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GCSE Chemistry > Bonding, Structure & Properties of Matter > Flashcards

Bonding, Structure & Properties of Matter Flashcards

1
Q

What is the primary reason atoms combine with other atoms?

A

To achieve a greater level of stability by obtaining a full outer shell of electrons.

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2
Q

What are the three types of bonding studied at GCSE?

A
  • Ionic bonding
  • Covalent bonding
  • Metallic bonding
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3
Q

What occurs during ionic bonding?

A

Metals and non-metals react by transferring electrons.

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4
Q

What are negative ions called?

A

Anions.

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5
Q

What are positive ions called?

A

Cations.

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6
Q

What charge do all metals form when they lose electrons?

A

Positive charge.

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7
Q

What charge do all non-metals form when they gain electrons?

A

Negative charge.

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8
Q

What is a dot and cross diagram used for?

A

To show the arrangement of electrons in an ionic compound.

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9
Q

Why do ionic compounds have high melting and boiling points?

A

Due to strong electrostatic forces of attraction in the lattice structure.

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10
Q

What is covalent bonding?

A

Non-metal atoms share electrons to obtain a full outer shell.

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11
Q

What is the difference between covalent bonds and ionic bonds?

A

In covalent bonds, electrons are shared; in ionic bonds, electrons are transferred.

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12
Q

What is a characteristic of simple covalent molecules?

A

They do not conduct electricity as they do not contain free electrons.

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13
Q

What are some examples of simple covalent molecules?

A
  • Cl2
  • H2O
  • CO2
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14
Q

What do we call large covalent structures, such as graphite and diamond?

A

Giant covalent structures.

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15
Q

What is an advantage of dot and cross diagrams?

A

They illustrate the transfer of electrons.

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16
Q

What is a disadvantage of ball and stick models?

A

They fail to indicate the movement of electrons.

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17
Q

What is the main limitation of 2D representations of molecules?

A

They cannot give an idea of the shape of a molecule in 3D space.

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18
Q

What is the primary characteristic of metallic bonding?

A

Metal atoms share delocalized electrons, forming a ‘sea of electrons’.

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19
Q

True or False: Intermolecular forces are considered chemical bonds.

A

False.

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20
Q

What happens to the electrons in the outer shell of metal atoms?

A

Electrons in the outer shell of metal atoms are lost

This loss leads to the formation of positively charged metal ions.

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21
Q

How are individual metal atoms held together?

A

Individual metal atoms are held together by strong metallic bonds forming a lattice structure

The lattice structure is essential for the stability of metallic compounds.

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22
Q

What is a metallic bond?

A

A metallic bond is the attraction between delocalised electrons and positively charged metal ions

This bond type is characteristic of metals and metal alloys.

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23
Q

What occurs within the metal lattice?

A

Within the metal lattice, atoms lose their valence electrons and become positively charged metal ions

The loss of valence electrons is a key feature of metallic bonding.

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24
Q

What are delocalised electrons?

A

Delocalised electrons are electrons that no longer belong to any specific metal atom and can move freely

They create a ‘sea of electrons’ that contributes to many metallic properties.

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25
What does the term 'sea of electrons' refer to?
The 'sea of electrons' refers to the freely moving delocalised electrons between positive metal ions ## Footnote This concept helps explain the electrical conductivity of metals.
26
True or False: Delocalised electrons are transferred as in ionic bonding.
False ## Footnote In metallic bonding, delocalised electrons move freely rather than being transferred.
27
Fill in the blank: The arrangement of atoms in metals forms a _______.
lattice structure ## Footnote The lattice structure is fundamental in defining the physical properties of metals.
28
What are the three states of matter?
Solids, liquids, and gases
29
What occurs at the melting point?
Solid to liquid and liquid to solid transitions
30
What occurs at the boiling point?
Liquid to gas and gas to liquid transitions
31
Describe the arrangement of particles in a solid.
Regular arrangement
32
How do particles move in a liquid?
Move around each other
33
What is the closeness of particles in a gas?
Far apart
34
Changing states of matter is considered what type of change?
Physical change
35
What is melting?
When a solid changes into a liquid
36
What is boiling?
When a liquid changes into a gas
37
What is freezing?
When a liquid changes into a solid
38
What is evaporation?
When a liquid changes into a gas at temperatures below its boiling point
39
What is condensation?
When a gas changes into a liquid on cooling
40
What is sublimation?
When a solid changes directly into a gas
41
What does particle theory explain?
How matter changes state depending on energy and forces between particles
42
What is a limitation of particle theory?
It doesn’t consider differences caused by different particles or intermolecular forces
43
What is the state symbol for aqueous?
(aq)
44
Why do ionic compounds have high melting and boiling points?
They have giant structures and strong electrostatic forces of attraction between ions
45
When can ionic compounds conduct electricity?
When molten or in solution
46
Why are small molecules poor conductors of electricity?
There are no free ions or electrons to move and carry the charge
47
What are the two types of bonds in substances consisting of small molecules?
* Covalent bonds (between atoms) * Intermolecular forces (between molecules)
48
What is a polymer?
Very large molecules made by linking together smaller molecules called monomers
49
What is the simplest polymer?
Poly(ethene)
50
What is the structure of poly(chloroethene)?
Made from long carbon chains linked by covalent bonds
51
What is the simplest of all polymers?
poly(ethene) ## Footnote Poly(ethene) is also known as polyethylene.
52
What is the monomer that forms poly(1,2-dichlorethene)?
1,2-dichlorethene
53
What are giant covalent structures?
Solids with high melting points made of non-metal atoms bonded via strong covalent bonds ## Footnote These structures can also be called giant lattices.
54
List three examples of giant covalent structures.
* Diamond * Graphite * Silicon dioxide
55
What are the properties of giant covalent structures?
High melting points due to strong covalent bonds requiring a lot of energy to overcome
56
What are the components of diamond and graphite?
Made from carbon atoms
57
What is silicon dioxide made from?
Silicon and oxygen atoms
58
What is the characteristic of giant covalent structures at room temperature?
They are solids
59
What are the strong forces of attraction in metallic bonds?
Between positive metal ions and negative delocalised electrons
60
What is a key property of most metals?
High melting and boiling points
61
What does malleable mean in terms of metal properties?
Can be hammered into shape
62
What is an alloy?
A mixture of two or more metals or a metal with a non-metal
63
Give an example of an alloy.
Steel (made from iron and carbon)
64
Why are alloys usually harder than pure metals?
Alloys contain atoms of different sizes, distorting the layers
65
What happens to the layers of positive ions in metals when a force is applied?
They slide over each other
66
How do metals conduct electricity?
Delocalised electrons move through the structure and carry a charge
67
What is the metallic bond?
The strong force of attraction between positive metal ions and delocalised electrons
68
How do metals conduct heat?
Delocalised electrons transfer thermal energy through the structure
69
What is the thermal conductivity of silver?
406 W/mK
70
Fill in the blank: Metals are good conductors of _______.
heat
71
What is the thermal conductivity of copper?
385 W/mK
72
What is the thermal conductivity of gold?
314 W/mK
73
What is the thermal conductivity of brass?
109 W/mK
74
What is the thermal conductivity of aluminum?
205 W/mK
75
What is the thermal conductivity of iron?
79.5 W/mK
76
What is the thermal conductivity of steel?
50.2 W/mK
77
What is the thermal conductivity of lead?
34.7 W/mK
78
What are the three categories of particles based on their diameter?
Coarse particles, Fine particles, Nanoparticles
79
What is the diameter range for nanoparticles?
1 to 100 nanometres
80
What is a micrometre in relation to a metre?
1x10^-6 of a metre
81
What is a nanometre in relation to a metre?
1x10^-9 of a metre
82
What do the terms PM2.5 and PM10 refer to?
Fine and coarse particles respectively
83
What is the significance of the surface area to volume ratio in nanoparticles?
It is very high, leading to different properties compared to bulk materials
84
How does the surface area to volume ratio change as the size of a cube decreases?
It increases by a factor of 10 for every factor of 10 decrease in size
85
What are fullerenes?
Nanoparticles made of carbon
86
What is nanoscience?
The field of study focused on particles at the nanoscale
87
What is nanotechnology?
Research into the production and application of nanoscience
88
What are the main industrial applications of nanoparticles?
Catalysis due to high surface area to volume ratios
89
What is titanium dioxide used for in nanoparticle form?
In sunscreens to block UV light without leaving white marks
90
How does titanium dioxide behave differently in bulk form compared to nanoparticle form?
In bulk form, it is used as a white pigment in paints
91
What are some applications of fullerenes?
Medicine, drug design, electronic circuitry, coatings for artificial limbs
92
How are silver nanoparticles used in medical clothing and masks?
They provide antibacterial properties while maintaining material flexibility
93
What are the advantages of nanoparticles?
Widespread uses and applications that advance materials technology
94
What are some disadvantages of nanoparticles?
Unknown factors and potential health risks, long-term side effects
95
Fill in the blank: The use of nanoparticles in science is in its _______.
early stages
96
True or False: There have been serious short term side effects from nanoparticles.
False
97
What causes caution in the medical application of nanoparticles?
High surface area to volume ratio and difficulty in disposal by the body
98
How do you calculate the amount of gas (mol)?
Amount of gas = volume/24

GCSE Chemistry (12 decks)

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