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Chemical Bonding and Molecular Structure
Define lattice enthalpy. How is it violated to the stability of an ionic compound?
The lattice enthalpy (lattice energy) of an ionic solid is defined as the enthalpy required to completely separate one mole of a solid ionic compound into gaseous constituent ions. e.g. the lattice enthalpy of NaCl is 788 kJ mol–1. This means that 788 kJ of enthalpy is required to separate an infinite distance I mol of solid NaCl into 1 mol of Na+ (s) and one mole of Cl– (g).
The greater the lattice enthalpy, more stable is the ionic compound.
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Two elements A and B have the electronic configuration as:
A = 1s22s22p63s2 and B = 1s22s22p5
Write the empirical formula of the substance containing A and B.
What type of bonding would you expect between:
(i) a metal and a non-metal
(ii) a non-metal and another non-metal?
Give reasons in one or two sentences for the observation that in their compounds non-metals form anions and not cations.
Out of Na and K, which will form a more stable ionic bond?
Which will have a greater lattice enthalpy: NaCl or MgO?
Is a covalent molecule always formed between two similar atoms?
Why sodium chloride is a solid whereas carbon tetrachloride is a liquid?
Why NaCl gives a white percipitate with AgNO3 solution but CCl4 does not?
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