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

Short Answer

Expert verified
BaO is more basic than MgO because barium is lower in Group 2 of the periodic table than magnesium.

Step by step solution

01

Review Chemical Elements

Look up Magnesium (Mg) and Barium (Ba) in the periodic table. Magnesium is in Group 2, Period 3, whereas Barium is also in Group 2 but in Period 6.
02

Relationship between basicity and position

Knowing that the basicity of the oxides usually increases down a group in the periodic table, identify which element is lower.
03

Identify the more basic oxide

Since Barium (Ba) is lower in the group than Magnesium (Mg), BaO is likely to be more basic than MgO.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Periodic Table Trends
Understanding the periodic table trends is crucial in predicting how different elements will behave in various chemical scenarios. When we look closely at the periodic table, one notable trend is the change in properties of elements as you move down a group. The group number designates columns within the periodic table and represents elements that have the same number of valence electrons, hence showing similar chemical behavior.

Within a given group, as we move from top to bottom, the atomic size increases. This is due to an increase in the number of electron shells as you go down in the group. The larger the atomic size, the lesser the nuclear attraction on the valence electrons, making them easier to lose and thus increasing the element's metallic character. Since more metallic elements tend to form more basic oxides, we can infer a relationship between the position in a group and the basicity of the oxides formed. This trend of increasing basicity going down a group is what students often remember as the 'metallic trend' and plays a key role in predicting and comparing the basicity of oxides.
Chemical Properties
The chemical properties of an element are deeply intertwined with its atomic structure. Elements within the same group in the periodic table tend to exhibit similar chemical properties because they have the same number of electrons in their outermost shell - their valence electrons. These electrons are important as they participate in chemical bonds.For metal oxides, such as those of magnesium (MgO) and barium (BaO), the chemical properties are influenced by their respective metals' ability to donate these electrons. The more readily an atom can lose its electrons to form a positive ion, the more basic its oxide will be. Naturally, as you move further down a group in the periodic table, the atoms get larger and the outermost electrons are more shielded by the inner layers of electrons from the nucleus, making them easier to remove. This results in increasingly basic oxides. Hence, identifying the chemical properties of elements, like ionization energy and electron affinity, are important in understanding why certain oxides are more basic than others.
Oxide Basicity Comparison
When we compare the basicity of oxides, especially those within the same group, it is essential to look at the elements from which the oxides are formed. The basic exercise here gave us a comparison between MgO and BaO, where we apply our understanding of periodic trends and chemical properties. From our trend analysis, we expect the oxide of the metal that is lower in the group to be more basic.

This is perfectly illustrated in the case of magnesium oxide and barium oxide. Since barium is further down Group 2 than magnesium, its atomic radius is larger, and it is more metallic. This means Barium tends to lose its valence electrons more easily compared to Magnesium, favoring the creation of a stronger, more stable base upon reacting with water. Therefore, BaO is correctly identified as the more basic oxide, consistent with the periodic trend of basicity increasing down a group. This knowledge, when applied, enables us to predict the relative acidity or basicity of a wide range of oxides and is an invaluable tool for students studying chemistry.

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Most popular questions from this chapter

Arrange the following species in isoelectronic pairs: \(\mathrm{O}^{+}, \mathrm{Ar}, \mathrm{S}^{2-}, \mathrm{Ne}, \mathrm{Zn}, \mathrm{Cs}^{+}, \mathrm{N}^{3-}, \mathrm{As}^{3+}, \mathrm{N}, \mathrm{Xe}\)

As discussed in the chapter, the atomic mass of argon is greater than that of potassium. This observation created a problem in the early development of the periodic table because it meant that argon should be placed after potassium. (a) How was this difficulty resolved? (b) From the following data, calculate the average atomic masses of argon and potassium: Ar-36 (35.9675 amu; 0.337 percent), \(\begin{array}{lll}\text { Ar- } 38 & (37.9627 & \text { amu } ; & 0.063 \text { percent), } & \text { Ar-40 }\end{array}\) \((39.9624 \mathrm{amu} ; 99.60\) percent \() ; \mathrm{K}-39(38.9637 \mathrm{amu} ;\) 93.258 percent \(,\) K- 40 ( 39.9640 amu; 0.0117 percent), K-41 \((40.9618\) amu; 6.730 percent).

Arsenic (As) is not an essential element for the human body. (a) Based on its position in the periodic table, suggest a reason for its toxicity. (b) When arsenic enters a person's body, it quickly shows up in the follicle of the growing hair. This action has enabled detectives to solve many murder mysteries by analyzing a victim's hair. Where else might one look for the accumulation of the element if arsenic poisoning is suspected?

Both \(\mathrm{Mg}^{2+}\) and \(\mathrm{Ca}^{2+}\) are important biological ions. One of their functions is to bind to the phosphate groups of ATP molecules or amino acids of proteins. For Group 2 A metals in general, the tendency for binding to the anions increases in the order \(\mathrm{Ba}^{2+}\) \(<\mathrm{Sr}^{2+}<\mathrm{Ca}^{2+}<\mathrm{Mg}^{2+} .\) Explain the trend.

State whether each of the following elements is a gas, a liquid, or a solid under atmospheric conditions. Also state whether it exists in the elemental form as atoms, as molecules, or as a three-dimensional network: \(\mathrm{Mg}, \mathrm{Cl}, \mathrm{Si}, \mathrm{Kr}, \mathrm{O}, \mathrm{I}, \mathrm{Hg}, \mathrm{Br}\)

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