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M2:Chapter 5 & 6=> Electrons+Bonding & Shapes Of Moelcules+Intermolecular Forces > 5.1 - 5.3 > Flashcards

5.1 - 5.3 Flashcards

1
Q

How many sub shells are electron shells split into

A
  • 4 sub shells
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2
Q

Name the 4 sub shells

A
  • s
  • p
  • d
  • f
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3
Q

How many orbitals does a s orbital have

A
  • 1
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4
Q

How many orbitals does a p orbital have

A
  • 3
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5
Q

How many orbitals does a d orbital have

A
  • 5
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6
Q

How many orbitals does a f orbital have

A
  • 7
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7
Q

How many electrons can a s orbital hold

A
  • 2
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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
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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
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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
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11
Q

How many electron can be held in the first shell

A

2

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12
Q

How many electron can be held in the second shell

A

8

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13
Q

How many electron can be held in the third shell

A

18

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14
Q

What is another name for shell number

A
  • principal quantum number
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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
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16
Q

What is the shape of an s orbital described as

A
  • spherical shape
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17
Q

What is the shape of an p orbital described as

A
  • dumbbell shaped
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18
Q

Name and describe the 3 types of p orbitals

A

1) Px orbital ( horizontal)
2) Py orbital (vertical)
3) Pz orbital (diagonal)

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19
Q

Define spin-paring

A
  • when 2 electron occupy 1 orbital they ‘spin’ in opposite directions
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20
Q

Define ionic bonding

A
  • compounds that are oppositely charged and held together by strong electrostatic attractions
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21
Q

Describe characteristics of a giant ionic structure

A

1) regular structure
2) cubic shape
3) giant repeating pattern

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22
Q

What is an example of an ionic compound

A
  • Sodium Chloride
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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
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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
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25
Q

Do ionic compounds have a high melting point, if so why?

A
  • 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
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26
Q

Define covalent bonding

A
  • the sharing of outer electrons in order for the atoms to obtain a full shell with a strong electrostatic attraction
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27
Q

Define a dative covalent bond

A
  • where one atom donates 2 electrons to an atom or ion to form a bond
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28
Q

How are covalent bonds represented

A
  • as lines
29
Q

How are dative covalent bonds represented

A
  • as arrows
30
Q

How do you work out the shape of a molecule

A
  • using the number of bond pairs and lone pairs
31
Q

What do lone pairs do to the shape of a molecule

A
  • 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
Q

What would be the name of this shape in a molecule:
Bond pairs= 2
Lone Pairs= 0

A

Linear (180 degrees)
E.g BeCl2

33
Q

What would be the name of this shape in a molecule:
Bond pairs= 3
Lone Pairs= 0

A

Trigonal planar (120)
E.g. BF3

34
Q

What would be the name of this shape in a molecule:
Bond pairs= 4
Lone Pairs= 0

A

Tetrahedral (109.5 degrees)
E.g. CH4

35
Q

What would be the name of this shape in a molecule:
Bond pairs= 5
Lone Pairs= 0

A

Trigonal Bipyramidal (90 degrees and 120 degrees)
E.g. PCl5

36
Q

What would be the name of this shape in a molecule:
Bond pairs= 6
Lone Pairs= 0

A

Octahedral (90 degrees)
E.g. SF6

37
Q

What would be the name of this shape in a molecule:
Bond pairs= 3
Lone Pairs= 1

A

Trigonal Pyramidal (107 degrees)
E.g NH3

38
Q

What would be the name of this shape in a molecule:
Bond pairs= 2
Lone Pairs= 2

A

Non-linear (104.5)
E.g H2O

39
Q

What would be the name of this shape in a molecule:
Bond pairs= 3
Lone Pairs= 2

A

Trigonal planar (120 degrees)
* bond angle remains the same as the 2 lone pairs repel equally from opposite sides

40
Q

What would be the name of this shape in a molecule:
Bond pairs= 4
Lone Pairs= 2

A

Square Planar (90 degrees)
E.g XeF4
* bond angle remains the same as the 2 lone pairs repel equally from opposite sides

41
Q

Define electronegativity

A
  • the ability for an atom to attract electrons towards itself in a covalent bond
42
Q

What is the most electronegative element

A
  • Fluorine
43
Q

How do we quantify how electronegative an element is

A
  • Using a Pauling Scale
44
Q

What does a bigger difference in electronegativity mean

A
  • the more ionic the compound will be
45
Q

What does a difference of zero in electronegativity mean

A
  • that the compound is purely covalent
46
Q

How do covalent bonds become polar

A
  • because the atoms attached to it have a difference in electronegativity
47
Q

Fill in the blanks:
The bigger the difference in electronegativity, the ____ _____ the bond will be

A

1) MORE
2) POLAR

48
Q

Are hydrocarbons classed as polar

A
  • No, because the difference in electronegativity is small
49
Q

True or False:
If the polar bonds are arranged symmetrically then you have no overall polarity

A
  • True
    E.g. is CO2
50
Q

What are the three types of intermolecular bonding in covalent molecules

A
  • London forces
  • Permanent dipole- dipole
  • Hydrogen bonding
51
Q

What are London forces

A
  • FORCES THAT EXIST BETWEEN ATOMS AND MOLECULES
52
Q

How do London forces occur

A
  • 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
Q

Describe the bonding in Iodine (I2)

A
  • weak London forces holding the I2 molecules together but strong covalent bonds holding the 2 iodine atoms together
54
Q

What does a bigger molecule or atoms mean for the London force

A
  • the more induced the London forces are as you have larger electron clouds
55
Q

When we boil a liquid what bond are we breaking

A
  • the intermolecular London forces NOT the covalent bonds as they require more energy to break
56
Q

What does a longer hydrocarbon mean for the boiling point

A
  • it increases and we need more energy to overcome the intermolecular London forces
57
Q

What does branched hydrocarbons mean for the boiling point

A
  • it means they can’t pack together as close which weakens the London forces lowering the boiling point
58
Q

What is permanent dipole-dipole bonding

A
  • interactions that exist in molecules with a permanent polarity
59
Q

True or false:
Molecules that have permanent dipole-dipole interactions also have London forces too

A
  • true, we just say it has permanent dipole-dipole as that is the strongest forces they have
60
Q

How do you test polar molecules

A
  • 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
Q

Define hydrogen bonding

A
  • the strongest intermolecular force that occurs when you have hydrogen interacting with the lone pair on either nitrogen, oxygen or fluorine
62
Q

How do we show hydrogen bonding

A
  • dotted lines
63
Q

True or false:
If a molecules has hydrogen bonding it also have permanent dipole-dipole forces and London forces

A
  • True
64
Q

What is the weakest type of intermolecular forces

A
  • London forces
65
Q

When you freeze water what happens

A
  • it gets bigger, expands, becomes less dense
66
Q

Why is ice less dense

A
  • because ice forms a regular structure held by hydrogen bonding. The molecules are further apart which makes ice less dense than water
67
Q

Why does HF has a high boiling point than HCl

A
  • because HF has hydrogen bonding so more energy is required to overcome the electrostatic forces
68
Q

Why does HI have a higher boiling point than HCl

A
  • because there is an increase in the mass of the molecule so more London forces so more energy is needed to overcome them
69
Q

Is the melting and boiling point of simple covalent molecules high or low

A
  • low because you are breaking weak intermolecular forces

M2:Chapter 5 & 6=> Electrons+Bonding & Shapes Of Moelcules+Intermolecular Forces (1 decks)

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