Final Chemistry Notebook

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Sulfur hexafluoride Chemical Name Sf 6 Chemical Formula Octahedral Sp 3 d 2 Molecular Geometry none Side View Orbitals Lone Pairs Molecular Drawing With Angles Top View Xenon Tetraflouride Chemical Name XEF 4 Chemical Formula Square Planar Molecular Geometry Sp 3 d 2 2 Side View Orbitals Lone Pairs Molecular Drawing With Angles Top View 77
Finding Bond Angles, Shapes, and Hybridizations Sometimes people have a hard time with the whole VSEPR thing. In this helpdesk section we'll discuss what VSEPR means, what it's all about, and how you can use a great big flow chart to figure out the bond angles, shapes, and hybridizations of various covalent compounds. This whole thing assumes, by the way, that you know how to draw Lewis structures. If you don't, click here. What is VSEPR? VSEPR stands for Valence Shell Electron Pair Repulsion. It's a complicated acronym, but it means something that's not difficult to understand. Basically, the idea is that covalent bonds and lone pair electrons like to stay as far apart from each other as possible under all conditions. This is because covalent bonds consist of electrons, and electrons don't like to hang around next to each other much because they have the same charge. This VSEPR thing explains why molecules have their shapes. If carbon has four atoms stuck to it (as in methane), these four atoms want to get as far away from each other as they can. This isn't because the atoms necessarily hate each other, it's because the electrons in the bonds hate each other. That's the idea behind VSEPR. What is hybridization (AP <strong>Chemistry</strong>)? Now, one problem with the whole VSEPR thing is that if you have four things stuck to carbon, for example, there are no orbitals that want to get 109.5 degrees apart from each other (109.5 degrees corresponds to the geometric maximum distance the atoms can get apart). After all, s-orbitals go in a complete sphere (360 degrees) and p-orbitals are 90 degrees apart. What happens instead of using s- or p- orbitals is that when covalent bonds are formed, the s- and p- orbitals mix to form something called hybrid orbitals. "Hybrid" just means "mixture of two different things", and that's exactly what a hybrid orbital is. When three p-orbitals with 90 degree angles combine with one s-orbital with 360 degrees, they average to form four sp3 orbitals with 109.5 degree bond angles. Depending on the numbers of s- and p-orbitals that mix, you can get a bunch of different bond angles. Common shapes you should know There are a whole bunch of common shapes you need to know to accurately think of covalent molecules. Here they are: Tetrahedral: Tetrahedral molecules look like pyramids with four faces. Each point on the pyramid corresponds to an atom that's attached to the central atom. Bond angles are 109.5 degrees. Trigonal pyramidal: It's like a tetrahedral molecule, except flatter. It looks kind of like a squished pyramid because one of the atoms in the pyramid is replaced with a lone pair. Bond angles are 107.5 degrees (it's less than tetrahedral molecules because the lone pair shoves the other atoms closer to each other). Trigonal planar: It looks like the hood ornament of a Mercedes automobile, or like a peace sign with that bottom-most line gone. The bond angles are 120 degrees. 78
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. Chemistry Honors Notebook 2017-20
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Table E Selected Polyatomic Ions Fo
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Table H Vapor Pressure of Four Liqu
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Table K Common Acids Table N Select
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Table R Organic Functional Groups C
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Table S Properties of Selected Elem
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Table T Important Formulas and Equa
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Activity Series of Metals Name Symb
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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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7
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Print vs. print Online vs. online P
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11 To use the Stair-Step method, fi
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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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25 The following rule applies for m
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1qt=32 oz 1gal = 4qts 1.00 qt = 946
Page 47 and 48: Chapter 6 The Periodic Table The st
Page 49 and 50: Atoms Are Building Blocks Atoms are
Page 51 and 52: Electrovalence Don't get worried ab
Page 53 and 54: Summary Atoms are the most importan
Page 55 and 56: Research the Scientist and summariz
Page 57 and 58: 39 Electron Configuration Color the
Page 59 and 60: Electron Configuration In order to
Page 61 and 62: Ca= Calcium Ni=nickel C=carbon Xe=x
Page 64: 10. Name __________________________
Page 67 and 68: Using Wikipedia, define the 8 categ
Page 69 and 70: Define Ionization Energy: Ionizatio
Page 71 and 72: 51 Define Ion Size: Ion Size Ion si
Page 73 and 74: The Nucleus A typical model of the
Page 75 and 76: Gamma Radiation After a decay react
Page 77 and 78: Nuclear Fission The word fusion mea
Page 79 and 80: Students will be able to predict sh
Page 81 and 82: electrons in the outer energy level
Page 83 and 84: Non-metals, which lack only one or
Page 85 and 86: AlCl3+ HgI2 But remember to look ba
Page 87 and 88: POLAR BONDING results when two diff
Page 89 and 90: Step 6 Put the atoms in the structu
Page 91: Orbitals Equation Lone Pairs Angle
Page 94 and 95: Carbon dioxide Chemical Name CO 2 C
Page 96 and 97: Hydronium Chemical Name H 3 O + Che
Page 100 and 101: Bent: They look, well, bent. Bond a
Page 102 and 103: 4. the chlorine atom in hydrochlori
Page 104 and 105: Chapter 23 Functional Groups The st
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Page 108 and 109: anched chains: Hexane - a 6-carbon
Page 110 and 111: Isomers Because carbon can bond in
Page 112 and 113: Chapter 12 Stoichiometry The studen
Page 114 and 115: Other atomic weights are listed on
Page 116 and 117: Find Molecular Mass 1- 10 1. NaBr N
Page 118 and 119: Right side: 1 carbon, 2 hydrogen an
Page 120 and 121: Add a coefficient of 5 to the oxyge
Page 122 and 123: 1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2
Page 124 and 125: 4) Double displacement: This is whe
Page 126 and 127: Decomposition ab=>A+B Determine the
Page 128 and 129: we can determine that 2 moles of HC
Page 130 and 131: When there is no limiting reagent b
Page 132 and 133: Example 7 How much 5M stock solutio
Page 134 and 135: Theoretical and Actual Yields Key T
Page 136 and 137: Review Purposes To get an over
Page 138 and 139: STP-Standard Temperature And Pressu
Page 140 and 141: Chapter 14 The Behavior of Gases Th
Page 142 and 143: CORNELL NOTES Learning Goal: Differ
Page 144 and 145: Questions/Main Ideas NOTES 13.4 cha
Page 146 and 147: It is important that you realize th
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127 3. The pressure of nitrogen gas
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This formula is strictly valid only
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dissolved in water. All electrolyte
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Create and interpret potential ener
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Structure effects: determines what
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Specific Heat Here is the definitio
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Step One: solid ice rises in temper
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Step Three: liquid water rises in t
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Step Five: steam rises in temperatu
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then it is exothermic, meaning the
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Define the types of reactions. Give
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1. If this compound was at room tem
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1. In what part of the curve would
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Reduction Oxidation reduction react
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So far, the properties have an obvi
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The acid base theory of Brønsted a
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IV. Problems with the Theory This t
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Let's discuss significant figures a
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On your calculator you would input
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Ag+ + Cu ---> Ag + Cu2+ I have deli
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7. Half Reactions A half-reaction i
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Notice that each separate substance
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