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Alevel Chemistry OCR A > Module 2: Section 2- Electrons Bonding And Structure > Flashcards

Module 2: Section 2- Electrons Bonding And Structure Flashcards

1
Q

Electronic structure
What are electron shells made up of

A

Sub shells and orbitals

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2
Q

Electronic structure
In current accepted model of the atom what energy do electrons have

A

Fixed energies

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3
Q

Electronic structure
Where are electrons

A

Move around the nucleus in shells (energy levels)

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4
Q

Electronic structure
What are all shells given

A

Numbers called principal quantum numbers

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5
Q

Electronic structure
Which shells have highest energy

A

Shells furthest from nucleus

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6
Q

Electronic structure
What are shells divided into

A

Sub shells

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7
Q

Electronic structure
What are the type of sub shells

A

S p d and f (in order)

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8
Q

Electronic structure
How may electrons can orbitals hold

A

2

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9
Q

Electronic structure
How many orbitals in s subshell

A

1

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10
Q

Electronic structure
Maximum electrons in s subshell

A

2

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11
Q

Electronic structure
How many orbitals in p subshell

A

3

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12
Q

Electronic structure
Maximum electrons in p subshell

A

6

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13
Q

Electronic structure
How many orbitals in d subshell

A

5

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14
Q

Electronic structure
Maximum electrons in d subshell

A

10

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15
Q

Electronic structure
How many orbitals in f subshell

A

7

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16
Q

Electronic structure
Maximum electrons in d subshell

A

10

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17
Q

Electronic structure
How many orbitals in f subshell

A
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18
Q

Electronic structure
Maximum electrons in f subshell

A

14

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19
Q

Electronic structure
Subshells in 1st shell

A

1s

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20
Q

Electronic structure
Total number of electrons in 1st shell

A

2

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21
Q

Electronic structure
Subshells in 2nd shell

A

2s 2p

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22
Q

Electronic structure
Total number of electrons in 2nd shell

A

8

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23
Q

Electronic structure
Subshells in 3rd shell

A

3s 3p 3d

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24
Q

Electronic structure
Total number of electrons in 3rd shell

A

18

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25
Q

Electronic structure
Subshells in 4th shell

A

4s 4p 4d 4f

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26
Q

Electronic structure
Total number of electrons in 4th shell

A

32

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27
Q

Electronic structure
What is an orbital

A

Region of space that an electron moves in

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28
Q

Electronic structure
Which orbitals have same energy

A

Orbital within the same sub shell

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29
Q

Electronic structure
What has to be true of electrons to be in same orbital

A

Have to spin in opposite directions

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30
Q

Electronic structure
What shape is an s orbital

A

Spherical

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31
Q

Electronic structure
What shape is a p orbital

A

Dumbbell

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32
Q

Electronic structure
What is and atom or ions electron configurations

A

Number of electrons and how they’re arranges

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33
Q

Electronic structure
How can electron configuration be shown

A

Subshell notation
Electrons in boxes

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34
Q

Electronic structure
Subshell notation

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 …

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35
Q

Electronic structure
What does each box represent in electronic configuration

A

Orbitals

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36
Q

Electronic structure
What does each arrow represent in ewlecxtronic configuration

A

An electron

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37
Q

Electronic structure
Why are the arrows opposite facing in electronic configuration

A

Show opposite spin

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38
Q

Electronic structure
Rules for filling shells

A

Fill lowest energy Subshells first
Fill orbitals with the same energy singly before they start sharing
Fills 4s subshell before 3d Subshells

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39
Q

Electronic structure
2 exceptions for 3d and 4s filling

A

Chromium and copper

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40
Q

Electronic structure
Nobles gas symbols in configuration

A

Used to shorten eg Calcium as [Ar] 4s2

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41
Q

Ionic bonding
Definition

A

Electrostatic force of attraction between two oppositely charged ions

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42
Q

Ionic bonding
When are ions formed

A

When electrons are transferred from one atom to another so as to have a full outer shell

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43
Q

Ionic bonding
What is electrostatic attraction

A

Holds positive and negative ions together which is very strong

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44
Q

Ionic bonding
When do you get an ionic compound

A

When oppositely charges ions form an ionic bond

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45
Q

Ionic bonding
What do dot and cross diagrams show

A

Arrangement of electrons in an atom or ion

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46
Q

Ionic bonding
What are giant ionic lattices

A

Structure is giants as each ion is electrostatically attracted in all directions to ions of opposite charge

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47
Q

Ionic bonding
Why do ionic compounds have high melting and boiling points

A

Strong electrostatic force of attraction which take lots of energy to overcome

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48
Q

Ionic bonding
Why do ionic compounds conduct electricity when they’re molten or dissolved

A

Ions in a liquid are mobile and came carry charge

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49
Q

Ionic bonding
Why do ionic computers not conduct electricity when solid

A

Ions fixed in position by strong ionic bonds so can’t carry charge

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50
Q

Ionic bonding
Why do ionic compounds tend to dissolve in water

A

Water molecules are polar(part of molecule has a small negative charge and other bits have small positive charge) water molecules are attracted to charge ions and pull them away from the lattice causing it to dissolve

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51
Q

Covalent bonding
What are molecules

A

When two or more atoms bond together covalently

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52
Q

Covalent bonding
What happens in coolant bonding

A

Electrons are shared so atoms have full outer shells

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53
Q

Covalent bonding
Definition

A

Strong electrostatic attraction between a shared pair of electrons and nuclei of bonded atoms

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54
Q

Covalent bonding
What do dot and cross diagrams show

A

How electrons behave in covalent bonds

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55
Q

Covalent bonding
Covalent exceptions

A

Some compounds have less than 8 electrons in the outer shell and some can use the d orbital to ‘expand the octet, meaning they have more than 8 electrons in the outer shell

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56
Q

Covalent bonding
Example of compound with less than 8 electrons in outer shell

57
Q

Covalent bonding
Example of compound with more than 8 electrons in outer shell

58
Q

Covalent bonding
What is average bond enthalpy

A

Measures energy required to break a covalent bond

59
Q

Covalent bonding
What’s a double covalent bond

A

Two paired of shared electrons

60
Q

Covalent bonding
What’s a triple covalent bond

A

Three pairs of shared electrons

61
Q

Covalent bonding
What’s a dative bond

A

Both electrons come from one atom

62
Q

Covalent bonding
Example of covalent molecule with a dative bond

A

Ammonium
NH4 ^+

63
Q

Covalent bonding
How’s dative covalent bond shown on diagram

A

Arrow pointing away from donor atom

64
Q

Shapes of molecules
What does molecular shape depend on

A

Electron pairs around the central atom

65
Q

Shapes of molecules
What are bonding pairs

A

Pair of electrons which are shared with another atom

66
Q

Shapes of molecules
what are lone pairs

A

Pair of electrons which are not shared

67
Q

Shapes of molecules
Why do electron pairs repel each other as much as they can

A

Electrons are all negatively charged

68
Q

Shapes of molecules
What type of pair repels the most

A

Lone pairs repel more than bonding pairs

69
Q

Shapes of molecules
What is the order of the strength of repulsion

A

Lp lp > bp lp > bp bp

70
Q

Shapes of molecules
What is th bond angles in a molecule with 4 bp

71
Q

Shapes of molecules
What is the bond angle in a molecule with 3bp and 1lp

A

All three bond angles are 107

72
Q

Shapes of molecules
What is the bond angle in a molecule with 2bp and 2lp

A

The bond angle is 104.5

73
Q

Shapes of molecules
What are the two types of flying wedges

A

Soldi triangle wedge
Broken lines wedge

74
Q

Shapes of molecules
What does the solid triangle wedge mean

A

Bond coming out the page

75
Q

Shapes of molecules
What does the broken lines wedge mean

A

Bond going into page

76
Q

Shapes of molecules
How do you predict the shapes of molecules step by step

A
  1. Find central atom
  2. Work out number of electrons in the outer shell from periodic table and take into account charge
  3. Add the number of bonded atoms
  4. Divide number of electrons by 2 to find the number of electron pairs
  5. Compare number of electron pairs with number of bonding pairs to find lone pairs
  6. Corresponding to different pairs
77
Q

Shapes of molecules
What is the name of the molecule with 2 bp and what is the bond angle

A

Linear
180’

78
Q

Shapes of molecules
What is the name of the molecule with 3 bp and bond angle

A

Trigonal planar
120’

79
Q

Shapes of molecules
What is the name of the molecule with 4 bp and what’s the bond angle

A

Tetrahedral
109.5’

80
Q

Shapes of molecules
What is the name of the molecule with 3bp and 1lp

A

Trigonal pyramid
107’

81
Q

Shapes of molecules
What is the name of the molecule of 2bp and 2lp and what’s the bond angle

82
Q

Shapes of molecules
What is the name of the molecule with 5bp and what’s the bond angle

A

Trigonal bipyramidal
120’ 90’

83
Q

Shapes of molecules
What is the name of the molecule with 6bp and he wants the bond angle

A

Octahedral
All 90’

84
Q

Polarity and electronegativity
What’s electronegativity

A

Atoms ability to attract the electron pair in a covalent bond

85
Q

Polarity and electronegativity
Electronegativity trend in periodic tab;e

A

Increases across periods and decreases down groups

86
Q

Polarity and electronegativity
How is electronegativity measured

A

On the Pauling scale

87
Q

Polarity and electronegativity
What makes a bond polar

A

In a covalent bond between atoms of different electronegativities the bonding electrons are pulled towards the more electronegative atom

88
Q

Polarity and electronegativity
In a polar bond what dos the difference in electronegativity cause

A

A permanent dipole

89
Q

Polarity and electronegativity
What is a dipole

A

Difference in charge between two atoms cased by a shift in electron density in the bond

90
Q

Polarity and electronegativity
What makes a bond more polar

A

The greater the difference in electronegativity

91
Q

Polarity and electronegativity
What is a non polar covalent bond

A

Atoms have equal electronegativity and so electrons are equally attracted to both nuclei

92
Q

Polarity and electronegativity
Examples of non polar bonds

A

Diatomic gases eg Cl2 and H2

93
Q

Polarity and electronegativity
What determines whether or not the molecule will have an overall dipole

A

Arrangement of polar bonds in a molecule

94
Q

Polarity and electronegativity
What happens if the polar bonds are arranged symmetrically so that the dipoles are opposite and equal

A

The molecule has no overall dipole and is non polar

95
Q

Polarity and electronegativity
What is carbon dioxide an example of

A

A molecule which contains two polar bonds but no overall dipole

96
Q

Polarity and electronegativity
When is there and overall dipole

A

If polar bond are arranged so that they don’t cancel each other out then charge is arranged unevenly across whole molecule and will have an overall dipole

97
Q

Polarity and electronegativity
Example of polar molecule

A

Water is polar as the negative charge is positioned more towards the oxygen atom

98
Q

Polarity and electronegativity
What’s re the notions for dipole

A

Delta + and delta - (delta- for more electronegative)
+———> (arrow towards more electronegative)

99
Q

Polarity and electronegativity
What bond between elements are purely covalent and why

A

Bond between atoms of a single element because the electronegativity difference between the atoms is zero and so the bonding electrons are arranged completely evenly within the bond

100
Q

Polarity and electronegativity
Transition between ionic to covalent bonding

A

Changes and most compounds between the two meaning often have covalent and ionic properties

101
Q

Polarity and electronegativity
How can you use electronegativity to predict what type of bonding will occur between two atoms

A

Higher difference in electronegativity, more ionic in character the bonding becomes

102
Q

Polarity and electronegativity
How can a molecule contain polar bonds but not be polar

A

If there are permanent dipoles but they are opposite and equal so they cancel out

103
Q

Polarity and electronegativity and IMF
What are intermolecular forces

A

Attraction which holds molecules together

104
Q

Polarity and electronegativity and IMF
Are IMF strong or weak

A

Much weaker than covalent ionic and metallic bonds

105
Q

Polarity and electronegativity and IMF
What are the three type of IMF

A

Induced dipole-dipole or London forces
Permanent dipole-dipole interactions
Hydrogen bonding

106
Q

Polarity and electronegativityand IMF
What is the strongest type of IMF

A

Hydrogen bonding

107
Q

Polarity and electronegativity and IMF
what factors affect electronegativity

A

Nuclear charge
———————-
Atomic radius
Shielding

108
Q

Polarity and electronegativity and IMF
Which element do electrons move towards

A

Element with highest electronegativity

109
Q

Polarity and electronegativity and IMF
What type of IMF do all atoms and molecules have

A

London forces

110
Q

Polarity and electronegativity and IMF
What causes an instantaneous dipole

A

Electrons in charge cloud are always moving really quickly and at any instant the electrons in an atom are likely to be more to one side

111
Q

Polarity and electronegativity and IMF
What does an instantaneous dipole cause

A

An induced dipole in a neighbouring atom which causes the two dipole to be attracted to each other

112
Q

Polarity and electronegativity and IMF
What happens in London forced because the electrons are constantly moving

A

Dipoles being created and destroyed but overall effect for atoms to be attracted to each other

113
Q

Polarity and electronegativity and IMF
Are all London forced the same strength

114
Q

Polarity and electronegativity and IMF
What causes a larger London force

A

Larger molecules with larger electron clouds
Molecules with greater surface areas as have bigger exposed electron cloud

115
Q

Polarity and electronegativity and IMF
What needs to happen when you boil a liquid and link to London forces

A

Need to overcome IMF so that particles can escape to liquid surface so need more energy to overcome stronger IMFS so liquid worth stronger London forces will have higher boiling points

116
Q

Polarity and electronegativity and IMF
What can London forces hold molecules in

117
Q

Polarity and electronegativity and IMF
How do London forced hold iodine together

A

Iodine atoms are held together in pairs bu strong covalent bonds to form I2 but the molecules are help together in a molecular lattice arrangement by weak induced dipole-dipole attractions

118
Q

Polarity and electronegativity and IMF
What type of IMF do polar molecules form

A

Permanent dipole dipole

119
Q

Polarity and electronegativity and IMF
What are permanent dipole dipole imfs

A

Delta negative and delta positive polar molecules cause weak electrostatic forces of attraction between molecules

120
Q

Polarity and electronegativity and IMF
What is the strongest type of IMF

A

A hydrogen bond

121
Q

Polarity and electronegativity and IMF
What is a hydrogen bond

A

Strong dipole dipole interaction between a hydrogen atom and a lone pair of electrons on a highly electronegative atom

122
Q

Polarity and electronegativity and IMf
What are the highly electronegative atoms which form hydrogen bonds

A

NOF
Nitrogen
Oxygen
Fluorine

123
Q

Polarity and electronegativity and IMF
Which are hydrogen bonded HF, HCl, N2O, H2O, NH3 and PH3

A

HF NH3 H2O

124
Q

Polarity and electronegativity and IMF
What is see to show a hydrogen bond in a diagram and why

A

A dashed line to show the weakness of the iMF

125
Q

Polarity and electronegativity and IMF
What has to be shown on a diagram of a hydrogen bond

A

Dipoles (delta + and - )
Lone pairs
Hydrogen bonds

126
Q

Polarity and electronegativity and IMF
What is commonly lot marks for on a diagram with hydrogen bonds

A

Hydrogen has to come from between a lone pair of electrons

127
Q

Polarity and electronegativity and IMF
What are the effects of hydrogen bonding on the properties of substances

A

Soluble in water and have higher boiling and freezing point than molecules of a similar size which are unable to form hydrogen bond

128
Q

Polarity and electronegativity and IMF
Why do molecules with hydrogen bonds often have higher melting and boiling points

A

More energy’s required to overcome hydrogen bonds

129
Q

Polarity and electronegativity and IMF
What are the anomalous properties of water

A

Ice is less dense than water
Relatively high melting and boiling points

130
Q

Polarity and electronegativity and IMF
Reason for ice being less dense than water

A

Hydrogen bonds hold the molecule in an open lattice structure

131
Q

Polarity and electronegativity and IMF
Reason for relatively high melting and boiling point of water

A

Hydrogen bonds are the strongest of the IMF so need more energy to overcome and desperate the molecules

132
Q

Polarity and electronegativity and IMF
What is the main factor that determine the boiling point of a substance

A

Strength of the induced dipole dipole forces unless it can form hydrogen bonds

133
Q

Polarity and electronegativity and IMF
Explanation for why the boiling points if the group 7 increase from HCl to HI

A

Although he permanent dipole dipole interactions are decreasing, the number of electrons in the molecule increases so the strength of the London forced increases

134
Q

Polarity and electronegativity and IMF
What is true if two molecules have a similar number of electrons but one is more polar

A

Strength of the London forces will be similar but the more polar one will have stronger permanent dipole dipole interaction so a higher boiling point

135
Q

Polarity and electronegativity and IMF
Explanation for simple covalent compound have low melting and boiling points

A

IMF that hold the molecules in the structure are weak so don’t need much energy to break so the melting points are normally low and often liquids or gases at room temperature

136
Q

Polarity and electronegativity and IMF
Explanation for why polar molecules are soluble in water

A

What is a polar molecule so only tends a to dissolve other polar substances. Compounds won’t hydrogen bonds such as ammonia can form hydrogen bond with water molecules so will be soluble

137
Q

Polarity and electronegativity and IMF
Are molecules that only have London forces soluble

A

No such as methane

138
Q

Polarity and electronegativity and IMF
Explanation for why simple covalent compound don’t conduct electricity

A

Even though some have permanent dipoles, overall covalent molecules are uncharged which means they can’t conduct electricity

Alevel Chemistry OCR A (18 decks)

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