Trends in Ionization Energy

Which would be harder to separate: the two spheres in Diagram A or the two spheres in Diagram B? Why?

• The spheres in diagam A would be harder to separate because the force of attraction is less due to the lower charge difference (+3 and -3) and also the spheres are further apart which makes them harder to separate just like magnets that are further apart.

• The spheres in Diagram B would be harder to separate because the force of attraction is greater due to the higher charge difference (+4 and -4) and also the spheres are closer together which makes them harder to separate just like magnets that are very close together.

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Draw Bohr diagrams of the following atoms: lithium, nitrogen and fluorine.

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For each of the atoms in question two compare the attraction between the nucleus and the outer level of electrons. Which atom has the strongest attraction between the nucleus and outer electrons?

• Fluorine has the strongest attraction. A +7 force from the nucleus is attracting the outer energy level.

• Nitrogen has the strongest attraction. A +5 force from the nucleus is attracting the outer energy level.

• Lithium has the strongest force. A +1 force from the nucleus is attracting the outer energy level.

• Fluorine has the strongest attraction. A +9 force from the nucleus is attracting the outer energy level.

• Nitrogen has the strongest attraction. A +7 force from the nucleus is attracting the outer energy level.

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Which would be more difficult: if you wanted to remove an electron from an atom of fluorine or from an atom of nitrogen?

• It would take more energy to remove an outer electron from an atom of fluorine than from nitrogen. The outer electron from fluorine feels a stronger force from the nucleus.

• It would take more energy to remove an outer electron from an atom of nitrogen than from fluorine. The outer electron from nitrogen feels a stronger force from the nucleus.

• It would take more energy to remove an outer electron from an atom of fluorine than from nitrogen. This is because fluorine has a larger atomic radius.

• It would take more energy to remove an outer electron from an atom of nitrogen than from fluorine. This is because nitrogen has a larger atomic radius.

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Would it be easier to remove an electron from lithium or nitrogen?

• It would be easier to remove an outer electron from lithium because lithium's outer electron experiences a weaker force of attraction from the nucleus.

• It would be easier to remove an outer electron from nitrogen because nitrogen's outer electron experiences a weaker force of attraction from the nucleus.

• It would be easier to remove an outer electron from lithium because lithium has a smaller atomic radius.

• It would be easier to remove an outer electron from nitrogen because nitrogen has a smaller atomic radius.

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Which would have a higher first ionization energy: phosphorus or aluminum? (You may want to draw a Bohr diagram to help you determine the answer.)

• Phosphorus because it has a higher attraction (+5) between the nucleus and outer electrons than aluminum (+3).

• Phosphorus because it has a higher attraction (+3) between the nucleus and outer electrons than aluminum (+5).

• Aluminum because it has a higher attraction (+5) between the nucleus and outer electrons than phosphorus (+3).

• Aluminum because it has a higher attraction (+3) between the nucleus and outer electrons than phosphorus (+5).

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Phosphorus and aluminum are in the same row of the periodic table. Lithium, nitrogen, and fluorine are also in the same row. Using your answers to questions 3, 4, and 6 what do you notice about the ionization energy of elements proceeding from left to right across a row of the periodic table? Does the ionization energy increase or decrease as you go across a period?

As you move from ​left to right across a row (or period), the ionization energy ​ (a)   .

• increases
• decreases
• stays the same

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This trend exists because as you move from left to right across a row, the attraction between the nucleus and ​ (a)   electrons also ​ (b)   . For atoms with a ​ (c)   attraction for the outer electrons, it requires ​ (d)   ionization energy to remove the electron.

• outer
• increases
• stronger
• more
• inner
• decreases
• weaker

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Consider this Bohr diagram of sodium. Do you expect the first ionization energy to be high or low for sodium?

• Sodium has a low first ionization energy because of the low attraction from the nucleus (+1) for the electron in the third energy level.

• Sodium has a high first ionization energy because of the low attraction from the nucleus (+1) for the electron in the third energy level.

• Sodium has a high first ionization energy because of the high attraction from the nucleus (+1) for the electron in the third energy level.

• Sodium has a low first ionization energy because of the high attraction from the nucleus (+1) for the electron in the third energy level.

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The second ionization energy of all elements is higher than the first ionization energy, but in sodium the second ionization energy is extra large. Considering the structure of the sodium atom explain why this might be. (HINT: after one electron is removed, what is sodium’s electron arrangement like?).

• After the first electron is removed, sodium has only core electrons left. It is very difficult to remove core electrons as they are much closer to the nucleus.

• After the first electron is removed, sodium has only core electrons left. It is very easy to remove core electrons as they are much closer to the nucleus.

• After the first electron is removed, sodium has only core electrons left. It is very easy to remove core electrons as they are much further away from the nucleus.

• After the first electron is removed, sodium has only core electrons left. It is very difficult to remove core electrons as they are much further away from the nucleus.

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