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Chapter 2: Problem 69

The formula for calcium oxide is \(\mathrm{CaO}\). What are the formulas for magnesium oxide and cesium oxide?

Short Answer

Expert verified
Magnesium oxide is MgO and cesium oxide is Cs_2O.

Step by step solution

01

Determine the Ion Charges

Magnesium (Mg) belongs to Group 2 of the periodic table, just like calcium (Ca), and thus has a charge of +2 (Mg^{2+}). Cesium (Cs) belongs to Group 1 and has a charge of +1 (Cs^+). Oxygen (O), a non-metal, typically forms a -2 charge (O^{2-}).
02

Balance the Charges for Magnesium Oxide

To form a neutral compound with magnesium, which has a +2 charge, and oxygen, which carries a -2 charge, one atom of each will balance the overall charge to zero. Therefore, the formula for magnesium oxide is written as MgO.
03

Balance the Charges for Cesium Oxide

To form a neutral compound with cesium, which has a +1 charge, two cesium ions are needed to balance the charge of one oxygen ion, which is -2. So, the formula for cesium oxide is Cs_2O.

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Key Concepts

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

Ion Charges
Understanding how ions form and their respective charges is crucial when predicting the formulas of compounds. Atoms or molecules that have gained or lost electrons are referred to as ions. Metals, which are typically located on the left side of the periodic table, tend to lose electrons and form positively charged ions known as cations. Non-metals, usually found on the right side, tend to gain electrons and form negatively charged ions, called anions.

  • Group 1 metals lose one electron to form ions with a +1 charge (e.g., Na鈦�, Cs鈦�).
  • Group 2 metals lose two electrons, resulting in ions with a +2 charge (e.g., Mg虏鈦�, Ca虏鈦�).
  • Non-metals, like oxygen, often gain two electrons, forming ions with a -2 charge (e.g., O虏鈦�).
The charge of these ions plays a crucial role in how they combine to form compounds.
Neutral Compound
In chemistry, a neutral compound is one where the total positive charge equals the total negative charge. This balance can be achieved by following simple mathematics: matching total positive charges from cations with total negative charges from anions.

To achieve neutrality:
  • Identify the charges of the respective ions involved.
  • Balance the number of positive and negative charges to sum to zero.
For instance, to form magnesium oxide, MgO, one needs one Mg虏鈦� ion and one O虏鈦� ion as their charges (+2 and -2) balance each other to zero. Whereas in cesium oxide, Cs鈧侽, two Cs鈦� ions each with a +1 charge balance one O虏鈦� ion with a -2 charge. The principle of neutrality is a guiding factor in determining chemical formulas.
Periodic Table Groups
The periodic table is organized into columns known as groups, which help predict the behavior of elements, particularly their ion charges. Group numbers are aligned with the number of valence electrons, which are the electrons available for bonding with other atoms. This understanding allows us to predict an element's charge as they turn into ions.

For example:
  • Group 1 elements like sodium (Na) and cesium (Cs) have one valence electron, leading to a typical ion charge of +1 after losing this electron.
  • Group 2 elements such as magnesium (Mg) and calcium (Ca) have two valence electrons, leading to a charge of +2 when these are lost.
Understanding the group an element belongs to allows predictions of its chemical bonding characteristics, simplifying the determination of chemical formulas of compounds.

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Most popular questions from this chapter

Give the number of protons and electrons in each of the following common ions: \(\mathrm{Na}^{+}, \mathrm{Ca}^{2+}, \mathrm{Al}^{3+}, \mathrm{Fe}^{2+}\), \(\mathrm{I}^{-}, \mathrm{F}^{-}, \mathrm{S}^{2-}, \mathrm{O}^{2-}, \mathrm{N}^{3-}\)

Write the formulas for these compounds: (a) rubidium nitrite, (b) potassium sulfide, (c) perbromic acid (d) magnesium phosphate (e) calcium hydrogen phosphate (f) boron trichloride, (g) iodine heptafluoride (h) ammonium sulfate (i) silver perchlorate (j) iron(III) chromate, (k) calcium sulfate dihydrate

Calculate the number of neutrons of \({ }^{239} \mathrm{Pu}\).

Give an example of each of the following: (a) a monatomic cation, (b) a monatomic anion, (c) a polyatomic cation, (d) a polyatomic anion.

Give the number of protons and electrons in each of the following common ions: \(\mathrm{K}^{+}, \mathrm{Mg}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Br}^{-}\), \(\mathrm{Mn}^{2+}, \mathrm{C}^{4-}, \mathrm{Cu}^{2+}\)
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