Chemistry Unit 3 Test Answers

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  They typically tend to only affect the solid and liquid phases. Three types of intermolecular forces exist between electrically neutral molecules: London dispersion forces, dipole-dipole attractions, and hydrogen bonding. And another kind of attractive force, ion-dipole is important in solutions. They are the only types of forces to exist between two non-polar molecules and noble gases solid or liquid form. They can easily be forgotten so make sure they always show up in your answer along with any other forces present! At any given time, one nonpolar molecule might have more electrons on one side than another side, making it polar. For that instant, the molecule would have a partial negative side and a partial positive side and it becomes a temporary dipole.
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  That temporary dipole molecule then induces a dipole on its neighboring molecule and there are LDF forces between the partial negative side of one molecular and the partial positive side of another molecule. This is because more electrons yield a stronger instantaneous dipole due to a more polarizable electron cloud. Polarizability is the ease at which an electron cloud could be distorted to give a dipole charge distribution. Dipole-Dipole Interactions Dipole-Dipole attractions occur due to the opposite partial charges that exist on the opposite ends of a dipole.
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  Dipole-dipole attractions only occur in a sample of polar molecules and are slightly stronger than LDFs. The dipoles in HCl lead to a positive side and a negative side that are attracted to each other Image Courtesy of EMedicalPrep As you decrease the distance between the two dipoles, you strengthen the attraction and dipole-dipole interaction. This also means that the more polar the molecules, the greater the dipole-dipole attraction, which also relates to higher melting and boiling points. All credit to College Board. In terms of the types and relative strengths of all intermolecular forces in each compound, explain why the boiling point of CS2 l is higher than that of COS l. Therefore, CS2 has a higher boiling point.
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  The hydrogen bonded to the F, O or N is partially positively charged and is attracted to the neighboring unshared electrons on the F, O, or N. Since these attractions are so so strong, the boiling points of molecules with hydrogen bonds are very high! An example of a molecule that has hydrogen bonding is water H2O. Let's clear a quick misconception before moving on: On the AP Exam, you may be asked to draw a molecule with the proper orientation and create hydrogen bonding. Fiveable's here to help! Image Courtesy of ck An example of an ion-ion interaction would be NaCl being attracted to other NaCl molecules to form a crystal lattice.
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