science 10 chapter 4.3 balancing chemical equations
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Science 10 Chapter 4.3 Balancing Chemical Equations. Today. Learning check Review chemical compounds and formulas Chemical Reactions!!!. Silver chloride__________ 2. Sulphur dioxide__________ 3. Lead (II) acetate decahydrate _______________ Silver dichromate__________ - PowerPoint PPT PresentationTRANSCRIPT
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Science 10 Chapter 4.3 Balancing Chemical Equations
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Today
Learning check Review chemical compounds and formulas Chemical Reactions!!!
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1. Silver chloride__________2. Sulphur dioxide__________3. Lead (II) acetate decahydrate_______________4. Silver dichromate__________5. Silicon tetraflouride__________6. Ammonium phosphate __________7. Copper (I) iodide__________8. Iron (II) fluoride nonahydrate_____________9. Zinc hydrogen sulphite______________10. Manganese (IV) monohydrogen phosphate
trihydrate ________________
Name into Formula
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Formula into Name
1. NI3 _______________________________
2. Ca(OH)2 _______________________________
3. Fe2(SO4)3.H2O _______________________________
4. (NH4)2C2O4 _______________________________
5. Co3(PO4)2.8H2O_______________________________
6. H3PO4 _______________________________
7. HClO2 _______________________________
8. N3O _______________________________
9. HI _______________________________10. Mg3P2 _______________________________
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Chemical Changes
• Nothing is created or destroyed, only rearranged• Reactants = products• 200 yrs ago John Dalton realized
atoms rearrange • # of each atom in reactants = # of each atom in products
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The LAW: Conservation of mass• Antoine and Marie-Anne Lavoisier in the 1700’s
• Atoms are neither created or destroyed in chemical reactions
• Mass reactants = mass products
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Indicators of chemical change
1. Colour changes2. Temperature changes3. A gas is produced4. A precipitate (solid form
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Chemical Reactions
• Occur when new substances are createdreactants products
Can be written as:• A word equation:
nitrogen monoxide + oxygen nitrogen dioxide• A symbolic equation:
2NO(g) + O2(g) 2NO2(g)
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Word equations (the simplest)
Potassium metal + oxygen gas potassium oxide
Provides limited information
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Skeletal Equations (Symbolic)
• Show formulas of compounds/elements, but not quantities of atoms
e.g.,K + O2 K2O
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Symbolic Equations
2NO(g) + O2(g) 2NO2(g)
Coefficients – indicate ratio of cmpdsState of matter – dissolved in water/aqueous (aq), solid (s), liquid (l), or gas (g)
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Balanced chemical equation• Shows all atoms and their quantities• Number of each atom should be equal on both
sides of the reaction arrow• Always use smallest whole-number ratio• To balance, change coefficients, never subscripts
e.g., 4K + O2 2K2O
HgO Hg + O2
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Helpful hints
1. Balance metals first2. Count polyatomic groups as 1 atom3. Balance oxygen atoms last4. Odd/even problem? Double it!
____Mg + ____HCl → ____MgCl2 + ____H2
____H2 + ____ N2 → ____ NH3
____ Fe + ____ Br2 → ____ FeBr3
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TRY THESE!____Sn(NO 2)4 ___K3PO4 → ___KNO2 ___Sn3(PO4)4
____P4 + ____I2 → ____PI3
____Al + ____O2 → ____Al2O3
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Today Learning check Review chemical compounds and formulas Chemical Reactions
#X#(s) A B Due tomorrow: workbook pages 71 and 73 Due Monday: workbook pages 77, (78-79 even #’s), 80