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Chapter 19: Problem 3

Use the shell model of atoms and the concept of core charge to explain why the AVEE of atoms generally increases from left to right across a period.

Short Answer

Expert verified
The AVEE of atoms generally increases from left to right across a period due to an increase in core charge. As we move across a period, the number of protons and electrons increases, but the electrons enter the same energy level. This results in increased attractive force, pulling the electrons closer to the nucleus, and making it harder for them to escape. The increased difficulty for electrons to escape, in turn, increases the energy of the electrons (AVEE).

Step by step solution

01

Understand Atomic Volume Electron Energy and Core Charge

AVEE refers to the energy of an electron in an atom. The shell model explains the arrangement of electrons in an atom in terms of energy levels. Core charge, on the other hand, is the unshielded nuclear charge experienced by the outermost electrons. It affects the attraction and repulsion force on the electrons.
02

Comprehend the changes in AVEE across the Period

Going from left to right across a period in the periodic table, the number of electrons and protons in an atom increases. The added electrons go into the same energy level or shell, which brings the electrons closer to the nucleus due to increased core charge. The increased number of protons also increases the attractive force.
03

Connect Core charge with AVEE

The increased attractive force from the nucleus makes it more difficult for outermost electrons to escape, thus increasing the orbital energy of the electrons, i.e., the AVEE. In other words, as we move from left to right across a period on the periodic table, the increased core charge pulls the electrons closer to the nucleus, thus increasing the AVEE.

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Most popular questions from this chapter

Describe the trend in EN moving down a group of the periodic table.

Use the shell model of atoms and the concept of core charge to explain why the AVEE of atoms generally decreases from top to bottom down a group.

a) There is one valence electron in a \(\mathrm{H}\) atom. What is the average ionization energy of the one valence electron in \(\mathrm{H}\) ? (Note that this is a very easy question because there is only one valence electron!) b) There are two valence electrons in a He atom. What is the average ionization energy of the two valence electrons in He? (Again, an easy question because both valence electrons have the same IE!) c) Which atom, \(\mathrm{H}\) or He, holds its valence electron(s) "more tightly" on average? Explain your reasoning.

In terms of AVEE, explain why Na is more likely to form \(\mathrm{Na}^{+}\) than \(\mathrm{O}\) is to form \(\mathrm{O}^{+}\)

Describe the trend in EN moving left to right across a period of the periodic table.
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