For each pair of bonds, predict which will be the shorter. (a) Si-N or P-O (b) Si-O or C-O (c) C

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For each pair of bonds, predict which will be the shorter....

For each pair of bonds, predict which will be the shorter. (a) $\mathrm{Si}-\mathrm{N}$ or $\mathrm{P}-\mathrm{O}$ (b) $\mathrm{Si}-\mathrm{O}$ or $\mathrm{C}-\mathrm{O}$ (c) $\mathrm{C}-\mathrm{F}$ or $\mathrm{C}-\mathrm{Br}$ (d) The $\mathrm{C}=\mathrm{C}$ or the $\mathrm{C} \equiv \mathrm{N}$ bond in acrylonitrile, $\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}-\mathrm{C}=\mathrm{N}$

For each pair of bonds, predict which will be the shorter.
(a) $\mathrm{Si}-\mathrm{N}$ or $\mathrm{P}-\mathrm{O}$
(b) $\mathrm{Si}-\mathrm{O}$ or $\mathrm{C}-\mathrm{O}$
(c) $\mathrm{C}-\mathrm{F}$ or $\mathrm{C}-\mathrm{Br}$
(d) The $\mathrm{C}=\mathrm{C}$ or the $\mathrm{C} \equiv \mathrm{N}$ bond in acrylonitrile, $\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}-\mathrm{C}=\mathrm{N}$

Key Concepts

Atomic Radius

This concept refers to the size of an atom's electron cloud. In bonding, smaller atoms tend to form shorter bonds because their electrons are held closer to the nucleus, resulting in a more compact and stronger overlap with adjacent atoms. When comparing bonds, differences in atomic radii are a primary factor that influences the bond length.

Bond Order

Bond order represents the number of electron pairs shared between two atoms. Higher bond orders, such as double or triple bonds, involve more shared electrons and produce a shorter, stronger bond because the increased electron density holds the nuclei closer together. This concept is essential when comparing bonds of different multiplicities.

Electronegativity

Electronegativity is the ability of an atom to attract shared electrons in a bond. Variations in electronegativity between bonded atoms can affect the electron density distribution, which in turn can influence the bond length. A significant difference in electronegativity may lead to a stronger pull on the bonding electrons, subtly affecting the bond contraction.

Multiple Bonding

Multiple bonding refers to the existence of more than one bond between a pair of atoms, as in double or triple bonds. These bonds are generally shorter than single bonds due to the increased electron sharing and stronger attraction between the atoms. Evaluating which bonds in a molecule are single versus multiple is crucial to predicting relative bond lengths.

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