Question

What's the difference between bond order, bond length and bond strength?

Answer 1

Bond order is the number of bonding pairs of electrons between two atoms.
Bond length is the distance between the centers of two covalently bonded atoms.
Bond strength depends on
------>Bond Order increases Bond Strength increases
------>Bond Length increases Bond Strength decreases

Answer 2

Thank you, can u explain which one of the following has lowest electrical conductivity and why:

Cu(s)
Hg(l)
H2(g)
LiOH(aq)

Answer 3

oh and also, which compound contains both ionic and covalent bond?

MgCl2
HCl
H2CO
NH4Cl

Answer 4

Bright, can you look up your notes and tell me why does something conduct electricity? Then we can reason through your second question. Here is the way to approach it:
Why does something conduct electricity?
What are the differences between the 4 choices? And how would these differences influence the ability to conduct electricity?

Answer 5

OK.
I know that something conducts electricity when it has free (valence electrons) or free ions in the case of ionic compounds. I also know that metals are very good conductors of electricity, so that means the Copper and Mercury is out. What i don't know is why hydrogen gas is not a good conductor. is it because it doesn't have any free electrons to conduct electricity, or does it have something to do with it being a gas.

Answer 6

@brightdiwa , I think you're going in a correct way.

Hg(l) and Cu(s) are conductors, so they will conduct electricity well.

LiOH is an ionic aqueous solution, so it will also conduct electricity .

H2(g) can not conduct electricity well as e- (electrons) are strongly bounded to proton in hydrogen. So there is no charge carrier which can move to produce an electric current.

Answer 7

so by charge carrier, do you mean free/valence electrons?