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are shared equally between the atoms However, if the atoms are different (eg, the H and C1 atoms of HCl), the shared electrons are generally attracted more strongly by one of the atoms (C1 in the case of HCl), and this atom is said to be more electronegative than the other Thus, electronegativity is a measure of the relative ability of an atom in a molecule to attract electrons to itself The notion of electronegativity was introduced in 1932 by pauling;15 he was the first of several to propose a quantitative scale for its expression Based largely on thermochemical data, Pauling's electronegativity Xp assumes values between about 07 and 40 for those elements known to participate in compound formation Metallic elements have values less than about 20; nonmetals, values greater than about 20 Table 164 shows Pauling electronegativities for ten nonmetallic elements Of these, fluorine is the most electronegative (Xp = 40), and hydrogen, the least (Xp = 21) An intermolecular hydrogen bond forms between a hydrogen-donor molecule (conventionally represented as A-H) and an electron-rich acceptor site (conventionally denoted by the letter B) Entity A is an atom (possibly attached to other atoms), which is more electronegative than hydrogen Hydrogen-acceptor site B may be an atom more electronegative than hydrogen; the site may also be a double or triple bond, or it may be an aromatic hydrocarbon ring The hydrogen-bonded complex is conventionally represented as A-H B, where the three dots denote the hydrogen bond Examples of strong hydrogen donors include hydrogen fluoride (HF), water (HOH), hydrogen peroxide (HOOH), alcohols (ROH), carboxylic acids (RCOOH), ammonia (H2NH), primary amines (RNH2), and secondary amines (R2NH) In each of these molecules, one or more hydrogen atoms is attached to an atom of a highly electronegative element (F, 0 , or N; Table 164) The halogen acids HC1, HBr, and HI are also hydrogen donors, as are a few species containing the C-H bond However, the difference in electronegativity between carbon and hydrogen is not large (Table 164), and the ability of the H in C-H to function as a donor hydrogen seems possible only when the carbon atom is itself attached to highly electronegative atoms or electron-rich sites Verified examples of C-H hydrogen donors thus include chloroform (C13CH), dichloromethane (C12CH2),and hydrogen cyanide (NCH) The highly electronegative elements F, 0,and N serve as atomic hydrogen-acceptor sites Hence HF, HOH, HOOH, ROH, RCOOH, HzNH, R2NH and NCH are hydrogen acceptors But so are aldehydes (ROCH), ketones (ROCR), ethers (ROR), esters (ROCOR), and tertiary amines (R3N), species which have no active hydrogens.

The best program in the world would never generate errors, I guess. But come on, it s not reality. If a multimillion-dollar Mars probe is going to crash on a planet millions of miles away, even after years of advanced engineering, my customer-tracking application for a local video rental shop is certainly going to have a bug or two. But you can mitigate the impact of these bugs using the error-management features included with Visual Basic.

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The phenomenon of hydrogen bonding is easily rationalized The H in donor species A-H is electron deficient because of the higher electronegativity of A Hence the H is attracted to the electron-rich acceptor site B Unfortunately,such a simple electrostatic picture is unable to account quantitatively for some important features of the hydrogen bond16 As a result, an algebraic contribution cannot generally be ascribed to the intermolecular potential function U ( r )for hydrogen-bonding interactions Nevertheless, we can by example indicate the kinds of intermolecular pairs for which hydrogen-bondinginteractions are important Convenience here suggests division of hydrogen-bondinginteractions into two classes: association and solvation Association is an attractive interaction between molecules of the same kind In the context of hydrogen bonding, an associating species must have both an active hydrogen and a hydrogen-acceptor site Examples include water (the O is an acceptor site), ammonia (with N the acceptor site), alcohols, primary and secondary amines, and carboxylic acids Hydrogen bonding by association is often reflected dramatically in the properties (eg, boiling points, heats of vaporization, and viscosities) of the pure species

Table 165 Hydrogen-bonding Interactions among Pairs of Species 2)= nonassociating H-donor; A = nonassociating H-acceptor; AD = associating species

This chapter s project code will be somewhat brief. Error-handling code will appear throughout the entire application, but we ll add it in little by little as we craft the project. For now, let s just focus on the central error-handling routines that will take some basic action when an error occurs anywhere in the program. As for lambda expressions, we ll hold off on such code until a later chapter.

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