I have learned about:

1. I have learned about: Scientific notation significant figures metric system classification of matter physical properties of matter chemical properties of matter phases of matter

2. I have learned about: Law of conservation of mass Periodic Table Basics Temperature Heat Specific Heat Heat Equation

3. I have learned about: Atoms (protons, neutrons, e-) Ions Isotopes Average atomic mass e- configurations ground state excited state Bright line spectra

4. 1 2 11 10 100 1000 1000. One sig fig One sig fig Two sig figs One sig fig One sig fig One sig fig four sig figs Significant Figures

5. 1200 1200. 1263 1207 two sig figs four sig figs four sig figs four sig figs Significant Figures

6. 0.1 0.01 0.0004 0.203 0.62397 0.00694 one sig fig one sig fig one sig fig three sig figs five sig figs three sig figs Significant Figures

7. 56.2 56.007 56.0 56 50.00 3 5 3 2 4 Significant Figures

8. Sig Figs in Scientific Notation 5.347 x 10 16 5.347 4 sig figs 5.000 x 10 -6 5.000 4 sig figs 5 x 10 -6 5 1 sig fig

9. Multiplying with Sig Figs

10. Adding with Sig Figs

11. Classification of Matter

12. States of Matter GAS LIQUID SOLID

13. Physical Properties of Matter The properties of a substance that can be demonstrated without changing the composition of the substance Size (length, volume) Density Mass Color

14. Physical Properties Melting Point Ex. Ice (solid water) starts to melt to liquid water at 0 degrees Celsius Boiling Point Ex. Water boils into steam at 100 degrees Celsius

15. Physical Properties Malleability: can be pounded into a new shape without breaking Metals are malleable

16. Physical Properties Iron is malleable Fe

17. Physical Properties Ductility Can be pulled into long wires without breaking Metals are ductile

18. Physical Properties Crystal Shape Reflects the regular arrangement of atoms in the solid

19. Physical Change A change in the sample of matter that does not result in a NEW substance: Phase Changes Changes in shape Solid liquid gas

20. Chemical Properties of Matter How matter behaves when it changes into a NEW substance. EX. Iron rusts silver tarnishes Milk sours sugar ferments eggs rot leaves turn paper burns

21. Chemical Change Substance changes into a NEW substance. This change is often an irreversible and permanent change in composition

22. Burning

23. Tarnishing

24. Rusting

25. Oxidizing

27. Chemical Reaction Chemical changes mean a chemical reaction has occurred REACTANTS PRODUCTS old substances become new substances Sodium + Chlorine sodium chloride (table salt) Na + CL NaCL

28. Classify the following samples:

29. Classify the particles of matter

30. Identify the following changes as Physical or Chemical

31. Identify the following changes as Physical or Chemical Fe

32. Identify the following changes as Physical or Chemical

33. Periodic Table Review • Elements are arranged according to______ • Vertical columns are called________ • Horizontal rows are called ________ • There are ______ periods in the table • Most elements are classified as _____ • Where are the transition metals? • What are the metalloids?

34. Units of Energy Energy is measured in JOULES Also in calories or kilocalories (food) How many calories are in a kilocalorie?

35. What is temperature? A measure of the average kinetic energy of the particles in a sample of matter. All atoms are moving! High temperature = moving faster

36. Once again…… TEMPERATURE = AVERAGE KINETIC ENERGY

37. Temperature Scales Kelvin: 0 K = absolute zero (-460 oF) all motion of particles stops! Water freezes @ 273 K Water boils @ 373 K Kelvin never goes below zero (no negative numbers!)

38. Temperature Scales Kelvin = Celsius + 273 Celsius = Kelvin – 273 If it is 32O Celsius, what temperature is it in Kelvin? If it is 100 Kelvin, what temperature is it in Celsius?

39. What is Heat? Heat is the sum total of all the kinetic energy in a sample of matter. How is heat different from temperature???

40. Heat ≠ Temperature Both the water in the bath tub and in the cup are at 25 oC Which contains more HEAT?

41. Specific Heat Capacity The amount of energy (in JOULES) needed to raise the temperature of 1 gram of the sample by 1 oC Which water sample has a higher specific heat ?

42. HEAT EQUATION(in Table T) Q = mc∆t Q = heat energy in JOULES (J) m = mass of the sample in GRAMS (g) C = specific heat in J/goC ∆t = change in temperature (oC) or final temp – initial temp

43. Ion • An atom that has gained an electron is called an anion. It has a net negative charge. • An atom that has lost an electron is called a cation. It has a net positive charge.

44. Isotope Atoms of the same element that have different atomic masses (but same atomic number) WHY do they have different atomic masses?

45. Isotope • If two atoms are of same element, they MUST have the same number of protons (the same atomic number) • But…. they can have different number of NEUTRONS. The more neutrons, the heavier the atom

47. Isotopes of Lithium 3 neutrons 5 neutrons 4 neutrons

48. Average Atomic Mass • In nature, most elements are a mixture of different isotopes • The mass of a sample of an element is a weighted average of all the isotopes in the sample

49. Calculating Average Atomic Mass • The element Chlorine Cl has two naturally occurring isotopes: Cl-35 and Cl-37 • Which isotope has more neutrons? • How many more neutrons?

50. Calculating Average Atomic Mass • Out of 100 chlorine atoms, 75 will have a mass of 35 amu. • 25 will have a mass of 37 amu