1 82 Chapter 6 Acid-ase and Donor-Acceptor Chemistry CATER 6: ACID-ASE AD DR-ACCETR CEMISTRY 6.1 Acid ase Definition a. Alr 3 r Lewis b. Cl 4 C 3 C Lewis, rønsted-lowry c. i 2+ 3 Lewis d. Cl 3 Lewis e. S 2 Cl 3 Lewis f. C 3 7 C Lewis, rønsted-lowry 6.2 Acid ase Definition a. Xe 3 Lewis This is not a rønsted-lowry reaction since the product connectivity is [Xe 3 ()]. b. t Xe 4 Lewis c. 2 Se 4 C 2 5 Lewis, rønsted-lowry d. [C 3 g( 2 )] + S Lewis This reaction likely occurs via the following steps: [C 3 g( 2 )] + S [C 3 g(s)] + 2 [C 3 g(s)] + 2 [C 3 gs] While a rønsted-lowry reaction occurs in the second step, the species listed in roblem 6.2d are involved in the initial Lewis acid-base reaction. e. C 3 C (benzyl) 3 Lewis, rønsted-lowry f. Cl S 2 Lewis 6.3 Al 3+ is acidic: [Al( 2 ) 6 ] [Al( 2 ) 5 ()] The hydronium ions react with the basic bicarbonate to form C 2 : 3 + (aq) + C 3 (aq) 2 2 (l) + C 2 (g) With pk a values of 5.0 for [Al( 2 ) 6 ] 3+, 6.4 for 2 C 3, and 2.0 for S 4, the p is about 3, low enough to convert the bicarbonate to C 2.
2 Chapter 6 Acid-ase and Donor-Acceptor Chemistry An increase in conductivity suggests that ions are formed: r 3 + K r 4 + K a. The ions are [r 6 ] and [r 4 ] + : 2 Cs[r 6 ] + [r 4 ][Sb 2 11 ] 3 r CsSb 6 b. [r 6 ] : h (this complex features a stereochemically inactive nonbonding pair on the central r atom. See A. R. Mahjoub, X. Zhang, K. Seppelt, Chem. Eur. J. 1995, 1, 261.) [r 4 ] + : C 2v c. [r 4 ] + acts as a Lewis acid, accepting. r S 4 3 S S 4 and form enough ions to allow conductance in the pure acids. 6.7 Gas-phase basicity is defined as G for + (g) (g) + (g), while proton affinity is for the same reaction. Since G T S, and S is undoubtedly positive for these reactions (where one mole of gaseous reactant is converted to two moles of gaseous products), it makes sense that the gas-phase basicities in Table 6.6 are less positive than the corresponding proton affinities. 6.8 These data suggest the following basicity ranking for these ketones: < < 3 C C 3 3 C 2 C C 2 C 3 h h A convenient way to rationalize this basicity ranking is to examine the conjugate acids via resonance arguments. ne resonance form features a positive charge on the carbonyl carbon (structure, right). Since benzophenone can further delocalize this positive charge into its phenyl groups, the conjugate acid of benzophenone is the most stabilized of the three acids, leading to benzophenone being the strongest base. Since an ethyl group is slightly more electron-releasing than a methyl group, the conjugate acid of diethylketone is slightly more stabilized relative to the conjugate acid of acetone (structure is more effectively stabilized in the conjugate acid of diethylketone relative to A, the conjugate acid of acetone). Acetone is R R R consequently the weakest base among these ketones. A 6.9 These data indicate that triphenylphosphine ( h 3 ) is more basic than triphenylamine ( h 3 ) in the gas phase. n the sole basis of electronics, triphenylamine would be expected to be more basic by virtue of the higher electronegativity of relative to, leading to the center being more electron rich than the center. owever, the origin of the observed gas-phase basicity ranking must be the varying abilities of these atoms to accommodate the tetrahedral geometries of the conjugate acids. The larger covalent radius of relative to results in longer C(phenyl) bonds than C(phenyl) bonds, resulting in less steric strain between the phenyl rings in R
3 84 Chapter 6 Acid-ase and Donor-Acceptor Chemistry [h 3 ] relative to [h 3 ]. The conjugate acid [h 3 ] has less steric hindrance than [h 3 ], and h 3 is more basic The data are graphed below. Diethylether Dimethylether Ethanol Methanol Water pk a of Conjugate Acid in Water Gas-hase asicity (kj mol -1 ) a. The gas-phase and aqueous basicity data correlate poorly. The strongest base in aqueous solution ( 2 ) is the weakest base in the gas phase. While basicity in water increases as Me 2 < Et 2 < Me < Et < 2, the basicity in the gas-phase increases as 2 < Me < Et < Me 2 < Et 2. b. The ethers are the strongest gas-phase bases within this series on the basis of the electronic impact of two electron-releasing alkyl groups bound to the oxygen atom compared to one group (R) or no alkyl groups ( 2 ). The oxygen atoms of these ethers are relatively electron rich as a result. owever, the ethers are the weakest bases in water of this series; their conjugate acids have fewer sites for hydrogen bonding with 2 relative to the conjugate acids of alcohols and water. The poorer ability of the conjugate acids of the ethers to be solvated by water renders these ethers very poor bases in aqueous solution. c. As shown in the graph and the basicity rankings above, the ethyl molecule is more basic than the methyl molecule in both the gas-phase and in aqueous solution. This is undoubtedly an inductive effect; the more electron-releasing ethyl group renders Et 2 and Et more basic than Me 2 and Me, respectively, in both phases. d. 2 is the strongest base in water of this series on the basis of the excellent ability of its conjugate acid ( 3 + ) to be solvated by water via hydrogen bonding. It is the weakest gas-phase base within this series as a consequence of the relatively poor inductive effect of compared to methyl and ethyl in increasing electron density at the oxygen atom.
4 Chapter 6 Acid-ase and Donor-Acceptor Chemistry This 3 affinity trend is strongly correlated to the inductive ability of the groups bound to sulfur. These data suggest that the electron-releasing ability of substituents in sulfoxides ( R 2 S) increases as R h Me n u cyclo-(c 2 ). A resonance argument can be employed to further rationalize the relatively low 3 affinities of h 2 S and hsme. The phenyl group permits delocalization of the formal positive charge at the oxygen in structure C (below), rendering this oxygen atom less Lewis basic than when alkyl groups which cannot enable this attenuation of the positive formal charge are present instead of phenyl groups. S 3 S 3 S 3 ther resonance forms with further delocalization of positive charge into phenyl rings A C 6.12 a. According the the authors, a reference acid should be a strong enough Lewis acid to react with most common bases; form 1:1 acid-base adducts; have spectroscopic characteristics that can be monitored to observe variations in the strength of Lewis bases when reactions are conducted; and should not undergo side reactions while acting as a Lewis acid. b. Lewis basicity towards the zinc(ii) reference is governed significantly by the steric hindrance created at the nitrogen upon complexation. The bases quinuclidine and pyridine, both of which feature insignificant geometric changes at nitrogen upon binding, were found more Lewis basic than all primary, secondary, and tertiary amines examined with the zinc(ii) reference. This is not the case when assessing Lewis basicity via 3 affinities. or example, the 3 affinity for pyridine ( kj mol ) is less than for some tertiary amines (for example, the 3 affinity of Me 3 is kj mol ). c. The importance of steric hindrance is reflected in the trends observed. When acyclic amines are considered, the less hindered primary amines were generally the strongest Lewis bases. A clear trend was not observed with secondary and tertiary amines, but secondary amines were found stronger bases than tertiary amines when bases with the same alkyl group were examined. Among alicyclic amines, the trend is opposite in that quinuclidine (tertiary) was found stronger than the secondary amine piperidine. The authors state the relative order of the Lewis basicity for acyclic amines as primary > secondary > tertiary, but an inverted order for alicyclic amines ( tertiary > secondary primary (acyclic) ) a. The frustrated Lewis pair of the sterically encumbered (t-c 4 9 ) 3, in combination with the highly Lewis acidic (C 6 5 ) 3, binds 2 to give a linkage. t u t u t u C 6 5 b. This complex has been characterized by single crystal X-ray crystallography (figure at right). C 6 5 C 6 5
5 86 Chapter 6 Acid-ase and Donor-Acceptor Chemistry 6.14 a. The reaction coordinate diagram is below. The van der Waals complex is hypothesized to be stabilized via significant pi-stacking between the aromatic rings of the borane and the secondary amine. In the transition state, the bond has fully formed, and the proton is beginning to form a C bond with the previously aromatic ring of the amine. The formal positive charge of the hydrogenated intermediate (not shown on the ispo carbon of the amine) is stabilized by resonance. C 6 5 C 6 5 C 6 5 t u C 6 5 van der Waals complex (12.3 kcal/mol) TS 15.7 kcal/mol t u C 6 5 C 6 5 t u ydrogenated Intermediate (4.8 kcal/mol) t u h C 6 5 C C 6 5 rustrated Lewis air and ydrogen (0.0 kcal/mol) [h( t u) 2 ][(C 6 5 ) 3 ] (-10.0 kcal/mol) [(C 5 11 )( t u) 2 ][(C 6 5 ) 3 ] (Relative energy unspecified) b. As proposed in the reference, the phenyl ring of the amine in the van der Waals complex rotates towards the boron atom. The hydrogen molecule is then split in this cavity formed by the borane and the phenyl ring of the secondary amine. The hydride bonds to the boron, and the proton binds to the para carbon of the amine phenyl ring. c. The activation barrier for hydrogenation of the phenyl ring of the secondary amine is higher than that for formation of [h(tu) 2 ][(C 6 5 ) 3 ], which is considered the resting state for this reaction. Therefore the rate of the hydrogenation reaction is exceedingly low in pentane at ambient temperature, but viable in refluxing toluene. d. The salt [ i r 2 h][(c 6 5 ) 3 ] forms when the more basic i r 2 h is employed. It is hypothesized that i r 2 h is sufficiently basic to not allow formation of the areneborane van der Waals complex necessary to permit hydrogenation of the aromatic ring of the amine The distance in the complex 2b is pm, longer than the corresponding bond in free (115.1 pm). ond lengthening is expected since likely uses its * orbital (its LUM) to accept electron density from the phosphine. opulation of an orbital that is antibonding with respect to the bond will result in a longer bond distance. It is also noteworthy that the LUM of features greater orbital contribution from the nitrogen atom relative to the oxygen atom, and the nitrogen atom binds to the phosphorous atom in 2b. a. Complex 2b has strong radical character at oxygen, and reacts with 1,4-cyclohexadiene via a hydrogen-atom abstraction pathway to afford benzene.
6 Chapter 6 Acid-ase and Donor-Acceptor Chemistry 87 (C 6 5 ) 2 (C 6 5 ) 2 + Resonance stabilzed radical (C 6 5 ) 2 Complex 2b also reacts with the stronger C bond of toluene, with hydrogen-atom abstraction followed by radical coupling to form an C bond. (C 6 5 ) 2 + (C 6 5 ) 2 2 C (C 6 5 ) C (C 6 5 ) 2 (C 6 5 ) 2 2 C b. While the radical formed upon hydrogen-atom abstraction from the C 3 group of toluene is resonance stabilized, C coupling involving a carbon atom in the ring would lead to a nonaromatic product (one such product is shown at right). Coupling at the primary carbon results in the retention of aromaticity in the product (left). (C 6 5 ) 2 vs. (C 6 5 ) 2 C a. The pk a for the water/sc pair is much smaller than for the water/c pair. The hydrogen bonding between water and SC is predicted as much stronger. b. The hydrogen bond donors that have the smallest pk a with nitriles are Cl 4 and I. c. (C) 3 C has the smallest pk a with organic sulfides among the organic acids. d. Classification on the basis of estimated pk a values from the Slide Rule and the criteria in Section 6.5.1: Amines (medium strong), triphosphines (medium strong), sulfoxides (medium), ketones (medium/medium weak), and nitro compounds (medium weak).
7 88 Chapter 6 Acid-ase and Donor-Acceptor Chemistry 6.17 a. The structure has the r atoms in a staggered structure, resulting in S 6 symmetry. b. It is convenient to visualize this using tetrahedral, sp 3 hybridized As. An sp 3 orbital on each As points inward toward the benzene ring. If the hybrid lobes have opposite signs of their wave functions, they fit the symmetry of the π orbitals of the benzene ring to form bonding and antibonding molecular orbitals. The bonding interaction is shown. As As 6.18 a. The very high electronegativity of in comparison with Al pulls the bonding pair very close to. This increases the repulsion between the bonding pairs and causes the large angle. The steric bulk of the AlCl 3 and Cl 3 is not considered an important factor in dictating the large angle. b. The dative bond between Cl 3 and AlCl 3 likely employs a nonbonding donor orbital of Cl 3. The donation of electron density from a nonbonding orbital of Cl 3 would not be expected to significantly impact the bond order a. The methyl groups in (C 3 ) 3 S 3 donate electrons to the nitrogen, making (C 3 ) 3 a stronger Lewis base and strengthening and shortening the S bond. (C 3 ) 3 S 3 3 S 3 S pm pm S b. The greater concentration of electrons in the S bond of (C 3 ) 3 S 3 increases electron-electron (bp-bp) repulsions, opening up the S bond in comparison with 3 S a. The polarity of the Xe bonds concentrates electrons on the fluorine atoms, which act as the centers of Lewis basicity. As shown in the reference, which provides the structure of [Cd(Xe 2 )]( 4 ) 2, the Xe Cd bond is strongly bent at the fluorine and the geometry around xenon is nearly linear, with an Xe bond angle of b. The 4 ion is smaller than As 6, and the charge per fluorine is also greater in 4, making 4 the stronger Lewis base. In addition, the higher oxidation state of cadmium(ii) in [Cd(Xe 2 )]( 4 ) 2 enables stronger interaction with the fluorines in 4 than occurs between the silver(i) ion and As 6 in [Ag(Xe 2 )]As 6.
8 Chapter 6 Acid-ase and Donor-Acceptor Chemistry An energy level diagram for - is below. The M is the π* orbital. onding with + depends on which end of the π* orbital carries more electron density. Calculation shows slightly more electron density on, making the more likely (bent) molecule. This is consistent with the energy of the nitrogen 2p subshell ( ev) relative that of the oxygen 2p subshell ( ev); the nitrogen 2p orbitals should contribute more to these π* orbitals relative to the oxygen 2p orbitals. roblem 6.43 asks for calculation of the molecular orbitals of both and to address this question from an alternate perspective. 2p 2p 2p 2p 2p 2p 2s 2s 2s 2s 6.22 a. This is similar to the effects described in Section for I 2. r 2 forms charge-transfer complexes with donor solvents such as methanol. b. The 500 nm band (π* *) should shift to shorter wavelength (higher energy) because the difference in energy between the π* and * orbitals is greater in r 2 C 3 than in r Al 3 + Al 4. The a +, Al 4 salt can dissolve in. When 3 is added, it has a stronger attraction for the fluoride ions, with the reaction Al Al Soft metal ions do not combine with oxygen as strongly as hard metal ions, so reactions such as 2 g 2 g + 2 (g) 2 Cu 2 Cu + 2 (g) 2 Ag 2 4 Ag + 2 (g) Cu + C Cu + C(g) 2 Cu + C 2 Cu + C 2 (g) are more easily carried out. Reduction of some of the softer metals can be carried out with relatively low temperatures (campfires); some think use of rocks containing ores could have led to accidental reduction to the metals and discovery of the smelting process. arder metals such as iron require much higher temperatures for the reduction process.
9 90 Chapter 6 Acid-ase and Donor-Acceptor Chemistry 6.25 g is a much softer metal, and combines with the soft sulfide ion more strongly. Zinc and cadmium are more borderline metals, and combine with all the anions with more nearly equal facility When any of these salts vaporize, the vapor phase consists of molecules. When they are in the solid state, they are ionic, with some covalent properties. The liquid state is between the two, and can be made up of ions, covalent molecules, or something between these two extremes. If the liquid is molecular, vaporization should be easier (molecules in the liquid phase being converted to molecules in the vapor phase). If the liquid is mostly ionic, vaporization is more difficult. Using this criterion, the most ionic liquids should be Zn 2 and Cd 2, and the most molecular liquids should be g 2 and gcl 2. n a more general view, mercury, as the softest metal in the series, forms the more molecular compounds and zinc, as the hardest, forms the more ionic compounds. Cadmium forms the most molecular compound with the borderline bromide a. pyridine + 3 : = E py E 3 C py C 3 = [(1.17)(9.88) + (6.40)(1.62)] = 21.9 kcal/mol or 91.6 kj/mol. This predicted value is roughly 13% less exothermic than the experimental value of -105 kj/mol. pyridine + (C 3 ) 3 : = E py E (C3 ) 3 C py C (C3 ) 3 = [(1.17)(6.14) + (6.40)(1.70)] = 18.1 kcal/mol, or 75.7 kj/mol. This predicted value is more exothermic than the experimental values of -64 and kj/mol, respectively. b. luorine is electron-withdrawing, and C 3 electron-releasing. Therefore, in 3 carries a greater positive charge and interacts more strongly with Lewis bases such as pyridine. c. The harder acid 3 interacts more strongly with the borderline base pyridine : = E 3 E 3 C 3 C 3 = [(1.36)(9.88) + (3.46)(1.62)] = 19.0 kcal/mol, or 79.5 kj/mol 3 + (C 3 ) 3 : = E 3 E (C3 ) 3 C 3 C (C3 ) 3 = [(1.36)(6.14) + (3.46)(1.70)] = 14.2 kcal/mol, or 59.4 kj/mol The order is pyridine + 3 > > pyridine + (C 3 ) 3 > 3 + (C 3 ) 3. The change from 3 to (C 3 ) 3 is larger than the change from pyridine to 3.
10 Chapter 6 Acid-ase and Donor-Acceptor Chemistry Absolute hardness parameters: I A C (C 3 ) The difference between the M of pyridine (9.3) and the LUM of 3 ( 3.5) is smaller than the other possible interaction, so this pair has the largest, in spite of the difference in hardness. y comparison with the nitrogen compounds, (C 3 ) 3 is expected to have an absolute hardness lower than that of 3, approximately CsI and Li fit asalo s principle that ions of similar size and equal (but opposite) charge form the least soluble salts. Cs and LiI have ionic sizes that are very different, and they do not fit as well into an ionic lattice. In addition, CsI and Li are soft soft and hard hard combinations, which combine better than the hard soft LiI and soft hard Cs The following reaction is unlikely since C is soft and is hard. 3 C C 3 3 C + C 3 The second reaction is is more likely. Adding the carbonyl oxygen makes C harder, and C in C 3 and the atom are soft. 3 C C C 3 3 C C + C a. Solubilities: MgS 4 > CaS 4 > SrS 4 > as 4 Electrostatic forces predict the reverse order due to cation sizes (the charge density of Mg 2+ is greater than that of the larger a 2+ ), but the larger cations fit better with the large sulfate anion in the crystals. ydration of the cations is the strongest for Mg 2+, weakest for a 2+, agreeing with the solubility order. b. Solubilities: bcl 2 > br 2 > bi 2 > bs As a moderately soft cation, b 2+ has stronger interactions with the softer anions (hardness order: Cl > r > I > S 2 ). In addition, hydration of the anions is largest for the chloride, smallest for sulfide, based on size The order is Al C W (see igure 13.17). The oxygen of C is the harder end of this molecule and bonds with the harder Al atom; carbon and W engage in a soft soft interaction.
11 92 Chapter 6 Acid-ase and Donor-Acceptor Chemistry 6.34 a. Te 2 is the strongest acid, because Te is more electronegative than either Sn or Sb. Therefore, the hydrogen is more positive and acidic. b. 3 is the strongest base because is more electronegative than either or Sb. c. (C 3 ) 3 is the strongest base in the gas phase because the methyl groups contribute electron density to the nitrogen. In solution, the order is scrambled, probably due to solvation (Section 6.3.6). d. 4-Methylpyridine > pyridine > 2-methylpyridine. Again, the methyl group adds electron density to the. owever, with methyl in the 2 position, steric hindrance makes bonding to Me 3 more difficult In general, oxide ion reacts with water to form hydroxide: In 2 3, the small, hard 3+ holds on to the oxide ions strongly. As a result, () , and the solution is very weakly acidic (pk a = 9.25). In Al 2 3, the Al 3+ ion is larger and softer. It can form either [Al() 4 ] (acting as an acid) or [Al( 2 ) 6 ] 3+ (acting as a base), depending on the other species in solution. Sc 3+ is still larger and softer, so it combines better with water than with hydroxide ion. The result is the reaction Sc [Sc( 2 ) 6 ] a. Ca Ca Calcium has a lower electronegativity than hydrogen, so Ca 2 is Ca 2+ ( ) 2 and the hydride ions react with water. b. r r romine is more electronegativite than hydrogen, so the hydrogen is strongly positive and is readily transferred to the lone pair of water. c. 2 S S Sulfur is slightly more electronegative than hydrogen, and the positive hydrogen in 2 S can dissociate to a small extent. d. C no reaction. The C bond is almost nonpolar; the interaction between the oxygen atom of water and this C bond required for hydrogen ion transfer is exceedingly weak > (C 3 ) 3 > (C 2 5 ) 3 > (C 6 2 (C 3 ) 3 ) 3 Alkyl groups are electron-donating and increase the electron density on and reduce the attraction for the lone pair of 3. The bulky mesityl groups render (C 6 2 (C 3 ) 3 ) 3 less Lewis acidic on the basis of the steric hindrance introduced when these boron centers adopt the required tetrahedral geometry upon complexation of a. C 3 2 is a stronger base on the basis of the electron-releasing ability of the methyl group. b. Although 2-methylpyridine is the stronger base with smaller acid molecules, the methyl group interferes with adduct formation with trimethylboron (-strain) and the pyridine-trimethylboron dative bond is stronger.
12 Chapter 6 Acid-ase and Donor-Acceptor Chemistry 93 c. Trimethylboron forms a stronger adduct with ammonia because the three phenyl rings of triphenylboron cannot bend back readily to allow the boron to become tetrahedral (-strain) a. With the acids listed in order of increasing acidity: 3 As 4 2 S 3 2 S 4 Mn 4 pk a (9-7n) pk a (8-5n) pk a (exp) b. With the acids listed in order of increasing acidity: Cl Cl 2 Cl 3 Cl 4 pk a (9-7n) pk a (8-5n) pk a (exp) Dimethylamine acts as weak base in water, with a very small amount of provided by the reaction (C 3 ) (C 3 ) Acetic acid is a stronger acid than water, so dimethylamine acts as a stronger base, and the reaction (C 3 ) 2 + Ac (C 3 ) Ac goes to completion. 2-utanone is a neutral solvent; there is no significant acid-base reaction with dimethylamine Sb 5 in reacts to increase the + concentration and decrease 0 : Sb Sb 6. These ions then can react with alkenes a. As the Lewis acids 3 and Cl 3 interact with 3, the geometry around boron changes from planar to trigonal pyramidal; however, in accord with the LC model the nonbonded and Cl Cl distances are nearly constant, suggesting that these atoms remain in contact with each other. ecause these nonbonded distances remain essentially constant, the boron halogen distance must increase as the distortion from trigonal geometry occurs. ecause of the strength of the bond, a consequence of the large electronegativity difference between and and the small size of the fluorine atom, more energy is required to distort 3 from planarity than to similarly distort Cl 3. (Calculations in support of this argument are presented in the reference.) The consequence of this energy requirement is that 3 is a weaker Lewis base than Cl 3 toward 3. The article does not address the relative Lewis basicity of r 3, but a similar argument could apply for this compound. b. This article does not consider the LC model but focuses on ab initio calculations on the adducts X 3 3. These calculations show a higher bond dissociation energy in the Cl 3 adduct than in the 3 adduct. Although many factors are involved, an important issue is that Cl 3 has a lower energy LUM that is able to interact more strongly with the donor orbital of 3, giving a stronger covalent interaction (and stronger bond) in Cl 3 3.
13 94 Chapter 6 Acid-ase and Donor-Acceptor Chemistry 6.43 a. The energy diagram and the orbitals are shown below. 2p 2p 2p 2p 2p 2p 2s 2s 2s 2s The M is the π*, with greater concentration of electron density on. This orbital can overlap with the empty + 1s orbital, forming, a bent molecule. b. Calculations predict that is more stable than, with the energy of the M lower than the energy of the M. The M and M-1 of and, respectively, two of the nine molecular orbitals of these species arising from the valence orbitals, are shown below. M M 1
14 Chapter 6 Acid-ase and Donor-Acceptor Chemistry LUM M M 1 M 2 r 2 r 2 C 3 C 3 The interaction of the M of the methanol and the LUM of the r 2 results in the adduct LUM and M 2 orbitals, respectively. The geometry shown features the r 2 at approximately a trigonal angle ( r is 113 and C r is 106 in a M3 calculation) a. or orbitals of 3 and 3, see igures 5.32 and 5.30, respectively. b. The bonding molecular orbital, shown below, is polarized toward the more electronegative nitrogen; the matching antibonding orbital, which has a node between the boron and nitrogen atoms, is polarized toward the boron a. The sketch below is a first approximation of the postulated interaction responsible for the halogen bond with acetylene.
15 96 Chapter 6 Acid-ase and Donor-Acceptor Chemistry The donor orbital of acetylene is a pi-bonding orbital The acceptor orbital of r 2 is its * orbital b. A key orbital to look for is one in which the adjacent lobes of the pi-bonding orbital of acetylene, shown an a, and the * orbital of r 2 have merged into a larger lobe (occupied by an electron pair) that links the two molecules. This bonding orbital should have a matching antibonding orbital (empty) at higher energy.
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds: Acids and Bases Modified by Dr. Daniela R. Radu Why This Chapter? Description of basic ways chemists account for chemical
Benzene 1 NT 87 90 ompound 87 has the formula 6 6, is known as benzene, and it is a hydrocarbon derived from petroleum distillates. Benzene is the parent compound for a class of compounds known as aromatic
John E. McMurry http://www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds; Acids and Bases Javier E. Horta, M.D., Ph.D. University of Massachusetts Lowell Polar Covalent Bonds: Electronegativity
Bonds hapter 8 Bonding: General oncepts Forces that hold groups of atoms together and make them function as a unit. Bond Energy Bond Length It is the energy required to break a bond. The distance where
CHAPTER EIGHT BNDING: GENERAL CNCEPT or Review 1. Electronegativity is the ability of an atom in a molecule to attract electrons to itself. Electronegativity is a bonding term. Electron affinity is the
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
Substituted Alkanes While alkanes have very few reactions that occur, combustion and some radical reactions, substituted alkanes display a variety of reactions and properties X ften the amount of information
Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms 1 11.1 Periodic Trends in atomic properties 11.1 Periodic Trends in atomic properties design of periodic table is based on observing properties
rganic hemistry M 314 Dr. Laurie S. Starkey, al Poly Pomona Structure & Shape of rganic Molecules - hapter 1 (Wade) rganic (living things, chemistry of carbon) Examples of rganic ompounds: Inorganic (rocks,
Chapter 7 covalent bonding Introduction Lewis dot structures are misleading, for example, could easily represent that the electrons are in a fixed position between the 2 nuclei. The more correct designation
324 Chapter 6 Electronic Structure and Periodic Properties of Elements 6.5 Periodic Variations in Element Properties By the end of this section, you will be able to: Describe and explain the observed trends
CHAPTER 14 Practice Exercises 14.1 White phosphorus consists of individual P 4 molecules. Red phosphorus consists of linear chains of P 4 molecules. Black phosphorus consists of crosslinked chains of P
Name Date lass APTER 6 REVIEW hemical Bonding SETIN 1 SRT ANSWER Answer the following questions in the space provided. 1. a A chemical bond between atoms results from the attraction between the valence
Topic 4. Chemical bonding and structure There are three types of strong bonds: Ionic Covalent Metallic Some substances contain both covalent and ionic bonding or an intermediate. 4.1 Ionic bonding Ionic
INTDUCTIN T LEWIS ACID-BASE CEMISTY DEINITINS Lewis acids and bases are defined in terms of electron pair transfers. A Lewis base is an electron pair donor, and a Lewis acid is an electron pair acceptor.
CHAPTER NOTES CHAPTER 16 Covalent Bonding Goals : To gain an understanding of : NOTES: 1. Valence electron and electron dot notation. 2. Stable electron configurations. 3. Covalent bonding. 4. Polarity
New Section 3 Page 1 2:37 PM Friedel-Crafts reaction: Mechanism: Carbocation is the reactive electrophile. AlCl4- picks up a proton. Limitations come from the mechanism: Carbocationic intermediates prone
Bonding Models Section (Chapter, M&T) Chemical Bonding We will look at three models of bonding: Lewis model Valence Bond model M theory Bonding Models (Lewis) Bonding Models (Lewis) Lewis model of bonding
UTID: 2013 Objective Test Section Identify the choice that best completes the statement or answers the question. There is only one correct answer; please carefully bubble your choice on the scantron sheet.
APTER SEVEN Molecular Geometry 7.13 Molecular geometry may be defined as the three-dimensional arrangement of atoms in a molecule. The study of molecular geometry is important in that a molecule s geometry
CHAPTER 10: INTERMOLECULAR FORCES: THE UNIQUENESS OF WATER Problems: 10.2, 10.6,10.15-10.33, 10.35-10.40, 10.56-10.60, 10.101-10.102 10.1 INTERACTIONS BETWEEN IONS Ion-ion Interactions and Lattice Energy
Illustrating Bonds - Lewis Dot Structures Lewis Dot structures are also known as electron dot diagrams These diagrams illustrate valence electrons and subsequent bonding A line shows each shared electron
12. Alcohols and Phenols Based on McMurry s Organic Chemistry, 6 th edition Alcohols and Phenols Alcohols contain an OH group connected to a saturated C (sp 3 ) They are important solvents and synthesis
Andrew Rosen Chapter 2 - Families of Carbon Compounds 2.1 - Hydrocarbons: Representative Alkanes, Alkenes, Alkynes, and Aromatic Compounds - Hydrocarbons are compounds that contain only hydrogen and carbon
INTERMOLECULAR FORCES Intermolecular forces- forces of attraction and repulsion between molecules that hold molecules, ions, and atoms together. Intramolecular - forces of chemical bonds within a molecule
Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching
Chem 121 Problem set VIII LUTI - 1 Problem et VIII Liquids, olids, Intermolecular orces and Phase Diagrams 1a) this is a point on the vapour pressure curve 1b) gas 1c) gas to liquid Water C 2 2a) solid
11 Chemical Bonds The Formation of Compounds from Atoms Chapter Outline 11.1 11.2 Lewis Structures of Atoms 11.3 The Ionic Bond Transfer of Electrons from One Atom to Another 11.4 Predicting Formulas of
KOT 222 ORGANIC CEMISTRY II CAPTER 17 REACTIONS of AROMATIC COMPOUNDS 1 Electrophilic Aromatic Substitution Substitution of an electrophile for a proton on the aromatic ring. benzene s pi electrons are
Periodic Trends and Lewis Dot Structures Chapter 11 Review PERIODIC Table Recall, Mendeleev and Meyer organized the ordering the periodic table based on a combination of three components: 1. Atomic Number
GRADE 11 PHYSICAL SCIENCES SESSION 3: CHEMICAL BONDING Key Concepts In this session we will focus on summarising what you need to know about: Bonding Covalent bonding Electronegativity in covalent bonding
Chapter 8 Concepts of Chemical Bonding Chemical Bonds Three types: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms Ionic Bonding
Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.
Intermolecular forces are electromagnetic forces that hold like molecules together. Strong intermolecular forces result in a high melting point and a solid state at room temperature. Molecules that are
1 Bonding There is almost always a chemical bonding question. Since this is such an important topic, you should be prepared for any and all bonding questions. Prepare well for this topic!! Some suggestions
HM 200/202 xam 3 ovember 15, 2014 ame: Lab Section #: Please mark your answers on the scantron sheet using a #2 pencil and also mark your answers on the exam itself. Mark Test rom A on your scantron. 1.
Use the Force! Noncovalent Molecular Forces Not quite the type of Force we re talking about Before we talk about noncovalent molecular forces, let s talk very briefly about covalent bonds. The Illustrated
Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents (atoms, ions etc.) together in a chemical species. Various theories
6 th Year Chemistry Higher Level Sinéad Nolan Chemical Bonding No part of this publication may be copied, reproduced or transmitted in any form or by any means, electronic, mechanical, photocopying, recording,
* Enter your answers on the bubble sheet. Turn in all sheets. * This exam is composed of 25 questions on 7 pages total. Go initially through the exam and answer the questions you can answer quickly. Then
Inorganic Chemistry with Doc M. Day 3. Covalent bonding: Lewis dot structures and Molecular Shape. Topics: 1. Covalent bonding, Lewis dot structures in review, formal charges 2. VSEPR 6. Resonance 3. Expanded
AP hemistry Practice Test #6 hapter 8 and 9 1. Which of the following statements is incorrect? a. Ionic bonding results from the transfer of electrons from one atom to another. b. Dipole moments result
1 SAPES MLEULES (VSEPR MDEL) Valence Shell Electron-Pair Repulsion model - Electron pairs surrounding atom spread out as to minimize repulsion. - Electron pairs can be bonding pairs (including multiple
Section 8.5 Objectives Describe how electronegativity is used to determine bond type. Compare and contrast polar and nonpolar covalent bonds and polar and nonpolar molecules. Generalize about the characteristics
Worksheet 11 - Periodic Trends A number of physical and chemical properties of elements can be predicted from their position in the Periodic Table. Among these properties are Ionization Energy, Electron
ATER 10 TE AE MLEULE EMIAL ETI BED READIG RBLEM B10.1 lan: Examine the Lewis structure, noting the number of regions of electron density around the carbon and nitrogen atoms in the two resonance structures.
1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides
Lab 5: Periodic Trends Part I: (Prelab) A Computer Study and Introduction to ChemDraw Part II: Acid-Base Properties of Period 3 and Group 5A Elemental Oxides Part III: Oxidizing Ability of the Elemental
Lecture otes Chem 51B S. King Chapter 18 Electrophilic Aromatic Substitution I. Electrophilic Aromatic Substitution The most characteristic reaction of aromatic compounds is electrophilic aromatic substitution,
CHEMISTRY 101 EXAM 3 (FORM A) DR. SIMON NORTH 1. When considering conjugate acids and bases, (2 points) a) Strong acids have strong conjugate bases. b) Strong bases have strong conjugate acids. c) Weak
Aromatic compounds GE 1 BENZENE Structure Primary analysis revealed benzene had an... empirical formula of and a molecular formula of 6 6 Q.1 Draw out some suitable structures which fit the molecular formula
: General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
Acids and Bases Know the definition of Arrhenius, Bronsted-Lowry, and Lewis acid and base. Autoionization of Water Since we will be dealing with aqueous acid and base solution, first we must examine the
INTRDUCTIN T INIC MECANISMS PART I: FUNDAMENTALS F BRNSTED-LWRY ACID-BASE CEMISTRY YDRGEN ATMS AND PRTNS IN RGANIC MLECULES - A hydrogen atom that has lost its only electron is sometimes referred to as
Unit 8: Drawing Molecules bjectives Topic 1: Lewis Dot Diagrams & Ionic Bonding 1. Draw a Lewis dot diagram of any representative element. 2. Draw a Lewis dot diagram of any ionic compound. A Lewis structure
ATER 10 TE AE MLEULE 10.1 To be the central atom in a compound, the atom must be able to simultaneously bond to at least two other atoms. e,, and cannot serve as central atoms in a Lewis structure. elium
LS1a Fall 2014 Section Week #1 I. Valence Electrons and Bonding The number of valence (outer shell) electrons in an atom determines how many bonds it can form. Knowing the number of valence electrons present
2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution Oxides; acidic, basic, amphoteric Classification of oxides - oxide
Structure and Molecular Bonding CAPTER 9 1 Introduction Bonds - Attractive forces that hold atoms together in compounds Valence Electrons - The electrons involved in bonding are in the outermost (valence)
Comparing Ionic and Covalent Bonds Chapter 7 Covalent Bonds and Molecular Structure Intermolecular forces (much weaker than bonds) must be broken Ionic bonds must be broken 1 Ionic Bonds Covalent Bonds
Lecture 2 (9-12-16) Chapters 2 and 3 Goals: Review Periodic Table and the atom, types of bonding for carbon (hybridization), and Lewis structure Learn how to draw bond-line structures Problems: (for all
EM 2323 Unit 1 General hemistry Review I. Atoms A. The Structure of the Atom B. Electron onfigurations. Lewis Dot Structures II. Bonding A. Electronegativity B. Ionic Bonds. ovalent Bonds D. Bond Polarity
EXPERIMENT 9 Dot Structures and Geometries of Molecules INTRODUCTION Lewis dot structures are our first tier in drawing molecules and representing bonds between the atoms. The method was first published
Bonding and Lewis Structures 1 There are two types of chemical bonds: ionic and covalent. owever, some bonds are frequently in between. A. Ionic Bonds In an ionic bond, at least one electron is completely
Molecular and VSEPR We gratefully acknowledge Portland ommunity ollege for the use of this experiment. Objectives To construct molecular models for covalently bonded atoms in molecules and polyatomic ions
Version PREVIEW Exam 1 JOHNSON (53140) 1 This print-out should have 30 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. Cl Cl C Cl LDE Identifying
Electrophilic Aromatic Substitution Reactions, Course Notes Archive, 1 Electrophilic Aromatic Substitution Reactions An organic reaction in which an electrophile substitutes a hydrogen atom in an aromatic
Reactions of Aromatic Compounds Aromatic compounds are stabilized by this aromatic stabilization energy Due to this stabilization, normal S N 2 reactions observed with alkanes do not occur with aromatic
Chapter 9 Tro 1. Bromine tends to form simple ions which have the electronic configuration of a noble gas. What is the electronic configuration of the noble gas which the bromide ion mimics? A) 1s 2 2s
A REVIEW OF GENERAL CEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES A STUDENT SOULD BE ABLE TO: 1. Draw Lewis (electron dot and line) structural formulas for simple compounds and ions from molecular
ucleophilic Substitution & Elimination hemistry 1 eginning patterns to knowfor S and E eactions - horizontal and vertical templates for practice Example 1 - two possible perspectives (deuterium and tritium
Chapter 2 The Chemical Context of Life Multiple-Choice Questions 1) About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living
Class: Date: Chapter 9-10 practice test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which one of the following is most likely to be an ionic compound?
Chapter 9 Molecular Geometry and Bonding Theories 1. or a molecule with the formula AB 2 the molecular shape is. (a). linear or trigonal planar (b). linear or bent (c). linear or T-shaped (d). T-shaped
hemistry 15, hapter 7 Exercises Types of Bonds 1. Using the periodic table classify the bonds in the following compounds as ionic or covalent. If covalent, classify the bond as polar or not. Mg2 4 i2 a(3)2
Your consent to our cookies if you continue to use this website.