Bonding and Molecular Structural Problem?
827720
Bond polarity refers to difference of electronegativity between two atoms in a bond. \n\nMolecular polarity is the sum of all the forces\n\nThat's all I know.
879729
Please see my answer to your previous question for more details.\n\nThe more unshared pairs of e-, the more distortion in the geometry of the molecule.
1107805
study on intermolecular particals and there behavior
273309
wat r u ppl talking about....u ppl r absolutely wrong.....its alkynes n i am 100% sure about\n\nthey r more reactive becoz of there triple bonds...\n\n\n2 ppl in a row a row giving a wrong answer can confuse a person completely
387688
I have seen sulfur compounds with 2, 4, and 6 covalent bonds attached the the sulfur atom. I can't think of any sulfur compounds with 5 bonds around the sulfur atom at the top of my head.
621085
http://www.chemguide.co.uk/atoms/bonding/vdw.html
496847
N2- has a bond order of 3.\n\nhttp://www.meta-synthesis.com/webbook/39_diatomics/diatomics.html
1090457
a the number of outer electron that will bond with other atoms to fill thei valence shells
811335
when bonding takes place by sharing of electrons then it is said to be covalent bond. now it can be possible in two ways.\n\nfor eg if two hydrogen are combining to form a bond then they both will share one electon each and the force applied from there nucleus will be same so the elecron pair will remain nearly equal with both the hydrogen.so you can say that it remains exactly at centre from both the nucleus\n\nbut if you consider HCl. here also both hydrogen and chlorine are going to share one elctron each when bond formation takes place. but as electronegativity of chlorine is quite high(ie its attraction from nucleus is quite high) compared to that of hydrogen so eventhough they both have shared one electron each but still electron pair will remain towards chlorine.\n\ni hope this will help you out
549677
This is a chemistry question, the anomaly is due to Hydrogen bonding.
825051
Covalent bonds, as in NH4+
139994
Is its structure a ring with double bonds?
761407
lewis dot structure shows the molecule's valence e-s and the bonding of the molecule \n\nit is very easy to draw \nhere are some hints for drawing lexis structure\nfirst you need to find out the valence e-s of that molecule i.e. h2O have 8 VALENCE e-s 2 from the hydrogens abd 6 from oxygen \nthere is is Carbon present in a molecule than carbon should be placed in the middle  if there is no carbon present than least electronegative atom should be in the middle \nput one or two or three pair(s) of electrons in the middle depending on the octet rule which states that all atoms want 8 valence e-s other than H, Be, and S. H bond to get 2 valence electron, Be bonds to get 6 valence e-s and S can get more than 8 valence electrons \nif you are confused or need help with any of the models just email me i will try my best to reply
884142
It is just Cl single bonded to each of the O's.  Ther are 26 available electrons (7+(6*3)+1(because it is negative)) and to fill their valence shells 32 are needed which means 6 are shared which means there are 3 bonds and since all of the atoms must be bonded there must be 3 single bonds. There are 10 lone pairs I think(you can check)
884877
Bond length = valence electrons divided by two.
953050
If the difference in the electronegativity between the two elements is less than 1.67, the bond will be covalent.\n\nNote: As to the statement that electronegative atoms don't form covalent bonds, that's nonsense.  ALL atoms are electronegative to some extent.  Just go look up the electronegativity series in any general chem. text.  Or check out this:\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Bonding/Electroneg-Bond-Polarity.html
929337
a) Tetrahedral shape. bond angle : 109.5\nNo lone pair on central carbon\n\nb) Linear shape. Bond angle: 180\nNo lone pair on central Be\n\nc) Trigonal pyramdial shape. Bond angle less than 109.5\na lone pair on Cl. 2 oxgen double-bonded and 1 oxygen single-bonded to Cl. 0 formal charge on Cl and the O=Cl. Formal charge on Cl-O is -1.