1. Unit 1 - Introduction to Chemistry
What Matters?
1.A.2(b) – use appropriate SI units…describe the relationship among SI unit prefixes

2. SI Base Units 1.A.2(b) – use appropriate SI units…describe the relationship among SI unit prefixes
Length – meter
Mass – kilogram
Time – second
Temperature – Kelvin
Quantity of Matter – mole
Volume - liter
This will be on the test

3. SI Derived Units Combinations of base units
Ex – velocity = meters/second (m/s)
acceleration = meters/second ∙ second m/s2)
density = kg/m∙m∙m (kg/m3)

4. Non-SI Units Length – foot, mile, Mass – ounce
Temperature – Centigrade, Celsius, Fahrenheit
Volume - gallon

5. Commonly Used Prefixes
Centi- 1/100 or 0.01
Kilo or 1.0 x 103
Milli- 1/1000 or 0.001

6. States of Matter
II.B.1(a) – compare the definition of matter and energy and the laws of conservation of matter and energy

7. Matter Def- anything that has mass and occupies space
3 States of matter
Solid
Liquid
Gas

8. Solids, Liquids, and Gases
Solids – have both definite volume and shape
Liquids – have definite volume but not shape
Gases – have neither definite volume or shape
Particles have increasing velocity from solids to liquids to gases

9. II.B.2(c) – describe the phase and energy changes associated with them
Changes of State
II.B.2(c) – describe the phase and energy changes associated with them

10. Phase Changes Melting Freezing Vaporization/Evaporation Condensing
Sublimation
Deposition

11. Melting/Freezing Energy must be ADDED for a substance to melt
Energy must be REMOVED for a substance to freeze

12. Vaporization & Condensation
Energy must be ADDED for a substance to boil
Energy must be REMOVED for a substance to condense

13. Deposition/Sublimation
Energy must be ADDED for a substance to sublime
Energy must be REMOVED for a substance to undergo deposition

14. Law of Conservation of Energy
Energy cannot be created or destroyed
Energy of a reaction MUST be conserved

15. Law of Conservation of Matter
Matter cannot be created or destroyed
Mass of a chemical reaction MUST be conserved

16. Elements, Compounds & Mixtures
II.A.2(b) – compare the characteristics of elements, compounds and mixtures

17. Elements An element is matter in its simplest form
Cannot be broken down by chemical means
Periodic Table (118 elements)

18. Compounds Are combinations of elements Have the same composition
Can be broken down by chemical means

19. Mixtures Have variable composition
Can be separated physically or chemically
Homogeneous Mixtures – are the same throughout
Heterogeneous Mixtures – have different regions

20. Separatory Techniques
IV.A.1(b) – describe and perform common separation techniques

21. Filtration Used for separating undissolved solids
Pour through a mesh (filter paper)

22. Distillation Used to separate dissolved solids or liquid mixtures
Uses physical changes

23. Chromatography
Uses chemicals to separate the pigments of plant or chemicals
Various Methods
Gas chromatography
Liquid chromatography
Thin-layer chromatography
Ion-exchange chromatography

24. Chemical vs Physical
II.B.1(e) – define chemical and physical properties and compare them by providing examples

25. Physical Properties Physical Properties… Odor Color Volume State
Can be observed without changing a substance into another substance.
Boiling point, density, mass, volume, etc.
Odor
Color
Volume
State
Density
Boiling point
Melting point

26. Chemical Properties Chemical Properties… Wood burning Iron rusting
Can only be observed when a substance is changed into another substance.
Flammability, corrosiveness, reactivity with acid, etc.
Wood burning
Iron rusting
Digestion
photosynthesis

27. Chemical and Physical Changes
II.B.1(d) – explain the difference between chemical and physical changes and demonstrate how these changes can be used to separate mixtures and compounds into their components

28. Physical Change
These are changes in matter that do not change the composition of a substance.
Changes of state, temperature, volume, etc.

29. Chemical Change Chemical changes result in new substances.
Combustion, oxidation, decomposition, etc.

30. Indicators of Chemical Change
Formation of a gas (bubbles)
Formation of a precipitate (solid)
Change in temperature
Exothermic
Endothermic
Color change

31. Properties
Extensive Properties – depend on the amount of substance present
Volume
Mass
Energy present
Intensive Properties – do NOT depend on the amount of substance present
Melting point
Boiling point
Density
Conductivity

32. Elements & The Periodic Table
Periods – horizontal rows
Groups – vertical columns
Group 1A – alkalai metals
Group 2A – alkalai earth metals
Group 3A-12A – transition metals
Group 16A – chalcogens
Group 17A – halogens
Group 18A – noble gases

33. Group 1 – Alkali Metals

34. Group 2 – Alakali Earth Metals

35. Transition Metals

36. Chalcogens

37. Halogens

38. Noble Gases

39. The Periodic Table

41. Metals
Conduct heat and electricity
Malleable
Ductile
Luster (shiny)

42. Non-metals Poor conductors of heat Poor conductors of electricity
Many are gases at room temp
5 solid non-metals
Phosphorous
Sulfur
Carbon
Selenium
Iodine

43. Metalloids
Have some characteristics of both metals and non-metals

44. Noble Gases
Least reactive of all elements
All gases at room temp