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Lyrx [107]
1 year ago
7

How do two sublevels of the same principal energy level differ from each other?

Chemistry
1 answer:
dem82 [27]1 year ago
3 0

Two sublevels of the same principal energy level differ from each other through shape and size.

There are mainly 4 energy level s, p, d and f.

The s level has one orbital and one orbital have two electrons. So the maximum number of electron in s sublevel is 2.

The p level has three orbital and one orbital have two electrons. So the maximum number of electron in s sublevel is 6.

The d level has five orbital and one orbital have two electrons. So the maximum number of electron in s sublevel is 10.

The f level has 7 orbital and one orbital have two electrons. So the maximum number of electron in s sublevel is 14.

They may be differ in magnetic level.

Thus, we concluded that Two sublevels of the same principal energy level differ from each other through shape and size.

learn more about energy level:

brainly.com/question/14654539

#SPJ13

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PH scale is used to determine how acidic, basic or neutral a solution is
pH can be calculated using the H₃O⁺
ph can be calculated as follows
pH = - log[ H₃O⁺]
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The pka of a carboxylic can be affected greatly by the presence of various functional groups within its structure. An example of an inductive effect changing the pka can be shown with trichloroacetic acid, Cl3CCOOH. This molecule has a pka of 0.7. The decrease in pka relative to formic acid is due to the presence of the Cl3C- group, and more specifically the presence of the chlorine atoms. The electronegative chlorine atoms are able to withdraw the electron density away from the oxygen atoms and towards themselves, thus helping to stabilize the negative charge and stabilize the conjugate base. This results in an increase in acidity and decrease in pka.

The same Cl3CCOOH example can be used to explain how dipoles can effect the acidity of carboxylic acids. Compared to standard acetic acid, H3CCOOH with a pka of 4.76, trichloroacetic acid is much more acidic. The difference between these structures is the presence of C-Cl bonds in place of C-H bonds. A C-Cl bond is much more polar than a C-H bond, due the large electronegativity of the chlorine atom. This results in a carbon with a partial positive charge and a chlorine with a partial negative charge. In the conjugate base of the acid, where the molecule has a negative charge localized on the oxygen atoms, the dipole moment of the C-Cl bond is oriented such that the partial positive charge is on the carbon that is adjacent to the oxygen atoms containing the negative charge. Therefore, the electrostatic attraction between the positive end of the C-Cl dipole and the negative charge of the anionic oxygen helps to stabilize the entire species. This level of stabilization is not present in acetic acid where there are C-H bonds instead of C-Cl bonds since the C-H bonds do not have a large dipole moment.

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