Question

When one atom of carbon (C) combines with four atoms of hydrogen (H), four nonpolar covalent bonds form, resulting in a molecule of methane (CH4). Which of the following describes the arrangement of valence electrons in a bond between C and H?

Answer 1

The valence electrons spend more time around the atom of C.

The valence electrons spend more time around the atom of H.

The valence electrons are shared equally between C and H.

The valence electrons are given up by the H and gained by the C.

Answer 2

What do u think it should be ?

Answer 3

the 3rd option???

Answer 4

Why ?

Answer 5

opps i meant the 2 one

Answer 6

Random guessing ??

Answer 7

What are the electronegativities of hydrogen and carbon ?

Answer 8

carbon is 2.5 and hydrogen is 2.1

Answer 9

is it right?

Answer 10

Who will attract the shared electrons more ?

Answer 11

hydrogen

Answer 12

The element which has higher electronegativity attracts the shared electron pair more.

Answer 13

Carbon has > EN than hydrogen so it will attract the shared electron pair more.

Answer 14

oh

Answer 15

So the correct option will be ??

Answer 16

second

Answer 17

How ???
Carbon will attract the shared pair more, so it will spend more time around carbon.

Answer 18

getting my points ?

Answer 19

yeah it the first one

Answer 20

Yep, but then why it's non polar ?

Answer 21

because it contains one element

Answer 22

It's due to its tetrahedral geometry. Net dipole moment becomes zero

Answer 23

okay, alright that does make sentence. Thank you!!

Answer 24

Sentence ?

Answer 25

@Abmon98 need ur opinion !

Answer 26

Sense I meant lol

Answer 27

If the atoms are equally electronegative, both have the same tendency to attract the bonding pair of electrons, and so it will be found on average half way between the two atoms.

Answer 28

\(\color{blue}{\text{Originally Posted by}}\) @Abhisar
but electronegativity of H and C is diff
\(\color{blue}{\text{End of Quote}}\)

Answer 29

Let's apply the first step to CH4.
The electronegativity of Carbon is 2.55
The electronegativity of Hydrogen is 2.20
Electronegativity difference between C and H = 2.55-2.20= 0.35
(The electronegativity difference ranging from 0.0 - 0.5 is considered to be negligible. Thus, non-polar.)

Answer 30

So non-polarity is nothing to do with dipole moment ?

Answer 31

yes :)

Answer 32

u mean they have no relation ?

Answer 33

yes is confusing me !

Answer 34

Dipole Moment is related to polar molecule

Answer 35

yeah i got uh now, actually question seeks bond polarity...ryt ??

Answer 36

yes thats right

Answer 37

@Abmon98 what about CCl bond ?

Answer 38

It will have polar bond...ryt ?

Answer 39

Electronegativity diff in CCl bond is 3-2.5 = 0.5, so it should be something like barely polar ryt ?
@Abmon98

Answer 40

Its Polar, polarity results in unequal sharing of valence electrons due to electronegativity therefore electrons will be more often located around the chlorine atom. this makes it a bit negative and electron cloud would spend more time and yes as you said due to small difference molecule is considered to be barely polar

Answer 41

yep, because upto 0.5 it's considered non-polar.

Answer 42

If the electronegativity difference is less than 0.5, then the bond is nonpolar covalent.

Answer 43

ryt !

Answer 44

not upto..it should be less than 0.5

Answer 45

Thanx for the help @Abmon98 !
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Answer 46

Your most welcome :)

Answer 47

@abmon98 thanks for your help but I am really confused to which option it is according to your explanation.

Answer 48

Check this @superhelp101
http://openstudy.com/updates/53ba5410e4b09f140ca6f6cd

Answer 49

yes. so it should be the second option right?

Answer 50

@Abhisar

Answer 51

\(\bf Update:\)
Electronegativity of carbon and hydrogen are 2.55 and 2.20 respectively which gives an electronegativity difference of 0.35. Any bond having a EN difference less than 0.4 is non-polar and hence electrons between hydrogen and carbon are shared equally. So the correct answer to the question on top should be option C

Reference:
http://www.chm.davidson.edu/ronutt/che115/electroneg.htm

http://preparatorychemistry.com/Bishop_molecular_polarity.htm