When you balance a redox equation using the half-reaction method, what do you do after you write the oxidation and reduction half-reactions? OA Determine the oxidation numbers for the elements. OB. Balance the atoms and charges. Add back in any spectator ions. O D. Add the two half-reactions to show the overall redox equation. O E Use a coefficient to make the number of electrons lost equal the number of electrons gained.

14,16 18 reacts with group

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.