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Chapter 8: Problem 16

A neutral atom of a certain element has 17 electrons. Without consulting a periodic table, (a) write the ground-state electron configuration of the element, (b) classify the element, (c) determine whether the atoms of this element are diamagnetic or paramagnetic.

Short Answer

Expert verified
The ground-state electron configuration of the element with 17 electrons is \(1s^2, 2s^2, 2p^6, 3s^2, 3p^5\). The element belongs to p-block. It is paramagnetic because it contains one unpaired electron.

Step by step solution

01

Determining Electron Configuration

The task is to find the ground-state electron configuration for an atom with 17 electrons. Go through each energy level and fill them according to the Aufbau principle, until all 17 electrons are placed. The order of filling is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, etc. In this case, the ground state electron configuration is \(1s^2 2s^2 2p^6 3s^2 3p^5\).
02

Classify the Element

Argon is classified according to the periodic table's blocks. The last electron, number 17, is added to the p-block. Therefore, the element belongs to the p-block.
03

Determining Diamagnetic or Paramagnetic

An atom is diamagnetic if all of its electrons are paired in its ground state, and it is paramagnetic if it has at least one unpaired electron. In the case of this atom, where the electron configuration ends with 3p^5, it has one unpaired electron. Thus, it is paramagnetic.

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Most popular questions from this chapter

Use the second period of the periodic table as an example to show that the sizes of atoms decrease as we move from left to right. Explain the trend.

Write ground-state electron configurations for these ions, which play important roles in biochemical processes in our bodies: (a) \(\mathrm{Na}^{+},\) (b) \(\mathrm{Mg}^{2+},\) (c) \(\mathrm{Cl}^{-}\) (d) \(\mathrm{K}^{+},\) (e) \(\mathrm{Ca}^{2+},\) (f) \(\mathrm{Fe}^{2+},(\mathrm{g}) \mathrm{Cu}^{2+},\) (h) \(\mathrm{Zn}^{2+}\)

Acidic oxides are those that react with water to produce acid solutions, whereas the reactions of basic oxides with water produce basic solutions. Nonmetallic oxides are usually acidic, whereas those of metals are basic. Predict the products of the reactions of these oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}\), \(\mathrm{N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions.

The first and second ionization energies of \(\mathrm{K}\) are \(419 \mathrm{~kJ} / \mathrm{mol}\) and \(3052 \mathrm{~kJ} / \mathrm{mol}\), and those of \(\mathrm{Ca}\) are \(590 \mathrm{~kJ} / \mathrm{mol}\) and \(1145 \mathrm{~kJ} / \mathrm{mol}\), respectively. Compare their values and comment on the differences.

Which of these elements are metals, nonmetals, and metalloids: \(\mathrm{As}, \mathrm{Xe}, \mathrm{Fe}, \mathrm{Li}, \mathrm{B}, \mathrm{Cl}, \mathrm{Ba}, \mathrm{P}, \mathrm{I}, \mathrm{Si} ?\)
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