C3- Structure and bonding Flashcards

1
Q

2 assumptions about particle model
2 key facts when we change the temp of the model

A

Solid spheres of identical size
No forces between particles
-Size and shape stays same
-Energy changes, faster if hotter

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2
Q

3 limitations of the particle model

A

-Particles aren’t solid
-Particles aren’t spherical
-There are forces between the particles

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3
Q

Solid particle model
spacing?
forces?
energy?
motion?
compression?
shape?

A

Closely packed
Strong forces between
Low energy
Vibrate about fixed positions
Can’t be compressed
Fixed shape

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4
Q

Liquid particle model spacing?
forces?
energy?
motion?
compression?
shape?

A

Closely packed
Medium forces between
Medium energy
Can slide over each other
Can’t be compressed
Fills container bottom

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5
Q

Gas particle model
spacing?
forces?
energy?
motion?
compression?
shape?

A

Spread out
Weak forces between
High energy
Free, random motion
Can be compressed
Fills whole container

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6
Q

Metallic bonding Defintion

A

Strong force of attraction between positive metal ions and negative delocalised electrons

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7
Q

Metallic bonding
Structure

A

A giant lattice of metal ions with delocalised electrons

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8
Q

Metallic bonding
Melting point

A

High melting point, strong electrostatic attraction between metal ions and delocalised electrons, takes high energy to break

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9
Q

Metallic bonding
Electrical conductors

A

Good electrical conductors, delocalised electrons can carry charge through the lattice

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10
Q

Metallic bonding
Thermal conductors

A

Good thermal conductors, delocalised electrons move through the lattice transferring thermal energy

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11
Q

Alloy definition

A

A mixture of two or more elements, one of which is a metal

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12
Q

Are alloys soft and why?

A

Alloys are harder than pure metals because of the irregular pattern of dif sized atoms

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13
Q

Ionic bonding
Definition

A

The strong force of electrostatic attraction between positive ions and negative ions

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14
Q

Ionic bonding is between…

A

Metals and non-metals

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15
Q

Ionic bonding
Structure

A

Giant lattice of cations and anions

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16
Q

Ionic bonding
Melting point

A

High melting point, strong forces of attraction between ions of opposite charge, takes lots of energy to break

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17
Q

Ionic bonding
Thermal conductors

A

Poor conductors, no free electrons

18
Q

Ionic bonding
Electrical conductors

A

Conducts electricity when dissolved or molten as the ions are free to move

19
Q

Covalent bonding
Definition

A

Strong electrostatic forces between a shared pair of electrons and the nuclei

20
Q

Covalent bonding is between…

A

Non-metals

21
Q

Simple covalent bonding
Structure

A

Simple structure with a fixed number of two or more atoms joined together

22
Q

Simple covalent molecule
Bonding

A

Strong covalent bonds between atoms
Weak intermolecular forces between molecules

23
Q

Simple covalent bonding
Melting point

A

Low melting point, weak intermolecular forces need little energy to overcome

24
Q

Simple covalent bonding
Electrical conductors

A

Do not conduct electricity, they have no free electrons

25
Simple covalent bonding Thermal conductors
Poor conduction, they have no free electrons
26
Giant covalent structure Structure
Giant structure with a variable number of atoms
27
Diamond Structure? Melting point? Electrical conductor? Thermal conductor?
Giant 3d structure, each atom to 4 other carbon High melting point, strong covalent bonds Insulator, no free electrons Thermal conductor, through the layers
28
Graphite Structure? Melting point? Electrical conductor? Thermal conductor?
Giant layers, each atom to 3 other carbon High melting point, strong covalent bonds Good conductor as has delocalised electrons
29
Graphene Structure? Melting point? Electrical conductor? Thermal conductor?
Giant layer with each atom to 3 other carbon High melting, strong covalent bonds Good conductor as has delocalised electrons
30
Fullerenes Structure? Melting point? Uses?
Simple hollow 3d molecules Variable, strong covalent in each shape, weak between shapes Carry drugs in body, as catalysts, as lubricants
31
Nanoscience
The study of particles between 1-100nm in size
32
Nanoparticle Diameter (nm)
1-100
33
Fine particle Symbol Diameter(nm)
PM2.5 100-2500
34
Coarse particle Symbol Diameter(nm)
PM10 2,500-10,000
35
Why are nanoparticles more effective than materials in bulk?
They have a high surface area to volume ratio, so a higher percentage of atoms are exposed at the surface. So smaller quantities are needed.
36
Dot and cross diagram Ads and dis
Ad- Clear where electrons come from Dis- Shows the electrons to be still
37
Structural formula Ad & Dis
Ad- Shows the bonds between atoms Dis- Can't tell where electron came from
38
Ball and stick diagram Ad and Dis
Ad- Shows ions as 3 dimensional Dis-Shows too much space
39
Inter molecular forces definition
Weak force of attraction between molecules in a covalent structure
40
Uses of nanoparticles Dangers of nanoparticles
Sun creams, cosmetics, medicine, catalysts Could absorb into skin and affect living cells or harm aquatic life