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∙ 13y agoThink about the amount of valance electrons. Sulfur has two more than Carbon. Carbon wants to share its four valance to make it feel like it has 8 and does so with oxygen. Because there are no lone pair electrons left on carbon it is a linear structure and has no dipole (both oxygen's stick out giving bot ends a pseudo negative charge).
Sulfur on the other hand lives in resonance with a double bond on one oxygen switching back and forth (look into resonance if you don't understand this). It keeps two of its electrons giving it a lone pair. this lone pair pushes the oxygen atoms downward giving the Sulfur end a pseudo charge and the oxygen end a pseudo charge.
Happy carbon = linear molecule = no dipole
Unhappy Sulfur = bent molecule = dipole
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∙ 13y agoSO2 molecule has a dipole moment because of the difference in electronegativity between sulfur and oxygen atoms, leading to an uneven distribution of electron density and a separation of charges. CO2 molecule, on the other hand, has a linear geometry with a symmetrical distribution of electron density, resulting in a net zero dipole moment despite the polar nature of the C-O bonds.
Wiki User
∙ 13y agoThe S-O bonds are polar because oxygen is more electronegative than sulfur.
Unlike CO2, the molecular geometry of SO2 is bent rather than linear, giving SO2 a net dipole moment.
An overall dipole moment is H2S.
Carbonate (CO3 2-) is trigonal planar with a central C and three O's 120 degrees from each other (D3h symmetry). All the O's have the same electron density because of resonance. This gives carbonate no dipole.
CO2 is a nonpolar molecule because it has a linear shape with a symmetrical distribution of its oxygen atoms on either side of the carbon atom. This symmetrical arrangement results in the overall molecule having a net dipole moment of zero, making it nonpolar.
CO2 is a linear molecule...the C in the middle and the the oxygens double bonded on opposite ends.... the electronegativities of the oxygens cancel each other out and Dipole moment becomes zero. http://en.wikipedia.org/wiki/File:Carbon-dioxide-2D-dimensions.svg (picture from wikipedia).
A molecule that is symmetrical in shape with equal distribution of electrons is most likely to be nonpolar. For example, molecules like CO2, O2, and CH4 are nonpolar due to their linear or symmetrical structures, which result in no net dipole moment.
Symmetric molecules such as carbon dioxide (CO2) have zero dipole moment because the individual bond dipoles cancel each other out due to the molecule's symmetric geometry. This results in no overall net dipole moment for the molecule.
Carbon dioxide (CO2) possesses zero dipole moment because the two polar C=O bonds are oriented in opposite directions, resulting in the bond dipoles cancelling each other out. On the other hand, sulfur dioxide (SO2) does not possess a zero dipole moment because its bond dipoles do not cancel out due to the bent molecular geometry of SO2.
Yes, the shape of a molecule can determine its dipole moment. In general, a molecule with an uneven distribution of charge due to differences in electronegativity between atoms will have a dipole moment. The spatial arrangement of the atoms in the molecule will determine the overall direction and magnitude of the dipole moment.
The dipole moment of CO2 is zero because the molecule has a linear geometry with the two oxygen atoms symmetrically arranged on either side of the carbon atom. The dipole moments of the two C=O bonds cancel each other out, resulting in a net dipole moment of zero for the molecule.
The molecules with a dipole moment are H2O and SO2. H2O has a bent shape with unequal distribution of electrons, creating a dipole moment due to the electronegativity difference between hydrogen and oxygen atoms. SO2 has a bent shape with a sulfur atom surrounded by oxygen atoms, resulting in a dipole moment.
An overall dipole moment is H2S.
HCl and CO2 are dipole molecules because they have a significant difference in electronegativity between the bonded atoms, creating a dipole moment. Cl2 and CCl4 are nonpolar molecules as they have either symmetrical distribution of charge (Cl2) or the vector sum of the dipole moments cancel out (CCl4).
The pair of molecules with the strongest dipole-dipole interactions would be NH3-NH3 because ammonia (NH3) is a polar molecule with a significant dipole moment, leading to stronger attractions compared to the other options listed.
Carbonate (CO3 2-) is trigonal planar with a central C and three O's 120 degrees from each other (D3h symmetry). All the O's have the same electron density because of resonance. This gives carbonate no dipole.
CO2 is a nonpolar molecule because it has a linear shape with a symmetrical distribution of its oxygen atoms on either side of the carbon atom. This symmetrical arrangement results in the overall molecule having a net dipole moment of zero, making it nonpolar.
Symmetric molecules like carbon dioxide (CO2) have no dipole moment because the bond dipoles cancel each other out, resulting in a net dipole moment of zero. Other examples include benzene (C6H6) and methane (CH4).
Absorption of energy from IR radiation can only occur when the wavelength of radiation and the wavelength of the bond vibration match. If a molecule has symmetry...for example no dipole, we say it is IR inactive. CO2 has no dipole....this would be an IR inactive gas...Cl2 as well. A gas that has a dipole would be IR active. Propene would be a nice example of an IR active gas.It possesses a dipole. One would see a signal around 1650.A:CO2 has no permanent dipole. However, when CO2 undergoes a bending vibration, its dipole moment changes from zero to some non-zero value. This vibration produces a change in dipole moment and is therefore IR active.