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My Chemistry > Shapes of molecules and intermolecular forces > Flashcards

Shapes of molecules and intermolecular forces Flashcards

1
Q

What is the shape and bond angle in methane?

A

Tetrahedral and 109.5°

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2
Q

Why do lone pairs have higher repulsion than bonded pairs?

A

The lone pair is slightly closer to the central atom and occupies more space

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3
Q

What is the bond angle?

A

The angle between the bonded pairs of electrons

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4
Q

What is the shape and bond angle of NH3?

A

Pyramidal and 107°

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5
Q

What is the shape and bond angle of water?

A

Non-linear (bent) 104.5°

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6
Q

What is the shape and bond angle of carbon dioxide?

A

Linear and 180°

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7
Q

What is the shape and bond angle of BF3?

A

Trigonal planar and 120°

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8
Q

What is the shape and bond angle of SF6?

A

Octahedral and 90°

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9
Q

What are bonding regions?

A

Bond angles or lone pairs

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10
Q

What factors affect electronegativity?

A

Nuclear charge and size of the atoms

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11
Q

What is electronegativity?

A

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

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12
Q

What element has the highest electronegativity value and what is it?

A

Fluorine at 4.0

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13
Q

What electronegativity values determine the bond type?

A

Covalent 0
Polar covalent 0-1.8
Ionic 1.8+

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14
Q

What are intermolecular forces?

A

Weak interactions between dipoles of different molecules

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15
Q

What are the three main categories of intermolecular forces?

A

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

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16
Q

What is the average bond enthalpy of London forces?

A

1-10kJ mol-1

17
Q

What is the average bond enthalpy of permanent dipole-dipole interactions?

A

3-25kJ mol-1

18
Q

What is the average bond enthalpy of hydrogen bonds?

A

10-40kJ mol-1

19
Q

What is the average bond enthalpy of single covalent bonds?

A

150-500kJ mol-1

20
Q

What happens in induced dipole-dipole interactions as the number of electrons increases?

A

The strength of the bond increases and the boiling and melting point is higher

21
Q

When do London Forces occur?

A

ALL molecules and noble gases

22
Q

What causes London Forces?

A

Instantaneous dipole will result from a temporary unequal sharing of electrons, which induces a dipole in a neighbouring molecule

23
Q

What causes permanent dipole-dipole interactions?

A

If a molecule is polar, then this type of force operated because of the difference in electronegativity

24
Q

When does hydrogen bonding occur?

A

NH OH FH

25
Q

What is the order of intermolecular force strength?

A

Hydrogen bonds > permanent dipole/dipole > temporary/induced dipole

26
Q

How does solubility work?

A

For one substance to be soluble in another they must have compatible bonds

My Chemistry (9 decks)

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