Group 1A Group 3A Grоцр 7А Слиир 2А Crоир бл ut 0.90 0.59 1.25 0.41 1.19 LI 1.25 a54 0.96 057 Na L16 Mg O86 1.70 1.67 Na 1.66 Mg 141 AI 1.21 1.05 1.02 к 1.52 Ca Ga a76 Br 1.2 1.14 1.84 Ca 1.76 Ga 1.22 Hr 1.20 1.20 2.00 кь 166 Te- 2.00 1- 2.06 a94 1.32 In 1.42 кь 2.20 Te 1.35 1.95 1.39 cation anion - neueral amm AFigure 7 Lattice Energies for Some Ionic Compounds TABLE 8.1 Lattice Energy (kJ/mol) Compound Lattice Energy (kJ/mol) Compound 1030 LiF MgCl2 2526 LİCI 834 SrCl2 2127 Lil 730 NaF 910 MgO 3795 NaCl 3414 788 Cao NaBr 732 Sro 3217 Nal 682 KF 808 ScN 7547 КСІ 701 Kвг 671 CSCI 657 600 CsI
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
Consider the ionic compounds KF, NaCl, NaBr, and LiCl.
(a) Use ionic radii (Figure 7.8) to estimate the cation–anion
distance for each compound. (b) Based on your answer to
part (a), arrange these four compounds in order of decreasing
lattice energy. (c) Check your predictions in part (b) with the
experimental values of lattice energy from Table 8.1. Are the
predictions from ionic radii correct?
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