IB Bonding
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| Ionic bond | electrons transferred from one atom to another to form ions with complete outer shells of electrons. High melting pt.
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| Polyatomic ions | charge is delocalized over whole ion
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| Covalent bonding | sharing of one or more pairs of electrons so that each atom in the molecule achieves a stable outer shell of electrons
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| Single covalent bond | sharing of one pair of electrons. sigma bond. longest and weakest covalent bond.
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| Double covalent bond | sharing of two paris of electrons. sigma and pi bond. moderate covalent bond length and strength
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| triple covalent bond | sharing of three pairs of electrons. sigma and two pi bonds. shortest and strongest covalent bond.
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| co-ordinate covalent bond | electrons in the shared pair originate from the same atom
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| Polar bonds | when one atom is more electronegative than another resulting in slightly + and - atoms
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| VSPER theory (valence shell electron pair repulsion) | pairs of electrons arrange themselves around the central atom so that they are as far apart from each other as possible. greater repulsion between non-bonded pairs than between bonded pairs.
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| linear | 180
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| trigonal planar | 120
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| tetrahedral | 109.5
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| trigonal bipyramidal | 90, 120
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| octahedral | 90
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| how to work out the actual shape | calculate the number of pairs of electrons around central atom, work out how many bonding pairs/non-bonding pairs
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| molecular polarity | depends on relative electronegativities of the atoms and on the shape
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| Van der Waals forces | electrons unevenly spread at any one moment that produces temporary instantaneous dipoles that induce another dipole in a neighboring particle. Increase with increasing mass.
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| intermolecular forces | forces of attraction between molecules
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| dipole-dipole forces | polar molecules are attracted to each other by electrostatic forces. stronger than Van der Waals
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| hydrogen bonding | occurs when H is bonded directly to a small, highly electronegative element like F, O, N, resulting in a very strong dipole-dipole force.
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| metallic bonding | valence electrons in metals become detached from the atoms so that metals consist of a close packed lattice of positive ions in a sea of delocalized electrons.
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| Melting and Boiling Points | indicates strength of intermolecular forces. BP is when the attractive forces are completely broken; MP is when the crystal solid structure is broken and some intermolecular forces remain
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| solubility | "like dissolves like". Polar dissolves in polar, non-polar in non-polar. The longer an organic molecule, the less soluble it is in water.
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| Conductivity | substance must possess electrons or ions that are free to move. Metals and molten ionic salts conduct electricity.
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| sigma bond | formed when two atomic orbitals on different atoms overlap "head-on".
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| pi bond | formed when two p orbitals overlap "sideways-on". Made of two regions of electron density
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| sp3 hybridization | 4 sp orbitals, 4 single bonds. tetrahedryl shape
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| sp2 hybridization | 3 sp orbitals, 1 p orbital. 3 single bonds; 2 single bonds, 1 double bond. trigonal planar shape
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| sp hybridization | 2 sp orbitals, 2 p orbitals. 2 single bonds; 2 double bonds; 1 single 1 triple bond. linear shape
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| resonance structure | when it is possible to write more than one correct structure with regard to bonds.
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| delocalization of electrons | can occur whenever alternate double and single bonds occur between carbon atoms.
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| diamond | sp3 hybridized.
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| graphite | sp2 hybridized. delocalized electrons-conduct electricity.
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