Calculate the oxidation number of the indicated atoms in the following reaction.

검증된 단계별 안내

Identify the atoms in the reaction for which you need to calculate the oxidation numbers. Typically, these are the atoms that undergo a change in oxidation state during the reaction.

Recall the general rules for assigning oxidation numbers: (1) The oxidation number of an atom in its elemental form is 0. (2) For monoatomic ions, the oxidation number is equal to the charge of the ion. (3) Oxygen usually has an oxidation number of -2, and hydrogen usually has +1. (4) The sum of oxidation numbers in a neutral compound is 0, and in a polyatomic ion, it is equal to the ion's charge.

Apply these rules to assign oxidation numbers to each atom in the reactants and products. Start with atoms that have known oxidation states, such as oxygen and hydrogen, to help deduce the oxidation states of other atoms.

Compare the oxidation numbers of the indicated atoms in the reactants and products. Determine if there is an increase or decrease in the oxidation number, which indicates oxidation or reduction, respectively.

Summarize the changes in oxidation numbers to identify which atoms are oxidized and which are reduced. This will help in understanding the redox process occurring in the reaction.

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Oxidation Number

The oxidation number, or oxidation state, is a theoretical charge assigned to an atom in a molecule or ion, reflecting its degree of oxidation. It helps in tracking electron transfer in redox reactions. The rules for determining oxidation numbers include assigning -2 to oxygen, +1 to hydrogen, and using the charge of ions to deduce the oxidation states of other elements.

Redox Reactions

Redox reactions involve the transfer of electrons between two species, leading to changes in their oxidation states. Oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. Understanding redox reactions is crucial for calculating oxidation numbers, as it helps identify which atoms are oxidized and which are reduced.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is equal on both sides of the reaction, maintaining the law of conservation of mass. In redox reactions, balancing also involves ensuring that the total increase in oxidation numbers equals the total decrease, which is essential for accurately determining the oxidation states of atoms.