Course Content
Introduction to Environmental Chemistry
Environmental chemistry is the study of the chemical and biochemical phenomena that occur in nature. It involves the understanding of how the uncontaminated environment works, and which naturally occurring chemicals are present, in what concentrations and with what effects. Environmental chemistry; is the study of sources, reactions, transport, effects and fate of chemical species in water, soil and air environment as well as their effects on human health and natural environment
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Introduction
Origin of the solar System
Cosmology; is the branch of astronomy involving the study of the of the universe and the solar system. Cosmo-chemistry ;( chemical cosmology); is the study of chemical composition of the matter in the universe and the process that led to those compositions The solar system is made up of the sun (a star) with nine planets orbiting around it. These planets together with all the other heavenly bodies moving around or between individual planet form members of the solar system. Other heavenly body include; asteroids, comets, meteors, meteorites and satellites such as moon. The solar system does not include other stars .
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Origin of The Universe and Solar System
Solutions
Solutions are defined as homogeneous mixtures that are mixed so thoroughly that neither component can be observed independently of the other. The major component of the solution is called solvent, and the minor component(s) are called solute.
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Introduction
Solubility of Solutions
Solubility Product
Solution Concentrations
Chemical Equilibria
Chemical equilibrium in the environment refers to the state where the rates of forward and reverse reactions of a chemical reaction reach a balance. In this state, the concentrations of reactants and products remain constant over time, although the reactions continue to occur.
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Introduction
The Concept of Equilibrium
Relation Between Chemical Kinetics and Chemical Equilibrium
Factors Affecting Chemical Equilibrium
Laws of Chemical Equilibria
Phase Interactions
Phase interactions in solutions refer to the behavior and changes that occur when two or more substances (solutes and solvents) mix together to form a homogeneous mixture. These interactions are related to the different phases of matter, such as solids, liquids, and gases, and how they interact and transform during the process of solution formation.
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Introduction
 Phase interactions
Colligative Properties of Solutions
COLLIGATIVE PROPERTIES OF SOLUTIONS Colligative properties are physical properties of solutions that depend on the concentration of solute particles, rather than the specific identity of the solute. The four colligative properties that can be exhibited by a solution are: 1.Boiling point elevation 2.Freezing point depression 3.Relative lowering of vapour pressure 4.Osmotic pressure
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Introduction
Colligative Properties Examples
Introduction To Organic Chemistry
Organic chemistry is the study of carbon containing compounds and their properties. This includes the great majority of chemical compounds on the planet, but some substances such as carbonates and oxides of carbon are considered to be inorganic substances even though they contain carbon.
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Introduction
The IUPAC Naming (nomenclature) 
Alkyl halides, Alkenes and Alkynes
Alcohols , Ethers, Aldehydes and Ketones
Carboxylic Acids, Esters and Amines
Simple Organic Molecules in the Environment
Soil Chemistry and Pollution
soil
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Introduction to Soil Chemistry
Chemical Characteristics of Soil
Biological Characteristics of Soil
Physical Characteristics of Soil
Soil Salinity, Conductivity and Ion Exchange Capacity
Soil Pollution
Water Chemistry and Polution
Water Chemistry
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Water and the Environment
Water Chemistry
Characteristics and Properties of Water
Portable water 
Water pollution
Water Quality Analysis
Biological Oxygen Demand (BOD)
Chemical Oxygen Demand (COD)
Air Quality and Pollution
Air Quality and Pollution
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Air Quality
Testing Air Quality
Biodegradation
Biodegradation
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Biodegradation
Mechanisms of Biodegradation 
Role of Microorganisms in Biodegradation
BioGeoChemical Cycles
BiogeoChemical Cycles
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Biogeochemical cycles
The Water Cycle
The Carbon Cycle
The Nitrogen Cycle
The Phosphorus Cycle
The Sulfur Cycle
Introduction To Environmental Chemistry
About Lesson

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SOLUTIONS

Solutions are defined as homogeneous mixtures that are mixed so thoroughly that neither component can be observed independently of the other. The major component of the solution is called solvent, and the minor component(s) are called solute.

If both components in a solution are 50%, the term solute can be assigned to either component. When a gaseous or solid material dissolves in a liquid, the gas or solid material is called the solute. When two liquids dissolve in each other, the major component is called the solvent and the minor component is called the solute.

Many chemical reactions are carried out in solutions, and solutions are also closely related to our everyday lives. The air we breathe, the liquids we drink, and the fluids in our body are all solutions. Furthermore, we are surrounded by solutions such as the air and waters (in rivers, lakes and oceans).

Types of Solutions

A mixture  is a substance that is composed of two or more substances.  Mixtures can be of two types: Homogeneous and Heterogeneous, where homogeneous mixtures combine so intimately that they are observed as a single substance, even though they are not. Heterogeneous mixtures, on the other hand, are non-uniform and have regions of the mixture that look different from other regions of the mixture.

Homogeneous mixtures can be further broken down into two classifications: Colloids and true  Solutions.

A colloid is a mixture that contains particles with diameters ranging from 2 to 500 nm. Colloids appear uniform in nature and have the same composition throughout but are cloudy or opaque. Milk is a good example of a colloid.

True solutions have particle sizes of a typical ion or small molecule (~0.1 to 2 nm in diameter) and are transparent, although they may be colored. This chapter will focus on the characteristics of true solutions.

Material exists in three states: solid, liquid, and gas. Solutions also exist in all these states:

Solid solution:

They contain two or more metals and are called alloys. they are formed  by melting the component metals and mixing them together then allowing them to cool.

Many alloys, ceramics, and polymer blends are solid solutions. Within a certain range, copper and zinc dissolve in each other and harden to give solid solutions called brass.

 Silver, gold, and copper form many different alloys with unique colors and appearances. Alloys and other solid solutions are important in the world of materials chemistry

Gaseous solution: they contain two or more gases (which do not react with each other) mixed together in a container to form a solution. The properties of gaseous solutions depend on the properties of its components . Gaseous mixtures are usually homogeneous and are commonly gas-gas solutions. The atmosphere is a gaseous solution that consists of nitrogen, oxygen, argon, carbon dioxide, water, methane, and some other minor components.  Some of these components, such as  water, oxygen, and carbon dioxide may vary in concentration in different locations on the Earth depending on factors such as temperature and  altitude.

Liquid solution: they have both the solute and solvents in liquid forms. liquid solutions can be said to be miscible or immiscible depending on the proportion they mix in each other. Miscible liquids mix evenly in all proportion whereas immiscible liquids cannot mix in any proportions e.g. oil and water

Aqueous solutions; these are solutions whose solvent is water. Substances dissolved in water are classified according to whether they yield ions or molecules. ionic compounds dissolve in water to give positive and negative ions which move freely in water making it possible for electric current to pass through and are hence called electrolytes. In contrast, solution containing neutral solute molecules do not conduct electricity because they do not have charged particles and are therefore said to be non-electrolytes

When molecules of gas, solid or liquid are dispersed and mixed with those of liquid, the homogeneous (uniform) states are called liquid solutions. Solids, liquids and gases dissolve in a liquid solvent to form liquid solutions.  In this chapter, most of the chemistry that we will discuss occurs in liquid solutions where water is the solvent..

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