Chapter 6 - Shapes of molecules and intermolecular forces Flashcards

1
Q

What is the electron-pair repulsion theory?

A

Used to predict shapes of molecules or ions
Electron pairs repel each other so they are as far apart as possible
Lone pairs repel more than bonding pairs

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2
Q

What is bond length?

A

Distance between the nuclei of the two bonded atoms

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3
Q

What is bond angle?

A

Angle between two covalent bonds

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4
Q

Describe the linear shaped molecule.

A

EP - 2
BP - 2
LP - 0
180°
e.g. CO2

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5
Q

Describe the trigonal planar shaped molecule.

A

EP - 3
BP - 3
LP - 0
120°
e.g. BF3

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6
Q

Describe the non-linear shaped molecules.

A

EP - 3
BP - 2
LP - 1
119°
e.g. SO2

OR

EP - 4
BP - 2
LP - 2
104.5°
e.g. H2O

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7
Q

Describe the tetrahedral shaped molecule.

A

EP - 4
BP - 4
LP - 0
109.5°
e.g. CH4

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8
Q

Describe the pyramidal shaped molecule.

A

EP - 4
BP - 3
LP - 1
107°
e.g. NH3

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9
Q

Describe the trigonal bipyramidal molecule.

A

EP - 5
BP - 5
LP - 0
90° and 120°
e.g. PF5

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10
Q

Describe the octahedral molecule.

A

EP - 6
BP - 6
LP - 0
90°
e.g. SF6

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11
Q

Describe the distorted square pyramid molecule.

A

EP - 6
BP - 5
LP - 1
89°
e.g. ClF5

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12
Q

Describe the square planar molecule.

A

EP - 6
BP - 4
LP - 2
90°
e.g. XeF4

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13
Q

What is electronegativity?

A

The ability of an atom to attract the bonding electrons in a covalent bond

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14
Q

Which element has the highest electronegativity and why?

A

Fluorine
Small atomic radius (less repulsion)
Low electron shielding (less repulsion)
Relatively high nuclear charge to outweigh the others to attract the electrons

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15
Q

What is a polar bond?

A

Then the electron pair is shared unequally between the bonded atoms due to a difference in electronegativity
Making there permanent dipoles with partially positive/negative charges on each end.

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16
Q

How can you determine whether a molecule is bonded ionically or covalently?

A

Electronegative difference
<1.8 = covalent bond
> 1.8 = ionic bond

17
Q

What is a polar molecule?

A

Polar bonds need to reinforce each other in into one direction to create poles
If they cancel each other out then they are no longer polar
Just because a molecule has polar bonds doesn’t make it a polar molecule

18
Q

What are intermolecular forces?

A

Weak interactions between dipoles of different molecules.

19
Q

What are the three types of intermolecular forces?

A

Induced dipole-dipole forces (London forces)
Permanent dipole-dipole forces
Hydrogen bonding

20
Q

Describe induced dipole-dipole forces.

A

Between all molecules
Movement of electrons in a molecule is random meaning an instantaneous dipole can form which will induce a force upon a neighboring molecule, therefore attraction each other and forming intermolecular forces
Relatively weakest of the intermolecular forces

21
Q

Describe permanent dipole-dipole forces.

A

Occurs in polar molecules
Stronger than London forces in the same molecule

22
Q

Describe hydrogen bonding.

A

Special permanent-permanent dipole force
Must involve an electropositive hydrogen and an electronegative O, N or F
The electronegative atom must have a lone pair
Strongest type of intermolecular force

23
Q

Describe the anomalous trends of water.

A

Solid state is less dense than the liquid state - hydrogen bonding holds the molecules apart in the lattice structure
Relatively high melting and boiling point - hydrogen bonding is stronger than London forces so it has higher energy required compared to similar molecules

24
Q

What are the simple molecular lattices?

A

Solid structures made up of simple molecules
e.g. Iodine
Molecules held together by weak intermolecular forces
Atoms in a molecules held together by strong covalent bonds

25
Q

Why do simple molecular substances have low boiling/melting points?

A

Weak intermolecular forces

26
Q

What is the solubility of non-polar simple molecular substances?

A

Soluble in non-polar substances - Intermolecular forces form between the two substances and these weaken the IMFs in the simple molecular substance and it dissolves into the solvent
Insoluble in polar substances - Very little interactions with each other

27
Q

What is the solubility of polar simple molecular substances?

A

Solubility depends on the strength of the dipoles
Many do dissolve in both polar and non-polar substances as they attract each other

28
Q

What is the electrical conductivity of simple molecular substances?

A

No mobile charged particles therefore there is nothing to complete an electrical circuit
They do not conduct electricity