2. Welcome to CP Chemistry!!!

3. Matter & Change

4. What is Chemistry? Chemistry: the study of the composition, structure, and properties of matter, and the changes matter undergoes

5. Branches of Chemistry: Organic Inorganic Physical Analytical Biochemistry Theoretical

6. Organic Chemistry -The study of carbon containing compounds from living or once living things Inorganic Chemistry -The study of non-carbon compounds, from non- living sources

7. Physical Chemistry -The study of properties, changes, and relationships between energy and matter Analytical Chemistry -Identification of the composition and components of matter

8. Biochemistry -Study of the chemical processes occurring within living things Theoretical Chemistry -The application of math and technology to predict the properties of matter

9. Matter: Matter- anything that has mass and takes up space Atoms- the smallest unit of an element that maintains the properties of the element Elements- a pure substance made of only one type of atom ex: O 2 (oxygen) Compounds- a substance made of 2 or more different elements that are chemically bonded ex: NaCl (table salt) *Molecules- compounds containing only covalent bonds ex: H 2 O (water)

10. Classifications of Matter Pure Substance- has a fixed composition Mixture- a blend of 2 or more different kinds of matter NOT BONDED together –Each substance in a mixture retains it ’ s original properties Ex: salt water, chocolate milk, salad dressing –The parts of a mixture can be physically separated Ex: centrifuge, filter, evaporation –Different from a pure substance because every sample of a mixture does not have the exact same composition

11. Types of Mixtures: Homogeneous Mixture- same throughout, 2 substances are equally mixed xoxo ex: kool-aid, salt water, chocolate milk oxox Heterogeneous Mixture- unequal distribution of molecules within a mixture ex: salad dressing, orange juice w/ pulp oooo xxxx

12. Properties of Matter Extensive Properties: depend on the amount of matter present –Examples: volume, mass Intensive Properties: do not depend on the amount of matter present –Examples: melting point, boiling point, density, conductivity

13. Properties of Matter Continued… Physical Properties: characteristics that can be observed or measured without changing the identity of the substance –Examples: melting point, boiling point, color Chemical Properties: relate to a substance’s ability to undergo changes that transform it into different substances –Examples: burning, rusting

14. Changes in Matter Physical Change: change that doesn’t involve changing the identity of the substance –Examples: cutting, phase change Chemical Change/Chemical Reaction: a change in which one or more substances are converted into different substances –Reactants –Products –Yields

15. The Periodic Table:

16. Groups(families)- Vertical columns on periodic table #1-18 –Elements in the same group share similar properties Periods- Horizontal rows on the periodic table –Trends exist across periods from L to R

17. Element Boxes C 6 12.01 Atomic # - # of protons or electrons in an atom Atomic Mass - # of protons + # of neutrons Symbol # of Neutrons = atomic mass – atomic # (round answer to whole #)

18. Types of Elements: - Properties, Characteristics, and Position on Periodic Table Metals: –Good conductors of heat and electricity Malleability- can be bent without breaking Ductile- can be drawn into a wire Luster- shiny Melting & Boiling Point- are high, except mercury (Hg) *Metals are found to the LEFT of the “ staircase ”

19. Types of Elements Continued… - Properties, Characteristics, and Position on Periodic Table Non-Metals: -Poor conductors of heat and electricity (insulators) -Many are gases at room temperature -Noble Gases- group 18 on the periodic table -are the least reactive elements -Ex. He, Ne, Ar, Kr, Xe, Rn *Non-Metals are found to the RIGHT of the “ staircase ”

20. Types of Elements Continued… - Properties, Characteristics, and Position on Periodic Table Metalloids: –Have characteristics of both metals and non- metals, are often semi-conductors –Ex: silicon(Si): conducts electricity well, does not conduct much heat *Metalloids boarder the “ staircase ”

21. Positions on Periodic Table

22. Measurements & Calculations

23. The Scientific Method: -a logical approach to problem solving Steps: 1)Make Observations 2)Form a Hypothesis 3)Conduct an Experiment 4)Collect and Analyze Data - Qualitative Data: non-numerical information - Quantitative Data: numerical information 5)Form Conclusions

24. S.I. Units: S.I.(Metric) System – international system of measurement Base Units: Length – meters (m) Mass – grams (g) Time – seconds (sec) Temperature – Celsius(ºC) or Kelvin(K) # of Particles – moles (mol)

25. Derived Units: Area- length x width (m 2 ) Volume- length x width x height (m 3 or L) Density- mass/volume (g/cm 3 ) Molar Mass- mass/moles (kg/mol) Concentration- moles/volume (mol/L)

26. Prefixes: 10 -9 = 1/1,000,000,000 = nano (n) 10 -6 = 1/1,000,000 = micro (µ) 10 -3 = 1/1,000 = milli (m) 10 -2 = 1/100 = centi (c) 10 -1 = 1/10 = deci (d) 1 = no prefix 10 3 = 1,000 = kilo (k) 10 6 = 1,000,000 = mega (M) 10 9 = 1,000,000,000 = giga (G) 10 12 = 1,000,000,000,000 = tera (T) Smaller Larger

27. Conversions: -Use conversion factors -Go through the base unit -Always show ALL of your work! ex: 5.0 kg  ____________ mg = 5,000,000 mg 24.3 mL  ____________ L = 0.0243 L 55.0 km/hr  __________ m/sec = 15.27 m/sec

28. Accuracy- is the closeness of a measurement to an accepted value Precision- is the closeness of a set of measurements to one another -All darts hit the bulls-eye -All darts land together

29. % Error: Accepted Value – Experimental Value ----------------------------------------------- x 100 Accepted Value ex: (23.5 – 21.4) / (23.5) x 100 = 8.94% error

30. ***SIGNIFICANT FIGURES*** # ’ s other than 0(zero) are ALWAYS significant ex: 123456789 Zeros sandwiched between non-zero # ’ s are significant ex: 12006.73 Zeros before the 1 st non-zero # are NEVER significant ex: 0.00012345 If there is a decimal, zeros to the RIGHT of the last non-zero are ALWAYS significant

31. Adding/Subtracting with “Sig Figs” When there are only whole numbers: The answer must have the same number of sig figs as the measurement with the fewest number of sig figs –Ex. 5400g + 365g = 5800g

32. Adding/Subtracting with “Sig Figs” Continued… When adding/subtracting with decimals: The answer must have the same number of digits to the RIGHT of the decimal as there are in the measurement with the fewest decimals. –Ex. 25.1g + 2.03g = 27.13g rounds to 27.1g –Ex. 2.5 + 1 = 3.5 rounds to 4

33. Multiplying/Dividing with “Sig Figs” The answer must have no more sig figs than the measurement with the fewest sig figs –Ex. 2.4 g/mL x 15.82mL = 38g

34. Scientific Notation- -a way of writing very large or very small # ’ s using exponents ex: 2,000,000,000 = 2.0 x10 9 ex: 0.0000000238 = 2.38 x10 -8

35. Proportions: Direct Proportions- equation(k=x/y) –Both variables increase or decrease at the same rate ex: Density (D=m/V) Inverse Proportions- equation(k=xy) –As one variable increases the other decreases ex: Speed of Light (c=ƒ£)

36. END OF CH 1&2 NOTES!!!