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Chapter 8: Problem 40

List all the possible bonds that can occur between the elements P, Cs, O, and 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 and their types between the elements P, Cs, O, and H are: 1. P and Cs: Polar covalent 2. P and O: Polar covalent 3. P and H: Covalent (non-polar) 4. Cs and O: Ionic 5. Cs and H: Polar covalent 6. O and H: Polar covalent

Step by step solution

01

List all possible element pairings

: First, we need to list all unique possible combinations of these 4 elements. There are 6 pairs: 1. P and Cs 2. P and O 3. P and H 4. Cs and O 5. Cs and H 6. O and H
02

Determine the type of each bond using electronegativity values

: To determine the bond type, we can use the difference in electronegativity values between the elements in each pair. We can consult a periodic table or electronegativity table for these values: - Phosphorus (P): 2.19 - Cesium (Cs): 0.79 - Oxygen (O): 3.44 - Hydrogen (H): 2.2 Based on the electronegativity values, we can determine the bond type using the following guidelines: - If the difference is 0, the bond is covalent (non-polar). - If the difference is between 0 and 1.6, the bond is polar covalent. - If the difference is 1.7 or greater, the bond is ionic. Let's apply this to the 6 pairings. 1. P and Cs: Electronegativity difference: |2.19 - 0.79| = 1.4 Bond type: Polar covalent 2. P and O: Electronegativity difference: |2.19 - 3.44| = 1.25 Bond type: Polar covalent 3. P and H: Electronegativity difference: |2.19 - 2.2| = 0.01 Bond type: Covalent (non-polar) 4. Cs and O: Electronegativity difference: |0.79 - 3.44| = 2.65 Bond type: Ionic 5. Cs and H: Electronegativity difference: |0.79 - 2.2| = 1.41 Bond type: Polar covalent 6. O and H: Electronegativity difference: |3.44 - 2.2| = 1.24 Bond type: Polar covalent
03

Summarize the bonding types for each pair of elements

: Using electronegativity differences, the bond types for each element pair are: 1. P and Cs: Polar covalent 2. P and O: Polar covalent 3. P and H: Covalent (non-polar) 4. Cs and O: Ionic 5. Cs and H: Polar covalent 6. O and H: Polar covalent

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Most popular questions from this chapter

Consider the following energy changes: $$\begin{array}{ll} \text {} & \quad { \Delta H} \\ \text {} & {(k J / m o l)} \\ \hline \\ {\mathrm{Mg}(g) \rightarrow \mathrm{Mg}^{+}(g)+\mathrm{e}^{-}} & {735} \\ {\mathrm{Mg}^{+}(g) \rightarrow \mathrm{Mg}^{2+}(g)+\mathrm{e}^{-}} & {1445} \\ {\mathrm{O}(g)+\mathrm{e}^{-} \rightarrow \mathrm{O}^{-}(g)} & {-141} \\ {\mathrm{O}^{-}(g)+\mathrm{e}^{-} \rightarrow 0^{2-}(g)} & {878}\end{array}$$ Magnesium oxide exists as \(\mathrm{Mg}^{2+} \mathrm{O}^{2-}\) and not as \(\mathrm{Mg}^{+} \mathrm{O}^{-}\) Explain.

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Use the following data (in kJ/mol) to estimate \(\Delta H\) for the reaction \(S^{-}(g)+e^{-} \rightarrow S^{2-}(g)\) . Include an estimate of uncertainty. $\begin{aligned} \mathrm{S}(s) \longrightarrow \mathrm{S}(g) & \Delta H=277 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{S}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{S}^{-}(g) & \Delta H=-200 \mathrm{kJ} / \mathrm{mol} \end{aligned}$ Assume that all values are known to \(\pm 1 \mathrm{kJ} / \mathrm{mol}\)
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