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Chemical bond

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.

Biology

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AP BIOLOGY VOCABULARY BioChemistry anion atomic mass atomic number cation chemical equilibrium covalent bond electronegativity hydrogen bond ionic bond isotope mass number orbital trace element valence valence electron van der Waals interaction acid adhesion aqueous solution base buffer cohesion heat heat of vaporization hydration shell hydrophilic hydrophobic molarity mole molecular mass pH solution specific heat surface tension temperature alcohol amino group carbonyl group carboxyl group enantiomer functional group hydroxyl group isomer organic chemistry phosphate group sulfhydryl group helix pleated sheet amino acid antiparallel carbohydrate cellulose chaperonin chitin cholesterol condensation reaction conformation denaturation deoxyribose fatty acid gene glycogen hydrolysis

Chapter 3 Notes

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Joey Miller AP Biology Chapter 3: Water and Life The Molecule that Supports Life Water is the biological medium here on Earth. Water is the only common substance to exist in the natural environment in all three physical states of matter. The solid state of water floats on the liquid, a rare property emerging from the chemistry of the water molecule. Polar Covalent Bonds in Water Molecules Result in Hydrogen Bonding Polar Covalent Bonds ? the electrons of the covalent bonds spend more time closer to one atom than another atom Polar Molecule ? The overall charge of a molecule is unevenly distributed

Biology Chemical Bonds PPT

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Chemical Bonds

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?

What is a molecule?

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Molecule Main article: Molecule A molecule is the smallest indivisible portion of a pure chemical substance that has its unique set of chemical properties, that is, its potential to undergo a certain set of chemical reactions with other substances. Molecules can exist as electrically neutral units unlike ions. Molecules are typically a set of atoms bound together by covalent bonds, such that the structure is electrically neutral and all valence electrons are paired with other electrons either in bonds or in lone pairs.

Notes

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Name: _________________________________ What You Need To Know for the Chemistry Regents Exam The Test The Chemisty Regents Exam is broken down into three sections: Part A: 35 mulitple choice questions from all units covered over the course of the school year. Part B: Approximately 25 questions, with a mix of short answer and multiple choice. Questions focus on the Reference Tables, graphing, and laboratory experiments. Part C: Approximately 15 short answer questions, most broken down into smaller parts. This is often an eclectic, unpredictable mix of questions from various units, and may demand students write short paragraphs, use equations and reference tables, or draw graphs and diagrams in order to correctly answer the questions.

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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Inter/IntraMolecular Forces

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3 Types of bonds: [IONIC, COVALENT, METALLIC] ---> Intramolecular forces INTERmolecular Forces: Force of attraction between molecules Ionic > [Hydrogen Bonding > Dipole-Dipole > LDF] <---Covalent A. Dipole-Dipole 1. Definition - Positive (Polarity) seeks negative 2. Happens between POLAR molecules EX: HCl attracts HCl H-Cl --><-- H-Cl B. Hydrogen Bonding 1. Definition - Attraction between Hydrogen atoms and unshared electrons of Hydrogen (H), Oxygen (O), or Florine (F). 2. STRONG attraction <---IMPORTANT 3. Holds DNA strands together EX: H2O attracts H2O (Dipole-Dipole is there too) HAVE POLARITY C. London Dispersion Forces (LDF)

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