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kari74 [83]
3 years ago
15

Sodium is much more apt to exist as a cation than chlorine because:

Chemistry
1 answer:
8090 [49]3 years ago
7 0

Answer:

(D) chlorine has a greater ionization energy than sodium

Explanation:

Sodium is the element of the group 1 and period 3 which means that the valence electronic configuration is [Ne]3s^1.

Chlorine is the element of the group 17 and period 3 which means that the valence electronic configuration is [Ne]3s^23p^5.

Ionization energy is the minimum amount of energy which is required to knock out the loosely bound valence electron from the isolated gaseous atom.

<u>Thus, removal of one electron in sodium is easy as it will gain noble gas configuration and become stable. But this case does not exist in chlorine and hence, chlorine has a greater ionization energy than sodium.</u>

So,

Sodium is much more apt to exist as a cation than chlorine because chlorine has a greater ionization energy than sodium.

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Answer:

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Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to figure out the required net ionic equation by firstly writing out the complete molecular equation between aspirin and sodium acetate:

C_9H_8O_4+NaC_2H_3O_2\rightarrow C_2H_4O_2+NaC_9H_7O_4

Whereas acetic acid and sodium acetylsalicylate are formed. Now, we write the complete ionic equation whereby sodium acetate and sodium acetylsalicylate are ionized because they are salts yet neither aspirin nor acetic acid are ionized as they are weak acids:

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Finally, for the net ionic equation we cancel out the sodium spectator ions to obtain:

C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-

Regards!

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