1. Introduction to Chemistry

2. Chemistry The study of the composition, structure, and properties of matter, the processes that matter undergoes, and the energy changes that accompany these processes.

3. Branches of Chemistry Organic – carbon containing compounds Inorganic – metals and anything not organic Physical – properties / changes / energy Analytical – identification and composition of materials Biochemistry – living things Theoretical – math & computers to understand

4. Research & Technology Basic Research – for the sake of knowledge Applied Research – to solve a problem Technological Development – improve quality of life

5. Matter is anything that has mass and takes up space.

6.  Mass is a measure of the amount of matter.  Volume is the amount of space an object occupies.

7. Building Blocks of Matter Atom – smallest unit of an element that maintains the chemical identity of that element. Element – pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom.

8. Compound – substance that can be broken down into simple stable substances. Each compound is made from the atoms of two or more elements that are chemically bonded.

9. Extensive Properties  Volume  Mass  Amount of energy depend on the amount of matter present.

10. Intensive Properties  Melting Point  Boiling Point  Density  Electrical Conductivity do not depend on the amount of matter present.

11. Physical Properties  Density  Color  Melting point can be observed or measured without changing the identity of a substance.

12. Chemical Properties  Flammability (tendency of a substance to burn in air)  Reactivity  Toxicity relate to a substance’s ability to undergo changes that transform it into a different substance.

13. Physical Changes  If it is still the same substance when you are done with it, it is a physical change.  Ex: Crushing, tearing, Evaporating Water (still H 2 O), any phase change.

14. Chemical Changes  If it is NOT the same substance when you are done with it, it is a chemical change.  Ex: Cooking or burning something, Rusting metal.

15. How Do You Know?  Chemical Change: Bubbling, color change, temperature change.

16.  Energy is always either used or given off in any physical or chemical change.  Energy cannot be created or destroyed (Law of Conservation of Energy). Energy

17. *Ask Yourself …  Has the change altered the identity of the substance?  If yes … Chemical Change  If no … Physical Change

18. States of Matter  Solid – definite shape and definite volume.

19. States of Matter  Liquid – indefinite shape but definite volume – takes shape of container.

20. States of Matter  Gas – no definite shape or volume – expands to fill container and takes shape of container.

21. States of Matter  Plasma – no definite shape or volume – a high temperature state where atoms lose most of their electrons.

22. States of Matter

23. Changes in State

24. Changes in Matter

25.  Mixture: A blend of two or more kinds of matter, each of which retains its own identity and properties. Can be separated.  Pure Substance: Has a fixed composition. Classification of Matter

26.  Compounds (Ex: water, sodium chloride, sucrose)  Elements (Ex: gold, aluminum, oxygen, chlorine) Pure Substances

27.  Homogeneous: same throughout (Ex: air, stainless steel, solutions like sugar-water)  Heterogeneous: not the same throughout (Ex: granite, wood, blood) *Mixtures

28.  Filtration – pour liquid through paper that catches solid and lets liquid pass through.  Can only be used on a heterogeneous mixture of a liquid and a solid. Separating Mixtures

29.  Distillation  Crystallization  Chromatography Separating Homogeneous Mixtures by……

30.  Chromatography – solution is separated by allowing it to flow along a stationary substance. Separating Homogeneous Mixtures

31.  Distillation – separates by different boiling points. Separating Homogeneous Mixtures

32.  Crystallization – boil off or evaporate off the liquid and you are left with the solid. *Separating Homogeneous Mixtures

33. Intro to Periodic Table

34.  Metals  Nonmetals  Metalloids Organizing the Squares  Groups or families – Vertical columns  Groups have similar chemical and physical properties.  Periods – Horizontal Rows

35.  Luster - shiny  Conduct Electricity & Heat  Malleable – hammered into thin sheets  Ductile – drawn into wire Properties of Metals

36.  No Luster – not shiny  Nonconductors  Brittle  Non-Ductile Properties of Non-Metals SULFUR Helium

37.  Also called semimetals  Have properties of both metals and non-metals.  B, Si, Ge, As, Sb Properties of Metalloids

38. Group Names  Alkali Metals  Alkaline Earth Metals  Transition Metals  Halogens  Noble Gases

39.  Inert Gases do not readily react.  Are gases at room temperature. *Noble Gases