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chemistry one > bonding, structure, properties of matter > Flashcards

bonding, structure, properties of matter Flashcards

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1
Q

what are ionic bonds

A

two ions (metal and non metal) have opposite charges and therefore are attracted to each other by electrostatic forces. these created ionic compounds

  • the transfer of electrons
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2
Q

what is the structure of an ionic compound and how are these presented

A

3D lattice structure because each ion is attracted to all those around it

ball and stick diagrams

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3
Q

what are the properties of ionic compounds

A

high melting and boiling points
conductors of electricity

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4
Q

why are high melting and boiling points required for breaking ionic compounds

A

high melting and boiling points - determined by the strength of the bonds. because there is loads of ionic bonds, a lot of energy is required to break these. therefore needing a high temperature

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5
Q

what form do ionic compounds need to be in, in order to conduct electricity and why

A

conducts electricity when melted or disolved in water
when in solid form, all particles are fixed and therefore when melted or in liquid, ions are free to move. this movement of charged particles conduct electricity

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6
Q

what is the formular for the ionic compounds:
- hydroxide ions
- sulphate ions
- nitrate ions
- carbonate ions
- aluminium ions

A

hydroxide ions = OH-
sulphate = SO-2
nitrate = NO3-
carbonate = CO3 -2
aluminium = NH4 +

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7
Q

what are covalent bonds

A
  • sharing of electrons between non metals

when both metals are missing electrons and therefore create a bond to share meaning they both have a full outer shell

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8
Q

what diagrams do you use for covalent bonds

A

dot and cross OR displayed formular. for a displayed formular you place a line where there was a covalent bond

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9
Q

what type of substances do covalent bonds make

A
  • simple molecular substances such as chlorine
    -methane, water
  • larger structures such as polymers and giant covalent structures
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10
Q

what is metallic bonding

A

bonding between metals
- giant structure of metal atoms are arranged in a regular pattern. they share their outer shell of electrons meaning they become positive ions. there will be strong electrostatic attractions meaning metals are held together making it strong

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11
Q

what are properties of metallic bonding

A
  • very strong
  • high melting and boiling point
  • good conductors of electricity and heat because of delocalised electrons
  • malleable because of the regular structure, layers slide over each other
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12
Q

what are delocalised electrons

A

Bonding electrons that are no longer associated with any particular atom. electrons that are free to move

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13
Q

what are alloys

A

metallic bonds that contain two or more different elements. two different metals or non metals with different sized atoms

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14
Q

why do the two different elements need different sized atoms

A

disrupts the regular structure and layers can no longer slide over each other making them much harder than pure metal.

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15
Q

what is an example of an alloy and where is it used

A

steel, this is used in cars/ planes

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16
Q

what are the three states of mater and explain the properties and how they change between states

A

solid - strong forces of attraction meaning the particles are held together. this means there is a definite shape or volume

liquid - adding heat to solid meaning particles gain more energy causing them to vibrate breaking the bonds. weak forces of attraction meaning the particles are free to move

gas - more heat added, particles gain more energy weakening force holding particles. once at boiling point, particles will be able to break bonds all together. liquid evaporates to gas.

17
Q

what are the positives and negatives of the particle model

A

negatives - particles aren’t actually solid, inelastic or sphered shape
- doesn’t include details of the forces between particles such as how strong

positives - it is a useful simplification to allow understanding of the complicated concept

18
Q

what are state symbols for each state of matter

A

solid (s), liquid (l), gas (g), aqueous (aq) - disolved in water

19
Q

how can you predict what state something is when given an exam question with information

A

use an increasing temperature timeline

20
Q

what are polymers

A

chain of molecules, each polymer molecules is made up of smaller units called monomers

21
Q

how do you know that a molecule is a polymer

A

identify the repeating monomer

22
Q

use the monomer polypropene and identify the repeating monomer

H CH3 H CH3 H CH3 H
| | | | | | |
H - c - c - c - c - c - c - c - H
| | | | | | |
H H H H H H H

A

H CH3
| |
(- C - C -) n
| |
H H

23
Q

describe a polymers melting and boiling point

A

polymers intermolecular forces are quite weak ( weaker than covenant and iconic) yet because polymers have a large surface area, melting and boiling points a pretty high

24
Q

what are simple molecular substances

A

small molecules made up of a few covalently bonded atoms with weak intermolecular forces

25
Q

what is an example of a simple molecular force

A

ammonia/ chlorine

26
Q

why do simple molecular forces only need low temperatures for a melting and boiling point

A

only low temperatures are needed to break simple molecule forces because they only are breaking intermolecular forces and not covalent bonds

27
Q

what happens when you decrease down a group of simple molecular forces

A

the boiling point increases because molecules get larger and therefore increase the amount of intermolecular forces between them.

28
Q

what is another property of simple molecular forces

A

not a conductor of electricity
- this is because there are no free electrons and molecules have no electrical charge

29
Q

what is a giant covalent structure

A

huge numbers of non metals bonded together by covalent bonds. structured in a regular repeating lattice

30
Q

what are the properties of a giant covalent structure

A
  • they are very strong
  • have very high melting and boiling points
  • don’t conduct electricity
31
Q

what is an allotrope

A

different forms of the same element in the same physical state

32
Q

what are two allotropes of carbon and what are their structures

A

diamond and graphite
- giant covalent structures

33
Q

what are the properties of diamond and why

A
  • very strong
  • high melting point because they are covalently bonded
  • doesn’t conduct electricity because the carbon atoms are bonded to four other carbon atoms meaning there are delocalised electrons
34
Q

what are the structure and properties of graphite and why

A

atoms are arranged into hexagons which are arranged into flat sheets on top of each other to form layers

  • soft because the layers are held together weakly with no covalent bonds
  • high melting point because the INDIVIDUAL LAYERS have covalent bonds
  • conduct electricity because there are only three electrons and therefore electron gets delocalised
35
Q

what is a single layer of graphite called

A

graphene

36
Q

how is a fullerene formed

A

layers of graphite (graphene) is taken from the ground and turned into tubes and spheres

37
Q

what are the uses of fullerenes

A
  • used to surround drugs because they can be formed around other molecules
  • because of the large surface area: volume they can be used as an industrial catalyst
  • nanotubes can be used to make nanotechnology because they can conduct electricity
  • silver nanoparticles can kill bacteria in things like plasters because of their antibacterial properties
38
Q

what are some issues of nanoparticles give an example

A

because they are relatively new the effect on our bodies isn’t fully understood
an example would be sun cream
- it is more effective at protecting our skin yet we don’t know if it is getting into our skin and harming our cells
- also don’t know if it is harming our environment and what happens when they are washed into the sea

chemistry one (8 decks)

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