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Chemistry - Miss Nichols > 3.1 - 3.7 Bonding > Flashcards

3.1 - 3.7 Bonding Flashcards

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1
Q

What is an ionic bond?

A

The electrostatic attraction between oppositely charged ions

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2
Q

Positive ion

A

Cation

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3
Q

Negative ion

A

Anion

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4
Q

What is a covalent bond?

A

A shared pair of electrons. The electron pair is attracted to both nuclei so resist separation.

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5
Q

What is a co-ordinate bond?

A

A covalent bond where both electrons in the shared pair originate from the same atom

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6
Q

What is metallic bonding?

A

The attraction between positive metal atoms and the surrounding delocalised sea of electrons

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7
Q

What is electronegativity?

A

The power of an atom to attract the pair of electrons in a covalent bond

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8
Q

Nuclear charge up = electronegativity ?

A

Electronegativity up

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9
Q

Atomic radius up = shielding ? = electronegativity ?

A

Shielding up = electronegativity down

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10
Q

What is used to measure electronegativity?

A

The Pauling scale

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11
Q

What happens to electronegativity across a period?

A
  • Increases
  • Same no. of energy levels BUT
  • Increasing no. of protons/nuclear charge
  • Decreasing atomic radius
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12
Q

What happens to electronegativity up a group?

A
  • Increases
  • Fewer energy level in use
  • Less shielding
  • Decreasing atomic radius
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13
Q

What is a polar molecule?

A

One in which the electron density across the whole molecule is unevenly distributed

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14
Q

What is a permanent dipole?

A

When one side of the molecule is permanently more negative, happens when a molecule is not symmetrical

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15
Q

What are the 3 main types of inter-molecular forces?

A
  • Dipole-dipole interactions
  • Hydrogen bonding
  • Van der Waal’s forces
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16
Q

What are dipole-dipole interactions?

A
  • Attractive forces between polar molecules

- Whatever their starting position, molecules will ‘flip’ to attract

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17
Q

What are hydrogen bonds?

A
  • Not a bond, an inter-molecular force

- Only takes place when H bonded to O, F or N with at least one lone pair

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18
Q

What are Van der Waal’s forces?

A
  • Also known as temporary dipole-induced dipole interactions
  • Caused by the movement of electrons so the more electrons there are the stronger the force
  • Exist between all molecules at all times, in addition to any other forces
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19
Q

List the three main inter-molecular forces from weakest to strongest

A
  • Van der Waal’s
  • Dipole-dipole
  • Hydrogen bonding
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20
Q

Describe the particles in a solid

A

Regular, close, vibrate about a fixed position

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21
Q

Describe the particles in a liquid

A

Random, close, can move past each other

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22
Q

Describe the particles in a gas

A

Far apart, rapid and random motion

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23
Q

What is the name for the energy required to boil a liquid?

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A

Enthalpy of vaporisation

24
Q

What is the name for the energy required to melt a solid?

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A

Enthalpy of fusion

25
What are the four types of crystal structure?
- Ionic - Metallic - Molecular (simple covalent) - Macromolecular (giant covalent)
26
What is an ionic crystal?
Positive and negative ions held together in a giant ionic lattice by strong electrostatic attraction between oppositely charge ions
27
Describe and explain the melting points of ionic compounds
- High | - Strong electrostatic attraction between oppositely charged ions
28
Describe and explain the electrical conductivity properties of ionic compounds
- Does not conduct when solid - No ions (charged particles) free to move - Does conduct when molten or in solution - Ions free to move and carry charge
29
Describe and explain the physical properties of ionic compounds
- Hard but brittle | - A force can move the ions and produce contact between like charges causing them to repel
30
Describe and explain the solubility of ionic compounds
- Often dissolve in water | - Ions become solvated and surrounded by water molecules
31
What is a metallic crystal?
A giant lattice of positive ions held together by a sea of delocalised electrons
32
Describe and explain the melting points of metals
- High melting and boiling points | - Strong electrostatic attraction between metal ions and delocalised sea of electrons
33
Describe and explain the electrical conductivity of metals
- Conduct in all states | - Delocalised electrons free to move and carry charge
34
Describe and explain the physical properties of metals
- Malleable and ductile | - Metal ions can slide past each other while retaining their lattice structure and metallic properties
35
Describe and explain the solubility of metals
- Insoluble in water | - Metallic bonds are too strong for water so overcome so metal ions cannot become solvated
36
What is a molecular crystal?
Individual molecules held together by weak intermolecular forces
37
Describe and explain the melting points of molecular solids
- Low melting points | - Weak intermolecular forces (VDW) do not require much energy to overcome
38
Describe and explain the physical properties of molecular solids
- Soft and easily breakable | - Weak intermolecular forces (VDW) do not require much energy to overcome
39
Describe and explain the electrical conductivity of molecular solids
- Never conduct electricity | - No charged particles free to move
40
What is a macromolecular crystal?
A giant arrangement of atoms joined by covalent bonds
41
Describe and explain the melting point of diamond
- Very high (3,000C +) | - Strong covalent bonds require a lot of energy to break
42
Describe and explain the physical properties of diamond
- Very hard | - Strong covalent bonds require a lot of energy to break
43
Describe and explain the melting point of graphite
- Very high (3,000C +) | - Strong covalent bonds require a lot of energy to break
44
Describe and explain the physical properties of graphite
- Soft, flaky and slippery | - Layers slide over each other because of delocalised electrons between layers
45
Describe and explain the electrical conductivity of graphite
- Conducts electricity | - Delocalised electrons free to move and carry charge
46
How does the bond angle change when a molecule's loan pair forms a hydrogen bond?
- Increases - Loan pair more like bonding pair so does not repel so strongly
47
How can electronegativity values be used to predict whether a given chloride is likely to be ionic or covalent?
Large difference in electronegativity = Ionic | Small difference in electronegativity = Covalent
48
Explain the formation of hydrogen bonding between protein molecules
- C=O and N-H bonds are polar - O more electronegative than C, N more electronegative than H - H-bonding between Hpartial+ and Opartial- of different molecules - Using lone pair of electrons from oxygen
49
Why does the boiling point of fluorine compounds not fit into other trends?
- Unexpectedly high - Due to hydrogen bonding - Caused by large differences in electronegativity of fluorine and other element
50
Give an equation for a reaction in which a co-ordinate bond is formed
NH₃ + H⁺ → NH4⁺
51
Why is aluminium chloride covalent rather than ionic?
- Smaller electronegativity difference | - So more equal sharing
52
How do you know if two atoms will bond ionically of covalently?
Ionic = Big electronegativity difference Covalent = Small electronegativity difference
53
How does hydrogen bonding work?
Hpartial+ attracted to lone pair of another partially negative molecule
54
Define polar bond
A bond where the bonding pair is shared unequally
55
Why does a lone pair of electrons repel more strongly than a bonding pair?
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Chemistry - Miss Nichols (17 decks)

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