Which neutral atom has the following electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2?

Answer 1

There are 56 electrons in this neutral atom, so it has 56 protons. That makes it to be element with atomic number 56, which is named Barium (Ba).
It is the fifth element in Group 2, a soft silvery metallicalkaline earth metal.

Answer 2

Because this ion is doubly positive, it means that when it is in a neutral state, it has two more electrons. This means the ground state is 1s2 2s2 2p6 3s2 3p6 3d8. This corresponds to nickel.

Answer 3

Counting the total number of electrons, one gets 38. This corresponds to Strontium. This is an s-block element in period 5 and group 2. Thus, it should have a 5s2 highest energy electron and it does. So, that fits.

Answer 4

The neutral atom with this electron configuration is Radon (Rn), which has a total of 86 electrons.

Answer 5

that would be delta 9 tetrahydracannibinol.

Answer 6

Delta 9 tetrahydracannibinol is the doubly positive ion. It contains the following ground-state electron configuration 1s2 2s2 2p6 3s2 3p6.

Answer 7

Well, I count 30 electrons so I look at my Periodic Table and I see that only Zinc fills the bill here.

Answer 8

This is for Zirconium, 40Zr.

Answer 9

Selenium.

Answer 10

Argon