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Chapter 8: Problem 42

Predict the empirical formulas of the ionic compounds formed from the following pairs of elements. Name each compound. a. \(\mathrm{Al}\) and \(\mathrm{Cl}\) c. \(\mathrm{Sr}\) and \(\mathrm{F}\) b. \(\mathrm{Na}\) and \(\mathrm{O}\) d. Ca and Se

Short Answer

Expert verified
The empirical formulas and names of the ionic compounds formed from the given pairs of elements are: a. Aluminum and Chlorine: AlCl3, called "aluminum chloride." b. Sodium and Oxygen: Na2O, called "sodium oxide." c. Strontium and Fluorine: SrF2, called "strontium fluoride." d. Calcium and Selenium: CaSe, called "calcium selenide."

Step by step solution

01

a. Al and Cl

1. Determine the charges: Based on the periodic table, Al (aluminum) is a Group 3 element and commonly forms a 3+ ion, while Cl (chlorine) is a Group 7 element and commonly forms a 1- ion. 2. Combine to form a neutral compound: To balance the charges, we will need 3 Cl- ions to balance the 3+ charge on the Al ion. Thus, the empirical formula for the aluminum chloride compound will be AlCl3. 3. Name the compound: The compound formed from aluminum and chlorine is named "aluminum chloride."
02

b. Na and O

1. Determine the charges: Based on the periodic table, Na (sodium) is a Group 1 element and commonly forms a 1+ ion, while O (oxygen) is a Group 6 element and commonly forms a 2- ion. 2. Combine to form a neutral compound: To balance the charges, we will need 2 Na+ ions to balance the 2- charge on the O ion. Thus, the empirical formula for the sodium oxide compound will be Na2O. 3. Name the compound: The compound formed from sodium and oxygen is named "sodium oxide."
03

c. Sr and F

1. Determine the charges: Based on the periodic table, Sr (strontium) is a Group 2 element and commonly forms a 2+ ion, while F (fluorine) is a Group 7 element and commonly forms a 1- ion. 2. Combine to form a neutral compound: To balance the charges, we will need 2 F- ions to balance the 2+ charge on the Sr ion. Thus, the empirical formula for the strontium fluoride compound will be SrF2. 3. Name the compound: The compound formed from strontium and fluorine is named "strontium fluoride."
04

d. Ca and Se

1. Determine the charges: Based on the periodic table, Ca (calcium) is a Group 2 element and commonly forms a 2+ ion, while Se (selenium) is a Group 6 element and commonly forms a 2- ion. 2. Combine to form a neutral compound: The charges on Ca and Se ions are equal and opposite. We just need one ion of each to balance the charges. Thus, the empirical formula for the calcium selenide compound will be CaSe. 3. Name the compound: The compound formed from calcium and selenium is named "calcium selenide."

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Most popular questions from this chapter

A compound, \(\mathrm{XF}_{5}\), is \(42.81 \%\) fluorine by mass. Identify the element \(X\). What is the molecular structure of \(\mathrm{XF}_{5}\) ?

Write electron configurations for a. the cations \(\mathrm{Sr}^{2+}, \mathrm{Cs}^{+}, \mathrm{In}^{+}\), and \(\mathrm{Pb}^{2+}\). b. the anions \(\mathrm{P}^{3-}, \mathrm{S}^{2-}\), and \(\mathrm{Br}^{-}\).

The most common type of exception to the octet rule are compounds or ions with central atoms having more than eight electrons around them. \(\mathrm{PF}_{5}, \mathrm{SF}_{4}, \mathrm{ClF}_{3}\) and \(\mathrm{Br}_{3}^{-}\) are examples of this type of exception. Draw the Lewis structure for these compounds on ions. Which elements, when they have to, can have more than eight electrons around them? How is this rationalized?

Give the formula of a negative ion that would have the same number of electrons as each of the following positive ions. a. \(\mathrm{Na}^{+}\) c. \(\mathrm{Al}^{3+}\) b. \(\mathrm{Ca}^{2+}\) d. \(\mathrm{Rb}^{+}\)

In general, the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have \(+1\) charged ions even though \(+4,+5\), and \(+6\) charged ions would have a more favorable lattice energy?
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