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| Question | Answer |
| What are intermolecular forces? | Weak interactions between dipoles of different molecules. |
| Intermolecular forces fall into which 3 categories? | Induced dipole-dipole interactions (London forces) Permanent dipole-dipole interactions Hydrogen bonding |
| Intermolecular forces are largely responsible for what? | Physical properties such as melting and boiling points. |
| Covalent bonds determine what? | Identity and chemical reactions of molecules |
| What are induced dipole-dipole interactions? (London forces) | Weak intermolecular forces that exist between all molecules, whether polar or non-polar. They act between induced dipoles in different molecules. |
| What is the origin of induced dipoles? | - Movement of electrons produced a changing dipole in a molecule - At any instant, an instantaneous dipole will exist, but its position is constantly shifting - The instantaneous dipole induces a dipole on a neighbouring molecule - The induced dipole induces further dipoles on neighbouring molecules, which then attract one another |
| Are induced dipoles temporary or permanent? | Temporary |
| Induced dipoles result from interactions of electrons between molecules. The more electrons in each molecule ....(3) | - The larger the instantaneous and induced dipoles - The greater the induced dipole-dipole interactions - The stronger the attractive forces between molecules |
| What is the correlation between larger induced dipoles and boiling point? | - Larger numbers of electrons mean larger induced dipoles - More energy is then needed to overcome the intermolecular forces, increasing the boiling point |
| What is van der Waals' forces? | Used for both permanent and induced dipole-dipole interactions |
| What are permanent dipole-dipole interactions? | Permanent dipole-dipole interactions act between the permanent dipoles in different polar molecules. |
| Polar molecules have ______ dipole interactions as well as permanent dipole-dipole interactions. | Induced |
| Draw a diagram showing permanent dipole-dipole interactions between hydrogen chloride, HCl, molecules. | |
| HCl and F2 have the same number of electrons and the same shape, so the strength of the London forces in hydrogen chloride and fluorine should be similar. Why is HCl's boiling point higher than fluorine? | - Fluorine molecules are non-polar and only have London forces between molecules - Hydrogen chloride molecules are polar and have London forces and permanent dipole-dipole interactions between molecules - Extra energy is needed to break the additional permanent dipole-dipole interactions between hydrogen chloride molecules - The boiling point of hydrogen chloride is therefore higher than fluorine |
| In a solid state, simple molecules form a regular structure called what? | Simple molecular lattice |
| What is in the simple molecular lattice? | - the molecules are held in place by weak intermolecular forces - the atoms within each molecule are bonding together strongly by covalent bonds |
| Do simple molecular substances have high or low melting and boiling points? | Low |
| What happens when simple molecular substances are solidified into simple molecular lattices by reducing the temperature? | - In a simple molecular lattice, the weak intermolecular forces can be broken even by the energy present at low temperatures - Simple molecular substances have low melting and boiling points |
| What happens when a simple molecular lattice is broken apart during melting? | - only the weak intermolecular forces break - the covalent bonds are strong and do not break |
| Why are non-polar simple molecular substances soluble in non-polar solvents? | - When a simple molecular compound is added to a non-polar solvent, such as hexane, intermolecular forces form between the molecules and the solvent - The interactions weaken the intermolecular forces in the simple molecular lattice. The intermolecular forces break and the compound dissolves. |
| Why are simple molecular substances non-polar insoluble in polar solvents? | - When a simple molecular substance is added to a polar solvent, there is little interaction between the molecules in the lattice and the solvent molecules - The intermolecular bonding within the polar solvent is too strong to be broken |
| Can polar covalent substances dissolve in polar solvents? | Yes Polar solute molecules and polar solvent molecules can attract each other |
| What does solubility depend on? | Strength of the dipole and can be hard to predict |
| Give example of strength of dipole. | Ethanol C2H5OH, contains both polar (O-H) and non-polar (carbon chain) parts in their structure and can dissolve in polar and non-polar solvents |
| What happens when some biological molecules have hydrophobic and hydrophilic parts? (Solubility) | Hydrophilic part will be polar and contain electronegative atoms (oxygen) and can interact with water Hydrophobic part will be non-polar and comprised of a carbon chain |
| Property of electrical conductivity in simple molecular substances. | - There are no mobile charged particles in simple molecular structures - With no charged particles that can move, there is nothing to complete and electrical circuit. Non-conductors of electricity |
| Permanent dipole-dipole interactions exist in molecules with a what? | Polarity |
| The δ+ is acctracted to what? | δ- of another molecule |
| There are weak what forces that exist between molecules with a polarity? | Intermolecular forces |
| Unlike induced dipole-dipole forces, permanent dipole-dipole interactions involves molecules with a permanent dipole and so are ________. | Stronger |
| How can polar molecules like water be tested? | Placing a charged rod near a steady stream of polar liquid. You should see the liquid bent towards the rod as the molecules align to face the oppositely charged rod. |
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