The charge and identity of an ion with 16 protons, 18 electrons and 17 neutrons would be?
16 protons makes it sulfur. 18 electrons makes it a 2- charge. 17 neutrons makes mass number 33. Therefore this is
1633S=
That’s great
Well, if we do a little math, we can figure it out. We start with 16 protons, which gives us a positive charge of +16. Then we have 18 electrons, and since each electron carries a negative charge of -1, that gives us a total negative charge of -18. If we subtract the negative charge from the positive charge (+16 -18), we end up with a net charge of -2. So, the ion would have a charge of -2! As for the identity of this ion, I'm sorry to say it's not my area of expertise. Maybe it's an "Unidentifi-tron"? Just kidding, it's probably better known as an oxyanion of some element.
To determine the charge and identity of an ion with a given number of protons, electrons, and neutrons, we need to follow a few steps.
Step 1: Identify the element. Since the ion has 16 protons, its atomic number is 16. Using the periodic table, we can find that element 16 is sulfur (S).
Step 2: Determine the number of electrons in a neutral atom. Since the ion has 16 protons, which is also the atomic number, a neutral atom of sulfur would have 16 electrons.
Step 3: Calculate the number of electrons gained or lost. In this case, the ion has 18 electrons, while a neutral sulfur atom has 16 electrons. To determine the charge, we subtract the number of electrons lost from the number of electrons gained.
18 electrons - 16 electrons = +2 electrons
Since the ion has gained 2 more electrons than a neutral atom, it carries a charge of -2.
Step 4: Write the ion's charge and symbol. With a charge of -2 and the element being sulfur (S), we can write the ion as S2-. The negative sign indicates the gained electrons, making it an anion.
Therefore, the charge and identity of the ion with 16 protons, 18 electrons, and 17 neutrons is S2- (sulfide ion).