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

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

1
Q

What is ionic bonding?

A

lonic bonding is the electrostatic attraction between positive and negative ions.

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2
Q

How are ionic compounds held together?

A

• They are held together in a giant lattice.

• It’s a regular structure that extends in all directions in a substance.

• Electrostatic attraction between positive and negative ions holds the structure together.

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3
Q

State properties of ionic substances

A

• High melting and boiling point (strong electrostatic forces between oppositely charged ions)

• Do not conduct electricity when solid (ions in fixed positions).

• Conduct when molten or dissolved in water - ions are free to move.

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4
Q

Give 5 examples of positive ions

A

E.g. Positive: Nat, Mg^2+, Al^3+, Ca^2+, Rb+.

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5
Q

.

A

.

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6
Q

How are ionic compounds formed? Explain in terms of MgO case.

A

Reaction of a metal with a non-metal.
Electron transfer occurs - metal gives away its outer shell electrons to non-metal.

Mg is in Group Il, so has 2 available outer shell electrons.

O is in Group VI, so can accept 2 electrons to get a full outer shell configuration.

Mg becomes Mg land O becomes O2- (oxide).

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7
Q

What is a covalent bond?

A

Covalent bond is a shared pair of electrons between two atoms.

(Non metal)

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8
Q

Describe the structure and properties of simple molecular covalent substances

A
  • Do not conduct electricity (no ions)
  • Small molecules
  • Weak intermolecular forces, therefore:
  • Low melting and boiling points
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9
Q

How do intermolecular forces change as the mass/size of the molecule increases?

A

They increase. That causes melting/boiling points to increase as well (more energy needed to overcome these forces).

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10
Q

What are polymers?

A

Polymers are very large molecules (>100s, 1000s of atoms) with atoms linked by covalent bonds.

Poly- many

Mer- Repeating unit

Polymer long string like structures

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11
Q

What is thermosofeting polymers

3 things

A

Thermosoftening polymers - special type of polymers; they melt/soften when heated.

There are no bonds between polymer chains. Strong intermolecular forces ensure that the structure is solid at room temperature.

These forces are overcome with heating - polymer melts.

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12
Q

What are giant covalent substances?Give examples

A
  • Solids, atoms covalently bonded together in a giant lattice.
  • High melting/boiling points - strong covalent bonds.
  • Mostly don’t conduct electricity (no delocalised e)
  • Diamond, graphite, silicon dioxide.
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13
Q

Properties of diamond

(4)

A
  • four, strong covalent bonds for each carbon atom
  • very hard (Strong bonds)
  • very high melting point (strong bonds)
  • does not conduct (no delocalised electrons)
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14
Q

Propierties of Graphite

A

three covalent bonds for each carbon atom
- layers of hexagonal rings

  • high melting point
  • layers free to slide as weak intermolecular
    forces between layers; soft, can be used as a lubricant
  • conduct thermal and electricity due to one delocalised electron per each carbon atom
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15
Q

Properties of fullernes

A
  • hollow shaped molecules
  • based on hexagonal rings but may have
    5/7-carbon rings
  • C(small)6o has spherical shape, simple molecular structure (Buckminsterfullerene)
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16
Q

Properties of Nanotubes

A
  • cylindrical fullerene with high length to diameter ratio

High tensile strength (strong bonds)

Conductivity (deloc. electrons)

17
Q

Properyies of Graphene

A
  • a single layer of graphite.
18
Q

What is metallic bonding?

A

Forces of attraction between delocalised electrons and nuclei of metal ions.

19
Q

Describe properties of metals

A
  • High melting/boiling points (strong forces of attraction)
  • Good conductors of heat and electricity (delocalised electrons)
  • Malleable, soft (layers of atoms can slide over each other whilst maintaining the attraction forces)
20
Q

What are alloys?Why are they harder than pure metals?

A

Alloys:
- mixtures of metal with other elements, usually metals

The smaller or bigger atoms distort the layers of atoms in the pure metal. This means that a greater force is required for the layers to slide over each other

21
Q

What does the amount of energy needed to change state from solid to liquid or liquid to gas depend on?

(3 points)

A

The strength of the forces between the particles of the substance.

The nature of the particles involved depends on the type of bonding and the structure of the substance.

The stronger the forces between the particles the higher the melting point and boiling point of the substance

22
Q

A pure substance will melt or boil at..? What about the mixture?

A

A fixed temperature.

A mixture will melt over a range of temperatures.

23
Q

What are the three states of matter?

A

Solid, liquid and gas

24
Q

What is nanoscience?

A

Science that studies particles that are 1 - 100nm in size

25
Q

State the uses of nanoparticles

A
  • Medicine (drug delivery systems)
  • Electronics
  • Deodorants
  • Sun creams (better skin coverage and more effective protection against cell damage)
26
Q

What are fine and coarse particles?

A
  • Fine particles (soot), 100-2500 nm diameter
  • Coarse particles (dust), 2500 to 10,000 nm diameter
27
Q

Why do nanoparticles have different properties to those for the same materials in bulk?

A

High surface area to volume ratio

28
Q

What is relatively a strong attraction

A

Ionic bonding

29
Q

Give 5 examples of negative ions

A

Negative: Cl−, Br−, SO 2−, NO −, OH− (chloride, bromide, sulfate, nitrate, 43
hydroxide).

30
Q

What is important when working out a formula of
an ionic compound?

A

Ionic compounds are electrically neutral, i.e. positive and negative charges balance each other.

31
Q

What is important when working out a formula of
an ionic compound?

A

Ionic compounds are electrically neutral, i.e. positive and negative charges balance each other.

32
Q

What are the allotropes of carbon

5

A

Diamond

Fullerenes

Graphite

Nanotubes

Grapheme(a single layer of graphite)

33
Q

Why are alloys harder than pure metals?

A
  • different sizes of atoms distorts the layers, so they can’t slide over each other, therefore alloys are harder than pure metals
34
Q

What is a Buckminsterfullerne molecule also known as

A

A bucky ball

Ball/Sphere shape

35
Q

What should you do if the units aren’t the same

A

Insure units are the same for instance if have a volume of ..cm^3 and … g/dm^3

Divide by 1000

36
Q

What do nano particels have more of than coarse particels

A

Nano particels have a greater surface area to volume ratio than coarse particels

Chemistry (10 decks)

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