C3 - Structure and Bonding Flashcards

1
Q

States of matter: Solids

A

Solids have a fixed shape and volume, are packed and vibrate.

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2
Q

States of matter: Liquids

A

Liquids also have a fixed volume but they can flow and change their shape, they are packed and slide over one another.

closely spaced but still in constant motion and therefore are constantly colliding

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3
Q

States of matter: Gases

A

Gasses have no fixed shape or volume, can be compressed easily and have lots of space and so can move randomly in all directions.

widely spaced and in constant motion. Collisions are frequent and elastic

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4
Q

Physical Changes: How to get from one state to another

A
solid to liquid: melting
liquid to gas: evaporating/boiling 
gas to liquid: condensing
liquid to solid: freezing
solid to gas: sublimation
gas to solid: deposition

 Melting and boiling – energy transferred from surroundings
 Freezing and condensation – energy transferred to surroundings.

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5
Q

Limitations of the particle model

A

– atoms, molecules and ions are not all the same shape and size,
atoms are mainly empty space and not solid.

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6
Q

How do atoms become ions and types of bonding

A

atoms either lose or gain electrons to have full outer shells so they are stable.

Ionic bonding = transferring electrons
Covalent Bonding = sharing electrons

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7
Q

Ionic Bonds

A
  • strong electrostatic attraction between oppositely charged ions, thse forces act in all directions in the lattice forming a giant structure/ lattice
  • compound formed when metals react with non-metals
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8
Q

Ionic compound properties

A

Ionic compounds have high melting and boiling points, as the strong electrostatic attractions are hard to overcome.

When in molten or in solution, ionic compounds can conduct electricity as the lattice breaks apart and ions can carry charge.

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9
Q

Covalent Bonds

A
  • compounds formed when non-metals react with non-metals
  • many covalent compounds consist of small molecules e.g. water
  • strong covalent bonds but weak intermolecular forces
  • simple molecules have no overall charge so they don’t carry electricity
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10
Q

Giant covalent structure

A

huge network of atoms connected by strong covalent bonds

  • high mpt and bpt
  • insoluble in water
  • hard
  • do not conduct electricity except graphite
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11
Q

Comment on the Melting point curve

A

A pure solid will melt at a fixed temperature and the line will stay horizontal when it is melting.

The temperature does not rise when the solid is melting because the heat is absorbed to break the bonds between the solid particles.

The temperature will start to rise again when all the solid has melted.

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12
Q

Empirical formula

A

The empirical formula is the simplest ratio of ions in a compound.

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13
Q

Intermolecular force

A

force of attraction between molecules. These forces increase with the size of the molecules, so larger molecules have higher melting and boiling points.

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14
Q

Polymers

A

they are made up of a long chain of molecules so there are more intermolecular forces, and higher melting/ boiling points than in smaller molecules.

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15
Q

Model of Graphite and properties

A

Graphite has giant hexagonal layers with weak intermolecular forces. The layers can slide over each other.
Since each carbon atom only forms 3 covalent bonds in each layer this leaves 1 electron which moves freely in between the layers of carbon.
Due to this spare delocalised electron graphite can conduct electricity and heat.

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16
Q

Fullerenes and uses

A

hollow-shaped molecules of carbon
uses:
drug delivery in bodies, lubricants and catalysts.

17
Q

Properties of carbon nanotubes (cylndrical fullerenes )

A
  • high tensile strength (used in tennis rackets)

- high electrical and heat conductivity

18
Q

Graphene

A

one atom-thick layer of graphite
- excellent electricity and heat conductivity,
- low density,
- reactive,
- strong
These properties will help create new developments in the electronics industry in the future.

19
Q

Metallic bonding

A

electrostatic attraction between metal ion and delocalised electron.

The strength of Metallic bonds = Mg2+ woul

20
Q

Alloy

A

a mixture of two or more elements, at least one of which is a metal. They are harder than pure metals as the differently sized atoms to the metal distort the orderly layers.

21
Q

Properties of metals

A
  • malleable (due to the delocalised electrons allowing the metal atoms to slip past one another),
  • ductile,
  • high melting point (due to their giant structures),
  • high conductivity (due to the sea of delocalised electrons).
22
Q

Nanoparticles

A

part of Nanoscience (the study of small particles 1-100nm in size)

high SA:V and many atoms are exposed at the surface.

23
Q

Uses of Nanoparticles

A
Glass coating
Sunscreens
Cosmetics
Drug delivery
material reinforcement
antibacterial coating
24
Q

Risks of nanoparticles

A

breathing in tiny particles could damage one’s lungs,
many catalysts can cause explosions,
and they can accumulate in organisms over time.

25
Q

Properties of diamond

A

n diamond, each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure, so diamond is very hard, has a very high melting point and does not conduct electricity.

26
Q

Difference between Pure metal and alloy

A

In pure metals, the atoms are all the same size. The layers of atoms are able to slide over each other. This means metals can be bent and shaped. Most metals in everyday use are alloys. Purecopper, gold, iron and aluminium are too soft for many uses and so are mixed with other metals to make alloys.The different sizes of atoms in an alloy distortthe layersin the structure, making it more difficult for them to slide over each other, so alloysare harder than pure metals