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A-LEVEL CHEMISTRY > COVALENT BONDING > Flashcards

COVALENT BONDING Flashcards

1
Q

What is dative bonding also called? (1)

A

coordinate bonding

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2
Q

why is diamond a good thermal conductor? (1)

A

vibrations travel easily through the stiff lattice

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3
Q

what is dative covalent bonding? (1)

A

where both electrons come from one atom

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4
Q

how are dative bonds shown? (1)

A

by arrows

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5
Q

what are the properties of substances with molecular structures? (3)

A

-low melting points
-poor conductors of electricity
-don’t dissolve

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6
Q

why cant diamond be cut? (1)

A

its structure makes it refract light a lot which is why is sparkles

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7
Q

how are atoms held together by covalent bonds? (1)

A

by the electrostatic forces of attraction between the nuclei and the shared electrons

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8
Q

why won’t diamond dissolve in solvent? (1)

A

the covalent bonds are too strong to break

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9
Q

why won’t diamond conduct electricity? (1)

A

all the outer electrons are held in localised bonds

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10
Q

what happens in dative covalent bonding? (2)

A

-the atom accepts the electron pair is an atom that does not fill the outer main level of electrons (electron deficient)
-the atom that is donating the electrons has a pir of electrons that is not being used in a bond (lone pair)

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11
Q

why does diamond have a extremely hard structure? (1)

A

because of its rigid strong covalent structure (can be used in drills and saws)

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12
Q

what is the structure of diamond? (2)

A

-each carbon atom is covalently bonded to 4 other carbon atoms
-the atoms are arranged in a tetrahedral shape.

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13
Q

what are the properties of graphite? (5)

A

-layers
-carries a charge
-low density
-high melting point
-insoluble in any solvent

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14
Q

why does diamond have a high melting point? (1)

A

because of its strong covalent bonds and the energy that is needed to break them (sublimes over 3900K)

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15
Q

what are the properties of diamond? (6)

A

-high melting point
-extremely hard
-good thermal conductor
-can’t conduct electricity
-won’t dissolve in any solvent
-can’t be cut

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16
Q

why does graphite have a low density? (1)

A

because the layers are quite far apart compared to the length of covalent bonds hence it has a low density (used for light weight sports equipment)

17
Q

why is graphite insoluble? (1)

A

the covalent bonds in the sheets are to strong to break.

18
Q

why does graphite carry a charge? (1)

A

the delocalised electrons in graphite aren’t attached to any particular carbon and are free to move along the sheets carrying a charge (electrical conductor)

19
Q

why does graphite have a high melting point? (1)

A

because of the strong covalent bonds in the hexagon sheets (sublimes over 3900K)

20
Q

what does sublime mean? (1)

A

means to change straight from a solid to gas

21
Q

what properties does graphite have because of its layers? (1)

A

the weak bonds between the layers in graphite are easily broken, so the sheets can slide over each other - feels slippery and can be used as a dry lubricant

22
Q

how many pairs of electrons are shared in a triple covalent bond? (1)

A

3 pairs of electrons

23
Q

what structures do covalent bonds form? (1)

A

giant covalent structures (sometimes called macromolar structures)

24
Q

why do carbon atoms form a giant covalent structure? (1)

A

because they can form 4 strong covalent bonds

25
Q

what are the types of giant covalent structures? (2)

A

-graphite
-diamond

26
Q

what is covalent bonding? (1)

A

molecule formed when two or more atoms bond together (by strong covalent bonds) (atoms are non-metal)

27
Q

how many pairs of electrons are shared in a single covalent bond? (1)

A

one pair of electrons

28
Q

how many pairs of electrons are shared in a double covalent bond? (1)

A

two pairs of electrons

A-LEVEL CHEMISTRY (42 decks)

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