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

검증된 단계별 안내

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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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.