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Chemistry > Structure And Bonding > Flashcards

Structure And Bonding Flashcards

1
Q

What is ionic bonding?

A

Ionic bonding is a chemical bond that involves the electrostatic attraction between oppositely charged ions. It is between a metal and a non metal

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2
Q

What is the structure all ionic compounds form?

A

Giant Ionic lattices

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3
Q

What is a lattice?

A

An ionic structure where ions are arranged regularly with no gaps.

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4
Q

What holds together ions in a lattice?

A

Electrostatic forces of attraction

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5
Q

What state must ionic substances be in to conduct electricity?

A

Molten or dissolved

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6
Q

What are properties of ionic compounds?

A
  • Solid at room temperature
  • Conduct electricity when molten improve dissolved
  • Soluble in water
  • Very high melting points
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7
Q

Why can ionic substances conduct electricity when molten or dissolved?

A

As the charged particles are free to move around (as the lattice is broken) and so can carry and charge

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8
Q

Why do ionic substance have high melting and boiling points?

A

The strong electrostatic attractions between oppositely charged ions require a lot of energy to break apart

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9
Q

What is covalent bonding?

A

When two non metals react, both wanting to gain electrons to make a full outer shell, so they share a pair of electrons

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10
Q

How man bonds do non metals have?

A

The same number of electrons on their outer shell

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11
Q

What are properties of simple molecular compounds?

A
  • Low melting and boiling points
  • Do not conduct electricity (other then water)
  • Low density
  • Soluble
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12
Q

What are properties of giant molecular compounds?

A
  • High melting and boiling points
  • Generally do not conduct electricity
  • High density
  • Insoluble
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13
Q

Why do simple molecular have low melting and boiling points?

A

A structure when only the weak intermolecular forces between molecules are broken (not strong covalent one). So only small amounts of energy are needed to break the weak forces.

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14
Q

Why can’t simple molecular conduct electricity?

A

As there are no free charged particles (only ions or electrons) to allow a current to flow.

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15
Q

What is the structure of polyethene?

A

Between the carbon atoms there are strong covalent bonds and between the layers there are weak intermolecular forces

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16
Q

Why do polymers have high melting and boiling points?

A

As the longer the chain length, the more intermolecular forces between the monomers, meaning more energy is needed to break them apart

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17
Q

What are allotropes?

A

Allotropes are different structural forms of the same element

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18
Q

What are some properties of the allotrope diamond?

A
  • Hard
  • High letting point
  • Shiny
  • Does not conduct electricity
19
Q

What are some properties of the allotrope graphite?

A
  • soft
  • high melting point
  • black
  • does conduct electricity
20
Q

Why does diamond have a large tetrahedral structure?

A

As each carbon forms four covalent bonds with other carbon atoms

21
Q

What is the stricture of graphite?

A

Each carbon forms three covalent bonds with other carbon atoms. This forms hexagonal rings which have intermolecular forces between the layers

22
Q

Why is diamond hard?

A

Because each carbon is bonded covalently to 4 other carbon atoms meaning it is in a tetrahedral structure - difficult to break

23
Q

Why cannot diamond conduct electricity?

A

As all electrons are used within covenant bonds so there are no free electrons to carry a charge.

24
Q

Why does diamond have such a high melting point?

A

As they are giant covalent molecules (macromolecules). This means they have strong electrostatic forces that require a lot of energy to break apart.

25
Q

Why is graphite soft?

A

As it has weak intermolecular forces between layers meaning they can slide and break easily.

26
Q

What can graphite conduct electricity?

A

As each carbon atoms makes 3 bonds yet each carbon atoms has 4 electrons, so this leaves a free electron that can carry a charge.

27
Q

What does graphite have a high melting and boiling point?

A

As it is giant covalent structure (macromolecules) meaning it has strong covalent bonds that require lots of energy to break apart.

28
Q

What is Graphene’s structure?

A

Large sheet of carbon (giant covalent structure)

29
Q

What is fullerenes structure?

A

A spherical allotrope of carbon which is covalently bonded to 3 carbons.

30
Q

Why does Graphene have exceptional strength?

A

Due to strong covalent bonds

31
Q

What is Graphene an extremely light material?

A

As it is only 1 atom thick (2D)

32
Q

Why is Graphene an electrical conductor?

A

Due to electrons moving across its surface and that it can be rolled into nanotubes

33
Q

Why does fullerene have a low melting point?

A

Due to weak intermolecular forces between molecules

34
Q

Why does fullerene conduct electricity

A

Due to delocalised electrons that can carry a charge

35
Q

What are some properties of metals?

A
  • Conducts electricity
  • high melting and boiling points
  • malleable
  • ductile
  • sonorous
36
Q

What is the structure of a metal?

A

Rows of metal cations (positive ions) held together by a sea of delocalised electrons

37
Q

What does delocalised mean?

A

Not fixed in a certain position and free to move around

38
Q

What happens if there are mor delocalised electrons?

A

The stronger the metal is as the positive to negative attraction is a lot greater

39
Q

Why is metallic bonding strong?

A

As the cations and electrons are strongly attracted to each other. This means a lot of energy is needed to break this bond and cause a change in state

40
Q

Why can metals conduct electricity?

A

As the delocalised electrons are free to more. This means when a potential difference is applied the electrons flow in one direction.

41
Q

Why are metals malleable?

A

As when a force is applied, the regularly arranged electrons are free to move over one another. Yet, ions are still held together by delocalised electrons so do not fully break

42
Q

When do ionic bonds occur?

A

Between a metal and a non-metal, between a cation and an anion come together

43
Q

What happens to the ending of a non-metal when an ionic bond is formed?

A

It changes to -ide

Chemistry (12 decks)

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