2. What is simplified in this picture?

3. TheThompson: Discovery of the Electronthe Electron (Thomson)
Cathode Ray Tube
Charged particles produced (affected by magnetic field)

4. Concluded that atom must have positive and negative parts
Electron – negative part of the atom
Only knew the e/m ratio
Plum Pudding Model

6. Charge and Mass of the Electron (Millikan)
Oil drop experiment
Determines charge on electron (uses electric field to counteract gravity)
Quantized
e = X C
m = 9.11 X kg

8. The Nucleus (Rutherford)
Gold Foil Experiment
Discovers nucleus (disproves Plum Pudding Model)
Planetary Model

12. Atoms:Basic Facts Three particles Particle Charge Mass Proton +1
~1 g/mol
Electron -1
g/mol (1/1837)
Neutron

13. Photo of a single Barium atom

14. 5 million Cl atoms can be lined up in 1 mm.
Atoms:Basic Facts
Size – Measured in Angstroms
1 A = 1 X m
1 Cl atom = 2.0 A
5 million Cl atoms can be lined up in 1 mm.

15. Atoms:Basic Facts Mass – grams/mole H = 1.00794 grams/1 mole
g/6.022 X 1023 atoms
C = 12 g/mol

16. Isotopes
Isotopes – Atoms with the same # of protons, but different # of neutrons
Copper p 34 n
Copper p 36 n
2. Atomic Mass –weighted average of all the isotopes

17. p n E
13C
90Sr
24Mg 16 18 12 10 17 19

18. Ions
Cation – Positive Ion
Anion – Negative Ion
Review Common Charges

19. P N E
Cl-
O2-
Mg+
Mg2+

20. Stable vs. Unstable Nuclei Nuclear Changes
Most nuclei are stable – do not change
Some nuclei are unstable (radioactive)
Change into a different nucleus (decay)
Spontaneous process – happens naturally, by itself
Releases radiation
Only nuclear reactions can change a nucleus.
No chemical process can

21. Radium  Radon + Radiation
Decay
-New element and alpha, beta, or gamma
-lost mass becomes kinetic energy

22. Types of Nuclear Radiation
Alpha particle
(42He)
Helium nucleus
Beta particle
(0-1e)
fast-moving electron.
Gamma rays

high energy electromagnetic radiation
Positron
(0+1e)
positive electron (anti-matter)
Types of Nuclear Radiation
2 p+
2 n e-

23. What Stops Radiation Al Foil Wood Lead. Iron, Concrete Paper Alpha ()
Beta ()
Gamma ()

24. Decay Equations Alpha Decay 23892U  42He + 23490Th Beta Decay
23490Th  0-1e Pa

25. Decay Equations Gamma Decay Occurs with alpha and beta decay
No change in atomic mass (gamma radiation has no mass 00)

26. Decay: Ex 1
What product is formed when radium-226 undergoes alpha decay?
22688Ra  42He +

27. Decay: Ex 2 What element undergoes alpha decay to form lead-208?
 42He Pb

28. Decay: Ex 3 What isotope is produced when thorium-231 beta decays?
23190Th  0-1e +

29. Write the equation that describes oxygen-15 undergoing positron emission.

30. Which nuclei are radioactive (unstable)
All elements have at least one radioactive isotope
All isotopes of elements heavier than Lead (82) 82 Pb
207.2
At least one radioactive isotope
All isotopes are radioactive

31. Transmutation Rutherford(1919) – First successful alchemist
147N + 42He  178O + 11H
Modern methods
Particle Accelerators (Cyclotrons)
Use neutrons or other elements (creation of transuranium elements)

32. Periodic Table Dmitri Mendeleev – 1869
Used atomic mass (modern is by atomic #)
Period – Across
Group – Down
Metals
Non-Metals
Metalloids - Semiconductors

35. Discuss placement of Lanth/Act
Periodic Table
Group 1 Alkali metals
Group 2 Alkaline earth metals
Transition Metals
Group 7 Halogens
Group 8 Noble Gases
Lanthanides
Actinides
Discuss placement of Lanth/Act

36. Average Atomic Mass
Atomic Mass – Weighted Average of all the isotopes

38. Average Atomic Mass
Calculate the ave atomic mass of Boron if it exists as 19.90% Boron-10 ( g/mol) and 80.10% B-11 ( g/mol)?
(Ans: g/mol)

39. Mixing Elements
Ionic = Metal + Non-metal (NaCl)
Molecular = Non + Non (CH4)
Alloy = Metal + Metal
Stainless steel (Fe/Cr)
Brass (Cu/Zn)
Bronze (Cu/Sn)

42. Ionic vs. Molecular Ionic Compounds Molecules Start w/ Metal
Stealing of Electrons
Clumps of Ions(crystals)
Called Salts
No prefixes, may need Roman #
Two Non-metals
Sharing of electrons
Separate Molecules
Shapes (tetrahedral, etc…)
Polar and Non-Polar Molecules (H2O vs CH4)
Prefixes

43. Ionic Solids

44. Ionic vs. Molecular
Ionic or molecular?
HCl
CO2
VO3
H2O
BaF2

46. What ionic compound would form between:
Ba and Cl
Ba and Te
Al and S
Fe3+ and O
Fe2+ and O

47. H He Al

48. Naming Ionics Binary Compounds Gr I and Gr II metals (and Aluminum)
NaCl
BaO
Al2O3
magnesium bromide
aluminum sulfide
potassium oxide

49. Naming Ionics Sodium hydroxide Sodium carbonate Aluminum Sulfate NaNO3
Compounds with Polyatomics
Sodium hydroxide
Sodium carbonate
Aluminum Sulfate
NaNO3
Ca(OH)2
(NH4)3PO4

50. Mixed Examples
Magnesium Sulfide
Magnesium Sulfite
Magnesium Sulfate
Lithium Phosphide
Lithium Phosphate
Ba(ClO3)2
BaCl2

51. Roman # Ionics 2. Metals which have multiple oxidation states
1. Example
Fe(II)and oxygen
Fe(III) and oxygen
How do we distinguish?
2. Metals which have multiple oxidation states
Transition and post-transition metals

52. Iron (III)Bromide
Tin(II) nitrate
Cobalt(III)Oxide
CoCl2
MnO2
Ru2(SO4)3
VO3

53. Mixed Examples
Calcium Bromide
Chromium (III)Nitrate
Aluminum Sulfate
Iron(III)Carbonate
Li2S
CoCl2
Ti3N2
Mg(NO2)2

54. Magnesium Sulfide
Magnesium Sulfite
Magnesium Sulfate
Mn2(SO4)3
Lithium Phosphide
Lithium Phosphate
Ba(ClO3)2
Copper(II)nitrate

55. All big clumps (crystals) of Ions
Household Ionics
Many ionic compounds are called salts
CaCl2 – Calcium Chloride (Quik-Joe)
NaHCO3 – Sodium bicarbonate(Baking soda)
CaCO3 – Calcium Carbonate(Chalk, antacid)
NaOH - Sodium Hydroxide (Drano)
MgSO4 – Magnesium Sulfate(Epsom Salts)
All big clumps (crystals) of Ions

56. Naming Molecules Prefixes mono hexa di hepta tri octa tetra nona
penta deca
May skip “mono” for first element

57. CO
CO2
Cl2O7
SF6
Chlorine dioxide
Diphosphorus tetroxide
Carbon tetrachloride

58. Naming Molecules
Household Molecules
H2O
HCl
NH3
H2SO4
HC2H3O2

59. Review of all naming
CS2 N2O
NaI PCl5
FeF2 HgI2
K2CO3 NO3
Ba(OH)2

60. Calcium Chloride
Silicon Dioxide
Copper(II)Carbonate
Magnesium Phosphate
Dicarbon Octahydride
Chromium(III)Oxide
Dihydrogen Monoxide

61. Acids Binary Acids HCl hydrochloric acid HF hydrofluoric acid
H2S hydrosulfuric acid

62. Acids 2. Oxoacids Acid Ion HClO4 perchloric acid perchlorate (ClO4-)
HClO3 chloric acid chlorate (ClO3-)
HClO2 chlorous acid chlorite (ClO2-)
HClO hypochlorous acid hypochlorite (ClO- )

63. Examples
HCN
HNO3
H2SO4
H2SO3

64. Examples
HNO2 HI
H3PO4
H3CO3
HClO3

65. H2 Hydrogen (H- Hydride)
N2 Nitrogen (N3- Nitride)
O2 Oxygen (O2- Oxide)
F2 Fluorine (F- Fluoride)
Cl2 Chlorine (Cl- Chloride)
Br2 Bromine (Br- Bromide)
I2 Iodine (I- Iodide)

67. 26
Xe-130 has one more neutron
50)

68. Molecular PF5, SCl, N2O4
Ionic NaI Ca(NO3)2, FeCl3, LaP, CoCO3

69. g/mol
a) CuBr2 b) Fe2O3 c) Hg2CO3
d) Ca3(AsO4) e) (NH4)2CO3
58. Na2O CaO FeO Al2O3
NaNO3 Ca(NO3)2 Fe(NO3)2 Al(NO3)3
Na2SO4 CaSO4 FeSO4 Al2(SO4)3
Na3AsO4 Ca3(AsO4)2 Fe3(AsO4)2 AlAsO4
a) Cu2+ b) Ag+ c) Al3+ d) Co2+
e) Pb2+

70. 85.47 g/mol
Cu2+ S2-
Ag+ SO42-
Al3+ ClO3-
Co2+ OH-
Pb2+ CO32-