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A somewhat typical TCP conversation is shown in Figure 7.7. here, an entire (albeit short) TCP conversation is shown from start to finish. note that this is a simplified example in which host 1 is sending data to host 2, but host 2 is simply acknowledging the data and is not sending any data of its own to host 1. host 2 could send data of its own to host 1 because TCP is a full-duplex protocol; it is just not doing so in this example.



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The most extensive generalization of the concept of acids and bases was that proposed in 1938 by G. N. Lewis, who concluded that the Br0nsted concept of limiting the group of acids to substances with a dissociable hydrogen prevents the general understanding of the chemistry of acids, in the same way as the early definition of oxidants as oxygen-containing substances impeded the general understanding of oxidation-reduction reactions. In view of this, he related the acidic and basic character of substances to their electron structure by the following definition: A base is a substance capable of acting as an electron-pair donor. An acid is a substance capable of acting as an electron-pair acceptor. According to this definition the group of bases practically includes just about the same substances as the Br0nsted conception, but with a few additions such as the inert gases (e.g. argon reacts as a base with boron trifluoride). On the other hand, the category of acids is much wider than





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60 under the Br0nsted definition, as it includes species such as H + , HCl, A1C13, SnCl3, SO2, SO3, O, Ag + , Be 2+ , Cu 2+ , etc. The Lewis acids that also fulfil the Br0nsted definition form a special group of protonic acids and can be formally considered to be the products of neutralization of a proton by a base (for example Cl~). The reaction between an acid and a base produces a coordination compound (complex). In contrast to former theories, this is more an addition than an exchange reaction. On the other hand, an exchange reaction in the Lewis sense is the result of competition between two acceptors for a single donor or between two donors for a single acceptor. Thus the typical Br0nsted acid-base reaction HA + B ^A + HB is the result of competition between two bases :A and :B for the acceptor H + . The reactions (A1C13 <- A) + :B < (A1C13 <-B) + :A are analogous. The classical reactions depend on replacement of one base (Bx) by another (B n ): HCl + NH3 -* NH 4 + + Cl" HCl + H 2 O ^ H 3 O + + C r H2O + NH3 -* NH 4 + + OH" H2O + CH3COO~ -* CH3COOH 4- OH" Salt formation Dissociation (1.4.33) Dissociation Hydrolysis

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The Lewis concept permits inclusion of acids and oxidants in a single group of electrophilic substances and bases and reductants in a single group of nucleophilic substances. The only difference between acid-base and redox reactions lies in the nature of the bond formed. However, a wide generalization usually brings a number of complications. The reactions between acids and bases have become so specific that they evade mutual comparison and arrangement in a series according to their strengths. Consequently, Lewis complemented his original definition by further, purely phenomenological definitions that are not in any way related to the theory of the structure of molecules and are based only on the behaviour of substances during chemical reactions: Bases are substances that (similar to OH~ ions) neutralize hydrogen ions or some other acid. Acids are substances that (similar to H + ions) neutralize hydroxide ions or other bases. Acids and bases have the following properties: (a) The mutual neutralization reaction is fast and has low activation energy. (b) Species of the same type can exchange with one another (e.g. one base for another one). (c) They can be titrated with the help of acid-base indicators. (d) They catalyse chemical reactions. These complementary definitions, however, do not solve the problems, as

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