Talk:S-block

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This is the talk of s-block.

Wait for QD

A3:Has been copied and pasted from another Wikipedia: Any article or section from an article that has been copied and pasted with little or no change. I have made changes. You can see it! I think the reason why you put {{qd|a3|||}} is you saw the table. Actually, I asked it at WP:ST#On the s-block. --Kc kennylau (talk) 14:42, 16 February 2012 (UTC)

Copy-paste examples. The following are unsimplified copy-pastes. We've been down this road recently. QD, please. No need to wait.

• Among alkali metal cations, lithium has the smallest size and highest polarizing power. This separates lithium from its family members. Its covalence character is higher, which is responsible for its solubility in organic solvent.

• Diagonal relationship

Lithium and Beryllium, the first elements in group 1 and group 2 respectively, show some properties which are different from other from other members of their respective groups. In these anomalous properties they resemble the second element of the succeeding group. Thus lithium shows similarities to magnesium and beryllium to aluminum in many of their properties.

• This type of relationship in the periodic table is known as a Diagonal relationship. The diagonal relationship is due to the similarities in ionic sizes and charge/radius ratio of the element. The similarity between lithium and magnesium is due to their same sizes:

• Anomalous behaviour of lithium Lithium-the first element of group 1 differs from rest of this group in many respects. This anomalous behaviour of lithium is due to the following reasons: a. small size of lithium atom and its ion. b. higher polarization power of li+ (i.e charge size ratio) resulting in increased covalent character of its compounds which is responsible for their solubility in organic solvents c. comparatively high ionisation enthalpy and low electropositive character of lithium as compared to other alkali metals d. non availability of d-orbitals in its valence shell e. strong intermetallic bonding Some of the properties in which lithium differs from other members of its group illustrating its anomalous behaviour are as follows:

• Lithium is harder than sodium and potassium which are so soft that they can be cut by a knife. 2. The melting and boiling points of lithium are comparatively high. 3. Lithium forms monoxide with oxygen, other alkali form peroxide and superoxide. 4. Lithium combines with nitrogen to form nitrides, while other alkali metals do not. 5. Lithium Chloride is deliquescent and crystallizes as a hydrate LiCl.2H2O, whereas other alkali metal chlorides do not form hydrates.

End of comment. Gotanda (talk) 09:02, 17 February 2012 (UTC)

QD denied

This page has been copied from enwiki. There has been some work done to simplify the article. There is obviously quite a bit to go to get the article close to our standards. However, this is an important topic, the periodic table is studied at secondary school level, and so this article (when simplified further) will be of help to our readers. --Peterdownunder (talk) 11:40, 17 February 2012 (UTC)

History of abuse

@Bsadowski1 and Peterdownunder: Seems that this is getting spammed repeatedly. Can I recommend that it has some extended protection and/or watchlisting and/or AF on it. Thanks. Billinghurst (talk) 16:20, 1 August 2021 (UTC)

Semi-protected and on my watchlist now. `Peterdownunder (talk) 03:54, 6 August 2021 (UTC)