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Chapter 8: Problem 58

Write the full electron configuration of the Period 3 element with the following successive IEs (in \(\mathrm{kJ} / \mathrm{mol}\) ): \(\mathrm{IE}_{1}=738\) \(\mathrm{IE}_{2}=1450\) $$ \mathrm{IE}_{3}=7732 $$ \(\mathrm{IE}_{4}=10,539\) \(\mathrm{IE}_{5}=13,628\)

Short Answer

Expert verified
1s虏 2s虏 2p鈦� 3s虏

Step by step solution

01

- Identify the element based on ionization energies

The ionization energies are given: IE鈧� = 738 kJ/mol IE鈧� = 1450 kJ/mol IE鈧� = 7732 kJ/mol IE鈧� = 10,539 kJ/mol IE鈧� = 13,628 kJ/mol. Notice the significant increase between IE鈧� and IE鈧�. This indicates the removal of an electron from a stable, filled shell, suggesting that the element has 2 electrons in its outermost shell.
02

- Determine the Period and Group

Elements in Period 3 with two electrons in the outer shell belong to the second group of the periodic table, i.e., Group 2 (alkaline earth metals). The elements are: - Sodium (Na), - Magnesium (Mg), and - Aluminium (Al). Based on the ionization energy pattern, the significant jump after IE鈧� strongly indicates magnesium (Mg).
03

- Write the electron configuration

Magnesium (Mg) has an atomic number of 12. Therefore, its electron configuration can be written by filling up the orbitals in the order of their energy levels: 1s虏 2s虏 2p鈦� 3s虏.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electron Configuration
Electron configuration is the arrangement of electrons in an atom's orbitals. Each element has a unique configuration that determines its chemical properties. For magnesium, which has an atomic number of 12, its electron configuration is written by filling the orbitals in order of their energy levels. This follows the Aufbau principle, which states that electrons occupy the lowest energy orbitals first. Therefore, magnesium's configuration is 1s虏 2s虏 2p鈦� 3s虏. This means it has two electrons in the first shell, eight in the second, and two in the third.
Ionization Energy
Ionization energy is the energy required to remove an electron from an atom in the gas phase. Magnesium's successive ionization energies are given: IE鈧� = 738 kJ/mol, IE鈧� = 1450 kJ/mol, IE鈧� = 7732 kJ/mol, IE鈧� = 10,539 kJ/mol, and IE鈧� = 13,628 kJ/mol. Notice the significant increase between IE鈧� and IE鈧�. This large jump indicates the removal of an electron from a more stable, inner shell, confirming that magnesium has two outer electrons in its 3s orbital.
Periodic Table
The periodic table arranges chemical elements in order of increasing atomic number. Elements in the same column, or group, have similar properties. Magnesium is located in Period 3 and Group 2. It belongs to the alkaline earth metals, characterized by having two electrons in their outermost shell. This group includes elements like beryllium, calcium, and barium. The periodic table helps predict element properties and behaviors, such as ionization energies and electron configurations.
Atomic Structure
Atomic structure refers to the composition of an atom, which includes a nucleus (containing protons and neutrons) and surrounding electrons. Magnesium's atomic structure consists of 12 protons, 12 neutrons, and 12 electrons. The electrons are arranged in different energy levels or shells: two in the first shell, eight in the second, and two in the third. This structure explains magnesium's chemical behavior, such as its low ionization energy due to the relative ease of removing its two outermost electrons.

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Most popular questions from this chapter

Draw a partial (valence-level) orbital diagram, and write the condensed ground-state electron configuration for each: (a) Mn (b) \(P\) (c) Fe

Rank the ions in each set in order of increasing size, and explain your ranking: (a) \(\mathrm{Li}^{+}, \mathrm{K}^{+}, \mathrm{Na}^{+}\) (b) \(\mathrm{Se}^{2-}, \mathrm{Rb}^{+}, \mathrm{Br}^{-}\) (c) \(\mathrm{O}^{2-}, \mathrm{F}^{-}, \mathrm{N}^{3-}\)

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Write the full ground-state electron configuration for each: (a) Br (b) Mg (c) Se
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