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GCSE AQA Chemistry Flashcards > C3 Structure and Bonding > Flashcards

C3 Structure and Bonding Flashcards

1
Q

What are the three types of strong bonding?

A

Ionic,covalent and metalic

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2
Q

What is a metalic bond?

A

Electrostatic attraction between delocalised outer shell electrons and metal ions

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3
Q

Electrical conductivity of a metalic bond?

A

Good as a solid
Good as a liquid

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4
Q

What is an ionic bond?

A

Electrostatic attraction between oppositely charged ions

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5
Q

What is the electrical conductivity of an ionic bond?

A

Poor as a solid
Good as liquid or aqueous

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6
Q

What is a covalent?

A

Electrostatic attraction between a shared pair of electrons and the nuclei of two atoms

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7
Q

What is electrical conductivity of a covalent bond?

A

Poor as a solid (with some exceptions)
Poor as a liquid and gas

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8
Q

What are the three chemical structures?

A
  • Giant (Metalic/Ionic/Covalent)
  • Simple Molecular
  • Monatomic
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9
Q

Which structure ONLY conduct as liquid?

A
  • Giant Ionic
  • Giant Covalent (graphite,diamond,SiO2)
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10
Q

What happens when elements react?

A

They form compounds by either: gaining, losing or sharing electrons

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11
Q

In Ionic bonding the particles are….

A

Oppositely charged ions.

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12
Q

In Covalent bonding the particles are….

A

non-metal atoms which share pairs of electrons

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13
Q

Properites of ionic compounds:

A
  • High melting points
  • Good conductors of electricity when melted or dissolved in water
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14
Q

Properties of Metalic bonds:

A
  • High melting points
  • Good conductors of heat and electricity in any state
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15
Q

What are the properites of small molecules?

A
  • Low melting poins
  • Poor conductors of electricty
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16
Q

Why are metalic bonds good conductors?

A

Structures contain charged particles (delocalised electrons) that can move through the whole structure

17
Q

What are the carbon allotropes?

A
  • Diamond
  • Graphite
  • Fullerene
18
Q

Properties of diamond:

A
  • Colourless, Transparent
  • Lustrous (shiny)
  • Hard
  • Solid at room temperature
  • Has 4 strong Covalent bonds per Carbon atom
19
Q

Properties of graphite :

A
  • Black , Opaque
  • Lustrous
  • Soft and slippery
  • Solid at room temp
  • Delocalised electrons, weak forces between layers
  • 3 Strong Covalent bonds per Carbon atom
20
Q

Fulleren properties :

A
  • Dark
  • Needle like crystals
  • 3 strong covalent bonds per Carbon atom
21
Q

How are atoms in metals arranged?

A

Closely packed together in regular layers

22
Q

1 nanometre is …..

A

1x10^-9 meters

Billionth of a metre

23
Q

What does prefix ‘nano-‘ mean?

A

Nano- means one billionth

24
Q

Why is silver nanoparticles in socks?

A

Silver nano-particles have longer-lasting properties (such as anti-bacterial) than bigger particles of silver. That why they are used in socks to kill bacteria and prevent bad smells

25
Q

What is the diameter of a nano particle?

A

1 - 100 nanometrs
1 x 10^-9 meters - 1 x 10^7 meters

26
Q

What is the diameter of a fine particle?

A

100 - 2500 nanometers
(1x10^-7 - 2.5x10^-6 meters)

27
Q

What is the diameter of coarse particles?

A

2500 - 10000 nanometers
2.5x10^-6 - 1x10^-5

28
Q

Why are nanoparticles more useful?

A

They have a larger surface area to volume ratio

29
Q

Uses of nanoparticles :

A
  • Medicine : MRI scanning and cancer therapies
  • Electronics : Used in memory chips
  • Cosmetics : Used in skincare lotions to encapsule nutrients
  • Sun Cream : Replaced zinc oxide to make it clear
  • Deodorant : Silver has antibacterial properties
  • Catalysts : Self-Cleaning windows
30
Q

How to find the surface area to volume ratio?

A

Surface area to volume ratio = Surface area/Volume

31
Q

What is the charge of a non-metal ion?

A

Negative (Gaining Electrons)

32
Q

What is the charge of a metal ion?

A

Positive (Lose Electrons)

33
Q

Uses of fullerene:

A
  • Catalysts
  • Reinforcements for composite material
  • In drugs
34
Q

What is graphene?

A

A single layer of graphite

35
Q

What is the formula for buckminister fullerene?

A

C60

36
Q

How can graphite conduct electricity?

A

Because delocalised electrons cam move through it’s layers

37
Q

What makes metals malleable?

A

Layers of atoms in a metal can slide over

38
Q

Why is graphite a good electrical conductor?

A

Only three electrons per carbon atom is used in covalent bonds so one electron is delocalised. These delocalised electrons can move through the whole structure carrying an electrical charge

39
Q

Why is graphite soft and slippery?

A

It’s particles are in fixed layer with weak intermolecular forces between them.
This allows the layers to slide across each other easily.

GCSE AQA Chemistry Flashcards (15 decks)

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