What are the formal charges on the sulfur (S), carbon (C), and nitrogen (N) atoms, respectively, in the resonance structure that contributes most to the stabilit thiocyanate ion, SCN-? A Lewis structure for the thiocyanate ion. The possible resonance structures for the thiocyanate ion, SCN-, are [S=C=N]¹ Structure A Express your answers as integers separated by commas. ►View Available Hint(s) -1 formal charge on sulfur (S), carbon (C) and nitrogen (N) atoms = [:S-C=N] [:S=C-N:]¹ Structure B Structure C

Inert xenon actually forms many compounds, especially with highly electronegative fluorine. 0 The AH values for xenon difluoride, tetrafluoride, and hexafluoride are -105, -284, and f -402 kJ/mol, respectively. Find the average bond energy of the Xe- -F bonds in each fluoride. Xenon difluoride kJ/mol Xenon tetrafluoride kJ/mol Xenon hexafluoride kJ/mol

The formal charge on sulfur in the following structure is: :0: || +1 -2 0. +2 IO O 0 E

If the following reaction is given: C2H5F + Cl2 || AHran If the bond energy for C-H is 414 kJ/ mole, the bond energy for C-C is 347 kJ/mole, the bond energy for C-Cl is 377 kJ/ mole, the bond energy for Cl-Cl is 243 kJ/ mole, the bond energy for C-F is 450 kJ/ mole and the done energy for H-Cl is 431 kJ/ mole, determine the bond energy for the H-F bond in kJ/mole. C2H4Cl2 + HF 151kJ mole Give your answer as a positive value as all energies for bond values should be written in terms of a positive value (the energy needed to break the bond = endothermic)