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Reduction Oxidation reduction reaction Oxidation number Half reaction Electrochemical process Battery Cathode Anode Electrolysis 149
The Learning Goal for this section is: The student will be able to relate activity and basicity to hydronium and hydroxyl ion concentration and pH. Acids and Bases The Observable Properties of Acids and Bases The words acid and alkaline (an older word for base) are derived from direct sensory experience. Acid Property #1: The word acid comes from the Latin word acere, which means "sour." All acids taste sour. Well known from ancient times were vinegar, sour milk and lemon juice. Aspirin (scientific name: acetylsalicylic acid) tastes sour if you don't swallow it fast enough. Other languages derive their word for acid from the meaning of sour. So, in France, we have acide. In Germany, we have säure from saure and in Russia, kislota from kisly. Base Property #1: The word "base" has a more complex history (see below) and its name is not related to taste. All bases taste bitter. For example, mustard is a base. It tastes bitter. Many medicines, because they are bases, taste bitter. This is the reason cough syrups are advertised as having a "great grape taste." The taste is added in order to cover the bitterness of the active ingredient in cough syrup. Acid Property #2: Acids make a blue vegetable dye called litmus turn red. Base Property #2: Bases are substances which will restore the original blue color of litmus after having been reddened by an acid. Acid Property #3: Acids destroy the chemical properties of bases. Base Property #3: Bases destroy the chemical properties of acids. Neutralization is the name for this type of reaction. Acid Property #4: Acids conduct an electric current. Base Property #4: Bases conduct an electric current. This is a common property shared with salts. Acids, bases and salts are grouped together into a category called electrolytes, meaning that a water solution of the given substance will conduct an electric current. Non-electrolyte solutions cannot conduct a current. The most common example of this is sugar dissolved in water. 150
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Chemistry Notebook By: Joel J
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Unit 1 Measurement Lab Separation o
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Unit 5 (28 days) Chapter 10 Chemica
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30. Always lubricate glassware (tub
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Chapter 1 Unit 1 Introduction to Ch
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To use the Stair-Step method, find
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Using SI Units Match the terms in C
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Standards of Measurement Fill in th
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SCIENTIFIC NOTATION RULES How to Wr
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Convert each number from Scientific
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Significant Figures Rules There are
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How Many Significant Digits for Eac
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The following rule applies for mult
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1qt=32 oz 1gal = 4qts 1.00 qt = 946
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Chapter 5 Electrons in Atoms The st
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Atoms Are Building Blocks Atoms are
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Electrovalence Don't get worried ab
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Summary Atoms are essentially the b
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Electron Configuration Color the su
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Electron Configuration In order to
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Calcium (Ca) Nickel (Ni) Carbon (C)
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Research the Scientist and summariz
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Using Wikipedia, define the 8 categ
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Ionization Energy Define Ionization
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Ion Size Define Ion Size: Ion size
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Chapter 7 Ionic and Metallic Bondin
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10. Name __________________________
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The Nucleus A typical model of the
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Gamma Radiation After a decay react
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This analysis shows that sodium has
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Metals, with only a few electrons i
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POLAR BONDING results when two diff
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Step 6 Put the atoms in the structu
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Trigonal Planal Molecular Geometry
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Tetrahedral Molecular Geometry Orbi
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Bent Molecular Geometry Orbital Equ
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T-Shaped Molecular Geometry Orbital
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Square Planar Molecular Geometry Or
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sp 3 d 2 AX6 None 90 Octahedral sp
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Chapter 9 Unit 4 Chemical Names and
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Learning Goals: Describe the proper
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Unit 5 Chapter 10 Chemical Quantiti
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www.youtube.com/watch?v=AsqEkF7hcII
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Categories of Reactions All chemica
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List what type the following reacti
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How to Balance Chemical Equations A
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Step 5 Balance the hydrogen atoms n
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6) ___ Mn(NO2)2 + ___ BeCl2 ___ Be
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The Learning Goal for this assignme
Page 101 and 102: Stoichiometry and Balanced Equation
Page 103 and 104: Step 1: 200g C3H8 is equal to 4.54
Page 105 and 106: Stoichiometry and balanced equation
Page 107 and 108: %yield = 6.1 tons × 100 = 64% 9.6t
Page 109 and 110: Use the space provided to write out
Page 111 and 112: Unit 6 Chapter 13 States of Matter
Page 113 and 114: The Learning Goal for this assignme
Page 115 and 116: uniform internal structure, and amo
Page 117 and 118: Volume Pressure Temperature is Aver
Page 119 and 120: Volume and temperature (in Kelvins)
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Page 125 and 126: Combined Gas Law: This gas law comb
Page 129 and 130: Unit 7 Chapter 16 Solutions The stu
Page 133 and 134: Part 5: Molarity Molarity (M) is th
Page 137 and 138: The Time-Temperature Graph We are g
Page 139 and 140: Step Two: solid ice melts Now, we c
Page 141 and 142: Step Four: liquid water boils Now,
Page 143 and 144: The following table summarizes the
Page 145 and 146: The Learning Goal for this section
Page 147 and 148: B. decreasing the concentration of
Page 149 and 150: everse reaction rate as well. 11. I
Page 151: Unit 8 Chapter 19 Acid and Bases Th
Page 155 and 156: This would be a generic base: XOH -
Page 157 and 158: HCl + H2O ⇌ H3O + + Cl¯ HCl - th
Page 159 and 160: Several categories of substances ca
Page 161 and 162: 1. 2.82 2. 8.30 3. 0.00 4. 3.485 5.
Page 165: 2. What is the oxidation number of
Page 170 and 171: Table E Selected Polyatomic Ions Fo
Page 172 and 173: Table H Vapor Pressure of Four Liqu
Page 174 and 175: Table K Common Acids Table N Select
Page 176 and 177: Table R Organic Functional Groups C
Page 178 and 179: Table S Properties of Selected Elem
Page 180 and 181: Table T Important Formulas and Equa
Page 182 and 183: CHEMISTRY EXAM FORMULA AND RESOURCE
Page 184: Activity Series of Metals Name Symb
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