13 September 2011 Objective: You will be able to: review chapter 2 concepts Homework Quiz: Give the number of protons and electrons in the ion Mg2+ Name the compound BaCl2 Write the formula for iodine heptachloride

Agenda Homework Quiz Ch. 1 #105 Chapter 2 Review Problems in Chapter 2? Homework: Chapter 1 Problem Set: Thurs.

Announcement Do I have your signed syllabus page yet? You really want to be a TA for chemistry…

Chapter 2 Review: Atoms, Molecules, Ions

Atoms, Molecules and Ions Review your notes from 2.1 – 2.5

Ionization A review of how to determine which ion an atom makes

Valence Shell Valence Shell: The most outer energy level. 1s22s22p63s23p3 1s 2s 2p 3s 3p

Stability 1s 2s 2p 3s 3p 1s 2s 2p 3s 3p

Valence Electrons: Label on your PTE 1 8 2 3 4 5 6 7

Group 1 s p s p New valence shell

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

Octet Rule Octet Rule: All atoms lose and gain electrons to form a full valence shell H, He = 2 All other elements = 8

Ions formed by group - Add to your PTE 1+ 1 8 2 2+ 3+ 3 4 3- 5 6 2- 1- 7 Gain e- Lose e- Anions Cations

Set up a table: Element # Valence E- Loses or Gains E-? Cation or Anion? Charge of Ion Symbol of Ion Name of Ion Set up a table:

Set up a table: Element # Valence E- Loses or Gains E-? Cation or Anion? Charge of Ion Symbol of Ion Name of Ion Set up a table:

Number of Valence Electrons Li Be B F O N Cl P K Ca Al Se Br Kr

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?

Symbols for Ions Element SymbolCharge Li+ Cl- Al3+ Number, then + or – No need to write a “1” 1 is often invisible in chemistry

Names for Ions Cations: Same name as the element Li+: lithium ion Sr2+: strontium ion

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

Polyatomic Ions NH4+ ammonium CO32- carbonate HCO3- hydrogen carbonate ClO3- chlorate CrO42- chromate Cr2O72- dichromate CN- cyanide PO43- phosphate HPO42- hydrogen phosphate H2PO4- dihydrogen phosphate

More Polyatomic Ions SO32- sulfite SO42- sulfate HSO4- hydrogen sulfate OH- hydroxide NO3- nitrate NO2- nitrite MnO4- permanganate O22- peroxide

14 September 2011 Objective: You will be able to: Name ionic and covalent compounds Homework Quiz: Write the formulas for: iron (III) chloride ammonium sulfate dihydrogen monoxide

Agenda Homework Quiz Questions about ch. 1 problem set? Chapter 2 review Homework: Ch. 1 problem set due tomorrow

Formulas of Ionic Compounds Formed by electrostatic attraction between cations and anions. Examples: potassium bromide zinc iodide aluminum oxide magnesium nitrate iron (II) chloride (p. 54 for charges of transition metals)

Practice rubidium sulfate barium hydride manganese (IV) oxide ammonium carbonate

Names of Ionic Compounds Examples KBr CuCl FeCl3 Cu(NO3)2 KH2PO4 NH4ClO3

Practice MgBr2 Li2SO3 PbO FeCO3

Molecular Compounds 1 mono (**only used for second 2 di 3 tri 4 tetra Prefix system 1 mono (**only used for second element in compound) 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9nona 10 deca

Naming Molecular Compounds Examples CO CO2 N2O4

Practice Naming Molecular Compounds SiCl4 P4O10

Writing Formulas for Molecular Compounds Examples nitrogen dioxide dihydrogen monoxide

Practice Writing Formulas for Molecular Compounds nitrogen trihydride (a.k.a. ammonia) carbon tetrachloride (a.k.a. freon) carbon disulfide disilicon hexabromide

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 acid HCl hydrochloric acid HBr hydrobromic acid HI hydriodic acid HCN hydrocyanic acid H2S hydrosulfuric acid

Oxoacids Contain hydrogen, oxygen and another element. Used as reference acids to name other acids H2CO3 carbonic acid HClO3 chloric acid HNO3 nitric acid H3PO4 phosphoric acid H2SO4 sulfuric acid

More oxoacids Often, two or more oxoacids have the name central atom but a different number of O atoms Adding one O atom to an “-ic” acid = “per… -ic” acid Removing one O atom from an “-ic” acid = “-ous” acid Removing two O atoms from an “-ic” acid = “hypo…-ous” acid

Oxyacid examples HClO3 chloric acid Add an oxygen: HClO4 perchloric acid Remove an oxygen: HClO2 chlorous acid Remove two oxygens: HClO hypochlorous acid

Oxyacid Problems Name the following oxyacids HNO2 H2SO3 H2CO4 H2SO2

Naming Bases A base yields hydroxide (OH-) ions when dissolved in water NaOH sodium hydroxide Ba(OH)2 barium hydroxide (Some bases don’t contain OH-, but more on that later.)

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

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.

Agenda Questions about chapter 2 summer assignment? Chapter 2 problem set Design an procedure! Homework: Chapter 2 problem set: Tues. Ch. 1-2 quiz Tues.

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.

Your procedure… A complete list of steps which include specific quantities names of equipment you’ll need to use some way to determine when your procedure is “finished” Directions and equations for any calculations you’ll need to make Due: Monday!

Homework Quiz on ch. 1-2 Tuesday Lab procedure: Monday

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.

Agenda Procedure discussion Carry out your procedure Make calculations Homework: Quiz on ch. 1-2 tomorrow Chapter 2 problem set: Tues. Complete calculations (including name of hydrate): Thurs.

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.

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.

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.

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

Homework Quiz on ch. 1-2 tomorrow Chapter 2 problem set: Tues. Complete calculations (including name of hydrate): Thurs.