Problem 11
Determine the net molecular dipole of each species: a) \(\mathrm{BF}_{3}\) b) \(\mathrm{NH}_{3}\)
Problem 12
Estimate the enthalpy change for this reaction. Start by drawing the Lewis electron dot diagrams for each substance. \(4 \mathrm{NH}_{3}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{~N}_{2}+6 \mathrm{H}_{2} \mathrm{O}\)
Problem 12
Which ionic compound has the higher lattice energy-KI or LiF? Why?
Problem 12
Draw the Lewis electron dot diagram for each ion. a) \(\mathrm{H}^{+}\) b) \(\mathrm{H}^{-}\)
Problem 12
Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed. a) \(\mathrm{CN}^{-}\) b) \(\mathrm{C}_{2} \mathrm{Cl}_{2}\) (assume two central atoms)
Problem 13
Which ionic compound has the higher lattice energy-BaS or MgO? Why?
Problem 13
Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed. a) \(\mathrm{CS}_{2}\) b) \(\mathrm{NH}_{2} \mathrm{CONH}_{2}\) (assume that the \(\mathrm{N}\) and \(\mathrm{C}\) atoms are the central atoms)
Problem 13
Ethylene ( \(\mathrm{C}_{2} \mathrm{H}_{4}\) ) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.
Problem 14
Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed. a) \(\mathrm{POCl}\) b) \(\mathrm{HCOOH}\) (assume that the \(\mathrm{C}\) atom and one \(\mathrm{O}\) atom are the central atoms)
Problem 14
Which ionic compound has the higher lattice energy - \(\mathrm{NaCl}\) or NaI? Why?
