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AQA GCSE (9-1) Chemistry Higher > C2 Chemical Bonding > Flashcards

C2 Chemical Bonding Flashcards

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1
Q

<p>What are the three types of <b>chemical bonding</b>?</p>

A

<ul><li>Ionic Bonding</li><li>Covalent Bonding</li><li>Metallic Bonding</li></ul>

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2
Q

<p>What is <b>Ionic Bonding</b>?</p>

A

<p>Ionic Bonding is bonding between two oppositely charged ions</p>

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3
Q

<p>Where is Ionic Bonding found?</p>

A

<p>Ionic Bonding is found in compounds made of metals and non-metals</p>

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4
Q

<p>What is <b>Covalent Bonding</b>?</p>

A

<p>Covalent bonding is the bonding of two atoms sharing 1 or more pairs of electrons</p>

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5
Q

<p>Where is Covalent bonding found?</p>

A

<p>Covelant bonding is found in most non-metal elemnts and in compounds of non-metals</p>

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6
Q

<p>What is <b>Metallic Bonding</b>?</p>

A

<p>Metallic Bonding is the attraction between positively charged ions and negatively charged delocalised electrons</p>

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7
Q

<p>Where is Metallic Bonding found?</p>

A

<p>Metallic Bonding is found in metals and alloys</p>

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8
Q

<p>What are <b>Ions</b>?</p>

A

<p>Ions are charged particles</p>

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9
Q

<p>How are positively charged ions formed?</p>

A

<p>Positively charged ions are formed when an atom or molecue loses electrons</p>

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10
Q

<p>What is another name for positevely charged ions?</p>

A

<p>Cations</p>

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11
Q

<p>How are negatively charged ions formed?</p>

A

<p>Negatively charged ions are formed when an atom or molecule gains electrons</p>

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12
Q

<p>What is another name for negatively charged ions?</p>

A

<p>Anions</p>

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13
Q

<p>What are <b>Ionic Lattices</b>?</p>

A

<p>Ionic Lattices are giant structures held together by strong electrostatic forces between oppositely charged ions</p>

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14
Q

<p>What are the three states of matter?</p>

A

<ul><li>Gas</li><li>Liquid</li><li>Solid</li></ul>

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15
Q

<p>What is <b>melting</b>?</p>

A

<p>Melting is when a solid is heated to its melting point and changes into a liquid</p>

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16
Q

<p>What is <b>boiling</b>?</p>

A

<p>Boiling is when a liquid is heated to its boiling point and evaporates into a gas</p>

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17
Q

<p>What is <b>condensing</b>?</p>

A

<p>Condensing is when a gas is cooled to its boiling point and turns into a liquid</p>

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18
Q

<p>What is <b>freezing</b>?</p>

A

<p>Freezing is when a liquid is cooled to melting point and turns into a solid</p>

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19
Q

<p>Why do some substances have high melting points?</p>

A

<p>Some substances have high melting points as there are strong intermolecular forces between the particles</p>

<p>This means a lot of energy is required to melt the solid</p>

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20
Q

<p>What is <b>sublimation</b>?</p>

A

<p>Sublimation is a process that changes a solid to a gas</p>

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21
Q

<p>What is <b>desublimation</b> or <b>deposition</b>?</p>

A

<p>Desublimation or Deposition is a process that changes a gas to a solid</p>

22
Q

<p>What type of structures do Ioonic Compounds form?</p>

A

<p>Ionic Compounds always form Giant Ionic Lattice Structures</p>

23
Q

<p>What are the properties of Ionic Compounds?</p>

A

<ul><li>High Melting and Boiling Points</li><li>Conducts electricity when molten or dissolved</li></ul>

24
Q

<p>Why can Ionic Compounds conduct electricity when molten or dissolved?</p>

A

<p>The Ions in the lattice are free move so charge can flow</p>

25
Q

<p>Why can't Ionic Compounds conduct electricity as a solid?</p>

A

<p>Ions in the lattice are fixed so charges cannot flow</p>

26
Q

<p>Why do Ionic Compounds have high melting and boiling points?</p>

A

<p>To break the ionic bonds, large amounts of energy is needed to overcome the electrostatic forces between the ions in the lattice</p>

<p>Due to this, the ionic compounds have very high melting and boiling points</p>

27
Q

<p>Why do <b>simple covalent molecules</b> have low melting and boiling points?</p>

A

<p>The small covalent molecule is held together by strong covalent forces</p>

<p>Lots of small covalent molecules are held together by <b>Intermolecular forces</b></p>

<p>The intermolecular forces are weak and easy to break so little energy is required to overcome them. This meands small covalent molecules have low melting and boiling points</p>

28
Q

<p>What are <b>polymers</b>?</p>

A

<p>Polymers are large chain-like molecules, made up of repeating units</p>

29
Q

<p>Why are polymers often solids at room temperature?</p>

A

<p>Polymers are quite large so the intermolecular forces add up to be quite strong, holding the molecules together</p>

30
Q

<p>What are the properties of pure metals?</p>

A

<ul><li>Sonorous</li><li>Soft and Malleable</li><li>Ductile</li><li>High melting and Boiling Points</li><li>Conductors of Heat and Electricity</li></ul>

31
Q

<p>Why are pure metals soft and malleable?</p>

A

<p>As the metal ions are arranged in layers, they slide over each other easily when a force is applied</p>

32
Q

<p>Why do metals have high melting and boiling pounts?</p>

A

<p>Metals have high melting and boiling points as there are strong electrostatic forces between the metal ions and delocalised electrons</p>

33
Q

<p>What are <b>alloys</b>?</p>

A

<p>Alloys are a mixture of two or more elements where at least one is a metal</p>

34
Q

<p>Why are alloys harder than pure metals?</p>

A

<p>As alloys are made up of different sized ions, this distorts the regular layers of atoms in metals</p>

<p>This means its harder for the metal ions to slide over each other as the atoms are different sizes</p>

35
Q

<p>Why are metals <b>good conductors</b> of <b>electricity</b>?</p>

A

<p>Metals are good conductors of electricity as their delocalised electrons can carry a charge through the structure</p>

36
Q

<p>What are the properties of <b>diamond</b>?</p>

A

<ul><li>High melting point</li><li>Each Carbon atom forms 4 covalent bonds</li><li>Hard</li></ul>

37
Q

<p>What are the properties of <b>graphite</b>?</p>

A

<ul><li>Each carbon atom forms 3 covalent bonds</li><li>Soft</li><li>Conducts Electricity</li></ul>

38
Q

<p>Why is Graphite soft?</p>

A

<p>In Graphite, the carbon atoms form layers of hexagonal rings</p>

<p>The intermolecular forces between these layers are very weak, so the layers can slide over another easily. This makes Graphite soft</p>

39
Q

<p>Why can <b>Graphite</b> conduct electricity?</p>

A

<p>In Graphite, each carbon atoms forms 3 covalent bonds</p>

<p>This means there is a delocalised electron from each carbon atom. As the electrons are delocalised, they are free to move so Graphite can conduct electricity</p>

40
Q

<p>What is <b>Graphene</b>?</p>

A

<p>Graphene is a single layer of Graphite</p>

41
Q

<p>What are <b>fullerenes</b>?</p>

A

<p>Fullerenes are molecules of carbon atoms that have hollow shapes</p>

42
Q

<p>How many carbon atoms does buckministerfullerene have?</p>

A

<p>Buckministefullerene is made up of 60 carbon atoms</p>

43
Q

<p>What are the uses of spherical fullerenes?</p>

A

<ul><li>Catalysts</li><li>Lubricants</li><li>Delivering drugs into the body</li></ul>

44
Q

<p>What are the uses of cylindrical fullerenes?</p>

A

<ul><li>Electronics</li><li>Nanotechnology</li><li>Strengthening materials</li></ul>

45
Q

<p>How big is one nanometre in metres?</p>

A

<p>1×10⁻⁹m</p>

46
Q

<p>Why are <b>nanoparticles</b> cheap and efficient?</p>

A

<p>Nanoparticles have a high volume to area ratio</p>

<p>This means smaller amounts of materials are required for the same desired purpose, making them much more cheaper and efficient than larger particles</p>

47
Q

<p>How can nanoparticles be used as <b>catalysts</b>?</p>

A

<p>As there is a large surface area to volume ratio on nanoparticles, there is a larger area where the reactions can be catalysed</p>

48
Q

<p>How can nanoparticles be used in <b>medicine</b>?</p>

A

<p>Fullerene molecules can be used to efficiently deliver drugs to a specific area of the body to target disease</p>

49
Q

<p>How are nanoparticles used in <b>deoderant</b>?</p>

A

<p>Nanoparticles can have antimicrobial properties. They make deoderants more effective by killing bacteria</p>

50
Q

<p>What is the <b>Law of Conservation of Mass</b>?</p>

A

<p>The Law of Conservation of Mass states that</p>

<p><b>Total Mass of Products = Total Mass of Reactants</b></p>

51
Q

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A

<p></p>

AQA GCSE (9-1) Chemistry Higher (12 decks)

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