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Covalent bond

Holt Biology Chapter 2 Section 1

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Unit 1 Chapter 2: Chemistry of Life Section 1: Nature of Matter Atom Smallest unit of matter that can?t be broken down by chemical means Protons, Neutrons, Electrons Electron cloud Region around nucleus that electrons can occupy at any time Stable atoms usually have no charge 1 electron for every 1 proton Elements Pure substance made of one kind of atom Differ in number of protons Ex. Carbon-12 (Carbon has 6 protons) 12-6=6 Carbon-12 has 6 neutrons Compound Substance made of joined atoms of 2 or more different elements Chemical formula identifies what is in compound and those elements? proportions Ex. NaCl 1 Sodium for every 1 Chlorine Covalent Bonds Two or more atoms share electrons to form a molecule Molecule Group of atoms held together by covalent bonds

Bob Jones PPT Notes -- Chapter 7b

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Chemistry
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Covalent bond
VSEPR theory
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Hydrogen bond
Electronegativity
molecular geometry
Ionic bond
Sigma bond
Technology

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 7a

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Molecular orbital
Valence bond theory
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Antibonding
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Sigma bond
Delta bond
Resonance
Covalent bond
Lewis structure

Bond Theories 1 Lewis Structures Tell us about bonds in a molecule Do not tell us about the shape of the molecule Valence Bond Theory Based on the quantum model Says that covalent bonds form when orbitals of different atoms overlap sigma (?) ? the ends of the orbitals overlap pi (?) ? the sides of the orbitals overlap Types When Orbitals Overlap Bonds: sigma bond Single Bond s sublevel 5 Chemistry textbook, p. 162 sigma bond Single Bond p sublevel 6 Chemistry textbook, p. 162 Which type of bond forms first between covalently bonded atoms? Sigma Pi Depends on the atom Question 7 sigma and pi bond Double Bond 8 Chemistry textbook, p. 162 sigma and 2 pi bonds Triple Bond 9 Chemistry textbook, p. 162 pi bond forms only after a sigma bond weaker than a sigma bond double bond

Bob Jones PPT Notes -- Chapter 6c

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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 bond
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Lewis structure
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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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Fluorine
Sigma bond
Technology

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

Campbell Biology Test Bank Chapter 2

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electron
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Covalent bond
Chemical polarity
Proton
Technology

Campbell's Biology, 9e (Reece et al.) Chapter 2 The Chemical Context of Life This chapter presents basic chemical principles for understanding the chemical context of living organisms, from atomic structure to the nature of chemical bonds and an introduction to chemical equilibrium. These questions focus on elements most important to life or the study of life, including the elements that comprise organic molecules and important trace elements. Some isotopes are important in geologic dating and in biological tracer studies. How elements participate in forming different types of chemical bonds is essential to mastering subsequent topics on the behavior and properties of biological molecules, structures, and energy metabolism. Multiple-Choice Questions

Chapter 8

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electron
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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-

Cambell Biology 7th edition Chemistry notes

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The Chemical Basis of Life ?We are stardust? nasa.gov Students should be able to: Define: element, atom and molecule Name the components of atoms and their physical arrangements. Draw a diagram of an atom, given the atomic number. Distinguish between the types of chemical bonds. Element: a substance that cannot be broken down to other substancesPeriodic Table: organizational chart of all the elements http://www.periodictable.com/ Table 2.1 5 Table 2.1 Elements In the Human Body ATOM: from Greek atomos, ?unable to be cut? Atomic Structure An atom is the smallest unit of matter that still retains the properties of an element. Three subatomic particles in atoms are relevant to our discussion of the properties of elements. Protons are positively charged.

The Chemistry Of Life

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#AP Biology #AP Bio #Biology

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

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