Chemistry Set 1

Group One are all metals.

They form positive ions, with each having a +1 charge.

For example, potassium would be K+.

Similarly, Sodium would be Na+.

Therefore, although each of the metals in group one get more and more reactive as we go down the group, every element in the group has a +1 charge on It.

Questions-

What does group one consist of?

Are the ions of this group positive, negative, or neutral?

What is the charge of Francium?

As with group one, group two consists solely of metals.
They also from positive ions. However, they possess a charge of +2.
For example, Calcium would be Ca2+
Following the same rule, Barium is Ba2+

Questions-

What is the charge on Group Two metals?

What is the symbol for magnesium?

What is Magnesium's symbol including the charge?

Group 7, the Halides, are relatively inert non-metals.
They form negative ions, with a -1 charge on them.
For example, Chlorine/Chloride is Cl-
Following this rule, bromine/bromide is Br-
Again, the fact that the Halides get less inert as you scroll down group seven has no effect on it's charge,

Questions-

What do the negative ions end In? (Word-wise)

What is the charge of a halide?

What is the charge on Fluorine/Fluoride?

Group six also consist if non-metal elements.
They, also, from negative ions which also end in -ide.
They have a -2 charge upon them.
Therefore, Oxygen's charge is O2-
Similarly, Sulfur's charge is S2-

Questions-

What charge do group six possess?

What is the charge on the element arsenic?

Aluminium is a metal, used in everyday life.
It forms positive ions.
These ions have a +3 charge.
This means that Aluminium's charge is Al3+

Questions-

What is Aluminium's symbol?

Furthermore, what is it's symbol including it's relative charge?

There are seven ions whom's names and formulae need to be remembered.

They are -

The Ammonium Ion, formulae being NH4+
Zinc, formulae being Zn2+
Silver, formulae being Ag+
Sulphate, formulae being SO4 2-
Nitrate, formulae being NO3-
Carbonate, formulae being CO3 2-
Hydroxide, formulae being OH-