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AS Chemistry > Shapes Of Molecules and Intermolecular Forces > Flashcards

Shapes Of Molecules and Intermolecular Forces Flashcards

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1
Q

What does the arrangement of electron pairs do?

A

Minimises repulsion and holds the bonded atoms in a definitive shape

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2
Q

What causes different shapes?

A

Different numbers of electron pairs

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3
Q

What shape is it if there are four electron powers?

A

Tetrahedral

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4
Q

What is the bond angle in a tetrahedral shape?

A

109.5degress

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5
Q

Why is a lone pair more stronger repelling than a bonded pair of electrons?

A

A lone pair of electrons is slightly closer to the central atom and occupies more space

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6
Q

What shape is the molecule if there are 3 bonded pairs and one lone pair?

A

Pyramidal

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7
Q

What is the bond angle of a pyramidal molecule?

A

107degress

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8
Q

What is the shape of a water molecule?

A

Bent linear

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9
Q

What is the bond angle in a non linear shape? (Bent linear)

A

104.5degrees

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10
Q

What makes the bond angle smaller?

A

More electron pairs

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11
Q

What angle does a trigonal planar molecule have?

A

120 degrees

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12
Q

What bond angle does an octahedral molecule have?

A

90 degrees

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13
Q

What is electronegativity?

A

The attraction of a bonded atom for the pair of electrons in a covalent bond

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14
Q

What scale measures electronegativity?

A

The Pauling scale

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15
Q

What happens as you go right across the periodic table?

A

The electronegativity increases

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16
Q

What happens as you travel up the periodic table

A

The electronegativity increase

17
Q

What happens in a covalent molecule if there is a difference in electronegativity?

A

The covalent bond is pulled closer to the atom with more electronegativity

18
Q

Describe an ionic bond in terms of electronegativity

A

Large electronegativity difference
One atom has more of an attraction to the shared pair
More electronegative atom gained control of electrons

19
Q

What determine the shape of the molecule?

A

The electron pairs surrounding a central atom

20
Q

What is a non polar bond?

A

Where the bonded electron pair is shared equally between the bonded atoms

21
Q

When will there be a non polar bond?

A

When the bonded atoms are the same

The bonded atoms have the same or similar electronegativity

22
Q

What is a polar bond?

A

Where the bonded electron pair is shared unequally between the atoms

23
Q

What is a non polar bond also called?

A

A pure covalent bond

24
Q

Give an example of a polar molecule

A

Water

25
Q

What are intermolecular forces?

A

Weak interactions between dipoles of different molecules

26
Q

What are the three types of intermolecular forces?

A

Induced dipole to dipole (ldf)
Permanent dipole to dipole
Hydrogen bonding

27
Q

What are intermolecular forces responsible for?

A

Physical properties eg melting and boiling points

28
Q

How is an induced dipole created?

A

The movement of electrons creates a changing dipole in a molecule
Creating constantly shifting instantaneous dipole
Which induces a dipole on its neighbour
And so on

29
Q

What happens to the ldf the more electrons are in a molecule?

A

Larger the instantaneous and induced dipole
Greater induced dipole to dipole interactions
Stronger attractive forces between molecules

30
Q

Where do permanent dipoles happen?

A

Between the dipoles in polar molecules

31
Q

Are simple molecular forces soluble in polar solvents?

A

No

32
Q

Where is a hydrogen found between?

A

Molecules containing:
An electronegative atom with a lone pair of electrons
A hydrogen atom attached to an electronegative atom

33
Q

What does the hydrogen bond act between?

A

The lone pair of electrons on me molecule and the hydrogen atom on the other molecule

34
Q

What gives water it’s weird properties?

A

The hydrogen bonding

35
Q

Why is ice less dense than water?

A

Hydrogen bond holds water further apart in an open lattice structure with holes in it decreasing its density

AS Chemistry (16 decks)

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