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Chapter 7: Problem 112

Arrange the following groups of atoms in order of increasing size. a. Rb, Na, Be b. Sr, Se, Ne c. Fe, P, O

Short Answer

Expert verified
The order of increasing atomic size for each group is as follows: a. Be, Na, Rb b. Ne, Se, Sr c. O, P, Fe

Step by step solution

01

Locate the elements on the periodic table

Determine the location of Rb, Na, and Be on the periodic table. Rb (Rubidium) is in Group 1 and Period 5, Na (Sodium) is in Group 1 and Period 3, and Be (Beryllium) is in Group 2 and Period 2.
02

Apply periodic trends for atomic radius

Recall that atomic size increases going down a group and decreases across a period. Comparing Rb and Na, both in Group 1, Rb is further down the group, so it is larger. Be is in a higher group (Group 2) and a higher period (Period 2), so it is smaller than both Rb and Na.
03

Arrange in increasing order of size

Based on the analysis in Step 2, the order of increasing atomic size is: Be, Na, Rb. b. Sr, Se, Ne
04

Locate the elements on the periodic table

Determine the location of Sr, Se, and Ne on the periodic table. Sr (Strontium) is in Group 2 and Period 5, Se (Selenium) is in Group 16 and Period 4, and Ne (Neon) is in Group 18 and Period 2.
05

Apply periodic trends for atomic radius

Recall that atomic size increases going down a group and decreases across a period. Sr is further down the group and in a lower period compared to Se, so it is larger. Ne is further to the right (higher group number) and at a higher period compared to Se, so it is smaller.
06

Arrange in increasing order of size

Based on the analysis in Step 2, the order of increasing atomic size is: Ne, Se, Sr. c. Fe, P, O
07

Locate the elements on the periodic table

Determine the location of Fe, P, and O on the periodic table. Fe (Iron) is in Group 8 and Period 4, P (Phosphorus) is in Group 15 and Period 3, and O (Oxygen) is in Group 16 and Period 2.
08

Apply periodic trends for atomic radius

Recall that atomic size increases going down a group and decreases across a period. Comparing Fe and P, Fe is in a lower group (lower group number) and a higher period compared to P, so it is larger. Comparing P and O, P is further down the group and in a lower period compared to O, so it is larger.
09

Arrange in increasing order of size

Based on the analysis in Step 2, the order of increasing atomic size is: O, P, Fe.

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Most popular questions from this chapter

Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff using the spectroscope they invented in 1859. The name came from the Latin caesius (“sky blue”) because of the prominent blue line observed for this element at 455.5 nm. Calculate the frequency and energy of a photon of this light.

Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by \(n=1,\) by \(n=2\)

Identify the following elements. a. An excited state of this element has the electron configu- ration 1$s^{2} 2 s^{2} 2 p^{5} 3 s^{1}$ b. The ground-state electron configuration is [Ne \(] 3 s^{2} 3 p^{4}\) . c. An excited state of this element has the electron configu- ration \([\mathrm{Kr}] 5 s^{2} 4 d^{6} 5 p^{2} 6 s^{1}\) d. The ground-state electron configuration contains three unpaired 6\(p\) electrons.

For each of the following pairs of elements $$(\mathrm{C} \text { and } \mathrm{N}) \quad(\text { Ar and Br })$$ pick the atom with a. more favorable (exothermic) electron affinity. b. higher ionization energy. c. larger size.

Draw atomic orbital diagrams representing the ground-state electron configuration for each of the following elements. a. Na b. Co c. Kr How many unpaired electrons are present in each element?
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