<span>Naphthalene has a higher melting point than biphenyl because naphthalene is a polar compound while biphenyl is a non-polar compound.</span> Studies show <span>that polar compounds have higher melting and boiling points than nonpolar compounds. It is because polar compounds have strong intermolecular forces.</span>
To classify the elements and make them easier to understand
Answer:
True
Explanation:
It is true as metals form a positive ion when they take part in a chemical reaction. Nonmetals form an anion when bonding.
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Answer: D) The effect of gravity on an object
Explanation: We're not talking about mass, we're talking about weight. Weight is measured by the force of gravity on a object. For examples, you might be 100 pounds on Earth but 12 pounds on the moon.
Answer:
- <em>The strongest type of intermolecular force present in </em>CHF₃<em> </em><u>is dipole - dipole interaction.</u>
Explanation:
There are 3 basic types of<em> intermolecular forces</em> (forces between molecules):
- London dispersion force
- Dipole - dipole force
- Hydrogen bonds.
London dispersion forces are weak attraction forces between molecules due to temporary displacement of the electron density over the atoms, resulting in the formation of temporary dipoles. The electrostatic attraction between those dipoles is the weak dispersion force.
Dipole - dipole attraction forces happen in polar molecules, such as CHF₃, because the dipoles are permanent. The dipoles are the result of the assymetryc distribution of the electron charge, due to the presence of atoms with different electronegativities. In CHF₃, F is much more electronegative than C, causing the uneven distribution of the electrons, which leads to the formation of the dipoles and the dipole - dipole forces which are stronger than london dispersion forces.
Hydrogen bonds, the strongest intermolecular forces, are only present when hydrogen is bonded to a small a very electronegative atom, like oxygen, nitrogen or fluor. Since, in CHF₃, hydrogen is bonded to C, there is not formation of hydrogen bonds.
