In the last lesson we learned about naming cations
which are positive ions notice i didn't use specific types
elements to determine the name of the ion but i used
the term cation that is a positive is a positive charged ion
now in this case you're going to use the term anions
which are use to identify negative ions
so here we are going to look at the name of an anion
so anions are basically
negative charged ions
now how do we name the negative charged ions
there are two things we need to do
first we drop the ending
of the element on the periodic table
second after we drop the ending we add -ide
to replace
that ending
so how does that work
we know that the majority of the anions on the periodic table
will form a negative anions because
all the elements from group 5A all the way to 7A
they all gain there electrons to be stable
so lets look at those elements specifically
here i zoom the first is in group 5A
where nitrogen what is the ending for nitrogen it turns
out to be -ogen so therefore we erase that and put -ide
the ions for nitrogen will be nitrite
that is when you have 3- we don't call it nitrogen anymore
formula for the ions of nitrogen which N^3-
this is called nitrite not nitrogen
now we go to phosphorus which will form
a P^3- ion so again this is the formula for the ions
so what's the ending for Phosphorous it turns out to be   -orus
and it's going to be of course add -ide so we have Phosphide
now going down here we have arsenic which will also form
a 3- charge As^3-
and what's the ending for it where going to draw -ic part
so therefore we add -ide to it and we have arsenide
so lets ignore the rest of the elements down here
at the bottom because they are acceptation to this rule
then we go to oxygen group 6A which they form a 2-
because it gains 2 electrons to be that way right to be stable
so in this case what's the ending for oxygen
just like nitrogen in this case oxygen is -gen
so we drop that and add -ide
and the formula for oxygen ion is 2-
so when you see O^2- we will say oxide not oxygen
what about Sulfur the formula for Sulfur ion is 2-
but we don't call it Sulfur ion
we drop the ending of Sulfur which is -ur and we add that -ide
so Sulfite so the formula for Sulfite is S^2-
and we also ignore Selenium for now lets go over here
here we have Fluorine in 7A which will gain 1 electron
to be stable and electrons are negative so therefore
we have a 1- charge what is the formula for Fluorine when it becomes an ion
so Fluorine is going to be F^1- or just F^- because
we ignore the 1 all the time
so what's the ending for Fluorine it turns out -ine
so it can be -ide Fluoride will be the name of the ion for Fluorine
what about Chlorine the ending is also the same as Fluorine
-ine which means we have Chloride
Chloride formula will look like Cl^1- or Cl^-
again sometimes we ignore the one
then we have Bromine of course the same ending as
Chlorine and Fluorine and we drop that ending and add   -ide
and what's the formula to Bromide which is the ions
of Bromine we have Br^1- or Br^- only
and lastly we have Iodine which is drop the same ending
so we have Iodide so what's the formula for Iodide
is basically I^1- or just I^-
what about group 8A if we zoom out
remember this group is a stable group and all the elements
want to have the Lewis Dot Structure of the Noble gas
which in this case Helium will look something like this
or the rest of Noble gases will look something like this
where they have a beautiful 8 valence electrons
that is the golden rule to be stable
and that's how you name negative ions on the periodic table
