Write the ground-state electron configurations of the following transition metal ions. (a) Sc3 (b) Cr3 (c) Cu (d) Au

Full electron configuration is shown in the  image attached

Explanation:

In writing electron configuration for ions we first have to know the atomic number of the element. This will tell us the number of electrons in the neutral atom. Then we proceed to remove or add the number of electrons shown by the magnitude of charge on the ion. Then write the electron configuration following this new number of electrons.

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.