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Chapter 5: Problem 18

Within our model and referring to the Coulombic Potential Energy expression, explain why the IE increases from left to right across a row of the periodic table.

Short Answer

Expert verified
Ionization energy increases from left to right across a row of the periodic table because, as the atomic number increases in a period, the nuclear charge also increases and the atomic radius decreases. This stronger attraction between nucleus and electron requires more energy to remove an electron, making the ionization energy higher. This fact is reflected in the Coulombic Potential Energy equation, where a larger charge and a smaller distance lead to higher energy.

Step by step solution

01

Understanding atomic structure

In a neutral atom, the number of electrons equal the atomic number. Going from left to right in a period of the periodic table, the atomic number increases, meaning that there are more electrons and protons in an atom. More protons mean a stronger nuclear charge, attracting the layer of electrons more strongly thereby reducing the atomic radius.
02

Applying the Coulombic potential energy

The decrease in atomic radius and the increase in nuclear charge going from left to right in a period both cause the energy required to remove an electron, also known as the ionization energy, to increase. The equation of Coulombic Potential Energy, \(U = k*Q1*Q2/d\), perfectly describes this phenomenon. Here, 'Q1' and 'Q2' are the charges of a nucleus and an electron, and 'd' is the distance between them. Given that 'Q1' increases and 'd' decreases, the energy 'U' will increase.
03

Summary

So, as we move from left to right across a period, the number of protons in the atom increases, which increases the positive charge of the nucleus and attracts the electrons more strongly. This stronger attraction (higher nuclear charge and smaller radius) means that more energy is required to remove an electron, thus the ionization energy increases.

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Most popular questions from this chapter

Locate \(\mathrm{F}\) and \(\mathrm{Cl}\) on the periodic table. a) Describe any relationship between the core charge of these atoms, the number of valence electrons, and their position in the periodic table. b) Describe any relationship between the valence shell of these atoms and their position in the periodic table. c) Within our model and referring to the Coulombic Potential Energy expression, explain why the \(\mathrm{IE}_{1}\) of \(\mathrm{Cl}\) is less than that of \(\mathrm{F}\).

How does the core charge on the neutral atom change as we move from left to right across a row (period) of the periodic table?

a) How many electrons are in the valence shell of \(\mathrm{H}\) ? Of He? Of Li? b) How many inner shell (core) electrons does H have? He? Li? c) What is the core charge of \(\mathrm{H}\) ? Of He? Of \(\mathrm{Li}\) ?

How does the core charge for Na compare to the core charge for Li?

a) Why is the nuclear charge of Be "+4"? b) How many inner shell (core) electrons does Be have? c) How many valence electrons does Be have? d) Show how the core charge for Be was calculated. e) What is the relationship between the number of valence electrons and the core charge of a neutral atom?
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