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tayk477
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#1
oes anyone know what working out I would use for this?
which of the following have significant bond dipoles, but no molecular dipoles?
1) benzene 2) tetrachloromethane 3) sulfur dioxide 4) phosphorus pentachloride 5) dichloromethane
which of the following have significant bond dipoles, but no molecular dipoles?
1) benzene 2) tetrachloromethane 3) sulfur dioxide 4) phosphorus pentachloride 5) dichloromethane
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Sophie123.sdr
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(Original post by tayk477)
oes anyone know what working out I would use for this?
which of the following have significant bond dipoles, but no molecular dipoles?
1) benzene 2) tetrachloromethane 3) sulfur dioxide 4) phosphorus pentachloride 5) dichloromethane
oes anyone know what working out I would use for this?
which of the following have significant bond dipoles, but no molecular dipoles?
1) benzene 2) tetrachloromethane 3) sulfur dioxide 4) phosphorus pentachloride 5) dichloromethane
to find out if molecule dipoles, draw the shape of molecule and if all polar bonds are opposites, then they cancel out and have no molecular dipole. Symmetrical molecules are non-polar.
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e.g. in benzene, carbon and hydrogen have simillar negativity so no dipoles (bond or molecular) but dichloromethane contains 2 polar bonds (C-Cl) which don't cancel out so there will be both bond dipoles and a molecular dipole.
Does this make sense?
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