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On your calculator you would input 10, ^, (-), 5 and you would get 0.00001. This is also the way to find the amount of OH + that are present in a base. To find the pH: -log(concentration) To find the concentration: 10 -pH Define these terms: pH scale A scale used to measure the acidity (or alkalinity) of a substance; the scale is measured from 1-14, 1 being most acidic, 14 being most basic, and 7 being neutral. Hydronium ion H - + or H 3O ,occurs when a proton attaches to a water molecule. Appears in solutions of acids, and behaves like a hydrogen ion. Arrhenius acid/base + Acid - any substance which delivers hydrogen ion (H ) to the solution Base - any substance which delivers hydroxide ion (OH- ) to the solution Lewis acid/base Base - Electron donor Acid - Electron acceptor Does NOT require solvent Does NOT require hydronium ion Bronsted-Lowry acid/base Acid - A substance from which a proton can be removed Base - A substacne that can remove a proton from an acid + *Remember* : Proton, hydrogen ion, and H all mean the same thing An acid is a "proton donor" A base is a "proton acceptor" Strong acid/base An acid or base with a high or low pH does not necessarily mean that it is stronger than another base or acid with a higher or lower pH. Strength is impacted by both pH and ionization energy. The more readily available the H + , or OH - , the more potent the base or acid. Weak acid/base An acid or base with a high low pH does not directly translate to it being stronger than another base with a higher or lower pH. Strength is determined by both pH and ionization energy. The harder it is to remove the H + or OH - , the weaker the base or acid. Neutralization reaction A reaction where enough of one substance (either basic or acidic) completely saturates the opposite substance (acid or base), so that there is neither an excess of hydronium, nor of hydroxide. Titration When a solution of known concentration is used to calculate the concentration of an unknown solution. Titrant - Known concentration added to Analyte - Unknown concentration until the reaction is entirely complete. 159
The Learning Goal for this assignment is: Describe oxidation reduction reactions in living and non-living systems. 1. Oxidation Numbers Redox Reactions Oxidation and reduction Every atom, ion or polyatomic ion has a formal oxidation number associated with it. This value compares the number of protons in an atom (positive charge) and the number of electrons assigned to that atom (negative charge). In many cases, the oxidation number reflects the actual charge on the atom, but there are many cases where it does not. Think of oxidation numbers as a bookkeeping exercise simply to keep track of where electrons go. 2. Reduction Reduction means what it says: the oxidation number is reduced in reduction. This is accomplished by adding electrons. The electrons, being negative, reduce the overall oxidation number of the atom receiving the electrons. 3. Oxidation Oxidation is the reverse process: the oxidation number of an atom is increased during oxidation. This is done by removing electrons. The electrons, being negative, make the atom that lost them more positive. I use this mnemonic to help me remember which is which: LEO the lion says GER. LEO = Loss of Electrons is Oxidation GER = Gain of Electrons is Reduction Another well-known mnemonic is this: OIL RIG OIL = Oxidation Is Loss (of Electrons) RIG = Reduction Is Gain (of Electrons) Another way is to simply remember that reduction is to reduce the oxidation number. Therefore, oxidation must increase the value. 4. Reduction-Oxidation Reactions There are many chemical reactions in which one substance gets reduced in oxidation number (reduction) while another participating substance gets increased in oxidation number (oxidation). Such a reaction is called called a REDOX reaction. The RED, of course, comes from REDuction and OX from OXidation. However, it is pronounced re-dox and not red-ox. Here is a simple example of a redox reaction: 160
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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
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Stoichiometry and Balanced Equation
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Step 1: 200g C3H8 is equal to 4.54
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Stoichiometry and balanced equation
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%yield = 6.1 tons × 100 = 64% 9.6t
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Use the space provided to write out
Page 111 and 112: Unit 6 Chapter 13 States of Matter
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Page 117 and 118: Volume Pressure Temperature is Aver
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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 and 152: Unit 8 Chapter 19 Acid and Bases Th
Page 153 and 154: The Learning Goal for this section
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: 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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