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Chemistry GCSE > Covalent Bonding, Metallic Bonding and Ionic bonding, Properties of metals, nanoparticles > Flashcards

Covalent Bonding, Metallic Bonding and Ionic bonding, Properties of metals, nanoparticles Flashcards

1
Q

What is covalent bonding?

A

When atoms share pairs of electrons. (strong bond)

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2
Q

Advantages of displayed formula

A
  • quick and easy to draw and identify
  • shows how they are bonded to each other
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3
Q

Advantages of ball and stick models

A
  • shows the shape of the molecule
  • 3D
  • shows which atoms are bonded to which
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4
Q

Advantages of dot and cross diagrams

A
  • shows which atoms are bonded to each other
  • shows electrons
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5
Q

Disadvantages of displayed formula

A
  • 2D
  • cannot see electrons
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6
Q

Disadvantages of ball and stick models

A
  • does not show electrons
  • hard to draw when there are many atoms
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7
Q

Disadvantages of dot and cross diagrams

A
  • does not show electrons orbiting
  • hard to draw if there are many atoms
  • 2D
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8
Q

Size of atom

A

1 nanometer (1x10^-9m)

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9
Q

Size of nucleus

A

About 1x10^-14m

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10
Q

Difference between simple and giant covalent structures

A

simple covalent structures have a fixed number of atoms (eg. ammonia) and giant covalent structures have large and variable amounts of atoms

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11
Q

Properties of giant covalent structures

A
  • high boiling and melting points (strong intermolecular forces)
  • strong (covalent bonds)
  • cannot conduct electricity (except for graphite and graphene)
  • has a lattice structure
  • not soluble in water
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12
Q

Properties of simple covalent molecules

A
  • low boiling and melting points
  • weak intermolecular forces
  • do not conduct electricity as they do not have an overall electric charge
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13
Q

What are polymers?

A

large molecules with many small repeating units called monomers that are joined with strong covalent bonds

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14
Q

What is graphene?

A

A single layer of graphite

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15
Q

Properties of graphene

A
  • very high melting point
  • very strong
  • conducts electricity well due to having delocalised electrons
  • often used in electronics and composites
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16
Q

What are fullerenes?

A
  • Molecules of carbon atoms with hollow shapes
  • based on hexagonal rings of carbon atoms but may also contain rings of five or seven carbon atoms
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17
Q

What was the first fullerene that was discovered?

A

Buckminsterfullerene (C60)

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18
Q

Properties of fullerenes

A
  • low melting and boiling point (weak intermolecular forces
  • cage like structure (can transport substances inside it eg. medicine)
  • good catalyst (large surface area compared to volume)
  • has a delocalised electron that can carry the charge
  • lightweight
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19
Q

Are the intermolecular forces of polymers strong

A

yes, so they remain as solids at room temperature

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20
Q

How is ethene converted to polyethene?

A

the double covalent bond between the carbon atoms are broken and is joined to a neighboring molecule

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21
Q

Draw the shorthand way of representing a polymer

A

(see goodnotes)

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22
Q

Compare diamond to graphite

A

(see notability)

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23
Q

Where do we find metals on the periodic table?

A

on the left

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24
Q

What is metallic bonding?

A
  • A strong electrostatic force of attraction between positive and delocalised electrons
  • the delocalised electrons are free to move through (not throughout) the whole structure, leaving positive ions.
  • positive metal ions surrounded by sea of delocalised electrons
25
Q

Advantages of the 2D diagram of metallic bonding

A
  • can see the “sea” of electrons
  • can see every atom easily (none are blocked or covered)
26
Q

Advantages of the 3D diagram of metallic bonding

A
  • shows layer arrangement of the atoms and the giant lattice structure
27
Q

Disadvantages of the 2D diagram of metallic bonding

A
  • cannot see the layer arrangement of the atoms/ the giant lattice structure
  • doesn’t show each indivual electron
28
Q

Disadvantages of the 3D diagram of metallic bonding

A
  • doesn’t show electrons at all
  • can only see outermost atoms
29
Q

Properties of metals

A
  • high melting and boiling point: strong electrostatic forces of attraction so it takes a lot of thermal energy to break the bond
  • malleable: metals consist of layers of ions that are the same size that can slide over each other when the metal is bent, hammered, or pressed
  • electrical conductor: delocalised electrons can carry electrical charge through the metal and move through the structure
30
Q

Why are alloys stronger and harder than pure metals

A
  • the layers are distorted so the particles cannot slide over each other as well
31
Q

Why do alloys not conduct as well as pure metals

A
  • distorted layers cause the delocalised electrons to not be able to move through the structure as easily.
32
Q

Describe ionic bonding

A

the metal atom loses its outermost electrons and transfers them to the non metal atom to complete the non metal atom’s outer shell. This makes the metal atom a positive ion and the non metal atom a negative ion as there aren’t enough electrons to balance the charge of the protons and vice versa. there is a strong electrostatic force of attraction between the oppositely charged ions

33
Q

Properties of ionic compounds

A
  • high melting and boiling point : the lattice structure and the strong electrostatic forces between the ions require a lot of thermal energy to break
  • Crystalline : this reflects the regular arrangement of teh ions
  • brittle : small distortions in the crystal bring ions with the same charge together and similar charges repel each other, breaking the crystal apart
  • soluble in water : the slightly negative oxygen in the water attracts the positive ions while the slightly negative hydrogen in the water attracts negative ions, pulling the crystal apart
  • do not conduct when solid : the ions cannot move when the ionic compound is solid there cannot carry any charge and cannot conduct electricity
  • conduct when molten/ in solution : the ions are free to move when molten or dissolved and will carry the charge and conduct electricity
34
Q

Draw a ionic bonding diagram for sodium chloride

A

see goodnotes

35
Q

What does the particle model of the three states of matter assume?

A

1) there are no forces between the particles
2) all particles in a substance are spherical
3) spheres are solid

36
Q

What are fullerenes usually used for?

A
  • lubricants
  • drug delivery
37
Q

Why do nanoparticles have different properties to bulk materials of the same substance?

A
  • high surface area to volume ratio
38
Q

What are nanoparticles used for?

A
  • healthcare, electronics, cosmetics, and as catalysts
39
Q

What is the size of the structures that nanoscience refers to?

A

structures that are 1-100 nm in size
(a few hundred atoms)

40
Q

How does the surface area to volume ratio change when the side of a cube decreases by a factor of 10?

A

it increases by a factor of 10

41
Q

What is the diameter of a coarse particle?

also refered to dust

A

1 x 10^-5m - 2.5 x 10^6 m

42
Q

What is the diameter of a fine particle?

A

1 x 10^-7 m and 2.5 x 10^-6 m
or 100-2500 nm

43
Q

Which type of particle is the smallest?

A

nanoparticle < fine particle < coarse particle

44
Q

What is 1nm in m?

A

1 x 10^-12m

45
Q

What is an application of nanoparticles in fabrics?

A
  • nanosilver woven into fabric to give anti-microbial properties
  • nano-titanium used to add sun protection to clothing
46
Q

What are the benefits of using nanoparticles in fabrics?

A
  • fends off bacteria that makes clothes smell after you sweat
  • adds sun protection (also used in sunscreen)
47
Q

What are the disadvantages of using nanoparticles in fabrics?

A
  • little known about effects of exposure to nanosilver for human body
  • nanosilver washes off clothes-> goes into wash water -> goes into sewage sludge/ biosolids that are treated for use
48
Q

What is an application of nanoparticles in medicine?

A
  • silver nanoparticles used to coat dressings + make surgical masks
  • antimicrobial properties
49
Q

What are the benefits of using nanoparticles in medicine?

A
  • incrediably small = can penetrate cell walls = makes them ideal to deliver drugs to cancer patient
50
Q

What are the potential disadvantages of using nanoparticles in medicine?

A
  • unaware of long term effects in body
  • small enough to penetrate blood brain barrier
  • may be toxic to brain
51
Q

What is an application of nanoparticles in electronics?

A
  • nanotubes conduct small electrical circuits for computers
  • allows display screens to be very thin
52
Q

What are the benefits of using nanoparticles in electronics?

A
  • decreases power consumption + weight
  • reduces size in translators and ICs
53
Q

What are the potential disadvantages of using nanoparticles in electronics?

A
  • could harm environment at disposal
54
Q

What is an application of nanoparticles in cosmetics?

A
  • used in creams, deodrants + suncreams
55
Q

What are the benefits of using nanoparticles in cosmetics and suncreams?

A
  • can be absorbed much deeper into the skin
  • absorbs UV light better = stops UV light penetrating into skin
56
Q

What are the potential disadvantages of using nanoparticles for cosmetics?

A
  • breathing in particles could affect lungs
  • could accumulate in organisms = unaware of effects
  • possible skin damage
57
Q

What are the applications of nanoparticles in catalysts?

A
  • speeds up reaction without being used up
  • platinum in fuel cells
58
Q

What are the benefits of using nanoparticles in catalysts?

A
  • large SA to volume ratio allows them to catalyse reactions effectively
59
Q

What are the potential disadvantages of using nanoparticles in catalysts?

A
  • may catalyse harmful reactions in the body

Chemistry GCSE (9 decks)

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