What element does the following electron configuration represent?

Rubidium (Rb).

Explanation:

From the question given above, the following data were obtained:

Electronic configuration => 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹

Name of element =?

To know the name of the element with the above electronic configuration, we shall determine the atomic number of the element. This can be obtained as follow:

Number of electrons = 2 + 2 + 6 + 2 + 6 + 2 + 10 + 6 + 1

Number of electrons = 37

Next, we shall determine the number of protons. This can be obtained as follow:

From the question given above, the element has no charge. Hence the element contains equal numbers of protons and electrons.

Number of electrons = 37

Number of protons = number of electrons = 37

Next, we shall determine the atomic number. This can be obtained as follow:

The atomic number of an element is simply defined as the number of protons present in the atom of the element. Thus,

Atomic number = proton number

Proton is = 37

Therefore,

Atomic number = 37

Finally, we shall determine the name of the element by comparing the atomic number of those in the periodic table.

Thus, the element with the above electronic configuration is Rubidium (Rb) since no two elements have the same atomic number

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

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~ trueboss72