Atom electrovalent bonding

The process of the shifting of an electron from one electrical field to another, as in the formation of an electrovalent bond, in which an electron moving in an orbit about one atom shifts to move in an orbit around the two bonded atoms. 

OXIDATION NUMBER. In its original and restrictive sense, the number of electrons which must be added to a cation to neutralize the charge. The concept has been extended to anions by assignments of negative oxidation numbers. Moreover, it has been further extended, first to all atoms or radicals joined by electrovalent bonds, and then to covalent compounds in which the shared electrons are distributed equally. For the broadest use of the concept, the expression oxidation state is often used. 

The ionic or electrovalent bond is a third kind of linkage. When EN between the binding atoms exceeds the value of 1.7, there is hardly question of common electron pairs. In that case the valence electrons of the atom with the smallest EN-value are almost entirely transferred to the other atom with the largest EN-value. One atom loses one or more electrons and becomes a positively charged ion, whereas the other gains one or more electrons and becomes a negatively charged... 

Electrovalent bonds are formed between oppositely charged ions, and typically a metal donates electrons to a nonmetal. For example, sodium chloride (common salt, an important constituent of the body s fluids) is written as Na Cl. For sodium chloride only one electron is involved in the transfer and the molecular formula is written as NaCl. However, if sodium forms an ionic compound with oxygen, an oxygen atom needs two electrons to form an ion, so it will need to have two sodium atoms donating electrons ... 

It can still be seen in mineralogical museums how Berzelius classified many compounds as adducts of oxides, as when alum is written K20 A1203 4 S03 24 H20 whereas it was later written KA1(S04)2 12 H20 and the crystal structure indicates only half of the water molecule oxygen atoms directly connected to aluminum K[A1(0H2)6](S04)2(0H2)6. Actually, the large majority of minerals are mixed oxides (and though these formulae derive from the precursor ideas of electrovalent bonding, considering calcium sulfate as an adduct CaO S03, they have the undoubted... 

Bonds which cannot be represented as Hnks between specific atoms, such as pi bonds and electrovalent bonding between ions, will still be handled by representations. 

Ionic (or electrovalent) bonds can be formed by transfer of electrons. For instance, the calcium atom has an electron configuration of [Ar]4s, i.e. it has two electrons in its outer shell. The chlorine atom is [NeJSs Sp, with seven outer electrons, if the calcium atom transfers two electrons, one to each chlorine atom, it becomes a Ce ion with the stable configuration of an inert gas [Ar]. At the same time each chlorine, having gained one electron, becomes a Ck ion, also with an inert-gas configuration [Ar]. The bonding in calcium chloride is the electrostatic attraction between the ions. 

Acid dyes form ionic bonds (also known as electrovalent bonds), where one atom relinquishes one or more electrons to another atom. 

Ionic (or electrovalent) bonds are formed by the transfer of one or more electrons from one atom to another to create ions. 

Modern bonding theory treats the electron pairing in terms of the interaction of electron (atomic) orbitals and describes the covalent bond in terms of both bonding and anti-bonding molecular orbitals. See also coordinate bond electrovalent bond polar bond. 

Inorganic salts are composed of ions, each bound by strong electrostatic attractive forces (interaction of the type ion-ion). This ion (electrovalent) bond generally occurs between two atoms of different electronegativity by transfer of one or more electrons from one atom to another. For example, sodium (Na) is a typical metal (alkali metal) with low electronegativity (0.9 eV) while chlorine is... 

Sidwick and Lowry gave the electronic interpretation of Werner s theory of coordination compounds. According to them p-imary valencies result from the transference of electrons, whereas secondary valencies result frem the sharing of electrons, i.e. there is a formation of electrovalent bond in primary valencies and coordinate bond in secondary valencies. They also pointed out that all ligands (neutred molecules or anions) have atoms with at least one lone pair of electrons. They donate this lone pair of electrons to the central metal ion and form coordinate... 

A catalyst (CatE+) with electron-deficient atom/centre (E ) can accept a pair of electrons from an electron-rich atom/center (N) of a snbstrate (NXSub) and thns forms a stable electrovalent bond. Snch electrovalent bonding interaction between the catalyst and snbstrate will increase the electrophilicity of the atom X bonded covalently to the electron-rich atom (N) of the substrate as exhibited by Equation 2.7... 

Nearly KP- to 10 -fold larger values of ko° compared with Iq, for M = Zn +, Mg +, and Cu + are attributed to increase in electrophilicity of phosphoryl phosphorous (P) owing to intramolecular electrovalent bonding interaction between anionic oxygen attached to P and 38-bound metal ion as shown in Scheme 2.24. Nearly lO -fold larger value of Iq, compared with Iq, for M = La " is attributed to greater enhancement of electrophilicity of P because of more extensive coordination between oxygen atoms attached to P and M + in complexes 38 M + and 39 M + when M + = La +, than when M + = Zn +, Mg +, and Cu + as shown in Scheme 2.24 and Scheme 2.25. 

HB-5) unusually high cationic character of central atom B and anionic character of terminal atoms A and C, as reflected in natural atomic charges Qa, Qb, Qc), ionic bond orders (6AB(ion) and Aiic<1011)), and electrovalencies (TA(lon), IV1011 . Vc(l0n)). 

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