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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 01-26-2007, 08:24 PM   #1636
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Reaction with water
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Old 01-26-2007, 08:25 PM   #1637
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Beryllium chloride reacts vigorously and exothermically with water with the evolution of acidic, steamy hydrogen chloride gas. This is typical of covalent chlorides.
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Old 01-26-2007, 08:25 PM   #1638
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In the first instance, it reacts to give hydrated beryllium ions, [Be(H2O)4]2 , and chloride ions.
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Old 01-26-2007, 08:25 PM   #1639
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But the hydrated beryllium ions (called tetraaquaberyllium ions) are quite strongly acidic. The small beryllium ion at the centre attracts the electrons in the bonds towards itself, and that makes the hydrogen atoms in the water even more positive than they usually are. If the solution is hot and concentrated (as it is likely to be if you add water to solid beryllium chloride - a very exothermic reaction), chloride ions can remove one or more of these hydrogen ions to produce hydrogen chloride gas.
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Old 01-26-2007, 08:26 PM   #1640
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All the other ionic chlorides in Group 2 dissolve in water without any obvious reaction.
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Old 01-26-2007, 08:26 PM   #1641
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Note: There is actually a very small amount of reaction between anhydrous magnesium chloride and water, although you wouldn't notice it. Magnesium chloride isn't quite as purely ionic as we sometimes pretend!
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Old 01-26-2007, 08:26 PM   #1642
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Follow this link if you are interested in exploring the naming of complex ions.
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Old 01-26-2007, 08:26 PM   #1643
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. . . or this one for detailed explanations of why complex ions similar to the beryllium one are acidic.
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Old 01-26-2007, 08:27 PM   #1644
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The structure of beryllium chloride
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Old 01-26-2007, 08:27 PM   #1645
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As a gas . . .
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Old 01-26-2007, 08:27 PM   #1646
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Beryllium chloride, BeCl2, is a linear molecule with all three atoms in a straight line. Showing only the outer electrons:
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Old 01-26-2007, 08:29 PM   #1647
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Beryllium chloride is known as an electron-deficient compound because it has the two empty orbitals at the bonding level.
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Old 01-26-2007, 08:29 PM   #1648
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As a solid . . .
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Old 01-26-2007, 08:29 PM   #1649
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If it had this same simple structure as a solid, you would expect the melting point to be much lower than it actually is. It is a very small molecule, and so the intermolecular attractions would be expected to be fairly weak.
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Old 01-26-2007, 08:29 PM   #1650
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Note: If you aren't sure about intermolecular forces (Van der Waals forces) you could follow this link to find out more about them.
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