4.1 Covalent bonding Flashcards

1
Q

what is the definition of covalent bonding

A

the electrostatic attraction between a bonded positive nuclei and a shared pair of electrons.

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2
Q

how would you describe covalent bonding

A

Very strong

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3
Q

what is a small group of atoms held together by covalent bonds called

A

Simple Molecule

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4
Q

what kind of boiling points do Simple molecular substances have

A

Low boiling points

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5
Q

Why do molecular substances have low boiling points

A

because they have weak intermolecular forces between molecules, which are easy to break.

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6
Q

Can Simple molecular substances conduct electricity

A

No

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7
Q

Why can’t simple molecular substance conduct electricity

A

Because the substance are neutral and can not carry charge.
not free to move

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8
Q

what happens as the molecular mass increases

A

the strength of the weak IMFs this results in the boiling point increasing

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9
Q

what is c60 Fullerene

A

c60 Fullerene is a unique molecule composed of sixty carbon atoms in a ball

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10
Q

Does c60 have a high Melting/boiling point and state a reason why

A

yes- because it has a larger molecular mass meaning stronger intermolecular forces which require more energy to break.

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11
Q

what is Diamond

A

Diamond is a form of pure carbon arranged into a giant lattice

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12
Q

Describe the structure of diamond

A

-Every c makes 4 covalent bonds
-Tetrahedral shape
-Strong, grid-like arrangement

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13
Q

does diamond sublime at a high temp if so why.

A

covalent bonds are very strong
it has Lots of bonds in the giant lattice
lots of energy is required to break all the bonds

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14
Q

what is diamond used for

A

cutting
because it is one of the hardest substances

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15
Q

can diamond conduct electricity if yes/no state why.

A

No it can’t beaus it doesn’t have any freely moving particles and can not carry charge.( all its atoms are neutral)electrons are stuck inside an atom.;

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16
Q

what is a graphite

A

a pure carbon arranged in a different giant lattice

17
Q

describe the structure of graphite

A

-Layers of hexagons of c atoms
-every c makes 3 covalent bonds
-weak intermolecular forces between layers
-delocalised electrons inside each layer

18
Q

does graphite sublime at a high temperature

A

yes because it has lots of strong covalent bonds in the giant lattice
which require a lot of energy to break

19
Q

what is the texture of diamond and why

A

soft and slippery
layers that can slide easily over each other
used as a solid lubricant

20
Q

what is graphite used for

A

A solid lubricant

21
Q

can graphite conduct electricity and why

A

yes because it has delocalised electrons which are free to move and carry charge

22
Q

what structure does silicon dioxide have

A

giant covalent structure

23
Q

describe the structure of silicon Dioxide

A

every Silicon makes 4 covalent bonds
every oxygen makes two covalent bonds
Tetrahedral shape ( like diamond )
strong grid-like arrangement

24
Q

what is silicon dioxide similar to

A

diamond

25
Q

ionic bonding is between which two elements

A

metal + non-metal

26
Q

what is the structure for ionic bonding

A

Giant lattice

27
Q

Covalent bonding is between which elements

A

only non-metal

28
Q

what is the structure of a covalent bonds

A

Simple molecules

29
Q

metallic boning is between which elements

A

only metals

30
Q

what is the structure of a Metallic bond

A

Giant lattice

31
Q

what are properties of Ionic bonds

A

Brittle
usually soluble in water
High MP/BP
insulator when a solid
Conductor when a liquid
conductor when an aqueous

32
Q

what are properties of Covalent bonds

A

Low MP/BP
Insulator
usually insoluble in water
Dull

32
Q

what are properties of Metallic bonds

A

High MP/BP
Conductor
Malleable
Shiny