covalent bonding 4.2 Flashcards

1
Q

what’s covalent bonding dot cross diagrams?

A

when non-metal atoms bond, they share pairs of electrons to get a full outer shell

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2
Q

what is the definition of covalent bonding?

A

covalent bonding is the electrostatic attraction between protons in two nuclei and a shared pair of electrons between them

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3
Q

what’s type of attraction is covalent bonding?

A

very strong attraction

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4
Q

what is a simple molecule?

A

a small group of atoms held together by covalent bonds

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5
Q

why do simple molecular substances of covalent bonds have low boiling points?

A

simple molecules contain very strong covent bonds but also weak intermolecular forces between the molecules

when simple molecular substances boil it’s the weak IMFs which break

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6
Q

what’s the relation between simple molecular substances and molecular mass?

A

as molecular mass increases, so does the strength of the weak IMFs
increasing the boiling point

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7
Q

do simple molecular substances conduct electricity?

A

no
as they don’t have charged particles that can move freely

molecules are neutral

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8
Q

what’s an example of a simple molecular substance?

A

C60 fullerene
composed of sixty carbon atoms
low boiling point, but not as low as others as it has a high molecular mass

soft and slippery solid as molecules can roll over each other
electrical insulator as the molecules are neutral

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9
Q

what is diamond - covalent bonding?

A

a pure carbon
arranged into a giant lattice
every carbon makes 4 covalent bonds
tetrahedral shape
strong
sublimes at a very high temperature

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10
Q

why does diamond and silicon sublime at a very high temperature?

A

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

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11
Q

what is one of the uses of diamond?

A

cutting
as it is a hard substance

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12
Q

can the giant lattice of diamond and silicon conduct electricity?

A

it cannot conduct electricity as there are no moving particles
all the atoms are neutral and the electrons are stuck inside a bond

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13
Q

what is graphite - covalent bonding?

A

pure carbon
giant lattice
layers of hexagons of carbon atoms
every carbon makes 3 covalent bonds
weak intermolecular forces between layers
delocalised electrons inside each layer

soft and slippery as layers can slide easy, used as a solid lubricant

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14
Q

why does graphite sublime at a high temperature?

A
  • covalent bonds are strong
  • lots of bonds in the giant lattice
  • lots of energy is needed to break the bonds
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15
Q

can graphite conduct electricity?

A

yes as the delocalised electrons can move freely inside the layers

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16
Q

what is silicon - covalent bonding?

A

giant covalent structure
every Si makes up 4 covalent bonds
every O makes up 2 covalent bonds
tetrahedral shape
strong