Chemical Bonding and Structure Flashcards

1
Q

Multiple covalent bonds are caused by what?

A

Strong electrostatic forces of attraction between the nuclei and shared electrons

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2
Q

Lone pairs of electrons can affect what about the molecule?

A

It’s shape.

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3
Q

Lone pairs of electrons can form what with other atoms?

A

Dative covalent bonds (coordinate bonds).

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4
Q

A sigma bond is what?

A

A sigma bond is your basic head-on covalent bond with the bond in line with the bonding orbitals.

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5
Q

How many sigma bonds can you only ever have between any two atoms?

A

One.

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6
Q

A pi bond is what?

A

A pi bond is a covalent bond between orbitals perpendicular to the bond direction. This is usually p-orbitals, never s.

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7
Q

Electron pairs do what to each other?

A

Repel each other, as they are negatively charged.

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8
Q

Molecules are shaped so that what can be said to be true?

A

Molecules are shaped so that electron pairs are arranged to be as far away from each other as possible.

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9
Q

2e pairs makes what shape and what bond angle?

A

Linear, 180 degrees.

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10
Q

3e pairs are arranged in why shape with what bond angle?

A

Trigonal planar, 120 degrees.

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11
Q

4e pairs makes what shape with what bond angle?

A

Tetrahedral, 109.5 degrees.

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12
Q

Electron pair repulsion theory is the theory that…

A

…a lone pair exerts more repulsion than a bonded pair. This is about 2.5 degrees per lone pair and examples of these are water and ammonia bond angles (104.5 and 107).

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13
Q

Double and triple bonds act as what when we consider molecule shapes?

A

They act as a centre of negative charge causing similar shapes to molecules with singly bonded electron pairs.

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14
Q

If the two atoms covalently bonded are the same what can be said about the electrons?

A

They are shared equally between the two atoms.

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15
Q

What is a polar covalent bond?

A

When two atoms are covalently bonded but one atom has a nucleus that the electrons are more attracted too.

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16
Q

What happens to a atoms of they have a polar covalent bond between them?

A

Dipoles form with a delta negative where the electrons are closer too and a delta positive where the electrons are further from. Overall there is no charge as these charges are equal and cancel.

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17
Q

What is electronegativity?

A

Electronegativity is the ability of an atom to attract the bonding electrons in a covalent pair.

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18
Q

How can electronegativity be used to predict the extent to which the bonds between different atoms can be polar?

A

The greater the difference of the electronegativity of the atoms bonding, the greater the polarity of the covalent bond between them.

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19
Q

Electronegativity does what across a period?

A

Increases.

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20
Q

Why does electronegativity increase across a period?

A

The nuclear charge increases but the number of shielding electrons remains constant, so the attraction for the shared electrons pairs increases.

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21
Q

What type of diffraction can be used for chemists to work out structure?

A

X-ray diffraction.

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22
Q

Microwave spectroscopy can give chemists information about what?

A

Bond lengths between atoms.

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23
Q

Bond length depends on what?

A

Size of atom. Single bonds are longer than multiple bonds as there are less electrons in the shared electron cloud.

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24
Q

Sigma bonds are how strong relative to pi bonds?

A

Sigma bonds are far stronger as they are closer to the nucleus and experience stronger attraction, therefore are more difficult to break.

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25
Q

Lone pairs of electrons can be used to form what?

A

Dative covalent bonds (coordinate bonds).

26
Q

Example of a dative covalent bond:

A

An ammonium ion, +1 charge due to a H+ bonding with the lone pair on ammonia.
An hydroxonium ion, +1 charge due to a H+ bonding with a lone pair on water.

27
Q

Electronegativity is what?

A

Electronegativity is the pull of atoms on electrons or electron pairs.

28
Q

What happens to electronegativity across a period?

A

Electronegativity increases across a period.

29
Q

What happens to electronegativity as we go up a group?

A

It increases.

30
Q

Why does electronegativity increase up a group?

A

It increases due to decreasing atomic radius.

31
Q

Pauling did what?

A

Gave elements values based on their electronegativity on a scale from 0-4.

32
Q

What are the three most electronegative elements?

A

Nitrogen, oxygen and fluorine (3.0, 3.5 and 4.0 on Pauling’s system).

33
Q

If two atoms are covalently bonded together and are exactly the same is the molecule polar and if so where are the poles?

A

No, because both atoms have the same electronegativity and neither attracts the electrons slightly more than the other, therefore no partial charges are present.

34
Q

If two atoms covalently bonded are not the same, for example HCl, is the molecule polar and if so where are the poles?

A

Yes, because the chlorine is more electronegative than hydrogen meaning there is a δ- charge towards the chlorine and a δ+ charge towards the hydrogen.

35
Q

Polar bonds in a molecule don’t necessarily mean that the molecule is polar. Why not?

A

If the molecule is symmetrical the dipoles can cancel.

36
Q

Why is there no difference in charge between carbon and hydrogen?

A

They have a similar electronegativity (difference of 0.4) so no dipoles form.

37
Q

What type of force is a London force?

A

A weak intermolecular force.

38
Q

What happens to cause London forces?

A

Electrons are never in a fixed position so temporary dipoles within the molecule can form which induce temporary dipoles in neighbouring molecules. Opposites attract and intermolecular forces are experienced.

39
Q

Do London forces only occur when electrons are symmetrical or asymmetrical?

A

Asymmetrical.

40
Q

Dipole-dipole forces occur in addition to what forces?

A

London forces.

41
Q

Dipole-dipole interactions take place when?

A

When molecules have permanent dipoles.

42
Q

How does dipole-dipole bonding work?

A

The positive dipole on one molecule attracts the negative of another and vice-versa.

43
Q

Molecules with permanent dipoles have a higher what than those without?

A

Boiling and melting point(s).

44
Q

Hydrogen bonding can be described as an extreme type of what?

A

Dipole-dipole bonding.

45
Q

How many times weaker than a covalent bond is a hydrogen bond?

A

At least 10 times.

46
Q

Hydrogen bonding acts in addition to…

A

…London forces and dipole-dipole forces.

47
Q

Hydrogen bonding effects:

A

Molecules with a H bonded to a NOF.

Molecules with a lone pair on a NOF atom.

48
Q

How does hydrogen bonding work?

A

The NOF atom attracts electrons strongly away from the H leaving it δ+. The re is then a strong intermolecular force between the δ+ H and the lone pair on another atom on a nearby molecule.

49
Q

What is the bond angle of hydrogen bonding?

A

180 degrees.

50
Q

For one substance to dissolve another what must happen?

A

The bonds in the substance have to break.
The bonds in the solvent have to break.
New bonds must form between the substance and the solvent.

51
Q

Ionic substances dissolve in polar solvents because:

A

The ions are attracted to the oppositely charged poles of the solvent molecules.
The ions are pulled away from the ionic lattice by the solvent molecules.

52
Q

Ions being pulled away from the lattice by water molecules and surrounding the ions is known as what?

A

Hydration.

53
Q

Alcohols dissolve in polar solvents because:

A

The polar OH bond in an alcohol is attracted to the poles in a polar solvent.
The carbon chain of the alcohol isn’t attracted to the solvent, so the more carbon atoms in the chain the less soluble the alcohol in a polar solvent.

54
Q

Alcohols dissolve in water because:

A

The polar OH bond in an alcohol is attracted to the polar OH bonds in water. Hydrogen bonds form between the lone pairs on the oxygen and the delta + hydrogen.

55
Q

Which molecules have polar bonds but don’t dissolve in water?

A

Halogenoalkanes.

56
Q

Why can halogeboalkanes dissolve in water?

A

The dipoles in halogenoalkanes aren’t strong enough to form hydrogen bonds with water. The hydrogen bond in water is stronger than the bonds between halogenoalkanes.

57
Q

Non polar substances dissolve best in what?

A

Non polar substances.

58
Q

Why do non polar substances dissolve best in other non polar substances?

A

They form similar bonds (London forces) between molecules.

59
Q

Why don’t polar substances substances dissolve very well in non polar solvents and vice-versa?

A

The molecules of the polar substance are attracted together more strongly than non polar molecules.

60
Q

What phrase can we use for solubility?

A

“Like dissolves like”

61
Q

What does miscible mean?

A

When two liquids mix to form a homogeneous mixture.

62
Q

What is the opposite to miscible?

A

Immiscible.