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Gonna try and describe this the best I can
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^really hope it helps :)
keith
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Is ClF4- polar or non polar?
There are two allowed structures of SF4Cl2... the cisform where one chlorine is in an equitorial position and one is axial, and the trans form where both chlorines are in axial positions. In the trans form the S-F bond dipoles all cancel each other, as do the S-Cl bond dipoles, because they are opposite each other. Therefore the molecule is non-polar. In the cisform, two of the S-F bond dipoles cancel, but because the other S-F bond dipoles are across from S-Cl bond dipoles, they do not cancel (S-F is more polar than an S-Cl bond). Therefore, the cisform is polar.
How does dipole moment help us to predict geometry of molecules?
The dipole moment tells us that there is net dipole on the molecule which indicates that any dipoles due to polarity of the covalent bonds do not cancel each other out. For example H2O has a dipole moment which rules out a linear structure where the bond dipoles would cancel each other out.
Any molecule that has a polar geometry is called what?
A good clue is to look at the symmetry of the molecular geometry. Molecules that are not symmetric are polar.In a bond, the more electronegative atom attracts a bigger share of the shared electrons than the other. This separation of charge results in a bond dipole. When all the bond dipoles of a molecule are added, the net dipole is called the permanent dipole moment. When the bond dipoles cancel, the molecule's dipole moment is zero and the molecule is called nonpolar. If the bond dipoles do not cancel, the molecule is polar.Lone pairs contribute to the polarity of a molecule. Since there is no positive nucleus to offset the negative charge of the lone pair, the end with the lone pair will always have a higher partial negative charge than any atom.The key to determining whether or not dipoles cancel is to consider their direction as well as their magnitude. The direction is determined by the molecular geometry. The Lewis structure does not represent the molecular geometry.
What is dipolar nature of water?
A dipole refers to two electrostatic charges which are separated by distance. In chemical compounds a dipole refers to unequal distribution of charge across a molecule that leads to an effective dipole often due to vector sum of bond dipoles.
What bond bonds water molecules with other water molecules?
hydrogen bond bonds water molecules with other water molecules.
Which structural formula represents a nonpolar molecule?
In the linear configuration, the bond dipoles cancel. Thus, the configurations of molecules with a bond dipole must be tetrahedral and linear respectively.
Which tends to have a greater degree of symmetry a polar molecule or a nonpolar molecule?
A non-polar molecule. Bond dipoles tend to cancel each other out in the more symmetric molecules.
In DNA molecules nucleotides bond together according to the nitrogenous bases Which of the following correctly describes how nitrogenous bases bond together?
Purines bond to pyrimidines
Is PVC hydrophilic?
Yes, PVC is polar. First off, its C-Cl bond has an electronegativity difference of more than 1.4, which means it has a polar bond. Second, its molecular structure is formed in a way that is not very symmetrical (most symmetrical molecules are non-polar) and its bond dipoles don't cancel out. So PVC is polar because it contains polar bonds, and its bond dipoles in its structure don't cancel out.
Why are the forces that hold atoms together in molecules stronger than the forces that hold the molecules together in a gas?
Molecules are two or more atoms held together by a covalent bond. This is a very strong bond as it is held together by strong electrostatic charges. All covalent molecules (apart from those held together in a covalent lattice such as Diamond) are bonded to other molecules by Van der Waal forces. Its is these intermolecular bonds that control boiling and melting points. Van der Waals are (in this case) the attractive force between molecules, they are temporary bonds between temporary dipoles and as electrons orbit the nuclei of atoms the position changes. This temporary dipole induces other molecules to form induced dipoles. Strength varies due to shape of molecule (the more "oblong" the greater the strength of the bond) and by size (the greater the size the greater the strength of the bond.)
Is ClF4- polar or non polar?
There are two allowed structures of SF4Cl2... the cisform where one chlorine is in an equitorial position and one is axial, and the trans form where both chlorines are in axial positions. In the trans form the S-F bond dipoles all cancel each other, as do the S-Cl bond dipoles, because they are opposite each other. Therefore the molecule is non-polar. In the cisform, two of the S-F bond dipoles cancel, but because the other S-F bond dipoles are across from S-Cl bond dipoles, they do not cancel (S-F is more polar than an S-Cl bond). Therefore, the cisform is polar.
What is the difference between individual bond polarity and molecular polarity?
bond polarity is the polarity particular bond within a molecule, while molecular polarity is the polarity of the whole molecule. take for example water (H20): you could find the bond polarity of each H-0 bond (polar covalent), or the polarity of the whole molecule together (polar, because the electronegativity of oxygen is higher than the hydrogen atoms)
How might a molecule with two strong bond dipoles have no molecular dipole at all?
A molecule with two strong bond dipoles can have no molecular dipole if the bond dipoles cancel each other out by pointing in exactly opposite directions. For example, in carbon dioxide (a linear molecule), the carbon-oxygen bonds have a large dipole moment. However, because one dipole points to the left and the other points to the right, the dipoles cancel and overall there is no molecular dipole.
How might a molecule with two strong bond dipoles have no molecule dipole at all?
A molecule with two strong bond dipoles can have no molecular dipole if the bond dipoles cancel each other out by pointing in exactly opposite directions. For example, in carbon dioxide (a linear molecule), the carbon-oxygen bonds have a large dipole moment. However, because one dipole points to the left and the other points to the right, the dipoles cancel and overall there is no molecular dipole.
How does a molecule that has polar bonds be nonpolar?
A molecule with polar bonds can be overall non-polar if the bond dipoles cancel each other out. For example the following all have polar bonds but the bond dipoles cancel each other out (vector addition) to make the molecule non-polar. Linear - CO2 trigonal planar - BF3 tetrahedral molecules, CF4 trigonal bipyramidal PF5 octahedral SF6
How can a molecule be non polar when it consists of atoms that have different electronagativities?
When the bond dipoles cancel one another out. Fro example in CCl4 the bonds are polar but the molecule is non-polar (no dipole moment) as the bond dipoles all cancel out.
Why is cyclohexane a nonpolar molecule The electronegativity difference between Carbon and Hydrogen is point 5 so why is it nonpolar?
Since syclohexane is a symmetrical molecule, the sum of the bond dipoles is zero and the molecules is therefore non-polar
