Download - Time for Prayer Check Next Prayer Attendance
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Prayer/Next PrayerCheck Homework
Attendance
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CHAPTER 5 REVIEW NAMING POLYATOMIC IONS & ACIDS
Ms. Doshi
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Naming Compounds that Contain Polyatomic Ions
polyatomic ions -charged entities made of many atomsExample: NH4NO3 contains these polyatomic ions: NH4
+ and NO3-
oxyanions-polyatomic anions that contain an atom of a given element and different number of oxygen atoms.
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Memorize these!Need to give memory aid to students.
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Naming Compounds with Polyatomic Ions1. Similar to binary ionic compoundsmust memorize common polyatomic ionsand learn the composition and charge of each ion in Table 5.4Example: NH4C2H3O2 is ammonium acetate.
2. When you see a metal that can form one or more cation, use a Roman Numeral. Similar to Type II binary ionic compounds.Example: FeSO4 is iron(II) sulfate
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Now, you try!
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Name the following compounds
a) Na2CO3b) FeBr3c) CsClO4d) PCl3e) CuSO4
a) NaHCO3b) BaSO4c) CsClO4d) BrF5e) NaBrf) KOClg) Zn3(PO4)2
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Naming Acids
acid:-a molecule with one or more H+ ions attached to an anion
Examples: H2SO4, H3PO4
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Rules (in your textbook)
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Use Rule 2
Acid Anion Name
HClO4
HClO3
HClO2
HClO
perchlorate
chlorate
chlorite
hypochlorite
perchloric acid
chloric acid
chlorous acid
hypochlorous acid
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Names of acids that do not contain oxygen-MEMORIZE
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Names of some acids that contain Oxygen-MEMORIZE
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Naming Acids: Practice
Name each of the following acids:
Name the Acid Name the Acid
HOCl HBrO4
H2SO3 H2S
HBrO3 H2Se
HOI H3PO3
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Write the Formulas from Names
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Chapter 5 Review Questions
4, 8, 10, 12, 14, 24, 26, 28, 30, 34, 38, 42, 44, 46, 48
Answers are in your textbook!
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CHAPTER 6CHEMICAL REACTIONS: AN INTRODUCTION
Ms. Doshi
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Evidence for a Chemical Reaction
How do we know that a chemical reaction has occurred?1.The color changes. (We can see this)2.A solid forms. (We can see this.)3.Bubbles form. (We can see this.)4.Heat and/or a flame is produced, or heat is absorbed. (We can’t see heat but we can feel it).
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Evidence of a Chemical ReactionPicture Explanation
An electric current passes through water, hydrogen and oxygen gas are formed. http://www.youtube.com/watch?v=cJmuMBfVtLo
Cold pack. You break an ampule, the reaction begins causing that pack to absorb heat quickly.
Warm pack. Open the package. Oxygen reacts with chemicals in the bag, heat is produced for many hours.
HCl (colorless)+ cobalt(II)nitrate (red) produces a blue solutionhttp://www.youtube.com/watch?v=ryWsghHblWQ
sodium dichromate + lead nitrate forms a solid. http://www.youtube.com/watch?v=Jt0eGtHHV04
calcium (metal) + water forms hydrogen gas (bubbles)http://www.youtube.com/watch?v=UMqPKQKamhk
methane gas + oxygen forms a flame in a Bunsen Burner http://www.youtube.com/watch?v=cmXbGbj6ipM
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A Chemical Reactionchemical reaction-represented by a chemical equationreactants-chemicals present before the reaction products-chemicals formed by the reactionreactants productsExample:
arrow = direction of change, read as “yields” or “produces”
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Very IMPORTANT!!!
In a chemical reaction, atoms are neither created or destroyed. The number of each type of atom on the reactant side = the number of each type of atom on the product side.This is called balancing the chemical equation
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Unbalanced Equation and Balanced Equation
Unbalanced Equation
Balanced Equation
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Physical StatesSymbol State(s) solid(l) liquid(g) gas(aq) dissolved in water
(aqueous solution)
Example:Unbalanced Equation with Physical States
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Write Unbalanced Equations
Read and Understand Example 6.1 Do Exercise 6.1.
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A Chemical Equation
A chemical equation gives us this information:1.the reactants and products2.the numbers of each3.the physical states
We want our equations to be balanced and show the physical states of all of our reactants and products.
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How to Write and Balance Chemical EquationsLet’s do together: Let’s balance the equation for liquid ethanol. (p154)1. Read the description of the chemical reaction. What are the reactants? The products, and their states? Write the formulas. 2. Write the unbalanced equation. 3. Balance the equation. Start with the most complicated molecule (the one with the most elements). 4. Check to see that the coefficients used give the same number of each type of atom on both sides of the arrow.
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Balancing Chemical Equations I
Let’s do together:
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Balancing Chemical Equations II
Let’s do together:
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Balancing Chemical Equations III
Let’s do together:
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Exercise 6.3
Now, it’s your turn:
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Problems to do: RIGHT NOW!
Chapter 6 Review
6.28, 10, 14, 16, 18, 20, 22, 24, 26, 28, 30, 32
6.338, 40, and 42
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WE ARE NOT FINISHED!
Review Exercise to do for Chapters 4 and 5!19, 21, 22, 23, 24, 26, 28, 30, and 31
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Any Questions?Any Answers?
Any Comments?