Consider the collection of nonmetallic elements O, P, Te, I, and B. (b) Which two would form the longest single bond?

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insert step 1> Identify the elements in the problem: O (Oxygen), P (Phosphorus), Te (Tellurium), I (Iodine), and B (Boron).

insert step 2> Recall that the length of a single bond between two atoms is influenced by the size of the atoms involved. Larger atoms tend to form longer bonds.

insert step 3> Consider the periodic trends: Atomic size increases as you move down a group in the periodic table and decreases as you move across a period from left to right.

insert step 4> Compare the atomic sizes of the given elements. Te and I are in the same period and are larger than O, P, and B, which are in higher periods.

insert step 5> Conclude that the longest single bond would likely be between the two largest atoms, which are Te and I.

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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 distance between the nuclei of two bonded atoms. It is influenced by the size of the atoms and the type of bond formed (single, double, or triple). Generally, single bonds are longer than double or triple bonds, and larger atoms tend to form longer bonds due to their increased atomic radii.

Atomic Size and Trends

Atomic size refers to the distance from the nucleus to the outermost electrons. In the periodic table, atomic size increases down a group and decreases across a period. Nonmetals like oxygen and iodine have different atomic sizes, which affects the bond length when they form bonds with each other.

Types of Bonds

The type of bond formed between two elements can significantly affect bond length. Single bonds, formed by the sharing of one pair of electrons, are generally longer than double or triple bonds. In the context of nonmetals, the nature of the bond (e.g., covalent) and the specific elements involved will determine the bond length.

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Textbook Question

Construct a Born–Haber cycle for the formation of the hypothetical compound NaCl₂, where the sodium ion has a 2⁺ charge (the second ionization energy for sodium is given in Table 7.2). (a) How large would the lattice energy need to be for the formation of NaCl₂ to be exothermic?

Textbook Question

Consider the collection of nonmetallic elements O, P, Te, I, and B. (a) Which two would form the most polar single bond?

Textbook Question

The substance chlorine monoxide, ClO(g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of 1.24 D, and the Cl—O bond length is 160 pm. (b) Based on the electronegativities of the elements, which atom would you expect to have a partial negative charge in the ClO molecule?

Textbook Question

(b) Using these partial charges and the atomic radii given in Figure 7.8, estimate the dipole moment of the molecule.

Textbook Question

(c) The measured dipole moment of BrCl is 0.57 D. If you assume the bond length in BrCl is the sum of the atomic radii, what are the partial charges on the atoms in BrCl using the experimental dipole moment?