pg1 pg2 pg3 pg4 pg5 pg6 pg7 pg8 pg9 pg10 pg11 Chemical Reactions Academic Chemistry Summary: Chemical reactions require the use of the law of conservation of mass to write, predict, balance, understand, and differentiate among oxidation-reduction (synthesis, decomposition, and single-replacement), precipitation (double-replacement), and acid-base reactions (neutralization). Objectives: Use the law of conservation of mass to write and balance chemical equations Understand and differentiate among acid-base reactions and oxidation-reduction reactions Vocabulary: atoms, molecules, compounds, acid, base, polyatomic ions, oxidation number, coefficient, subscript, catalyst, reactant, product, aqueous, precipitate, synthesis, decomposition, single-replacement, double-replacement, oxidation-reduction, combustion, neutralization, endothermic, exothermic Memorize: Provided: Periodic table CHECKLIST: How to be successful in OTHS Academic Chemistry Pay attention and take notes in class Ask questions in class on material that is not clear Work every page in the practice packet for the unit Check answers to the practice packet online at http://othschem.weebly.com/ Come to tutorials with any chemistry teacher Do the online homework and check solutions once they become available Always do the practice test for every test & ask good questions on review day Keep up with the calendar for the class/be aware of approaching quizzes, tests, & other deadlines Use videos posted on website as a quick and convenient tutorial Read the chapter in the book
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pg1 pg2 pg3 pg4 pg5 pg6 pg7 pg8 pg9 pg10 pg11
Chemical Reactions Academic Chemistry
Summary: Chemical reactions require the use of the law of conservation of mass to write, predict, balance,
understand, and differentiate among oxidation-reduction (synthesis, decomposition, and single-replacement), precipitation (double-replacement), and acid-base reactions (neutralization). Objectives: Use the law of conservation of mass to write and balance chemical equations
Understand and differentiate among acid-base reactions and oxidation-reduction reactions
CHECKLIST: How to be successful in OTHS Academic Chemistry
Pay attention and take notes in class Ask questions in class on material that is not clear Work every page in the practice packet for the unit Check answers to the practice packet online at http://othschem.weebly.com/ Come to tutorials with any chemistry teacher Do the online homework and check solutions once they become available Always do the practice test for every test & ask good questions on review day Keep up with the calendar for the class/be aware of approaching quizzes, tests, & other deadlines Use videos posted on website as a quick and convenient tutorial Read the chapter in the book
Formula Writing/Equation Writing Practice Worksheet
1. Classify the compound as Ionic, Molecular, Acid, or Base. Write the formula for the compound. Classify Formula
a. aluminum hydroxide ______________ ___________________
b. sodium oxide ______________ ___________________
c. hydrofluoric acid ______________ ___________________
d. potassium phosphate ______________ ___________________
e. copper (I) sulfate ______________ ___________________
f. phosphorus pentabromide ______________ ___________________
2. Equation writing: Convert all chemical names to formulas and write a balanced equation. a. Solid barium reacts with oxygen gas to produce solid barium oxide.
b. Solid iron (III) oxide decomposes to form metallic iron (solid) and oxygen gas.
c. Solid iron and aqueous copper (II) sulfate react to form solid copper and aqueous iron (III) sulfate.
d. Aqueous copper (II) chloride and aqueous lead (IV) nitrate react to form aqueous copper (II) nitrate and solid lead (IV) chloride.
e. Metallic magnesium (solid) reacts with aqueous silver nitrate to form aqueous magnesium nitrate and metallic (solid) silver.
f. Aqueous sulfuric acid reacts with aqueous potassium hydroxide to form aqueous potassium sulfate and water.
g. Chlorine gas reacts with aqueous potassium bromide to form aqueous potassium chloride and liquid bromine.
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Directions: Write an example of an actual chemical reaction fitting each of the following types of reactions.
1. Synthesis: Example __________________________________________
2. Decomposition: Example __________________________________________
3. Single Replacement:
Example _____________________________________ Example _____________________________________
(Metal) (Halogen)
4. Double Replacement: Example __________________________________________
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Name Class Date
Types of Chemical Reactions
Write the type chemical reaction on the line—synthesis (combination), decomposition, combustion, single
replacement, or double replacement. Then, balance the equations using the lowest possible integers. For
questions 21 and 22, predict the products before balancing.
16. ___AlCl3 + ___NaOH 17. ___AgNO3 + ___KCl 18. ___Ba(NO3)2 + ___Li2SO4 The next 2 reactions are a special type of double replacement called neutralization. This occurs when an acid and a base react to form a salt + water. 19. ___ HCl + ___ KOH 20. ___ H2SO4 + ___ Ca(OH)2 V.
Name___________________________ Period ____ Date______
Oxidation Number Practice Based on the oxidation numbers known for the other element(s), determine the oxidation number of the underlined element. 1. Na2SO4 ______ 16. CO2 ______ 2. CaO ______ 17. CaCO3 ______ 3. K2CrO4 ______ 18. KClO4 ______ 4. Cr2O3 ______ 19. SO3 ______ 5. KIO3 ______ 20. Cu2O ______ 6. H2O ______ 21. KClO3 ______ 7. SO4
First, indicate the type of chemical reaction (synthesis, decomposition, single replacement, or double replacement). Then, label the oxidation numbers for each element in the reaction on both the reactants and products side. Last, identify which element has been oxidized and which has been reduced.
1. 2Ag + S Ag2S Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced
2. 2Na + FeCl2 2NaCl + Fe Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced
3. 2AlCl3 2Al + 3Cl2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced
4. Fe2O3 + 6HCl 2FeCl3 + 3H2O Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced
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5. 3Mg + N2 Mg3N2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced
6. 2NaBr +Cl2 2NaCl + Br2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced
7. 2HgO 2Hg + O2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced
8. 3Ca + 2AlCl3 3CaCl2 + 2Al Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced