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GCSE Revision > Chemistry C3 > Flashcards

Chemistry C3 Flashcards

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1
Q

What are the three states of matter?

A

Solid, liquid, gas

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2
Q

What symbols represent the three states of matter?

A

s (solid), l (liquid), g (gas)

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3
Q

How can data be used regarding the state of a substance?

A

To determine the state at a given temperature

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4
Q

What model describes the changes in energy, movement, and attraction between particles as temperature changes?

A

Particle model

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5
Q

What processes can be described in terms of states of matter?

A

Melting, freezing, boiling, and condensing

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6
Q

What happens to particles at the melting point or boiling point?

A

Energy and temperature change

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7
Q

Why do substances have different melting and boiling points?

A

Due to differences in particle arrangement and attraction

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8
Q

How can the particle model be used to represent states of matter?

A

By drawing arrangements of particles

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9
Q

What factors affect the rate of evaporation?

A

Temperature, surface area, and air movement

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10
Q

What should be evaluated when discussing models?

A

The limitations of the model

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11
Q

What diagrams can be drawn for compounds formed between Group 1 and Group 7 elements?

A

Dot and cross diagrams

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12
Q

What can be drawn for unfamiliar ionic compounds?

A

Dot and cross diagrams

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13
Q

How does a Group 1 metal atom become a positive ion?

A

By losing an electron

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14
Q

What allows ionic bonding to occur in Group 1 and Group 7 reactions?

A

Electron transfer

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15
Q

How can the charge of a monatomic ion be suggested?

A

Based on its position in the periodic table

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16
Q

How does a Group 7 non-metal atom become a negative ion?

A

By gaining an electron

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17
Q

Fill in the blank: The three states of matter are solid, liquid, and _______.

A

gas

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18
Q

True or False: The particle model shows that particles in a solid are closely packed and vibrate in place.

A

True

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19
Q

What happens to opposite charges?

A

Opposite charges attract

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20
Q

How does the position of an element on the periodic table relate to its most stable monatomic ion?

A

It determines the charge on its most stable monatomic ion

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21
Q

How can you suggest the charge on unfamiliar ions?

A

Using the position of the element in the periodic table

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22
Q

What are the charges of ions for Group 1 elements?

A

+1

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23
Q

What are the charges of ions for Group 2 elements?

A

+2

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24
Q

What are the charges of ions for Group 6 elements?

A

-2

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25
What are the charges of ions for Group 7 elements?
-1
26
How do unfamiliar elements become ions?
In terms of electronic structure
27
What is the ratio of metal and non-metal ions in compounds?
Determined by the charges of the ions
28
What is an ionic lattice?
A structured arrangement of ions in a compound
29
How can you interpret the formula of familiar ionic compounds?
To determine the number and type of each ion present
30
What can you generate when the charges of the ions are given?
Formula of a wide range of ionic compounds
31
What is a characteristic of ionic compounds regarding melting points?
They have high melting points
32
Why do ionic compounds have a high melting point?
Due to strong electrostatic forces between ions
33
Can ionic compounds conduct electricity when solid?
No
34
When can ionic compounds conduct electricity?
When molten or dissolved in water
35
How does an ionic compound conduct electricity?
In terms of movement of ions
36
What justifies that a compound has ionic bonding?
Properties of the compound
37
What is a covalent bond?
A bond formed by the sharing of electrons
38
How does a covalent bond form in terms of electronic structure?
By the sharing of electron pairs between atoms
39
What types of diagrams can be drawn for small molecules?
Dot and cross diagrams, ball and stick diagrams
40
What familiar examples of small molecules contain covalent bonds?
H2, Cl2, O2, N2, HCl, H2O, NH3, CH4
41
What is a double bond in a diatomic molecule?
A bond formed by two pairs of shared electrons
42
How could the properties of a double bond differ from a single covalent bond?
In terms of bond strength and reactivity
43
What is a characteristic of small molecules regarding their melting and boiling points?
Small molecules have low melting and boiling points.
44
How does the size of molecules affect melting and boiling points?
Larger molecules generally have higher melting and boiling points.
45
What can be predicted about the physical properties of unfamiliar covalently bonded substances?
The physical properties can be predicted based on their structure and bonding.
46
Do small molecules conduct electricity?
No, small molecules do not conduct electricity.
47
Why do small molecules and polymers not conduct electricity?
They lack free-moving charged particles.
48
What can be compared and contrasted regarding substances?
The properties of substances with different bonding can be compared and contrasted.
49
Define an intermolecular force.
An intermolecular force is a force that exists between molecules.
50
Which substances would have weak intermolecular forces?
Small molecules typically have weak intermolecular forces.
51
What is a justification for using a model to explain the physical properties of a small molecule?
Models help visualize and predict properties, though they have limitations.
52
List the main physical properties of diamond and graphite.
* High melting point * Hardness * Electrical conductivity (graphite only)
53
How can the structure of diamond and graphite be recognized?
Through written descriptions or diagrams.
54
What can be predicted and explained using a molecular model of an unfamiliar giant covalent structure?
Its physical properties can be predicted and explained.
55
What is a characteristic of giant covalent structures regarding their melting points?
Giant covalent structures have high melting points.
56
Explain the properties of diamond in terms of its bonding.
Diamond has strong covalent bonds, contributing to its hardness and high melting point.
57
Justify a use for graphite based on its properties.
Graphite is used as a lubricant due to its layered structure allowing easy sliding.
58
Describe the structure of graphite.
Graphite consists of layers of carbon atoms that can slide over each other.
59
Explain the properties of graphite in terms of its bonding.
Graphite has delocalized electrons that allow for electrical conductivity.
60
Justify a use for diamond based on its properties.
Diamond is used in cutting tools due to its hardness.
61
What is the relationship between graphite and graphene?
Graphene is a single layer of carbon atoms from the structure of graphite.
62
How can the structure of a fullerene or nanotube be recognized?
Through diagrams and written descriptions.
63
What are the applications of fullerenes?
Fullerenes are used in drug delivery and materials science.
64
List the main physical properties of fullerenes.
* High stability * Unique electronic properties * Ability to form complex structures
65
Explain the structure of fullerenes.
Fullerenes consist of carbon atoms arranged in hollow spheres, ellipsoids, or tubes.
66
What properties can be explained using molecular models of graphene, nanotubes, and fullerenes?
Their strength, electrical conductivity, and thermal properties.
67
What is the molecular formula of buckminsterfullerene?
C60
68
List the properties and consequent uses of fullerenes and carbon nanotubes.
* High strength - used in composites * Electrical conductivity - used in electronics * Lightweight - used in materials science
69
Justify a use for graphene, nanotubes, and fullerenes based on their properties.
They are used in advanced materials due to their strength and conductivity.
70
What type of structure do metals form?
Giant structure ## Footnote Metals form extensive networks of atoms, contributing to their unique properties.
71
What is metallic bonding?
A type of bonding where metal atoms share delocalized electrons ## Footnote This results in the formation of a lattice structure that gives metals their characteristic properties.
72
How do metal atoms form giant structures?
By closely packing together in a lattice arrangement ## Footnote This packing allows for strong metallic bonds due to the attraction between positively charged metal ions and delocalized electrons.
73
What can be recognized in diagrams of metallic bonding?
Metallic bonding structures ## Footnote Diagrams typically illustrate the arrangement of metal ions and the sea of delocalized electrons.
74
What are the physical properties of metals?
Conductivity, malleability, ductility, and luster ## Footnote These properties result from the structure and bonding in metals.
75
How does metallic bonding explain the physical properties of metals?
Delocalized electrons allow for conductivity and malleability ## Footnote The metallic bond's flexibility contributes to the ductility and malleability of metals.
76
What effect does alloying have on metals?
Changes the structure and bonding, enhancing properties ## Footnote Alloying can improve strength, corrosion resistance, and other desirable characteristics.
77
What is the structure of a pure metal?
A regular arrangement of metal atoms in a lattice ## Footnote This regular arrangement is crucial for the properties exhibited by pure metals.
78
Why are metals alloyed?
To improve strength, durability, and other characteristics ## Footnote Alloys can provide better performance than pure metals in various applications.
79
Why are alloys more often used than pure metals?
Alloys typically have superior properties ## Footnote The enhanced properties can include increased strength, reduced corrosion, and better mechanical performance.

GCSE Revision (10 decks)

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