2. Bonding, Structure, and the Properties of Matter Flashcards
(99 cards)
1
Q
What are the three types of strong chemical bonds?
A
Ionic, covalent, and metallic bonds.
2
Q
What characterizes ionic bonding?
A
Ionic bonding involves oppositely charged ions.
3
Q
What characterizes covalent bonding?
A
Covalent bonding involves atoms that share pairs of electrons.
4
Q
What characterizes metallic bonding?
A
Metallic bonding involves atoms that share delocalized electrons.
5
Q
In which types of elements does ionic bonding occur?
A
Ionic bonding occurs in compounds formed from metals combined with non-metals.
6
Q
In which types of elements does covalent bonding occur?
A
Covalent bonding occurs in most non-metallic elements and in compounds of non-metals.
7
Q
In which types of elements does metallic bonding occur?
A
Metallic bonding occurs in metallic elements and alloys.
8
Q
How do metal atoms behave during ionic bonding?
A
Metal atoms lose electrons to become positively charged ions.
9
Q
How do non-metal atoms behave during ionic bonding?
A
Non-metal atoms gain electrons to become negatively charged ions.
10
Q
What is the electronic structure of ions produced by metals in Groups 1 and 2 and non-metals in Groups 6 and 7?
A
They have the electronic structure of a noble gas (Group 0).
11
Q
What is an ionic compound?
A
An ionic compound is a giant structure of ions held together by strong electrostatic forces of attraction.
12
Q
What is the nature of the forces in ionic bonding?
A
The forces act in all directions in the lattice.
13
Q
What is a dot and cross diagram used for?
A
It represents the electron transfer during the formation of an ionic compound.
14
Q
What should students be able to do with dot and cross diagrams?
A
Students should be able to draw dot and cross diagrams for ionic compounds formed by metals in Groups 1 and 2 with non-metals in Groups 6 and 7.
15
Q
How can the charge on ions be determined?
A
The charge on the ions relates to the group number of the element in the periodic table.
16
Q
Which groups of metals and non-metals are relevant for determining ionic charges?
A
Metals in Groups 1 and 2 and non-metals in Groups 6 and 7.
17
Q
What is the significance of the arrangement of atoms in materials?
A
The arrangement of atoms in materials explains their physical and chemical properties.
18
Q
How do chemists use theories of structure and bonding?
A
Chemists use these theories to engineer new materials with desirable properties.
19
Q
What is the role of ionic compounds in chemistry?
A
Ionic compounds exemplify the properties of ionic bonding and are used in various applications.
20
Q
What is the importance of understanding chemical bonding?
A
Understanding chemical bonding helps explain how atoms are held together in different structures.
21
Q
What can the analysis of structures reveal?
A
Analysis of structures shows that atoms can be arranged in a variety of ways, including molecular and giant structures.
22
Q
What is the relationship between structure and technology?
A
The properties of materials, derived from their structure, may offer new applications in various technologies.
23
Q
What type of bond is formed when atoms share pairs of electrons?
A
Covalent bonds.
24
Q
What are the three states of matter?
A
Solid, liquid, and gas.
25
What is the structure of sodium chloride primarily characterized as?
Ionic.
26
What should students be able to deduce from a diagram of a compound's structure?
That a compound is ionic.
27
What are the limitations of using dot and cross, ball and stick, and 2D/3D diagrams in chemistry?
They may not accurately represent the giant ionic structure or the complexity of molecular bonding.
28
What is the empirical formula of an ionic compound?
It can be worked out from a model or diagram showing the ions in the structure.
29
What types of structures can covalently bonded substances form?
Small molecules, polymers, or giant covalent structures.
30
Name two examples of giant covalent structures.
Diamond and silicon dioxide.
31
What is a characteristic feature of metals in terms of atomic structure?
They consist of giant structures of atoms arranged in a regular pattern.
32
What happens to the electrons in the outer shell of metal atoms?
They are delocalised and free to move through the whole structure.
33
What gives rise to strong metallic bonds in metals?
The sharing of delocalised electrons.
34
How can covalent bonds in molecules be represented?
Using a line to represent a single bond.
35
What should students be able to recognize from chemical formulas?
Common substances that consist of small molecules.
36
What is the representation of polymers in chemistry?
They can be represented in the form of repeating units where n is a large number.
37
What is the importance of understanding the bonding and structure of substances?
It relates to the properties of those substances.
38
What is a key skill students should develop regarding molecular diagrams?
To deduce the molecular formula from given models or diagrams.
39
What are the two types of representations for bonding in metals?
2D and 3D forms.
40
What is the significance of the delocalised electrons in metallic bonding?
They contribute to the strength and conductivity of the metal.
41
What should students be familiar with regarding sodium chloride?
The structure of sodium chloride, but not necessarily other ionic compounds.
42
What is a key opportunity for skills development in chemistry according to the notes?
Visualizing and representing 2D and 3D forms.
43
What is the role of diagrams in understanding chemical bonding?
They help recognize substances and their bonding types.
44
What type of bonding is characterized by strong bonds between atoms?
Covalent bonding.
45
What processes occur at the melting point?
Melting and freezing.
46
What processes occur at the boiling point?
Boiling and condensing.
47
How can the three states of matter be represented in a simple model?
Particles are represented by small solid spheres.
48
What does particle theory explain regarding changes of state?
It helps to explain melting, boiling, freezing, and condensing.
49
What determines the amount of energy needed to change state from solid to liquid and from liquid to gas?
The strength of the forces between the particles of the substance.
50
How do the strength of forces between particles affect melting and boiling points?
Stronger forces result in higher melting and boiling points.
51
What are some limitations of the simple particle model?
It does not account for forces, represents all particles as spheres, and assumes spheres are solid.
52
What state symbols represent solid, liquid, gas, and aqueous solutions in chemical equations?
(s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solutions.
53
What structure do ionic compounds have?
Regular structures known as giant ionic lattices.
54
Why do ionic compounds have high melting and boiling points?
Because of the large amounts of energy needed to break the strong electrostatic forces between oppositely charged ions.
55
What happens to ionic compounds when they are melted or dissolved in water?
They conduct electricity because the ions are free to move.
56
What are the typical states and properties of substances that consist of small molecules?
They are usually gases or liquids with relatively low melting and boiling points.
57
What type of forces are present in small molecular substances?
Weak intermolecular forces.
58
What is overcome when small molecular substances melt or boil?
The intermolecular forces, not the covalent bonds.
59
How do intermolecular forces relate to the size of molecules?
Intermolecular forces increase with the size of the molecules, leading to higher melting and boiling points for larger molecules.
60
Why do small molecular substances not conduct electricity?
Because the molecules do not have an overall electric charge.
61
What should students be able to predict regarding states of substances?
The states of substances at different temperatures given appropriate data.
62
What should students explain about changes of state?
The different temperatures at which changes of state occur in terms of energy transfers and types of bonding.
63
What misconception about atoms should students recognize?
That atoms themselves do not have the bulk properties of materials.
64
What should students explain regarding the limitations of particle theory?
The limitations when particles are represented by solid inelastic spheres with no forces between them.
65
What is the significance of the AQA specification link provided?
It directs students to the most up-to-date specification, resources, support, and administration.
66
What are polymers and how are their molecules structured?
Polymers are substances with very large molecules where atoms are linked by strong covalent bonds, resulting in strong intermolecular forces that keep them solid at room temperature.
67
What are giant covalent structures and what are their melting points?
Giant covalent structures are solids with very high melting points, where all atoms are linked by strong covalent bonds that must be overcome to melt or boil the substance.
68
Name three examples of giant covalent structures.
Diamond, graphite, and silicon dioxide (silica) are examples of giant covalent structures.
69
What is the structure of pure metals and how does it affect their properties?
Pure metals have atoms arranged in layers, allowing them to be bent and shaped, but they are too soft for many uses.
70
Why are alloys harder than pure metals?
Alloys are harder than pure metals because the mixing of different metals distorts the layers of atoms, preventing them from sliding over each other easily.
71
What makes metals good conductors of electricity?
Metals are good conductors of electricity due to delocalised electrons that carry electrical charge through the metal.
72
How do delocalised electrons contribute to thermal conductivity in metals?
Delocalised electrons in metals transfer thermal energy, making them good conductors of thermal energy.
73
Describe the bonding structure of diamond.
In diamond, each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure, resulting in its hardness and high melting point.
74
What are the electrical conductivity properties of diamond?
Diamond does not conduct electricity due to the absence of free-moving electrons.
75
What is the bonding structure of graphite?
In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, creating layers of hexagonal rings with no covalent bonds between the layers.
76
How does the structure of graphite affect its electrical conductivity?
Graphite has delocalised electrons, similar to metals, allowing it to conduct electricity.
77
What is graphene and what are its applications?
Graphene is a single layer of graphite with properties that make it useful in electronics and composites.
78
What are the properties of graphene related to its structure and bonding?
Graphene has a two-dimensional structure with a hexagonal lattice of carbon atoms, exhibiting high electrical conductivity, strength, and flexibility.
79
What are fullerenes and how are they structured?
Fullerenes are molecules of carbon atoms with hollow shapes, based on hexagonal rings, and may include rings with five or seven carbon atoms.
80
What is Buckminsterfullerene and what is its shape?
Buckminsterfullerene (C60) is the first fullerene discovered, characterized by its spherical shape.
81
What are carbon nanotubes and what are their properties?
Carbon nanotubes are cylindrical fullerenes with high length to diameter ratios, making them useful in nanotechnology, electronics, and materials.
82
How can students recognize graphene and fullerenes?
Students should be able to identify graphene and fullerenes from diagrams and descriptions of their bonding and structure.
83
What are some applications of fullerenes and carbon nanotubes?
Fullerenes and carbon nanotubes are used in nanotechnology, electronics, and materials due to their unique properties.
84
What is the size range of nanoparticles in nanoscience?
Nanoscience refers to structures that are 1-100 nm in size, consisting of a few hundred atoms.
85
How do nanoparticles compare in size to fine and coarse particles?
Nanoparticles are smaller than fine particles (100-2500 nm) and coarse particles (1 x 10^-5 m to 2.5 x 10^-6 m), which are often referred to as dust.
86
What happens to the surface area to volume ratio as the side of a cube decreases?
As the side of a cube decreases by a factor of 10, the surface area to volume ratio increases by a factor of 10.
87
Why do nanoparticles have different properties compared to bulk materials?
Nanoparticles may have different properties due to their high surface area to volume ratio, often requiring smaller quantities to be effective.
88
What are some applications of nanoparticles?
Nanoparticles are used in medicine, electronics, cosmetics, sun creams, deodorants, and as catalysts.
89
What should students evaluate regarding the use of nanoparticles?
Students should evaluate the advantages and disadvantages of nanoparticulate materials for specified purposes.
90
What are the risks associated with the use of nanoparticles?
There are possible risks associated with the use of nanoparticles that students should be aware of.
91
What is the purpose of quantitative analysis in chemistry?
Quantitative analysis is used to determine the formulae of compounds and the equations for reactions, allowing for purity determination and yield monitoring.
92
Why is classifying chemical reactions important for chemists?
Classifying chemical reactions helps chemists understand how different chemicals react, establish patterns, and make predictions about chemical behavior.
93
How do chemical equations function in chemistry?
Chemical equations represent chemical reactions and serve as a key means for chemists to communicate chemical ideas.
94
What is the significance of the surface area to volume ratio in nanoparticles?
The high surface area to volume ratio in nanoparticles can lead to enhanced reactivity and different physical properties compared to bulk materials.
95
What is the relationship between particle size and the effectiveness of materials?
Smaller particles, such as nanoparticles, may require smaller quantities to achieve the same effectiveness as larger particles.
96
What is the typical size range for fine particles (PM2.5)?
Fine particles (PM2.5) have diameters between 100 and 2500 nm.
97
What is the typical size range for coarse particles (PM10)?
Coarse particles (PM10) have diameters between 1 x 10^-5 m and 2.5 x 10^-6 m.
98
What are the dimensions students should compare when studying nanoscience?
Students should compare 'nano' dimensions to typical dimensions of atoms and molecules.
99
What skills should students develop when studying nanoparticles?
Students should develop skills in making order of magnitude calculations, using ratios, fractions, percentages, and estimating results of simple calculations.
