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Chapter 9: Problem 32

Compare the elements \(\mathrm{Na}, \mathrm{Mg}, \mathrm{O},\) and \(\mathrm{P}.\) (a) Place the elements in order of increasing ionization energy. (b) Place the elements in order of increasing electron affinity.

Short Answer

Expert verified
The elements in order of increasing ionization energy are: Na, Mg, P, O. The elements in order of increasing electron affinity are: Na, Mg, P, O.

Step by step solution

01

Understanding Periodic Table Trends

The positioning of elements in the periodic table profoundly affects their ionization energy and electron affinity. In general, as you move across a period (left to right), the ionization energy and electron affinity increases. This occurs because the number of protons in the nucleus increases, attracting the electrons more strongly and making it harder to remove an electron (higher ionization energy) and easier to accept an electron (higher electron affinity). But as you move down a group (top to bottom), both ionization energy and electron affinity decrease due to increases in atomic radius and electron shielding.
02

Ordering Elements by Increasing Ionization Energy

Arrange the elements in order of increasing atomic number: Na, Mg, O, P. Using the rule that ionization energy increases as you move from left to right across a period and from bottom to top in a group, the following sequence from lowest to highest ionization energy would be Na < Mg < P < O.
03

Ordering Elements by Increasing Electron Affinity

Again using the atomic number, the elements are arranged as follows: Na, Mg, O, and P. As noted, electron affinity typically increases as you move from left to right across a period. However, it's important to note that in some cases there can be exceptions. Therefore, using general trends, the expected sequence from lowest to highest electron affinity would be Na < Mg < P < O.

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Most popular questions from this chapter

Two elements, \(A\) and \(B\), have the electron configurations shown. $$ \mathrm{A}=\left[\begin{array}{ll} \mathrm{Ar} & 4 s^{1} \end{array} \quad \mathrm{B}=\left[\begin{array}{l} \mathrm{Ar} \end{array}\right] 3 d^{10} 4 \mathrm{s}^{2} 4 p^{3}\right. $$ (a) Which element is a metal? (b) Which element has the greater ionization energy? (c) Which element has the larger atomic radius? (d) Which element has the greater electron affinity?

For each of the following pairs, indicate the atom that has the larger size: (a) Te or Br; (b) \(\mathrm{K}\) or \(\mathrm{Ca} ;\) (c) Ca or Cs; (d) \(\mathrm{N}\) or \(\mathrm{O} ;\) (e) \(\mathrm{O}\) or \(\mathrm{P} ;\) (f) \(\mathrm{Al}\) or \(\mathrm{Au}.\)

How much energy, in kilojoules, is required to remove all the third-shell electrons in a mole of gaseous silicon atoms?

Among the following ions, several pairs are isoelectronic. Identify these pairs. \(\mathrm{Fe}^{2+}, \mathrm{Sc}^{3+}, \mathrm{Ca}^{2+}, \mathrm{F}^{-}\) \(\mathrm{Co}^{2+}, \mathrm{Co}^{3+}, \mathrm{Sr}^{2+}, \mathrm{Cu}^{+}, \mathrm{Zn}^{2+}, \mathrm{Al}^{3+}.\)

Must all atoms with an odd atomic number be paramagnetic? Must all atoms with an even atomic number be diamagnetic? Explain.
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