BONDING AND STRUCTURE Flashcards

1
Q

what bonds are in a giant covalent structure?

A

all the atoms are bonded by strong covalent bonds

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2
Q

what are the properties of a giant covalent structure?

A

🌡very high melting and boiling points - lots of energy required to break the covalent bonds
🌡They don’t have any ions, so they don’t conduct electricity. even when they are molten
🌡 they are insoluble in water

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3
Q

give three examples of giant covalent structures?

A

💎diamond
💎graphite
💎silicon dioxide

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4
Q

properties of a diamond?

A

💎it has 4 covalent bonds
💎 exceptionally hard
💎 has a boiling point of 4827°
💎 arranged in a perfect giant lattice

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5
Q

what are the properties and structure of graphite?

A

✏️only 3 bonds forming hexagons
✏️ in layers connected by weak intermolecular forces. this means the layers can slide making it a soft and slippery material
✏️there is one spare electron which can move freely throughout the layers
✏️ delocalised electrons mean they can conduct electricity and thermal energy

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6
Q

what are fullerenes?

A

fullerenes are a structure of carbon atoms that join together to create a hollow shape.
the structure is based on hexagonal rings however some are made up of pentagonal or heptagonal carbon atoms

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7
Q

what was the first fullerene to be discovered?

A

buckminsterfullerene which was made up of 60 carbon atoms in a spherical form

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8
Q

how are fullerenes used?

A

👩‍🔬to deliver drugs into the body
👩‍🔬as lubricants
👩‍🔬as catalysts because they have a large surface area to volume ration

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9
Q

what are cylindrical fullerenes called?

A

carbon nanotubes

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10
Q

what are the properties of cylindrical fullerenes?

A

🎾the have high tensile strength ( they are capable of being drawn out or stretched)
🎾high electrical and thermal conductivity ( because bonding gives them a delocalised electron)

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11
Q

what is graphene?

A

graphene is a single layer of graphite. it is a layer of hexagonal rings. around 1 atom thick

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12
Q

what are the properties of graphene?

A

👉good conductor of thermal energy and electricity (even better than graphite
👉has a very low density
👉most reactive form of carbon

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13
Q

properties of metallic structures?

A

➕ metal ions are arranged in regular layers
➕ the outer electron from each metal atom can move freely throughout the structure to form a SEA OF DELOCALISED ELECTRONS
➕strong electrostatic attraction between the electrons and the metal ions hold the structure together
➕able to slide over eachother due to tightly packed layers, therefore, are extremely mailable

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14
Q

what is an alloy?

A

an alloy is a mixture of metals. for example, steel is made up of iron and carbon. carbon atoms are much bigger than iron atoms making ht layers uneven and harder for them to slide over one another.
this makes alloys harder than metals

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15
Q

uses of metallic structures?

A

🙃 good conductors of thermal energy and heat

🙂 this is because they have high melting points

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16
Q

how do the metal ions hold together?

A

the delocalised electrons are connected by electrostatic forces of attraction

17
Q

why are metallic structures malleable?

A

because the electrons can move while holding the electrostatic forces, the lattice can distort.
when struck, the metals can slip past one another without braking up the metallic structure

18
Q

why do metallic structures have high melting points?

A

the electrostatic forces of attraction extend in all directions within the lattice and requires a lot of energy to break up.

19
Q

what is the diameter of a nanoparticle?

A

1nm to 100nm

20
Q

how do nanoparticles behave?

A

nanoparticles have a high surface area to volume ratio, meaning that they are more reactive than normal particles

21
Q

what are the uses of nanoparticles

A

👉🏻cosmetics - they are used in deodorants and face creams as they absorb deeper into the skin
👉🏻medicine - carbon nanocages are used to deliver drugs. in wound dressings, silver nanoparticles are used to protect the skin against bacteria
👉surface area to volume ration makes them effective catalysts