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Chapter 7: Problem 105

Arrange the following groups of atoms in order of increasing size. a. \(\mathrm{Te}, \mathrm{S}, \mathrm{Se}\) b. \(\mathrm{K}, \mathrm{Br}, \mathrm{Ni}\) c. \(\mathrm{Ba}, \mathrm{Si}, \mathrm{F}\)

Short Answer

Expert verified
Arrange the groups of atoms in order of increasing size as follows: a. \(\mathrm{S}, \mathrm{Se}, \mathrm{Te}\) b. \(\mathrm{Br}, \mathrm{Ni}, \mathrm{K}\) c. \(\mathrm{F}, \mathrm{Si}, \mathrm{Ba}\)

Step by step solution

01

a. Arrange \(\mathrm{Te}, \mathrm{S}, \mathrm{Se}\) in order of increasing size

We can find these elements in the same group (Group 16) of the periodic table. Since atomic size increases from top to bottom in a group, we can arrange them in the order of their position in the periodic table: S < Se < Te So the order of increasing size for these atoms is \(\mathrm{S}, \mathrm{Se}, \mathrm{Te}\).
02

b. Arrange \(\mathrm{K}, \mathrm{Br}, \mathrm{Ni}\) in order of increasing size

These elements belong to different groups but they are in the same period (Period 4). Since atomic size decreases from left to right in a period, we can arrange them in the order of their position in the periodic table: K > Ni > Br So the order of increasing size for these atoms is \(\mathrm{Br}, \mathrm{Ni}, \mathrm{K}\).
03

c. Arrange \(\mathrm{Ba}, \mathrm{Si}, \mathrm{F}\) in order of increasing size

These elements are neither in the same group nor in the same period. Therefore, we have to use both the group and period trends to determine their order. Ba is in Group 2 and Period 6. Si is in Group 14 and Period 3. F is in Group 17 and Period 2. Comparing Ba and Si: Ba has more energy levels than Si since it is below Si in the periodic table. Thus, Ba has a larger atomic size than Si. Comparing Si and F: Si is left of F in the periodic table within Period 3. Thus, Si has a larger atomic size than F. From the above comparisons, the order of increasing size for these atoms is \(\mathrm{F}, \mathrm{Si}, \mathrm{Ba}\).

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Most popular questions from this chapter

Which of the following statements is(are) true? a. \(\mathrm{F}\) has a larger first ionization energy than does \(\mathrm{Li}\). b. Cations are larger than their parent atoms. c. The removal of the first electron from a lithium atom (electron configuration is \(1 s^{2} 2 s^{1}\) ) is exothermic - that is, removing this electron gives off energy. d. The He atom is larger than the \(\mathrm{H}^{+}\) ion. e. The \(\mathrm{Al}\) atom is smaller than the \(\mathrm{Li}\) atom.

Which of elements \(1-36\) have one unpaired electron in the ground state?

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Microwave radiation has a wavelength on the order of \(1.0 \mathrm{~cm}\). Calculate the frequency and the energy of a single photon of this radiation. Calculate the energy of an Avogadro's number of photons (called an einstein) of this radiation.

The elements \(\mathrm{Si}, \mathrm{Ga}\), As, \(\mathrm{Ge}, \mathrm{Al}, \mathrm{Cd}, \mathrm{S}\), and Se are all used in the manufacture of various semiconductor devices. Write the expected electron configuration for these atoms.
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