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GCSE- Chemistry > Topic 1.3- Key concepts/ types of a substance > Flashcards

Topic 1.3- Key concepts/ types of a substance Flashcards

Types of a substance

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1
Q

Why can elements be classified as Ionic, Simple/giant covalent, or metallic.

A

-Different atoms cuase different bonds:
- Ionic, Covalent or metallic bonds.

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2
Q

What is an ionic structure?

A
  • Gas (non-metal) and a metal
  • Held together by strong electrostatic forces between charged ions
  • E.g magnesium oxide
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3
Q

What is a simple molecular structure?

A
  • Strong covalent bonds between thee atoms of the molecules
  • Weak intermolecular forces between the molecules (e.g water)
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4
Q

What is a giant covalent structure?

A
  • Covalent bonds form one structure
  • Graphite, diamond
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5
Q

What is a metallic structure?

A
  • Lattice of positive metal ions
  • and free electrons
  • Strong electrostatic forces of attraction
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6
Q

What and why is Ionic melting point?

A

-High
-Strong electrostatic forces between the positive metal and negative gas

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7
Q

What and why is simple molecular melting point?

A

-Low
-Covelant
-Weak intermolecular forces between molecules

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8
Q

What and why is giant covalent melting point?

A

-High
-It is one molecule and therefore has no weak intermolecular forces
-Strong electrostatic forces

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9
Q

What and why is Metallic melting point?

A

-High
-Strong electrostatic forces between delocalised electrons and positive ions.

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10
Q

What and why is Ionic bonds physical state?

A

-solid
-high melting point

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11
Q

What and why is simple molecular bonds physical state?

A

-gas
-low melting point

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12
Q

What and why is giant covalent bonds physical state?

A

-solid
-high melting point

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13
Q

What and why is metallic bonds physical state?

A

-solid high melting point

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14
Q

What and why is Ionic solubility in water?

A
  • Many are soluble
  • Water molecules ( electrons are generally closer to oxygen as oxygen has more protons)
  • In water Oxygen is more negative and hydrogens are more positive
  • Positive metal will move to oxygen
  • Negative gas will move to hydrogen
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15
Q

What and why is simple molecular solubility in water?

A
  • Few are soluble
    -Water is polar and simple molecular structures are normally non-polar
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16
Q

What and why is giant covelant solubility in water?

A

-Insoluble
-Strong covalent bonds

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17
Q

What and why is metallic solubility in water?

A

-Insoluble
-Non polar and water is polar

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18
Q

What and why does/ doesn’t Ionic conduct electricity?

A

-Only in molten form/ in solution
- Ions can move freely

19
Q

What and why does/ doesn’t simple molecular conduct electricity?

A
  • Most do not
  • they are neutral
20
Q

What and why does/ doesn’t giant covalent conduct electricity?

A
  • Most do not conduct
  • Most have no free electrons
21
Q

What and why does/ doesn’t metallic conduct electricity?

A
  • Can conduct
  • Free delocalised electrons
22
Q

What are two main examples of giant covalent structures made of carbon?

A
  • Diamond
  • Graphite
23
Q

What is the structure of graphite?

A
  • One atom thick
  • Light
  • Strong
  • Conducts electricity
  • high melting and boiling point
24
Q

Why can graphite conduct electricity?

A
  • Graphite is made of three carbon atoms bonded to one carbon atom
  • Carbon has 4 electrons on outer shell
  • One free electron
  • Hexagonal shape
  • High melting point
25
Q

Why does graphite have a high boiling point?

Despite weak intermolecular forces between layers

A
  • Strong covalent bonds
26
Q

Properties of diamond?

A
  • Very strong
  • High melting/ boiling point
  • Does not conduct electricity
  • rigid lattice structure
27
Q

Why can’t diamonds conduct electricity?

A
  • Carbon has four bonds each, no free electrons
28
Q

Why do diamonds have a high melting/boiling point?

A
  • No weak intermolecular forces
  • All strong covalent bonds between atoms
29
Q

Why is diamond used in cutting?

A
  • Strong
  • Hard
  • strong covalent bonds
30
Q

Why is graphite used in lubrication?

A
  • Hexagonal sheets can slide past each-other due to weak intermolecular forces.
  • Soft, slippery
  • High melting point due to strong covalent bonds
31
Q

Why is graphite used in electrodes?

A
  • Free electron
32
Q

What is graphene and what are its properties?

thickness, electrical, boiling points

A
  • One layer of graphite
  • Conducts electricity (free electrons)
  • High melting/boiling point (no layers, no weak intermolecular forces)
33
Q

What are fullerenes?

A

-Hollow carbon structures
- Made of hexagonal shapes
( could have parts of 5, or 7 connected, pentagonal or heptagonal)

34
Q

What was the first fullerene

A
  • Buckminsterfullerene
  • 60 carbon atoms
  • Ball shape
35
Q

What are the uses of fullerenes like Buckminsterfullerene?

A
  • Deliver drugs
  • Lubricants
  • Catalysts
36
Q

Uses of carbon Nanotubes ?

(rolled graphene sheet)

A
  • Very long, small diameter
  • Extremely elastic
  • Reinforce materials ( tennis rackets)
37
Q

Describe poly(ethene)

A
  • C2H4
  • chain of carbon that consists of large molecules
  • Hydrocarbon
38
Q

Metals properties?

A
  • Conduct electricity - free delocalised electrons
  • Malleable, uniform layers can slide over each-other.
39
Q

Describe most metals?

A
  • High melting and boiling point
  • Shiny
  • Conduct electricity well
40
Q

Describe most non- metals

A
  • Low melting and boiling point
  • poor conductors of electricity
41
Q

Limitations of the dot and cross diagram?

A
  • Not 3-D
  • looks like electrons are different
42
Q

Limitations of the ball and stick diagram?

A
  • Atoms are far apart
  • Doesn’t include electrons are protons
43
Q

Ideas needed to see in models?

A
  • Electrons the same
  • Protons
  • 3-D
  • Bonded and close together
  • Respective sizes of atoms
  • Number of atoms included

GCSE- Chemistry (9 decks)

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