1. 1.1 What is Chemistry? Pg 4-9

2. Objectives Describe ways in which Chemistry is part of your life. Describe characteristics of three common states of matter. Describe physical and chemical changes, giving examples. Identify reactants and products in chemical reactions. List observations which imply a chemical change.

3. Chemicals Chemical – any substance that has a definite composition or make up. – Water, Carbon Dioxide, ATP, DNA, etc. Are chemicals bad?

4. Reactions Chemical Reaction – the process by which one or more substances change to produce one or more different substances. Physical Change – a change in the physical characteristics of a chemical such as size, shape, temperature, state, or texture. The chemical remains unchanged.

5. States of Matter Liquid – has a fixed volume but not a fixed shape. Gas – has neither a fixed volume nor a fixed shape. Solid – has a fixed volume and a fixed shape.

6. Chemical Changes Reactant – substances that you begin with before a chemical reaction. Product – substances that you end up with after a chemical reaction.

8. Evidence of Chemical Reactions Gas – if a gas is produced, often observed from bubbling or a change in odor. Formation of a Precipitate – if after mixing two clear substances the solution becomes cloudy a precipitate has formed. Endothermic/Exothermic – the release or absorption of energy (change in temp or giving off light).

12. 1.2 Describing Matter Pg 10-19

13. Objectives Distinguish between different characteristics of matter, including mass, volume and weight. Identify and use SI units in measurements and calculations. Set up conversion factors and use them in calculations. Identify and describe physical properties, including density. Identify chemical properties.

14. Definitions Matter – Anything that has mass and volume. Mass – the quantity of matter contained in an object. Weight – the force gravity exerts on a mass. Volume – the space an object occupies. Quantity – something that has magnitude, size, or amount. Unit – a quantity adopted as a standard of measurement.

15. Base SI Units

16. Derived Units Derived Units – any unit that can be found by multiplying or dividing any of the seven base SI units together. – EX – m/s, m/s^2, N, J, or mass/volume …

17. Density Density – The amount of mass per unit volume. (g/cm^3, kg/m^3), etc.) Iridium Osmium

20. Using SI Units and Prefixes Combining any SI Base Unit with a prefix only changes the magnitude (size) of the unit. – Exs: a gram is the SI Base unit of mass. A kilogram (kg) is 1,000 times larger than a gram. A gigagram (Gg) is 1,000,000 times larger than a gram, and a yottagram (Yg) is 1,000,000,000,000,000,000,000,000 times larger than a gram.

21. Dimensional Analysis You can multiply and divide by conversion factors in order to cancel out units and convert from any given SI base to another. – Ex: Convert 1 second to centiseconds.

22. Significant Digits Significant Digits – the valid digits in a measurement. – Ex: You measure a pen to be 12.6 cm long with a ruler which has only cm markings. Therefore, it has three digits all of which are significant. Two which you are certain of, and one which you estimated.

23. A digit 1 through 9 is always significant, in any single number. A 0 can be significant or insignificant: – Significant: 102 or 13.01 or 12.0 – Insignificant: 120 or 100,000,000,000 or 1.2x10 23 How many digits are significant? – 12 – 10,003 – 1.650 – 1300

24. Chemical and Physical Properties Physical – a property that can be determined without changing the nature of the substance. Chemical – a property of matter that describes a substance’s ability to participate in chemical reactions.