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BRaymiller Assignment 22: Periodic Trends Part 2

Last updated 6 months ago
10 questions
When we study the trends in the periodic table, we cannot stop at just atomic size. In this section of the chapter, we will begin an understanding of an important concept, namely ionization energy and recognize its trend on the periodic table.

Lithium has an electron configuration of 1s22s1. Lithium has one electron in its outermost energy level. In order to remove this electron, energy must be added to the system. This energy is known as the ionization energy. The ionization energy is the energy required to remove the most loosely held electron from atom. The higher the value of the ionization energy, the harder it is to remove that electron.

We can see a trend when we look at the ionization energies for the elements in period 2. Look at the table below which shows the ionization energy for element in period 2.
1

In order to remove an electron from an atom, energy is....

1

According to the reading, what is the definition of ionization energy?

1

If an electron is tightly held in an atom, will it have a high or low ionization energy?

As we move across the period, the atoms become smaller which causes the nucleus to have greater attraction for the valence electrons. Therefore, the electrons are more difficult to remove.
1

Looking at the chart, what general trend do you notice with the ionization energy as you go across the periodic table? (Ignore Beryllium and Nitrogen which are exceptions)

1

Based on the information above, why do you notice the trend?

Similiar to how we can observe trends regarding periods on the periodic table, we can also see trends that exist in terms of ionization energy within groups on the periodic table. Look at the table below which shows trends in terms of group 1 on the periodic table.
Comparing the electron configurations of lithium to potassium, we know that the electron to be removed is further away from the nucleus. We know this because the energy level where the valence electron is held is larger. Therefore it is easier to remove the most loosely held electron because the atom is larger and the electrons are getting pulled less by the protons in the nucleus.
1

What trend do you notice regarding ionization energy on the periodic table?

1

Based on the information above, why does this trend exist?

1
In summary, as you go across the periodic table to the right, the ionization energy _______. As you go down the periodic table, the ionization energy _______.
1

Which of the following will have a higher ionization energy: Te or I?

1

Which of the following will have a higher ionization energy: Se or Te?