1. Chapter 1 Matter and Change a) Matter and Its Properties. a) Matter and Its Properties. b) Elements. a) Matter and Its Properties. a) Matter and Its Properties. b) Elements.

2. Chemistry It is the study of the composition, structure and properties of matter and the changes it undergoes. It is the study of the composition, structure and properties of matter and the changes it undergoes. Instruments are used for observations and measurements in microstructures, helping to explain the behavior of macrostructures. Instruments are used for observations and measurements in microstructures, helping to explain the behavior of macrostructures.

3. Branches of Chemistry Chemistry Organic Chemistry Inorganic Chemistry Physical Chemistry Analytical Chemistry Biochemistry Theoretical Chemistry

4. Important Definitions Mass: It is a measure of the amount of matter in an object. Mass: It is a measure of the amount of matter in an object. Matter: Anything that has mass and volume. Matter: Anything that has mass and volume. Weight: The forced produced by gravity acting on mass. Weight: The forced produced by gravity acting on mass. Volume: The space an object occupies. Volume: The space an object occupies. Atom: Smallest unit of an element that keeps the properties of that element. Element: Pure substance made of only one kind of atom. Element: Pure substance made of only one kind of atom. Compound: Substance made of atoms of two o more elements chemically bonded. Compound: Substance made of atoms of two o more elements chemically bonded. Molecule: Smallest unit of an element or compound with all of the properties of that element or compound. Molecule: Smallest unit of an element or compound with all of the properties of that element or compound.

5. Properties of Matter  Extensive Properties Depend on the amount of matter present. Depend on the amount of matter present. Examples: Examples: - volume - volume - mass - mass - amount of energy - amount of energy  Intensive Properties Do not depend on the amount of matter present. Examples: - melting point - density - heat - ability to conduct electricity

6. States of Matter State State  Solid  Liquid  Gas  Plasma Characteristics: High density Density little affected by pressure Holds its own shape in a container High density Density little affected by pressure Adopt the shape of its container Low density Density depends on pressure Expands to fill its container Low density Density depends on pressure Expands to fill its container Exists only at high temperatures

7. Changes of Matter  Physical Changes: Change in a substance that does not involve change in the identity of the substance. Examples: Change of state Boiling a material Melting a substance Cutting  Chemical Changes: Change in a substance that transform it into different substances. Examples: Burning charcoal in air Oxidation of iron in air Decomposition of mercury oxide

8. Important Definitions Chemical Reaction: The process by which elements and /or compounds interact with one another to form new substances. Chemical Reaction: The process by which elements and /or compounds interact with one another to form new substances. It is represented by a chemical equation. Reactant 1 + Reactant 2 → Product 3 + Product 4 Endothermic reactions: Reactions that absorb energy. Exothermic reactions: Reactions that release energy.

9. Law of Conservation of Matter Matter is neither created nor destroyed in any process. Matter is neither created nor destroyed in any process. The total mass does not change during any chemical reaction. The total mass does not change during any chemical reaction.

10. Important Definitions Pure Substance: All samples has exactly the same Pure Substance: All samples has exactly the same composition and the same characteristic properties. Element: It can not be broken down into simpler elements. Compounds: It can be decomposed into simpler compounds or elements. Mixture: It is a blend of two or more kinds of matter, with their own identity and properties. Components can be separated. Homogeneous Mixture: Uniform composition. Ex: NaCl + H 2 O Heterogeneous Mixture: Not uniform composition. Ex: Clay + H 2 O

11. Types of Homogeneous Mixtures Gas - Gas Gas - Gas Liquid - Gas Liquid - Gas Gas - Liquid Gas - Liquid Liquid -Liquid Liquid -Liquid Solid - Liquid Solid - Liquid Solid - Solid Solid - Solid Carbon dioxide and oxygen in nitrogen. Water vapor in air. Carbon dioxide in water. Acetic acid in water. Sodium chloride in water. Copper in silver.

12. Types of Separation of Mixture Homogeneous Homogeneous  Distillation  Crystallization  Chromatography Heterogeneous  Filtration  Condensation  With a magnet

13. Introduction to the Periodic Table General Information : Chemical Symbol Name Atomic Number Average Atomic Mass Electron Configuration Element Arrangement in the Periodic Table Groups or Families: Each element in the vertical columns has similar chemical properties. Periods: The physical and chemical properties of the elements in a row change regularly across the period. There are seven periods. The last two sets or elements are called Lanthanide and Actinide Series.

14. Types of Elements Elements MetalsNonmetalsMetalloids Noble Gases

15. Important Characteristics Nobel Gases: Generally unreactive Gases at room temperature Metals: Good Metals: Good conductors of heat and electricity Solids at room temperature except Hg Malleable and ductile, but some are brittle Silvery or grayish white luster. Nonmetals: Poor conductors of heat and electricity Many are gases at room temperature except bromine Brittle rather than malleable and ductile Low conductivity of heat and electricity. Metalloids: Elements with some characteristics of metals and nonmetals Solids at room temperature Less malleable than metals but not as brittle as nonmetals Semiconductors of electricity.