Reminders End of semester Fri. Jan 24 th (15 school days) Finals Jan 22-24 Chp 6 E.C. (Passed out...
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Transcript of Reminders End of semester Fri. Jan 24 th (15 school days) Finals Jan 22-24 Chp 6 E.C. (Passed out...
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Reminders
• End of semester Fri. Jan 24th (15 school days)
• Finals Jan 22-24
• Chp 6 E.C. (Passed out today/ due Mon. Jan 13th)
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One cool thing you did over break…
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Today
• Chp 9 Learning Targets
• Unexpected Changes Lab
• Introduction to Chp 9
• Handout E.C. assignment
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Chapter 9(Last one for the semester!)
Chemical Reactions and Writing Equations
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1/6/14 Learning Targets
• Describe the characteristics of a chemical reaction.
• Explain how a chemical equation describes what happens in a chemical reaction.
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Important Terms:
• Chemical Change (Reaction)- a process in which pure substance(s) are converted into different pure substance(s)
• Conservation of Matter- in chemical and physical reactions, matter is neither created nor destroyed
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Examples
Combustion of Ethanol
Oxidation of Iron
Precipitation of Silver
Formation of Coral Reefs (from Calcium Carbonate)
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How do we describe/represent what happens in a chemical reaction?
Reactants- substances which are present before a chemical reaction
Products- substances which are present after a chemical reaction
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What causes chemical reactions?
• What do we know about the importance of valence electrons?
Chemical reactions provide atoms the opportunity to achieve a full set of valence electrons and
become more stable (more energetically favorable)
Since some elements/molecules are already stable, energy sometimes has to be supplied to initiate a
chemical reaction (think back to the flame test lab) (strike a match!)
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Reminders
• End of semester Jan 24 (14 school days)
• Finals Jan 22-24
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1/7/14 Learning Targets
• Explain how a balanced chemical equation illustrates the law of conservation of matter.
• Understand the five general types of reactions and how to balance them.
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Types of Chemical Reactions1) Synthesis2) Decomposition3) Single Replacement4) Double Replacement5) Combustion
By knowing the type of reaction that is occurring, you can predict the products that will be formed.
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Chemical Equations- How we describe what is happening
Using Words-Hydrogen reacts with oxygen to form (or yield)
water
Using Formulas and Symbols
2H2 + O2 2H2O
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Breaking down the Notation of Chemical Equations
2H2(g) + O2(g) 2H2O(l)
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Describing the physical state of each substance
■Solid (s)■Liquid (l)■Gas (g)■Aqueous (aq)means dissolved in water
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Coefficient
• Like in math, the coefficient is the number placed in front of a formula. This number indicates the quantity of each molecule or atom in the reaction.
• Ex. 2Ca(s) + O2(g) 2CaO(g)
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Symbols used in Chemical Equations
• Double arrow indicates a reversible reaction
• Shows that heat is supplied to the reaction
• Used to indicate a catalyst is supplied, in this case, platinum.
All of these are special conditions
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Balancing Chemical Equations
• Since the conservation of mass says matter is neither created nor destroyed, we have to make sure our equation agrees
• # reactant atoms must = # product atoms
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Step 1: Balancing Equations
• Write the word equation that describes the reaction.
iron reacts with oxygen to yield iron oxide
Or
Iron + Oxygen Iron Oxide
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Step 2: Balancing Equations
2. Replace the words in the equation withsymbols and formulas.
Fe + O2 Fe2O3
Do we have the same numbers of each element on both sides of arrow?
Does this follow the law of conservation of matter?
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Step 3: Balancing Equations
3. Count the # of atoms of each elementon both sides of the equation.
Fe + O2 Fe2O3
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Step 4: Balancing Equations
4. Starting with elements that only occurin one substance on each side of theequation, make sure that each side of theequation has an equal # of that element.
Proceed with all elements.
Remember that changing the # of one element may alter elements that have already been balanced.
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Fe + O2 ―› Fe2O3
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Let’s try:
CH4 +2O2 CO2 + 2H2O
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• Never change a subscript to balance an equation.■ If you change the formula you are describing a
different reaction.
■H2O is a different compound than H2O2
• Never put a coefficient in the middle of a formula■ 2 NaCl is okay, Na2Cl is not.
!
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Step 5: Check Your Work5. Make sure that the equation is properly
balanced.
CH4 + 2O2 CO2 + 2H2O
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Balancing Equations: Examples
■ H2 + O2 → H2O
■ Co + O2 → Co2O3
■ Pb(NO3)2 + K2S → PbS + KNO3
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Balance the following
iron(II) chloride + sodium phosphate → sodium chloride + iron (II) phosphate
FeCl2 + Na3PO4 → NaCl + Fe3(PO4)2
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Today
■ Look at 3 different types of reactions.
■ Begin “Single-Replacement Lab” set-up.
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Five General Types of Chemical Reactions
• Direct Combination (Synthesis)• Decomposition• Single-Replacement• Double-Replacement• Combustion
By knowing the type of reaction that is occurring, you can predict the products that will be formed.
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I. Direct Combination Reactions (also called synthesis reactions).
General form: A + B → AB (two reactants make a single product)
A, B = elements or compoundsAB = compound consisting of A
and B
■ This is the only type of chemical reaction in which there is a single product formed. This single product is always more complex than the reactants.
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Examples of Synthesis Reactions
■calcium + oxygen yields calcium oxide
2Ca + O2 → 2CaO
■ carbon dioxide + water yields carbonic acidCO2 + H2O → H2CO3
■ Notice: All equations show two (or more) reactants, but only one product.
■ http://www.ric.edu/ptiskus/reactions/Index.htm
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II. Decomposition Reactions
General form: AB → A + B (one reactant makes two or more
products)
AB = compoundA, B = elements or simpler
compounds
▪ This is the only type of chemical reaction in which there is a single reactant. This single reactant is always more complex than the products.
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Decomposition Reactions: Examples
■ water yields hydrogen and oxygen2H2O → 2H2 + O2
■ marble (calcium carbonate) yields calcium oxide and carbon dioxideCaCO3 → CaO + CO2
■ Notice: all equations show a single reactant decomposing into two (or more) products.
■ http://www.ric.edu/ptiskus/reactions/Index.htm
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III. Single-Replacement Reactions
General Form: A + BX → AX + BOne element and one compound
recombine (switch partners)AX, BX = ionic compounds
A, B = MetalsX = ion that switches partners
*Metal ‘A’ must be more reactive than ‘B’ for this to occur
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Single-Replacement Examples
■ Copper metal and silver nitrate:
Cu + AgNO3 → CuNO3 + Ag
■ Notice: In the reaction, an copper combines with silver nitrate to create copper nitrate and silver
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■ Zn + HCl → ZnCl2 + H2
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IV. Double-Replacement Reactions
General form: AX + BY → AY + BX(Positive ions in two compounds are exchanged)
A,B = positive ionsX,Y = negative ions
■ This is the only type of chemical reaction with two compounds as reactants and two compounds as products.
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Double Replacement Examples
■ calcium carbonate and hydrochloric acid yield calcium chloride and carbonic acid
CaCO3 + 2HCl → CaCl2 + H2CO3
■Notice: in this reaction, two ionic compounds exchange ions to form two new ionic compounds
www.ric.edu/ptiskus/reactions/Index.htm
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IV. Double-Replacement Reactions
General form: AX + BY → AY + BX(Positive ions in two compounds are exchanged)
A,B = positive ionsX,Y = negative ions
■ This is the only type of chemical reaction with two compounds as reactants and two compounds as products.
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Double Replacement Examples
■ calcium carbonate and hydrochloric acid yield calcium chloride and carbonic acid
CaCO3 + 2HCl → CaCl2 + H2CO3
■Notice: in this reaction, two ionic compounds exchange ions to form two new ionic compounds
www.ric.edu/ptiskus/reactions/Index.htm
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Rules of Double-Replacement Reactions
■ Reactants must be dissolved in water (releasing the ions).
■ Will occur if one of the products :• is a molecule (covalent), • a precipitate (solid comes out of
solution), or• an insoluble gas.
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V. Combustion Reactions
General Form: CxHy + O2 → H2O + CO2
(hydrocarbon and oxygen react to form carbon dioxide and water)
■ This is the only type of chemical reaction where something reacts with oxygen and forms carbon dioxide and water
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Combustion Examples
▪ Methane reacts with oxygen:CH4 (methane) + O2 → H2O + CO2
▪ Gasohol reacts with oxygen:C2H5OH (ethanol) + O2 → H2O + CO2
▪ Notice: in both cases, water and carbon dioxide are the products.
www.ric.edu/ptiskus/reactions/Index.htm
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1. Write the word equation2. Write the balanced formula equation■ Solid iron (III) sulfide reacts with
gaseous hydrogen chloride to form iron (III) chloride and hydrogen sulfide gas.
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1. Write the word equation2. Write the balanced formula equation
■ Nitric acid reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate.