; methods and techniques that characterize science and technology 3. apply and use a body of knowledge; methods and techniques that
characterize science and technology 4. develop an ability to analyse; evaluate and synthesize scientific information 5. develop a critical awareness of the need for; and the value of; effective collaboration and communication during scientific activities 6. develop experimental and investigative scientific skills including the use of current technologies 7. develop and apply 21st century communication skills in the study of science 8. become critically aware; as global citizens; of the ethical implications of using science and technology 9. develop an appreciation of the possibilities and limitations of science and technology 10. develop an understanding of the relationships between scientific disciplines and their influence on other areas of knowledge.

II. Curriculum model overview

Component Core 1. Stoichiometric relationships 2. Atomic structure 3. Periodicity 4. Chemical bonding and structure 5. Energetics/thermochemistry 6. Chemical kinetics 7. Equilibrium 8. Acids and bases 9. Redox processes 10. Organic chemistry 11. Measurement and data processing
About the IB: For over 40 years the IB has built a reputation for high-quality; challenging programmes of education that develop internationally minded young people who are well prepared for the challenges of life in the 21st century and able to contribute to creating a better; more peaceful world.
For further information on the IB Diploma Programme; and a complete list of DP subject briefs; visit: http://www.ibo.org/diploma/.
Complete subject guides can be accessed through the IB online curriculum centre (OCC) or purchased through the IB store: http://store.ibo.org.
For more on how the DP prepares students for success at university; visit: www.ibo.org/recognition or email: [email protected].
Additional higher level (AHL) 12. Atomic structure 13. The periodic table—the transition metals 14. Chemical bonding and structure 15. Energetics/thermochemistry 16. Chemical kinetics 17. Equilibrium 18. Acids and bases 19. Redox processes 20. Organic chemistry 21. Measurement and analysis
60 2 4 7 7 6 4 10 6 12 2
Option (Choice of one out of four) A. Materials B. Biochemistry C. Energy D. Medicinal chemistry
25 25 25 25 25
Practical scheme of work Prescribed and other practical activities Individual investigation (internally assessed) Group 4 project
60 40 10
10
The group 4 project The group 4 project is a collaborative activity where students from different group 4 subjects; within or between schools; work together. It allows for concepts and perceptions from across disciplines to be shared while appreciating the environmental; social and ethical implications of science and technology. It can be practically or theoretically based and aims to develop an understanding of the relationships between scientific disciplines and their influence on other areas of knowledge. The emphasis is on interdisciplinary cooperation and the scientific processes.

III. Assessment model

Studying this course; students should be able to fulfill the following assessment objectives: 1. Demonstrate knowledge and understanding of: • facts; concepts; and terminology • methodologies and techniques • communicating scientific information. 2. Apply: • facts; concepts; and terminology • methodologies and techniques • methods of communicating scientific information. 3. Formulate; analyse and evaluate: • hypotheses; research questions and predictions • methodologies and techniques • primary and secondary data • scientific explanations.
4. Demonstrate the appropriate research; experimental; and personal skills necessary to carry out insightful and ethical investigations.
Assessment at a glance Type of assessment Format of assessment
Time (hours)
Weighting of final grade (%) External 4.5 80 Paper 1 40 multiple-choice questions (Core and AHL) 1 20 Paper 2 Short answer and extended response questions (Core and AHL) 2.25 36 Paper 3 Data- and practical –based questions; plus short answer and extended response questions on the option 1.25 24 Internal 10 20 Individual investigation Investigation and write-up of 6 to 12 pages 10 20

IV. Sample questions

• What is the sum of the coefficients when the equation for the combustion of ammonia is balanced using the smallest possible whole numbers?
___ NH3 (g) + ___ O2 (g) ___ N2 (g) + ___ H2O (g)

A. 6 B. 12 C. 14 D. 15 (Paper 1)
• The two isomers of [Pt(NH3)2Cl2] are crystalline. One of the isomers is widely used in the treatment of cancer. i. Draw both isomers of the complex; ii. Explain the polarity of each isomer using a diagram of each isomer to support your answer; iii. State a suitable method (other than looking at dipole moments) to distinguish between the two isomers iv. Compare and contrast the bonding types formed by nitrogen in [Pt(NH3)2Cl2] (Paper 2)

V. Prescribed practicals (labs)

Included in the “Applications and skills” sections of the guide are a series of practicals that students must cover either in a laboratory environment or as a simulation. The skills and general techniques associated with these common practicals may be assessed as part of the external assessment.

Topic 1.2
Obtaining and using experimental data for deriving empirical formulas from
reactions involving mass changes.
Determine the formula of MgO
Determine the formula of hydrated copper sulfate
Topic 1.3
Use of the experimental method of titration to calculate the concentration of a
solution by reference to a standard solution.
Preparation of a standard solutioN/Acid base titration
Determine the percentage CaCO3 in eggshells
Topic 1.3
Obtaining and using experimental values to calculate the molar mass of a gas from
the ideal gas equation.
Determine the molar mass of a gas (CO2) experimentally
Topic 5.1
A calorimetry experiment for an enthalpy of reaction should be covered and the
results evaluated.
Calculate enthalpy change of neutralisation (HCl and NaOH)
Calculate enthalpy change Zn and CuSO4
Topic 6.1
Investigation of rates of reaction experimentally and evaluation of results.
Sodium thiosulfate and hydrochloric acid reaction
Iodine clock reaction
Topic 8.2
Candidates should have experience of acid–base titrations with different indicators.
Covered in topic 1.3
Topic 8.3
Students should be familiar with the use of a pH meter and universal indicator.
Reactions of acid and bases lab
Topic 9.2
Performance of laboratory experiments involving a typical voltaic cell using two
metal/metal–ion half-cells.
Voltaic cell with Zn and Cu half-cells
Topic 10.1
Construction of 3D models (real or virtual) of organic molecules.
Molecular shapes simulation https://phet.colorado.edu/en/simulation/molecule-shapes
Molymods http://www.molymod.com/
Chemdoodle https://www.chemdoodle.com/
Topic 19.1
Perform lab experiments which could include single replacement reactions in
aqueous solutions.
Displacement reactions

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Approved competency code

• LCHM
• Chemistry

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Online / Virtual