Bond lengths are smaller when atoms form multiple bonds. Single overlap between two atoms forms a single covalent bond. So, when they overlap twice and thrice to form double and triple bonds the atoms to come closer to form a tight-knit. Such bonds are even harder to break. So, the bond length of a triple is smaller than a double and single bond.
A metallic bond is a chemical bond seen in metals consisting of tightly bound metal atoms of the same type.
Metals are large atoms that do not firmly hold their outermost valence electrons and easily lose them. Once the electrons are lost, the metal atoms become positively charged, called kernels. The position of these kernels is fixed to avoid repulsions and is part of the solid structure.
Atom, the omnipresent particle that builds the universe, hides its identity in a tiny, sub-atomic particle- the proton, where the proton number decides the type of the atom. However, an outer-nuclear component- the electrons- determines an atom's reactivity.
In nuclear reactions, the proton number can change so that the atom's identity also changes. However, in organic chemical reactions, only the electron count changes without affecting an atom's identity.
London dispersion force is the weakest of the three van Der Waal forces of interactions universally found in all the atoms and molecules. It is caused by the constant fluctuations in the electron position, creating a temporary dipole. When other nonpolar molecules are in its vicinity, the instantaneous temporary dipole formed earlier distorts the electron cloud of an adjacent molecule, creating another dipole.
Bi (V) represents the +5-oxidation state of Bismuth (Bi). It means Bi has lost 5 electrons from its valence shell. Bi, therefore, wants to gain the lost electrons and is called an oxidizing agent. The process of electron uptake is a reduction reaction.
Bi (V) is a stronger oxidizing agent than Sb (V) and, therefore, will pick up the electrons faster than Sb (V). Due to the electron uptake, it will then go from a +5-oxidation state to a +3-oxidation state. Bi is now less by only three electrons due to the two-electron gain.
All atoms and molecules show London Dispersion Force, a primary way atoms and molecules interact. Most of the time, molecules have additional stronger forces than the London Dispersion Force, which is the weakest. Therefore, London Dispersion forces are exclusively seen in the nonpolar molecules since they don't have other competing functional groups leading to other interfering intermolecular interactions.
A chemical bond strength is a force holding the atoms in a bond, and separating such atoms requires energy input. The bonds are of two types- Intermolecular and Intramolecular bonds.
Intramolecular bonds join the atoms in a molecule, whereas Intermolecular bonds are only responsible for closely associating the molecules. Therefore, Intramolecular bonds require higher energy to break than intermolecular bonds.
A radical reaction usually happens in three steps- Initiation (creation of free radicals), Propagation (multiplication and growth of radical reaction), and Termination (stopping of the free radical reaction).
Radical inhibitors are chemical species that inhibit radical reactions by halting the chain propagation step.
Examples of such inhibitors are Hydroquinone, BHT (2,6-di-t-butyl-4-methylphenol), etc.
The replacement of the hydrogen in acetic acid (H-CH2-COOH) with the chloro gives chloroacetic acid (Cl-CH2-COOH). Therefore, Acetic acid and Chloroacetic acid have carboxylic acid (R-COOH) as the principal functional group.
The bond angle is the angle at which two adjacent bonds converge and meet at the central atom in molecules.