Draw Lewis structures for the acetonitrile molecule (CH3CN), the methylamine molecule (CH3NH2), and the methanimine molecule (CH2NH) in the window below, and then answer the questions that follow. (Draw one structure per sketcher box, and separate added sketcher boxes with the + sign. Do not include overall ion charges or formal charges in your drawing. Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule.)

i look it up online and i'll tell you

what are the choices?

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.