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A-Level Chemistry COPY > Bonding > Flashcards

Bonding Flashcards

(70 cards)

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1
Q

What is ionic bonding?

A

The electrostatic force of attraction between oppositely charged ions

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2
Q

How are ions formed?

A

Ions are formed when atoms lose or gain electrons

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3
Q

What type of ions do metals form?

A

Positive ions because they lose electrons

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4
Q

What type of ions do non-metals form?

A

Negative ions because they gain electrons

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5
Q

What are compound ions?

A

Ions made up of a group of atoms with an overall charge

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6
Q

What is the structure of ions?

A

They have a giant ionic lattice

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7
Q

What are the properties of ionic compounds?

A

They have:

  • high melting points
  • conduct electricity when molten or dissolved
  • tend to dissolve in water
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8
Q

How would you prove if a substance is ionic?

A
  • dissolve the substance in water
  • add a cathode and anode into the solution with a bulb in the circuit
  • if the solution conducts electricity(bulb switches on), then it is ionic
  • if insoluble melt the substance
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9
Q

How would you determine which ionic compound has a higher melting point?

A

Charge determines which ionic compound has a higher melting point, not the size

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10
Q

What happens down the group as the ions become larger?

A

Charge density decreases

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11
Q

What is charge density?

A

The ratio of the charge of an ion to its volume

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12
Q

Which are the five common compound ions?

A 
sulfate-SO4^2-
hydroxide-OH-
nitrate-NO3-
carbonate-CO3^2-
ammonium-NH4+
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13
Q

What is a covalent bond?

A

A single shared pair of electrons

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14
Q

What is the structure of diamond?

A

Giant covalent
Tetrahedral
Carbon makes 4 covalent bonds

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15
Q

What are the properties of diamond?

A

Very high melting point
Hard
insoluble
Non-conductor of electricity(the outer electrons are held in localised bonds)

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16
Q

What is the structure of graphite?

A

Giant covalent
Planar- arranged in layers
Carbon makes 3 covalent bonds

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17
Q

What are the properties of graphite?

A

High melting point
Conducts electricity(each carbon has one delocalised electron)
Slippery-the layers can slide over each other easily
(used in pencils and as a dry lubricant)
Soft
Insoluble

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18
Q

Which forces bond together the layers of graphite?

A

Weak van der Waals forces

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19
Q

What is the structure of iodine?

A

Molecular covalent

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20
Q

What are the properties of iodine?

A

Low boiling and melting point

Poor conductor of electricity(no charged particles)

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21
Q

What is dative covalent bonding?

A

A covalent bond where both of the shared pair of electrons come from one atom

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22
Q

What are the common examples of dative covalent bonding?

A

NH4+
H3O+
NH3BF3

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23
Q

What is metallic bonding?

A

The electrostatic force of attraction between the positive metal ions and the delocalised electrons

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24
Q

What is the structure of metallic bonding?

A

A giant metallic lattice

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25
What are the properties of metals?
High melting point Good thermal and electrical conductors Soft, ductile and malleable Arranged in layers
26
How does the number of delocalised electrons per atom affect the melting point?
The more delocalised electrons there are per atom, the stronger the bonding and the higher the melting point
27
What happens to the metallic bonding strength going down a group?
Going down a group, the ions become larger, the charge density decreases and the weaker the metallic bonding
28
How many bonding and lone pairs are there in a LINEAR molecule and what is the bond angle of the molecule?
Bonding pairs - 2 Lone pairs - 0 Bond angle - 180
29
How many bonding and lone pairs are there in a TRIGONAL PLANAR molecule and what is the bond angle of the molecule?
Bonding pairs - 3 Lone pairs - 0 Bond angle - 120
30
How many bonding and lone pairs are there in a TETRAHEDRAL molecule and what is the bond angle of the molecule?
Bonding pairs - 4 Lone pairs - 0 Bond angle - 109.5
31
How many bonding and lone pairs are there in a TRIGONAL PYRAMID molecule and what is the bond angle of the molecule?
Bonding pairs - 3 Lone pairs - 1 Bond angle - 107
32
How many bonding and lone pairs are there in a BENT(angular, V-shaped, non-linear) molecule and what is the bond angle of the molecule?
Bonding pairs - 2 Lone pairs - 2 Bond angle - 104.5
33
How many bonding and lone pairs are there in a TRIGONAL BIPYRAMID molecule and what are the bond angles of the molecule?
Bonding pairs - 5 Lone pairs - 0 Bond angles - 120 and 90
34
How many bonding and lone pairs are there in an OCTRAHEDRAL molecule and what is the bond angle of the molecule?
Bonding pairs - 6 Lone pairs - 0 Bond angle - 90
35
How many bonding and lone pairs are there in a SEESAW molecule and what is the bond angle of the molecule?
Bonding pairs - 4 Lone pairs - 1 Bond angle - 117.5-120 and 87-88
36
How many bonding and lone pairs are there in a T-SHAPED molecule and what is the bond angle of the molecule?
Bonding pairs - 3 Lone pairs - 2 Bond angle - 88
37
How many bonding and lone pairs are there in a SQUARE PLANAR molecule and what is the bond angle of the molecule?
Bonding pairs - 4 Lone pairs -2 Bond angle 90
38
What type of repulsion is the greatest creating the biggest bond angles?
Lone pair-lone pair repulsion
39
What type of repulsion is the smallest creating the smallest bond angles?
Bonding pair-bonding pair repulsion
40
By how much do lone pairs reduce bond angles?
2.5 degrees per lone pair
41
What is electronegativity?
The ability of an atom to attract the pair of electrons in a covalent bond towards itself
42
Which is the most electronegative element?
Fluorine
43
Why is fluorine the most electronegative element?
It is the smallest atom with the most need to fill its outer shell it has the least number of shells and electrons
44
What is a polar bond?
A bond where a bonding pair is shared unequally and there are partial charges on the atoms in the bond
45
What is a dipole?
A difference in charge between two atoms caused by a shift in electron density in the bond
46
Why are symmetrical molecules not polar?
The dipoles cancel out and there is no permanent dipole
47
What is a permanent dipole?
It is the unequal sharing of electrons in a covalent bond leading to partial charged due to the difference in electronegativity
48
What are intermolecular forces?
Forces between molecules
49
What are the three intermolecular forces?
Van der Waals forces Permanent dipole-dipole Hydrogen bonding
50
What are van der Waals forces?
They are found between all atoms and molecules They cause atoms and molecules to be attracted to each other Weakest intermolecular forces
51
What affects the magnitude of the van der Waals forces?
The number of electrons | The shape of the molecule
52
How does the number of electrons affect the size of the van der Waals forces?
As the number of electrons increases, the larger the molecule and therefore the stronger the van der Waals forces
53
How does the shape of the molecule affect the van der Waals forces?
Long straight molecules have a larger surface area of contact and therefore the stronger the forces between them
54
What are permanent dipole-dipole forces?
They occur between polar molecules which have a permanent dipole They are stronger than van der Waals forces
55
What would happen if you placed a charged rod next to a jet of a polar liquid?
The liquid will move towards the rod
56
Why would the liquid move towards the rod?
The polar liquid contains molecules with permanent dipoles It doesn't matter if the rod is positively or negatively charged because the polar molecules can turn around so that the oppositely charged end is attracted towards the rod
57
What is hydrogen bonding?
It occurs only when hydrogen is covalently bonded to nitrogen, oxygen and fluorine It is the strongest intermolecular force
58
Why does hydrogen bonding only occur when hydrogen is covalently bonded to nitrogen, oxygen and fluorine?
They are very electronegative compared to hydrogen
59
What are the properties of substances with hydrogen bonding?
They have higher melting and boiling points compared to similar molecules because extra energy is needed to break the hydrogen bonds
60
What happens as water cools to form ice?
The molecules make more hydrogen bonds and arrange themselves into a regular lattice
61
Why does ice float?
In the regular structure, the molecules are further apart and therefore, ice is less dense than liquid water
62
What determines the melting and boiling points of a substance?
The strength of the attraction between its particles
63
What are the properties of ionic bonding?
``` High melting and boiling points Solid at room temperature Don't conduct electricity when solid Conduct electricity when molten or dissolved Soluble in water ```
64
What are the properties of simple covalent bonding?
Low melting and boiling points Can be solid but usually liquid or gas at room temperature Don't conduct electricity when a solid or liquid Solubility in water depends on the polarity of the molecule
65
What are the properties of giant covalent bonding?
High melting and boiling points Solid at room temperature Don't conduct electricity except graphite Insoluble
66
What are the properties of metallic bonding?
High melting and boiling points Solid at room temperature Conduct electricity as a solid and molten Insoluble
67
What are the physical properties of solids?
The particles are very close together High density which makes solids incompressible The particles vibrate about a fixed point as they can't move freely
68
What are the physical properties of liquids?
Similar density to a solid which makes liquids incompressible The particles vibrate freely and randomly within the liquid allowing it to flow
69
What are the physical properties of gases?
The particles have more energy and are further apart The density is low which makes gases very compressible The particles move freely and diffuse.
70
Describe the bonding between hydrogen chloride molecules
The delta negative charge on the chlorine would be attracted to the delta positive charge on the hydrogen on the next molecule

A-Level Chemistry COPY (30 decks)

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