Ionic bond The attraction between oppositely charged ions

Ionic bond the attraction between oppositely charged ions. 

The attraction between oppositely charged ions results in an ionic bond, such as the one that holds NaCl together. The oppositely charged ions Na+ and CP, attract each other in such an ordered manner that a crystal results (fig. 3). 

We ve seen that when sodium reacts with chlorine, each atom becomes an ion. Sodium chloride, like all ionic substances, is held together by the attraction existing between positive and negative charges. An ionic bond is the attraction between oppositely charged ions. 

FIGURE 1.4 An ionic bond is the force of attraction between oppositely charged ions. Each Na ion (yellow) in the crystal lattice of solid NaCI is involved in ionic bonding to each of six surrounding Cl ions (green) and vice versa. 

Ionic bonding is the electrostatic force of attraction between oppositely charged ions (+ and -), which are formed as a result of electron transfer between atoms. 

The energy required for the formation of ionic bonds is supplied largely by the coulombic attraction between oppositely charged ions the ionic model is a good description of bonding between nonmetals and metals, particularly metals from the s block. 

Covalent bonds result from the Columbic attraction for one or more shared pairs of electrons between two nuclei. Ionic bonds result from the Columbic attraction between oppositely charged ions. 

Ionic bonds are formed by electrostatic attractions between oppositely charged ions. These ions are formed when atoms of low ionization energy (weak attraction for valence electrons) lose one or more electrons to atoms with high electron affinity (strong attraction for electrons). At this point, we can use the octet rule to guide us through the process. 

Ionic bonds are very strong bonds that are formed between a cation and an anion. The ionic bond is formed when a metal loses or transfers an electron (or electrons) to a nonmetal so that the metal and nonmetal form ions that have a full outermost principal energy level. The cations and anions thus formed then attract each other s opposite charges. The attraction between oppositely charged particles is called an electrostatic force. 

Today, an ionic bond is recognized as the nondirectional electrostatic attraction between oppositely charged ions. For an isolated ion pair, the Coulomb potential energy, U, is simply... 

Because anions and cations have opposite charges, they attract each other. This force of attraction between oppositely charged ions is called ionic bonding. As shown in Fig. 2.18, sodium metal and chlorine gas (a green gas composed of CI2 molecules) react to form solid sodium chloride, which contains many Na+ and Cl- ions packed together (Fig. 2.19). The solid forms the beautiful, colorless cubic crystals shown in Fig. 2.18. 

An ionic bond is one in which one or more electrons are transferred from one atom s valence shell (becoming a positively charged ion, called a cation) to the others valence shell (becoming a negatively charged ion, called a anion). The resulting electrostatic attraction between oppositely charged ions results in the formation of the ionic bond. 

FIGURE 1.5 An ionic bond is the force of electrostatic attraction between oppositely charged ions, illustrated in this case by Na" (red) and Cl (green). In solid sodium chloride, each sodium ion is surrounded by six chloride ions and vice versa in a crystal lattice. 

Fundamentally, a chemical bond involves either the sharing of two electrons or the transfer of one or more electrons to form ions. Two atoms of nonmetals tend to share pairs of electrons in what is called a covalent bond. By sharing electrons, the atoms remain more or less electrically neutral. However, when an atom of a metal approaches an atom of a nonmetal, the more likely event is the transfer of one or more electrons from the metal atom to the nonmetal atom. The metal atom becomes a positively charged ion and the nonmetal atom becomes a negatively charged ion. The attraction between opposite charges provides the force that holds the atoms together in what is called an ionic bond. Many chemical bonds are also intermediate in nature between covalent and ionic bonds and have characteristics of both types of bonds. 

The ionic bond is physically the simplest of the four types of interatomic binding force, and arises from the electrostatic attraction between oppositely charged ions. We must therefore first consider the conditions under which ions of the various elements are formed. 

The force of electrostatic attraction between oppositely charged ions constitutes the ionic or electrovalent bond. It must not be assumed that any given structure is necessarily ionic just because it consists of particles some of which can exist as cations and others as anions, for we shall find that in many such cases the binding is in fact of a different kind. Nevertheless, there are numerous structures in which the binding forces are predominantly ionic in character, and it is convenient to introduce our discussion of the structures of ionic crystals by considering the simplest of such examples, namely, the alkali halides and some other compounds of the general composition AX. 

These final states of the sodium and chlorine atoms are known as ions. The sodium atom becomes a positive ion Na+, and the chlorine atom becomes a negative ion CP. The attraction between oppositely charged species would constitute a bond and in this case the bond is said to be ionic or electrovalenu Since the sodium atom, in forming a bond lost one electron, and the chlorine atom gained one electron, both these atoms are said to have a valency of one for sodium, it is equal to the number of electrons in its outermost orbit. For the chlorine atom, the valency can be seen to be equal to eight minus the number of electrons in its outer orbit. 

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