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Ch.7 - Periodic Properties of the Elements
Chapter 7, Problem 86

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 236 and 194 pm, 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.

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1
Identify the given bond lengths: A-A bond length is 236 pm and B-B bond length is 194 pm.
Understand the structure of the compound AB2, which is linear (B-A-B = 180°). This implies that the molecule is straight with atom A in the middle and two B atoms on either side.
Recognize that the separation between the two B nuclei in AB2 will be twice the length of the B-A bond since the molecule is linear.
Assume that the B-A bond length can be approximated by the average of the A-A and B-B bond lengths. Calculate this average: (236 pm + 194 pm) / 2.
Multiply the average bond length by 2 to find the separation between the two B nuclei in the AB2 molecule.

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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 the types of atoms involved and the nature of the bond (single, double, or triple). In this case, the bond lengths of A-A and B-B provide insight into the size and strength of the bonds, which is essential for predicting the geometry and distances in the compound AB2.
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Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. The linear structure of AB2 indicates that the atoms are arranged in a straight line, with bond angles of 180°. Understanding molecular geometry is crucial for predicting the spatial relationships between atoms, which directly affects the separation between the B nuclei in the compound.
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VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of molecules based on the repulsion between electron pairs surrounding a central atom. In the case of AB2, the linear arrangement suggests that the two B atoms are positioned to minimize repulsion, leading to a specific separation that can be calculated using the bond lengths and the linear structure.
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Related Practice
Textbook Question
In Table 7.8, the bonding atomic radius of neon is listed as 58 pm, whereas that for xenon is listed as 140 pm. 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?
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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?

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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?

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Open Question
Elements in group 17 in the periodic table are called the halogens; elements in group 16 are called the chalcogens. For each of the following periodic properties, state whether the halogens or the chalcogens have larger values: atomic radii, ionic radii of the most common oxidation state, first ionization energy, and second ionization energy.
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?

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Textbook Question
Note from the following table that there is a significant increase in atomic radius upon moving from Y to La, whereas the radii of Zr to Hf are the same. Suggest an explanation for this effect. Atomic Radii (pm) Sc 170 Ti 160 Y 190 Zr 175 La 207 Hf 175
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