Skip to main content
Pearson+ LogoPearson+ Logo
Ch.7 - Periodic Properties of the Elements
All textbooksBrown 14th EditionCh.7 - Periodic Properties of the ElementsProblem 85b
Chapter 7, Problem 85b

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?

Verified step by step guidance
1
Identify the atomic radii of arsenic (As) and chlorine (Cl) from Figure 7.7.
Recall that the bond length in a molecule is approximately the sum of the atomic radii of the two bonded atoms.
Add the atomic radius of arsenic to the atomic radius of chlorine to estimate the As-Cl bond length.
Express the bond length in appropriate units, typically in Ångströms (Å).
Verify the calculated bond length with known data or literature values, if available, to ensure accuracy.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1m
Was this helpful?

Key Concepts

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

Bond Length

Bond length is the distance between the nuclei of two bonded atoms. It is influenced by the size of the atoms involved and the type of bond (single, double, etc.). Understanding bond lengths helps predict molecular geometry and reactivity, as shorter bonds typically indicate stronger interactions.
Recommended video:
Guided course
00:36
Average Bond Order

Atomic Radii

Atomic radii refer to the size of an atom, typically measured from the nucleus to the outermost electron shell. These values vary across the periodic table and are crucial for estimating bond lengths in compounds. The effective atomic radius can change depending on the bonding environment and the type of atoms involved.
Recommended video:
Guided course
03:07
Ranking Ionic Radii

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonds and lone pairs around the central atom, influencing properties like polarity and reactivity. Understanding molecular geometry is essential for predicting bond lengths and angles in compounds like AsCl3.
Recommended video:
Guided course
01:33
Molecular Geometry with Two Electron Groups
Related Practice
Textbook Question
In Table 7.8, the bonding atomic radius of neon is listed as58 pm, whereas that for xenon is listed as 140 pm. A classmateof yours states that the value for Xe is more realisticthan the one for Ne. Is she correct? If so, what is the basisfor her statement?
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. (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?

Textbook Question
The following observations are made about two hypotheticalelements A and B: The A¬A and B¬B bond lengths in theelemental forms of A and B are 236 and 194 pm, respectively.A and B react to form the binary compound AB2, which hasa linear structure (that is B-A-B = 180°). Based on thesestatements, predict the separation between the two B nucleiin a molecule of AB2.
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?