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Old 01-21-2007, 06:30 PM  
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The Beryllium Thread
I'm putting this in here so that it won't hang around the top of the lounge while I cut and paste information in to post after post.

This is part of my ongoing offseaon attempt to get us ranked on the first page of some search engine(s) when nerds search for "beryllium".

Before you PM me with "Why?", the answer is simply that I am sitting around reading log files at work and cutting and pasting into this thread requires absolutely NO mental stress.
Last edited by Dartgod; 04-14-2011 at 09:18 PM..
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Old 01-27-2007, 11:20 AM   #1711
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The other Group 2 hydroxides
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Old 01-27-2007, 11:21 AM   #1712
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The other hydroxides of the Group 2 metals are all basic. They react with acids to form salts. For example:
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Old 01-27-2007, 11:21 AM   #1713
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Calcium hydroxide reacts with dilute hydrochloric acid to give calcium chloride and water.
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Old 01-27-2007, 11:21 AM   #1714
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Beryllium hydroxide
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Old 01-27-2007, 11:22 AM   #1715
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Beryllium hydroxide reacts with acids, forming solutions of beryllium salts. For example:
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Old 01-27-2007, 11:22 AM   #1716
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But it also reacts with bases such as sodium hydroxide solution. Beryllium hydroxide reacts with the sodium hydroxide to give a colourless solution of sodium tetrahydroxoberyllate.
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Old 01-27-2007, 11:22 AM   #1717
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This contains the complex ion, [Be(OH)4]2-. The name describes this ion. Tetra means four; hydroxo refers to the OH groups; beryllate shows that the beryllium is present in a negative ion. The "ate" ending always shows that the ion is negative.
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Old 01-27-2007, 11:22 AM   #1718
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A simple explanation of what is happening
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Old 01-27-2007, 11:23 AM   #1719
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You need to think about where the beryllium hydroxide came from in the first place. It would probably have been made by adding sodium hydroxide solution to a solution of a beryllium salt like beryllium sulphate.
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Old 01-27-2007, 11:23 AM   #1720
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Remember that beryllium ions in solution exist as the hydrated ion, [Be(H2O)4]2 . The beryllium has such a strongly polarising effect on the water molecules that hydrogen ions are very easily removed from them.
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Old 01-27-2007, 11:23 AM   #1721
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The sodium hydroxide solution contains hydroxide ions which are powerful bases. If you add just the right amount of sodium hydroxide solution, you get a precipitate of what is normally called "beryllium hydroxide" - but which is a shade more complicated than that!
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Old 01-27-2007, 11:24 AM   #1722
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The product (other than water) is a neutral complex, and it is covalently bonded. All that has happened to the original complex ion is that two hydrogen ions have been removed from the water molecules.
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Old 01-27-2007, 11:24 AM   #1723
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You get a precipitate of the neutral complex because of the lack of charge on it. There isn't enough attraction between this neutral complex and water molecules to bring it into solution.
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Old 01-27-2007, 11:24 AM   #1724
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What happens if you add an acid to this?
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Old 01-27-2007, 11:25 AM   #1725
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The hydrogen ions that were originally removed are simply replaced. The precipitate dissolves as the original hydrated beryllium ion is re-formed.
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