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15 Cards in this Set
- Front
- Back
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metallic bond |
- EFOA between sea of delocalized electrons and metal cations - giant metallic lattice structure - strength of metallic bond depends on size of cation, charge & no. of delocalized electrons |
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properties of metals |
1) high mp = strong EFOA 2) malleable & ductile = layers of cations can slide over each other and remain connected via sea of delocalized electrons 3) good electrical conductors = mobile charge carriers |
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alloys |
- usually lower melting point than pure metals - can conduct electricity - not as malleable & ductile as pure metals - larger atoms disrupt lattice structure |
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electronegativity |
measure of an atom's ability to attract electrons in a covalent bond to itself |
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ionic bond |
- EFOA between oppositely charged ions due to the complete transfer of electrons - giant ionic lattice structure - strong EFOA - non-directional ionic bond |
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properties of ionic compounds |
- hard but brittle = when force is applied, same charge ions will repel each other away - high melting point = strong EFOA - conduct electricity only in molten/aqueous states = mobile ions persent after EFOA are overcome - soluble in water = water forms ion-dipole bond to break lattice structure - insoluble in organic solvent = do not react |
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covalent bond |
- EFOA between shared pair of electrons & the nuclei of both atoms - between non-metallic atoms whose difference in electronegativity is not too big - single/double/triple bond |
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simple molecular structure |
- weak intermolecular forces (van der waals' forces/hydrogen bond) - discrete molecules |
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hydrogen bond |
- EFOA between atoms with big difference in electronegativity - lowers density = open structures with empty spaces - only for F, N, O |
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properties of simple molecular structure compounds |
- low mp/bp = weak intermolecular FOA/van der Waals' forces - not able to conduct electricity = no mobile ions/electrons - insoluble in water - soluble in organic solvent |
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giant molecular structure |
- produces allotropes - giant network of atoms that are covalently bonded |
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properties of giant molecular compounds |
- high melting point = strong covalent bonds - very hard (tetrahedron), soft & slippery (layers) - does not conduct electricity (tetrahedron), conducts electricity (layers) |
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tetrahedron |
- diamond & silicon dioxide - 1 atom bonded tetrahedrally to 4 other atoms by strong covalent bonds - diamond is lightly packed - silicon dioxide is loosely packed |
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layers |
- graphite - hexagonal layers of atoms - within each layer, 1 atom forms strong covalent bonds with 3 other atoms - 1 atom is left delocalized - weak van der Waals' FOA holding the layers together |
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dot & cross diagram |
- no electrons are to be drawn for cation - don't draw electrons for catio next to each other in anion - only use ● or ×, no ○ |
