C3 Structure & Bonding Flashcards
1
Q
What is an allotrope?
A
Different structure forms of the same element in the same physical state
2
Q
What are the 5 main allotropes of carbon?
A
- Diamond
- Graphite
- Fullerene (buck minister)
- Graphene (one layer of graphite)
- Carbon nano tubes
3
Q
What are the properties of Diamond?
A
- Giant covalent structure
- regular repeating lattice covalently bonded
- very strong meaning lots of energy needed to break bonds (high melting/boiling point)
-each carbon is covalently bonded to 4 other carbon atoms
-regular 3D pattern
4
Q
What are the properties of Graphite?
A
-each carbon is bonded to 3 other carbon atoms
-soft but high melting point
5
Q
What is the special property of Graphite?
A
Has one delocalised electron meaning graphite can conduct heat and electricity
6
Q
What is a single layer of Graphite called?
A
Graphene
7
Q
What are the tiny tubes and spheres that are made out of graphene called?
A
Fullerenes
8
Q
What are the tubes made out of graphene called?
A
Nanotubes
9
Q
What are the spheres made out of graphene called?
A
Buckministerfullerene
10
Q
What do we call technology that uses fullerenes (nanotubes and buckministerfullerenes) ?
A
Nanotechnology
11
Q
What are fullerenes?
A
Fullerenes are allotropes of carbon with hollow shapes like spheres or tubes
12
Q
What are Ions?
A
Atoms that lose 🥚 or gain electrons to have a full outer shell
13
Q
What process takes place in Ions?
A
The transfer of electrons
14
Q
How are elements in an Ionic compound attracted to each other?
A
Due to opposite charges, meaning they are attracted to each other by ELECTROSTATIC FORCES
15
Q
What is an intermolecular force?
A
The force between other molecules in the element
16
Q
What is an Ionic bond?
A
Electrostatic attraction between oppositely charged ions
17
Q
What does Ionic bonding occur in?
A
Metals & Non-metals
18
Q
What are properties of Ionic bonds?
A
Very strong
Needs lots of energy to break the intermolecular forces
19
Q
What is an Ion?
A
An Atom with an overall CHARGE
20
Q
Explain the process of the ionic bonding between Sodium and Chlorine?
A
Sodium transfers one electrons from its out shell to chlorine, leaving sodium with a 1+ positive charge due to it loosing an electron. Chlorine now gaining the electron forms an ion with a 1- negative charge due to it gaining an electron. Now this means that both now have full outer shells, meaning they have stable electronic structures like noble gases.
21
Q
What do Ionic compounds form?
A
Giant structures called a giant ionic lattice
22
Q
How are the Positive and Negative ions arranged in a Giant Ionic Lattice?
A
Every positive ions is surrounded by negative ions, and every negative ion is surrounded by positive ions.
23
Q
What type of structure is a Giant Ionic Lattice?
A
Giant Ionic Lattices are Three Dimensional structures (3D structures)
24
Q
What type of attraction is there between the positive and negative ions.
A
There are very strong electrostatic forces of attraction between the positive and negative ions.
25
What do Electrostatic forces of attraction do?
Electrostatic forces of attraction hold the positive and negative ions in place (also the electrostatic forces of attraction act in all directions)
26
What is another name for electrostatic forces of attraction?
Ionic bonds
27
In what direction do Ionic bonds act in?
Ionic bonds act in all directions
28
Why do Ionic compounds have very high melting and boiling points?
Ionic compounds have very high melting and boiling points because of the strong electrostatic forces of attraction requiring a large amount of heat energy to be broken.
29
Why cant Ionic compounds conduct electricity when in a solid state?
Because ions are locked in one place, meaning the ions can vibrate but not move.
30
Why can Ionic bonds conduct electricity when melted or dissolved in water?
The ions can now move and carry the electrical charge
31
What is one important thing to remember of Ionic compounds conducting electricity when melted or dissolved in water?
REMEMBER THAT IT IS THE IONS AND NOT ELECTRONS THAT ARE MOVING!
32
What do covalent bonds do with their electrons to gain a full outer shell?
Covalent bonds share electrons
33
How can covalent bonding be drawn?
- Dot & Cross Diagrams
- Or a displayed formula like Cl - Cl
- 3D Models
34
What are the positives of a displayed formula?
It is easier to draw big molecules which would have been more complicated and took more long with dot & cross diagrams.
35
What are the downsides of a displayed formula?
They don't shows anything about the 3D shape of the molecule.
36
What do 3D models do ?
3D- Models show how the atoms are actually arranged in real life, though it is hard to predict the shape.
37
Why do Small covalent molecules have low melting and boiling points?
This is because the intermolecular forces between the molecules are WEAK, meaning they DO NOT require that much energy to break.
38
What does small covalent molecule mean by having low melting and boiling points?
Means that they are usually gases at room temperature
39
What are the atoms in the molecule held together by in small covalent molecules.?
Strong covalent bonds
40
What is one important thing to remember about covalent bonds, when they are melted or boiled?
That the covalent bonds are NOT broken when a substance melts or boils
41
Why do small covalent molecules NOT conduct electricity?
This is because they do not have an overall charge
42
How does the size of a simple covalent molecule affect the melting and boiling points?
The bigger the molecule, the more intermolecular forces there is between the molecules meaning more energy is needed to break these forces, so the melting and boiling point increase.
43
What is a good thing about Dot & Cross diagrams?
We use dots to represent electrons from one atom and crosses to represent the electrons from the other atom, which clearly and easily identifies where the electrons have come from.
44
What is a downside to Dot & Cross diagrams?
They do not tell us about the shape of the molecule
45
What are the disadvantages to 2 Dimentional Stick diagrams?
- Because the covalent bond is shown as a stick we cannot tell where the electron is coming from which atom
- No accurate information on the shape of the molecule
- shows nothing about the other electrons that are not in bonds
46
What is a good thing about 3D-Stick diagrams?
Show us the shape of the molecule
47
What molecular diagram shows giant ionic lattices?
Ball and stick diagrams
48
What are the advantages of ball & stick diagrams?
we can clearly see ions in 3-dimensions
49
What is a negative about ball and stick diagrams?
- Ions are shows as widely spaced apart when in reality they are packed together
- The diagram only shows a tiny part of the GIANT CRYSTAL LATTICE - when they are actually giant structures which may give us the idea of the giant crystal lattice being small
50
What is a advantage of space filling diagrams?
Gives us a good ideas of how closely packed together the ions are.
51
What are the disadvantages of space filling diagrams?
- may be difficult to see 3-dimensional (3D) packing
- Only shows a tiny part of the GIANT CRYSTAL LATTICE which may give an idea of them being small when they are actually GIANT STRUCTURES
52
What is the formula for ammonium ion?
NHv4 ^+
53
What is the formula for hydroxide?
OH^-
54
What is the formula for nitrate?
NOv3 ^-
55
What is the formula for sulfate?
SOv4 ^2-
56
What is the formula for carbonate?
COv3 ^2-
57
What do all Giant covalent structures have?
High melting and boiling points
58
Why does small covalent molecules have low melting and boiling points?
This is due to them only having a small number of covalent bonds an have weak INTERMOLECULAR forces BETWEEN the molecules.
59
What and why are Covalent structures always at in room temperature?
A SOLID due to high melting and boiling point
60
Why does Diamond have high melting and boiling points?
This is because diamond contains a huge number of strong covalent bonds, meaning a big amount of energy is needed to break these bonds.
61
What element is diamond formed by?
Carbon
62
How many electrons does carbon have in its outer shell?
4 electrons in its outer shell
63
What does carbon do to have a full outer shell?
Carbon needs 4 electrons, to have a full outer shell. Meaning each carbon atom forms covalent bonds to FOUR other carbon atoms, sharing their electrons.
64
Why is diamond a very hard substance?
Due to lots of carbon atoms joined by covalent bonds, this makes diamond a very HARD substance.
65
Why cant diamond conduct electricity?
This is due to all the outer shell electrons being in covalent bonds, meaning that the diamond has no free electrons to carry an electrical charge.
66
What does Silicon dioxide contain?
This contains silicon and oxygen COVALENTLY bonded together.
67
What is another name for silicon dioxide?
Silica
68
Why does Silicon dioxide have a very high melting a boiling point?
This is due to the huge number of strong covalent bonds, and to melt or boil these bonds, the bonds must be broken which takes a great deal of energy.
69
How much of a melting and boiling does Silica have?
Very high melting and boiling point
70
What is Graphite a form of?
Carbon
71
What type of molecule is Graphite?
A Giant Covalent Molecule
72
Why does Graphite have a high melting and boiling point?
This is due to the large number of strong covalent bonds. Which takes a GREAT DEAL of ENERGY to break
73
What is Graphite formed by?
Carbon
74
What do each of the Carbon atoms do in Graphite?
Each carbon atom forms Covalent bonds to 3 (THREE) other carbon atoms.
75
What shape does graphite form and what is it made up of?
Hexagonal rings, which are rings of 6 (SIX) carbon atoms.
76
What are the hexagonal rings in Graphite arranged in?
Arranged in layers
77
Why is Graphite SOFT and SLIPPERY?
This is because there are NO COVALENT BONDS between the layers, meaning the can SLIDE OVER each other.
78
What is a good use of Graphite due to it being soft and slippery?
Graphite is often used as a LUBRICANT in machines, reducing FRICTION between the moving parts.
79
What is Graphite a good conductor of?
Good conductor of both HEAT ENERGY and ELECTRICITY.
80
Why is Graphite a good conductor of both electricity and heat energy?
This is because Graphite is formed from carbon atoms, which have 4 (FOUR) outer shell electrons.
In Graphite each CARBON atom forms COVALENT BONDS with 3 (THREE) OTHER CARBON ATOMS.
However, each carbon atom has one electron in its OUTER SHELL, that is NOT in a COVALENT BOND.
These ELECTRONS are released from the CARBON atoms, meaning now there are DELOCALISED ELECTRONS that can freely move THROUGH the structure carrying a CHARGE.
81
What are Fullerenes are Graphenes based on?
Carbon atoms
82
What is Graphene and how thick is it?
Graphene is a SINGLE LAYER of GRAPHITE, meaning it is only 1(ONE) cell thick.
83
What are the 2 properties of graphene?
- Good conductor of ELECTRICITY and HEAT
- EXTREMELY STRONG
84
Why is graphene a good conductor of electricity?
This is because graphene has delocalised electrons, which can MOVE THROUGH the graphene molecule carrying electrical charge.
85
What are the uses of graphene?
Useful in ELECTRONICS due to it being graphene being able to conduct ELECTRICITY, and these PROPERTIES will make graphene useful for producing NEW MATERIALS
86
Why is Graphene extremely strong?
Due to the very HIGH melting and boiling point, this is because a GREAT DEAL of ENERGY is needed to break the large number of STRONG COVALENT BONDS.
87
What are fullerene molecules based on?
Carbon atoms
88
What shape do fullerene molecules have?
Have HOLLOW shapes, usually in HEXAGONAL RINGS of CARBON atoms. Fullerenes can also have rings with 5 (FIVE) or 7 (SEVEN) CARBON atoms.
89
What is the first fullerene to be discovered?
Buckminsterfullerene
90
What does the Buckminsterfullerene contain and how is it structured?
Contains 60 (SIXTY) CARBON atoms arranged in a hollow sphere, these form rings with 6 (SIX) other CARBON atoms or with 5 (FIVE) CARBON atoms.
91
What is the molecular formula of the buckminsterfullerene?
C60
92
What are 3 (three) uses of a buckminsterfullerene?
- They can be used to DELIVER drugs such as PHARMACEUTICALS INTO the BODY
- Can also be used as LUBRICANTS in machines where THEY REDUCE FRICTION between moving parts
- They can be used as catalysts to speed up chemical reactions.
93
What is the structure of Carbon nanotubes?
Shaped into a LONG CYLINDER with a relatively small diameter, the rings are formed from 6 (SIX) CARBON atoms.
94
What is the ratio of Carbon nanotubes?
Have a VERY HIGH Length to diameter ratio
95
What are the 2 properties of Carbon nanotubes?
- They have a HIGH TENSILE STRENGTH
- They are also good conductors of ELECTRICITY and HEAT
96
Why or how are carbon nanotubes good conductors of electricity and heat?
Carbon nanotubes have delocalised electrons, meaning the electrons can move freely through the structure carrying a charge.
97
What does having a high tensile strength mean in terms of carbon nanotubes?
We are able to apply a great deal of STRETCHING FORCE, to a CARBON NANOTUBE before it BREAKS.
98
What is 1 (ONE) use of carbon nanotubes?
Carbon Nanotubes are used to REINFORCE MATERIALS, in high end TENNIS RACKETS.
99
What do metals form and how are they structured?
GIANT STRUCTURES, metals consist of a GIANT STRUCTURE of atoms arranged in REGULAR LAYERS.
100
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101
What is special about electrons in Metallic bonding?
The electrons in the outer shell are delocalised, meaning the outer electrons are FREE TO MOVE THROUGH the whole structure.
102
How is a positive metal ion formed in metallic bonding?
When the metal has LOST ITS OUTER ELECTRON we now refer to them POSITIVE METAL IONS (though this is NOT ionic bonding)
103
What is the electrostatic force of attraction?
An attraction between a POSITIVE object and a NEGATIVE object.
104
What is the force that is between delocalised electrons and the metal ions?
Between the SEA of delocalised negative electrons and the positive metal ions, we have a STRONG ELECTROSTATIC ATTRACTION.
105
What is the force between positive and negative objects called in metallic bonding and what does this mean?
Electrostatic attraction, meaning metallic bonds are strong.
106
Why do metals have high melting and boiling points?
This is due to the STRONG METALLIC BONDS we need to BREAK, which requires a GREAT DEAL of ENERGY.
107
Why are metals good conductors of heat and electricity?
This is because the DELOCALISED ELECTRONS can MOVE THROUGH the structure CARRYING AND ELECTRICAL CHARGE.
The moving delocalised electrons are also able to carry thermal energy, which allows metals to conduct heat.
108
What is another property of metals?
That they are MALLEABLE - they can be bend and shaped without BREAKING and DUCTILE - they are be drawn/pulled into wires making them suitable for electric cables
109
How are metals malleable?
This is because the layers of atoms can SLIDE OVER each other.
110
What is an Alloy?
An alloy is a MIXTURE OF METALS
111
What makes an alloy stronger / harder than pure metals?
The DIFFERENT SIZED ATOMS in the alloy DISTORTS THE LAYERS, making it more difficult for the LAYERS to SLIDE OVER each other, making alloys HARDER than pure metals.
112
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