main points of fajan's rules
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ғᴀᴊᴀɴs' ʀᴜʟᴇs
- ʜɪɢʜ ᴄʜᴀʀɢᴇ ᴀɴᴅ sᴍᴀʟʟ sɪᴢᴇ ᴏғ ᴛʜᴇ ᴄᴀᴛɪᴏɴ. ɪᴏɴɪᴄ ᴘᴏᴛᴇɴᴛɪᴀʟ Å ᴢ+/ʀ+ (= ᴘᴏʟᴀʀɪᴢɪɴɢ ᴘᴏᴡᴇʀ)
- ʜɪɢʜ ᴄʜᴀʀɢᴇ ᴀɴᴅ ʟᴀʀɢᴇ sɪᴢᴇ ᴏғ ᴛʜᴇ ᴀɴɪᴏɴ. ᴛʜᴇ ᴘᴏʟᴀʀɪᴢᴀʙɪʟɪᴛʏ ᴏғ ᴀɴ ᴀɴɪᴏɴ ɪs ʀᴇʟᴀᴛᴇᴅ ᴛᴏ ᴛʜᴇ ᴅᴇғᴏʀᴍᴀʙɪʟɪᴛʏ ᴏғ ɪᴛs ᴇʟᴇᴄᴛʀᴏɴ ᴄʟᴏᴜᴅ (ɪ.ᴇ. ɪᴛs "sᴏғᴛɴᴇss")
- ᴀɴ ɪɴᴄᴏᴍᴘʟᴇᴛᴇ ᴠᴀʟᴇɴᴄᴇ sʜᴇʟʟ ᴇʟᴇᴄᴛʀᴏɴ ᴄᴏɴғɪɢᴜʀᴀᴛɪᴏɴ.
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Thus sodium chloride (with a low positive charge (+1), a fairly large cation (~1 Å) and relatively small anion (0.2 Å) is ionic; but aluminium iodide (AlI3) (with a high positive charge (+3) and a large anion) is covalent.
Polarization will be increased by:
high charge and small size of the cation
Ionic potential Å Z+/r+ (= polarizing power)
High charge and large size of the anion
The polarizability of an anion is related to the deformability of its electron cloud (i.e. its "softness")
An incomplete valence shell electron configuration
Noble gas configuration of the cation produces better shielding and less polarizing power
e.g. Hg2+ (r+ = 102 pm) is more polarizing than Ca2+ (r+ = 100 pm)
Polarization will be increased by:
high charge and small size of the cation
Ionic potential Å Z+/r+ (= polarizing power)
High charge and large size of the anion
The polarizability of an anion is related to the deformability of its electron cloud (i.e. its "softness")
An incomplete valence shell electron configuration
Noble gas configuration of the cation produces better shielding and less polarizing power
e.g. Hg2+ (r+ = 102 pm) is more polarizing than Ca2+ (r+ = 100 pm)
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