Basically, look at each bond in the molecule, and the greater the difference in the electronegativities of the atoms in the bond, the more polar that bond is. In three-dimensional space, some of the bonds may cancel each other out. For example, take CF4.All four of the C-F bonds are polar, but in the molecule as a whole, they are all cancel each other out due to how they are oriented spacially. CH2F2, though, polar.This is because there are two different kinds of bonds, which are two C-H bonds and two C-F bonds. There is a net polarity to the molecule because of this. An easy way to look at it is if all the atoms connected to the central atom are the same, as in CF4, then the molecule will not be polar.or example, take CF4. All four of the C-F bonds are polar, but in the molecule as a whole, they are all cancel each other out due to how they are oriented spacially. CH2F2, though, polar.
https://answers.yahoo.com/question/index?qid=20090119195958AAgKavO
In $\ce{CF4}$, you are correct. The molecules is perfectly symmetrical, so every electron pair on each fluorine cancels out the electron pairs of every other fluorine. For this reason, this molecule is non-polar. In $\ce{CHF3}$, however, the hydrogen does not have 3 other electron clouds around it like the fluorine do.he molecules is perfectly symmetrical, so every electron pair on each fluorine cancels out the electron pairs of every other fluorine. For this reason, this molecule is non-polar. In $\ce{CHF3}$, however, the hydrogen does not have 3 other electron clouds around it like the fluorine do.
http://chemistry.stackexchange.com/questions/31604/why-is-cf4-non-polar-and-chf3-polar
BF3, XeF4 Symmetric ball shaped molecules such as tetrahedral and octahedral eg CF4 and SF6 The above apply in case of symmetrical substitution about the central atom eg CF4 is non polar but CH3F and CH2F2 and CHF3 are polar.xpect polar molecules in: V shaped (angular) molecules eg CF2 T shaped molecules eg ClF3 See-saw molecules eg SF4 Pyramidal molecules such as trigonal pyramidal or square pyramidal eg NF3, BrF5 Note: ClF3 and SF4 has to move in the polar molecules.
https://sg.answers.yahoo.com/question/index?qid=20100403235654AAgjl7z
BF3, XeF4 Symmetric ball shaped molecules such as tetrahedral and octahedral eg CF4 and SF6 The above apply in case of symmetrical substitution about the central atom eg CF4 is non polar but CH3F and CH2F2 and CHF3 are polar.F3, XeF4 Symmetric ball shaped molecules such as tetrahedral and octahedral eg CF4 and SF6 The above apply in case of symmetrical substitution about the central atom eg CF4 is non polar but CH3F and CH2F2 and CHF3 are polar.
http://www.experts123.com/q/which-molecules-are-polar-non-polar.html
Transcript: Hi, this is Dr. B. Let's do the Lewis structure for CH2F2: difluoromethane. On the periodic table, Carbon is in group 4, it has 4 valence electrons. Hydrogen, group 1, but we have 2 Hydrogens.Fluorine, 7 valence electrons, we have 2 of those as well, for a total of 20 valence electrons.We'll put the Carbon at the center, and then Hydrogens always go on the outside.luorine needs 8, this Fluorine has 8 and this Fluorine has 8. And then Carbon, in the center, needs 8, and it has 8. So we've used all the valence electrons. Everything has full outer shells. That is the Lewis structure for CH2F2. This is Dr. B., and thanks for watching.
http://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/CH2F2-lewis-structure.html
SCN is polar. This is because the bonds of the compounds have an  imbalance in the position of the electrons. Edit. Share to: 1  The Periodic Table of Elements Life is sustained by a number of chemical elements.2  They are responsible for the birth of planets and the evolution of cells to complex organisms.O is polar. If you compare the electronegativities (how strongly the element pulls on electrons) N 3.04 O 3.44 (bigger therefore pulls electrons harder) The electron … s will be drawn to the oxygen causing it to be slightly negative, and the N to be slightly positive.
http://www.answers.com/Q/CH2F2_polar_or_nonpolar
Share to: Those compounds which has partial positive and partial negative ends due to electronegative difference and there dnet dipole moment is not zero.for example: HCl,water.O is polar. If you compare the electronegativities (how strongly the element pulls on electrons) N 3.04 O 3.44 (bigger therefore pulls electrons harder) The electron … s will be drawn to the oxygen causing it to be slightly negative, and the N to be slightly positive.
http://www.answers.com/Q/CH2F2_polar_or_nonpolar
Chlorine's high electronegativity will give it a partial negative charge in the molecule as it pulls the electrons closer to itself and away from the carbon. A molecule like CH4, (methane), will be nonpolar.All the ligands attached to carbon have the same electronegativity, so there is no difference in dipole around carbon. Another determiner regarding polarity is the presence of lone pairs of electrons.Ammonia (NH3) has ligands that all have the same electronegativity.hlorine's high electronegativity will give it a partial negative charge in the molecule as it pulls the electrons closer to itself and away from the carbon. A molecule like CH4, (methane), will be nonpolar.
http://www.answers.com/Q/Is_CH2F2_polar_or_non_polar_molecule
NO is polar. If you compare the electronegativities (how strongly the element pulls on electrons) N 3.04 O 3.44 (bigger therefore pulls electrons harder) The electron … s will be drawn to the oxygen causing it to be slightly negative, and the N to be slightly positive.O is polar. If you compare the electronegativities (how strongly the element pulls on electrons) N 3.04 O 3.44 (bigger therefore pulls electrons harder) The electron … s will be drawn to the oxygen causing it to be slightly negative, and the N to be slightly positive.
http://www.answers.com/Q/CH2F2_polar_or_nonpolar
In order for hydrogen bonding to take place, the molecule in question must have a hydrogen atom attached to an N, O, or F atom. In the case of CH2F2, you have a Lewis structure with a central carbon atom and bound H atoms with bound F atoms arranged in an sp3 hybrid.......n the case of CH2F2, you have a Lewis structure with a central carbon atom and bound H atoms with bound F atoms arranged in an sp3 hybrid.......
http://science-mathematics.com/Chemistry/201109/12773.htm
which is nonpolar cf4 or ch2f2
CF4 is a nonpolar. Comparing between CF4 and CH2F2, CF4 is nonpolar. 