Media Portfolio

Chapter 1
Electronic Structure and Bonding

01-00-01CO

Title	Ethane, Ethene, and Ethyne
Caption
Notes
Keywords	ethane, ethene, ethyne

01-00-03UN

Title	Second Row of Periodic Table
Caption	The second row of the periodic table.
Notes	Atoms to the left of carbon have a tendency to give up electrons, whereas atoms to the right of carbon have a tendency to accept electrons.
Keywords	second, row, periodic, table, carbon, position

01-00-06T02UN

Title	Table 1.2 The Ground State Electronic Configuration of the Smallest Atoms
Caption	The ground-state electronic configurations of the lightest atoms.
Notes	The ground-state electronic configuration of an atom is a description of the orbitals occupied by an atom's electrons when they are all in the lowest available energy orbitals.
Keywords	ground-state, electronic, configuration, energy, orbitals

01-01

Title	Structures of Sodium Chloride
Caption	Sodium chloride crystals and ions.
Notes	Sodium chloride forms crystals with a distinct shape visible to the naked eye. At the submicroscopic level, sodium chloride is composed of negatively charged chloride ions and positively charged sodium ions in a regular alternating three-dimensional array.
Keywords	crystals, ions, sodium, chloride

01-01-06T03UN

Title	Table 1.3 The Electronegativities of Selected Elementsa
Caption	Electronegativity is the tendency of an atom to attract bonding electrons toward itself.
Notes	Electronegativity increases as you move across a row to the right and increases as you go up any of the columns of the periodic table.
Keywords	Pauling, electronegativity, trend, periodic

01-01-10UN

Title	Electrostatic Potential Maps
Caption	Electrostatic potential maps for LiH, H2, and HF.
Notes	Red regions have high electron density, and are attractive to cations and positively charged regions of molecules. Blue regions are electron deficient, and are attractive to anions and negatively charged regions of molecules. Yellow and green regions have mid-range electron densities, and are relatively uncharged.
Keywords	electrostatic, potential, maps, electron, density, charge, distribution

01-01-11UN

Title	Electrostatic Potential Maps
Caption	Electrostatic potential maps for LiH, H2, and HF.
Notes	Red regions have high electron density, and are attractive to cations and positively charged regions of molecules. Blue regions are electron deficient, and are attractive to anions and negatively charged regions of molecules. Yellow and green regions have mid-range electron densities, and are relatively uncharged.
Keywords	electrostatic, potential, maps, electron, density, charge, distribution

01-01-16.1UN

Title	Lewis Structures
Caption	Lewis structures of H2O, H3O+, HO–, and H2O2 showing lone-pair electrons.
Notes	Lewis structures show how atoms are bonded to one another, and depict formal charges and lone-pair electrons on atoms.
Keywords	lone-pair, Lewis, structures, formal, charges, water, hydronium, hydroxide, hydrogen, peroxide

01-01-171

Title	Electrostatic Potential Maps
Caption	Electrostatic potential maps for the hydronium ion, water, and the hydroxide anion.
Notes	The electrostatic potential maps show an increase in electron density (red color) on the oxygen atoms going from the hydronium ion (an acid) to the hydroxide anion (a base).
Keywords	electrostatic, potential, maps, electron, density, hydronium, water, hydroxide

01-01-36UN

Title	1s and 2s Atomic Orbitals
Caption	An orbital is a three-dimensional region around the nucleus where there is a high probability of finding an electron.
Notes	An electron in a 1s orbital can be anywhere within the 1s sphere, but a 2s atomic orbital is more complex. There is a part of the orbital, known as a node, where the probability of finding an electron falls to zero.
Keywords	orbitals,1s, 2s, node, electron

01-01-37UN

Title	Nodes
Caption	A node is a region where a standing wave has an amplitude of zero; the string rests motionless at the nodes with no transverse displacement.
Notes	Nodes are regions where wave activity (motion of a guitar string or probability of finding an electron) falls to zero.
Keywords	node, amplitude, zero, wave, activity, guitar, string, electron, probability

01-01-38UN

Title	Nodal Planes for p Orbitals
Caption	p Atomic orbitals have two lobes and are dumbbell-shaped. The two lobes are of opposite phase.
Notes	A nodal plane passes through the center of the nucleus, bisecting the two lobes of the p orbital. Because the standing wave has zero amplitude at the node, there is zero probability of finding an electron in the nodal plane of the p orbital.
Keywords	nodal, plane, p, orbital, lobes, probability, electron

01-01-39UN

Title	Degenerate 2p Atomic Orbitals
Caption	Three degenerate 2p atomic orbitals.
Notes	The px orbital is symmetrical about the x-axis, the py orbital is symmetrical about the y-axis, and the pz orbital is symmetrical about the z-axis.
Keywords	p orbitals, degenerate, px, py, pz

01-01-40UN

Title	Sigma Bonds
Caption	Sigma bonds form when two s orbitals overlap.
Notes	The electrons in a sigma bond are symmetrically distributed about the internuclear axis (an imaginary line between the two nuclei).
Keywords	sigma, bond, overlap, internuclear, axis, s, orbitals

01-02

Title	Bond Length for Hydrogen Atoms
Caption	The change in potential energy that occurs as two 1s atomic orbitals approach each other.
Notes	There is a net release of energy when a covalent bond forms. The internuclear distance at minimum energy is the length of the hydrogen–hydrogen covalent bond.
Keywords	covalent, bond, length, orbitals, hydrogen-hydrogen, minimum, potential, energy, 1s

01-03

Title	Combining Atomic Wave Functions
Caption	The wave functions of two hydrogen atoms can interact to reinforce each other (top) or cancel each other (bottom).
Notes	Bonding results when two orbitals with the same phase interact. When two out-of-phase atomic orbitals overlap, they cancel each other and produce a node between the nuclei.
Keywords	wave, in-phase, out-of-phase, node, atomic, orbitals, bonding, hydrogen

01-04

Title	Hydrogen MO Diagram
Caption	Atomic and molecular orbitals of H and H2.
Notes	Before covalent bond formation, each electron is in an atomic orbital. After covalent bond formation, both electrons are in the bonding molecular orbital. The antibonding molecular orbital is empty.
Keywords	bonding, antibonding, hydrogen, atomic, orbital, electrons, MO, diagram, bonding, molecular

01-05

Title	p Orbital Bonding (end-to-end)
Caption	End-on overlap of two p orbitals to form a sigma bonding molecular orbital and a sigma antibonding molecular orbital.
Notes	If the overlapping lobes of the p orbitals are in phase, a constructive bonding molecular orbital forms. If the lobes are out of phase, a destructive antibonding molecular orbital forms.
Keywords	overlap, bonding, antibonding, end-to-end, end-on, sigma, orbital

01-06

Title	p Orbital Bonding (side-to-side)
Caption	Side-to-side overlap of two parallel p orbitals to form a pi bonding molecular orbital and a pi antibonding molecular orbital.
Notes	A bond formed as a result of side-to-side overlap of p atomic orbitals is called a pi bond. Side-to-side overlap of two in-phase p atomic orbitals forms a pi bonding molecular orbital, while side-to-side overlap of out-of-phase p orbitals forms a pi antibonding molecular orbital.
Keywords	pi, bond,overlap,in-phase,out-of-phase,side-to-side, p, atomic, orbitals, bonding, antibonding

01-07

Title	MO Diagram for MOs Made from p Atomic Orbitals
Caption	MO diagram showing relative energies of all types of molecular orbitals which can be made from p atomic orbitals.
Notes	p Atomic orbitals can overlap end-on to form sigma bonding and antibonding molecular orbitals. The bonding combination has less energy than the antibonding combination. p Atomic orbitals can also overlap side-to-side to form pi bonding and antibonding molecular orbitals. The pi molecular orbitals have energies greater than those of sigma bonding orbitals and less than those of sigma antibonding orbitals.
Keywords	p, atomic, orbitals, overlap, end-on, sigma, bonding, antibonding, pi, side-to-side, energies

01-08

Title	CO Pi Bond Formation
Caption	MO diagram for C–O pi molecular orbital formation.
Notes	Side-to-side overlap of a p atomic orbital from carbon with a p atomic orbital from oxygen results in pi bonding and pi antibonding molecular orbitals. The bonding combination has greater electron density on oxygen (electronegativity), whereas the antibonding combination has smaller electron density on the more electronegative atom.
Keywords	side-to-side, overlap, carbon-oxygen, bonding, antibonding, electronegativity, electronegative

01-08-01UN

Title	Problem 14
Caption	Indicate the kind of molecular orbital (s, s, p, or p) that results when the orbitals are combined as indicated.
Notes	End-on combinations yield sigma atomic orbitals and side-to-side combinations yield pi molecular orbitals. Combining orbitals by overlapping like phases yields bonding combinations, whereas combining orbitals by overlapping opposite phases yields antibonding combinations.
Keywords	problem, 14, s, s, p, p

01-08-02

Title	Models of Methane
Caption	Four different ways to represent a methane molecule.
Notes	Molecules can be represented by giving structural formulas, showing ball-and-stick models, showing space-filling models, or by showing electrostatic potential maps.
Keywords	molecules, structural, formulas, ball-and-stick, models, space-filling, electrostatic, potential, maps, methane, represent

01-09

Title	Energy Promotion Potential Diagram
Caption	Energy diagram showing the results of 2sÑ2p electron promotion followed by formation of four covalent bonds.
Notes	By promoting a 2s electron out of the filled 2s orbital, carbon can use both 2s electrons and both 2p electrons to form a total of four bonds. This results in lower-energy molecules, and an octet of bonding electrons in carbon's valence shell.
Keywords	promotion, promoting, electron, lower-energy, octet

01-10

Title	Formation of sp3 Hybrid Orbital
Caption	Combination of 25% of the character of an s orbital with 75% of the character of a p orbital yields an sp3 hybrid orbital.
Notes	The positive lobe of the p orbital combines constructively with the s orbital, whereas the negative lobe of the p orbital combines destructively with the s orbital, yielding a hybrid orbital with a large positive lobe and a small negative lobe.
Keywords	positive, lobe, negative, constructively, destructively, combination, hybrid, s, p, orbital

01-11

Title	Formation of Four sp3 Hybrid Orbitals
Caption	One s atomic orbital combines with three p atomic orbitals to make four sp3 hybrid orbitals.
Notes	An sp3 hybrid atomic orbital is more stable than a p atomic orbital, but not as stable as an s atomic orbital.
Keywords	s, atomic, orbital, p, stable, orbitals

01-12

Title	Structure of Methane
Caption	Four sp3 orbitals are directed toward the corners of a tetrahedron.
Notes	The orbital structure of methane shows the overlap of the four sp3 orbitals of carbon with the s orbitals of four hydrogen atoms to form four sigma (covalent) bonds between carbon and hydrogen.
Keywords	methane, tetrahedral, tetrahedron, sp3, overlap

01-13

Title	Orbital Diagram for Ethane
Caption	Overlap of two sp3 hybrid orbitals on carbon atoms in ethane to form sigma bonding and antibonding orbitals.
Notes	The C–C bond in ethane is formed by overlap of two sp3 hybrid orbitals on bonded carbon atoms. Each C–H bond is formed by overlap of an sp3 hybrid orbital on carbon with the s atomic orbital on the attached hydrogen atom.
Keywords	C-C, bond, overlap, hybrid, orbital, bonded, C-H, ethane

01-13-02

Title	Structure of Ethane
Caption	The two carbons in ethane are tetrahedral. Each carbon uses four sp3 atomic orbitals to form four covalent bonds.
Notes	All of the bonds in methane and ethane are sigma bonds because they all are formed by end-on overlap of atomic orbitals.
Keywords	ethane, sp3, orbitals, covalent, bonds, sigma, end-on, overlap

01-14

Title	Bonding in Ethane
Caption	The carbon–carbon bond is formed by sp3Ñsp3 overlap, and each carbon–hydrogen bond is formed by sp3Ñs overlap.
Notes	One sp3 orbital of one carbon overlaps an sp3 orbital of the other carbon to form the carbon–carbon bond. The remaining three sp3 orbitals of each carbon overlap an s orbital of hydrogen to form carbon–hydrogen bonds.
Keywords	ethane, sp3, orbitals,overlap,carbon-carbon, carbon-hydrogen

01-15

Title	sp2 Hybrid Orbitals
Caption	Carbon bearing three sp2 hybrid orbitals and an unhybridized p orbital shown from two different viewpoints.
Notes	An sp2 hybrid orbital is made from 1/3 of an s orbital and 2/3 of a p orbital. The angle between the sp2 orbitals is 120 degrees, and the unhybridized p orbital is oriented perpendicular to the plane containing the three sp2 orbitals. Carbon starts with four orbitals in its valence shell. After hybridization it must still have a total of four orbitals.
Keywords	orbitals, sp2, unhybridized, valence, shell, 1/3, 2/3, 120, degrees

01-16

Title	Structure of a Double Bond
Caption	One bond in a double bond is a sigma bond, and the other is a pi bond. The carbon–hydrogen bonds are all sigma bonds.
Notes	The carbon–carbon sigma bond in ethene is formed by sp2Ñsp2 overlap, and the carbon–carbon pi bond is formed by side-to-side overlap of a p orbital of one carbon with a p orbital of the other carbon.
Keywords	sigma, bond, pi, double, overlap, side-to-side, carbon-carbon, carbon-hydrogen

01-16-01UN

Title	Structure of Ethene
Caption	Ethene consists of a carbon–carbon double bond and four carbon–hydrogen single (sigma) bonds.
Notes	Both bonds in the double bond of ethene contribute to its strength. In a carbon–carbon double bond, four electrons hold the carbons together.
Keywords	ethene, structure, double, bond, four, electrons

01-17

Title	sp-Hybridized Carbon Atom
Caption	Shown is a carbon atom bearing two sp hybrid orbitals (orange) and two unhybridized p orbitals (purple).
Notes	The two sp hybrid orbitals are 180 degrees from one another. The two unhybridized p orbitals are oriented perpendicular to the two sp hybrid orbitals and also perpendicular to each other. In molecules with carbon–carbon triple bonds, the sp orbitals form the sigma bonds, and the p orbitals form the pi bonds.
Keywords	sp, orbitals, p orbital, carbon, triple, bond, 180, degrees

01-18

Title	Orbital Structure of Ethyne
Caption	Ethyne consists of a carbon–carbon triple bond and two carbon–hydrogen single bonds.
Notes	The first bond of a carbon–carbon triple bond is formed by the overlap of two sp hybrid orbitals on adjacent carbons in an end-on fashion. The second and third bonds in a carbon–carbon triple bond are formed by side-to-side overlap of unhybridized p orbitals on adjacent carbons. The carbon–hydrogen bonds are formed by the overlap of an sp hybrid on carbon with an s orbital on hydrogen.
Keywords	ethyne, triple, bond

01-18-01

Title	Models of Ethyne
Caption	Structural formula, orbital model, space-filling model, and potential map of ethyne.
Notes	The two carbon atoms in a triple bond are held together by six electrons. Each of the unhybridized p orbitals engages in side-to-side overlap with a parallel p orbital on the other carbon, with the result that two pi bonds are formed.
Keywords	ethyne, triple, bond, orbital, model, space-filling, potential, map

01-18-02UN

Title	The Methyl Cation
Caption	Orbital depiction, two ball-and-stick models, and potential map of the methyl cation.
Notes	A positively charged carbon atom forms its three covalent bonds using three sp2 orbitals. Its unhybridized p orbital remains empty. Because the three sp3 orbitals lie in a plane, a carbocation is flat.
Keywords	cation, positive, charge, methyl, empty, orbital

01-18-03UN

Title	The Methyl Radical
Caption	Orbital, ball-and-stick, and potential-map depictions of the methyl radical.
Notes	The carbon atom in the methyl radical is sp2 hybridized. The unpaired electron occupies the p orbital.
Keywords	methyl, radical, unpaired, electron

01-18-04UN

Title	The Methyl Anion
Caption	Depictions of the methyl anion.
Notes	The methyl anion has two paired electrons (a nonbonding pair) occupying the unhybridized p orbital. The carbon atom carries a negative charge.
Keywords	anion, nonbonding, electrons, negative, charge

01-18-06UN

Title	Models of Water
Caption	Orbital, ball-and-stick, and potential-map depictions of the water molecule.
Notes	The central oxygen atom in water initially forms four sp3 hybrid orbitals. Two of these hybrids combine with s orbitals on hydrogens to make O–H single bonds. The remaining two sp3 hybrids each contain a pair on nonbonding electrons. The O–H bonds form a 104.5-degree angle about the central oxygen atom.
Keywords	water, central, oxygen, 104.5, degree, O-H

01-18-08UN

Title	Ammonia
Caption	Structure of ammonia.
Notes	The nitrogen–hydrogen covalent bonds in ammonia form as a result of the overlap of three sp3 orbitals of nitrogen and the three s orbitals of the attached hydrogen atoms. The single nonbonding pair of electrons occupies an sp3 orbital on nitrogen. Two N–H bonds form a 107.3-degree angle about the central nitrogen.
Keywords	ammonia, nitrogen, 107.3, degree, angle

01-18-09UN

Title	The Ammonium Ion
Caption	Structure of the ammonium ion.
Notes	The ammonium ion has four identical nitrogen–hydrogen bonds and has no nonbonding pairs of electrons.
Keywords	ammonium, ion

01-18-10UN

Title	Problem 18
Caption	Compare the potential maps for methane, ammonia, and water. Which is the most polar molecule? Which is the least polar?
Notes	Polarity increases as charge increases, as indicated by buildup of red and blue colors on opposite sides of a potential map.
Keywords	polarity, problem, 18, potential, map, polar

01-18-11

Title	Hydrogen Fluoride
Caption	Models of hydrogen fluoride.
Notes	Fluorine builds four sp3 hybrid orbitals and uses three of them to hold nonbonding pairs of electrons and the fourth to make a sigma bond with hydrogen. Note that since fluorine is much more electronegative than hydrogen, the potential map shows a high degree of polarity.
Keywords	hydrogen, fluoride, fluorine, polarity

01-18-12UN

Title	Hydrogen Halides
Caption	Space-filling models of HF, HCl, HBr, and HI.
Notes	As the distance between the center of the hydrogen atom and the center of the halogen atom increases in this series of molecules, the bond between hydrogen and halogen weakens.
Keywords	hydrogen, halides, distance, bond, halogen

01-18-13UN

Title	Orbital Overlap In HF and HCl
Caption	Overlap of the bonding sp3 hybrid orbital of F and Cl with H in HF and HCl.
Notes	Overlap of the 1s orbital of hydrogen is better with the smaller 2sp3 hybrid orbital of fluorine than with the larger 3sp3 hybrid orbital of chlorine, resulting in a shorter, stronger bond in HF than in HCl.
Keywords	overlap, HF, HCl, 2sp3, 3sp3, hydrogen, chlorine

01-18-14UN

Title	Bond Lengths and Strengths
Caption	Hydrogen–halogen bond lengths and bond strengths.
Notes	Hydrogen halides are compounds containing a hydrogen bonded to a halogen. The bond is formed by an overlap of an sp3 hybrid orbital of the halogen with the s orbital of hydrogen. The hydrogen–halogen bond becomes weaker and longer as the atomic weight of the halogen increases.
Keywords	hydrogen, halide, halogen, bond, strength, length, atomic, weight, hydrogen-halogen

01-18-21UN

Title	Carbon Dioxide and Carbon Tetrachloride
Caption	Structures, dipole moments, and potential maps of carbon dioxide and carbon tetrachloride.
Notes	Although both molecules are composed of polar bonds (especially evident in the map of carbon dioxide), they are nonpolar overall because the dipole moments of the bonds cancel each other out.
Keywords	carbon, dioxide, tetrachloride, dipole, moment, polar, nonpolar

01-18-22UN

Title	Chloromethane, Water, and Ammonia
Caption	Structures and dipole moments of chloromethane, water, and ammonia.
Notes	Overall dipole moments of these molecules are greater than dipole moments of one of their bonds because bond dipole moments reinforce each other in these molecules.
Keywords	overall, dipole, moments, chloromethane, water, ammonia

01-18-26UN

Title	pH Values of Some Common Substances
Caption	The pH of a water-based substance indicates the concentration of hydrogen ions in the substance.
Notes	Acidity increases with lower pH values. Compounds with a pH of 7 are neutral. Basicity increases with higher pH values.
Keywords	pH,acidity,basicity,neutral

01-18-38UN

Title	Relative Electronegativities of Second-Row Elements
Caption	Second-row elements from the periodic table increase in electronegativity from left to right.
Notes	In the series C, N, O, and F, C is least electronegative and F is most electronegative.
Keywords	second-row, elements, electronegativity, periodic, table

01-18-39UN

Title	Base Stabilities
Caption	Relative stabilities of bases bearing one negative charge made from second-row elements and hydrogen.
Notes	Anionic bases become more stable (weaker) as the atom bearing the negative charge moves to the right along a row of the periodic table, because atoms on the right-hand side of the periodic table hold excess electrons (negative charge) more easily than atoms further to the left, due to relative electronegativities.
Keywords	anionic, bases, negative, charge, second-row, stability, electronegativity

01-18-40UN

Title	Relative Acid Strengths of Second-Row Binary Acids
Caption	Acids made only of hydrogen and one other element (binary acids) increase in strength as the "other" element moves to the right along a row of the periodic table.
Notes	The stronger an acid is, the weaker its conjugate base is, and vice versa. Since weaker bases are made from elements on the right-hand side of a periodic-table row, their conjugate acids must be stronger. Thus, binary acid strengths increase as hydrogen is combined with elements progressively further to the right of a periodic-table row.
Keywords	relative, acid, strength, periodic-table, binary

01-18-41UN

Title	Methanol and Methylamine
Caption	pKa values for the conjugate acids of methanol and methylamine.
Notes	Since oxygen is more electronegative than nitrogen, oxygen holds a positive charge more easily than nitrogen, making the conjugate acid of methylamine more stable (weaker) than the conjugate acid of methanol. Thus, the conjugate acid of methylamine has a higher pKa value.
Keywords	oxygen, nitrogen, methanol, methylamine, conjugate, acid, pKa

01-18-43UN

Title	Acid–Base Properties of Halides
Caption	Relative sizes of halogen atoms, relative basicities of halides, and relative acidities of halogen binary acids.
Notes	As anions are created from elements further down a column in the periodic table, they get larger, spread out electron density, and thus become more stable (weaker bases) even though the atoms become less electronegative. The corresponding binary conjugate acids become stronger as they are created from elements further down a periodic-table column.
Keywords	halogen, halide, basicities, acidities, periodic-table, electron, density

01-18-44UN

Title	Electrostatic Potential Maps of Hydrogen Halides
Caption	Halogen atoms in binary acids increase in size dramatically from HF to HI.
Notes	Halogen atoms bonded to hydrogen increase in size dramatically from HF to HI. Even though HF is clearly more polar than HI due to electronegativity differences of the halogens, iodide ion is more stable than fluoride ion because the negative charge can spread out over such a large volume in iodide relative to fluoride. This results in an increasing acid strength from HF to HI.
Keywords	electrostatic, potential, maps, halides, halogens, electronegativity, volume

01-18-56

Title	Potential Maps of Substituted Acetic Acids
Caption	Electrostatic potential maps of some substituted acetic acid molecules arranged in order of increasing substituent electronegativity.
Notes	As a substituent attached to the methyl group of acetic acid becomes more electronegative, the electron density on the oxygens of the molecule diminishes. This results in less negative charge on the oxygen atoms in the conjugate base anion, a more stable conjugate base, and a stronger acid as the substituent electronegativity increases.
Keywords	substituent, acetic, acid, substituted, potential, maps

01-19

Title	Conjugate Acid/Base Composition and pH
Caption	The relative amounts of a compound with a pKa of 5.2 in the acidic and basic forms at different pH values.
Notes	When a compound with a pKa of 5.2 is in a solution of pH 5.2, half the compound will be in the acidic form and the other half will be in the basic form. In lower pH solutions the acidic form will predominate, and in higher pH solutions the basic form will predominate.
Keywords	pKa, acidic, basic, pH, conjugate, acid, base

01-19-06UN

Title	Lewis Acids and Bases
Caption	Lewis acids accept electrons from other substances and Lewis bases donate electrons to other substances.
Notes	Substances containing atoms with nonbonding electrons (e.g., nitrogen and oxygen) are often Lewis bases, whereas substances containing atoms with octet deficiencies (e.g., boron and aluminum) are often Lewis acids.
Keywords	Lewis, acid, base, boron, aluminum, nitrogen, oxygen

01-00-06T02UN

Title	Table 1.2 The Ground State Electronic Configuration of the Smallest Atoms
Caption	The ground-state electronic configurations of the lightest atoms.
Notes	The ground-state electronic configuration of an atom is a description of the orbitals occupied by an atom's electrons when they are all in the lowest available energy orbitals.
Keywords	ground-state, electronic, configuration, energy, orbitals

01-01-06T03UN

Title	Table 1.3 The Electronegativities of Selected Elementsa
Caption	Electronegativity is the tendency of an atom to attract bonding electrons toward itself.
Notes	Electronegativity increases as you move across a row to the right and increases as you go up any of the columns of the periodic table.
Keywords	Pauling, electronegativity, trend, periodic

01-01-26T05UN

Title	Table 1.5 Atoms bonded to a carbon.
Caption
Notes
Keywords

01-01-29T05UN

Title	Table 1.5 Groups bonded to the far right carbon.
Caption
Notes
Keywords

01-01-30T05UN

Title	Table (cont'd)Two or more identical groups considered bonded.
Caption	Electronic structures for different compounds
Notes	Compounds can be written in different forms. The condensed structures are simplified by omitting some or all of the covalent bonds (lines and dots) and listing atoms bonded to a particular carbon (or nitrogen, or oxygen) next to it with a subscript to indicate the number of such atoms.
Keywords	structure,condensed,electronic

01-01-31T05UN

Title	Table 1.5 An oxygen doubly bonded to a carbon.
Caption	Condensed structures can be written in different forms
Notes	The condensed structures are simplified by omitting some or all of the covalent bonds (lines and dots) and listing atoms bonded to a particular carbon (or nitrogen, or oxygen) next to it with a subscript to indicate the number of such atoms.
Keywords	condensed,structures

01-18-35T08UN

Title	Table 1.8 Approximate pKa values
Caption	The pKa equals the pH when the solution is at equilibrium.
Notes	The stronger the acid, the lower the pKa. Strong acids have weak,stable conjugate bases.
Keywords	pKa,conjugate,acid,base

01-TB01

Title	Table 1.1 Distribution of Electrons in the First Four Shells That Surround the Nucleus
Caption
Notes
Keywords

Title	Table 1.4 The Dipole Moments of Some Commonly Encountered Bonds
Caption
Notes
Keywords

Title	Table 1.5 KekulŽ and Condensed Structures
Caption
Notes
Keywords

Title	Table 1.7 Comparison of the Bond Angles and the Lengths and Strengths of the Carbon–Carbon and Carbon–Hydrogen Bonds in Ethane, Ethene, and Ethyne
Caption
Notes
Keywords

Title	Table 1.9 The Values of Some Simple Acids
Caption
Notes
Keywords

Chapter 1 Electronic Structure and Bonding

Chapter 1
Electronic Structure and Bonding