Help to answer this please

Question

A certain isotope has an atomic number of 16, a mass number of 37, and 16 electrons.

What element is this isotope? 

What is the charge on the isotope? 

How many neutrons does the nucleus of this isotope have?

Answer 1

The number of PROTONS (atomic number) always tells you the identity of the element

The element is SULFUR (S)

The charge on the isotope is the difference between the number of positive charges (protons) and the number of negative charges (electrons. Here we have equal numbers of protons (16) and electrons (16) so the charge is zero.

The atomic mass/mass number (37) is the sum of the protons and the neutrons. Thus, number of neutrons is mass number minus the number of protons. This is 37 - 16 = 21 neutrons

Answer 2

Sulfur-37 is a radioactive isotope of Sulfur with 16 protons, 16 electrons and 21 neutrons. It is neutrally charged

37-16 = 21 neutrons.

subtract the number of protons from the atomic mass to get the number of neutrons

actual atomic mass is 36.9711257, rounded off to 37

Pauling electronegativey for sulfur = 2.58

Anderson electronegativity for sulfur = 2.96