Ag +1, O (2 x 3-), N 5 +
the oxidation states are always 0 for both atoms
0 oxidation state
If you mean a reaction of AgNO3 + Na(s) ==> NaNO3 + Ag(s), there would be ONE electron transferred.Ag^+ + 1e- ==> Ag(s) Reduction reaction Na(s) ==> Na^+ + 1e- Oxidation reaction
-1 oxidation state
In a compound the sum of oxidation states of the elements contained is zero.E1 + E2 + ... = 0If you know the oxidation states of the elements E1... you can calculate the oxidation state of the element E2.
In AgNO3, since Ag is in Group 1A, it always has a +1 oxidation state. Oxygen is typically -2, so the sum of the oxidation states must equal the overall charge of the compound, which is 0 for AgNO3. Therefore, N must have an oxidation state of +5 to balance out the charges.
In Ag NO3 the oxidation number of Ag (Silver) is 1+, the oxidation number of N (Nitrogen) is 5+, and the oxidation number of O (Oxygen) is 2-.
In this reaction, silver (Ag) has been oxidized. This is because silver changes from an oxidation state of 0 in Ag metal to an oxidation state of +1 in AgNO3. Oxidation involves the loss of electrons.
AgNO3. +1 for Ag, +5 for N, -2 for each O
To find the sum of the oxidation states in a compound, we rely on the principle that the overall charge of the compound is zero. In this case, the oxidation state of hydrogen is +1, oxygen is -2 (except in peroxides), and we denote antimony as x. The compound is neutral, so the sum of the oxidation states must be equal to zero. Using these rules, we have 2(+1) + x + 3(-2) = 0. Solving, we find that x = +5.
Metals that exhibit multiple oxidation states can have different levels of positive charge, known as oxidation states. These can vary depending on the compound the metal is in. For example, iron can have oxidation states of 2 and 3.
0, 1 and 2 oxidation states
In AgNO3, silver (Ag) has an oxidation number of +1, nitrogen (N) has an oxidation number of +5, and oxygen (O) has an oxidation number of -2. This is because the overall compound is neutral, so the sum of the oxidation numbers must equal zero.
To find the mass of silver in 3.4g of AgNO3, you need to consider the molar mass of silver nitrate (AgNO3). The molar mass of AgNO3 is 169.87 g/mol. Since the molar ratio of Ag to AgNO3 is 1:1, the mass of silver in 3.4g of AgNO3 would be 3.4g * (1/169.87) ≈ 0.02g.
To find the number of moles, you need to divide the given mass (85 grams) by the molar mass of AgNO3 (169.87 g/mol). 85 grams of AgNO3 represents 0.500 moles.
To find the oxidation number of chlorine, consider that chlorine typically has an oxidation number of -1 in its compounds. However, in certain situations, such as when bonded with oxygen or other halogens, chlorine can have different oxidation states. It's important to follow the usual oxidation number rules and balance the charges in the compound to determine the oxidation number of chlorine.
Oxidation number is oxidation states of an element. It can be positive or negative.