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Chemical bond

Basic Chemistry Review (PreAP level)

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Chemistry
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Chemical bonding
Quantum chemistry
Chemical properties
Periodic Table
Atomic physics
Chemical bond
ion
Chemistry
Valence electron
Atom
Periodic trends
electron

1 THE MOST BASIC CHEMISTRY REVIEW This review is intended to remind you of the BASICS that you learned. It is NOT COMPLETE. CLASSIFYING MATTER elements, compounds, or mixtures PROPERTIES OF MATTER INTensive?a property that doesn?t depend on amount (ex- boiling point) Extensive?a property that does depend on amount (ex- mass or volume) density ? amount of matter in a given volume Density = mass volume units: g/cm3 for solids, g/mL for liquids density column Example A piece of wood that measures 3.0 cm by 6.0 cm by 4.0 cm has a mass of 80.0 grams. What is the density of the wood? Would the piece of wood float in water? If the wood were cut into three pieces would it have the same density?

AP Chemistry Zumdahl 7E Chapter 10 Notes

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Chemistry
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Chemical bonding
Gases
Materials science
intermolecular forces
Chemical properties
Properties of water
Chemical bond
Molecular solid
Hydrogen bond
Vapor pressure
Enthalpy of vaporization
Boiling point

1 Chapter 10 - Liquids and Solids 10.1 Intermolecular Forces A. Dipole-Dipole Forces 1. Attraction between molecules with dipole moments a. Maximizes (+) ----- ( - ) interactions b. Minimizes (+) ----- ( + ) and (-) ----- ( - ) interactions 2. About 1% of strength of ionic bonds a. Unimportant in gas phase due to distance between molecules B. Hydrogen Bonding 1. Special dipole-dipole attraction a. Hydrogen covalently bonded to highly electronegative elements (N, O, F) has a higher than normal d+ charge 2. Bond strength is higher than other dipole-dipole attractions 3. Important in the bonding of molecules such as water and DNA C. London Dispersion Forces 1. Instantaneous dipoles a. Random movement of electrons can create a momentary

AP Chemistry Zumdahl 7E Chapter 9 Notes

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Chemistry
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Chemical bonding
Orbital hybridisation
Molecular orbital
Covalent bond
Antibonding molecular orbital
Pi bond
Delocalized electron
Atomic orbital
Chemical bond
Double bond
Sigma bond
Unpaired electron

1 Chapter 9 - Covalent Bonding: Orbitals 9.1 Hybridization and the Localized Electron Model A. Hybridization 1. The mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies B. Hybrid Orbitals 1. Orbitals of equal energy produced by the combination of two or more orbitals on the same atom C. Evidence for hybridization of carbon - Methane and sp3 1. Four bonds of equal length and strength Carbon's isolated configuration Carbon's hybridized configuration 2. Four effective pairs of electrons surround the carbon 3. "Whenever a set of equivalent tetrahedral atomic orbitals is required by an atom, this model assumes that the atom adopts a set of sp3 orbitals; the atom becomes hybridized"

AP Chemistry Zumdahl 7E Chapter 8 Notes

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Chemistry
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Chemical bonding
Chemical bond
Octet rule
Lewis structure
Ionic bonding
Covalent bond
Resonance
Chemistry
Valence electron
Valence
Formal charge
VSEPR theory

AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy (greater stability) than separated ions B. Coulomb's Law 1. ? ? ? ? ? ? ? ? ?= - r QQ E nmJx 21191031.2 a. E = energy in joules b. Q1 and Q2 are numerical ion charges c. r = distance between ion center in nanometers d. negative sign indicates an attractive force C. Bond Length (covalent) 1. Distance at which the system energy is at a minimum 2. Forces at work a. Attractive forces (proton - electron) b. Repulsive forces (electron - electron, proton - proton) 3. Energy is given off (bond energy) when two atoms achieve greater stability together than apart

AP Chemistry Zumdahl 7E Chapter 2 Notes

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Chemistry
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ions
Chemistry
Charge carriers
atoms
Chemical properties
Chemical bond
Proton
Alkali metal
electron
Polyatomic ion
molecule
Oxidation state

AP Chemistry A. Allan Chapter 2 Notes - Atoms, Molecules and Ions 2.1 The Early History Refer to the Chemistry History Timeline for this chapter 2.2 Fundamental Chemical Laws A. Law of Conservation of Mass 1. "Mass is neither created nor destroyed" 2. Translation: In ordinary chemical reactions, the total mass of the reactants is equal to the total mass of the products B. Law of Definite Proportion 1. "A given compound always contains the same proportions of elements by mass" 2. Translation: Compounds have an unchanging chemical formula C. Law of Multiple Proportions 1. "When two elements form a series of compounds, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to small whole numbers

Raven Biology Chapter 2 Notes

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Biology
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Chemical bonding
Chemical bond
Hydrogen bond
Covalent bond
Chemistry
Properties of water
Chemical polarity
Chemical reaction
molecule
Ionic bonding
Energy level
Hydrogen

Gavin Morgan 8/31/2015 Chapter 2 2-Point Notes The Nature of Atoms Atomic structure includes a central nucleus and orbiting electrons: 1. Danish physicist Niels Bohr created the model of the atom in 1913, which is still used today. 2. An atom?s mass is measured in daltons (6.02 x 1023 daltons = 1 g). A proton and neutron each way 1 dalton. Electrons determine the chemical behavior of atoms: 1. The position of an electron cannot be determined at any given time. 2. Orbitals are predictions where electrons are most likely to be found. Atoms contain discrete energy levels: 1. Electrons contain discrete energy levels which correspond to quanta.

Campbell9thEdChapter2ChemicalContextofLife

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Biology
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Chemical bonding
Chemical bond
Covalent bond
Valence electron
Valence
Ionic bonding
Chemistry
Lewis structure
Electronegativity
Atomic orbital
Hydrogen bond
ion

The Chemical Context of Life Chapter 2 Matter consists of chemical elements in pure form and in combinations called compounds Organisms are composed of matter Matter is anything that takes up space and has mass ? 2011 Pearson Education, Inc. Elements and Compounds Matter is made up of elements An element is a substance that cannot be broken down to other substances by chemical reactions A compound is a substance consisting of two or more elements in a fixed ratio A compound has characteristics different from those of its elements ? 2011 Pearson Education, Inc. Figure 2.3 Sodium Chlorine Sodium chloride The Elements of Life About 20?25% of the 92 elements are essential to life, but it varies among organisms Humans need 25 elements while plants only need 17 elements

AP Bio Chp 4

Subject: 
Biology
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organic chemistry
Isomerism
Functional Groups
Isomer
Carbon
molecule
Chemical bond
Carbohydrate
Hydroxyl

AP Biology Reading Guide Chapter 4: Carbon and the Molecular Diversity of Life Fred and Theresa Holtzclaw Copyright ? 2010 Pearson Education, Inc. - 1 - Name_______________________Period___________ Chapter 4: Carbon and the Molecular Diversity of Life Concept 4.1 Organic chemistry is the study of carbon compounds 1. Study this figure of Stanley Miller?s experiment to simulate conditions thought to have existed on the early Earth. Explain the elements of this experiment, using arrows to indicate what occurs in various parts of the apparatus. 2. What was collected in the sample for chemical analysis? What was concluded from the results of this experiment?

AP Bio Chp 2 2

Subject: 
Biology
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Chemical bonding
Chemistry
Quantum chemistry
Chemical properties
Chemical bond
molecule
Covalent bond
Hydrogen bond
Valence electron
electron
Chemical reaction
Valence

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?

Ap Bio Chp 2

Subject: 
Biology
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Chemical bonding
Chemistry
Quantum chemistry
Chemical properties
Chemical bond
molecule
Covalent bond
Hydrogen bond
Valence electron
electron
Chemical reaction
Valence

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?

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