Testing

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What is simplified in this picture?
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TheThompson Discovery of the Electronthe
Electron (Thomson)

• Cathode Ray Tube
• Charged particles produced (affected by magnetic
  field)

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

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Charge and Mass of the Electron (Millikan)

• Oil drop experiment
• Determines charge on electron (uses electric
  field to counteract gravity)
• Quantized
• e 1.602 X 10-19 C
• m 9.11 X 10-31 kg

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The Nucleus (Rutherford)

• Gold Foil Experiment
• Discovers nucleus (disproves Plum Pudding Model)
• Planetary Model

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AtomsBasic Facts

• Three particles

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The Worlds Most Famous Neutron
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Photo of a single Barium atom
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AtomsBasic Facts

• Bohr Model Drawing for Carbon.
• Electrons DO NOT really move in rings, only an
  approximation.
• Valence Electrons Only electrons involved in
  most of chemistry.
• Electrons move in the atom at about
• 5 MILLION MILES PER HOUR!!

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AtomsBasic Facts

• Size Measured in Angstroms
• 1 A 1 X 10-10 m
• 1 Cl atom 2.0 A
• 5 million Cl atoms can be lined up in 1 mm.

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AtomsBasic Facts

• Mass grams/mole
• H 1.00794 grams/1 mole
• 1.00794 g/6.022 X 1023 atoms
• C 12 g/mol

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Isotopes

• Carbon example
• Atomic protons
• Atomic Mass p n
• Isotopes Atoms with the same of protons, but
  different of neutrons

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Isotopes

• 3. Elements often exist as a mixture of isotopes
• Copper-63 29 p 34 n
• Copper-65 29 p 36 n
• Atomic Mass a weighted average of all the
  isotopes

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Isotopes
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Ions

• Cation Positive Ion
• Anion Negative Ion
• Review Common Charges

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How many p, n, e in p n e Cl- O2- Mg
Mg2
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Stable vs. Unstable Nuclei
Nuclear Changes

• Most nuclei are stable do not change
• Some nuclei are unstable (radioactive)
• Change into a different nucleus
• Spontaneous process happens naturally, by
  itself
• Releases radiation
• Only nuclear reactions can change a nucleus.
• No chemical process can

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• Radium ? Radon
  Radiation
• The radium was unstable (radioactive)
• Turned into a different element (decayed)
• The lost mass was turned into radiation
  (invisible, odorless)

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Types of Nuclear Radiation
2 p 2 n
e-
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What Stops Radiation
Al Foil Wood
Lead. Iron, Concrete
Paper
Alpha (a)
Beta (b)
Gamma (g)
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Decay Equations

• Alpha Decay
• 23892U ? 42He 23490Th
• Beta Decay
• 23490Th ? 0-1e 23491Pa

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Decay Equations

• Gamma Decay
• Occurs with alpha and beta decay
• No change in atomic mass (gamma radiation has no
  mass 00g)

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Decay Ex 1

• What product is formed when radium-226 undergoes
  alpha decay?
• 22688U ? 42He ?
• 22688U ? 42He 22286Rn

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Decay Ex 2

• What element undergoes alpha decay to form
  lead-208?
• ? ? 42He 20882Pb
• 21284Po ? 42He 20882Pb

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Decay Ex 3

• What isotope is produced when thorium-231 beta
  decays?
• 23190Th ? 0-1e ?
• 23190Th ? 0-1e 23191Pa

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• 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
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Transmutation

• Rutherford(1919) First successful alchemist
• 147N 42He ? 178O 11H
• Modern methods
• Particle Accelerators (Cyclotrons)
• Use neutrons or other elements (creation of
  transuranium elements)

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Periodic Table

• Dmitri Mendeleev 1869
• Arranged his table by atomic mass, ours is by
  atomic number
• Period Across
• Group Down
• Metals
• Non-Metals
• Metalloids - Semiconductors

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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

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Average Atomic Mass

• Most Elements exist as several isotopes
• Some of the isotopes are more common
• Atomic Mass Weighted Average of all the isotopes

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Average Atomic Mass

• What is the ave atomic mass of Boron if it exists
  as 19.90 Boron-10 (10.013 g/mol) and 80.10 B-11
  (11.009 g/mol)?
• (Ans 10.811 g/mol)

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Mixing Elements

• 1. Drawing of Periodic Table (metals vs.
  Non-metals)
• Ionic Metal Non-metal (NaCl)
• Molecular Non Non (CH4)
• Alloy Metal Metal
• Stainless steel (Fe/Cr)
• Brass (Cu/Zn)
• Bronze (Cu/Sn)

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Ionic vs. Molecular
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Ionic Solids
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Ionic vs. Molecular

• Are the following ionic or molecular?
• HCl
• CO2
• VO3
• H2O
• BaF2

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• What ionic compound would form between
• Ba and Cl
• Ba and Te
• Al and S
• Fe3 and O
• Fe2 and O

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Naming Ionics

• I. Binary Compounds
• A. Used for Gr 1 and Gr 2 metals (and Aluminum)
• B. Metal has only one standard charge
• C. Rules
• Write Metal First
• Non-metal becomes ide

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Naming Ionics

• D. Examples
• NaCl
• BaO
• Al2O3
• magnesium bromide
• aluminum sulfide
• potassium oxide

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Naming Ionics

• II. Compounds with Polyatomics
• A. Polyatomic Ion - An Ion with more than one
  atom (Consider the overall charge)
• B. Examples
• Hydroxide Sulfate
• Nitrate Acetate

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Naming Ionics

• C. Examples
• Sodium hydroxide
• Sodium carbonate
• Aluminum Sulfate
• NaNO3
• Ca(OH)2
• (NH4)3PO4

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Naming Ionics

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

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Roman Ionics

• 1. An example
• Fe(II)and oxygen
• Fe(III) and oxygen
• How do we distinguish?
• 2. Metals which have multiple oxidation states
• Drawing of periodic table

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Roman Ionics

• 3. The Roman Numeral tells you the charge NOT
  how many atoms you have.
• Copper(II)Oxide
• Copper(III)Oxide

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Roman Ionics

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

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Roman Ionics

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

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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

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Naming Molecules

• Prefixes
• mono hexa
• di hepta
• tri octa
• tetra nona
• penta deca
• May skip mono for first element

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Naming Molecules

• P4O10
• N2O4
• SiO2

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Naming Molecules

• CO2
• Cl2O7
• SF6
• Chlorine dioxide
• Diphosphorus tetroxide
• Carbon tetrachloride

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Naming Molecules

• Household Molecules
• H2O
• HCl
• NH3
• H2SO4
• HC2H3O2

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Rev. of All Naming

• Remember to check if it is Ionic or Molecular
• CS2 N2O
• NaI PCl5
• FeF2 HgI2
• K2CO3 NO3
• Ba(OH)2

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Rev. of All Naming

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

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Acids

• Binary Acids
• HCl hydrochloric acid
• HF hydrofluoric acid
• H2S hydrosulfuric acid

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Acids

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

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Examples

• HCN
• HNO3
• H2SO4
• H2SO3

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• 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)

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