Textbook Question
Both vanadium and its 3+ ion are paramagnetic. Refer to their electron configurations to explain this statement.
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Ch.8 - Periodic Properties of the Elements
Chapter 8, Problem 99
Consider these elements: N, Mg, O, F, Al. a. Write the electron configuration for each element. b. Arrange the elements in order of decreasing atomic radius. c. Arrange the elements in order of increasing ionization energy. d. Use the electron configurations in part a to explain the differences between your answers to parts b and c.
Verified step by step guidance1
Step 1: Write the electron configuration for each element. For example, for Nitrogen (N), determine the number of electrons and fill the orbitals following the Aufbau principle.
Step 2: Arrange the elements in order of decreasing atomic radius. Consider the periodic trend that atomic radius decreases across a period and increases down a group.
Step 3: Arrange the elements in order of increasing ionization energy. Remember that ionization energy generally increases across a period and decreases down a group.
Step 4: Compare the electron configurations from part a to explain the differences in atomic radius. Consider the number of electron shells and the effective nuclear charge.
Step 5: Use the electron configurations to explain the differences in ionization energy. Consider the stability of the electron configuration and the energy required to remove an electron.
Related Practice
Open Question
Refer to their electron configurations to explain why copper is paramagnetic, whereas its 1+ ion is not.
Textbook Question
Life on Earth evolved based on the element carbon. Based on periodic properties, what two or three elements would you expect to be most like carbon?
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Open Question
Explain why atomic radius decreases as you move to the right across a period for main-group elements but not for transition elements.
Open Question
Explain why vanadium (radius = 134 pm) and copper (radius = 128 pm) have nearly identical atomic radii, even though the atomic number of copper is about 25% higher than that of vanadium. Predict the relative densities of these two metals. Look up the densities in a reference book, periodic table, or on the Internet to check if your predictions are correct.
Open Question
The lightest noble gases, such as helium and neon, are completely inert—they do not form any chemical compounds whatsoever. In contrast, the heavier noble gases do form a limited number of compounds. Explain this difference in terms of trends in fundamental periodic properties.