Chemistry - Bonding (1.3)

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Giant Ionic Lattices
Conducts electricity when molten/dissolved. High melting points (strong attraction between positive ions and negative delocalised electrons). Dissolve in water (polar water molecules pull ions from lattice)
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Giant Covalent Lattices- Graphite
Carbons arranged in sheets, covalently bonded with 3 carbons each (4th electron= delocalised). Slippery/ sheets slide over each other (Van der Waal's). Conducts electricity (delocalised electrons). High melting point (strong covalent). Insoluble.
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Giant Covalent Lattices- Diamond
Each carbon atom covalently bonded to 4 other carbons. High melting point, hard, good thermal conductor (vibrations travel easily through stiff structure (strong covalent). Cant conduct electricity (outer electrons in localised bonds). Insoluble.
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Why do simple covalent structures have low melting and boiling points>?
Because only weak intermolecular forces have to be broken.
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Why do giant covalent structures have high melting and boiling points?
Have to break strong covalent bonds.
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Co-ordinate/Dative Covalent Bonds
One atom provides both shared electrons- when one atom has a lone pair and the other atom doesnt have any electrons to share.
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What does solubility depend on?
Type of particles- polar/charged= dissolves easily.
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Metallic Bonding
Outermost shell of electrons is delocalised, positive ion lattice closely packed with sea of delocalised electrons. High melting point. Malleable and ductile. Conducts electricity and heat. Insoluble.
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Bonding Pairs
Shared electrons
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Lone pairs / Unbonding pairs
Unshared electrons
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Charge Cloud
Area with a big chance of finding an electron. Repel until as far apart as possible.
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Valence Shell Electron Pair Repulsion Theory
Lone pair charge clouds repel more than bonding pair charge clouds - bond angles reduced.Repel until as far apart as possible.
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2 bonding pairs
Linear (180)
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3 bonding pairs
Trigonal Planar (120)
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4 bonding pairs
Tetrahedral (109.5)
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5 bonding pairs
Trigonal Bipyramidal (120 and 90)
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6 bonding pairs
Octahedral (90)
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What do you do to the bonding angles for each lone pair?
Subtract 2.5
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How do you find the number of electron pairs?
1. Central atom. 2. No. electrons in outer shell. 3 Add 1 for every atom bonded to. 4. If an ion, add 1 for each - charge and minus 1 for each + charge. 5. Add up electrons. 6. Compare no. electron pairs to bonds to find no. lone pairs.
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Electronegativity
Ability to attract electrons in a covalent bond. F, O, N.
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Van der Waal's
Weakest. Temporary dipoles attracted to each other cause domino effect.
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Permanent Dipole
Attraction between positive and negative charges in neighbouring polar molecules.
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Hydrogen Bonding
Strongest. Need H covalently bonded to F, N or O. Covalent bond is so polarised, and H has such a high charge density, H forms weak bonds with lone pairs on F, N or O.
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Simple Covalent Molecules
Strong covalent bonds between molecules, but weak forces between molecules. Don't conduct electricity (no delocalised electrons), low melting point (weak intemolecular forces) and some are soluble (depending on polarity).
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Metallic Bonding
Positive ions in sea of delocalised electrons. High melting point (strong attrraction between positive ions and negative delocalised electrons). Malleable and ductile (no bonds holding specific ions togethe). Conducts electricity and heat
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How do you find the number of electron pairs?
1. Central atom. 2. No. electrons in outer shell. 3 Add 1 for every atom bonded to. 4. If an ion, add 1 for each - charge and minus 1 for each + charge. 5. Add up electrons. 6. Compare no. electron pairs to bonds to find no. lone pairs.
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Electronegativity
Ability to attract electrons in a covalent bond. F, O, N.
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Van der Waal's
Weakest. Temporary dipoles attracted to each other cause domino effect.
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Permanent Dipole
Attraction between positive and negative charges in neighbouring polar molecules.
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Hydrogen Bonding
Strongest. Need H covalently bonded to F, N or O. Covalent bond is so polarised, and H has such a high charge density, H forms weak bonds with lone pairs on F, N or O.
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Simple Covalent Molecules
Strong covalent bonds between molecules, but weak forces between molecules. Don't conduct electricity (no delocalised electrons), low melting point (weak intemolecular forces) and some are soluble (depending on polarity).
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Metallic Bonding
Positive ions in sea of delocalised electrons. High melting point (strong attrraction between positive ions and negative delocalised electrons). Malleable and ductile (no bonds holding specific ions together). Conducts electricity and heat
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How do you find the number of electron pairs?
1. Central atom. 2. No. electrons in outer shell. 3 Add 1 for every atom bonded to. 4. If an ion, add 1 for each - charge and minus 1 for each + charge. 5. Add up electrons. 6. Compare no. electron pairs to bonds to find no. lone pairs.
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Electronegativity
Ability to attract electrons in a covalent bond. F, O, N.
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Van der Waal's
Weakest. Temporary dipoles attracted to each other cause domino effect.
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Permanent Dipole
Attraction between positive and negative charges in neighbouring polar molecules.
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Hydrogen Bonding
Strongest. Need H covalently bonded to F, N or O. Covalent bond is so polarised, and H has such a high charge density, H forms weak bonds with lone pairs on F, N or O.
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Simple Covalent Molecules
Strong covalent bonds between molecules, but weak forces between molecules. Don't conduct electricity (no delocalised electrons), low melting point (weak intemolecular forces) and some are soluble (depending on polarity).
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Metallic Bonding
Positive ions in sea of delocalised electrons. High melting point (strong attrraction between positive and negative). Malleable/ductile (no bonds holding specific ions). Conducts electricity and heat (delocalised electrons). Insoluble-strongmetallic.
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Other cards in this set

Card 2

Front

Giant Covalent Lattices- Graphite

Back

Carbons arranged in sheets, covalently bonded with 3 carbons each (4th electron= delocalised). Slippery/ sheets slide over each other (Van der Waal's). Conducts electricity (delocalised electrons). High melting point (strong covalent). Insoluble.

Card 3

Front

Giant Covalent Lattices- Diamond

Back

Preview of the front of card 3

Card 4

Front

Why do simple covalent structures have low melting and boiling points>?

Back

Preview of the front of card 4

Card 5

Front

Why do giant covalent structures have high melting and boiling points?

Back

Preview of the front of card 5
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