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The compound name for CuSO4 is Copper (II) Sulfate. Here's a step-by-step explanation of how we arrive at this name:
Step 1: Identify the elements present in the compound. In CuSO4, we have Copper (Cu), Sulfur (S), and Oxygen (O).
Step 2: Determine the oxidation state of the metal. In this case, Copper (Cu) is the metal. The Roman numeral in parentheses after the name of the metal indicates its oxidation state. In CuSO4, Copper has an oxidation state of +2. This is because Sulfate (SO4) has a charge of -2, and the compound overall is neutral. Therefore, Copper must have a charge of +2 to balance out the -2 charge from Sulfate.
Step 1: Identify the elements present in the compound. In CuSO4, we have Copper (Cu), Sulfur (S), and Oxygen (O).
Step 2: Determine the oxidation state of the metal. In this case, Copper (Cu) is the metal. The Roman numeral in parentheses after the name of the metal indicates its oxidation state. In CuSO4, Copper has an oxidation state of +2. This is because Sulfate (SO4) has a charge of -2, and the compound overall is neutral. Therefore, Copper must have a charge of +2 to balance out the -2 charge from Sulfate.
Step 2: Determine the oxidation state of the metal. In this case, Copper (Cu) is the metal. The Roman numeral in parentheses after the name of the metal indicates its oxidation state. In CuSO4, Copper has an oxidation state of +2. This is because Sulfate (SO4) has a charge of -2, and the compound overall is neutral. Therefore, Copper must have a charge of +2 to balance out the -2 charge from Sulfate.
Step 3: Name the non-metal. The non-metal in this compound is Sulfate (SO4). When Oxygen is combined with another element to form a compound, the ending of the other element's name is often changed to "-ate" or "-ite". In this case, Sulfur (S) becomes "Sulfate".
Step 4: Combine the names. The name of the metal is written first, followed by the name of the non-metal. Therefore, the name of the compound CuSO4 is "Copper (II) Sulfate".
In conclusion, the compound name for CuSO4 is Copper (II) Sulfate. This name indicates that the compound is made up of Copper ions with a +2 charge and Sulfate ions with a -2 charge.
Step 3: Name the non-metal. The non-metal in this compound is Sulfate (SO4). When Oxygen is combined with another element to form a compound, the ending of the other element's name is often changed to "-ate" or "-ite". In this case, Sulfur (S) becomes "Sulfate".
Step 4: Combine the names. The name of the metal is written first, followed by the name of the non-metal. Therefore, the name of the compound CuSO4 is "Copper (II) Sulfate".
In conclusion, the compound name for CuSO4 is Copper (II) Sulfate. This name indicates that the compound is made up of Copper ions with a +2 charge and Sulfate ions with a -2 charge.
Naming inorganic compounds 1
Naming inorganic compounds 2
Exercise 2 - Name the following inorganic compounds: a. HI (aq) b. NiCr₂O₇ c.Al(ClO₄)₃ d. HNO₂(aq)
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Naming inorganic compounds 1
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In this video and in the next one,
we'll learn about the names and formulas of inorganic compounds.
Let's begin with a binary compounds of metals and nonmetals.
A binary compound involves 2 elements, that's the binary.
Binary compounds of a metal and non-metal are ionic compounds,
and they consist of a metal cation and a non-metal anion.
We write the name of the metal first and then the name of
the non-metal with the suffix ide.
Instead of chlorine, we'll have chloride.
We should note throughout and always check that the compound is electrically neutral.
Many metal ions have only one possibility,
that means there's only one oxidation state.
These include lithium plus, sodium plus,
potassium plus, rubidium plus,
cesium plus, magnesium 2 plus,
calcium 2 plus,
strontium 2 plus,
barium 2 plus,
aluminum 3 plus,
zinc 2 plus,
silver plus, and gold plus.
However, there are other metals that have more than one possibility.
That means there's more than one oxidation state.
For example, chromium can be 2 plus or 3 plus,
iron can be 2 plus or 3 plus,
cobalt can be 2 plus or 3 plus,
copper can be plus or 2 plus,
mercury can have 2 mercury atoms together,
Hg_2 and that's 2 plus or just one mercury atom Hg 2 plus.
Tin can be 2 plus or 4 plus,
and lead can be 2 plus or 4 plus.
Now there are far fewer nonmetal ions.
We have H minus,
that's called hydride, F minus,
fluoride, Cl minus,
chloride, Br minus, bromide,
I minus, iodide,
O 2 minus,
that's oxide, S^2 minus,
sulfide, N^3 minus nitrite.
Let's take some examples.
Here's one that you're very familiar with.
NaCl is sodium chloride, MgO,
magnesium oxide, Al_2O_3 aluminum oxide.
We can check that this is the correct formula.
Al is 3 plus,
that's 2 times 3 plus and oxygen is 2 minus,
that's 3 times 2 minus,
so we have plus 6 plus minus 6,
which gives us 0.
So 6 plus minus 6 giving us 0.
Now, when we have the possibility of more than one oxidation state,
then we have to distinguish between the different oxidation states in the name.
For example, FeO, we write iron II.
We use the II oxide.
That means iron has a plus 2 oxidation state.
If it's Fe_2O_3,
that's iron III oxide,
that means iron has a plus 3 oxidation state.
Remember for ions, the oxidation state and the ionic charge are the same,
so it's Fe_2 plus an oxidation state plus 2.
Where we have Cu_2O,
that's copper I oxide,
that means copper has the oxidation state of plus 1,
and CuO, that's copper II oxide,
that means copper has the oxidation state of plus 2.
Now we go on to the binary compounds of 2 nonmetals.
These are molecular compounds consisting of 2 nonmetals before we add ionic compounds.
We write the name of the element with the positive oxidation state
first and then the name of the negative oxidation state,
and we again have the suffix ide.
Now, very often an element has several oxidation states,
and then we use prefixes.
Here's a list of them.
Greek if it come from Greek.
Mono, di,
tri, tetra, penta,
hexa, hepta, octa, nona, and deca.
I will have some examples,
for example, carbon monoxide.
Here the carbon has the oxidation state of plus 2.
We don't write usually,
mono carbon monoxide, we just leave it as carbon.
Here is carbon dioxide,
the 2 oxygens,
and the oxidation state of carbon is plus 4.
If we're given a formula,
we can always check what the oxidation state is,
because oxygen is minus 2 and carbon therefore must be plus 4.
Now nitrogen has a lot of possible oxidation states and here are a few examples.
Dinitrogen oxide, that's N_2O.
The oxidation state of N must be plus 1.
NO_2 nitrogen dioxide.
The oxidation state of N must be plus 4.
N_2O_5 dinitrogen pentoxide.
The oxidation state here of N is plus 5.
We can check if that's correct.
There are 2 nitrogens,
so it's 2 times 5 and 5 oxygens,
so that's 5 times minus 2.
That gives us 10 plus,
minus 10 total of 0.
Now we get to phosphorus.
We can have phosphorus trichloride, PCl_3,
where the oxidation state of the phosphorus is plus 3 and PCl_5,
that's phosphorous pentachloride, where the oxidation states of phosphorus is plus 5.
Now we go into binary acids.
Binary acid is a compound consisting of hydrogen and a non-metal in an aqueous solution.
We write the prefix hydro,
followed by the name of the non-metal with the suffix ic.
Here's some examples.
HF is hydrofluoric acid,
HBr is hydrobromic acid, HCl,
with which you're all familiar,
is hydrochloric acid,
HI is hydroiodic acid,
H_2S is hydrosulfuric acid.
You have to remember all of these are in aqueous media,
they're all in water.
In this video, we talked about the names of inorganic compounds,
and we'll continue this in the next video.
This video provides an overview of the names and formulas of inorganic compounds. It begins with binary compounds of metals and nonmetals, which consist of a metal cation and a non-metal anion. The metal is written first, followed by the non-metal with the suffix “ide”. Many metal ions have only one oxidation state, while others have more than one. Nonmetal ions include hydride, fluoride, chloride, bromide, iodide, oxide, sulfide, and nitrite. Examples of binary compounds include sodium chloride, magnesium oxide, and aluminum oxide. Binary compounds of two nonmetals are molecular compounds, and the element with the positive oxidation state is written first. Prefixes are used to distinguish between different oxidation states. Examples of binary acids include hydrofluoric acid, hydrobromic acid, hydrochloric acid, hydroiodic acid, and hydrosulfuric acid.
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