Structure and Bonding revision.

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  • Created by: ElishaG
  • Created on: 05-02-17 13:05
What is ionic bonding?
The electrostatic attraction between positive and negative ions.
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What is a giant ionic lattice?
A 3D structure of oppositely charged ions, bonded by strong ionic bonds.
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What is metallic bonding?
The attraction of positive metal ions to delocalised electrons.
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What is periodicity?
The repeating pattern of properties across different periods of the periodic table.
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What is conductivity?
The degree to which a substance conducts electricity.
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What is solubility?
A measure of how well one substance dissolves into another.
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What is melting point?
The temperature at which a solid melts.
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What is boiling point.
The temperature at which a solid boils.
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What gives substances their physical properties?
Their bonding (covalent,ionic or metallic) and structure (simple or giant).
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Why do ionic compounds have high melting and boiling points?
1)Strong electrostatic forces of attraction between oppositely charged ions.2)High amounts of energy is required to break these bonds.
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What is the electrical conductivity of ionic compounds?
1)Conduct when aqueous or molten as ions are free to carry the charge. 2)Do NOT conduct when solid as ions are in a fixed lattice.
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What is the solubility of ionic compounds?
1)Generally soluble in polar solvents e.g. water. 2) Insoluble in non-polar solvents e.g. hexane.
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Why are ionic compounds usually soluble in water?
The slightly positive H ion attracts the negative ions in ionic compound.2)The slightly negative O ion attracts positive ions in ionic compound. 3)Water molecules pull ions away from lattice-they dissociate.
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Why do metals have high melting and boiling points?
1)Strong metallic bonds between positive ions and delocalised electrons.2)Lots of energy needed to break these bonds.
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Why does the melting point of the metals increase from Na to Al?
1)Charge of ions increases.2)More delocalised electrons per ion.3)Stronger attraction between positive metal ions and delocalised electrons.4)More energy needed to overcome attractions.
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Why do metals conduct electricity?
Delocalised electrons are free to move and carry the charge.
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Why is the electrical conductivity of aluminium higher than sodium?
1)Both Al and Na are giant metallic lattices.2)Al has more delocalised electrons per ion than Na.
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What is the solubility of metals?
Insoluble in both polar and non-polar solvents.
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Explain the physical properties of diamond in terms of structure and bonding.
1)Giant covalent structure.2)Hard and high melting point.3)Strong covalent bonds between carbon atoms.4)High amount of energy required to break these bonds.
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Explain the electrical conductivity of diamond.
1)Diamond cannot conduct electricity. 2) There are no delocalsied electrons to carry the charge.
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What is the solubility of diamond?
1)Insoluble in polar and non-polar solvents.2)Attractions between solvent molecules and carbon atoms not strong enough to overcome strong covalent bonds.
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What holds sheets of graphite together?
Weak van der Waals forces.
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Why does graphite have a high melting point?
There are strong covalent bonds between carbon atoms within layers so lots of energy is needed to break bonds.
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Explain the electrical conductivity of graphite.
1)Conducts electricity.2)Delocalised electrons free to move along layers.
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What is the solubility of graphite?
1)Insoluble in any solvent.2)Attractions between solvent molecules and carbon atoms will never be strong enough to overcome covalent bonds.
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What are the properties of graphene?
1)Very strong for its low weight.2)Good electrical conductor.3)Good conductor of heat.
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Explain the physical properties of silicon in terms of its structure and bonding.
1)Giant covalent structure.2)Hard and high meting point- lots of energy to break covalent bonds.3)Doesn't conduct electricity.
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Why does iodine have a low melting point?
1)Simple molecular.2)Little energy needed to break weak induced dipole-dipole attractions.
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Why does iodine not conduct electricity?
There are no mobile ions or delocalised electrons.
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What is the solubility of iodine like in polar solvents?
1)Partially soluble.2)Hydrogen bonds too strong for simple structures to break.3)Simple structures unable to make hydorgen bonds with water molecules. Solution turns light brown I2(aq).
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What is the solubility of iodine like in non polar solvents?
1)Soluble.2)Weak van der Waals forces weak enough for simple structures to break.3)Simple structures able to make weak van der Waals forces with non-polar solvents. Solution turns purple, I2(org).
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Why is the boiling point of water higher than expected?
1)It has hydrogen bonds that are stronger than the other types of intermolecular force.2)More energy is needed to break them.
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Explain why ice is less dense than water.
1)Hydrogen bonds hold molecules in ice in an open lattice structure.2)Lattice structure collapses when ice melts.3)Molecule are further apart in ice than water.
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Explain the melting points of P4/S8/Cl2 in terms of structure and bonding.
1)Simple molecular.2)Small amount of heat energy required to overcome weak van der Waals between molecules.
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Explain the conductivity of P4/S8/Cl2 in terms of structure and bonding.
1)All simple molecular.2)Electrons all localised in covalent bonds.
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Explain the trend in melting point of S8/P4/Cl2.
1)Simple molecular.2)MP determined by strength of van der Waals forces-which is determined by molecule size.3)S8 has biggest molecule, so highest MP. P4 has more electrons than Cl2- P4 need more energy to break bonds so higher MP/
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Other cards in this set

Card 2

Front

What is a giant ionic lattice?

Back

A 3D structure of oppositely charged ions, bonded by strong ionic bonds.

Card 3

Front

What is metallic bonding?

Back

Preview of the front of card 3

Card 4

Front

What is periodicity?

Back

Preview of the front of card 4

Card 5

Front

What is conductivity?

Back

Preview of the front of card 5
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