Y mandeleev was not able to classify the position of hydrogen in periodic table?

Question

Answer

No fixed position could be given to Hydrogen in periodic table. Mendeleev placed Hydrogen in both 1st and 7th group. Its properties resemble with both Alkali metals and Halogens. Because, Hydrogen can loose one electron (e-) like alkali and gain 1e- like halogens.

Answer

Because it forms positive Ion as HCL and negative Ion as NaH

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The position of hydrogen is unsatisfactory in Mendeleev's periodic table. It was placed with Cu, Ag Au ,etc. Hydrogen is a metal which shows resemblance with halogenslike Cl, F, etc and with alkali metalslike Na, K, etc. That is why no fixed position was given to hydrogen in Mendeleev's periodic table.

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The position of hydrogen in periodic table is not fixed because it shows properties of 1st group as well as 17th group elements, that's why it has not given any fixed place inside periodic table. so it is present just above first group.

Answer

**The Classification of Hydrogen in the Periodic Table**

**Introduction:**
The periodic table is a systematic arrangement of elements based on their atomic number, electron configuration, and chemical properties. It provides a comprehensive framework for organizing and understanding the properties of elements. However, the placement of hydrogen in the periodic table has been a topic of debate and controversy.

**The Dilemma of Hydrogen:**
Hydrogen is the most abundant element in the universe, constituting approximately 75% of its elemental mass. It is also the lightest element, with only one proton and one electron. Due to its unique characteristics, the classification of hydrogen has been challenging.

**1. Hydrogen's Electron Configuration:**
The position of an element in the periodic table is primarily determined by its electron configuration and the similarities it shares with neighboring elements. Hydrogen has one electron, which it can either gain or lose to achieve a stable electron configuration. This flexibility in electron configuration makes it difficult to classify hydrogen with other elements in a specific group or period.

**2. Similarities with Alkali Metals:**
Hydrogen shares some similarities with the alkali metals, such as lithium, sodium, and potassium, as they all have one valence electron. However, hydrogen also exhibits unique properties that set it apart from the alkali metals. For example, hydrogen can exist as a diatomic molecule (H2) and display both metallic and non-metallic properties. This further complicates its classification.

**3. Similarities with Halogens:**
Hydrogen also bears some resemblance to the halogens, such as chlorine and fluorine, as they have similar electron configurations and can form compounds by gaining one electron. However, hydrogen's ability to lose an electron and exhibit metallic properties differentiates it from the halogens.

**4. Placement in the Periodic Table:**
Given the challenges in classifying hydrogen, it is typically placed separately above the alkali metals in the periodic table. This positioning acknowledges its unique properties while still recognizing its similarities with alkali metals and halogens. Placing hydrogen in a specific group or period would not accurately represent its diverse characteristics.

**Conclusion:**
In conclusion, the classification of hydrogen in the periodic table is complex due to its unique electron configuration and diverse properties. While it shares similarities with both alkali metals and halogens, it also possesses distinct characteristics that set it apart. As a result, hydrogen is typically placed separately in the periodic table to reflect its individuality.

Answer

Similar Class 10 Doubts

Choose the incorrect statement in view of Mendeleev’s Periodic Table.

Why could no fixed position be given to hydrogen in Mendeleev's periodic table?

Why hydrogen does not given fix place in mendeleevs periodic table?

Hydrogen occupies a unique position in the Modern Periodic Table”. Justify .?

Hydrogen occupies a unique position in Modern Periodic Table”. Justify the statement.

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