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9 Cards in this Set
- Front
- Back
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Lewis theory |
Valence electrons are represented as dots surrounding four sides of achemical symbol. Single Electrons = unpaired electrons. Two electrons = lone pair of electrons. |
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Covalent Bonding |
When electrons (or electron density) within a covalent bond arecompletely shared between two atoms (ΔEN between 0 and 0.4). When two unpaired electrons combine |
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Polar Covalent Bonding |
When electrons (or electron density) within a covalent bondare unequally shared between two atoms (ΔEN between 0.4 and 2.0) |
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Ionic Bonding |
When electrons (or electron density) are transferred from one atom tothe other (ΔEN between 2.0 and 3.3) |
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Strength of Ionic Bonds |
Ions combine in a crystal lattice, alternating cations and anions. Stabilizing energy is called lattice energy. High amounts of energy are released when this occurs, which is why they are so hard to break. |
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Size of ion |
smaller ion = closer the ions can pack together and an increased lattice energy will occur. |
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Charge of the ion |
The greater charge of an ion the stronger the electrostatic interactions between ions |
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Properties of Ionic Compounds (3) |
Good conductors when dissolved in water. Poor conductors in solid state. High melting points. |
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Metallic Bonding |
Metals valence electrons are very weakly bound to the nucleus, causing a 'sea' of delocalized electrons. very good conductors. |
