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Chapter 8: Problem 38

Arrange the following atoms in order of decreasing atomic radius: \(\mathrm{Na}, \mathrm{Al}, \mathrm{P}, \mathrm{Cl}, \mathrm{Mg}\).

Short Answer

Expert verified
The atoms in order of decreasing atomic radius are Na, Mg, Al, P, Cl.

Step by step solution

01

Identify location of elements on the periodic table

First, locate each atom on the periodic table. Sodium (Na) and Magnesium (Mg) are in the third period while Aluminum (Al), Phosphorous (P), and Chlorine (Cl) are in the fourth period.
02

Apply periodic trends to arrange atoms

Next, apply the periodic trends to these elements. On moving from left to right across a period, atomic size decreases. Therefore, among Na, Mg, and Al, Na has the largest atomic radius, followed by Mg and Al. Similarly, in the 2nd group (Na and Mg), atomic radius increases down the group, so Na has a larger atomic radius than Mg.
03

Finalize order of atomic radii

Finally, put together the atomic radii in decreasing order. Starting from the atom with the largest atomic radius to the smallest, the order is: Na, Mg, Al, P, Cl

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Most popular questions from this chapter

What is Moseley's contribution to the modern periodic table?

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

On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of these pairs: (a) \(\mathrm{Na}, \mathrm{Cs} ;\) (b) Be, \(\mathrm{Ba}\); (c) \(\mathrm{N}, \mathrm{Sb}\) (d) \(\mathrm{F}, \mathrm{Br},(\mathrm{e}) \mathrm{Ne}, \mathrm{Xe}\)

Without referring to a periodic table, write the electron configurations of elements with these atomic numbers: (a) \(9,\) (b) \(20,\) (c) \(26,\) (d) 33. Classify the elements.
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