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A-Level Chemistry > 2.5 - The shapes of Simple Molecules & Ions > Flashcards

2.5 - The shapes of Simple Molecules & Ions Flashcards

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1
Q

what is the bond angle in a linear molecule

A

180˚

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2
Q

what is the bond angle in trigonal planar

A

120˚

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3
Q

what is the bond angle in non-linear/Bent molecule

A

104.5˚

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4
Q

what is the bond angle in a pyramidal molecule

A

107˚

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5
Q

What is the Bond angle in a tetrahedral molecule

A

109.5˚

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6
Q

what is the bond angle in a trigonal bipyramidal molecule

A

90˚ and 120˚

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7
Q

what is the bond angle in a octahedral molecule

A

90˚

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8
Q

What is the shape with 4 bonded pairs and no lone pairs

A

Tetrahedral

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9
Q

What is the shape with 3 bonded pairs and one lone pair

A

pyramidal

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10
Q

What is the shape with 2 bonded pairs and 2 lone pairs

A

non-linear

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11
Q

what is the shape with 2 bonded pairs

A

Linear

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12
Q

What is the shape with 3 bonded pairs

A

Trigonal planar

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13
Q

What is the shape with 6 bonded pairs

A

octahedral

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14
Q

What is the shape with 3 bonded and one lone pair

A

trigonal bipyramidal

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15
Q

what is the order of repulsion

A

lone pair – lone pair > lone pair – bond pair > bond pair – bond pair

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16
Q

what is electronegativity

A

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

17
Q

what happens to electronegativity down a group and why

A

Decreases
More shielding due to increase in shells

18
Q

what happens to electronegativity across a period and why

A

Increases
More protons so higher nuclear charge
shielding constant
small atomic radii

19
Q

what happens to electronegativity across a period and why

A

Increases
More protons so higher nuclear charge
shielding constant
small atomic radii

20
Q

what is a nonpolar bond

A

when 2 atoms in a covalent bond have the same electronegativity

21
Q

what is a dipole moment

A

a measure of how polar a bond is
points to the negative end

22
Q

what are intermolecular forces

A

Forces within a molecule and are usually covalent bonds

23
Q

what are the types of intermolecular forces

A

induced dipole dipole forces
permanent dipole dipole forces
hydrogen bonds

24
Q

what molecules have induced dipole dipole forces

A

all molecules

25
Q

what molecules have permanent dipole dipole forces

A

polar molecules

26
Q

what molecules have hydrogen bonds

A

ONF bonded to H

27
Q

Explain water’s high MP and BP

A

the strong intermolecular forces of hydrogen bonding between the molecules

28
Q

explain the density of ice compared with water

A

In ice however, the water molecules are packed in a 3D hydrogen-bonded network in a rigid lattice

Each oxygen atom is surrounded by hydrogen atoms

This way of packing the molecules in a solid and the relatively long bond lengths of the hydrogen bonds means that the water molecules are slightly further apart than in the liquid form

Therefore, ice has a lower density than liquid water

29
Q

describe the structure of iodine

A

Being a non-polar molecule, the weak intermolecular bonding is due to instantaneous dipole - induced dipole interactions
it is a molecular lattice

30
Q

What is the solubility like of molecular substances

A

non polar can dissolve in polar

polar can dissolve in polar - form hydrogen bonds with each other

Giant covalent substances generally don’t dissolve in any solvents

31
Q

What is the conductivity like of molecular substances

A

As covalent substances have no free charged particles they cant conduct electricity
However, under certain conditions some polar covalent molecules can ionise and will conduct electricity

Some giant covalent structures are capable of conducting electricity due to delocalised electrons

32
Q

what happens to solubility of polar substances as they become larger

A

As covalent molecules become larger their solubility can decrease as the polar part of the molecule is only a smaller part of the overall structure

A-Level Chemistry (13 decks)

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