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Structure 2 Flashcards

(67 cards)

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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
  2. Polar bond
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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
Which covalent network structure is similar to diamond in regards to its structure?
Silicon dioxide
26
How is silicon dioxide bonded?
Tetrahedrally by 4 oxygen atoms
27
What do the oxygen atoms act as in silicon dioxide?
Bridges to the other silicon atoms.
28
What are 4 properties of silicon dioxide?
Hard, high melting point, doesn't conduct electricity, insoluble in water and organic solvents.
29
Silicon dioxide and silicon's properties also apply to ... (2)
Glass and sand
30
What are the three forces of attractions?
London dispersion forces, dipole-dipole attractions, and hydrogen bonding
31
Where do you find London dispersion forces?
In all particles - and are the only forces of attraction between non-polar molecules.
32
When do London dispersion forces increase?
With increasing mass
33
Non polar molecules have what force(s) of attraction?
London dispersion forces only
34
Dipole-dipole attractions exist in which type of molecules? (2)
Polar molecules and molecules that have H-O, H-N or H-F bonds.
35
Where does hydrogen bonding exist?
In polar molecules that have H-O, H-N or H-F bonds.
36
What is the formula for retardation factor?
Distance travelled by component/Distance travelled by solvent from original spot
37
What two things to you need to calculate the retardation factor?
Height of solvent front and height of spot
38
Removing valence electrons from metals is endothermic or exothermic?
Endothermic
39
What is metallic bonding described as? (word for word)
A close-packed lattice of metal cations in a sea of delocalised electrons.
40
What are delocalised electrons?
Electrons that have become detached from the atoms
41
Why are metals good conductors of electricity?
As the delocalised electrons can move freely.
42
What happens when a metal is applied to a circuit?
The delocalised electrons move towards the positive pole, causing a current to flow.
43
In group 1, what happens to the melting points of metals as you go down the group (they get larger atoms)?
The melting point decreases.
44
How do you find where a material should be on the van Arkel-Ketelaar diagram?
Use the table of electronegativities, find the average and difference of the two elements, then plot x and y.
45
Pure metals with delocalised bonding are found where on the van Arkel-Ketelaar diagram?
To the left
46
On the van Arkel-Ketelaar diagram, the right side of the triangle further up indicates ...?
A higher difference in electronegativity.
47
When does a solid melt?
When the attractive forces between the particles are overcome.
48
What influences a melting point?
The way in which the particles pack in the solid state.
49
Ionic substances, simple covalent compounds, network covalent compounds
Simple covalent compounds, ionic substances, network covalent compounds.
50
When do ionic compounds conduct electricity?
When they are molten or in aqueous solution.
51
If a substance has delocalised electrons (metals, allotropes of non-metals), is it a good conductor?
Yes
52
What is elasticity?
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
When will an object be permanently deformed?
When the applied force is greater than the modulus of elasticity.
54
What happens with polymers in regards to elasticity?
They are stretched
55
Which type of solids tend to be brittle?
Covalent and ionic
56
Do alloys have low or high melting points compared to pure metals?
Low
57
Are alloys more or less malleable than the pure metals?
Less
58
Are alloys brittle or malleable?
Brittle
59
How do you change the properties of an alloy?
Change its composition
60
What is a thermoplastic polymer?
A recyclable one
61
What is a thermosetting polymer?
Not recyclable.
62
Three electron domains (two bonding and one non-bonding pairs of electrons)
V-shaped or bent
63
4 electron domains (4 bonding pairs) (what shape and the degrees)
Tetrahedral
64
4 electron domains (3 bonding and 1 non bonding pair of electrons) (what shape and degrees)
Trigonal pyramidal
65
4 electron domains (2 bonding and 2 non-bonding pair of electrons) (what shape and degrees)
V-shaped or bent
66
3 electron domains (what shape and degrees)
Trigonal planar
67
2 electron domains (what shape and degrees)
Linear

Chemistry (6 decks)

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