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Description
Flashcards by owen.strafford, updated more than 1 year ago
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Created by owen.strafford
almost 9 years ago
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| Question | Answer |
| Describe the shape of a trigonal planar molecule ? | -It has 3 electron pairs, -120 degrees bonding angle, - 0 lone pairs. |
| Describe the shape of a tetrahedral molecule ? | - It has 4 electron pairs, - 109.5 degree bonding angle, - 0 lone pairs. |
| Describe the shape of a Octahedral molecule ? | - It has 6 electron pairs, - 90 degree bond angle, - 0 lone pairs. |
| Describe the shape of a Pyramidal molecule ? | - It has 3 electron pairs, - 107 degree bonding angle, - 1 lone pair. |
| Describe the shape of a Non-linear molecule ? | - It has 2 electron pairs, - 104.5 bonding angle, - 2 lone pairs. |
| What does a lone pair do to the shape of a molecule ? | the lone pairs repel more than a bonding pair therefore it decreases the bonding angle by repulsing the bonding pairs closer together. |
| What is the definition for electronegativity ? | the tendency of an atom to attract electrons in a covalent bond. |
| Describe what happens when 2 bonding atoms are different ? | If the bonding atoms are different, one of the atoms is likely to attract the bonding electrons more. The bonding atom with a greater attraction for the electron pair is more electronegative. |
| Is BF3 polar or non-polar? | It is non-polar because the shape is symmetrical and so the dipoles cancel out. |
| Is PF3 polar or non-polar? | It is polar because the shape is non-symmetrical and so the dipoles don't cancel out. |
| What are intermolecular forces ? | Forces that are weaker than ionic and covalent bonds, they are caused by weak attractive forces between very small dipoles in different molecules. |
| What are the 3 common types of intermolecular forces ? | - Hydrogen bonds, - Permanent dipole-dipole , - London forces. |
| What is a Permanent dipole-dipole interaction? | Its a weak attractive force between permanent dipoles in neighbouring polar molecules. |
| What is an induced dipole-dipole force? | Are weak intermolecular attractions between very small, temporary dipoles in neighbouring molecules. |
| What are London Forces ? | They are attractive forces between induced dipoles in neighbouring molecules. |
| Describe the why London forces create a chain reaction ? | the movement of electrons causes a instantaneous dipole to be formed across a molecule. This instantaneous dipole will induce a dipole in the neighbouring molecule, this then forms a chain of temporary dipoles. |
| How do you increase London forces? | The greater number of electrons the larger the induced dipole, therefore the greater the attractive forces between molecules. (Therefore the boiling points increase.) |
| What are the 2 bonds that make a hydrogen bonds ? | 0-H and N-H |
| What are the hydrogen bonds like in a molecule? | They're permanent dipoles and are polar. |
| How does the Hydrogen bonds work? | The electron deficient delta H+ on one molecule attracts the lone pair of electrons on the delta O- or the delta N- on a different molecule. |
| What is the ice-lattice structure ? | its an open network of H20 molecules, Oxygen has 4 bonds: - 2 covalent bonds, - 2 hydrogen bonds, - makes 6 sided shape. |
| Why does a lone pair of electrons repulse more than a bonding pair of electrons ? | Because the lone pair of electrons is slightly more electron dense than the bonding pairs of electrons. |
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