Edward Valadez

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Covalent H - O 2+ H20,OH, H30 1,2,3,4 1same no prefix 2 di 3 tri 4 tetra CaF F 3 0 2 KO Potassium Oxide KO is WRONG its K 2 O SBr 2 = Sulfur DiBromide Br S Br NF 3 = Nitrogen Tri-Fluoride F N F F
Covalent bond A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding.[1] For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full outer shell, corresponding to a stable electronic configuration. Covalent bonding includes many kinds of interactions, including σ-bonding, π-bonding, metalto-metal bonding, agostic interactions, and three-center two-electron bonds.[2][3] The term covalent bond dates from 1939.[4] The prefix co- means jointly, associated in action, partnered to a lesser degree, etc.; thus a "co-valent bond", in essence, means that the atoms share "valence", such as is discussed in valence bond theory. In the molecule H 2, the hydrogen atoms share the two electrons via covalent bonding.[5] Covalency is greatest between atoms of similar electronegativities. Thus, covalent bonding does not necessarily require the two atoms be of the same elements, only that they be of comparable electronegativity. Covalent bonding which entails sharing of electrons over more than two atoms is said to be delocalized.
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Edward Valadez YEAR 2014
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Unit 1 Measurement Lab Separation o
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Unit 4 (15 days) Chapter 10 Chemica
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29. Never handle broken glass with
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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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SCIENTIFIC NOTATION RULES How to Wr
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1. 7,485 6. 1.683 2. 884.2 7. 3.622
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Significant Figures Rules There are
Page 32 and 33: Rule 3: A final zero or trailing ze
Page 34 and 35: 16) 3.88 x 10 = 3 17) 3004 = ____4_
Page 36: 15) 8000 ÷ 4.62 = __________ 16) 0
Page 40 and 41: 2. One cereal bar has a mass of 37
Page 42 and 43: 1. How many meters are in one kilom
Page 44 and 45: Dimensional Analysis This is a way
Page 47: Converting Real Things Table 1 Usin
Page 50 and 51: http://www.learner.org/interactives
Page 53: Electrovalence Don't get worried ab
Page 56: P N P N
Page 60 and 61: www.youtube.com/watch?v=jtYzEzykFdg
Page 62: In the space below, write the unabb
Page 70 and 71: Increases Atomic Size Increases Top
Page 72 and 73: Electronegativity Increases Electro
Page 74 and 75: Create groups for these Scientist a
Page 76 and 77: Radioactivity was discovered my Ant
Page 78 and 79: The students will learn how ionic c
Page 80 and 81: Metallic bounding Notes Lattice- a
Page 84 and 85: Name Formula Charge Dichromate Cr
Page 86 and 87: Bent Bent Octahedral Square Planar
Page 88 and 89: The Mole www.youtube.com/watch?v=As
Page 90 and 91: Mole Conversions The Three Steps to
Page 94 and 95: How to Balance Chemical Equations A
Page 96 and 97: Step 5 Balance the hydrogen atoms n
Page 98 and 99: 6) ___ Mn(NO 2 ) 2 + ___ BeCl 2 __
Page 100 and 101: Categories of Reactions All chemica
Page 102 and 103: 1) NaOH + KNO 3 --> NaNO 3 + KOH 2)
Page 104 and 105: Balancing Equations Practice Proble
Page 107 and 108: Percent Yield Practice Problems fro
Page 109 and 110: Liquids Liquids have a definite vol
Page 111 and 112: Changes of State When a solid is he
Page 113 and 114: Boyle’s Law States that for a giv
Page 115 and 116: Example http://www.youtube.com/watc
Page 117 and 118: Formula and Usage V 1 / T 1 = V 2 /
Page 119 and 120: Gay-Lussac’s Law States that if a
Page 121 and 122: Example http://www.youtube.com/watc
Page 123 and 124: Notes PV = nRT P = pressure V = vol
Page 125: Unit 5 Chapter 13 States of Matter
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Edward Valadez

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