Bonding

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  • Created by: AK
  • Created on: 04-01-19 11:42
What is ionic bonding?
Strong electrostatic forces of attraction between oppositely charged ions held in a lattice
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How high are ionically bonded substances boiling point and melting point, why?
High - takes lots of energy to break strong electrostatic forces of attraction between oppositely charged ions
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Do ionic compounds conduct electricity, why?
Yes, when molten or in solution as the ions are free to move and carry charge
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What is simple molecular covalent bonding?
Strong covalent bonds between atoms, weak van der waals forces of attraction between molecules
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Are there any lone electrons in simple covalent bonding?
No - they are all involved in bonding
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Can simple molecular covalent molecules conduct electricity, why?
No - all electrons are used in bonding so aren't free to move
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Do simple molecular substances have a high or low melting point and boiling point, why?
Low - weak vdw forces of attraction between molecules that don't take much energy to overcome
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Describe macromolecular covalent bonding
Lattice of many atoms held together by strong covalent bonds
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Do substances with macromolecular covalent bonds have high or low melting points and boiling points, why?
High - it takes alot of energy to overcome many strong covalent bonds
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Do substances with macromolecular covalent bonds conduct electricity?
Most don't as all electrons are used in bonding
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Draw and describe the structure of diamond
3D tetrahetral structure of carbon atoms, with each carbon atom bonded to four others
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Draw and describe the structure of graphite
Macromolecular covalent, but each carbon atom is only bonded to 3 others, so it is in layers
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Draw and describe metallic bonding
Lattic of positive metal ions strongly attracted to a sea of delocalised electrons, layers can slide over each other
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Do metallic compounds have high or low boiling points and melting points, why?
High as strong forces of attraction between positive metal ions and negatively charged sea of delocalised electrons
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Do metallic compounds conduct electricity, why?
Yes as delocalised electrons can move throughout the metal to carry charge
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How does the strength of metallic bonds change across the periodic table, why?
Increases, as higher melting and boiling points, higher charge on metal ions with delocalised electrons per ion
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Define electronegativity
The ability of an atom to attract the pair of electrons in a covalent bond
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What affects electronegativity?
Nuclear charge, atomic radius and electron shielding
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What is the most electronegative element?
Fluorine has the largest nuclear charge for its electron shielding and a small atomic radius
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How do you get a non-polar bond
Both bonding elements have the same electronnegativities
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When do you get a polar bond?
Bonding atoms have different electronegativities
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What is the strongest type of inter-molecular force?
Hydrogen bonding
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What is the weakest type of inter-molecular force?
Van der Waals forces
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Describe Van der Waals forces of attraction
Temporary dipoles are created by the random movement of electrons, induces a dipole in a neighbouring molecule
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Are Van der Waals forces stronger in smaller or larger molecules?
Larger - more electrons
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Describe permanent dipole-dipole attraction
Some molecules with polar bonds have permanent dipoles, forces of attraction between those dipoles and those of neighbouring molecules
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What conditions are needed for hydrogen bonding to occur?
O,N or F element with a lone pair of electrons
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Why is ice less dense than liquid water?
In ice, the hydrogen bonds hold the molecules in fixed positions, this makes them slightly further apart than in liquid water
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What is a dative covalent bond? When is it formed?
Formed when an electron deficient atom accepts a lone pair of electrons from an atom with a lone pair of electrons
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What does the shape of molecules depend on?
Number of electrons in the valence shell of the central atom, number of electrons which are bonded or lone pairs
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What does the electron pair repulsion theory state?
That electron pairs will take up positions as far away from each other as possible, to minimse the repulsive forces between them
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Which experience the most repulsion?
LP-LP repulstion strongest, LP-BP middle, BP-BP repulsion weakest
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What is the shape, diagram and bond angle in a shape with 2 bonded pairs and 0 lone pairs?
Linear and 180 angle
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What is the shape, diagram and bong angle in a shape with 3 bonded pairs and 0 lone pairs?
Trigonal planar and 120 angle
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What is the shape, diagram and bond angle in a shape with 4 bonded pairs and 0 lone pairs?
Tetrahedral and 109.5 angle
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What is the shape, diagram and bond angle in a shape with 5 bonded pairs and 0 lone pairs?
Trigonal bipyramid and 90 and 120 angle
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What is the shape, diagram and bond angle in a shape with 6 bonded pairs and 0 lone pairs?
Octahedral and 90 angle
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Other cards in this set

Card 2

Front

High - takes lots of energy to break strong electrostatic forces of attraction between oppositely charged ions

Back

How high are ionically bonded substances boiling point and melting point, why?

Card 3

Front

Yes, when molten or in solution as the ions are free to move and carry charge

Back

Preview of the back of card 3

Card 4

Front

Strong covalent bonds between atoms, weak van der waals forces of attraction between molecules

Back

Preview of the back of card 4

Card 5

Front

No - they are all involved in bonding

Back

Preview of the back of card 5
View more cards

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