lone pair造句
1. Wigeon A lone pair of gad wall preened on shrinking tussocks.
2. For the first time the significance of lone pairs of electrons, in determining the overall shape of molecules was recognised.
3. So how many lone pair electrons do we have?
4. In this paper, importance of the lone pair electrons in molecular structure and chemical reaction is expounded by effect of the lone pair electrons.
5. So, which atom is in need of those lone pair electrons?
6. So, if we want to figure out the formal charge on the carbon, we need to take the number of valence electrons, so that's 4. We need to subtract the lone pair, what number is that? It's 2.
7. And if we put that in our bond here, we have 1, 2, 3 bonds, plus we have one lone pair left over.
8. So in oxygen we have a similar situation where, in fact, we are not going to promote any of the electrons because we have two lone pair electrons no matter what we do.
9. For the carbon, we start with 4 valence electrons, we have 0 lone pair electrons minus 4, and we end up with a formal charge of 0.
10. So we need to add those 2 valence electrons left as lone pair electrons in our structure.
11. That's what we call when we have three bonding atoms and one lone pair.
12. Well, we're talking about a pretty high number here, so to make counting easier, we'll just say 10 lone pairs, because 20 lone pair electrons is the same thing as 10 lone pairs.
13. So it looks a lot less messy if we just draw our Lewis structure like this for h c n, where we have h bonded to c triple bonded to n, and then a lone pair on the nitrogen there.
14. And we give different names, depending on what kind of electrons we're dealing with, so, for example, with h c l here, we can talk about having bonded versus lone pair electrons.
15. So in terms of nitrogen that starts off with a valence number of 5, again we have 2 lone pair electrons in the nitrogen, and again, we have 6 electrons that are shared.
16. It has been reported that addition of trace quantity of DCl to NMR solns. of alkaloids resulted in extensive broadening signal of protons spatially closed to the nitrogen lone pair.
17. So if we take a look at nitrogen here, what you'll notice is we have thre available for bonding, - and we already have our lone pair -- one of our orbitals is already filled up.
18. Yeah, so also 4. We started with 10 valence electrons, we used up 6 of those as bonding electrons, so we have 4 left, which will be lone pair electrons.
19. The nitrogen atoms of amines have what chemists call a lone pair of electrons, and it is this which attaches each amine molecule to the nanotube.
20. For the sulfur, we start off with 6 valence electrons, minus 4 lone pair electrons, minus 2, taking in account our bonding electrons, so we end up with a formal charge of 0.