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Chapter 7: Problem 26

Using only the periodic table, arrange each set of atoms in (b) \(\mathrm{Sn}, \mathrm{Sb}, \mathrm{As} ;(\mathbf{c}) \mathrm{Al},\) order of increasing radius: (a) \(\mathrm{Ba}, \mathrm{Ca}, \mathrm{Na} ;\) Be, Si.

Short Answer

Expert verified
The order of increasing atomic radius for each set is: (a) Na < Ca < Ba; (b) As < Sb < Sn; (c) Be < Si < Al.

Step by step solution

01

Set (a): Arrange Ba, Ca, Na

To arrange Ba, Ca, and Na in order of increasing atomic radius, we look at their positions on the periodic table. Ba(Barium) is in Group 2 and Period 6, Ca(Calcium) is in Group 2 and Period 4, and Na(Sodium) is in Group 1 and Period 3. Since atomic radius increases down a group and decreases across a period, the order of increasing atomic radius will be: Na < Ca < Ba.
02

Set (b): Arrange Sn, Sb, As

To arrange Sn, Sb, and As in order of increasing atomic radius, we look at their positions on the periodic table. Sn(Tin) is in Group 14 and Period 5, Sb(Antimony) is in Group 15 and Period 5, and As(Arsenic) is in Group 15 and Period 4. Since atomic radius increases down a group and decreases across a period, the order of increasing atomic radius will be: As < Sb < Sn.
03

Set (c): Arrange Al, Be, Si

To arrange Al, Be, and Si in order of increasing atomic radius, we look at their positions on the periodic table. Al(Aluminium) is in Group 13 and Period 3, Be(Beryllium) is in Group 2 and Period 2, and Si(Silicon) is in Group 14 and Period 3. Since atomic radius increases down a group and decreases across a period, the order of increasing atomic radius will be: Be < Si < Al.

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Key Concepts

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

Atomic Radius
The atomic radius refers to the size of an atom, specifically the distance from the atom's nucleus to the outermost boundary of its electron cloud. It can be tricky to measure directly, as atoms aren't solid spheres, but chemists often determine it by looking at distances between atoms in a compound.
Understanding atomic radius is crucial because it influences an atom's reactivity, its ability to bond with other atoms, and even the general properties of the elements in its group. As we move down a group in the periodic table, the atomic radius increases. This is because new electron shells are added, making the atoms larger.
Conversely, as we move across a period from left to right, the atomic radius decreases. Even though electrons are added to the same shell, the increasing nuclear charge pulls electrons closer, shrinking the atomic radius slightly.
Group and Period Trends
Group and period trends are essential frameworks that help us predict the behavior of elements in the periodic table. Let's break it down for better understanding:
  • Groups: The vertical columns of the periodic table. Elements in the same group share similar properties, primarily due to their similar valence electron configurations. As you move down a group, the atomic radius increases because each row adds a new electron shell.
  • Periods: The horizontal rows in the periodic table. As you move across a period from left to right, a few things occur, including a decrease in atomic radius. This happens because even though electrons are being added to the same electron shell, the increasing positive charge from the protons in the nucleus pulls them closer together.
Combined, these trends help us understand why certain elements behave similarly and allow us to predict their atomic radii and other properties based on their position in the periodic table.
Element Arrangement
Arranging elements based on atomic radius is a tangible application of the principles of the periodic table. By simply looking at their positions, we can predict which atoms are larger or smaller.
For instance, atoms like barium ( Ba ), calcium ( Ca ), and sodium ( Na ) can be arranged in order of increasing atomic radius because they belong to different periods and groups with predictable trends. Sodium, being in a higher period, has a smaller overlapping of electron clouds compared to barium.
Similarly, elements like tin ( Sn ), antimony ( Sb ), and arsenic ( As ) can also be arranged by noting their positions. In general, moving down groups and across periods helps us establish a natural order of atomic radii, demonstrating how the periodic table is a tool not just for cataloging elements but for understanding and predicting their chemistry.

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Most popular questions from this chapter

Explain the following variations in atomic or ionic radii: (a) \(\Gamma>\mathrm{I}>\mathrm{I}^{+},(\mathrm{b}) \mathrm{Ca}^{2+}>\mathrm{Mg}^{2+}>\mathrm{Be}^{2+}\) (c) \(\mathrm{Fe}>\mathrm{Fe}^{2+}>\mathrm{Fe}^{3+}\)

It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measure how well electricity is conducted by each of the elements to determine how "metallic" the elements are. On the basis of conductivity, there is not much of a trend in the periodic table: Silver is the most conductive metal, and manganese the least. Look up the first ionization energies of silver and manganese; which of these two elements would you call more metallic based on the way we define it in this book?

We can draw an analogy between the attraction of an electron to a nucleus and seeing a lightbulb -in essence, the more \(n u=\) clear charge the electron "sees," the greater the attraction. (a) Within this analogy, discuss how the screening by core electrons is analogous to putting a frosted-glass lampshade between the lightbulb and your eyes, as shown in the illustration. (b) Explain how we could mimic moving to the right in a row of the periodic table by changing the wattage of the lightbulb. (c) How would you change the wattage of the bulb and/or the frosted glass to mimic the effect of moving down a column of the periodic table? [Section 7.2]

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist, explain why. (b) \(\mathrm{Sc}^{3+}\) (d) \(\mathrm{Zn}^{2+},(\mathrm{e}) \mathrm{Sn}^{4+}\) (a) \(\mathrm{Cl}\) (c) \(\mathrm{Fe}^{2+}\)

(a) One of the alkali metals reacts with oxygen to form a solid white substance. When this substance is dissolved in water, the solution gives a positive test for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\). When the solution is tested in a burner flame, a lilac-purple flame is produced. What is the likely identity of the metal? (b) Write a balanced chemical equation for reaction of the white substance with water.
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