From your pre$-$class reading, complete this set of instructions to determine what IM force is present in a given molecule by adding missing words or choosing the correct of two choices.

a$.$ This IM force exists between ALL molecules, regardless of polarity, and arises because of attractions between instantaneous dipoles and induced dipoles. The strength of this force depends on the polarizability of a molecule which is determined in part by its number of electrons $-$ more electrons $=$ STRONGER$/$WEAKER force. Type of IM force$=$

b$.$ Draw the Lewis structure and find the molecular geometry of the molecule to determine whether the molecule is POLAR: if polar, it will have this type of IM force: $\_$

A more polar molecule will have STRONGER$/$WEAKER force.

c$.$ This IM force is an especially strong example of the type of IM force in b above, so strong that it is considered a separate category of IM force. For this IM force to be present between molecules, there must be a hydrogen bonded to a very electronegative atom, such as and there must be a very electronegative atom with at least $1$ lone pair of electrons to act as an acceptor. Type of IM force $=$ The strength of this force depends on

d$.$ This IM force occurs when an ionic compound is mixed with a polar compound, like water: