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Chemistry (Triple) > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

What are the three ways atoms can chemically bond?

A
  • Ionic bonding
  • Metallic bonding
  • Covalent bonding
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2
Q

What is ionic bonding?

A

Ionic bonding involves an attraction between oppositely charged ions. Ionic bonds are found in compounds made of metals and non-metals.

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3
Q

What is covalent bonding?

A

Covalent bonding involves 2 atoms sharing one or more pairs of electrons. Covalent bonds are found in most non-metals elements and in non-metal compounds.

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4
Q

What is metallic bonding?

A

Metallic binding involves am attraction between positively charged ions and negatively charged delocalised electrons. Metallic bonds are found in metald and alloys.

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5
Q

What are ions?

A

Ions are particles that have a charge, they are created when an atom or molecule gains or loses electrons.

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6
Q

What are cations and how are they formed?

A

Cations are positive ions usually created when an atom/molecule loses electrons. They are most likely to be group 1 and 2 metals.

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7
Q

What are anions and how are they formed?

A

Anions are negative ions that are usually created when at atom/molecules gains electrons. Non-metals in group 7 are most likely to become negatively charged.

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8
Q

How are ionic lattices formed?

A

Ionic compounds form giant structures called ionic lattices that are held together by strong electrostatic forces of attraction between positive and negative ions.

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9
Q

What are the different types of covalent bonding?

A
  • Single covalent bond
  • Double covalent bond
  • Triple covalent bond
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10
Q

What are the differences of single covalent bonds compared to double and triple covalent bonds?

A

Triple covalent bonds are stronger and require more energy to break

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11
Q

What are the 3 different states of matter?

A

Solid, liquid, gas

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12
Q

What are the properties of a solid?

A
  • Particles are very close together and vibrate in a fixed position.
  • When heated, the particles vibrate more intensely
  • Solids have a fixed shape and volume
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13
Q

What are the properties of a liquid?

A
  • Particles are very close together but can move and flow past each other.
  • Liquids have a fixed volume but can change shape.
  • When heated, the average speed of particles increase.
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14
Q

What are the properties of a gas?

A
  • Particles are far apart and move randomly in all directions.
  • Gases can change shape and volume.
  • When heated, the average speed of particles increase.
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15
Q

What are the different processes of a substance changing state?

A

Melting - Solid to liquid
Boiling - Liquid to gas
Freezing - Liquid to solid
Condensing - Gas to liquid
Sublimation - Solid to gas
Deposition - Gas to Solid

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16
Q

What is aqueous?

A

Aqueous are substances dissolved in water.

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17
Q

What are the properties of ionic compounds?

A
  • High melting/boiling points
  • Don’t conduct electricity if solid
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18
Q

What are intermolecular forces?

A

Intermolecular forces are forces between different molecules.

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19
Q

Why do covalent molecules have low melting and boiling points?

A

Covalent molecules have weak intermolecular forces which are easy to break.

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20
Q

What are intramolecular forces?

A

The strong covalent bonds found within small molecules.

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21
Q

What does the size of a molecule affect overall?

A

The overall strength of intermolecular forces.

22
Q

What is graphite?

A

Graphite is a giant covalent structure that has a higher melting point that methane.

23
Q

Why does graphite have a higher boiling point than methane?

A

It requires you to break covalent bonds, rather than weak intermolecular forces.

24
Q

What are polymers?

A

Polymers are large, chain-like molecules that can extend for thousands of atoms.

25
Q

How are polymers held together?

A
  • Strong covalent bonds between atoms in molecules.
  • Weak intermolecular forces between molecules.
26
Q

What does the ‘n’ tell us in a repeat unit of poly(propene)?

A

How many times the unit is repeated to give the polymer.

27
Q

What are some properties of giant covalent structures?

A
  • No specific formula
  • Very high melting points
  • 1 Large molecule
28
Q

What are pure metals?

A

Pure metals have giant structures with strong electrostatic forces between positive ions and delocalised electrons.

29
Q

What are the properties of pure metal?

A
  • Soft / malleable
  • High melting / boiling points
30
Q

What is the structure of a diamond?

A

A diamond is a giant covalent structure, a small diamond can contain 50,000 carbon atoms, where a larger diamond could contain 1,000,000,000 carbon atoms.

31
Q

What is an alloy?

A

An alloy is a combination of 2+ elements where at least one is metal.

32
Q

What are the properties of alloys?

A
  • Mixture of 2+ elements
  • Layers are distorted
  • Harder than pure metals
33
Q

What are allotropes?

A

Allotropes are different forms of the same element e.g. diamond, graphite.

34
Q

What are the properties of diamond?

A
  • Diamond does not conduct electricity.
  • Every carbon atom in diamond is bonded to 4 other carbon atoms by strong covalent bonds.
  • Diamond is hard
  • Diamond has a high melting point.
35
Q

What are the properties of graphite?

A
  • Every carbon atom is graphite is bonded to 3 other carbon atoms by strong covalent bonds.
  • Graphite is soft.
  • Graphite conducts electricity.
36
Q

What are the properties of graphene?

A
  • Graphene conducts electricity
  • Graphenes are light but strong
  • Graphenes are 1 atom thick
37
Q

What are fullerenes?

A

Fullerenes are molecules of carbon atoms that take up hollow structures. Their structure is usually carbon atoms arranged in hexagonal rings (pentagonal and heptagonal carbon rings can be found).

38
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene

39
Q

What are the common uses for spherical fullerenes?

A
  • Catalysts
  • Lubricants
  • As vehicles for transporting drugs into our bodies
40
Q

What are carbon nanotubes?

A

Carbon nanotubes are fullerenes that take the shape of a cylinder, often called molecular wires because they have a tiny diameter but incredibly long.

41
Q

How strong are cylindrical fullerenes?

A

Because of the strong covalent bonds between carbon atoms, nanotubes are exceptionally strong for their size.

42
Q

What are the common uses for cylindrical fullerenes?

A
  • In electronics
  • In nanotechnology
  • For strengthening materials
43
Q

What is the formula for buckminsterfullerene?

A

C60

44
Q

How big is a nanoparticle?

A

1 - 100 nm long
10 - 1000 atoms

45
Q

How big are fine particles?

A

100 - 2500 nm long
1000 - 25000 atoms

46
Q

How big are coarse particles (dust)?

A

2,500 - 10,000 nm long
25,000 - 100,000 atoms

47
Q

What are nanoparticles?

A

Nanoparticles are tint particles between 1 - 100 nm in length. They are larger than individual atoms but too small to be seen with the human eye.

48
Q

How does the use of nanoparticles compare to that of larger particles?

A
  • Less expensive
  • More efficient
49
Q

How would you describe the surface area to volume ratio of nanoparticles?

A

Extremely high

50
Q

What are the main uses of nanoparticles?

A
  • Catalysts
  • Cosmetics
  • Medicine
  • Electronics
  • Deodorants

Chemistry (Triple) (7 decks)

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