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Chemistry > Bonding and Structure > Flashcards

Bonding and Structure Flashcards

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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
Q

Name three properties of ionic compounds

A

-High melting and boiling points
-Conduct electricity when molten or in a solution but not when solid
-Soluble in water

26
Q

Why do ionic compounds have a high melting, boiling point

A

A lot of energy is required to break the strong ionic bonds (electrostatic attraction) between the ions in the giant structure

27
Q

Why do ionic compounds conduct when molten or in a solution but not when solid

A

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
Q

Name the properties of molecular covalent compounds

A

-Low melting and boiling points
-Doesn’t conduct electricity
-Low solubility in water but dissolves in solvents

29
Q

Why molecular covalent compounds have a low melting boiling point

A

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
Q

Why do molecular covalent compounds not conduct electricity

A

The molecules are neutral and therefore they have no free electrons or ions to move and carry charge

31
Q

What is an allotrope

A

Are different forms of the same element in the same state

32
Q

What are the allotropes of carbon

A

diamond graphite graphene

33
Q

The structure of Diamond

A

Millions of covalent bonds. Each carbon atom is covalently bonded to 4 others in a tetrahedral arrangement in a giant covalent structure

34
Q

The structure of graphite

A

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
Q

The structure of graphene

A

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
Q

What are the properties of diamond

A

-Very high melting point
-Insoluble water
-Does not conduct
-Hard
-Used in cutting tools and drill bits

37
Q

What are the properties of graphite

A

-Very high melting point
-Insoluble in water
-Good conductor
-Soft
-Used for lubricants for machinery and in pencil leads

38
Q

What are the properties of graphene

A

-Very high melting point
-All insoluble in water
-Good conductor
-Very strong
-Used in solar cells and batteries of the future

39
Q

Why do diamond, graphite and graphene have a high melting point

A

A lot of energy is required to break the strong covalent bonds between the atoms in the giant structure

40
Q

Why does diamond not conduct

A

All outer electrons are bonded there are no free ions or electrons to move and carry charge

41
Q

Why are graphite and graphene good conductors

A

One outer electron per atom is unbonded this electron is delocalised and free to move and carry charge

42
Q

Why is graphene a better conductor than graphite

A

The 2D structure offers little resistance to the flow of electrons

43
Q

Why is diamond hard

A

Due to the 3D tetrahedral structure with strong covalent bonds throughout

44
Q

Why is graphite soft

A

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
Q

Why is graphene strong

A

Due to the strong covalent bonds within the layer structure

46
Q

Metallic Structure

A

-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
Q

Name the properties of metals and alloys

A

-Usually high melting and boiling point
-Conduct electricity
-Malleable and ductile

48
Q

Why do metals and alloys have a high melting and boiling point

A

A lot of energy is required to break the strong metallic bonds between the positive ions and delocalised electrons in the giant structure

49
Q

Why do metals and alloys conduct electricity

A

Contain delocalised electros which move and carry charge

50
Q

Why are metals and alloys malleable and ductile

A

The layers of ions can slide over each other without the metallic bonds breaking as the delocalised electrons still attract the ions

51
Q

How to calculate the % of gold in alloy

A

(number of carats X100) divided by 24

52
Q

What is the use and purpose of Stainless steel

A

Sinks and cutlery and it is alloyed as it is more resistant to rusting

53
Q

What is the use and purpose of solder

A

Soldering joints and it is alloyed as it lowers the melting point

54
Q

What is the use and purpose of brass

A

For decorative work and it is alloyed as it has a nice colour and is hard

55
Q

What is use and purpose of 18 carat gold

A

Jewellery and is alloyed for harder wearing

Chemistry (5 decks)

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