Discuss briefly the relationship between the dipole moment of a molecule and the polar character of the bonds within it. WIth this as a basis, account for the difference between the dipole moments of CH2F2 and CF4.
does anyone have any idea?
the greater the dipole moment of a molecule the more polar it's bonds.
A bond is polar when on atom is more electronegative than the other or the molecule is asymmetrical in geometry.
A bond is polar when an atom is more electronegative than the other. That is true. However, molecules made up of different atoms may have a dipole moment if they have atoms with different electronegativities AND they are not symmetrical. The CF4 molecule is tetrahedral but completely symmetrical; therefore, CF4 has no dipole moment even though C and F have different electronegativities. The individual polar C-F bonds add up to a net zero dipole moment for the molecule because of the symmetry of the tetrahedral arrangement. Replacing 2 of the F atoms with 2 H atoms destroys that symmetry.
what would the dipole moment be for CH2F2
Look on page one for the title "What causes chemical reactions to happen?" on the link below and you will see CH2F2 shows 2.29 Debeys. OR you can go to www.google.com and type in "dipole moment CH2F2" without the parenthese, click on the article and read all about it. I did that and never found the part that dealt with CH2F2 but perhaps I just overlooked it.
http://www.google.com/search?hl=en&q=dipole+moment+CH2F2&btnG=Google+Search
i don tknow
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Answer:
In order to have a dipole moment (i.e., to be a polar molecule) a molecule must have polar bonds and must have a molecular geometry which is not symmetrical (i.e., one in which the vector sum of the bond dipoles 0).
In CH2F2 the C-F and C-H bonds are polar and the molecule is not symmetrical; therefore, the molecules is polar and would show a dipole moment.
In CF4 the C-F bonds are polar, but the molecule is symmetrical; therefore, the molecule is non-polar and would not show a dipole moment.
I apologize if my previous response was confusing. The dipole moment of a molecule is determined by the polarity of its bonds and the molecular geometry. A bond is considered polar when there is an uneven distribution of electron density between two atoms due to differences in electronegativity.
In the case of CH2F2 (difluoromethane), the molecule has a bent molecular geometry, which means it is asymmetrical. The electronegativity of fluorine is higher than that of carbon and hydrogen, so the C-F bonds are polar. As a result, the molecule as a whole has a net dipole moment.
On the other hand, CF4 (tetrafluoromethane) has a tetrahedral molecular geometry, which is symmetrical. Although the C-F bonds in CF4 are polar due to the electronegativity difference, their polarity cancels out each other because of the symmetrical arrangement. As a result, CF4 has no net dipole moment.
Therefore, the difference in dipole moments between CH2F2 and CF4 can be explained by the asymmetrical and symmetrical geometries, respectively, which affect the overall polarity of the molecules.
The dipole moment of a molecule is a measure of the separation of positive and negative charges within the molecule. It is directly related to the polar character of the bonds within the molecule. A bond is polar when there is a significant difference in electronegativity between the atoms involved, causing the electrons to be unequally shared. This leads to a partial positive charge on one atom and a partial negative charge on the other, creating a dipole within the bond.
In the case of CH2F2, the molecule is not symmetrical due to the presence of the hydrogen atoms. The carbon-hydrogen bonds in CH2F2 are nonpolar because carbon and hydrogen have similar electronegativities. However, the carbon-fluorine bonds are polar because fluorine is more electronegative than carbon. The dipole moments of the polar carbon-fluorine bonds do not cancel each other out completely due to the presence of the hydrogen atoms, resulting in a nonzero dipole moment for the overall molecule.
On the other hand, CF4 is a symmetrical molecule with a tetrahedral geometry. All the carbon-fluorine bonds in CF4 are polar because of the difference in electronegativity between carbon and fluorine. However, due to the symmetrical arrangement of the four fluorine atoms around the carbon atom, the bond dipoles cancel each other out, resulting in a net dipole moment of zero for the molecule.
Therefore, the difference in dipole moments between CH2F2 and CF4 can be attributed to the asymmetry in CH2F2 caused by the presence of hydrogen atoms, while the symmetrical arrangement in CF4 leads to a cancellation of dipole moments.
The dipole moment of a molecule is a measure of its polarity and is influenced by the polar character of the bonds within it. A bond is considered polar when there is a difference in electronegativity between the atoms involved or when the molecule is asymmetrical in geometry.
In the case of CH2F2 (dichlorofluoromethane) and CF4 (carbon tetrafluoride), both molecules have polar C-F bonds due to the difference in electronegativity between carbon (C) and fluorine (F). However, CF4 is a symmetrical molecule with a tetrahedral arrangement, meaning that the individual polar C-F bonds cancel each other out, resulting in a net dipole moment of zero. This is because the molecule is symmetrically balanced, and the individual dipole moments of the C-F bonds cancel each other.
On the other hand, CH2F2 is not symmetrical due to the presence of hydrogen (H) atoms. By replacing two of the F atoms in CF4 with H atoms, the symmetry is broken, and the dipole moments of the C-F bonds no longer cancel each other out. As a result, the molecule has a net dipole moment, indicating its polarity.
To determine the exact dipole moment of CH2F2, you can refer to scientific literature or search online by typing in "dipole moment CH2F2." This will provide you with the specific value and further information about the molecule's polarity.