Using only the periodic table, predict the most stable ion for Na, Mg, Al, S, Cl, K, Ca, and Ga. Arrange these from largest to smallest radius, and explain why the radius varies as it does. Compare your predictions with figure 3-5. **Figure 3-5:** Sizes of ions related to positions of the elements on the periodic table. Note that size generally increases down a group. Also note that in a series of isoelectronic ions, size decreases with increasing atomic number. The ionic radii are given in units of picometers.**Diagram Explanation:**The diagram shows various ions with their ionic radii represented in picometers.- **Group 1 Ions:** - Li⁺: 60 pm - Na⁺: 95 pm - K⁺: 133 pm - Rb⁺: 148 pm- **Group 2 Ions:** - Be²⁺: 31 pm - Mg²⁺: 65 pm - Ca²⁺: 99 pm - Sr²⁺: 113 pm- **Group 13 and Group 14 Ions:** - Al³⁺: 50 pm - Ga³⁺: 62 pm - In³⁺: 81 pm - Sn⁴⁺: 71 pm - Sb⁵⁺: 62 pm- **Chalcogenides and Halides:** - O²⁻: 140 pm - F⁻: 136 pm - S²⁻: 184 pm - Cl⁻: 181 pm - Se²⁻: 198 pm - Br⁻: 195 pm - Te²⁻: 221 pm - I⁻: 216 pm**Isoelectronic Series:** For isoelectronic ions, size decreases as the nuclear charge (Z) increases.**Critical Thinking:** Ions have different radii than their parent atoms. What if ions stayed the same size as their parent atoms? How would this affect ionic bonding in compounds?**Interactive Example 3-2: Relative Ion Size I**Arrange the ions Se²⁻, Br⁻, Rb⁺, and Sr²⁺ in order of decreasing size.**Solution:**This is an isoelectronic series of ions with the krypton electron configuration. Since these ions all have the same number of electrons, their sizes will depend on the nuclear charge. The Z values are 34 for Se

The explanation is given below-

Using only the periodic table, predict the most stable ion for Na, Mg, Al, S, Cl, K, Ca, and Ga. Arrange these from largest to smallest radius, and explain why the radius varies as it does. Compare your predictions with figure 3-5.

Using only the periodic table, predict the most stable ion for Na, Mg, Al, S, Cl, K, Ca, and Ga. Arrange these from largest to smallest radius, and explain why the radius varies as it does. Compare your predictions with figure 3-5.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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