Electrovalency is favoured by
(A) Low IE values
(B) High EA values
(C) High lattice energy
(D) High electron sharing ability
Answers
Answer:
Concept:
When balancing chemical reactions, electrovalency, a measurement of the net electric charge of an ion, is used. The quantity of electrons required for an ion to have a balance electric charge is known as electrovalency, which is connected to the ideas of electronegativity and valence electrons. Atoms with nearly full or nearly empty valence shells are more likely to be highly reactive. Strongly electronegative atoms, such as those found in halogens, usually only have one or two missing electrons in their valence shell. These atoms frequently establish bonds with other molecules or obtain electrons to form anions. Alkali metals and other weakly electronegative atoms have a limited number of valence electrons that are rapidly lost to highly electronegative atoms.
Given:
Electrovalency is favoured by
(A) Low IE values
(B) High EA values
(C) High lattice energy
(D) High electron sharing ability
Find:
The alternatives that are right are A, B, and C.
Answer:
The choices that are right are A, B, and C.
A. Low IE values:
The number of electrons that are lost or gained during the creation of an ionic connection is the electrovalency of an element. Ionization
enthalpy must be below for an element's atom to easily lose its valence electron and generate cations. Low IE values hence favour electrovalency.
Ionization energy, also known as ionisation energy (IE) or ionisation energy (British English spelling), is the minimal amount of energy needed to free the most loosely bonded electron from an isolated gaseous atom, positive ion, or molecule in physics and chemistry.
B. High EA values:
Electron affinities need to be strong for an elemental atom to form an anion so that the cation's valence electron may be attracted to the atom's nucleus with ease. Therefore, high EA values favour electrovalency.
Its huge atomic radius, or size, can be linked to its strong affinity. Chlorine's electrons have a lot of space to exchange with an incoming electron because its outermost orbital is 3p.
C. High lattice energy:
Higher stability of the ionic compound and stronger attraction between cations and anions are two effects of high lattice energy. Therefore, electrovalency of both cations and anion is favoured by high lattice energy.
The energy that changes when one mole of a crystalline ionic compound is formed from its component ions, which are believed to begin be in the gaseous state, is known as the lattice energy. It gauges the cohesive forces that hold ionic solids together. Numerous additional physical characteristics, including as solubility, hardness, and volatility, are related to the magnitude of the lattice energy. The lattice energy is typically calculated using the Born-Haber cycle from experimental data because it is typically unable to detect it directly.
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