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Chapter 3: Problem 107

Magnesium has a higher first ionization energy than sodium, consistent with the periodic trend for first ionization energies. Postulate a reason why Mg has the higher first ionization energy.

Short Answer

Expert verified
Magnesium has a higher first ionization energy compared to sodium due to its position in the periodic table and its electronic configuration. As magnesium is to the right of sodium in the same period, it experiences a higher effective nuclear charge, holding its electrons more tightly. Consequently, more energy is needed to remove the first electron from magnesium than for sodium.

Step by step solution

01

Understand Ionization Energy

Ionization energy is the amount of energy required to remove an electron from a neutral atom in its gaseous state. The first ionization energy refers to the energy needed to remove the first (outermost) electron.
02

Analyze the Electronic Configurations of Sodium and Magnesium

Sodium (Na): Atomic number = 11, Electronic configuration = 1s² 2s² 2p⁶ 3s¹ Magnesium (Mg): Atomic number = 12, Electronic configuration = 1s² 2s² 2p⁶ 3s²
03

Understand the Periodic Trend for Ionization Energy

As we move from left to right across a period in the periodic table, the ionization energy generally increases. This is because of an increasing effective nuclear charge, which results from increasing protons in the nucleus attracting the electrons more strongly. As a result, more energy is required to remove electrons from atoms with greater effective nuclear charges.
04

Compare Sodium and Magnesium

Since magnesium is to the right of sodium in the same period (Period 3), magnesium should experience a higher effective nuclear charge. This means that it should have a higher first ionization energy.
05

Postulate a Reason for the Higher Ionization Energy of Magnesium

The reason for the higher first ionization energy of magnesium compared to sodium can be attributed to their positions in the periodic table as well as their electronic configurations. Magnesium, with an additional proton in its nucleus compared to sodium, experiences a higher effective nuclear charge, which results in it holding its electrons more tightly. As a result, it takes more energy to remove the first electron from magnesium than it does for sodium.

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Most popular questions from this chapter

Name and give symbols for five of the transition metals.

While an atom's mass number and its atomic mass are not the same, they are often quite close to one another. Consider the following: Uranium- 235 has an atomic mass of \(235.04393\) amu and a percent abundance of \(0.73 \%\). Uranium-238 has an atomic mass of \(238.0508\) amu and a percent abundance of \(99.27 \%\). Without doing any calculations or consulting any other sources, which of the following do you think represents the atomic mass of naturally occurring uranium? (a) \(234.04 \mathrm{amu}\) (b) \(236.03 \mathrm{amu}\) (c) \(237.03\) amu (d) \(238.03\) amu (e) \(238.07\) amu Explain how you made your choice.

It always takes energy to remove an electron from a neutral atom. Explain why, and name the minimum amount of energy it takes to do this.

Give the names associated with groups IA (1), IIA (2), VIA (16), VIIA (17), and VIIIA (18).

Although not discussed until the next chapter, what process do you think chemists mean by an atom's second ionization energy?
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