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Chapter 3: Problem 40

List all the possible bonds that can occur between the elements \(\mathrm{P}, \mathrm{Cs}, \mathrm{O},\) and \(\mathrm{H} .\) Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form for each bond.

Short Answer

Expert verified
The possible bonds between the elements P (Phosphorus), Cs (Cesium), O (Oxygen), and H (Hydrogen) and their type are: 1. P-H: Nonpolar Covalent 2. P-Cs: Ionic 3. P-O: Polar Covalent 4. Cs-O: Ionic 5. Cs-H: Ionic 6. O-H: Polar Covalent

Step by step solution

01

List all possible bonds

We have 4 elements: P, Cs, O, and H. Let's list down all the possible bonds between these elements: 1. P-H 2. P-Cs 3. P-O 4. Cs-O 5. Cs-H 6. O-H
02

Predict the type of bond for P-H

First, we will consider the electronegativity values of P and H. Phosphorus (P) has an electronegativity of 2.19, and Hydrogen (H) has an electronegativity of 2.20. The electronegativity difference between P and H is \(|2.20 - 2.19| = 0.01\). Since the electronegativity difference is very small, the bond between P and H is likely to be nonpolar covalent.
03

Predict the type of bond for P-Cs

Now let's consider the electronegativity values of P and Cs. Cesium (Cs) has an electronegativity of 0.79. The electronegativity difference between P and Cs is \(|2.19 - 0.79| = 1.40\). Since the electronegativity difference is greater than 1.7, the bond between P and Cs is likely to be ionic.
04

Predict the type of bond for P-O

We will now consider the electronegativity values of P and O. Oxygen (O) has an electronegativity of 3.44. The electronegativity difference between P and O is \(|3.44 - 2.19| = 1.25\). Since the electronegativity difference lies between 0.4 and 1.7, the bond between P and O is likely to be polar covalent.
05

Predict the type of bond for Cs-O

Let's now consider the electronegativity values of Cs and O. The electronegativity difference between Cs and O is \(|3.44 - 0.79| = 2.65\). Since the electronegativity difference is greater than 1.7, the bond between Cs and O is likely to be ionic.
06

Predict the type of bond for Cs-H

Now, let's consider the electronegativity values of Cs and H. The electronegativity difference between Cs and H is \(|2.20 - 0.79| = 1.41\). Since the electronegativity difference is greater than 1.7, the bond between Cs and H is likely to be ionic.
07

Predict the type of bond for O-H

Finally, let's consider the electronegativity values of O and H. The electronegativity difference between O and H is \(|3.44 - 2.20| = 1.24\). Since the electronegativity difference lies between 0.4 and 1.7, the bond between O and H is likely to be polar covalent. Summary: 1. P-H: Nonpolar Covalent 2. P-Cs: Ionic 3. P-O: Polar Covalent 4. Cs-O: Ionic 5. Cs-H: Ionic 6. O-H: Polar Covalent

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Most popular questions from this chapter

Write the formula for each of the following compounds: a. sodium oxide b. sodium peroxide c. potassium cyanide d. copper(II) nitrate e. selenium tetrabromide f. iodous acid g. lead(IV) sulfide h. copper(I) chloride I. gallium arsenide J. cadmium selenide k. zinc sulfide I. nitrous acid m. diphosphorus pentoxide

The designations \(1 \mathrm{A}\) through \(8 \mathrm{A}\) used for certain families of the periodic table are helpful for predicting the charges on ions in binary ionic compounds. In these compounds, the metals generally take on a positive charge equal to the family number, while the nonmetals take on a negative charge equal to the family number minus \(8 .\) Thus the compound between sodium and chlorine contains \(\mathrm{Na}^{+}\) ions and \(\mathrm{Cl}^{-}\) ions and has the formula NaCl. Predict the formula and the name of the binary compound formed from the following pairs of elements. a. Ca and N b. \(K\) and 0 c. \(\mathrm{Rb}\) and \(\mathrm{F}\) d. \(\mathrm{Mg}\) and \(\mathrm{S}\) e. Ba and I f. Al and Se g. Cs and \(P\) h. In and Br

Lewis structures can be used to understand why some molecules react in certain ways. Write the Lewis structures for the reactants and products in the reactions described below. a. Nitrogen dioxide dimerizes to produce dinitrogen tetroxide. b. Boron trihydride accepts a pair of electrons from ammonia, forming \(\mathrm{BH}_{3} \mathrm{NH}_{3}\) Give a possible explanation for why these two reactions occur.

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