Yes. If the shape of the molecule means that hhe bond moments (vectors) cancel each other out.
A molecule can have a completely nonpolar covalent bond when two atoms of the same element form the bond.
No. It is a polar molecule.
A covalent bond, as in all diatomic elements. To be specific, a nonpolar covalent bond, since the electronegativity values are identical
SO2 has polar bonds but is a polar molecule as it is bent and the bond dipoles do not cancel one another out.
Since syclohexane is a symmetrical molecule, the sum of the bond dipoles is zero and the molecules is therefore non-polar
A molecule can have a completely nonpolar covalent bond when two atoms of the same element form the bond.
One term refers only to the bond, another refers to the molecule.
For a molecule of oxygen, O2, the bond is nonpolar covalent.
A polar bond may be present in a nonpolar molecule. Examples: CH4, NH3, C2H2, CO2
No. It is a polar molecule.
Nonpolar covalent bond; the electronegativity values are identical.
This molecule contains polar covalent bonds.
A covalent bond, as in all diatomic elements. To be specific, a nonpolar covalent bond, since the electronegativity values are identical
SO2 has polar bonds but is a polar molecule as it is bent and the bond dipoles do not cancel one another out.
The shape of a molecule affects polarity because of how bond dipoles between two atoms is affected by other atoms in the molecule. Bond dipoles are vector quantities (which means they have magnitude and direction), so when a molecule has two or more bond dipoles they can cancel each other out if they perfectly oppose each other. For example CO2 (O=C=O) has two dipole bonds, but since they equaly oppose each other they cancel out and the molecule is nonpolar. In bent molecules like H2O, the two hydrogens bonded to the oxygen have equal dipole moments, but they do not directly oppose each other so they do not cancel out. As a result the molecule is polar. So in summery the molecule's geometry affects the polarity of the molecule by dictating the direction of the vector quantities of the dipole bonds, which determines whether they will be able to cancel each other out (nonpolar) or allow for non zero dipole moments (polar).
The shape of a molecule affects polarity because of how bond dipoles between two atoms is affected by other atoms in the molecule. Bond dipoles are vector quantities (which means they have magnitude and direction), so when a molecule has two or more bond dipoles they can cancel each other out if they perfectly oppose each other. For example CO2 (O=C=O) has two dipole bonds, but since they equaly oppose each other they cancel out and the molecule is nonpolar. In bent molecules like H2O, the two hydrogens bonded to the oxygen have equal dipole moments, but they do not directly oppose each other so they do not cancel out. As a result the molecule is polar. So in summery the molecule's geometry affects the polarity of the molecule by dictating the direction of the vector quantities of the dipole bonds, which determines whether they will be able to cancel each other out (nonpolar) or allow for non zero dipole moments (polar).
Since syclohexane is a symmetrical molecule, the sum of the bond dipoles is zero and the molecules is therefore non-polar