A common form of elemental phosphorus is the tetrahedral P 4 molecule, where all four phosphorus atoms are equivalent: (b) How many P-P bonds are there in the molecule?

Hey everyone, we're asked to identify two possible lewis structures for arsonists acid first. Let's go ahead and identify the total number of valence electrons will have. Starting with our hydrogen, we have three of hydrogen and so we're going to multiply that by one valence electron which will get us to a total of three. Next looking at our arsenic, we know that this is in our group five A. So we're going to multiply one times five to get five valence electrons. And lastly looking at our oxygen, we have three of oxygen and we're going to multiply this by six since it's in our group six A. This will get us to a total of 18, Adding these three values up. We get 26 valence electrons. Now let's go ahead and draw out our structures were given a hint right here, we're told that one structure has arsenic with three covalin bonds and the other has arsenic with five covalin bonds. Starting off with the three covalin bonds, we know that arsenic is going to be our central atom. And when we create three covalin bonds, we can go ahead and attach our oxygen's since those hydrogen are going to be attached to our oxygen's now completing our total number of valence electrons. We're going to add two lone pairs onto each oxygen. And lastly to complete arsenic octet, we add a lone pair onto our arsenic as well. So this is going to be one of the possible lewis structures for arsonist acid. Now let's look at our next structure, we're told that arsenic will have five covalin bonds. So drawing this out again, we know oxygen is going to be connected to our arsenic and we can go ahead and create a double bond between one oxygen, and we can go ahead and add our hydrogen onto an oxygen. So it would be the oxygen that is single bonded to our arsenic. And since we have one last hydrogen will make that fifth Covalin bond by adding that hydrogen onto arsenic. Now, to complete our octet for oxygen's will go ahead and add two lone pairs onto each, and arsenic is able to violate our octet rule, which is why we have five Covalin bonds here. So this is going to be our final structures for this question. Now, I hope this made sense. And let us know if you have any questions.

Ch.8 - Basic Concepts of Chemical Bonding

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Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 107b

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Chapter 8, Problem 107b

A common form of elemental phosphorus is the tetrahedral P₄ molecule, where all four phosphorus atoms are equivalent:
(b) How many P-P bonds are there in the molecule?

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Understand the structure of the P_4 molecule: The P_4 molecule is a tetrahedral structure, meaning it forms a shape similar to a pyramid with a triangular base.

Visualize the tetrahedral shape: In a tetrahedral P_4 molecule, each phosphorus atom is located at a vertex of the tetrahedron.

Identify the bonds: In a tetrahedral structure, each vertex (phosphorus atom) is connected to three other vertices (phosphorus atoms) by P-P bonds.

Count the bonds: Since each phosphorus atom forms bonds with three other phosphorus atoms, you might initially think there are 4 x 3 = 12 bonds.

Avoid double-counting: Each bond is shared between two phosphorus atoms, so the actual number of unique P-P bonds is 12/2 = 6.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molecular Structure

The molecular structure of a compound refers to the arrangement of atoms within the molecule. In the case of P4, the tetrahedral geometry indicates that the four phosphorus atoms are arranged at the corners of a tetrahedron, which influences the bonding and overall stability of the molecule.

Covalent Bonds

Covalent bonds are formed when two atoms share electrons, allowing them to achieve a more stable electron configuration. In P4, each phosphorus atom forms single covalent bonds with the other three phosphorus atoms, resulting in a network of interconnected atoms.

Counting Bonds

To determine the number of bonds in a molecule, one must consider how many pairs of atoms are connected. In P4, each of the four phosphorus atoms is bonded to three others, leading to a total of six P-P bonds, as each bond is counted once for each pair of atoms.

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Potassium peroxide is composed of 70.96% K and 29.04% O. Each peroxide ion has a net charge of 2-. (a) Given the molecular weight of the compound is 110.19, determine the chemical formula of potassium peroxide.

Textbook Question

Acetylene (C₂H₂) and nitrogen (N₂) both contain a triple bond, but they differ greatly in their chemical properties. (b) By referring to Appendix C, look up the enthalpies of formation of acetylene and nitrogen. Which compound is more stable?

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Textbook Question

Under special conditions, sulfur reacts with anhydrous liquid ammonia to form a binary compound of sulfur and nitrogen. The compound is found to consist of 69.6% S and 30.4% N. Measurements of its molecular mass yield a value of 184.3 g/mol. The compound occasionally detonates on being struck or when heated rapidly. The sulfur and nitrogen atoms of the molecule are joined in a ring. All the bonds in the ring are of the same length. (a) Calculate the empirical and molecular formulas for the substance.

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Textbook Question

A common form of elemental phosphorus is the tetrahedral P₄ molecule, where all four phosphorus atoms are equivalent:

Draw a Lewis structure for a linear P₄ molecule that satisfies the octet rule. Does this molecule have resonance structures?

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Textbook Question

Trifluoroacetic acid has the chemical formula CF3CO2H. It is a colorless liquid that has a density of 1.489 g/mL. (b) Trifluoroacetic acid can react with NaOH in aqueous solution to produce the trifluoroacetate ion, CF3COO2. Write the balanced chemical equation for this reaction.

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Textbook Question

Trifluoroacetic acid has the chemical formula CF3CO2H. It is a colorless liquid that has a density of 1.489 g/mL. (d) How many milliliters of a 0.500 M solution of NaOH would it take to neutralize 10.5 mL of trifluoroacetic acid?

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A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent: (b) How many P-P bonds are there in the molecule?

Verified Solution

Key Concepts

Molecular Structure

Covalent Bonds

Counting Bonds

A common form of elemental phosphorus is the tetrahedral P₄ molecule, where all four phosphorus atoms are equivalent:
(b) How many P-P bonds are there in the molecule?