Peters & Co. 2011 North American Oil & Gas Conference September 13, 2011
13 September 2011
description
Transcript of 13 September 2011
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13 September 2011
Objective: You will be able to: review chapter 2 concepts
Homework Quiz:1. Give the number of protons and
electrons in the ion Mg2+
2. Name the compound BaCl2
3. Write the formula for iodine heptachloride
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Agenda
I. Homework QuizII. Ch. 1 #105III. Chapter 2 ReviewIV. Problems in Chapter 2?Homework: Chapter 1 Problem Set:
Thurs.
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Announcement
Do I have your signed syllabus page yet?
You really want to be a TA for chemistry…
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CHAPTER 2 REVIEW: ATOMS, MOLECULES, IONS
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Atoms, Molecules and Ions
Review your notes from 2.1 – 2.5
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Ionization A review of how to determine which
ion an atom makes
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Valence Shell
Valence Shell: The most outer energy level.
1s22s22p63s23p3
1s 2s 2p 3s 3p
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Stability
1s 2s 2p 3s 3p
1s 2s 2p 3s 3p
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Valence Electrons: Label on your PTE1
2 3 4 5 6 78
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Group 1
s ps p
New valence shell
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Ions
Ion: An atom that has lost or gained one or more electrons
Cation: An atom that has lost an electron Positive Charge
Anion: An atom that has gained an electron Negative Charge
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Octet Rule
Octet Rule: All atoms lose and gain electrons to form a full valence shell H, He = 2 All other elements = 8
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Ions formed by group - Add to your PTE
12 3 4 5 6 7
81+
2+
3+ 3- 2- 1-
Cations Anions
Lose e- Gain e-
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Set up a table:Element
# Valence E-
Loses or Gains E-?
Cation or Anion?
Charge of Ion
Symbol of Ion
Name of Ion
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Set up a table:Element
# Valence E-
Loses or Gains E-?
Cation or Anion?
Charge of Ion
Symbol of Ion
Name of Ion
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Number of Valence Electrons
1. Li2. Be3. B4. F5. O6. N7. Cl
8. P9. K10. Ca11. Al12. Se13. Br14. Kr
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Anion or Cation?
Cation is positive because it has LOST electrons. It is a positive thing to have a cat,
and it would be sad if you lost your cat.
Anion is negative because it has GAINED electrons Mnemonic?
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Symbols for Ions
Element SymbolCharge
Li+
Cl-
Al3+
Number, then + or – No need to write a “1” 1 is often invisible in chemistry
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Names for Ions
Cations: Same name as the element Li+: lithium ion Sr2+: strontium ion
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Naming Ions
Anions: Ending changes to “-ide” N3-: nitride ion O2-: oxide ion F-: fluoride ion S2-: sulfide ion Cl-: chloride ion Br-: bromide ion I-: iodide ion
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Polyatomic Ions
NH4+ ammonium
CO32- carbonate
HCO3- hydrogen carbonate
ClO3- chlorate
CrO42- chromate
Cr2O72- dichromate
CN- cyanidePO4
3- phosphateHPO4
2- hydrogen phosphateH2PO4
- dihydrogen phosphate
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More Polyatomic Ions
SO32- sulfite
SO42- sulfate
HSO4- hydrogen sulfate
OH- hydroxideNO3
- nitrateNO2
- nitriteMnO4
- permanganateO2
2- peroxide
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14 September 2011
Objective: You will be able to: Name ionic and covalent
compounds Homework Quiz:
Write the formulas for:a. iron (III) chlorideb. ammonium sulfatec. dihydrogen monoxide
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Agenda
Homework Quiz Questions about ch. 1 problem set? Chapter 2 reviewHomework: Ch. 1 problem set due
tomorrow
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Formulas of Ionic Compounds
Formed by electrostatic attraction between cations and anions.
Examples:a. potassium bromideb. zinc iodidec. aluminum oxided. magnesium nitratee. iron (II) chloride(p. 54 for charges of transition metals)
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Practice
1. rubidium sulfate
2. barium hydride
3. manganese (IV) oxide
4. ammonium carbonate
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Names of Ionic Compounds
Examplesa. KBrb. CuClc. FeCl3
d. Cu(NO3)2
e. KH2PO4
f. NH4ClO3
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Practice
1. MgBr2
2. Li2SO3
3. PbO
4. FeCO3
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Molecular Compounds Prefix system
1 mono (**only used for secondelement in compound) 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9nona 10 deca
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Naming Molecular Compounds
Examplesa. COb. CO2
c. N2O4
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Practice Naming Molecular Compounds
1. SiCl4
2. P4O10
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Writing Formulas for Molecular Compounds
Examplesa. nitrogen dioxide
b. dihydrogen monoxide
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Practice Writing Formulas for Molecular Compounds
1. nitrogen trihydride (a.k.a. ammonia)
2. carbon tetrachloride (a.k.a. freon)
3. carbon disulfide
4. disilicon hexabromide
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Naming Acids
Acid: any substance that yields hydrogen ions (H+) when dissolved in water
If the anion ends in “-ide”, the acid is a “hydro –ic” acid
HF hydrofluoric acidHCl hydrochloric acidHBr hydrobromic acidHI hydriodic acidHCN hydrocyanic acidH2S hydrosulfuric acid
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Oxoacids
Contain hydrogen, oxygen and another element.
Used as reference acids to name other acids
H2CO3 carbonic acidHClO3 chloric acidHNO3nitric acidH3PO4 phosphoric acidH2SO4 sulfuric acid
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More oxoacids
Often, two or more oxoacids have the name central atom but a different number of O atoms
1. Adding one O atom to an “-ic” acid = “per… -ic” acid
2. Removing one O atom from an “-ic” acid = “-ous” acid
3. Removing two O atoms from an “-ic” acid = “hypo…-ous” acid
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Oxyacid examples
HClO3 chloric acid Add an oxygen: HClO4
perchloric acid Remove an oxygen: HClO2
chlorous acid Remove two oxygens: HClO
hypochlorous acid
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Oxyacid Problems
Name the following oxyacids1. HNO2
2. H2SO3
3. H2CO4
4. H2SO2
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Naming Bases
A base yields hydroxide (OH-) ions when dissolved in water
a. NaOH sodium hydroxideb. Ba(OH)2 barium hydroxide
(Some bases don’t contain OH-, but more on that later.)
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Hydrates
Hydrates are compounds with a specific number of water molecules attached to them
Example: CuSO4·5H2O copper (II) sulfate pentahydrate
BaCl2·2H2O barium chloride dihydrate
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15 Sept. 2011
Objective: You will be able to: Practice identifying subatomic
particles, isotopes, determining ionization, naming and writing formulas for compounds.
design a procedure to determine the formula of a hydrate.
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Agenda
I. Questions about chapter 2 summer assignment?
II. Chapter 2 problem setIII. Design an procedure!Homework: Chapter 2 problem set:
Tues.Ch. 1-2 quiz Tues.
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Your challenge!
Copper (II) sulfate hydrate Hydrate: a compound with water
“tagged on to” the crystal structure. Determine the number of molecules
of water of hydration per formula unit of copper (II) sulfate.
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Your procedure…
1. A complete list of steps which include
1. specific quantities2. names of equipment you’ll need to
use3. some way to determine when your
procedure is “finished”2. Directions and equations for any
calculations you’ll need to makeDue: Monday!
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Homework
Quiz on ch. 1-2 Tuesday Lab procedure: Monday
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19 September 2011
Take out your lab notebook and turn to your procedure
Objective: You will be able to: carry our your procedure and
collect data to determine the number of molecules of water of hydration of copper (II) sulfate hydrate.
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Agenda
I. Procedure discussionII. Carry out your procedureIII. Make calculationsHomework: Quiz on ch. 1-2
tomorrowChapter 2 problem set: Tues.Complete calculations (including
name of hydrate): Thurs.
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Safety
Wear goggles until all your equipment has been cleaned and returned.
A hot crucible looks just like a cold crucible! Always use crucible tongs.
Work efficiently but carefully.
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Technical notes
Heat the crucible uncovered or with the cover tilted to allow water vapor to escape.
Cool the crucible with the cover on. Cool the crucible in the desiccator
for very best results. Never mass a hot or warm crucible. Oil from your fingers will stick to the
crucible and effect your data.
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Work Ethic
Work quickly. If you have “down time,” think: “What can I do now to save time later?”
Set up data tables and calculations while you wait.
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This period
Carry out your procedure and collect data.
Begin calculations as soon as you can! Percent of water in the hydrate by
mass. Mole ratio of anhydrous CuSO4 to
H2O in your sample. Work to show how you got your
number of molecules of water of hydration.
Name of the hydrate
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Homework
Quiz on ch. 1-2 tomorrow Chapter 2 problem set: Tues. Complete calculations (including
name of hydrate): Thurs.