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Chemistry Paper 1 > Structure And Bonding > Flashcards

Structure And Bonding Flashcards

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1
Q

What are the three types of bonding

A

Covalent bonding
Ionic bonding
Metallic bonding

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2
Q

What is ionic bonding

A

Involves an attraction between oppositely charged ions. Found in compounds
Metal atoms lose electrons to become positively charged ions
Non metals gain electrons to become negatively charged ions

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3
Q

What is covalent bonding

A

Formed when 2 non metal atoms share pairs of electrons. Strong because the shared electrons are attracted to the nucleus of both atoms

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4
Q

What is metallic bonding

A

Involves an attraction between positively charged ions and negatively charged delocalised electrons

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5
Q

What are examples of covalent molecules

A

Small molecules- eg water
Large molecules- eg polyester
Giant covalent structures- eg diamond

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6
Q

What are the advantages and limitations of dot and cross diagrams

A

Shows the pairs of outer electrons and which atoms theyve come from
Doesn’t show how the atoms are arranged in space

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7
Q

What are the advantages and limitations of a ball and stick diagram

A

Fails at indicating movement of electrons
Also 2D

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8
Q

What are the properties of solids

A

Particles are very close and vibrate at a fixed position
Fixed shape and volume
When heated the particles vibrate with a greater amplitude

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9
Q

What are the properties of liquids

A

Particles are close together but they move and flow randomly
Have fixed volume but can change shape
When heated the average speed of particles increases

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10
Q

What are the properties of gases

A

Particles are far apart and move randomly in all directions
Gases change shape and volume
Negligible forces

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11
Q

What are the disadvantages to the “simple sphere” model

A

Forces between the particles aren’t shown as a result it’s impossible to know how strong these forces are and how much energy is needed
Portrays particles in a spherical way but they arnt
Portrays particles as solid when they arnt

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12
Q

What happens when particles gain or lose energy

A

Because of heating/cooling-they overcome or submit to the forces of other particles which causes them to change shape

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13
Q

What are the 4 types of state changes

A

Melting- (s-l)
Condensing- (g-l)
Boiling-(l-g)
Freezing-(l-s)

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14
Q

What happens with stronger forces

A

Stronger forces between particles means more energy is required to overcome those forces. They have higher melting and boiling points

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15
Q

What happens with weaker forces

A

Weaker forces between particles means less energy is required to overcome those forces. Have lower melting and boiling points

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16
Q

What does aq mean as a state symbol

A

Aqueous solutions (substances dissolved in water)

17
Q

What are the properties of ionic compounds

A

High melting and boiling points- lots of energy is needed to overcome the electrostatic forces between the ions and electrons in the lattices
Because if this they have high melting and boiling points

18
Q

Properties of ionic compounds (2)

A

Cannot conduct electricity when solid-when solid the ions in the lattice are fixed in place . TMT changes cannot flow so electricity can’t be conducted
Can conduct electricity when liquid-when dissolved in liquid the ions in the lattice are free to move because of this charge can flow and electricity can be conducted

19
Q

Why do small covalent molecules have low melting and boiling points

A

. Intermolecular forces are much weaker than the strong covalent bonds in molecules. When small molecular substances melt or boil, it is these weak intermolecular forces that are overcome. The covalent bonds are not broken. Relatively little energy is needed to overcome the intermolecular forces, so small molecular substances have low melting and boiling points.

20
Q

Why do bigger molecules have higher melting and boiling points

A

Because the smaller the molecule, the weaker the intermolecular forces.

21
Q

Why don’t small or big covalent molecules conduct electricity

A

They cannot conduct electricity because they do no have an overral electric charge

22
Q

Why are polymers solid at room temperature

A

They have very large molecules. Atoms in the polymer molecules are linked to other atoms by strong covalent bonds. Intermolecular forces between polymer molecules are relatively strong and require a lot of energy to overcome them

23
Q

What are the properties of Giant Covalent structures

A

No specific formula-because the structure can be any size
Very high melting points- because of strong covalent bonds
1 large molecule-Giant covalent structures exist as 1 large molecule. Means there are no intermolecular forces

24
Q

What are examples of giant covalent structures

A

Diamond
Graphite
Graphene
Fullerenes

25
Q

What are the properties of pure metals

A

High melting and boiling points-strong electrostatic forces between metal ions and delocalised electrons and giant structures of atoms
Soft and malleable-because the ions are arranged in layers they Slide Over eachother and be bent and shaped. This means they are too soft and should be mixed with other metals to make alloys which are harder

26
Q

What are metals as conductors like

A

Good conductors of electricity because the delocalised electrons in the metal carry electrical charge through it
Good conductors of heat because energy is transferred by the delocalised electrons

27
Q

What are alloys

A

A mixture is 2+ elements where at least one is a metal

28
Q

Why are alloys harder than metals

A

The different sized atoms distort the layer making them harder to Slide Over eachother. However the ions in metals are arranged in layers so they Slide Over eachother easily

29
Q

What are the properties of diamond

A

Doesn’t conduct electricity-because there are no delocalised electrons in its structure (bonded to 4 carbon atoms)
High melting point and is very hard- has lots of strong covalent bonds making it hard and having a high melting point

30
Q

What are the properties of graphite

A

Soft-carbon atoms form layers of hexagonal rings with each layer held together by weak intermolecular forces. Layers Slide Over and have no covalent bonds between the layers so it’s very soft
Conducts electricity-it is bonded to 3 carbon atoms which means that there is 1 delocalised electron which moves freely to carry the charge

31
Q

What are the properties of Graphene

A

Conducts electricity-single layer of graphite so it also conducts electricity
Light but strong-Graphene is 1 layer thick. Makes it light however the atoms within the layers are tightly bonded and elastic because the planes of atoms can flex relatively easily without the atoms breaking
Useful in electronics and composites

32
Q

What was the first fullerene to be discovered and properties

A

Buckminster fullerene
Molecules of carbon atoms with hollow shapes
Based on hexagonal rings of carbon atoms but they may also contain rings with 5 or 7 carbon atoms

33
Q

What is the formula of buckminster fullerene

A

C60

34
Q

What are the common uses of these fullerenes

A

Catalysts
Lubricants
Delivering drugs into the body

35
Q

What are the properties of carbon nanotubes

A

Cylindercal fullerenes with very high length to diameter ratios

36
Q

What are the uses of carbon nanotubes

A

Nanotechnology, electronics and materials

37
Q

What is the structure of sodium chloride

A

Na+ and Cl-

38
Q

What are the molecules of hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia and methane

A

H2, HCl, O2, Cl2, NH3 and CH4

39
Q

How does particle theory help to explain melting boiling freezing and condensing

A

The amount of energy needed to change state from a solid to liquid and from liquid to gas depends on the strength of the forces between particles
The nature of the particles involved depends on the type of bonding and the structure of the substance. The stronger the forces between the particles the higher the melting and boiling point

Chemistry Paper 1 (5 decks)

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