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Chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

Define electronegativity

A

Electronegativity is a measure of the tendency of an atom to attract electrons towards itself

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2
Q

Factors affecting electronegativity (3)

A

1) Nuclear charge
2) Shielding
3) Atomic radius

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3
Q

Explain the trends of electronegativity down a group and across a period

A

Electronegativity decreases down the group as atomic radius increases and shielding effect increases.
Electronegativity increases across a period as nuclear charge increases and shielding effect is almost the same. Atomic radius decreases

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4
Q

Using Pauling’s electronegativity values, what will it be when it is non-polar covalent?

A

Less than 0.4

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5
Q

Using Pauling’s electronegativity values, what will it be when it is polar covalent?

A

Between 0.4 and 1.7

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6
Q

Using Pauling’s electronegativity values, what will it be when it is ionic?

A

Greater than 1.7

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7
Q

Define ionic bonding

A

Ionic bonding consists of strong electrostatic forces of attraction between cations and anions

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8
Q

Define metallic bonding

A

Strong electrostatic forces between cations and delocalised electrons

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9
Q

Define covalent bonding

A

Strong electrostatic forces of attraction between the nucleus of an atom towards the electrons of another atom

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10
Q

What should we keep in mind when covalent bonding occurs for elements of period 3 and above?

A

Third row elements and above can use their empty d orbitals for bonding. Hence they can have more than 8 electrons in their outermost shell

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11
Q

When does coordinate (dative) bonding occur?

A

Dative covalent bond occurs when both electrons in the covalent bond are provided by the same atom

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12
Q

What causes sigma bond?

A

The head-on overlapping of orbitals

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13
Q

What causes the pi bond?

A

The sideways overlapping of p orbitals

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14
Q

Why can we not rotate a molecule about a pi bond?

A

Rotation is not possible as the overlap of orbitals is above and below the plane of the molecule

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15
Q

Define hybridisation

A

Hybridisation is the mixing of atomic orbitals

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16
Q

Shape and bond angle for molecule with 2 negative centres

A

Linear. 180º

17
Q

Shape and bond angle for molecule with 3 negative centres

A

Trigonal planar. 120º

18
Q

Shape and bond angle for molecule with 3 negative centres one being a lone pair

A

Non- linear. 118º

19
Q

Shape and bond angle for molecule with 4 negative centres

A

Tetrahedral. 109.5º

20
Q

Shape and bond angle for molecule with 4 negative centres one being a lone pair

A

Trigonal pyramidal. 107.5º

21
Q

Shape and bond angle for molecule with 4 negative centres two being a lone pair

A

Non-linear. 104.5º

22
Q

Shape and bond angle for molecule with 5 negative centres

A

Trigonal bipyramidal. 120º and 90º

23
Q

Shape and bond angle for molecule with 6 negative centres

A

Octahedral. 90º

24
Q

What are the different types of VDW forces?

A

1) Instantaneous dipole - induced dipole attraction
2) Permanent dipole - permanent dipole attraction
3) Hydrogen bonding

25
Q

What type of IMF is present in non-polar molecules?

A

Id-id

26
Q

Describe the IMF id-id

A

Electrons found in a molecule are in constant movement. This causes temporary dipoles on the molecule. These temporary dipoles induces a dipole on adjacent molecules and this induces further dipoles on other molecules. The id-id force is very weak and non-permanent

27
Q

What is the strength of the id-id proportional to?

A

The strength of id-id of forces is directly proportional to the number of electrons

28
Q

Describe the IMF pd-pd

A

An IMF attraction present between molecules that have a permanent dipole. Stronger than id-id

29
Q

What is the strength of the dipole dependant on?

A

1) The differences in electronegativities of atoms in the molecule
2) The distribution of electronegative atoms in the molecule

30
Q

Describe hydrogen bonding

A

A hydrogen bond is an IMF present between molecules having a H atom directly bonded to a very electronegative atom like N, O or F (a type of permanent bond)

31
Q

Why are some substances miscible while others are not?

A

Substances can mix with or dissolve in other substances if they have similar types of bonding

32
Q

Effects of H-bonding (4)

A

1) Hydrides of O, N and F have anomalously high melting and boiling points
2) Surface tension. A ‘film’ on the surface of a liquid that resists force
3) Ice has a lower density than liquid water. In the solid form, water molecules arrange themselves in an ‘open’ lattice structure that allows H-bonding

Chemistry (19 decks)

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