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Oxidation state trends in periodic table - Chemistry Video Lecture - Class 11

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FAQs on Oxidation state trends in periodic table - Chemistry Video Lecture - Class 11

1. What is an oxidation state?

Ans. An oxidation state, also known as oxidation number, is a concept in chemistry that represents the relative electron density of an atom within a compound or ion. It indicates the number of electrons that an atom has gained or lost in order to form a chemical bond.

2. How is the oxidation state of an element determined?

Ans. The oxidation state of an element is determined by assigning a set of rules to determine the distribution of electrons in a compound or ion. These rules include assigning a full negative charge to more electronegative elements, assigning positive charges to less electronegative elements, and considering the overall charge of the compound or ion.

3. What are the general trends in oxidation states across the periodic table?

Ans. The general trend in oxidation states across the periodic table is that elements tend to have higher oxidation states as you move from left to right across a period. This is because the number of valence electrons increases, leading to a greater likelihood of gaining or losing electrons to achieve a stable configuration. However, there are exceptions to this trend due to factors such as electron configuration and bonding characteristics.

4. How does the periodic table help predict oxidation states?

Ans. The periodic table provides a systematic arrangement of elements based on their electron configurations and properties. By analyzing the position of an element in the periodic table, you can make predictions about its tendency to gain or lose electrons and thus determine its possible oxidation states. Elements in the same group or column often have similar oxidation states due to similarities in their electron configurations.

5. Can oxidation states be negative?

Ans. Yes, oxidation states can be negative. A negative oxidation state indicates that an atom has gained electrons. This can occur when an atom forms a covalent bond with a more electronegative element and the electron density is shifted towards the more electronegative atom. Negative oxidation states are commonly seen in compounds such as hydrides (e.g., H-), where hydrogen gains an electron.

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Nov 14, 2024 Last updated

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