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August Turn in your signed documents if you haven’t already done so

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Presentation on theme: "August Turn in your signed documents if you haven’t already done so"— Presentation transcript:

1 August Turn in your signed documents if you haven’t already done so ( to the tray on my desk) DO NOT TURN IN HW!! Pick up a white board and sock On a sheet of blank paper answer the following: What MAIN group are the following elements in? Carbon Argon Calcium Give an example of a metalloid

2 HW Check 1-26-15 Give an example of an alkali metal
Give an example of a transition metal What is the most active nonmetal? Give an example of a noble gas

3 Today is January 26, 2015 Topic: Periodic Table and Trends
Lesson Objectives: SWBAT Interpret the name and formula of compounds using IUPAC convention Essential Question: 1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties.

4 Homework 1-26 Review the Periodic Table and Trends
Nomenclature Half Sheet Get contracts signed for the Syllabus, Safety contract

5 Important Dates Tuesday 2/27 – tutoring Tuesday 2/27 – quiz Thursday 2/29 – tutoring Friday 2/30 – lab Friday 2/6 – Test

6 Classroom Review Entry Turned back documents Grades

7 Reference Table

8 Wrap up Wanted! Poster You have 12 minutes to finish your wanted poster

9 Ions Cation: A positive ion Mg2+, NH4+ Anion: A negative ion Cl-, SO42-

10 Predicting Ionic Charge
NEITHER +/-4 +1 -1 +3 -2 -3 +2

11 Determine Charge Ca Se As Br

12 Predicting Ionic Charges
Transition Metals: Many transition elements have more than one possible oxidation state. Iron(II) = Fe2+ Iron(III) = Fe3+

13 Predicting Ionic Charges
Transition Metals: Some transition elements have only one possible oxidation state. Silver = Ag+ Zinc = Zn2+

14 Predicting Ionic Charge
Determining the Charge of a Transition Metal Find the total charge of the Anion Anion Oxidation # x Anion Subscript Determine charge of the transition metal Total Anion Charge ÷ Metal Subscript Transition Metal charge is ALWAYS positive (+)

15 Determine Charge CuO Mn3N4 CuCl2 ZnCl2 PdS

16 Revisit Periodic Table Puzzle
Working with your table partner complete number 7-10

17 Ionic Compound Formulas

18 Forming Binary Ionic Compounds
Binary = two elements Ionic = one metal and one nonmetal Transfer of electrons Not called molecules!

19 IUPAC IUPAC- International Union of Pure and Applied Chemists (created this naming system)

20 Writing Formulas All compounds have a charge of zero.
When writing formulas, all ions have to add up to zero. Example: Na – Charge of +1 Cl – Charge of -1 NaCl (charges cancel out for 0)

21 Writing Binary Ionics Write each ion (metal first)
Crisscross the charges Drop the + and – Write numbers as subscripts

22 Binary Ionic Compounds
Example: magnesium chloride Mg+2 Cl-1 MgCl2

23 Why does this work? MgCl2 means… Cl-1 Mg+2 Cl-1

24 Binary Ionic Compounds
Example: barium oxide Ba+2 O-2 BaO Ba2O2

25 Practice Sodium bromideNaBr Calcium fluoride CaBr2 Magnesium oxide
Lithium oxide Aluminum oxide Magnesium fluoride Potassium iodide Aluminum sulfide

26 Forming Ternary Ionics
Contain 3 or more elements Combination of a metal and a polyatomic ion Refer to page 7 of your reference tables for the list of polyatomic ions.

27 Writing Ternary Ionic Compounds
Write each ion (cation first) --- more than 3 uppercase letters means look at your polyatomic ion list! Crisscross the charges Drop the + and – Write numbers as subscripts Keep polyatomic ions in parentheses if more than 1(Blue sky rule!) Never change a polyatomic ion!!!!!

28 Ternary Ionic Compounds
Example: ammonium chloride NH4+1 Cl-1 NH4Cl

29 Ternary Ionic Compounds
Example: lithium carbonate Li+1 CO3-2 Li2CO3

30 Ternary Ionic Compounds
Example: calcium hydroxide Blue Sky Rule!!! Ca+2 OH-1 Ca(OH)2

31 Why does this work? Ca(OH)2 means… OH-1 Ca+2 OH-1

32 Practice Magnesium hydroxide Potassium sulfate  Sodium phosphate 
Calcium nitrate 

33 Stock System for Ionic Compounds
Some metals can have more than one oxidation state (i.e. transition metals) Use roman numerals Examples: Copper (I) chloride Cu+1 Cl-1 CuCl Copper (II) chloride CuCl2 Cu+2 Cl-1

34 Practice Mercury (II) oxide  Vanadium (V) bromide 
Copper (I) oxide  Tin (IV) bromide 

35 NB Raffle

36 Fist to Five 5- I could teach it 4 – I’ve got it 3 – I need to study some 2 – I need to study AND come to tutoring 1 – I have no idea what I am doing

37 HW headstart Work on your hw and ASK questions


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