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17 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Ionic Bonds (definition) |
Formed when electrons are transferred from one atom to another to form ions with full outer electron shells |
Electrons are transferred One atom to the next Full outer electron shells |
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Ionic Bonds (properties) |
-strong lattice -high melting point -no conductivity -overall charge: 0 |
Lattice Melting point Conductivity Charge |
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Polyatomic ions |
Ions containing more than one element; charge is spread (delocalized) over the whole ion; ex. sulfate So4^2- |
Multiple elements Delocalization |
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Covalent Bonds (definition) |
Formed by the sharing of one or more electron pairs to make each molecule achieve a noble gas configuration |
Sharing of electrons Noble gas configuration |
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Covalent Bonds (properties) |
-single bonds: longest, weakest, non-polar -double bonds: shorter, stronger, polar -triple bonds: shortest, strongest, polar |
3 types of bonds |
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Geometry |
-2 electron domains: linear, 180° -3: trigonal planar, 120° -4: tetrahedral, 109.5° -5: trigonal pyramidal, 90° 120° 180° |
No. of electron domains Shape name Bond angle(s) |
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Allotropes of Carbon |
1) Diamond: carbon atoms covalently bonded to 4 other carbons; very hard, strong bonds, no conductivity 2) Graphite: carbon atoms strongly bonded to 3 other carbons in hexagonal rings; bonds are weak between layers, good conductivity (sliding between layers) 3) Bucky Ball: 60 carbon atoms in hexagons and pentagons that form a ball |
3 kinds |
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Intermolecular Forces (IMF’s) |
1) London Dispersion Forces: weakest; for non-polar molecules; strength increases with mass 2) Dipole-dipole Forces: 2nd weakest; in polar molecules attracted by electrostatic forces 3) Hydrogen Bonds: the strongest; when hydrogen bonds directly with small, electronegative elements (ex. F, O, N) |
3 kinds |
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Melting Point |
-occurs only in solids -when the crystal structure is broken down but some attractive forces between particles remain |
Solids Break down of crystal structure |
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Boiling Point |
-when a liquid turns into a gas -the attractive forces between particles break completely |
Liquid to gas Forces break off |
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Conductivity |
-for it to occur substances must have free-to-move (delocalized) electrons -good in: metals, graphite, molten ionic salts -none in: diamond, simple molecules |
Delocalized electrons Good in None in |
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Solubility |
-polar substances dissolve in polar solvents (ex. water) -non-polar substances dissolve in non-polar solvents (ex. heptane) |
Like dissolves in like |
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Metals (lead-up to Metallic Bonding) |
-a close-packed lattice of positive ions in a clump of delocalized electrons (due to detached valence electrons from individual atoms) -malleable and ductile (due to layers positive ions being able to slide over themselves without breaking bonds) |
Close-packed in a sea Malleable and ductile |
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Metallic Bonding |
-the attraction two neighbouring positive ions have for delocalized electrons |
Positive ions and delocalized electrons |
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Alloys |
-aka metallic solid -made from multiple metals -less ductile and malleable than pure metals |
Aka _______ ________ Multiple metals combined Less m_____ and d______ |
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Solid States |
-ionic: ex. NaCl, CaF, CaCo3 -molecular covalent: allotropes -network covalent: when it isn’t any of the others -metallic: lone metal, ex. Cu, Fe |
4 states |
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General Knowledge Chain |
-when given an element/molecule, know its: molecular formula, Lewis structure, shape (geometry), polarity, IMF’s, and properties |
When given an element/molecule... |
