Describe the following trends in lattice energy

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Reference no: EM13163358

Explain the following trends in lattice energy. (Select all that apply.) (a) NaCl > RbBr > CsBr CsBr is smaller than RbBr and NaCl. NaCl is smaller than RbBr and CsBr. The ions in CsBr and RbBr are +2 and ?2; whereas in NaCl they are +1 and ?1. The ions in CsBr and NaCl are +2 and ?2; whereas in RbBr they are +1 and ?1. The Cs cation is larger than the Rb cation. The Na cation is larger than the Cs cation. (b) BaO > KF The ions in KF are +2 and ?2; whereas in BaO they are +1 and ?1. Fluorine is less electronegative than oxygen. The atomic radii of Ba and O are smaller than those of K and F. The atomic mass of K and F are larger than those of Ba and O. The ions in BaO are +2 and ?2; whereas in KF they are +1 and ?1. (c) SrO > SrCl2 The oxide ion is bigger than the chloride ion. The oxide ion has a ?2 charge; whereas the chloride ion is ?1. The oxide ion is smaller than the chloride ion. The oxide ion is less electronegative than the chloride ion. The oxide ion has a ?1 charge; whereas the chloride ion is?

Reference no: EM13163358

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