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Chapter 8: Problem 72

Which oxide is more basic, \(\mathrm{MgO}\) or \(\mathrm{BaO}\) ? Why?

Short Answer

Expert verified
\(\mathrm{BaO}\) is more basic than \(\mathrm{MgO}\) because \(\mathrm{Ba}\) is lower in Group 2 of the Periodic Table, and the basicity (a part of metallic character) increases as you move down a group.

Step by step solution

01

Identifying the element's group and period on the Periodic Table

Both \(\mathrm{Mg (Magnesium)}\) and \(\mathrm{Ba (Barium)}\) are in Group 2 (alkaline earth metals) on the Periodic Table. \(\mathrm{Mg}\) is in Period 3, and \(\mathrm{Ba}\) is in Period 6.
02

Understanding Trends in the Periodic Table

Down a Group in the Periodic Table, the metallic character (including basicity) increases. This is due to the increase in atomic size and the ability to lose electrons (which forms the basis for basicity: the ability to donate electrons to other reactions), as the electrons are less tightly held by the nucleus.
03

Comparing the Basicity of MgO and BaO

Since \(\mathrm{Ba}\) is below \(\mathrm{Mg}\) in Group 2 of the Periodic Table and the metallic character increases down a group, \(\mathrm{BaO (Barium Oxide)}\) is more basic than \(\mathrm{MgO (Magnesium Oxide)}\).

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Most popular questions from this chapter

Give the physical states (gas, liquid, or solid) of the representative elements in the fourth period at 1 atm and \(25^{\circ} \mathrm{C}: \mathrm{K}, \mathrm{Ca}, \mathrm{Ga}, \mathrm{Ge}, \mathrm{As}, \mathrm{Se}, \mathrm{Br}\).

Explain why, for isoelectronic ions, the anions are larger than the cations.

Based on your knowledge of the chemistry of the alkali metals, predict some of the chemical properties of francium, the last member of the group.

What do we mean when we say that two ions or an atom and an ion are isoelectronic?

Why is the radius of the lithium atom considerably larger than the radius of the hydrogen atom?
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