Phosphorus has a ionization energy than magnesium because . (LO 6.5, 6.6) (a) larger; the electron in phosphorus is in a higher n level than the electron in magnesium (b) larger; the electron in phosphorus has a higher Zeff than the electron in magnesium (c) smaller; the electron in phosphorus is in a lower n level than the electron in magnesium (d) smaller; the electron in phosphorus has a lower Zeff than the electron in magnesium

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

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Step 1: Understand the concept of ionization energy, which is the energy required to remove an electron from an atom in the gaseous state.

Step 2: Recall that effective nuclear charge (Zeff) is the net positive charge experienced by an electron in a multi-electron atom, influencing ionization energy.

Step 3: Consider the periodic trends: Ionization energy generally increases across a period from left to right due to increasing Zeff and decreases down a group due to increasing atomic size.

Step 4: Compare the positions of phosphorus and magnesium on the periodic table. Phosphorus is to the right of magnesium in the same period, suggesting a higher Zeff for phosphorus.

Step 5: Evaluate the options: Since phosphorus has a higher Zeff than magnesium, it will have a larger ionization energy, making option (b) the correct choice.

Concetti chiave

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Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It generally increases across a period due to increasing nuclear charge, which attracts electrons more strongly, and decreases down a group as electrons are added to higher energy levels, which are further from the nucleus.

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01:19

Ionization Energy

Effective Nuclear Charge (Zeff)

Effective nuclear charge (Zeff) is the net positive charge experienced by an electron in a multi-electron atom. It accounts for the shielding effect of inner electrons, meaning that outer electrons feel a reduced attraction to the nucleus. A higher Zeff leads to a stronger attraction between the nucleus and the outer electrons, resulting in higher ionization energy.

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01:51

Effective Nuclear Charge

Principal Quantum Number (n)

The principal quantum number (n) indicates the main energy level occupied by an electron in an atom. As n increases, the electron is located further from the nucleus, which generally results in a weaker attraction to the nucleus and lower ionization energy. Thus, electrons in higher n levels are easier to remove compared to those in lower n levels.

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