Explain why the thermal stability increases with nitrates and carbonated down group 1 and 2
Also what are the trends we have to know for group 1,2,7 and across the period? Just trends
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from group 1 NaC03 downwards ,the carbonates don't decompose when heated only the nitrates of group 1 from Na downwards decompose so the thermal stability increases down group 2 meaning the carbonates and nitrates become more stable to heat as the ionic radius of the positive ion increases down the group ie the positive ion becomes larger so polarisation of the carbonated electron cloud
i think the only trends you need to know are : solubility of group 2 hydroxides and sulfates thermal stabilities of group 1 and 2 and with group 7 there isnt a trend you need to learn except that the ionization energy decrease and the electro negativity also decreases down the group the main things you need to know about group 7 are its reactions and the test for halides
why does NH3 have a lower boiling point than HF and H2O have a higher boiling point than HF? Help, someone!!
as HF can form hydrogen bonding so more energy needed and H2O has greater b.p then HF as it can from up to 2 hydrogen bonds with one molecule so much stronger
as HF can form hydrogen bonding so more energy needed and H2O has greater b.p then HF as it can from up to 2 hydrogen bonds with one molecule so much stronger
Even NH3 can form H.B, but still why is it's boiling point lower than that of HF?
why does NH3 have a lower boiling point than HF and H2O have a higher boiling point than HF? Help, someone!!
H2O has a higher boiling point than HF because it can form 2 hydrogen bonds as there are 2 electron lone pairs on the oxygen while HF forms 1 hydrogen bond. So more energy required to break the intermolecular forces in H2O than in HF.
Not sure about why NH3 has a lower boiling point than HF
from group 1 NaC03 downwards ,the carbonates don't decompose when heated only the nitrates of group 1 from Na downwards decompose so the thermal stability increases down group 2 meaning the carbonates and nitrates become more stable to heat as the ionic radius of the positive ion increases down the group ie the positive ion becomes larger so polarisation of the carbonated electron cloud
i think the only trends you need to know are : solubility of group 2 hydroxides and sulfates thermal stabilities of group 1 and 2 and with group 7 there isnt a trend you need to learn except that the ionization energy decrease and the electro negativity also decreases down the group the main things you need to know about group 7 are its reactions and the test for halides
Thank you so much - appreciate it!
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H2O has a higher boiling point than HF because it can form 2 hydrogen bonds as there are 2 electron lone pairs on the oxygen while HF forms 1 hydrogen bond. So more energy required to break the intermolecular forces in H2O than in HF.
Not sure about why NH3 has a lower boiling point than HF
Cant the delta positive 2 hydrogens also form hydrogen bonds? So in all, 4 hydrogen bonds in water molecules?
Cant the delta positive 2 hydrogens in water molecule also form hydrogen bonds? So in all, 4 hydrogen bonds in water molecules?
They can form hydrogen bonds with the oxygen on another water molecule but that's the same as when the oxygen forms hydrogen bonds with hydrogen's if you know what I mean. So don't include them, it's 2 hydrogen bonds per water molecule because of 2 electron lone pairs.
They can form hydrogen bonds with the oxygen on another water molecule but that's the same as when the oxygen forms hydrogen bonds with hydrogen's if you know what I mean. So don't include them, it's 2 hydrogen bonds per water molecule because of 2 electron lone pairs.