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What is the difference between intermolecular forces and intramolecular forces? Which are stronger?

Draw the three-dimensional shape of methanol, \(\mathrm{CH}_{3} \mathrm{OH}\). Indicate the numeric value of all bond angles. Is this molecule polar? If so, draw the molecular dipole moment vector.

Explain the difference between electron-group geometry and molecular shape. How do you use electron-group geometry when deciding what shape a molecule has?

Which should have the largest dipole moment: \(\mathrm{O}_{3}, \mathrm{H}_{2} \mathrm{O}\), or \(\mathrm{OF}_{2} ?\)

Draw each ion or molecule showing its threedimensional shape and valence electrons. For each species, name the electron-group geometry around the central atom (or atoms) and the molecular shape. Indicate whether each species has a molecular dipole moment. If so, draw the dipole moment vector. (a) \(\mathrm{NCCN}\) (b) \(\mathrm{BF}_{4}\) (c) \(\mathrm{NClO}_{2}\) (d) \(\mathrm{SeH}_{2}\)

White phosphorus, \(\mathrm{P}_{4}\), consists of four phosphorus atoms, with each atom bonded to the other three. Draw the three-dimensional shape of this molecule, showing all valence electrons and bond angles. (Hint: Begin by drawing one atom bonded to the three others using VSEPR theory, and then make the remaining connections.)

Some molecules have central atoms with steric numbers greater than 4 . For example, the central sulfur atom in \(\mathrm{SF}_{6}\) has a steric number of 6 . Its actual geometry (called octahedral), is shown below (all the bond angles are \(90^{\circ}\) or \(180^{\circ}\) ). (a) Are the bonds in \(\mathrm{SF}_{6}\) polar, polar covalent, or ionic? Explain. (b) Would you predict the \(\mathrm{SF}_{6}\) molecule to be polar or nonpolar? Justify your answer.

One student claims \(\mathrm{XeF}_{4}\) will be polar. Another claims it will be nonpolar. Which is right, and why?

Is CIFs polar or nonpolar? Fully explain your answer.