BONDING : STURCTURE AND PROPERTIES
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- Created by: samsh
- Created on: 01-06-16 15:47
definition of an ionic bond
Strong electrostatic force of attraction between oppositely charged ions
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why does an ionic substance have a high melting point?
'X' Has an ioinc structure. A large amount of energy is needed to overcome a strong electrostatic attraction between the positive and negative ions
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why does an ionic substance not conduce electricity when a solid?
'X' has an ionic structure. The ions are fixed in a lattice structure and cannot move
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why does an ionic substance conduct electricity when molten or in aqueous solution
'X' has an ionic structure . The ions are free to move, so they can carry charge in one direction.
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why does an ionic substance dissolve well in polar solvents such as water?
'X' has an ioni structure. Polar solvent molecules attract ions out of the lattice into solution
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why is an ionic substance brittle
'X' has an ionic structure. the layers in the ionic lattice cant slide over each other.
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definition of metallic bonding
Strong electrostatic force of attraction between positive metal ions and delocalised electrons
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why do metallic substances have a high melting and boiling point
'X' has a metallic structure. A large amount of energy is required to break/overcome the strong electrostatic attraction between the positive ions and delocalised electrons
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why do metallic substances conduct electricity when solid or molten
'X' has a metallic structure. The delocalised electrons are free to move between the metal ions, so they can carry carry charge in one direction
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why are metallic substances malleable and ductile?
'X' has a metallic structure. The layers of ions in the metallic lattice can slide over each other due to delocalised electrons.
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definition of covalent bonding
A strong bond formed by a shared pair of electrons
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give two examples of giant covalent lattices
Diamond and Graphite
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Explain the carbon arrangement in diamond...
Each carbon atom is covalently bonded to 4 other carbon atoms in a tetrahedral arrangement.
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Explain why diamond has a very high melting and boiling point
has a giant covalent structure. A large amount of energy is required to break the strong covalent bonds between all atoms.
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Explain why diamond is extremely hard
Diamond has a giant covalent structure. All atoms are joined by strong covalent bonds in 3D.
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Explain why diamond does not conduct electricity
Diamond has a giant covalent structure. The electrons are fixed in the covalent bonds and cannot move.
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Explain the arrangement of carbons in Graphite
each carbon atom is bonded to 3 other carbon by strong covalent bonds in a hexagonal arrangement. they are arranged in layers which are held by Van Der Waals.
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Explain why Graphite has a high melting and boiling point
graphite has a giant covalent structure. A large amount of energy is required to break the strong covalent bonds between the atoms in the layers of C atoms.
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Explain why Graphite is soft
The weak van der Waals intermolecular forces between the layers of C atoms allow the layers to slide over each other.
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Explain why Graphite conducts electricity
graphite has a giant covalent structure, with delocalised elctrons between the layers of C atoms. the delacalsied electronsa re free to move between the layers, can can carry charge in one direction
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Give the definition of dative covalent bonding
a bond formed by a shared pair of electrons where both electrons come from one atom
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Give the definition of electro negativity
the power of an atom to attract the pair of electrons in a covalent bond
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what happens to electro negativity across a period?
Increases apart from group 8
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what happens to electro negativity down a group?
Deceases
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What are the three types of intermolecular forces?
Van der Waals' // permanent dipole-dipole forces // Hydrogen Bonding
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Explain what happens to the melting/boiling point when the size of molecule increases
the larger the atom/molecule the stronger the van der waals between molecules... and the higher the melting point and boiling point of the atom/ molecule becomes
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Explain what happens to the melting/boiling point when the amount of branching increases
the amount of branching increases the contact surface area between molecules decreases. so the van der waals intermolecular forces between molecules become weaker and the melting/boiling point decreases
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state how hydrogen bonding in ammonia arises
lager electro negativity different between N and H. Dipole is formed where N is and H is. The lone pair on the N forms a weak interaction with the H on the other molecule
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Other cards in this set
Card 2
Front
why does an ionic substance have a high melting point?
Back
'X' Has an ioinc structure. A large amount of energy is needed to overcome a strong electrostatic attraction between the positive and negative ions
Card 3
Front
why does an ionic substance not conduce electricity when a solid?
Back
Card 4
Front
why does an ionic substance conduct electricity when molten or in aqueous solution
Back
Card 5
Front
why does an ionic substance dissolve well in polar solvents such as water?
Back
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