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
0/4
Introduction
States of Matter
Physical and Chemical Properties and Changes
The Gas Laws
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
0/3
Introduction
Atomic Structure
Atomic Structure of Isotopes
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
0/3
Introduction
Families of the Periodic Table
The Periodic Trends
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
0/4
Introduction
Electronic Configuration of S-Block Elements
Physical Properties of S-Block Elements
Chemical Properties of S-Block Elements
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
0/2
Introduction
Types and Properties of Chemical Bonds
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
0/6
Introduction
Measuring Equilibrium Rates
Equilibrium Basics
Types of equilibria
Predicting The Direction of a Reaction
Factors Affecting equilibrium
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
0/10
Introduction
Functional Groups
Alkanes
Alkenes and Alkynes
Alkanols(Alcohols)
HaloAlkanes
Alkanals and Alkanones
Carboxylic Acids
Esters
Amines
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
Introduction
Properties Of Acids And Bases
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
0/5
Introduction
Neutral, acidic and basic solutions
PH and Its Importance
Determination Of PH
Buffer Solutions
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
0/5
Introduction
Types of Samples and Sampling
Sample preparation
Sample Losses During Preparation
Sample Identification and Storage
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
Introduction
Separation Techniques
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
0/1
Heating and Cooling Techniques used in the lab
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
0/3
Introduction
Types of Distillation Techniques 
Distillation and Reflux Condensers
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
0/1
Crystallization Technique
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
0/1
Introduction
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
0/6
Introduction to Chromatography Techniques
Types of Chromatography Techniques
Thin Layer Chromatography
Column Chromatography
Retardation Factor (Rf)
Gas-Liquid Chromatography
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
Introduction
Requirements For Titrimetric Analysis
Titration procedure:
Molarity
Apparatus for titrimetric analysis
Classification Of Reactions In Titrimetrlc Analysis
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.
0/5
Introduction
The oxidation number 
Balancing Redox Reactions
Examples Of Redox Titration
Standardization of Redox solutions
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 .
0/5
Introduction to Complexiometric Titration
EDTA titration
Types of EDTA titrations
EDTA titration experiment 
Mechanism of action of indicator:
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
Introduction
Principles Of Gravimetric Analysis
Determination of Mass in gravimetric analysis
Factors Affecting Separation Of Metals And Compounds
Preparation of pure precipitates
Example of gravimetric Analysis
Gravimetric Calculations
Draft Lesson
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
Introduction
Calorimetry
Heat Capacity
Enthalpy of Phase Transitions
Chemistry Techniques for Science Laboratory Technicians
About Lesson

Views: 125

Physical and Chemical  Properties and Changes

Physical properties can be observed or measured without changing the composition of matter. Physical properties are used to observe and describe matter. Physical properties of materials and systems are often described as intensive and extensive properties. This classification relates to the dependency of the properties upon the size or extent of the system or object in question.

An intensive property is a bulk property, meaning that it is a physical property of a system that does not depend on the system size or the amount of material in the system. Examples of intensive properties include temperature, refractive index, density, and hardness of an object. When a diamond is cut, the pieces maintain their intrinsic hardness (until their size reaches a few atoms thick). In contrast, an extensive property is additive for independent, non-interacting subsystems. The property is proportional to the amount of material in the system.

Intensive properties: A physical property that will be the same regardless of the amount of matter.

  • density: ρ=mvρ=mv
  • color: The pigment or shade
  • conductivity: electricity to flow through the substance
  • malleability: if a substance can be flattened
  • luster: how shiny the substance looks

Extensive Properties: A physical property that will change if the amount of matter changes.

  • mass: how much matter in the sample
  • volume: How much space the sample takes up
  • length: How long the sample is

Physical Change

Change in which the matter’s physical appearance is altered, but composition remains unchanged.

A physical change takes place without any changes in molecular composition. The same element or compound is present before and after the change.The same molecule is present through out the changes. Physical changes are related to physical properties since some measurements require that changes be made. The three main states of matter are: Solid, Liquid, Gas

  • Solid is distinguished by a fixed structure. Its shape and volume do not change. In a solid, atoms are tightly packed together in a fixed arrangement.
  • Liquid is distinguished by its malleable shape (is able to form into the shape of its container), but constant volume. In a liquid, atoms are close together but not in a fixed arrangement.
  • Gas is made up of atoms that are separate. However, unlike solid & liquid, a gas has no fixed shape and volume.

Physical properties are important in describing and identifying particular kinds matter. Physical properties are very useful in assessing the hazards and predicting the fates of  environmental pollutants.

An organic substance that readily forms a vapor (volatile organic compound) will tend to enter  the atmosphere or to pose an inhalation hazard.

A brightly colored water soluble pollutant may cause deterioration of water quality by adding water color

.Much of the health hazard of asbestos is its tendency to form extremely small diameter fibers that are readily carried far into the lungs and that can puncture individual  cells.

Several important physical properties of matter are density, color, solubility and Thermal Properties

Density (d) is defined as mass per unit volume and is expressed by the formula

          d = mass /volume

Density may be expressed in any units of mass or volume. The densities of liquids and solids  are normally given in units of grams per cubic centimeter (g/cm3, the same as grams per milliliter, g/ml

The volume of a given mass of substance varies with temperature, so the density is a  function of temperature.

This variation is relatively small for solids, greater for liquids, and very high for gases.

The temperature-dependent variation of density is an important property of water and results  in stratification of bodies of water, which greatly affects the environmental chemistry that  occurs in lakes and reservoirs.

The combined temperature/pressure relationship for the density of air causes air to become  stratified into layers, particularly the troposphere near the surface and the stratosphere from about 13 to 50 kilometers altitude.

Specific Gravity

Often densities are expressed by means of specific gravity defined as the ratio of the density of a substance to that of a standard substance. For solids and liquids, the standard substance is usually water; for gases it is usually air. For example, the density of ethanol (ethyl alcohol) at 20˚C is 0.7895 g/ml.

 The specific gravity of ethanol at 20˚C referred to water at 4˚C is given by

  • Specific gravity = density of ethanol   = 0.7895 g/ml    = 0.7895
  •                                 Density of water         1.000 g/ml

For an exact value of specific gravity, the temperatures of the substances should be specified. In this case the notation of specific gravity of ethanol at 20˚/4˚ C shows that the specific gravity is the ratio of the density of ethanol at 20˚C to that of water at 4˚C

Color is one of the more useful properties for identifying substances without doing any chemical or physical tests. A violet vapor, for example, is characteristic of iodine. A red/brown gas could well be bromine or nitrogen dioxide (NO2 ) A characteristic yellow/brown color in water may be indicative of organically bound iron.  Solutions are colored because of the light they absorb.

Red, orange, and yellow solutions absorb violet and blue light; purple solutions absorb green and yellow light; and blue and green solutions absorb orange and red light. Solutions that do not absorb light are colorless (clear); solids that do not absorb light are white

Changing states of matter

Matter can be changed from one state to another by changing it physically or chemically. The following are the important processes that facilitate changes in states of matter.

Melting

Melting occurs when heat is applied to a solid. The solid matter’s particles start to vibrate rapidly and move apart from each other. This process increases the distance between them. Once specific temperature and pressure conditions are achieved, the solid transforms into a liquid. This specific point is known as the solid’s melting point.

Different solids have different melting points. For instance, the melting point of ice (solid water) is above zero degrees Celsius (32 degrees Fahrenheit) at sea level. However, the melting point of solid oxygen is -218.4 degrees Celsius.

Freezing

Freezing occurs when heat is removed from the liquid, causing its particles to slow down and settle in one location. When the liquid reaches a specific temperature known as its freezing point, it transforms into a solid. For instance, in most cases, fresh water freezes at zero degrees Celsius (32 degrees Fahrenheit). Sea water has a lower freezing point due to its salt content.

Sublimation

Sublimation is a process in which a solid is converted directly into a gas, without going through the liquid phase. It is achieved by either increasing the temperature of the substance beyond the boiling point or by freeze-drying it by cooling it under vacuum conditions.

One common example of a solid that converts into a gas via sublimation is carbon dioxide. At room temperate and pressure, solid carbon dioxide is converted into its gaseous form, known as dry ice.

Vaporization

Vaporization is the process of converting a liquid to a gas, either by evaporation or boiling. Since the liquid particles constantly collide with each other, energy is transferred to particles near the surface. When enough energy gets transferred, some particles are removed from the substance as free gas particles. The temperature and pressure conditions under which a liquid becomes a gas is known as its boiling point.

Condensation

Condensation happens when a gas is transformed into a liquid. For instance, when water vapor — a gas — reaches its dew point, it condenses into liquid water called dew.

Deposition

Deposition is a process where a gas gets transformed directly into a solid, without going through the liquid phase. In this sense, deposition is the opposite reaction of sublimation. Deposition usually occurs when the air touching the solid is cooler than the   rest of the air. This is what happens when water vapor is transformed directly into ice as frost

Chemical Properties and Changes

Chemical properties of matter describes its “potential” to undergo some chemical change or reaction by virtue of its composition. What elements, electrons, and bonding are present to give the potential for chemical change. It is quite difficult to define a chemical property without using the word “change”. Eventually you should be able to look at the formula of a compound and state some chemical property. At this time this is very difficult to do and you are not expected to be able to do it. For example hydrogen has the potential to ignite and explode given the right conditions. This is a chemical property. Metals in general have they chemical property of reacting with an acid. Zinc reacts with hydrochloric acid to produce hydrogen gas. This is a chemical property.

Chemical change results in one or more substances of entirely different composition from the original substances. The elements and/or compounds at the start of the reaction are rearranged into new product compounds or elements. A CHEMICAL CHANGE alters the composition of the original matter. Different elements or compounds are present at the end of the chemical change. The atoms in compounds are rearranged to make new and different compounds.

Join the conversation
Previous
Next

You cannot copy content of this page