Which two electron configurations represent elements that would have similar chemical properties? (1) 1s22s22p4 (2) 1s22s22p5 (3) [ar]4s23d5 (4) [ar]4s23d104p5?

Two electron configurations of elements that would have similar chemical properties are (2) and (4).

Explanation:

(1)

(2)

(3)

(4)

Valence electrons : These are the electrons present in last principal quantum number of an atom of the element.

Two electron configurations represent elements that would have similar chemical properties are (2) and (4). This is because number of valence electrons present in both of them are same that is seven valence electrons . Also valence electrons of both the elements are present in p-orbital which means that they both belongs to same group  in a periodic table. The members of same group in a periodic table have similar chemical properties.

i don't know people like to fight everywhere rip.

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.