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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, 11:11 AM   #1681
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In order for an ionic bond to form, the beryllium has to let go of its electrons. It is too electronegative to do that.
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Old 01-27-2007, 11:11 AM   #1682
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Note: The trends in electronegativity in Group 2 are discussed on another page. That page looks at the way the electons are arranged in the beryllium-chlorine bond compared with the magnesium-chlorine bond.
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Old 01-27-2007, 11:11 AM   #1683
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Old 01-27-2007, 11:12 AM   #1684
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Beryllium forms 4-coordinated complex ions
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Old 01-27-2007, 11:12 AM   #1685
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Some simple background
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Old 01-27-2007, 11:12 AM   #1686
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Although beryllium doesn't normally form simple ions, Be2 , it does form ions in solution. In these, the beryllium ion becomes attached to four water molecules to give a complex ion with the formula [Be(H2O)4]2 .
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Old 01-27-2007, 11:13 AM   #1687
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The ion is said to be 4-coordinated, or to have a coordination number of 4, because there are four water molecules arranged around the central beryllium.
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Old 01-27-2007, 11:13 AM   #1688
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Many hydrated metal ions are 6-coordinated. For example, magnesium ions in solution exist as [Mg(H2O)6]2 .
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Old 01-27-2007, 11:13 AM   #1689
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The water molecules in these ions are attached to the central metal ion via coordinate bonds (dative covalent bonds). One of the lone pairs on each water molecule is used to form a bond with an empty orbital in the metal ion.
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Old 01-27-2007, 11:14 AM   #1690
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Each time one of these bonds is formed, energy is released, and the ion becomes more stable. It would seem logical for the metal ion to form as many bonds like this as it possibly can.
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Old 01-27-2007, 11:14 AM   #1691
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Note: If you aren't happy about coordinate bonding you must follow this link before you go on. You will find the bonding in hydrated metal ions discussed in some detail on that page.
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Old 01-27-2007, 11:14 AM   #1692
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Old 01-27-2007, 11:15 AM   #1693
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Why does beryllium only attach four water molecules?
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Old 01-27-2007, 11:15 AM   #1694
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The hydration of beryllium
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Old 01-27-2007, 11:15 AM   #1695
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The problem is that there has to be somewhere that the lone pairs on the water molecules can attach to. Beryllium has the electronic structure 1s22s2. It is helpful to draw this as an "electrons-in-boxes" diagram:
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