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Agenda: 3/27• Objective: to predict products in a chemical reaction
• Warm-up: Formative Assessment
• Chemical Reactions
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Objective: To predict what a chemical reaction will produce
•What will we learn?
• Balancing equations • Types of reactions • When reactions will take place
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Objective: To predict what a chemical reaction will produce
•What do we need to know?
• Names and formulas• Indicators of chemical change • Moles
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CHEMICAL REACTIONS
Reactants: Zn + I2 Product: Zn I2
")!
What are the indicators that there is a chemical reaction?
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What is a chemical reaction?
• Atoms are combined into compounds or separated and then rearranged.
• New substances must be formed• New physical and chemical properties
• Energy is always involved
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Notes: 1. Chemical Reactions• Process in which substances (reactants) change into
1 or more different substances (products)
Reactants → Products
Yields
Products have different physical and chemical properties than the reactants.
Explain why in your notes:
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Notes: Energy is always involved:
- In exothermic reactions, energy is released.
- In endothermic reactions, energy is added (absorbed)
Energy change (∆H = change in heat) is shown 2 ways:
Exothermic: ∆H = - or shown as a product
Endothermic: ∆H= + or shown as a reactant
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Notes: Chemical Change must take place.
• Indicators of chemical change:
1: change in temperature
2: producing bubbles (gas) without boiling
3: change in color
4: a precipitate is formed (solid from 2 liquids)
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Introduction: Chemical EquationsTheir Job: Way to represent the relative amounts of reactants and products and their relative amounts in a reaction.
4 Al (s) + 3 O2 (g) ---> 2 Al2O3 (s)
The numbers in the front are called coefficients.
____________The letters (s), (g), and (l) are the physical states of compounds.
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Word Equation for the reaction:The carbon reacts with oxygen to yield carbon dioxide.Chemical equation: C + O2 CO2
This contains the same information as the English sentence but has quantitative meaning as well.
The charcoal used in a grill isbasically carbon.
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Notes: Chemical Equations• Way to represent the relative amounts of reactant and
product. (A recipe)
• Satisfies the Law of Conservation of Matter (Mass)
Atoms are not created nor destroyed in a chemical reaction (just re-arranged)
Mass is neither created nor destroyed in a chemical reaction.
There must be the same amount of mass on the product side (after the reaction) as the reactant side (before the reaction.)
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• Solid ___• Liquid ____• Gas ___• Aqueous solution (aq)• Reversible reactions• Reactants are heated
• Catalyst H2SO4
• Escaping gas ()
Notes: Symbols Used in Equations
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Because of the principle of the conservation of matter,
an equation must be balanced.
It must have the same number of atoms of the same kind on both sides.
Introduction: Chemical Equations
Lavoisier, 1788
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BALANCING CHEMICAL REACTIONS
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Balancing EquationsBalancing Equations
___ Al(s) + ___ Br2(l) ---> ___ Al2Br6(s)
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• When balancing a chemical reaction Coefficients are added in front of a compounds to balance the reaction, but
you may not change the subscripts.
• Changing the subscripts changes the compound.
Important in Balancing Equations
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Subscripts vs. Coefficients
• The subscripts shows: ?
• The coefficient shows: ?
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Why balance chemical reactions?• Law of Conservation of Matter:
• matter is neither created nor destroyed in __ ________ _________.
• In a chemical reaction, atoms are combined, separated and/or rearranged.
• Not atoms are lost or gained in a chemical reaction.
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In a balanced reaction• Chemical reactions are shown with symbols (formulas in
an equation) • Starting materials = reactants • Produces, yields = arrow• End materials = products
• # atoms of reactants= # atoms of products
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Steps to balance equations:• Start with correct formulas for the compounds.
• Never, never change the formula (subscripts) • Put a box around the formulas as a reminder.
• Count how many atoms of each type of element on each side of the equation.
• Use multipliers (called coefficients) in front of the formulas on each side of the equation until the number on each side matches up.
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Notes: Methane and oxygen produces carbon dioxide and water.1. Correct formulas and symbols.• Put box around each formula.
2. Count the number of atoms on both sides of the equation
Methane + oxygen carbon dioxide + water
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Notes: Methane and oxygen produces carbon dioxide and water.3. Balance the equation using coefficients.(Coefficients are multipliers in front of the compounds)
4. Use the smallest whole number possible.
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Examples: • Copper and silver (I) nitrate combine to yield copper (II)
nitrate and silver.
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Examples• The reactants magnesium and aluminum chloride produce
aluminum and magnesium chloride.
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Examples for your notes: • Carbon reacts with oxygen to produce carbon dioxide.
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Practice balancing equations• ____ Ca + ____ O₂ ____ CaO
• ____ Br₂ + ____ LiF ____ LiBr + ____ F₂
• ____ V + ____ ZnBr₂ ____ VBr₃ + ____ Zn
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• ____ Li + ____ Pb(OH)₂ ____ Pb + ____ LiOH
• ____ C₄H₈ + ____ O₂ ____ CO₂ + ____ H₂O
• ____ Ga(OH)₃ + ____ KF ____ KOH + ____ GaF₃
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Chemical EquationsChemical Equations4 Al(s) + 3 O2(g) ---> 2 Al2O3(s)
This equation means
4 Al atoms + 3 O2 molecules ---produces--->
2 molecules of Al2O3
AND/OR
4 moles of Al + 3 moles of O2 ---produces--->
2 moles of Al2O3
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Balancing EquationsBalancing Equations
____C3H8(g) + _____ O2(g) ---->
_____CO2(g) + _____ H2O(g)
____B4H10(g) + _____ O2(g) ---->
___ B2O3(g) + _____ H2O(g)
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Balancing EquationsBalancing EquationsSodium phosphate + iron (III) oxide sodium oxide +
iron (III) phosphate
Na3PO4 + Fe2O3 ---->
Na2O + FePO4
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____ P + O2 → P4O10 ____ Mg + O2 → MgO
____ HgO → Hg + O2 ____ Al2O3 → Al + O2
____ Cl2 + NaBr → NaCl + Br2 ____ H2 + N2 → NH3
Balancing chemical reactions
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____ Na + Br2 → NaBr ____ CuCl2 + H2S → CuS + HCl
____ HgO + Cl2 → HgCl + O2 ____ C + H2 → CH4
____ KClO3 → KCl + O2 ____ S8 + F2 → SF6
____ BaCl2 + Na2 SO4 → NaCl + BaSO4