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17 Cards in this Set
- Front
- Back
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A mole |
Mole is the unit of 'amount of substance' |
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Moles of solid =.... |
Mas/ Mr |
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1 mole of any gas is ..... at r.t.p |
1 mole of any gas is 24dm3 at r.t.p |
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Moles of Solution |
conc x vol/1000 |
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Conc |
moles x 1000/vol |
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Orbital |
An Orbital is the area in which an electron spends 95% of its time |
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Ionic bond |
Ionic bond is the attraction between a positive and a negative ion |
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Covalent bond |
A covalent bond is a shared pair of electrons |
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Dative Covalent bond |
Dative Covalent bond occurs when both electrons come from the same atom |
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2 Electron groups |
2 electron groups: linear 180* e.g. BeCl2 |
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3 electron groups |
3 electron groups: trigonal planar 120* eg BF3 and ethene |
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4 electron groups |
tetrahedral 109* e.g. CH4 |
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6 electron groups |
6 electron groups: octahedral 90* eg SF6 |
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Electronegativity |
-Electronegativity is the tendency to attract electrons within a covalent bond. -The most electronegative atoms are in the top right of the periodic table - Electronegativity results in polar bonds - Some molecules with polar bonds have no overall polarity because they symmetrical: the dipoles cancel out. |
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Instantaneous dipoles |
Instantaneous dipoles are caused by random movement of electrons in atoms and molecules. They occur in all molecules but are weak. Instantaneous dipoles can induce dipoles in neighbouring molecules This causes a weak instantaneous dipole-induced dipole bond. The larger the molecule, the greater the effect of instantaneous dipole- induced dipole bonds |
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Permanent dipoles |
- Molecules with an electronegative atom have permanent dipoles - They have permanent dipole - permanent dipole intermolecular bonds, which are stronger than instantaneous dipole - induced dipole bonds - The stronger the intermolecular forces, the higher the boiling point of the substance |
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Oxidation |
s |
