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Ion

Rubric

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Socratic Seminar Rubric Name:____________________________ Date: _____________ Period: ____________ ?The student makes several comments during the seminar (4-5) ?The comments express original, deep thinking: beyond the literal, debatable, supported by the text. The comments may extend a previous comment, delving deeper into a previously mentioned issue or topic. ?The comments always/mostly refer to the text for supporting arguments, and that cited text is both a perfect match for the given argument and one that is not obvious to the group. ?The student always listens (by asking a follow-up question, responding to one, or jotting down notes.) ?The student gives evidence, states connections to related topics/texts, provides an

Bonding Structure

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Chemical? ?Bonding? ?and? ?Structure 1.1? ?chemical? ?bonding:? ?the? ?attraction? ?between? ?particles Atoms Ions Molecules Smallest? ?unit? ?of? ?elements? ?that cannot? ?be? ?broken? ?down? ?into anything? ?simpler Atoms? ?that? ?are? ?covalently? ?bonded and? ?carry? ?an? ?overall? ?electrical charge Groups? ?of? ?atoms? ?that? ?are covalently? ?bonded Calcium? ?atom,? ?carbon? ?atom Calcium? ?ion,? ?oxide? ?ion Carbon? ?dioxide? ?molecule 1.2? ?Metallic? ?bond 1.2.1? ?Bonding? ?and? ?Structure - Metallic? ?bond? ?is? ?the? ??electrostatic? ?force? ?of? ?attraction?? ?between? ??positive? ?metal? ?ions?? ?and? ?the? ??sea? ?of delocalised? ?electrons - Giant? ?metallic? ?lattice? ?structure - Non-directional

Organic Chemistry Lecture 12b

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Chapter 12 * IR Spectrum of Amides Amides will show a strong absorption for the C?O at 1630?1660 cm-1. If there are hydrogens attached to the nitrogen of the amide, there will N?H absorptions at around 3300 cm-1. Chapter 12 * Carbon?Nitrogen Stretching C?N 1200 cm-1 C?N 1660 cm-1 usually strong C?N > 2200 cm-1 For comparison, C?C

Bonding General concepts

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Bonding ? General Concepts Electronegativity: The ability of anatom in a molecule to attract shared electrons to itself. Ionic Bonds Electrons are transferred Electronegativity differences are generally greater than 1.7 The formation of ionic bonds is always exothermic! Determination of Ionic Character Compounds are ionic if they conduct electricity in their molten state Electronegativity difference is not the final determination of ionic character Coulomb?s Law ?The energy of interaction between a pair of ions is proportional to the product of their charges, divided by the distance between their centers? There will be a negative sign on the Energy once calculated?it indicates an attractive force so that the ion pair has lower energy than the separated ions.

Robbert Goddard

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The Unit 7 Test Review The test will consist of 25 multiple choice questions. Scantron answer documents will be used. You will need a #2 pencil and a calculator. A periodic table will be provided. In order to be successful with this test you need to know your diatomics and polyatomic ions. Be sure you can write formulas and balance ionic charges. Please study your notes, quizzes, and practice worksheets. Be sure to complete the WebAssign. Name a hydrate Write the formula for a hydrate Calculate the percent by mass of water in a hydrate using a given formula Calculate the percent by mass of water in a hydrate using lab data Determine the formula of a hydrate using lab data (similar to the hydrate lab) Differentiate between basic state of matter symbols: (s), (l), (g), (aq)

Chapter 2: Chemical Units and Their Identities

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ATOMS: - made of nucleus (protons (positive charge) and neutrons (neutral charge)) and electron cloud (electrons (negative charge) - smallest particle that still retains properties of element - atomic # - # of protons (unique to each element) (also # of electrons in neutral atoms) - mass # - # of protons + neutrons - atomic mass - actual (average) mass of atom (measured in daltons) - about mass # b/c electrons have very small mass compared to protons/neutrons - isotope - atom w/ more/less than usual # of neutrons ELECTRONS: - elemental form of element is when element is by itself - compound - joint of 2+ elements w/ own set of properties diff. from elements - elements in periodic table are arranged in atomic # and are in 18 columns (groups)

Biology Chemical Bonds PPT

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Biol 210 General Biology 1 Lecture 2 Review Chemical Bonds Atomic Structure Nucleus Protons, mass = 1, charge = +1 Neutrons, mass = 1, charge = 0 Electrons Mass = negligible Charge = -1 # e? = # protons Outer shell (most energenic) e??s form chemical bonds Isotopes Some isotopes are stable, such as 1H2 Other isotopes are unstable, such as 1H3. When tritium decays, it gives off ? particle. Because the mass of an element includes the average isotope abundance, the mass and the atomic weight differ slightly Helium, He, atomic number 4, mass 4.003 Important Elements C HOPKINS CaFe Mg C = carbon H = hydrogen O = oxygen P = phosphorous K = potassium I = iodine N = nitrogen S = sulfur Ca = calcium Fe = iron Mg = magnesium Na = sodium Cl = chloride

Chapter 2

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AP Biology Reading Guide Chapter 2: The Chemical Context of Life Fred and Theresa Holtzclaw Copyright ? 2010 Pearson Education, Inc. - 1 - Name_______________________Period___________ Chapter 2: The Chemical Context of Life This chapter covers the basics that you may have learned in your chemistry class. Whether your teacher goes over this chapter, or assigns it for you do review on your own, the questions that follow should help you focus on the most important points. Concept 2.1 Matter consists of chemical elements in pure form and in combinations called compounds 1. Define and give an example of the following terms: matter element compound 2. What four elements make up 96% of all living matter?

Ionic/Covalent Bonds

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Ionic bond is between a metal and non-metal and has the electronegativity difference of 1.7 or higher. Also Ionic bonds take electrons from other elements. Convalent is usually between a non-metal and non-metal and shares electrons.
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