5.1 - 5.3 Flashcards
1
Q
How many sub shells are electron shells split into
A
- 4 sub shells
2
Q
Name the 4 sub shells
A
- s
- p
- d
- f
3
Q
How many orbitals does a s orbital have
A
- 1
4
Q
How many orbitals does a p orbital have
A
- 3
5
Q
How many orbitals does a d orbital have
A
- 5
6
Q
How many orbitals does a f orbital have
A
- 7
7
Q
How many electrons can a s orbital hold
A
- 2
8
Q
How many electrons can each p orbital hold and so how many electron does a p orbital hold it total
A
- each orbital can hold 3 electrons
- p orbital holds 6 electrons in total
9
Q
How many electrons can each d orbital hold and so how many electron does a d orbital hold it total
A
- each orbital can hold 2 electrons (5 orbitals)
- so in total a d orbital can hold 10 electrons
10
Q
How many electrons can each f orbital hold and so how many electron does a f orbital hold it total
A
- each orbital can hold 7 electrons
- so in total a f orbital hold 14 electrons
11
Q
How many electron can be held in the first shell
A
2
12
Q
How many electron can be held in the second shell
A
8
13
Q
How many electron can be held in the third shell
A
18
14
Q
What is another name for shell number
A
- principal quantum number
15
Q
If there is a higher shell number what does this mean
A
- it means that the shell is further away from the nucleus which mean that it also has higher energy
16
Q
What is the shape of an s orbital described as
A
- spherical shape
17
Q
What is the shape of an p orbital described as
A
- dumbbell shaped
18
Q
Name and describe the 3 types of p orbitals
A
1) Px orbital ( horizontal)
2) Py orbital (vertical)
3) Pz orbital (diagonal)
19
Q
Define spin-paring
A
- when 2 electron occupy 1 orbital they ‘spin’ in opposite directions
20
Q
Define ionic bonding
A
- compounds that are oppositely charged and held together by strong electrostatic attractions
21
Q
Describe characteristics of a giant ionic structure
A
1) regular structure
2) cubic shape
3) giant repeating pattern
22
Q
What is an example of an ionic compound
A
- Sodium Chloride
23
Q
Do most ionic compounds dissolve in water, and if so why?
A
- yes most of them do dissolve in water, because water molecules are POLAR and they can attract the positive and negative ions and break the structure
24
Q
Can ionic compounds conduct electricity, if so why?
A
- yes they can conduct electricity when MOLTEN or dissolved in SOLUTION because the IONS ARE FREE to move around
25
Do ionic compounds have a high melting point, if so why?
- yes they do have a high melting point as there are many STRONG ELECTROSTATIC forces between oppositely charges ions therefore LOTS OF ENERGY NEEDED TO OVERCOME THESE FORCES
26
Define covalent bonding
- the sharing of outer electrons in order for the atoms to obtain a full shell with a strong electrostatic attraction
27
Define a dative covalent bond
- where one atom donates 2 electrons to an atom or ion to form a bond
28
How are covalent bonds represented
- as lines
29
How are dative covalent bonds represented
- as arrows
30
How do you work out the shape of a molecule
- using the number of bond pairs and lone pairs
31
What do lone pairs do to the shape of a molecule
- they change the shape of bond angles
- they push bonding pairs closer together
- for every lone pair you reduce the remaining bond angles by 2.5 degrees
32
What would be the name of this shape in a molecule:
Bond pairs= 2
Lone Pairs= 0
Linear (180 degrees)
E.g BeCl2
33
What would be the name of this shape in a molecule:
Bond pairs= 3
Lone Pairs= 0
Trigonal planar (120)
E.g. BF3
34
What would be the name of this shape in a molecule:
Bond pairs= 4
Lone Pairs= 0
Tetrahedral (109.5 degrees)
E.g. CH4
35
What would be the name of this shape in a molecule:
Bond pairs= 5
Lone Pairs= 0
Trigonal Bipyramidal (90 degrees and 120 degrees)
E.g. PCl5
36
What would be the name of this shape in a molecule:
Bond pairs= 6
Lone Pairs= 0
Octahedral (90 degrees)
E.g. SF6
37
What would be the name of this shape in a molecule:
Bond pairs= 3
Lone Pairs= 1
Trigonal Pyramidal (107 degrees)
E.g NH3
38
What would be the name of this shape in a molecule:
Bond pairs= 2
Lone Pairs= 2
Non-linear (104.5)
E.g H2O
39
What would be the name of this shape in a molecule:
Bond pairs= 3
Lone Pairs= 2
Trigonal planar (120 degrees)
* bond angle remains the same as the 2 lone pairs repel equally from opposite sides
40
What would be the name of this shape in a molecule:
Bond pairs= 4
Lone Pairs= 2
Square Planar (90 degrees)
E.g XeF4
* bond angle remains the same as the 2 lone pairs repel equally from opposite sides
41
Define electronegativity
- the ability for an atom to attract electrons towards itself in a covalent bond
42
What is the most electronegative element
- Fluorine
43
How do we quantify how electronegative an element is
- Using a Pauling Scale
44
What does a bigger difference in electronegativity mean
- the more ionic the compound will be
45
What does a difference of zero in electronegativity mean
- that the compound is purely covalent
46
How do covalent bonds become polar
- because the atoms attached to it have a difference in electronegativity
47
Fill in the blanks:
The bigger the difference in electronegativity, the ____ _____ the bond will be
1) MORE
2) POLAR
48
Are hydrocarbons classed as polar
- No, because the difference in electronegativity is small
49
True or False:
If the polar bonds are arranged symmetrically then you have no overall polarity
- True
E.g. is CO2
50
What are the three types of intermolecular bonding in covalent molecules
- London forces
- Permanent dipole- dipole
- Hydrogen bonding
51
What are London forces
- FORCES THAT EXIST BETWEEN ATOMS AND MOLECULES
52
How do London forces occur
- as electrons in a molecule or atom can move from one end to another, creating a temporary dipole
- temporary dipole only exists when 2 molecules or atoms are near by
53
Describe the bonding in Iodine (I2)
- weak London forces holding the I2 molecules together but strong covalent bonds holding the 2 iodine atoms together
54
What does a bigger molecule or atoms mean for the London force
- the more induced the London forces are as you have larger electron clouds
55
When we boil a liquid what bond are we breaking
- the intermolecular London forces NOT the covalent bonds as they require more energy to break
56
What does a longer hydrocarbon mean for the boiling point
- it increases and we need more energy to overcome the intermolecular London forces
57
What does branched hydrocarbons mean for the boiling point
- it means they can’t pack together as close which weakens the London forces lowering the boiling point
58
What is permanent dipole-dipole bonding
- interactions that exist in molecules with a permanent polarity
59
True or false:
Molecules that have permanent dipole-dipole interactions also have London forces too
- true, we just say it has permanent dipole-dipole as that is the strongest forces they have
60
How do you test polar molecules
- by placing a charged rod near a steady stream of a polar liquid
- you should see the liquid bend towards the rods as the molecules align to face the oppositely charged rod
61
Define hydrogen bonding
- the strongest intermolecular force that occurs when you have hydrogen interacting with the lone pair on either nitrogen, oxygen or fluorine
62
How do we show hydrogen bonding
- dotted lines
63
True or false:
If a molecules has hydrogen bonding it also have permanent dipole-dipole forces and London forces
- True
64
What is the weakest type of intermolecular forces
- London forces
65
When you freeze water what happens
- it gets bigger, expands, becomes less dense
66
Why is ice less dense
- because ice forms a regular structure held by hydrogen bonding. The molecules are further apart which makes ice less dense than water
67
Why does HF has a high boiling point than HCl
- because HF has hydrogen bonding so more energy is required to overcome the electrostatic forces
68
Why does HI have a higher boiling point than HCl
- because there is an increase in the mass of the molecule so more London forces so more energy is needed to overcome them
69
Is the melting and boiling point of simple covalent molecules high or low
- low because you are breaking weak intermolecular forces
