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Ionic bond

Chapter 9

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Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 15 Nov. 2012 Jespersen, Brady, Hyslop Chapter 9 Chemical Bonding: General Concepts Ionic Bonds Ch. 9.2 Ionic bonds are the attraction between positive and negative ions in an ionic compound. e.g. NaCl An electron is transferred from the metal (Na) to the nonmetal (Cl): Ionic compounds form when metals and nonmetals react and they are held together by ionic bonds. Compounds (ionic and molecular) are formed due to a decrease (lowering) of the potential energy of system. Net energy change associated with the electron transfer reaction. So, why does NaCl (s) form at all? 2 Lattice Energy of Ionic Compounds Ch. 9.2 The energy needed to produce separated gaseous ions from one mole of the solid is the lattice energy:

Campbell Biology Chapter 2 Study Guide

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Chemical bonding

Valence electron

Chemical reaction

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 to 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 Define and give an example of the following terms: matter: element: compound: What four elements make up 96% of all living matter? What is the difference between an essential element and a trace element? essential element: trace element: Concept 2.2 An element?s properties depend on the structure of its atoms

Bob Jones PPT Notes -- Chapter 7b

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Chemical bonding

Chemical polarity

Electronegativity

molecular geometry

Molecular Geometry 1 Valence Shell Electron Pair Repulsion (VSEPR) Theory Electron concentrations are arranged so as to be at maximum distance. Why? Electrons repel each other. Number of Electron Concentrations H H H H C ? ? ? ? Ex: CH4 O F F C ? ? ? ? Ex: CF2O Number of Electron Concentrations all 4 bonded = tetrahedral Ex: CH4 H H H H C ? ? ? ? 4 Regions of e? Conc. 5 Chemistry textbook, p. 169 3 bonded = pyramidal Ex: NH3 H H H N ? ? ? 4 Regions of e? Conc. 6 Chemistry textbook, p. 167 2 bonded = bent 104.5? Ex: H2O H H O ? ? 4 Regions of e? Conc. 7 Chemistry textbook, p. 170 1 bonded = linear Ex: HF H F ? 4 Regions of e? Conc. 8 Chemistry textbook, p. 170 All 3 bonded = trigonal planar 2 bonded = bent 120? Ex: BI3 Ex: GeF2 1 bonded = linear Ex: SO 3 Regions of e? Conc.

Bob Jones PPT Notes -- Chapter 6c

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Chemical bonding

Network covalent bonding

Properties of water

Properties of Compounds 1 Covalent distinct molecules held together by intermolecular forces relatively weak attractions, therefore low melting points not dense or hard poor heat and electricity conductors 2 Network Covalent exceptions continuous 3-D pattern?crystal Examples: diamonds, silicates 3 Network Covalent hard and brittle high melting points glassy luster 4 Ionic strong bonds, therefore high melting and boiling points hard solids can be split water-soluble good e? conductor in H2O, not as a solid 5 Ionic substances have low melting points. Ionic substances have low boiling points. Ionic substances don?t dissolve in water. Ionic substances are brittle. Question Because ionic bonds are strong, 6 Metallic carry electrons have luster (shine) malleable ductile 7 8

Bob Jones PPT Notes -- Chapter 6b

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Chemical bonding

Lewis structure

Valence electron

Delocalized electron

Section 6B Types of Bonds 1 Covalent Bonds usually nonmetals little or no ?EN (Therefore, atoms share electrons.) The 2 shared electrons are called a bonding pair. located between atoms most of the time Covalent Bonds The negative region between the atoms attracts the nuclei with an electrostatic force. Diatomic Elements H2 N2 O2 F2 Cl2 Br2 I2 ? triple bond ? double bond H N O Halogens Lewis Structures sometimes called dot diagrams show the valence e? only use a dash to represent a bonding pair Lewis Structures Cl2 + Cl Cl Cl Cl + Cl Cl Cl Cl Lewis Structures H2 + H H H H + H H H H Lewis Structures H2O + H O H + H O H + H O H + H O H Lewis Structures O2 O + O O O O + O O O Lewis Structures N2 N + N N N N + N N N Lewis Structures C2H2 + C C H + H + C C H H + C C H + H + C C H H

Bob Jones PPT Notes -- Chapter 6a

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Chemical bonding

Chemical polarity

Basics of Bonding 1 The second law of thermodynamics tells us that things tend to lose energy. Balls roll downhill. Electrons return to ground state. Atoms link or bond to each other. 2 Atoms bond because they Lose energy Gain stability 3 Energy/stability Unbonded Bonded 4 BJU Press Chemistry textbook p. 140 Noble gases (8 outer e?) are the most stable elements. Elements gain, lose, or share electrons to attain the ?noble-gas electron configuration.? This is called the octet rule. 5 Ionic: Metals/nonmetals Covalent: Nonmetals/nonmetals Metallic: Metals/metals Types of Bonds A property affecting ionic and covalent bonds The tendency of objects to have regions of opposite charge Polarity Examples: N and S poles (+) and (?) ends of a battery polar bond

Chapter 8

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Chemical bonding

Valence electron

Lewis structure

Claire Rafson Chapter 8 Notes 8.1- Bond Energy- The strength of a bonding interaction. The energy required to break the bond. Why do bonds occur? So the system can achieve the lowest possible energy by behaving in this way. Ionic bonding- electrostatic attractions of the closely packed, oppositiyly charged ions. Ionic compound- Metal reacts with a nonmetal Coulombs law- interaction between pair of ions. E= (2.31X 10^-19 J* nm) (Q1Q2/r) A bond will form if the energy of the aggregate is lower than that of the separated atoms. Covalent bonds- type of bonding in which electrons are shared by nuclei. (i.e Hydrogen bonding) Polar Covalent Bond- Atoms are different enough that they have unequal sharing results. 8.2-

The Chemistry Of Life

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Chemical bonding

Quantum chemistry

Chemical properties

Theoretical chemistry

Orbital hybridisation

Valence electron

#AP Bio #CampbellBiology

Chapter 2 The Chemical Context of Life Elements and Compounds 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 Sodium Chlorine Sodium chloride Essential Elements of Life Carbon, hydrogen, oxygen, and nitrogen make up 96% of living matter Trace elements are those required by an organism in minute quantities LE 2-3 Nitrogen deficiency Iodine deficiency LE 2-4 Nucleus Electrons Cloud of negative charge (2 electrons) Atomic Number and Atomic Mass Atoms of the various elements differ in number of subatomic particles Atomic number Mass number Atomic mass Isotopes Atoms of an element have the same number of protons but may differ in number of neutrons

Chemistry

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Chemical bonding

Valence electron

Lewis structure

Chemical reaction

Social issues in forbidden city Corrupted government Ignorant Deals issues in violent ways Their views on democracy which the students want Indifference Their views are based on Maoism (the PLA retaliated by using violence) Cultural Aspects Appearance Patriotic government very rightist (conservative) Traditional and hardworking society Food Housing Manners idk (the part where alex learns that it is expected to put a lot of food on the table but not eat it because it means that you?ve ate too much and you can?t eat anymore) Plot Talk about the student demonstration May 4th include hunger strike and martial law Death of Hu Yao Bang Li Peng PLA and talk about one part of like war ( teargas cannisters , AK47, Xin Hua Shot, Lao Xu Dead

chemical bonding review

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Chemical bonding

Chemical polarity

Lewis structure

Name: ________________________ Class: ___________________ Date: __________ ID: A 1 CH 6 Review Multiple Choice Identify the choice that best completes the statement or answers the question. ____ 1. The electrostatic attraction between positively charged nuclei and negatively charged electrons permits two atoms to be held together by a(n) a. chemical bond. c. neutron. b. London force. d. ion. ____ 2. As atoms bond with each other, they a. increase their potential energy, thus creating less-stable arrangements of matter. b. decrease their potential energy, thus creating less-stable arrangements of matter. c. increase their potential energy, thus creating more-stable arrangements of matter. d. decrease their potential energy, thus creating more-stable arrangements of matter.

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