Textbook Question
(b) Repeat these calculations using Slater’s rules.
Ch.7 - Periodic Properties of the Elements
Chapter 7, Problem 84a
The As ¬ As bond length in elemental arsenic is 2.48 Å. The Cl ¬ Cl bond length in Cl2 is 1.99 Å. (a) Based on these data, what is the predicted As ¬ Cl bond length in arsenic trichlo- ride, AsCl3, in which each of the three Cl atoms is bonded to the As atom?
Verified step by step guidance1
insert step 1> Determine the average bond length by using the bond lengths of As-As and Cl-Cl.
insert step 2> Use the concept of covalent radii to estimate the bond length of As-Cl.
insert step 3> Calculate the covalent radius of As by dividing the As-As bond length by 2.
insert step 4> Calculate the covalent radius of Cl by dividing the Cl-Cl bond length by 2.
insert step 5> Add the covalent radii of As and Cl to predict the As-Cl bond length in AsCl_3.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Bond Length
Bond length is the average distance between the nuclei of two bonded atoms. It is influenced by factors such as atomic size, bond order, and the presence of lone pairs. In general, shorter bond lengths indicate stronger bonds due to greater overlap of atomic orbitals.
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Average Bond Order
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of arsenic trichloride (AsCl3), arsenic undergoes sp3 hybridization, resulting in four equivalent hybrid orbitals that form sigma bonds with the three chlorine atoms and one lone pair.
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Trends in Bond Lengths
Trends in bond lengths can be predicted based on the types of atoms involved and their bonding characteristics. Generally, bond lengths increase with the size of the atoms and decrease with increasing bond order. By comparing known bond lengths, one can estimate the bond length in new compounds, such as AsCl3, by considering the influence of both As-As and Cl-Cl bonds.
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Related Practice
Textbook Question
(d) If you remove a single electron from a P atom, which orbital will it come from?
Textbook Question
In Table 7.8, the bonding atomic radius of neon is listed as 0.58 Å, whereas that for xenon is listed as 1.40 Å. A classmate of yours states that the value for Xe is more realistic than the one for Ne. Is she correct? If so, what is the basis for her statement?
Textbook Question
The following observations are made about two hypothetical elements A and B: The A—A and B—B bond lengths in the elemental forms of A and B are 2.36 and 1.94 Å, respectively. A and B react to form the binary compound AB2, which has a linear structure (that is, ∠B-A-B=180°). Based on these statements, predict the separation between the two B nuclei in a molecule of AB2.
Textbook Question
The As ¬ As bond length in elemental arsenic is 2.48 Å. The Cl ¬ Cl bond length in Cl2 is 1.99 Å. (b) What bond length is predicted for AsCl3, using the atomic radii in Figure 7.7?
Textbook Question
Elements in group 7A in the periodic table are called the halogens; elements in group 6A are called the chalcogens. (a) What is the most common oxidation state of the chalcogens compared to the halogens?