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Van der Waals Forces
CAVA chem302 303 4.14/4.15 Van der Waals Forces
| Question | Answer |
|---|---|
| The attraction and repulsion between molecules, are called [...] forces. | The attraction and repulsion between molecules, are called intermolecular forces. |
| Polar molecules do not share valence electrons [...-li]. | Polar molecules do not share valence electrons equally. |
| Unequal electron sharing makes one atom partially [...] and the other partially [...]. | Unequal electron sharing makes one atom partially negative and the other partially positive. |
| Polar molecules are sometimes called [...] because they have poles at two (di) ends. | Polar molecules are sometimes called dipoles because they have poles at two (di) ends. |
| Opposite charges [...]; like charges [...]. | Opposite charges attract; like charges repel. |
| A '[...] Moment' is not (as the name suggests) a moment. It's a measure of how polar a molecule is. | A 'Dipole Moment' is not (as the name suggests) a moment. It's a measure of how polar a molecule is. |
| Forces of attraction and repulsion between polar molecules are called [...]-[...] forces. | Forces of attraction and repulsion between polar molecules are called dipole-dipole forces. |
| Sometimes non-polar molecules become momentarily [...] because electrons just happen to be on one side. | Sometimes non-polar molecules become momentarily polar because electrons just happen to be on one side. |
| A momentary polarity in an otherwise non-polar molecule can induce [...] in other molecules. | A momentary polarity in an otherwise non-polar molecule can induce polarity in other molecules. |
| The force of attraction due to chance moments of polarity in one molecule (and induced polarity on other molecules) is called [...] (or [...]) force. | The force of attraction due to chance moments of polarity in one molecule (and induced polarity on other molecules) is called Dispersion (or London) force. |
| The [...-er] the molecule, the stronger the Dispersion (aka London) Forces will be. | The larger the molecule, the stronger the Dispersion (aka London) Forces will be. |
| Wax is an example of a large non-polar molecule held together entirely by [...] forces. | Wax is an example of a large non-polar molecule held together entirely by Dispersion (aka London) forces. |
| [...] forces explain why a gecko's feet stick to glass (and other surfaces), and how they can walk on the ceiling. | Dispersion (aka London) forces explain why a gecko's feet stick to glass (and other surfaces), and how they can walk on the ceiling. |
| [...] forces explain why some halogens are liquid or solid at room temperature. | Dispersion (aka London) forces explain why some halogens are liquid or solid at room temperature. |
| '[...] bonds' form between hydrogen atoms and partially negative atoms on adjacent molecules. | Hydrogen bonds' form between hydrogen atoms and partially negative atoms on adjacent molecules. |
| Hydrogen bonds explain why water [...] when it freezes. | Hydrogen bonds explain why water expands when it freezes. |
| Hydrogen bonds create surface [...] in liquid water. | Hydrogen bonds create surface tension in liquid water. |
| dipole-dipole, dispersion, and hydrogen bond forces are collectively called [...] forces. | dipole-dipole, dispersion, and hydrogen bond forces are collectively called Van de Waals forces. |
| Dipoles can also stick to ions. We call the forces of attraction here [...]-[...] forces. | Dipoles can also stick to ions. We call the forces of attraction here ion-dipole forces. |
| Even though chemists have all these names for different Van der Waals forces, these are ALL just examples of electrostatic force: the attraction between [...] electrical charges (and repulsion of [...] charges) | Even though chemists have all these names for different Van der Waals forces, these are ALL just examples of electrostatic force: the attraction between opposite electrical charges (and repulsion of like charges) |
Created by:
mr.shapard
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