Question

Compare the size of an orbital that has a shared electron pair with one that has a lone pair.

Short answer

The orbital size with a shared electron pair is larger than the orbital size with a lone pair due to the difference in electron density distribution and the number of nuclei attracting the electrons. Shared electron pairs are attracted to two nuclei, causing the electron density to be spread across a larger area, while lone pairs experience attraction by only one nucleus, localizing the electron density around that single atom.

Step-by-step solution

Understanding shared electron pair and lone pair

A shared electron pair consists of two electrons that are shared between two atoms participating in a covalent bond. A lone pair, on the other hand, is a pair of valence electrons that are not shared in a bond and remain with only one atom.

Comparing the sizes of orbitals with shared electron pairs and lone pairs

Orbitals with shared electron pairs have a larger size than those with lone pairs. This is because the shared electron pair is attracted to two nuclei, which causes the electron density to be spread across a larger area. On the other hand, the lone pair experiences attraction by only one nucleus, and the electron density is localized around that single atom. To summarize, the orbital size with a shared electron pair is larger than the orbital size with a lone pair due to the difference in electron density distribution and the number of nuclei attracting the electrons.

Key concepts

Shared Electron Pair

Understanding what a shared electron pair consists of is fundamental in chemistry, particularly when discussing molecular structures. In essence, a shared electron pair is comprised of two electrons that unite two atoms within a molecule. Imagine these electrons as the glue holding the atoms together.

When atoms come together to form a molecule, they often do so by sharing pairs of electrons in a process that results in the formation of a covalent bond. Each electron in the shared pair originates from a different atom, allowing both atoms to achieve a more stable electronic arrangement similar to the noble gases.

This sharing helps atoms complete their outermost electron shell, which is a natural drive for elements as it confers stability. The formation of shared electron pairs is a dance of attraction and repulsion, where atoms approach each other and adjust their relative positions to achieve maximum attraction between the positive nuclei and the negative electrons while minimizing electron-electron repulsion.

Lone Pair

A lone pair embodies the concept of exclusivity in the atomic realm. Unlike shared electron pairs, lone pairs are valence electrons that are not shared with another atom and, therefore, do not participate in bonding. They are like a private property.

The presence of lone pairs plays a significant role in determining the geometry and physical properties of a molecule. Since electron pairs are negatively charged, they repel each other, including those involved in bonding. As a result, lone pairs can alter the distribution of other electrons and affect the shape of the molecule.

Furthermore, lone pairs can also engage in chemical reactions under specific circumstances. They may be donated to form new covalent bonds, particularly in acid-base reactions where a lone pair from a base is donated to an acid, a process that is foundational to many biochemical interactions.

Covalent Bond

At the heart of molecular formation lies the covalent bond. It's like a strong handshake between atoms, where each contributes at least one electron to the shared pair. This bond is an enduring connection that results from the sharing of electron pairs between atoms.

The strength of covalent bonds can vary significantly. 'Single' covalent bonds involve the sharing of one electron pair, while 'double' and 'triple' bonds share two and three electron pairs, respectively, and are accordingly stronger.

The formation of a covalent bond is the strategic move atoms make to attain the electron configuration of a noble gas, which is typically associated with stability. Covalent bonding is indispensable when constructing intricate molecules that constitute everything from DNA to proteins and the materials that make up the world around us.

Electron Density Distribution

The electron density distribution within a molecule is a map that showcases where electrons are most likely to be found. It's akin to a population map for electrons, indicating regions of high and low electron concentration.

Electron pairs, both shared and lone, significantly influence this distribution. Orbitals with shared electron pairs distribute the density across a larger space because they are being pulled by two nuclei, leading to a decrease in electron density per unit area. On the contrary, lone pairs are localized around one nucleus, resulting in a more concentrated electron density in that specific region.

The shape and size of an orbital are influenced by this distribution. Shared pairs often result in larger, more diffuse orbitals because of the electron cloud stretching to accommodate the attraction from two nuclei. Meanwhile, lone pairs create smaller orbitals due to the concentrated attraction of one nucleus. This concept is critical when predicting and explaining the physical properties of molecules and their reactivity in chemical reactions.