Oxidation State numbers
For Fe3+ i got 3+ b/c Oxidation state monatomic ion = ionic charge and i got that answer wrong. i am receiving wrong answers for these below aswell.
I used these rules for the following
-Alkali metals are always +1; alkaline earths are always +2.
-Sum of oxidation states is zero for neutral compounds, and equal to the overall charge for polyatomic ionic species
CuCl2= Oxidation states of Cu? Cl2?
CO_2 Cu? O?
MnO_4^2- Mn? O
HSO_4^- H? So
+3 is correct for Fe^+3.
Cu in CuCl2 is +2.
Cl in CuCl2 is -1 each.
C in CO2 is +4; O is -2 each.
Mn in MnO4^- is +7; O is -2 each
H in HSO4^- is +1; SO4^-2 is -2; S is +6 and O is -2 each.
To determine the oxidation states of the elements in chemical compounds, you need to follow some rules and guidelines.
1. In many cases, alkali metals (Group 1) have an oxidation state of +1, and alkaline earth metals (Group 2) have an oxidation state of +2. However, there are some exceptions, so it's important to refer to reliable sources or periodic tables for specific elements.
2. In a neutral compound, the sum of the oxidation states of all the elements is zero. For polyatomic ions, the sum of the oxidation states is equal to the overall charge of the ion.
Let's apply these rules to the examples you provided:
1. CuCl2:
Since copper (Cu) is a transition metal, its oxidation state can vary. Let's assume it as "x." According to the rules, the total oxidation state of Cl2 is -2. Since there are two chloride ions (Cl^-) in the compound, their total oxidation state is -2. Therefore, the equation becomes:
x + 2(-1) = 0
x - 2 = 0
x = +2
So, the oxidation state of copper (Cu) in CuCl2 is +2.
2. CO2:
Oxygen (O) usually has an oxidation state of -2, and there are two oxygen atoms in CO2. Let's assume the oxidation state of carbon (C) as "y." The equation is:
y + 2(-2) = 0
y - 4 = 0
y = +4
Therefore, the oxidation state of carbon (C) in CO2 is +4.
3. MnO4^2-:
The overall charge of the ion is -2. The oxidation state of oxygen (O) is usually -2. Let's assume the oxidation state of manganese (Mn) as "z." The equation becomes:
z + 4(-2) = -2
z - 8 = -2
z = +6
Hence, the oxidation state of manganese (Mn) in MnO4^2- is +6.
4. HSO4^-:
The overall charge of the ion is -1. The oxidation state of oxygen (O) is usually -2. Let's assume the oxidation state of sulfur (S) as "w." The equation becomes:
w + 4(-2) + (-1) = -1
w - 8 - 1 = -1
w = +6
So, the oxidation state of sulfur (S) in HSO4^- is +6. The oxidation state of hydrogen (H) is generally +1, but it's best to confirm this using reliable sources.
Remember, these oxidation states are based on general trends, and exceptions can occur with certain elements or compounds. It's crucial to check specific rules or use reliable sources when dealing with unfamiliar compounds.