Oxidation Numbers

The oxidation number for Br in BrO3 is +5. This is because the overall charge of the BrO3 molecule is -1, and the oxygen atoms have an oxidation number of -2 each. Therefore, the oxidation number of Br must be calculated as +5 to balance the charges.

An oxidation number of -1 means that the element has gained one electron, indicating that it is in its reduced state (has undergone reduction). This often occurs when an element gains an electron to achieve a stable electron configuration.

The oxidation number for fluorine is -1.

Noble gases, also known as group 18 elements, will never have an oxidation number because they have a full valence shell of electrons, making them very stable and unreactive.

The oxidation number of an atom indicates the number of electrons it has gained, lost, or shared to reach a stable configuration. It provides information on an atom's electron distribution and helps predict its reactivity in chemical reactions.

The oxidation number of phosphorus in white phosphorus is 0.

Oxidation numbers generally increase from left to right on the periodic table. This is because elements on the left side have fewer valence electrons and are more likely to lose electrons (becoming more positive), while elements on the right side have more valence electrons and are more likely to gain electrons (becoming more negative).

The oxidation number of an element is the charge that atom has when it forms ions. The oxidation number varies depending on the compound the element is in. There isn't a strict rule for the oxidation numbers of the first twenty elements as they can exhibit various oxidation states depending on the specific compound they are present in.

Hydrogen chloride (HCl) is a covalent compound, where hydrogen typically has an oxidation number of +1 and chlorine has an oxidation number of -1.

The oxidation number of hydroxide (OH-) is -1. This is because oxygen typically has an oxidation number of -2, and hydrogen has an oxidation number of +1. In this case, there is one oxygen atom and one hydrogen atom, resulting in an overall oxidation number of -1.

The oxidation number of sulfur in H2SO4 is +6. This is determined by balancing the overall charge of the compound, which is 0, and taking into account the known oxidation numbers for hydrogen (+1) and oxygen (-2).

The oxidation number for lithium is +1 and for oxygen is -2. In lithium oxide (Li2O), lithium has an oxidation number of +1 and oxygen has an oxidation number of -2. Therefore, the change in oxidation number for lithium oxide is -1 for lithium.

Lithium typically exhibits an oxidation number of +1, as it tends to lose one electron to form a stable cation.

The oxidation number of vinegar, or acetic acid, is +3 for the carbon atom in the carboxyl group (-COOH) and -2 for the oxygen atoms in the molecule.

The oxidation number of manganese in 1 mole of permanganate (MnO4-) is +7. Each oxygen atom has a charge of -2 and the overall charge of the ion is -1, so the oxidation number of manganese can be calculated as +7.

A monatomic ion is an ion consisting of a single atom with a positive or negative charge. The oxidation number of a monatomic ion is equal to the charge of the ion.

Elements in the same group have similar chemical properties because they have the same number of valence electrons. This leads to similar reactivity and tendency to form compounds with the same oxidation number. The oxidation number is related to the number of electrons an atom gains, loses, or shares to reach a stable electron configuration.

The oxidation number of C in C₂O₄ is +3. Each oxygen atom carries a charge of -2, and since there are 4 oxygen atoms in total with a total charge of -8, the carbon atom's oxidation number must be +3 to balance the charges in the compound.

The oxidation number of an element tells you the charge that the element would have if electrons were transferred completely during the formation of a compound. It can help to determine the type of chemical reactions that an element is likely to undergo.

oxidation number is defined as a positive or negative number corresponding to the charge that an atom in a molecule or ion would have if the electron pairs belonged entirely to the more electronegative atom.

in this case, they're talking about 'valance electrons'. An example would be...fluorine has 7 valance electrons. when bonded with another element, it would in almost all of the cases want to gain 1 more electron to have a full valance shell of 8 electrons. Therefore, it would become F -1

As a result, fluorine's oxidation number becomes -1, the same as its CHARGE when bonded to ANOTHER element (NOT ITSELF)

when fluorine bonds to itself to become Fluorine gas, its oxidation number is zero. that goes for all ....elements which bond with itself to form a diatomic molecule (oxygen gas, hydrogen gas, etc)

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The oxidation number of nitrogen (N) in Ca3N2 is -3. This is because calcium (Ca) has an oxidation state of +2, and the overall compound is neutral, so the oxidation states must balance out to zero. Since there are three Ca atoms with an oxidation state of +2, the nitrogen atoms must have an oxidation state of -3 to balance the charges.

The oxidation number of hydrogen in hypochlorous acid (HClO) is +1. In this compound, chlorine has an oxidation number of +1 and oxygen has an oxidation number of -2. To determine the oxidation number of hydrogen, we can set up an equation where the sum of the oxidation numbers equals the charge of the molecule, which in this case is zero.

The oxidation number of nitrogen in N2O3 is +3. This can be determined by assigning a −2 oxidation number to each oxygen atom and setting up the equation 2x + 3(-2) = 0, where x is the oxidation number of nitrogen. This gives x = +3.

Oxidation numbers indicate the charge that an atom has when it gains or loses electrons in a compound or ion. They help determine how the electrons are distributed within a molecule and are useful in balancing chemical equations and predicting reaction outcomes.