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Chemistry > Bonding and Structure > Flashcards

Bonding and Structure Flashcards

1
Q

Ion

A

A charged particle formed when an atom loses or gains electrons

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2
Q

Molecular ion

A

A charged particle containing more than one atom

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3
Q

Cation

A

A positive ion

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4
Q

Anion

A

A negative ion

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5
Q

Electrostatic attraction

A

An attractive force which 2 unlike charges exert on each other when they are kept some finite distance apart

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6
Q

Molecule

A

A particle that consists of two or more atoms chemically bonded together

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7
Q

Diatomic molecule

A

Two atoms covalently bonded in a molecule

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8
Q

Allotrope

A

Different forms of the same element in the same state

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9
Q

Covalent bond

A

Formed by a shared pair of electrons

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10
Q

Ionic bond

A

The attraction between oppositely charged ions

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11
Q

Van der waal’s forces

A

Weak intermolecular forces which exist between covalently bonded molecules

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12
Q

Metallic bond

A

The attraction between delocalised electrons and the positive ions in a regular lattice

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13
Q

Delocalised electrons

A

Electrons that are free to move throughout the whole structure

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14
Q

Malleable

A

Can be hammered into shape

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15
Q

Ductile

A

Can be drawn out into wires

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16
Q

Alloy

A

A mixture of two or more elements at least one of which is a metal and the resulting mixture has metallic properties

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17
Q

Bonding

A

Describes how atoms or ions are held together

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18
Q

Structure

A

Describes how atoms or ions are arranged in space

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19
Q

Describe Ionic bonding

A

-Happens between metals and non-metals
-In Ionic bonding atoms will lose or gain electrons to have full outer shells
-Ions are produced
-The oppositely charged ions attract each other

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20
Q

Describe Covalent bonding

A

-Involves sharing of electron pairs usually one electron from each atom
-Takes place in non metal elements and compounds of non metal elements
-Produces uncharged molecules
-Shared electrons are counted as outer shell electrons for both atoms

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21
Q

What is a lone pair

A

Pairs of electrons in the outer shell which are not used up in bonding

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22
Q

Metallic bonding

A

-Occurs between metal elements and alloys
-Metallic bonding is the attraction between delocalised electrons and the positive ions in a regular lattice
The outer electrons are delocalized

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23
Q

What is the ionic bonding structure

A

Giant Ionic Lattice

24
Q

What is an ionic lattice

A

A 3D structure of oppositely charged ions held together by electrostatic forces of attraction called ionic bonds

25
Name three properties of ionic compounds
-High melting and boiling points -Conduct electricity when molten or in a solution but not when solid -Soluble in water
26
Why do ionic compounds have a high melting, boiling point
A lot of energy is required to break the strong ionic bonds (electrostatic attraction) between the ions in the giant structure
27
Why do ionic compounds conduct when molten or in a solution but not when solid
An electric flow of charged particles(either electrons or ions). Ions are free to move and carry charge when compound is a liquid or solution but not when it is solid
28
Name the properties of molecular covalent compounds
-Low melting and boiling points -Doesn't conduct electricity -Low solubility in water but dissolves in solvents
29
Why molecular covalent compounds have a low melting boiling point
Little energy is required to break the weak van der waal's forces between the molecules. The strong covalent bonds in the molecule don't break
30
Why do molecular covalent compounds not conduct electricity
The molecules are neutral and therefore they have no free electrons or ions to move and carry charge
31
What is an allotrope
Are different forms of the same element in the same state
32
What are the allotropes of carbon
diamond graphite graphene
33
The structure of Diamond
Millions of covalent bonds. Each carbon atom is covalently bonded to 4 others in a tetrahedral arrangement in a giant covalent structure
34
The structure of graphite
Each carbon atom is covalently bonded to three others in hexagonal rings producing layers of carbon atoms with weak van der waal forces of attraction between the layers it has a giant structure containing millions of carbon atoms
35
The structure of graphene
A single atom thick layer of graphite with strong covalent bonds between each carbon atom the atoms are arranged in hexagons it is considered a 2D giant covalent structure
36
What are the properties of diamond
-Very high melting point -Insoluble water -Does not conduct -Hard -Used in cutting tools and drill bits
37
What are the properties of graphite
-Very high melting point -Insoluble in water -Good conductor -Soft -Used for lubricants for machinery and in pencil leads
38
What are the properties of graphene
-Very high melting point -All insoluble in water -Good conductor -Very strong -Used in solar cells and batteries of the future
39
Why do diamond, graphite and graphene have a high melting point
A lot of energy is required to break the strong covalent bonds between the atoms in the giant structure
40
Why does diamond not conduct
All outer electrons are bonded there are no free ions or electrons to move and carry charge
41
Why are graphite and graphene good conductors
One outer electron per atom is unbonded this electron is delocalised and free to move and carry charge
42
Why is graphene a better conductor than graphite
The 2D structure offers little resistance to the flow of electrons
43
Why is diamond hard
Due to the 3D tetrahedral structure with strong covalent bonds throughout
44
Why is graphite soft
The layers of carbon atoms can slide over each other as the weak van der waal forces between the layers are easy to break
45
Why is graphene strong
Due to the strong covalent bonds within the layer structure
46
Metallic Structure
-High density as the ions are tightly packed in a small space -Quite hard as the metallic bond requires a lot of energy to break
47
Name the properties of metals and alloys
-Usually high melting and boiling point -Conduct electricity -Malleable and ductile
48
Why do metals and alloys have a high melting and boiling point
A lot of energy is required to break the strong metallic bonds between the positive ions and delocalised electrons in the giant structure
49
Why do metals and alloys conduct electricity
Contain delocalised electros which move and carry charge
50
Why are metals and alloys malleable and ductile
The layers of ions can slide over each other without the metallic bonds breaking as the delocalised electrons still attract the ions
51
How to calculate the % of gold in alloy
(number of carats X100) divided by 24
52
What is the use and purpose of Stainless steel
Sinks and cutlery and it is alloyed as it is more resistant to rusting
53
What is the use and purpose of solder
Soldering joints and it is alloyed as it lowers the melting point
54
What is the use and purpose of brass
For decorative work and it is alloyed as it has a nice colour and is hard
55
What is use and purpose of 18 carat gold
Jewellery and is alloyed for harder wearing

Chemistry (5 decks)

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