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Bonding Flashcards

(64 cards)

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1
Q

What happens when atoms bond together

A

They share or transfer electrons to achieve a more stable electron arrangement

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2
Q

Where do ionic bonds occur

A

Between metals and non-metals

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3
Q

What happens to the electrons in an ionic bond

A

They are transferred from metal atoms to non-metal atoms

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4
Q

What is formed in ionic bonds

A

Positive and negative ions

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5
Q

Why are the ions in ionic bonding attracted to eachother

A

Through electrostatic forces

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6
Q

What is a lattice

A

Ionic compounds always exist in a lattice- electrostatic attraction extends throughout the compound

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7
Q

What state are ionic compounds in at room temperature

A

Solid

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8
Q

Why do ionic compounds have high melting points

A

They are giant structures so a lot of energy is needed to break up the lattice of ions in order to melt the compound

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9
Q

Do ionic compounds conduct electricity?

A

When they are molten or dissolved in water but not when solid- the ions that carry current can move in liquid state but not is solid state

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10
Q

What are the physical features of an ionic compound

A

They are brittle and shatter easily because they form a lattice of alternating positive and negative ions

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11
Q

What does a covalent bond form between

A

A pair of non-metal atoms

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12
Q

What happens during a covalent bond

A

The atoms share some of their outer electrons so each atom has a stable noble gas arrangement

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13
Q

What is a molecule

A

A small group of covalently bonded atoms

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14
Q

How does sharing electrons hold atoms together

A

They are held together by the electrostatic attraction between the nuclei and the shared electrons- this takes place within the molecule

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15
Q

What is a double covalent bond

A

Four electrons are shared

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16
Q

Why do substances made of molecules have a low melting temperature

A

The strong covalent bonds are only between the atoms within the molecules, there is only weak attraction between the molecules so they don’t need much energy to move apart

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17
Q

Are covalently bonded structures good conductors

A

No because the molecules are neutral so there are no charged particles to carry the current,
Also not conductors when dissolved

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18
Q

What is a co-ordinate bond/dative covalent bond

A

When one atom provides both the electrons

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19
Q

What happens during a co-ordinate bond

A

The atoms that donates the electrons has a lone pair that is donates to the electron deficient atom

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20
Q

What happens during metallic bonding

A

The outer main levels of the atoms merge, the outer electrons are no longer associated with a particular atom which creates a lattice of positive ions in a ‘sea’ of delocalised electrons

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21
Q

Why are metals good conductors of electricity and heat

A

The delocalised electrons can move through the structure so can carry an electrical current across- an electrons joins at the negative terminal while at the same time a different electron leaves the wire at the positive terminal,
They can also conduct heat because the sea of electrons spreads increasingly vigorous vibrations

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22
Q

What does the strength of a metallic bond depend on

A

The charge on the ion- greater charge means more delocalised electrons and stronger electrostatic attraction
The size of the ion, smaller ions mean the electrons are closer to the positive nucleus so the bond is stronger

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23
Q

What are some other properties of metals

A

They are malleable and ductile (can be beaten into shape and pulled into thin wires)
Because after the distortion each metal ion is still in the same environment as before so the new shape is retained

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24
Q

Melting point of metals

A

High melting and boiling points because they have giant structures and there is a strong attraction between the metal ions and the electrons

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25
What is electronegativity
The power of an atom to attract the electron density in a covalent bond towards itself
26
What is the Pauling scale
It measures electronegativity, it runs from 0 to 4 and the greater the number, the more electronegative the atom
27
What does electronegativity depend on
The nuclear charger, The distance between the nucleus and the outer shell electrons The shielding of the nuclear charger by electrons in inner shells
28
Why do smaller atoms have greater electronegativity
The nucleus is closer to the shared outer main level electrons
29
What are the trends in negtivity
It increases going up the periodic table (less shielding), It increases going across a period in the periodic table (nuclear charge increases)
30
What is polarity
The unequal sharing of the electrons between atoms that are covalently bonded
31
What is the polarity between covalently bonded atoms that are the same
The electrons are shared equally as the electronegativity is the same so they are non-polar
32
What is the polarity between covalently bonded atoms that are not the same
The bond will not be shared equally, the electron pair will be attracted towards the more electronegative atom, These bonds are polar
33
What is a dipole moment
A measure of separation of charge between the slightly positive and slightly negative ends of a polar bond
34
What are dipole-dipole forces
They act between molecules that have permanent dipoles, two molecules that both have dipoles will attract one another
35
What are van der Waals forces
All atoms and molecules are made up of positive and negative charges, even though they are overall neutral, These charges produce very weak electrostatic attractions between all atoms and molecules
36
When does the size of the van der Waals forces increase
When there are more electrons present, so atoms or molecules with large atomic or molecular masses produce stronger van der Waals forces
37
What is hydrogen bonding
A type of permanent dipole-dipole force that forms when a hydrogen forms a covalent bond with a very electronegative element; either nitrogen, oxygen or fluorine
38
Why are hydrogen bonds important
They are not very strong bond by themselves but when there are a lot of them their effect can be very significant
39
Why is ice less dense than water
When water freezes, the water molecules are no longer free to move about and the hydrogen bonds hold the molecules in fixed positions- to fit into the structure the molecules are slightly less closely packed that in water so it forms on top of ponds rather than at the bottom- insulating them
40
What happens first when you heat a solid
They vibrate more in their fixed position which increased the distance between the particles so the solid expands
41
How do you turn a solid to a liquid
Supply more energy to weaken the forces between the particles
42
What is the enthalpy change of melting
The energy needed to melt a solid
43
What is the enthalpy change of vaporisation
The energy needed to turn a liquid into a solid
44
Is there a temperature change when a substance changes state
No because all the energy is absorbed as the forces are weakened
45
What is a crystal
Solids that have a regular arrangement and are held together by forces of attraction
46
Ionic crystals
Ionic compounds have strong electrostatic attractions so have high melting points
47
Molecular crystals
Molecules held in a regular array by intermolecular forces, covalent bonds within the molecules hold the atoms together but don't act between the molecules, Intermolecular forces are between them but they are much weaker then ionic, covalent or metallic so molecular crystals have a low melting point
48
Macromolecular crystals
When covalent bonds extend throughout the compound, they have the typical property of a giant structure (high melting temperature)
49
Diamond
Pure carbon with covalent bonding between every carbon atom, the bonds spread throughout the structure,
50
Why is diamond so strong
Each atom is in an identical position, surrounded by four other carbon atoms, it forms a giant 3d lattice
51
Structure of Graphite
Consists of pure carbon, Each carbon forms three single covalent bonds to other carbon atoms, These form a flat trigonal arrangement with a bond angle 120, leaving a spare electron, These electrons can move anywhere withing the layer,
52
Can graphite conduct electricity
Yes because of the delocalised electrons, but it can only conduct along the hexagonal planes
53
How are layers of graphite held together
Van der Waals forces are between the layers, they are very weak which allows the layers to slide across one another
54
What is a giant football
Another form of pure carbon, include closed cages of carbon atoms and nanotubes
55
What property is the best indicator of the type of bonding
Electrical conductivity, Metal= good conductor Ionic= only good conductor as a liquid Covalent= generally bad conductor
56
What indicates if a structure is giant or simple molecular
Melting/Boiling point Simple= low Giant= high
57
What is the electron pair repulsion theory
Each pair of electrons around an atom will repel all other electron pairs, The pairs of electrons will therefore take up position as far apart as possible to minimise repulsion
58
What is the name and bond angle of two pairs of electrons
Linear and 180
59
What is the name and bond angle of three pairs of electrons
Trigonal planar and 120
60
What is the name and bond angle of four pairs of electrons
Tetrahedral and 109.5
61
What is the name and bond angle of five pairs of electrons
Trigonal bipyramidal and 90 and 120
62
What is the name and bond angle of six pairs of electrons
Octahedral and 90
63
What happens to the repulsion of a lone pair
The repulsion between a lone pair of electrons and a bonding pair is greater than between two bonding pairs
64
What effect does a lone pair have on bond angles
It reduces the angles by about 2 degrees

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