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10a. Is there a difference between the outputs of the show router interface command and the show router route-table command what is the difference 11. Do the ultimate test to verify that interfaces are functioning properly: Use the ping command to check for connectivity from a router to the far end of each of the inter-router links, for example, between the two PE routers and between PE1 and CE1. You will need to think carefully to ensure that you use the correct IP address. (ICMP ping and ARP are covered more thoroughly in 6.)

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Fig. 1.5 A scheme of hydration: (1) cation, (2) primary hydration sheath (water molecules form a tetrahedron), (3) secondary hydration shell, (4) disorganized water, (5) normal water

*B:PE1>config>router# ping 140.10.0.97 PING 140.10.0.97 56 data bytes 64 bytes from 140.10.0.97: icmp_seq=1 ttl=64 64 bytes from 140.10.0.97: icmp_seq=2 ttl=64 64 bytes from 140.10.0.97: icmp_seq=3 ttl=64 64 bytes from 140.10.0.97: icmp_seq=4 ttl=64 64 bytes from 140.10.0.97: icmp_seq=5 ttl=64

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interactions are, for example, the important factors affecting the conformational stability of proteins in aqueous solutions. O. J. Samoilov proposed a statistical approach to hydration. Ions in solution affect the thermal, particularly translational, motion of the solvent molecules in the immediate vicinity of the ion. This translational motion can be identified with the exchange of the solvent molecules in the neighbourhood of the ion. Retardation of this exchange is thus a measure of the ion solvation. If the water molecule remains in the vicinity of other water molecules for a time r and in the vicinity of the ion for a time rh then the ratio XJT is a measure of the solvation. If T , / T 1 , the water molecule is bonded very strongly to the ion. On the other hand, r / / r < l indicates negative solvation the ion breaks the solvent structure and the solvent molecules in its vicinity can more readily be exchanged with other molecules than those in the solvent alone, where a certain degree of ordering remains. Experimental values of the ratio T//T for aqueous solutions using H218O molecules lie in the range from tenths to unities. Some molecular solvents (such as ammonia, aliphatic amines, hexamethylphosphortriamide) dissolve alkali metals; solutions with molalities of more than lOmol-kg" 1 are obtained. Ammonia complexes M(NH3)6 analogous

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---- 140.10.0.97 PING Statistics ---5 packets transmitted, 5 packets received, 0.00% packet loss round-trip min < 10ms, avg < 10ms, max < 10ms, stddev < 10ms *B:PE1>config>router#

21 to the amminates or hydrates of salts can be crystallized from these solutions The solutions are blue (absorb at 7000 cm"1, corresponding to the s->p electron transition) and paramagnetic Paramagnetic resonance measurements indicate that cavities in the liquid with dimensions of about 03 nm contain free electrons Compared with aqueous salt solutions, these metal solutions have about 105 times larger molar conductivity, indicating electronic conductivity Thus, the metals in solution are dissociated to yield solvated cations M+ and electrons e~ (also solvated) More concentrated solutions also contain species such as M + e~, M2 and Me" The stability of these solutions is low because of the formation, for example, of alkali metal amides in solutions of alkali metals in liquid ammonia A form of solvation also occurs in ionic solvents, but coulombic interactions predominate.

The following lab is designed to reinforce your knowledge of the content in this chapter. Please review the instructions carefully and perform the steps in the order in which they are presented. The practice labs require that you have access to three or more Alcatel-Lucent 7750 SRs or Alcatel-Lucent 7450 ESSs in a non-production environment.

The solvent structure can be conceived as resulting from the penetration of two sublattices cationic and anionic The cations of the dissolved salt are then scattered throughout the cationic sublattice and the anions in the anionic sublattice If the dissolved salt and the solvent have a common anion, for example, then the cations are scattered throughout the cationic sublattice and the anionic lattice remains almost unaffected Let us assume that only one kind of foreign ion, a cation or an anion, is introduced into ionic solvents (while the electroneutrality condition is maintained) If the cation of the dissolved salt has a larger charge than the solvent cation, then vacancies must be scattered throughout the cationic sublattice so that the distribution of electric charge remains neutral An example of a more complicated situation is the formation of Na+ and A1C14~ ions in an equimolar melt of A1C13 + NaCl.

These labs are designed to be used in a controlled lab environment. Please DO NOT attempt to perform these labs in a production environment.

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