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Chemistry > Bonding, structure and properties of matter > Flashcards

Bonding, structure and properties of matter Flashcards

1
Q

Describe a solid?

A

extremely hard to compress, particles are packed together(no spaces) in a regular pattern
Fixed shape, cannot flow but can vibrate

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2
Q

What happens when a solid or liquid changes state?

A

We can change the state by putting in or taking out energy

Melting and freezing takes place at the melting point

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3
Q

What happens when liquid goes to gas (vice versa)

A

strong forces there is a high boiling point

Boiling and condensing takes place at boiling point

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4
Q

What is ionic bonding?

A 
Elements have to react in order to get a full outer shell
metal+non-metal=ionic bonding 
ion is an atoms with an overall charge
METAL LOSES AN ION TO FORM + CHARGE
NON-METALGAIN AN ION TO FORM - CHARGE
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5
Q

What is the structure of an ionic compound?

A

Ionic compounds form giant structures where every positive ion is surrounded by a negative ion

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6
Q

What is metallic bonding?

A

Giant structure and regular layers
strong electrostatic attraction between sea of delocalised electrons and positive metal ions
electrons in the outer shell are delocalised

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7
Q

What are the properties of metallic bonding?

A
  • high melting and boiling points because lots of energy is required to break the strong metallic bonds
  • Layers of atoms can slide over each other so they can be bent and shaped
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8
Q

What is an alloy?

A

mixture of metals
pure metals are to soft to use
in alloys the added elements disturbs the regular pattern of metal atoms so layers do not slide over each other easily
alloys are stronger then pure metals

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9
Q

What is a Steel?

A

steel are alloys of iron containing specific amount of non-metal carbon

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10
Q

What is covalent bonding?

A

Share pair of electrons between atoms covalent bonding takes place between non-metal elements
H-H (single bond)
O=O(double bond)
H2O H-O-H

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11
Q

What is a simple molecule?

A

low melting and boiling points this means they are gases or liquid at room temp
The atoms in each molecule are held by strong covalent bonds

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12
Q

What do giant covalent structures do and give an example?

A

Always solid at room temperature and they have million strong covalent bonds
high melting point
EG. diamond and silicon dioxide and graphite

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13
Q

What is graphite made from?

A

FORM OF CARBON- each carbon atoms forms 3 covalent bonds, form hexagonal rings

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14
Q

What is fullerene and give an example?

A

Molecules of carbon atoms with hollow shapes
hexagonal rings
EG.BUCKMINISTER FULLERENE
CARBON NANOTUBES

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15
Q

What is graphene?

A

single layer of graphite
Extremely strong
Excellent conductor of electricity because it has delocalised electrons

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16
Q

What are the properties of polyemrs?

A 
Consist of very large molecules
plastics are made of polymers
atoms within the polymer molecules are held together by strong covalent bonds 
intermolecular forces are strong
solid at room temp
17
Q

What is a liquid?

A

extremely hard to compress, particles are close together, take the shape of their container and can flow because particles can move

18
Q

Describe a gas?

A

: easy to compress because particles are widely spaced, gases spread out and fill their container because particles move quickly/randomly

19
Q

How are solids broken?

A

Liquid has more kinetic energy than solid. Energy is put in to covert the state, the energy is used to break the force of attraction, once broken they move around
STRONGER THE FORCE OF ATTRACTION,MORE ENERGY IS NEEDED TO BREAK PARTICLES,HIGHER MELTING POINT

20
Q

What is the limitations of the particle model?

A
  • All particles are solid sphere(they have different shapes and not solid)
  • No forces between particles (forces have an impact on melting/boiling points)
21
Q

What are the properties of ionic bonding?

A

: high melting/boiling points, strong electrostatic forces require a great deal of heat energy to break

22
Q

Can ionic bonds conduct electricity?

A

Cannot conduct electricity when solid due to strong electrostatic forces and ions cannot move BUT can conduct electricity when they are molten because the ions can move and carry charge

23
Q

What do giant ionic lattice have?

A

very strong force of attraction between the positive/negative ions this is called electrostatic forces(ionic bonds)

24
Q

Why are metallic bonds a good conductor and why do they carry thermal energy?

A
  • Good conductors of heat and electricity because of delocalised electrons
  • electron carry electric current + carry thermal energy which allows metal to conduct heat
25
Q

Give an example of an alloy?

A 
EG. bronze is an alloy of copper and tin
 Brass is an alloy of copper and zinc 
Gold is mixed with silver,copper and zinc to form an 
alloy and is used for coins
24 CARAT GOLD IS 100% GOLD
26
Q

What does high/low carbon steel and aluminium alloy make?

A

High carbon steel- can make chisels
low carbon steel-soft, easily shaped and used to make car bodies
Aluminium alloys are low density and used to make aeroplanes

27
Q

Why does steal rust what is done to prevent this?

A

steel can rust because it contains iron to prevent this chromium and nickel is added to make stainless steel which is hard and corrosive resistant

28
Q

How does a simple molecule turn into a gas?

A

weak intermolecular forces between molecules
as temp increases molecules vibrate more and to a certain point were the weak intermolecular force is broken, molecules then turn into a gas

29
Q

Why does a simple molecule not conduct electricity?

A

do not conduct electricity because molecules do not have an overall electric charge

30
Q

Why does silicon dioxide have a very high melting/boiling point?

A

Contains silicon and oxygen

Very high melting and boiling point because there are a lot of covalent bonds and this takes a lot of energy to break

31
Q

What is the structure of diamond?

A

formed from the element carbon

each carbon atoms form four strong covalent bonds with other carbon atoms

32
Q

What are the properties of diamond?

A

High melting/boiling point
covalent bonds are broken when diamond is melted so we need a lot of energy
cannot conduct electricity because there’s no free electrons to carry charge

33
Q

Why does graphite have high melting/boiling point/Do they conduct electricity?

A

HIGH MELTING & BOILING POINTS-a lot of energy is needed to break bonds
CONDUCTORS OF HEAT AND ELECTRCITY-Delocalised electrons between layers

34
Q

Can layers of graphite slide?

A

SOFT AND SLIPPERY-arranged in layers and there’s no covalent bond between the layers so they can slide

35
Q

What are the properties of Buckminster fullerene?

A

contains 60 carbon atoms
Can be used as lubricant and catalyst
joined together as hexagons or pentagons

36
Q

What are the properties of carbon nanotubes?

A

High tensile strength (stretched without breaking)
cylindrical
excellent conductors of heat and electricity

Chemistry (10 decks)

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