Charge is exactly what it says, the number of positive or negative charges carried by a species, so as you say the oxide ion carries a charge of 2-. Oxidation state is a more general idea which helps us when thinking about redox. It is the charge which the atom would carry if the bond were ionic. Many bonds are not ionic, but covalent, yet one partner in the bond may be considered more positive and the other more negative. For instance, in the permanganate ion, MnO4- (where the 4 should be a subscript and the minus sign a superscript) the manganese is bonded with a lot of oxygen. If the internal bonds were ionic, the manganese would carry a charge of +7. In MnO2, it would only carry +4, so we say the manganese is less oxidised in MnO2. Oxidation state is the formal charge carried by an atom. It can be used for either ionic or covalent compounds and helps us to keep track of what electrons are doing in a reaction. If the compound contains only simple ions it's the same thing as the charge, but if we are looking at a covalent substance, (and remember that polyatomic ions like permanganate contain covalent bonds within them), then it's only an idea in our heads. Note that it's usual to put the sign first for an oxidation number and second for a charge. Thus we say the charge on an oxide ion is 2-, but it's in the -2 oxidation state.
Terminal oxidation is oxidation on the end of a molecule. An example would be oxidation of a terminal carbon atom in a carbon chain.
the difference between carbon and carbon dioxide is carbon is just carbon
The oxidation state of carbon in CH3OH is 4
Carbon has +2 oxidation number in Carbon monoxide. It gets this oxidation number when it loses or shares two electrons.
The difference is the way they obtain energy. Chemotrophs are organisms that obtain energy by the oxidation of electron donors in their environments. These molecules can be organic (chemoorganotrophs) or inorganic (chemolithotrophs). Photoheterotrophs are heterotrophic organisms that use light for energy, but cannot use carbon dioxide as their sole carbon source.
In lesser terms, oxidation is when a rock or mineral of some sort interacts with oxygen and carbonation is when a rock or mineral interacts with carbon or carbon dioxide.
In lesser terms, oxidation is when a rock or mineral of some sort interacts with oxygen and carbonation is when a rock or mineral interacts with carbon or carbon dioxide.
Terminal oxidation is oxidation on the end of a molecule. An example would be oxidation of a terminal carbon atom in a carbon chain.
KCo3
the difference between carbon and carbon dioxide is carbon is just carbon
The oxidation state of carbon in CH3OH is 4
Carbon has +2 oxidation number in Carbon monoxide. It gets this oxidation number when it loses or shares two electrons.
The difference is the way they obtain energy. Chemotrophs are organisms that obtain energy by the oxidation of electron donors in their environments. These molecules can be organic (chemoorganotrophs) or inorganic (chemolithotrophs). Photoheterotrophs are heterotrophic organisms that use light for energy, but cannot use carbon dioxide as their sole carbon source.
I believe K2CO3.
0 oxidation state
Valence is how many bonds an atom can form. Oxidation number can be though of as being similar to the charge on an ion, and is based on the difference in electronegativity between bonded atoms. If something is bonded to a more electronegative element, its oxidation state is positive, and if it is with a less electronegative on the state is positive. In a neutral substance the sum of the oxidation states is always zero. Valence and oxidation states are related, though.Example: In formaldehyde (CH2O) hydrogen has a valence of 1, oxygen a valence of 2, and carbon a valence of 4. Carbon is more electronegative than hydrogen, and less electronegative than oxygen. As a result, each hydrogen atom has an oxidation state of 1+ and the oxygen is in the 2- oxidation state. This puts carbon in an oxidation state of 0.
because carbon graphite had carbon but graphite does not have carbon