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SED122Education2 Unitsbeginner

Chemistry For Integrated Science

This course, General Chemistry for Integrated Science 1, provides a foundational understanding of chemistry principles essential for students in integrated science programs. It covers topics such as atomic structure, chemical bonding, the periodic table, and basic chemical reactions. The course aims to equip students with the language of chemistry and the ability to perform simple chemical calculations, preparing them for more advanced science courses.

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156h
Study Time
13
Weeks
12h
Per Week
basic
Math Level
Course Keywords
ChemistryAtomic StructureChemical BondingPeriodic TableChemical Reactions

Course Overview

Everything you need to know about this course

Course Difficulty

Beginner Level
Perfect for newcomers to the field
35%
beginner
➕
Math Level
Basic Math
🔬
Learning Type
Hands-on Practice

Course Topics

Key areas covered in this course

1

Atomic Structure

2

Chemical Bonding

3

Periodic Table

4

Acids, Bases, and Salts

5

Gas Laws

6

Liquids and Solids

7

Carbon and Its Compounds

Total Topics7 topics

Ready to Start

No specific requirements needed

This course is designed to be accessible to all students. You can start immediately without any prior knowledge or specific preparation.

Assessment Methods

How your progress will be evaluated (3 methods)

assignments

Comprehensive evaluation of course material understanding

Written Assessment

tutor-marked assessments

Comprehensive evaluation of course material understanding

Written Assessment

final examination

Comprehensive evaluation of course material understanding

Computer Based Test

Career Opportunities

Explore the career paths this course opens up for you

Lab Technician

Apply your skills in this growing field

Science Teacher

Apply your skills in this growing field

Chemical Analyst

Apply your skills in this growing field

Environmental Technician

Apply your skills in this growing field

Quality Control Analyst

Apply your skills in this growing field

Industry Applications

Real-world sectors where you can apply your knowledge

Chemical ManufacturingPharmaceuticalsEnvironmental MonitoringFood ScienceHealthcare

Study Schedule Beta

A structured 13-week journey through the course content

Week
1

Module 1:

8h

Unit 1: Elementary Units in Chemical Reactions

4 study hours
  • •Define atoms, molecules, elements, and compounds.
  • •Differentiate between atoms and molecules, as well as elements and compounds.
  • •Explain why matter is said to be electrical in nature.
  • •State the postulates of Dalton's atomic theory and explain modifications to it.
  • •List and give relative masses and charges of the subatomic particles.
  • •State the laws of chemical combinations.
  • •Write chemical symbols and formulae for common elements and compounds.
  • •Determine chemical formulae from experimental data.
  • •Write and balance simple chemical equations.

Unit 2: Electronic Configuration 1 – Static Model

4 study hours
  • •Discuss the scientific evidences for the electrical nature of the atom.
  • •Give the number of subatomic particles in atoms of given elements.
  • •Recall the relative masses and charges of the subatomic particles.
  • •Define isotope
  • •Explain the nuclear model of the atom proposed by Rutherford.
  • •State the limitations of Rutherford's theory.
  • •Explain the origin of electronic energy levels in atoms.
  • •Write electronic shell configuration for elements and ions.
Week
2

Module 1:

8h

Unit 3: The Nucleus And Radioactivity

4 study hours
  • •State some empirical observations suggesting that neutrons are partly responsible for nuclei stability.
  • •Define radioactivity.
  • •Balance nuclear reaction equation.
  • •List the three types of radiations from a radioisotope giving their relative charges and masses.
  • •Show the path of nuclear radiations in an electric field.
  • •Define fusion and fission
  • •List some uses of radioactivity.
  • •Explain why radioactive wastes are dangerous.

Unit 4: Chemical Bonding 1: Electrovalent, Covalent and Co-Ordinate Covalent

4 study hours
  • •Explain electrovalent and covalent bonding.
  • •Write electron dot formulae for compounds.
  • •List properties of electrovalent and covalent compounds.
  • •State the octet rule.
  • •Explain the importance of noble gas configuration on chemical bonding.
  • •Predict the type of bonds between atoms.
  • •Explain the difference between covalent and co-ordinate covalent bonding.
Week
3

Module 1:

4h

Unit 5: Chemical Bonding II: Metallic and Intermolecular Bonding

4 study hours
  • •Explain metallic bonding.
  • •Account for metallic properties.
  • •List metallic properties.
  • •Explain dipole-dipole interaction.
  • •Account for properties of covalent compounds.
  • •Explain hydrogen bonding.
  • •Account for the high boiling point of water compared to hydrogen sulphide.
Week
4

Module 2:

8h

Unit 1: Periodic Table I: Classification of Elements

4 study hours
  • •Identify the groups and periods of elements in the periodic table.
  • •List the first few members of each group.
  • •Identify the blocks of elements.
  • •State general trends of some characteristics of elements.

Unit 2: Electronic Configuration II: Atomic Orbital Model

4 study hours
  • •Describe the quantum theory of atomic orbitals.
  • •Illustrate the shapes of the electron clouds corresponding to s and p - orbitals.
  • •Write electronic configurations of atoms based on the orbital model.
  • •Relate the electron configuration of atoms to the classification of elements in the periodic table.
Week
5

Module 2:

8h

Unit 3: Periodic Table II: Gradations of Atomic Properties

4 study hours
  • •Explain the general trend in periodic properties down a group and across a period based on electronic configuration.
  • •Define atomic radii, ionic radii, ionization energy electron affinity and electronegativity.
  • •Explain the trend of the above properties within the periodic table.

Unit 4: Mole Concept 1

4 study hours
  • •Define the mole.
  • •Recall avogadro number.
  • •Calculate molar mass tan formula mass.
  • •Calculate percentage of elements in compounds with given formulae.
  • •Establish mole ratios of reactants and products in reaction.
  • •Calculate yield and percentage yield.
  • •Recall molar volume of gas at s.t.p.
  • •Use the above in calculations involving gases.
Week
6

Module 2:

4h

Unit 5: Acids, Bases and Salts: General Properties

4 study hours
  • •Define acid, base and salt.
  • •Describe some methods of preparation of each.
  • •List some properties and uses of each.
  • •Explain hygroscope, deliquescence and efflorescence.
  • •Differentiate between a weak and a strong acid.
  • •Explain, why acid/base solutions conduct electrically.
Week
7

Module 3:

4h

Unit 1: Carbon and Its Compounds

4 study hours
  • •Recognise the uniqueness of carbon as an element.
  • •Define allotropy and describe the various allotropic forms of carbon.
  • •Enumerate the important inorganic compounds of carbon.
  • •Describe the characteristics of some carbon compounds.
  • •Explain the carbon cycle
Week
8

Module 3:

4h

Unit 2: The Gas Laws (I): Boyle's And Charles' Laws And The General Gas Equations

4 study hours
  • •State the postulates of the kinetic molecular theory for gases.
  • •State the Boyle's and Charles' laws for gases.
  • •Illustrate Boyle's and Charles' laws graphically.
  • •Use the kinetic molecular theory to explain Boyle's and Charles' laws.
  • •Derive the general gas equation from Boyle's and Charles' laws.
  • •Carry out calculations based on the three gas laws.
  • •Explain the effect of temperature and pressure on the volume of a gas.
Week
9

Module 3:

4h

Unit 3: The Gas Laws II Dalton's, Graham's, Avogadro's And Gay Lussac's Laws

4 study hours
  • •Account for deviations of real gases from ideal behaviour.
  • •State the statement of the laws of dalton, graham, avogadro and gay lussac.
  • •What avogadro constant is and relate it to the mole.
  • •Use gay lussac's law to predict the volume of a gaseous product in a gas reaction.
  • •Apply the laws of dalton, graham, avogadro and gay lussac in simple calculations.
  • •Explain why gases diffuse faster than liquids and solids.
Week
10

Module 3:

4h

Unit 4: Liquids

4 study hours
  • •List some properties of liquids that make them resemble gases.
  • •Define saturated vapour pressure.
  • •List factors that affect the saturated vapour pressure of liquids.
  • •Define boiling and boiling point
  • •Define the term 'normal boiling point'.
  • •Describe a method to determine the boiling point of a liquid.
Week
11

Module 3:

4h

Unit 5: Solids

4 study hours
  • •List some use of solid matter.
  • •Identify the different classes of solids.
  • •List some properties of the different types of solids.
  • •Compare and contrast the properties of diamond and graphite.
  • •Describe a simple experiment to determine the melting point of a solid.
  • •Recall that the melting point is a criterion of purity.
Week
12

Review

6h

Module 1-3 Review

6 study hours
  • •Review all modules and units.
  • •Work on assignments.
  • •Prepare for tutor-marked assignments.
Week
13

Exam Preparation

6h

Final Revision

6 study hours
  • •Complete all assignments.
  • •Prepare for final examinations.
  • •Focus on key concepts and problem-solving techniques.

This study schedule is in beta and may not be accurate. Please use it as a guide and consult the course outline for the most accurate information.

Course PDF Material

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Study Tips & Exam Preparation

Expert tips to help you succeed in this course

1

Create flashcards for key definitions and chemical formulas from Units 1-5.

2

Practice balancing chemical equations from Unit 1 weekly.

3

Solve numerical problems related to gas laws (Units 13-15) using different formulas.

4

Create concept maps linking Units 7-9 periodic table trends and electronic configurations.

5

Review all tutor-marked assignments (TMAs) and focus on areas where you lost marks.

6

Allocate specific time slots for each topic based on its weightage in the syllabus.

7

Form a study group to discuss challenging concepts and practice problem-solving together.

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