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

2.2- Electrons, Bonding and Structure Flashcards

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
Why is boron trifluoride a strange covalent compound?
Boron only has 6 electrons in its outer shell
26
Why is sulphur hexafluoride a strange covalent compound?
It uses d orbitals to expand the octet and has more than 8 electrons in its outer shell
27
What is the strength of a covalent bond shown by?
It's average Bond enthalpy (the amount of energy required to break a covalent bond)
28
Why does oxygen have a high melting point?
Oxygen molecules form double covalent bonds which require lots of energy to break
29
What if an example of a molecule that can form triple Bond?
nitrogen
30
What is dative covalent bonding?
Where both electrons in the covalent bond come from one atom?
31
Where is dative covalent bond present? (example)
In an ammonium ion (NH4+)
32
What is the way to show dative covalent bonding in diagrams?
With an arrow pointing away from the donor atom
33
What is the shape of a molecule depend on?
The number of pairs of electrons in the outer shell of the central atom and the nature of these pairs
34
Why are electron pairs never shown close together in space?
Because electrons are negatively charged and will repel each other as much as they can
35
What is the way of predicting the shape of molecules known as?
Electron pair repulsion Theory
36
What is a great way to remember the different types of orbitals?
Student.Progress.Day.Fuck!
37
What is the bond angle and the number of BP's and LP's in a Linear Molecule?
180 degrees | 2BP 0LP
38
What is the bond angle and the number of BP's and LP's in a Trigonal planar Molecule?
120 degrees | 3BP 0LP
39
What is the bond angle and the number of BP's and LP's in a Tetrahedral Molecule?
109.5 degrees | 4BP 0LP
40
What is the bond angle and the number of BP's and LP's in a pyramidal Molecule?
107 degrees | 3BP 1LP
41
What is the bond angle and the number of BP's and LP's in a Non-Linear Molecule?
104.5 degrees | 2BP 2LP
42
What is the bond angle and the number of BP's and LP's in a Trigonal Bipyramid Molecule?
90 degrees and 120 degrees | 5BP 0LP
43
What is the bond angle and the number of BP's and LP's in a octahedral Molecule?
90 degrees | 6BP 0LP
44
What shape is a molecule that has a bond angle of 180 degrees?
Linear
45
What shape is a molecule that has a bond angle of 120 degrees?
Trigonal planar
46
What shape is a molecule that has a bond angle of 109.5 degrees?
Tetrahedral
47
What shape is a molecule that has a bond angle of 107 degrees?
Pyramidal
48
What shape is a molecule that has a bond angle of 104.5 degrees?
Non linear
49
What shape is a molecule that has a bond angle of 90 + 120 degrees?
Trigonal Bipyramid
50
What shape is a molecule that has a bond angle of 90 degrees?
Octahedral
51
What is the definition of electronegativity?
An atoms ability to attract the bonding pair of electrons in a covalent bond
52
What is the most electronegative element?
Fluorine
53
How is electronegativity measured?
On the pauling scale. | The higher an element pauling value, the higher it's electronegativity
54
Why are covalent bonds between elements with differences in electronegativity polar?
The bonding electrons are pulled towards the more electronegative atom which makes the bond polar The difference in electronegativity causes a permanent dipole
55
Robert says the chlorine gas is a polar molecule. Explain why Robert is almost certainly wrong.
Both chlorine atoms have equal electronegativities so the electrons are equally attracted to both nuclei. This makes the Bond nonpolar.
56
A bond between carbon and hydrogen atoms is considered non-polar. Explain why?
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
CO2 is a symetrical molecule. Why does it have no overall dipole?
the polar bonds are arranged so that they cancel each other out.
58
How can you predict how ionic/ covalend a bond is?
The higher the electronegetivity, the more ionic a bond will be
59
What are the three types of intermolecular forces?
Induced dipole-dipole interactions Permanent dipole-dipole interactions Hydrogen bonding
60
What are Van Der waals forces?
Induced dipole-dipole interactions and permanent dipole-dipole interactions
61
What do induced dipole-dipole interactions cause?
All atoms to be attracted to each other.
62
Why do induced dipole-dipole interactions occur?
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
How do induced dipole-dipole interactions affect boiling point?
Stronger forces mean higher boiling points has more energy is needed to overcome these intermolecular forces
64
Can induced dipole dipole forces hold molecules in a lattice?
Yes, they are responsible for holding iodine molecules together
65
What type of intermolecular forces do polar molecules have?
permanent dipole-dipole interactions caused by the charges on the polar molecule
66
What is the strongest type of intermolecular force?
Hydrogen bonding
67
Which elements can hydrogen bonding occur between?
Hydrogen and fluorine, nitrogen or oxygen
68
How does hydrogen bonding occur?
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
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?
Molecules which have hydrogen bonding usually contain OH or NH groups
70
How does hydrogen bonding affect the properties of a molecule?
They are soluble in water | They have higher melting and boiling points
71
Why is Ice less dense than liquid water?
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
Why do the boiling points of group 7 hydrides increase down the group?
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
Intermolecular forces explain trends in....
Boiling points
74
Why do simple covalent compounds have low melting and boiling points?
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
Why are polar molecules soluble in water?
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
Why do simple covalent compounds not conduct electricity?
The overall covalent molecules are uncharged which means they can't conduct electricity
77
Rodriguez says that when he heats up water he breaks the covalent bonds in the molecules. Explain why Rodriguez is wrong
To melt or boil a simple covalent compound, you only have to overcome intermolecular forces that hold the molecules together
78
Hannah suggests that the bonding between H2O is 100% covalent. Explain why Hannah is wrong.
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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