For this question, consider only the coulomb energy component (the largest) between two atoms. given that nacl (formed from na+ and cl–) has melting temperature of 1074 k (or 801 c), see table 2.3, roughly estimate the melting temperature in kelvin of mgo from that of nacl, i. e., the ratio of coulomb energy. (assume that the equilibrium bond lengths are given by the sum of ionic radii, see table inside front cover of textbook.)

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. the ionic radius for na+ is 102 pm and for cl– is 181 pm. in going from na to cl in period 3, why does the atomic radius decrease while the ionic radius increases? a. the inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do. b. the inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion. c. the outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do. d. the outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do. e. monatomic ions are bigger than the atoms from which they are formed.

What is the empirical formula of c6h18o3? ch3o c2h5o c2h6o c2h5o5

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