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Chemistry > Structure 2 > Flashcards

Structure 2 Flashcards

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1
Q

What is the only alloy that is not made up of only metals?

A

Steel (metal + carbon)

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2
Q

100% metallic properties

A

Good conductors of heat and electricity in the solid and liquid state

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3
Q

100% covalent properties

A

Poor conductors of heat and electricity

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4
Q

> 90% ionic properties

A

Good electrolytes (conduct when in molten or aqueous solution and decompose in the process)

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5
Q

50% ionic - 50% covalent properties

A

Properties vary depending on the compound

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6
Q

What two things increase the lattice enthalpy?

A

Smaller ion, greater charge

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7
Q

What is the lattice enthalpy?

A

How strong the ionic bonds are in a particular ionic lattice

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8
Q

Is solubility an exothermic or endothermic process?

A

Endothermic

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9
Q

Do ionic solids conduct electricity in the solid state?

A

No

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10
Q

What are the electrons in the molten state?

A

Electrolytes

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11
Q

How is the charge carried in the molten state?

A

Through mobile ions

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12
Q

As the number of shared pairs of electrons increases, what happens to the bond length and bond strength?

A

Bond length decreases and bond strength increases

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13
Q

Electronegativity values increase …

A

Across a period and up a group

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14
Q

If two atoms of the same element are covalently bonded, is it polar or non-polar?

A

Non-polar

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15
Q

If the covalent bond is between two different elements, the bonding pair of electrons will be more attracted to the (1) causing a (2)

A
  1. More electronegative element
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16
Q

What does molecular polarity depend on?

A

The electronegativities of the bonded atoms and the shape of the molecule.

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17
Q

When are molecules polar?

A

When the dipoles do not cancel each other out.

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18
Q

When are molecules non-polar? (2)

A

When the dipoles cancel each other out.

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19
Q

How is diamond bonded?

A

Tetrahedrally to 4 other atoms.

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20
Q

Why is diamond so hard?

A

There is no plane of weakness.

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21
Q

How is graphite bonded?

A

In a trigonal planar arrangement to 3 other atoms.

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22
Q

How are the layers held together in graphite, and what do they have?

A

By weak bonds that have delocalised electrons.

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23
Q

Why is graphite a good lubricant?

A

Because the layers can slide over each other.

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24
Q

Why is graphite a good electrical conductor?

A

Because the delocalised electrons can move through the layers.

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25
Q

Which covalent network structure is similar to diamond in regards to its structure?

A

Silicon dioxide

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26
Q

How is silicon dioxide bonded?

A

Tetrahedrally by 4 oxygen atoms

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27
Q

What do the oxygen atoms act as in silicon dioxide?

A

Bridges to the other silicon atoms.

28
Q

What are 4 properties of silicon dioxide?

A

Hard, high melting point, doesn’t conduct electricity, insoluble in water and organic solvents.

29
Q

Silicon dioxide and silicon’s properties also apply to … (2)

A

Glass and sand

30
Q

What are the three forces of attractions?

A

London dispersion forces, dipole-dipole attractions, and hydrogen bonding

31
Q

Where do you find London dispersion forces?

A

In all particles - and are the only forces of attraction between non-polar molecules.

32
Q

When do London dispersion forces increase?

A

With increasing mass

33
Q

Non polar molecules have what force(s) of attraction?

A

London dispersion forces only

34
Q

Dipole-dipole attractions exist in which type of molecules? (2)

A

Polar molecules and molecules that have H-O, H-N or H-F bonds.

35
Q

Where does hydrogen bonding exist?

A

In polar molecules that have H-O, H-N or H-F bonds.

36
Q

What is the formula for retardation factor?

A

Distance travelled by component/Distance travelled by solvent from original spot

37
Q

What two things to you need to calculate the retardation factor?

A

Height of solvent front and height of spot

38
Q

Removing valence electrons from metals is endothermic or exothermic?

A

Endothermic

39
Q

What is metallic bonding described as? (word for word)

A

A close-packed lattice of metal cations in a sea of delocalised electrons.

40
Q

What are delocalised electrons?

A

Electrons that have become detached from the atoms

41
Q

Why are metals good conductors of electricity?

A

As the delocalised electrons can move freely.

42
Q

What happens when a metal is applied to a circuit?

A

The delocalised electrons move towards the positive pole, causing a current to flow.

43
Q

In group 1, what happens to the melting points of metals as you go down the group (they get larger atoms)?

A

The melting point decreases.

44
Q

How do you find where a material should be on the van Arkel-Ketelaar diagram?

A

Use the table of electronegativities, find the average and difference of the two elements, then plot x and y.

45
Q

Pure metals with delocalised bonding are found where on the van Arkel-Ketelaar diagram?

A

To the left

46
Q

On the van Arkel-Ketelaar diagram, the right side of the triangle further up indicates …?

A

A higher difference in electronegativity.

47
Q

When does a solid melt?

A

When the attractive forces between the particles are overcome.

48
Q

What influences a melting point?

A

The way in which the particles pack in the solid state.

49
Q

Ionic substances, simple covalent compounds, network covalent compounds

A

Simple covalent compounds, ionic substances, network covalent compounds.

50
Q

When do ionic compounds conduct electricity?

A

When they are molten or in aqueous solution.

51
Q

If a substance has delocalised electrons (metals, allotropes of non-metals), is it a good conductor?

A

Yes

52
Q

What is elasticity?

A

The ability of a material to resist a distorting influence and return to its original size and shape when the distorting influence is removed.

53
Q

When will an object be permanently deformed?

A

When the applied force is greater than the modulus of elasticity.

54
Q

What happens with polymers in regards to elasticity?

A

They are stretched

55
Q

Which type of solids tend to be brittle?

A

Covalent and ionic

56
Q

Do alloys have low or high melting points compared to pure metals?

A

Low

57
Q

Are alloys more or less malleable than the pure metals?

A

Less

58
Q

Are alloys brittle or malleable?

A

Brittle

59
Q

How do you change the properties of an alloy?

A

Change its composition

60
Q

What is a thermoplastic polymer?

A

A recyclable one

61
Q

What is a thermosetting polymer?

A

Not recyclable.

62
Q

Three electron domains (two bonding and one non-bonding pairs of electrons)

A

V-shaped or bent

63
Q

4 electron domains (4 bonding pairs) (what shape and the degrees)

A

Tetrahedral

64
Q

4 electron domains (3 bonding and 1 non bonding pair of electrons) (what shape and degrees)

A

Trigonal pyramidal

65
Q

4 electron domains (2 bonding and 2 non-bonding pair of electrons) (what shape and degrees)

A

V-shaped or bent

66
Q

3 electron domains (what shape and degrees)

A

Trigonal planar

67
Q

2 electron domains (what shape and degrees)

A

Linear

Chemistry (5 decks)

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