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Chemistry > Bonding, Structure, and the Properties of Matter (C1-2) > Flashcards

Bonding, Structure, and the Properties of Matter (C1-2) Flashcards

and atomic structure / the periodic table

1
Q

Describe Rutherford’s particle scattering experiment

A
  • He fired alpha particles at thin gold foil in a vacuum
  • Most particles passed through
  • Some were deflected as they passed through
  • Few were deflected straight back
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2
Q

What did Rutherford’s experiment help him discover?

A
  • Most of the atom is empty space
  • Dense, positively charged nucleus
  • Mass concentrated at the centre
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3
Q

What did Niels Bohr discover?

A

That electrons orbit the nucleus at specific distances (energy levels)

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4
Q

In what order were the three subatomic particles discovered?

A
  1. Electron
  2. Proton
  3. Neutron
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5
Q

What did James Chadwick discover?

A

Neutrons

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6
Q

Explain Mendeleev’s periodic table

A
  • Ordered by atomic weights (didn’t account for isotopes)
  • Left gaps for undiscovered elements
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7
Q

Explain the modern periodic table

A
  • Ordered by relative atomic mass
  • Gaps filled in
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8
Q

Name the properties of metals

A
  • Good conductors
  • Malleable
  • Dense
  • High melting points
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9
Q

What is ionic bonding between?

A

Between oppositely charged ions

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10
Q

What is covalent bonding between?

A

Between two non-metals

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11
Q

What is metallic bonding between?

A

Between metals / alloys

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12
Q

How are ionic compounds held together?

A

Strong electrostatic forces

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13
Q

Why does ____ conduct electricity?

A

Delocalised electrons that are free to move across the structure

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14
Q

Describe the properties of giant covalent structures

A
  • High melting points
  • Insoluble
  • Hard
  • Electrical insulators
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15
Q

Describe the properties of giant ionic lattices

A
  • High melting points
  • When (aq) or (l), can conduct electricity as ions are free to move so charge can flow
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16
Q

Describe the bonding of small molecules

A
  • Strong covalent bonds hold atoms in a molecule together
  • Weak intermolecular forces hold molecules together
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17
Q

Describe the properties of small molecules

A
  • Low melting points
  • Electrical insulators
  • Melting points increase dependent on size of molecules
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18
Q

Describe the bonding in polymers

A
  • Atoms covalently bonded
  • Molecules are held together by relatively strong intermolecular forces (solid at RTP)
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19
Q

Why are alloys harder than pure metals?

A
  • In pure metals, atoms are arranged in layers, so they can slide over each other easily
  • In alloys, atoms of the other element disrupt these layers, stops sliding
20
Q

Describe the structure and bonding of graphite

A
  • Arranged in layers held together by weak intermolecular forces
  • Atoms in layers covalently bonded
  • Delocalised electrons (each carbon has 3 bonds and 4 electrons)
21
Q

What is graphene used for?

A

Electronics

22
Q

What are fullerenes used for?

A

Electronics, material, and medicine

23
Q

What are nanoparticles?

A
  • Particles 1-100nm in size
  • High surface area to volume ratio
24
Q

What are nanoparticles used for?

A

Medicine
Electronics
Sun cream
Deodorant

25
Q

What is a compound?

A

Two or more chemicals chemically combined in fixed proportions

26
Q

Describe the Bohr model and how it came about

A

Electrons orbit the nucleus at specific distances
Came from alpha scattering experiment

27
Q

Who discovered neutrons?

A

James Chadwick

28
Q

What is the radius of an atom?

A

0.1 nm

29
Q

How do you convert nm to mm?

A

1 nm = 0.000001 mm
1 mm = 1,000,000 nm

30
Q

What is the radius of a nucleus?

A

1 x 10^-14 m

31
Q

How much of an atom does the nucleus make up?

A

1/10000

32
Q

Do isotopes of an element have the same chemical properties?

A

Yes, because their electronic structure is the same

33
Q

How do calculate relative atomic mass (from abundance)

A

(Mass x Abundance) + (Mass x Abundance) / 2

34
Q

What happens to electrons in metallic bonding?

A

Delocalised electrons are shared

35
Q

What happens to electrons in covalent bonding?

A

They are shared

36
Q

What happens to electrons in ionic bonding?

A

They are given away

37
Q

Describe three properties of alkali metals

A
  • Soft
  • Low density
  • 1 electron in outer shell
38
Q

Alkali + Water –> ??

A

Salt + Hydrogen

39
Q

How does boiling point change going down group 0?

A

Increases

40
Q

How are ionic lattices held together?

A

Electrostatic forces

41
Q

What are some properties of ionic compounds?

A

High boiling points
Don’t conduct electricity except when in molten or aqueous form

42
Q

What are nanotubes?

A

Allotrope of carbon,

43
Q

What are fullerines?

A

Hollow shaped molecules
E.g. Buckminsterfullerene

44
Q

How big are nanoparticles?

A

1-100 nm

45
Q

How big are fine particles?

A

100-2500 nm

46
Q

How big are coarse particles?

A

1 x 10^-5 m and above

Chemistry (6 decks)

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