Periodic Table Help?

Question

What is the nuclear symbol, and the charge for the element that has 16 protons, 16 neutrons, and 18 electrons.

Any help is greatly appreciated!!

Answer 1

The atomic number of an element is the exact same as the number of protons in the atom.

So, your element is Sulfur.

With 16 neutrons the mass number becomes 32, (16 protons+16 neutrons) and with 18 electrons, you have two more electrons than protons, making your charge -2.

Your nuclear symbol should be written as

32/16 S -2 with the 32 as a superscript on the left, the 16 below that on the left, and the -2 as a superscript on the right.

Answer 2

16 proton is sulfur. SInce there is more electrons, than protons, you have a negative ion.

S(2-)

Answer 3

It has 16 protons, which gives you the identity of the element.  The number of protons never changes for a given element.  The number of protons is also the atomic number.  So number 16 on your PT is Sulfur (S).  It has 16 neutrons.  To get the mass, add the protons and neutrons (32 here).  That number goes to the left of the element symbol in a superscript.  This is most commonly only written when you have to specify the isotope you are talking about, which isn't very often.

You have 18 electrons, which it two more than your protons.  So there are two extra negative charges.  This number goes to the right of the element symbol also in a superscript.

So you would have (superscript)32 S (superscript)2-, which is a lot easier to write in a more feature-friendly program (or by hand!).  Hope this helped.