Course Content
Matter
OBJECTIVES By the end of this topic, the trainee should be able to 1.Define matter 2.Explain state of matter 3.Distinguish between physical and chemical changes 4.Explain the gas laws
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Atoms , Elements and Compounds
OBJECTIVES By the end of this topic , the trainee should be able to; 1.Define Elements, Compounds and Mixtures 2.Describe the structure of an atom 3.Describe how to determine the Atomic number ,Mass number and Isotopes
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The Periodic Table
OBECTIVES By the end of this topic, the trainee should be able to : 1.State the historical contribution on development of the periodic table 2.Explain the periodic trends of elements and their compounds 3.State the diagonal relationships of the periodic table
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The S-Block Element
OBJECTIVES By the end of this topic, the trainee should be able to: 1.Explain the chemistry of group I and II elements 2.State the application of group I and two elements and their compounds
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Chemical Bonds
OBJECTIVES By the end of these topic, the trainee should be able to 1.Identify different types of bonds 2.Describe their properties
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Chemical Equilibrium
OBJECTIVES By the end of this topic , the trainee should be able to : 1.Define chemical equilibria 2.Explain types of equilibria 3.Determine equilibrium constant 4.Describe factors affecting chemical equilibrium
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Introduction To Organic Chemistry
By the end of this topic , the trainee should be able to : 1.Explain the aspects of organic chemistry 2.Describe hydrocarbons 3.Classify organic molecules explain chemical reactions of simple organic molecules 4.Explain the properties , synthesis and uses of simple organic molecules
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Acids, Bases and Salts
OBJECTIVES By the end of this session , the trainee should be able to : 1.State properties of acids and bases 2.Differentiate between strong and weak acids 3.Explain types and properties of salts
0/2
PH Analysis
OBJECTIVES By the end of this topic, the trainee should be able to: 1.Define the term PH 2.Explain the basic theory of PH 3.State the relationship between PH and color change in indicators 4.Explain the term buffer solution 5.Describe the preparation of buffer solutions 6.State the application of buffer solutions
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Sampling and Sample Preparation
OBJECTIVE By the end of this topic, the trainee should be able to : 1.Define the terms used in sample preparation 2.State the importance of sampling 3.Describe the techniques of sampling 4.Describe the procedure for sample pre-treatment 5.State sample storage methods
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Separation Techniques
OBJECTIVES By the end of this topic , the trainee should be able to : 1.Define separation, extraction and purification 2.Describe the separation , extraction and purification techniques 3.Explain the methods of determining purity of substances
0/2
Heating and Cooling Techniques
OBJECTIVES To identify various techniques used for heating and cooling substances in the laboratory
Heating and Cooling Techniques
OBJECTIVES To identify various techniques used for heating and cooling substances in the laboratory
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Distillation Techniques
By end of this topic, Trainee should be able to : 1. Define distilation 2. State and explain various distillation techniques 3. Outline Various distillation techniques 4. Outline the applications of Distillation techniques
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Crystallization Techniques
OBJECTIVES By the end of the topic, the learner should be able to: 1.To define crystallization 2.To describe crystallization process 3.To carry out crystallization procedure
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Solvent Extraction Techniques
OBJECTIVES By the end of the topic, the learner should be able to 1.Define solvent extraction 2.Explain terms used in solvent extraction 3.Describe methods of solvent extraction 4.Describe selection of appropriate solvents for solvent extraction 5.Determine distribution ration 6.Outline factors actors influencing the extraction efficiency 7.Describe Soxhlet extraction
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Chromatography Techniques
OBJECTIVES By the end of this topic, the learner should be able to: 1.Define chromatography techniques 2.Explain terms used in chromatography techniques 3.Describe principles of chromatography techniques 4.Explain types of chromatography techniques 5.Carry out chromatography experiments 6.Determine RF factor 7.Outline electrophoresis
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Titrimetric Analysis
OBJECTIVES By the end of this topic, the trainee should be able to: 1.Define terms used in titrimetric analysis 2.Describe types of titrimetric analysis 3.Balance chemical reactions 4.Work out calculations involved in titrimetric analysis
0/6
Redox Titration
Redox Titration is a laboratory method of determining the concentration of a given analyte by causing a redox reaction between the titrant and the analyte. Redox titration is based on an oxidation-reduction reaction between the titrant and the analyte. It is one of the most common laboratory methods used to identify the concentration of unknown analytes. Redox reactions involve both oxidation and reduction. The key features of reduction and oxidation are discussed below.
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Complexiometric Titration
omplexometric Titration or chelatometry is a type of volumetric analysis wherein the colored complex is used to determine the endpoint of the titration. The method is particularly useful for determination of the exact number of a mixture of different metal ions, especially calcium and magnesium ions present in water in solution .
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Gravimetric Analysis
OBJECTIVES By the end of this topic, the trainee should be able to: 1.Define gravimetric analysis 2.Describe the principles of gravimetric analysis 3.Describe the steps involved in gravimetric analysis 4.Explain factors affecting gravimetric analysis 5.Describe the equipments and apparatus used in gravimetric analysis 6.Carry out gravimetric analysis
0/8
Calorimetric Analysis
OBJECTIVES By the end of this topic, the trainee should be able to: 1.Define terms and units used in thermochemistry 2.Determine enthalpy changes in chemical reactions 3.Determine heat capacity and specific heat capacity 4.Compare calorific values of different materials 5.Determine different heat reactions 6.Apply law of conservation of energy and Hess law in thermochemical calculations
0/4
Chemistry Techniques for Science Laboratory Technicians
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HYDROCARBONS

These are compounds composed of carbon and hydrogen. They are generally insoluble in water although those with lighter molecular masses are gases and are slightly soluble. Examples of hydrocarbons include methane – the gas we burn as natural gas, propane (also called liquid petroleum gas) and petroleum jelly.

Hydrocarbons with single carbon-carbon bonds are referred to as being saturated whilst any hydrocarbon that contains a double bond is said to be unsaturated.

Saturated hydrocarbons are also called the alkanes, whilst the unsaturated hydrocarbons include both those molecules that contain carbon-carbon double bonds (referred to as the alkenes) and those that contain carbon-carbon triple bonds (referred to as the alkynes).

Alkanes and alkenes are natural products that have resulted from the decay of organiccompounds from plants and animals that lived millions of years ago. They are found today as petroleum, which are mixtures of hydrocarbons containing up to 30 or 40 carbon atoms. Different components of petroleum can be isolated by fractional distillation.

These hydrocarbons are good sources of fuels, the so-called „fossil fuels‟. As mentioned previously, the global production of such fossil fuels is 3 billion tonnes. As they are produced in such large quantities, pollution of the environment with these fossil fuels is of concern. The major route of entry into the environment isn‟t through spectacular disasters such as the oil spills from ships, but rather through our daily activities. Pumping fuel into cars, and oil spilled onto the road as a result of old faulty cars are major contributors.

ALKANES

This family of compounds consists of substances that contain only carbon and hydrogen joined by single bonds. They obey the general formula

                               CnH2n + 2

Thus if an alkane has six carbons, its formula will be C6H14. The simplest alkane is methane, CH4. Methane is also the most abundant organic species in the atmosphere. It is produced mainly by organisms breaking down organic material in places such as marshes, lake bottoms, land fills and the stomach of ruminant animals. Reactions of Alkanes

Because they are saturated compounds and because the C-C and C-H bonds are relatively strong, the alkanes are fairly unreactive, (e.g. at room temperature they do not react with acids, bases, or strong oxidising agents) which makes them invaluable as lubricants and the backbone of plastics.

At sufficiently high temperatures, alkanes react vigorously with oxygen. This is known as a combustion reaction and is the basis for their widespread use as fuels. An example is the reaction of butane with oxygen. The production of carbon dioxide in the environment is of concern because it has been implicated in the green house effect. Animals and plants produce carbon dioxide. Recently there has been an increase in carbon dioxide production brought about by a combination of deforestation and the burning of fossil fuels. (Plants use up carbon dioxide in photosynthesis, so removing vegetation is a good way to increase the amounts of carbon dioxide in the atmosphere). Carbon dioxide is thought to act like a blanket placed over the earth, it captures infrared radiation and transforms it into heat (The so-called “Green House Effect”). This may lead to an increase in the earth‟s temperature, which may cause a melting of the earth‟s ice caps. This could have potentially devastating effects, particularly for people who live in seaside cities.

Alkanes also under-go reactions induced by UV light. Examples include the slowbreakdown of plastics in the sun, and halogenation reactions (reactions where halogen atoms such as Cl, Br, or I replace H in the molecule).

These are compounds composed of carbon and hydrogen. They are generally insoluble in water although those with lighter molecular masses are gases and are slightly soluble. Examples of hydrocarbons include methane – the gas we burn as natural gas, propane (also called liquid petroleum gas) and petroleum jelly.

Hydrocarbons with single carbon-carbon bonds are referred to as being saturated whilst any hydrocarbon that contains a double bond is said to be unsaturated.

Saturated hydrocarbons are also called the alkanes, whilst the unsaturated hydrocarbons include both those molecules that contain carbon-carbon double bonds (referred to as the alkenes) and those that contain carbon-carbon triple bonds (referred to as the alkynes).

Alkanes and alkenes are natural products that have resulted from the decay of organiccompounds from plants and animals that lived millions of years ago. They are found today as petroleum, which are mixtures of hydrocarbons containing up to 30 or 40 carbon atoms. Different components of petroleum can be isolated by fractional distillation.

These hydrocarbons are good sources of fuels, the so-called „fossil fuels‟. As mentioned previously, the global production of such fossil fuels is 3 billion tonnes. As they are produced in such large quantities, pollution of the environment with these fossil fuels is of concern. The major route of entry into the environment isn‟t through spectacular disasters such as the oil spills from ships, but rather through our daily activities. Pumping fuel into cars, and oil spilled onto the road as a result of old faulty cars are major contributors.

ALKANES

This family of compounds consists of substances that contain only carbon and hydrogen joined by single bonds. They obey the general formula

                               CnH2n + 2

Thus if an alkane has six carbons, its formula will be C6H14. The simplest alkane is methane, CH4. Methane is also the most abundant organic species in the atmosphere. It is produced mainly by organisms breaking down organic material in places such as marshes, lake bottoms, land fills and the stomach of ruminant animals. Reactions of Alkanes

Because they are saturated compounds and because the C-C and C-H bonds are relatively strong, the alkanes are fairly unreactive, (e.g. at room temperature they do not react with acids, bases, or strong oxidising agents) which makes them invaluable as lubricants and the backbone of plastics.

At sufficiently high temperatures, alkanes react vigorously with oxygen. This is known as a combustion reaction and is the basis for their widespread use as fuels. An example is the reaction of butane with oxygen. The production of carbon dioxide in the environment is of concern because it has been implicated in the green house effect. Animals and plants produce carbon dioxide. Recently there has been an increase in carbon dioxide production brought about by a combination of deforestation and the burning of fossil fuels. (Plants use up carbon dioxide in photosynthesis, so removing vegetation is a good way to increase the amounts of carbon dioxide in the atmosphere). Carbon dioxide is thought to act like a blanket placed over the earth, it captures infrared radiation and transforms it into heat (The so-called “Green House Effect”). This may lead to an increase in the earth‟s temperature, which may cause a melting of the earth‟s ice caps. This could have potentially devastating effects, particularly for people who live in seaside cities.

Alkanes also under-go reactions induced by UV light. Examples include the slowbreakdown of plastics in the sun, and halogenation reactions (reactions where halogen atoms such as Cl, Br, or I replace H in the molecule).

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