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AS- Chemistry > 2.2- Electrons, Bonding and Structure > Flashcards

2.2- Electrons, Bonding and Structure Flashcards

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1
Q

What are electron shells made up of?

A

Subshells and orbitals

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2
Q

How many electrons can an orbital hold?

A

Two electrons with opposite spins

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3
Q

What is another name for the energy shell?

A

Principal quantum number

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4
Q

What shape are s orbitals?

A

Spherical

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5
Q

What shape are p orbitals?

A

3D dumbbell shape

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6
Q

What is it called when electrons spin in opposite directions to fit within an Orbital?

A

Spin pairing

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7
Q

What are the two main ways we can show electron configuration?

A

Subshell notation eg.1s2 2s2

Electrons in boxes

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8
Q

Which orbitals will fill first?

A

The ones with the lowest energy levels

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9
Q

What is the subshell notation for how orbitals fill?

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 4f14

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10
Q

Why do orbitals fill singularly before they start pairing up?

A

Because this uses less energy

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11
Q

How many electrons can an S subshell hold?

A

2

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12
Q

How many electrons can a p subshell hold?

A

2

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13
Q

How many orbitals are in an s subshell?

A

1

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14
Q

How many orbitals are in a p subshell?

A

3

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15
Q

What is the definition of an Orbital?

A

An area of space in which you are likely to find two electrons with opposite spins

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16
Q

What is the definition of an ionic bond?

A

The electrostatic attraction between two oppositely charged ions

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17
Q

What two types of elements does ionic bonding generally occur between?

A

Metals and non-metals

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18
Q

How do we represent ionic bonding with what diagram?

A

We use dot and cross diagrams

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19
Q

Why does sodium chloride have a giant ionic lattice structure?

A

Each ion is electrostatically attracted in all directions to ions of opposite charge.
The same basic unit is repeated over and over again (giant)

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20
Q

Why do giant ionic compounds conduct electricity when they are molten or dissolved?

A

The ions in a liquid and mobile and can carry a charge

In a solid the ions of fixed in position by the strong ionic bonds

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21
Q

Why do ionic compounds have high melting and boiling points?

A

The lattices are held together by strong electrostatic forces.
It takes loads of energy to overcome this forces so the melting and boiling points are very high

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22
Q

Why do ionic compounds tend to dissolve in water?

A

Water molecules are polar and attracted to the charged ions.
They pull the ions away from the lattice and cause it to dissolve

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23
Q

What is the definition of a covalent bond?

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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24
Q

How can we draw diagrams of covalent bonding?

A

With dot and cross cross diagrams

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25
Q

Why is boron trifluoride a strange covalent compound?

A

Boron only has 6 electrons in its outer shell

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26
Q

Why is sulphur hexafluoride a strange covalent compound?

A

It uses d orbitals to expand the octet and has more than 8 electrons in its outer shell

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27
Q

What is the strength of a covalent bond shown by?

A

It’s average Bond enthalpy (the amount of energy required to break a covalent bond)

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28
Q

Why does oxygen have a high melting point?

A

Oxygen molecules form double covalent bonds which require lots of energy to break

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29
Q

What if an example of a molecule that can form triple Bond?

A

nitrogen

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30
Q

What is dative covalent bonding?

A

Where both electrons in the covalent bond come from one atom?

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31
Q

Where is dative covalent bond present? (example)

A

In an ammonium ion (NH4+)

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32
Q

What is the way to show dative covalent bonding in diagrams?

A

With an arrow pointing away from the donor atom

33
Q

What is the shape of a molecule depend on?

A

The number of pairs of electrons in the outer shell of the central atom and the nature of these pairs

34
Q

Why are electron pairs never shown close together in space?

A

Because electrons are negatively charged and will repel each other as much as they can

35
Q

What is the way of predicting the shape of molecules known as?

A

Electron pair repulsion Theory

36
Q

What is a great way to remember the different types of orbitals?

A

Student.Progress.Day.Fuck!

37
Q

What is the bond angle and the number of BP’s and LP’s in a Linear Molecule?

A

180 degrees

2BP 0LP

38
Q

What is the bond angle and the number of BP’s and LP’s in a Trigonal planar Molecule?

A

120 degrees

3BP 0LP

39
Q

What is the bond angle and the number of BP’s and LP’s in a Tetrahedral Molecule?

A

109.5 degrees

4BP 0LP

40
Q

What is the bond angle and the number of BP’s and LP’s in a pyramidal Molecule?

A

107 degrees

3BP 1LP

41
Q

What is the bond angle and the number of BP’s and LP’s in a Non-Linear Molecule?

A

104.5 degrees

2BP 2LP

42
Q

What is the bond angle and the number of BP’s and LP’s in a Trigonal Bipyramid Molecule?

A

90 degrees and 120 degrees

5BP 0LP

43
Q

What is the bond angle and the number of BP’s and LP’s in a octahedral Molecule?

A

90 degrees

6BP 0LP

44
Q

What shape is a molecule that has a bond angle of 180 degrees?

A

Linear

45
Q

What shape is a molecule that has a bond angle of 120 degrees?

A

Trigonal planar

46
Q

What shape is a molecule that has a bond angle of 109.5 degrees?

A

Tetrahedral

47
Q

What shape is a molecule that has a bond angle of 107 degrees?

A

Pyramidal

48
Q

What shape is a molecule that has a bond angle of 104.5 degrees?

A

Non linear

49
Q

What shape is a molecule that has a bond angle of 90 + 120 degrees?

A

Trigonal Bipyramid

50
Q

What shape is a molecule that has a bond angle of 90 degrees?

A

Octahedral

51
Q

What is the definition of electronegativity?

A

An atoms ability to attract the bonding pair of electrons in a covalent bond

52
Q

What is the most electronegative element?

A

Fluorine

53
Q

How is electronegativity measured?

A

On the pauling scale.

The higher an element pauling value, the higher it’s electronegativity

54
Q

Why are covalent bonds between elements with differences in electronegativity polar?

A

The bonding electrons are pulled towards the more electronegative atom which makes the bond polar
The difference in electronegativity causes a permanent dipole

55
Q

Robert says the chlorine gas is a polar molecule. Explain why Robert is almost certainly wrong.

A

Both chlorine atoms have equal electronegativities so the electrons are equally attracted to both nuclei.
This makes the Bond nonpolar.

56
Q

A bond between carbon and hydrogen atoms is considered non-polar. Explain why?

A

Carbon and hydrogen have very similar electronegativities so there is a very small difference in charge between the two atoms which is essentially nonpolar

57
Q

CO2 is a symetrical molecule. Why does it have no overall dipole?

A

the polar bonds are arranged so that they cancel each other out.

58
Q

How can you predict how ionic/ covalend a bond is?

A

The higher the electronegetivity, the more ionic a bond will be

59
Q

What are the three types of intermolecular forces?

A

Induced dipole-dipole interactions
Permanent dipole-dipole interactions
Hydrogen bonding

60
Q

What are Van Der waals forces?

A

Induced dipole-dipole interactions and permanent dipole-dipole interactions

61
Q

What do induced dipole-dipole interactions cause?

A

All atoms to be attracted to each other.

62
Q

Why do induced dipole-dipole interactions occur?

A

Electrons in charge cloud a moving really quickly and at any particular moment, the electrons in an atom are likely to be more on one side than the other.
At this moment they have a temporary dipole.
This can cause another temporary dipole in the opposite direction on a neighbouring atom
These two atoms are then attracted to each other

63
Q

How do induced dipole-dipole interactions affect boiling point?

A

Stronger forces mean higher boiling points has more energy is needed to overcome these intermolecular forces

64
Q

Can induced dipole dipole forces hold molecules in a lattice?

A

Yes, they are responsible for holding iodine molecules together

65
Q

What type of intermolecular forces do polar molecules have?

A

permanent dipole-dipole interactions caused by the charges on the polar molecule

66
Q

What is the strongest type of intermolecular force?

A

Hydrogen bonding

67
Q

Which elements can hydrogen bonding occur between?

A

Hydrogen and fluorine, nitrogen or oxygen

68
Q

How does hydrogen bonding occur?

A

Hydrogen has a high charge density because it’s so small and the NOF elements are very electronegative.
The covalent bond is so polarized that a weak Bond forms between the hydrogen and a lone pair of electrons in the NOF element

69
Q

Tony is looking at a diagram with a type of bonding. His teacher tells him it is hydrogen bonding. How does Tony know that his teacher is correct?

A

Molecules which have hydrogen bonding usually contain OH or NH groups

70
Q

How does hydrogen bonding affect the properties of a molecule?

A

They are soluble in water

They have higher melting and boiling points

71
Q

Why is Ice less dense than liquid water?

A

In ice, molecules of H2O are held together in a lattice by hydrogen Bond
When ice melts, hydrogen bonds are broken so ice has more hydrogen bonds than liquid water
Since hydrogen bonds are relatively long, this makes ice less dense than liquid water

72
Q

Why do the boiling points of group 7 hydrides increase down the group?

A

Although the permanent dipole-dipole interactions are decreasing, the number of electrons in the molecule increases, so the strength of the induced dipole dipole also increases

73
Q

Intermolecular forces explain trends in….

A

Boiling points

74
Q

Why do simple covalent compounds have low melting and boiling points?

A

The intermolecular forces that hold together the molecules in simple covalent compounds are weak so don’t need much energy to break.
So the melting and boiling points in normally low

75
Q

Why are polar molecules soluble in water?

A

Water is a polar molecule, so only tends to dissolve other polar substances
Compounds with hydrogen bonds can form hydrogen bonds with water molecules so will be soluble

76
Q

Why do simple covalent compounds not conduct electricity?

A

The overall covalent molecules are uncharged which means they can’t conduct electricity

77
Q

Rodriguez says that when he heats up water he breaks the covalent bonds in the molecules. Explain why Rodriguez is wrong

A

To melt or boil a simple covalent compound, you only have to overcome intermolecular forces that hold the molecules together

78
Q

Hannah suggests that the bonding between H2O is 100% covalent. Explain why Hannah is wrong.

A

The electronegativity difference isnt 0 so the bonding electrons arent arranged completely evenly. This means the bonding will be slightly ionic.

AS- Chemistry (7 decks)

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