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Chemistry C2 > 2 Structure and properties > Flashcards

2 Structure and properties Flashcards

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1
Q

What is a lattice?

A

a 3D arrangement of particles in a giant structure

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2
Q

What is an ion?

A

a charged particle made when an atom loses or gains electrons

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3
Q

What is an ionic bond?

A

the electrostatic force of attraction between oppositely charged ions

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4
Q

Why do ionic compounds have high melting points?

A

because they have strong bonds which need lots of energy to break down

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5
Q

Why might ionic compounds conduct in a solution?

A

the ions can move freely in the solution, so they carry the charge, unlike in a solid where they don’t move

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6
Q

Why might ionic compounds be soluble in water?

A

the water breaks the bonds, but the ions don’t bond with the water

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7
Q

When do ionic compounds conduct electricity e.g. sodium chloride?

A

When they are part of a solution (with water) they conduct but not when they are solid

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8
Q

Which will conduct better in a solution- sodium chloride or magnesium oxide? Why?

A

Magnesium oxide
Requires 2 electrons to create ionic compound meaning there are stronger electrostatic forces- these don’t dissolve as easily so electricity conduction is weaker compared to sodium chloride which only loses 1 electron to make the ionic compound

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9
Q

What kind of melting and boiling points do substances with covalent bonds made up of simple molecules have?

A

Low

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10
Q

What are the covalent bonds like within the simple molecule?

A

Strong

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11
Q

What are the forces like between simple molecules?

A

Weak (why they have low melting and boiling points)

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12
Q

What charge do simple molecules have? Can they conduct electricity?

A

No overall charge therefore they can’t carry electrical charge- don’t conduct electricity

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13
Q

What are the forces called between atoms?

A

Intramolecular

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14
Q

What are the forces called between molecules?

A

Intermolecular

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15
Q

Why do ionic compounds only conduct electricity when they are dissolved in water?

A

their ions can freely move around and carry charge through the liquid

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16
Q

What are three examples of giant covalent structures made of carbon?

A
  • diamond
  • graphite
  • buckminister fullurene (similar structure to a football)
17
Q

What are the properties of diamond? (12)

A
  • Giant lattice structure that continues in all directions
  • Lustrous
  • Very hard
  • Colourless
  • High melting point
  • High boiling point
  • Insoluble in water
  • All its carbon atoms form 4 strong covalent bonds
  • Doesn’t conduct electricity
  • It is the hardest natural substance currently known
  • Artificial diamonds can be made by heating pure carbon to very high temperatures under enormous pressure
  • Industrial diamonds are used in drill bits of oil companies
18
Q

What are the properties of graphite? (14)

A
  • Relatively weak intermolecular forces between the layer so they can slide over each other easily
  • Carbon atoms are arranged in hexagons
  • Carbon atoms form 3 strong covalent bonds
  • Each carbon atom has 1 spare electron
  • The spare electron is free to move through the layers
  • Feels slippery
  • This spare electron allows graphite to conduct electricity
  • Insoluble in water
  • The spare atom is called a delocalised electron
  • Lustrous
  • Opaque
  • Soft
  • High melting point
  • Conducts electricity
19
Q

What are the properties of Fullerene? (8)

A
  • Made of hexagonal rings of carbon atoms
  • Describes any carbon structure which forms a cage-like structure
  • Can conduct electricity as 1 electron has not formed a bond in each atom- these are free to move around and carry current
  • Other molecules can be stored inside these cages which could potentially be used in medicine to transport drugs to a specific body part
  • Insoluble in water
  • 3 strong covalent bonds per atom
  • Black solid
  • Soluble in petrol (deep red solution)
20
Q

What are they general properties of metals? (9)

A
  • delocalised electrons
  • good conductors of heat
  • good conductors of electricity
  • solid at room temperature (with the exception of mercury)
  • malleable/ductile
  • very dense
  • shiny
  • high melting/boiling points
  • sonorous
21
Q

Why are metals dense?

A

generally solid at room temperature meaning they have a regular lattice of layers - arranged particles

22
Q

Why do metals have high melting/boiling points?

A

because the inter/intra molecular forces are strong meaning it takes more energy to break the bonds

23
Q

Why do metals conduct heat/electricity?

A

the delocalised electrons can flow through the giant metallic lattice- the electrical current and heat are transferred quickly through the metal by free electrons

24
Q

Why are metals malleable and ductile?

A

We can bend and shape metals because the layers of atoms (or ions) in a giant metallic structure can slide over each other

25
Q

What are shape-memory alloys?

A

Metals which can be deformed into different shapes but upon heating will return to its original shape

26
Q

What are examples of uses with shape-memory alloys?

A
  • broken bones (cool alloy before it is shaped around the bone and when the body heats it up it pulls the bone with it back to its original shape)
  • braces
    NITINOL- made from nickel and titanium- successful but expensive
27
Q

What affects the properties of polymers?

A

Monomers

Changing the reaction conditions

28
Q

What are three examples of monomers and their properties in polymers?

A
  • poly(ethene) used for bottles and bags
  • poly(propene) used for high density stronger items
  • nylon (acid and base) used for clothing bags and other things
29
Q

What is LDPE and how is it made?

A

Low density poly(ethene)
Made under very high pressure
In the presence of small amount of oxygen
Branded chains don’t pack close together

30
Q

What HDPE and how is it made?

A

High density poly(ethene)
Made under slightly raised pressure
In the presence of a catalyst
Unbranched chains pack close together

31
Q

What is the difference between LDPE and HDPE?

A

HDPE is stronger and has a higher softening temperature than LDPE

32
Q

What are thermosetting polymers?

A

Able to soften and melt easily when heated

Tangled web of polymer chains

33
Q

What are thermosetting polymers?

A

Strong covalent bonds between chains which form cross links

Will not soften but will char if heated very strongly

34
Q

What is nanoscience?

A

The study of small particles which are between 1 and 100 nanometres in size

35
Q

Why are nanoparticles being used?

A

They behave differently from the materials they are made from on a large scale however much as they are exciting there may be possible issues which arise from increased use

Chemistry C2 (5 decks)

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