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Chemistry > 7 - Types of Substance > Flashcards

7 - Types of Substance Flashcards

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1
Q

What are the properties of a compound influenced by?

A
  • Atoms
  • Type of bonding
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2
Q

What is simple molecular also known as?

A

Simple covalent

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3
Q

What type of elements are simple molecular compounds made of?

A

Non metal

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4
Q

What are the physical properties of simple molecular substances?

A
  • LOW melting & boiling points
  • Insoluble in water (some are soluble)
  • CAN NOT conduct electricity
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5
Q

Why do simple molecular compounds not conduct electricity?

A

As the small molecules do not have an overall electric charge

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6
Q

Why are some simple molecular compounds soluble in water?

A

As they can form intermolecular forces with water which are stronger than those between water molecules or their own molecules already

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7
Q

What state are simple molecular substances often at room temperature?

A

Liquids or gases

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8
Q

Why does the larger simple molecular substances have higher mp &bp?

A

The intermolecular forces increase with molecular size, hence large molecules have higher melting and boiling points

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9
Q

What are the physical properties of ionic compounds?

A
  • High mp & bp
  • CAN conduct electricity as a liquid NOT SOLID
  • Soluble
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10
Q

What type of elements are ionic compounds made of?

A

metal & non metal

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11
Q

Why do ionic compounds have a high mp/bp?

A

As a lot of energy is required to break the many strong bonds

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12
Q

Why do ionic compounds conduct electricity ONLY when melted/dissolved?

A

The ions are free to move and carry current

They do not conduct electricity
as solids, because the ions are fixed and are not able to move

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13
Q

What type of structures are ionic compounds usually in?

A

Giant ionic lattices

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14
Q

What are the physical properties of Giant covalent structures?

A
  • Very high mp
  • SOME can conduct electricity
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15
Q

Why can’t most giant covalent structures conduct electricity?

A

As they do not have free electrons

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16
Q

What type of elements are Giant covalent structures made of?

A

Non metal

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17
Q

Why do Giant covalent structures have a high mp/bp?

A
  • Strong covalent bonds
  • These bonds must be overcome to melt or boil these substances
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18
Q

What are the different forms of carbon?

A
  • Diamond
  • Graphite
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19
Q

What are diamond & graphite examples of?

A

Giant covalent substances

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20
Q

Describe the structure of diamonds?

A
  • Each carbon is joined to 4 other carbons
  • Tetrahedron
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21
Q

What is an allotrope?

A

Different atomic or molecular arrangements of the same element in the same physical state

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22
Q

Why does diamond and graphite have completely different physical properties even though they are made of the same material?

A

Bc they have different bonding arrangements

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23
Q

Describe the physical properties of diamonds?

Study These Flashcards
A
  • Hard
  • Very high mp
  • Does NOT conduct electricity
24
Q

What are the uses of diamonds?

Study These Flashcards
A
  • Jewellery
  • Cutting tools
25
Describe the **structure** of *Graphite*?
Each carbon is bonded to 3 other carbons ---> Forms layers of hexagonal rings ---> No covalent bonds between the layers
26
Why can the layers in **Graphite** slide over each other?
As no covalent bonds are between the layers (only weak intermolecular forces)
27
Describe the **physical properties** of *Graphite*?
* Soft * Slippery * CAN conduct electricity
28
Why can **Graphite** conduct electricity?
As ONE electron from each carbon is delocalised & these can move in between the layers
29
What are the *uses* of **graphite**?
* Pencils * Industrial lubricants * Inert electrodes (for electrolysis)
30
What are the physical properties of *metals*?
* High mp & bp * CAN conduct heat & electricity * Insoluble in water (but can react w/ water) * Malleable * High density
31
Why can **metals** conduct electricity?
Due to the delocalised electrons
32
Why do **metals** have a **high mp/bp**?
Metallic bonds are very strong ---> Result of the attraction between positive metal ions & the negatively charged delocalised electrons
33
Why are **metals malleable**?
Layers of atoms in metals can slide over each other ---> Can be hammered and bent into shape
34
Compare the *difference of physical properties* between **metals & non-metals**
35
What are **fullerenes**?
A group of carbon allotropes which consist of molecules that form hollow tubes or spheres
36
What was the *first* **fullerene** to be discovered?
Buckminsterfullerene
37
Describe the **structure** of *buckminsterfullerene*?
60 carbon atoms are joined together forming 20 hexagons and 12 pentagons
37
Describe the **structure** of *graphene*?
* Single layer of graphite * ONE atom thick
37
What are some **physical properties** of **fullerenes**?
* High surface area * Good lubricants
38
What are the physical properties of **Graphene**?
* Extremely strong but also amazingly light * Conducts heat and electricity * Transparent * Flexible
39
Why can **Graphene** conduct electricity?
Has free electrons which can move along its surface allowing it to conduct electricity
40
Why is **graphene very strong**?
Due to its unbroken pattern and the strong covalent bonds between the carbon atoms
41
Why is **graphene transparent**?
Absorbs around 2% of the visible light that hits it ---> Means you can see through it without any glare
42
What are **polymers**?
Very large molecules which are built up by linking together 50 or more monomers
43
What *type* of **bonds** are **polymers** connected to each other by?
Covalent bonds
44
How is **poly(ethene)** formed?
From the addition of many ethene monomers together
45
What are the **physical properties** of **polymers**?
* Strong intermolecular forces * Solid at room temp
46
What are **homopolymers**?
Contain just one type of monomer unit
47
What are **copolymers**?
Contain two or more different types of monomer units
48
What are the **advantages** of **dot & cross diagrams**?
* Useful for illustrating the transfer of electrons * Indicates from which atom the bonding electrons come from
49
What are the **disadvantages** of **dot & cross diagrams**?
* Fails to illustrate the 3D arrangements of the atoms and electron shells * Doesn’t indicate the relative sizes of the atoms
50
What are the **advantages** of the **ball & stick model**?
* Useful for illustrating the arrangement of atoms in 3D space * Useful for visualizing the shape of a molecule
51
What are the **disadvantages** of the **ball & stick model**?
* Doesn't indicate the movement of electrons * Atoms are placed far apart from each other = In reality is not the case as the gaps between atoms are much smaller
52
What are the **advantages** of **2D representations of molecules**?
* Displayed formulae are 2D representations & are simpler versions of the ball and stick model * Indicates what atoms are in a molecule and how they are connected
53
What are the **disadvantages** of **2D representations of molecules**?
* Doesn't illustrate the relative sizes of the atoms and bonds * Doesn't give an idea of the shape of a molecule and what it looks like in 3D space
54
What are the **advantages** of **3D representations of ionic solids**?
* 3D drawings and models depict the arrangement in space of the ions * Shows the repeating pattern in giant lattice structures
55
What are the **disadvantages** of **3D representations of ionic solids**?
* Only illustrates the outermost layer of the compound * Difficult and time-consuming to draw

Chemistry (29 decks)

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