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: Ions Isotopes Average atomic mass
Atoms (protons, neutrons, e-)
Ions
Isotopes
Average atomic mass
e- configurations
ground state
excited state
Bright line spectra

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

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

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

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

8. Sig Figs in Scientific Notation
5.347 x 10 16
sig figs
5.000 x 10 -6
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. Ex. Water boils into steam at 100 degrees Celsius
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. Malleability: can be pounded into a new shape without breaking
Physical Properties
Malleability: can be pounded into a new shape without breaking
Metals are malleable

16. Physical Properties
Iron is malleable Fe

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

18. Reflects the regular arrangement of atoms in the solid
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. Substance changes into a NEW substance.
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 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 ChemicalFe

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. High temperature = moving faster
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. AVERAGE KINETIC ENERGY
Once again……
TEMPERATURE =
AVERAGE KINETIC ENERGY

37. Kelvin never goes below zero (no negative numbers!)
Temperature Scales
Kelvin: 0 K = absolute zero (-460 oF)
all motion of particles stops!
Water 273 K
Water 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. do they have different atomic masses?
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

51. Calculating Average Atomic Mass
If 75% of all chlorine atoms in nature are Cl-35 and 25 % are Cl-37, what is the average atomic mass of a sample of chlorine?
*** Remember, this is a weighted average!

52. Calculating Average Atomic Mass
The unweighted average of 35 and 37 is… 36
This is NOT our answer!

53. Calculating Average Atomic Mass
The weighted average is calculated using the following formula (memorize this!)
(mass of isotope A x %) + (mass isotope B x %)

54. Calculating Average Atomic Mass
(mass of isotope A x %) + (mass isotope B x %)
(35 amu x 75) + (37 amu x 25) =
100
35.5 amu

55. Atom Review 3. What is located in the nucleus of the atom?
4. What is the nuclear charge (the charge on an atom’s nucleus)?
5. Where in the atoms are e- found?
6. What is the atom mostly made of?

56. Atom Review For each of the subatomic particles, give
Mass Charge Location
Proton
Neutron
electron

57. Atom review What is an ion? Name the 2 kinds of ions
What is an isotope?

58. Atom Review
11. What information does the atomic number of an element tell you?
What 2 subatomic particles give the atom most of it’s mass?
What does AMU stand for and what atom is it based on?

59. Atom Review
14. Write the formula we use to find the average atomic mass of an element:

60. Atom Review Questions Neutral atoms contain equal numbers of
All isotopes of neutral sodium atoms contain _________ protons and ___________ electrons

61. Atom Review Questions
Hydrogen has 3 isotopes. For each one tell how many protons, neutrons and e-
H-1 H-2 H-3

62. Atom Review Questions
4. For each isotope of oxygen tell how many protons, neutrons and e-
O-16 O-17 O-18

63. Atom Review Questions
What is the charge on an atom that contains 9P, 10N, 9e-?
What is this atom’s atomic number?
What is its atomic mass?

64. Atom Review Questions Cl-35 contains ______protons ______ neutrons
______ electrons

65. Atom Review Questions
For the atoms below, list the number of protons, neutrons, and electrons Kr 84 36

66. Atom Review Questions
For the atoms below, list the number of protons, neutrons, and electrons Cu +2 64 29

67. Atom Review Questions
For the atoms below, list the number of protons, neutrons, and electrons F -1 19 9

68. Atom Review Questions
For the atoms below, list the number of protons, neutrons, and electrons P -3 31 15

69. Atomic Review Questions
Write an isotope of O
Write an ion of O 16 8 16 8

70. Atomic Review Questions
12. Describe Rutherfords Gold Foil Experiment
13. What were the 2 conclusions about the structure of the atom that resulted from the Gold Foil Experiment? 16 8 16 8

71. Excited State e-
Ground State

72. For an e- to jump from the ground state to the excited state,
it must absorb energy (a photon of light)
When an e- falls back down from excited state to ground state,
it releases energy (a photon of light)

73. The visible light produced by e- falling back to ground state is called a bright line spectrum
Light is emitted only at certain wavelengths

74. Each element has its own distinct bright line spectrum
Bright line spectra can be used to identify elements,
by comparing the spectral lines to known spectra

75. To Summarize: 7 energy levels 4 sublevels ( S, P, D, F)
S orbitals = holds 2 e-
P orbitals = holds 6 e-
D orbitals = holds 10 e-
F orbitals = holds 14 e-

76. Arrangement of e- in the atom
7 s 7 p 7 d 7 f
6 s 6 p 6 d 6 f
5 s 5 p 5 d 5 f
4 s 4 p 4 d 4 f
3 s 3 p 3 d
2 s 2 p
1 s

77. Electron configuration for Ne
___ ___ ____ ____ ____
1s 2s p 2 2 6

78. Write the e- configuration of As33

79. Write the e- configuration of As33
___ ___ ___ ___ ___ ___ ___ ___ ___
1s2 2s p s p6
___ ___ ___ ___ ___ ___ ___ ___ ___
4s d p3
e- will not pair up
in p, d or f orbitals
if there is room in the orbital for them to spread out !

80. 1s2 2s2 2p6 3s2 3p6 4s2
2 –

82. What element? 5 2 2

83. What element? 2 2 6 2 3