ionic plus covalent bonding particle model etc

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100 Terms

1
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what is an ion?

a charged particle formed by the gain or loss of electrons

2
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all metals ____ electrons to become _____ly charged ions

lose, positive

3
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all non metals ____ electrons to become ____ly charged ions

gain, negative

4
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what is ionic bonding?

transfer of electrons from a metal to a non metal to form a positively charged metal ion and a negatively charged non metal ion

5
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what holds ionic compounds together?

the positive and negative charges are held together by the strong electrostatic forces of attraction that act in all directions

6
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what are the structures of ionic compounds?

they are composed of 100s of ions both positive and negative, held together by strong electrostatic forces, this forms 3D structures called a giant lattice structure

7
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how can ionic compounds be represented?

using a ball and stick diagram

8
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what are the properties of ionic compounds?

- can only conduct electricity when melted or dissolved in water as the ions are free to move/ flow and are no longer fixed

- very high melting point as lots of energy is needed to overcome the electrostatic forces of attraction

9
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how does metallic bonding work?

each metal atom donates its outer electron to become a positively charged ion and these electrons are free to move creating a sea of electrons. The metallic bond is the electrostatic force of attraction between these positive metal ions and the negative electrons. This holds the metal together in a regular lattice structure

10
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what are alloys?

a mixture of two or more elements containing at least one metal

11
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why are alloys stronger than regular metals?

the different sized atoms disrupt the regular structure/causes distorted layers so the layers can no longer slide over each other so it’s stronger

12
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why do metals with a greater number of outer electrons have a higher melting point?

This is due to the increased positive charge on the metal ion and the increased number of electrons that are delocalised, resulting in stronger bonding.

13
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how do metals conduct electricity

their outer electrons of each metal atom are delocalised so they are free to flow within the structure and carry charge

14
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what is covalent bonding?

a shared pair of electrons between two non metal atoms

15
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what are polymers?

long chains made up of large repeating units called monomers

16
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are polymers solid at room temperature?

yes as the molecules are really big, so the intermolecular forces add up to be quite strong, however most polymers melt easily as the intermolecular forces remain less strong than the chemical bonds

17
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do covalent structures conduct electricity? explain your answer

no as they have no free electrons and they don’t have any charged particles( except graphite)

18
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why do simple covalent structures have a low melting point?

because they have small molecules causing them to have weak intermolecular forces so little energy is needed to overcome these

19
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do giant covalent structures have intermolecular forces?

no as it’s just one giant molecule

20
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why do giant covalent structures have high melting points?

because it takes a lot of energy to break all the strong covalent bonds between the atoms in the structure

21
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what are allotropes?

different structural forms of the same element in the same physical state

22
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what are the allotropes of carbon?

- diamond

- graphite

- graphene

- buckminsterfullerene

23
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what is the structure of diamond?

each carbon atom is covalently bonded to 4 other carbon atoms

24
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what are the properties of diamond?

- can’t conduct electricity as it has no free electrons or ions

- high melting point

- strong

25
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what is the structure of graphite?

each carbon atom is covalently bonded to three others, the atoms are arranged in hexagons that form flat sheets that form layers on top of each other

26
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what are the properties of graphite?

- slippery

- can conduct electricity

- high melting point

27
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why is graphite slippery?

they have layers that are held together by weak intermolecular forces as there are no covalent bonds between them so they can slide over each other making graphite soft and be used in pencil lead

28
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why can graphite conduct electricity?

because each carbon atom is only bonded to three others, and carbon can make 4 covalent bonds, so there’s a carbon atom that isn’t bonded, so there’s a delocalised electron that is free to flow and carry charge through the structure and conduct electricity

29
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what is graphene?

a singular layer of graphite

30
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how are fullerenes such as nanotubes made?

made by bending sheets of graphene

31
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what are fullerenes?

molecules of carbon with hollow shapes

32
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what is buckminsterfullerene?

C60 first fullerene to be discovered, spherical

33
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uses of fullerenes

- industrial catalysts (spherical)

- transporting drugs into the body (spherical)

- electronics (cylindrical)

- strengthening materials eg. in tennis rackets

- lubricants (spherical)

34
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what are the uses of nanoparticles

- silver nanoparticles have antibacterial properties so we can infuse them into surgical masks and wound dressings as they are lightweight as well

- catalysts due to their high surface area: volume ratio

- conducting electricity

- deodrants

- sunscreens

35
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what are the issues with using nanoparticles

- the use of nanoparticles is in ealry stages so we don’t know its long term effects on the human body ( if used in sunscreams for example)

- we don’t know if they damage the environment when they’re disposed of

- they aren’t easily disposed of

36
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what are the advantages of a dot and cross diagram?

- useful for illustrating the transfer of electrons

- indicates from which atom the bonding electrons come from

37
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what are the disadvantages of a dot and cross diagram?

- doesn’t indicate the relative sizes of atoms

- doesn’t illustrate the 3D arrangements of the atoms and electron shells

38
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what are the advantages of a ball and stick model?

- useful for illustrating the arrangement of atoms in 3D space

- useful for visualizing the shape of a molecule

39
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what are the disadvantages of a ball and stick model?

- doesn’t show movement of electrons

- gives no information about the forces of attraction between the ions

- the atoms are placed far apart from each other, which in reality is not the case as the gaps between the atoms are much smaller

40
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what are the advantages of 2D models?

- , shows what atoms are in a molecule and how they’re connected

- simpler versions of the ball and stick model

41
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what are the disadvantages of 2D models?

- fails to illustrate the relative sizes of the atoms and bonds

- can’t give you an idea of the shape of a molecule and what it looks like in 3D space

42
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describe the structure of a solid

strong forces of attraction holds the particles close together to form a regular lattice structure

definite shape and volume

can’t be compressed

strong forces of attraction

43
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what happens when a solid is heated

particles gain kinetic energy and vibrate more weakening the bonds between them until the melting point is reached and the particles gain enough energy to break free of their bonds

—>liquid

44
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describe the structure of a liquid

free to move

shape can flow to fit a container

definite volume

weak forces of attraction

45
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what happens when a liquid is heated

the particles gain more kinetic energy and move around faster/vibrate and slide over each other weakening the forces between them until boiling point is reached and the bonds are broken and the liquid evaporates into a gas

46
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describe the strucuture of a gas

free to move

no definite shape or volume

very weak forces of attraction

constantly move with random motion

47
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what happens when a gas is heated

if it’s in an expandable container the gas will expand

if it’s in a fixed container the pressure will increase

48
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what happens when a gas is cooled down

won’t have enough energy to overcome bonds as energy is transferred to the surroundings so bonds will form again and it will condense into a liquid

49
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what happens when a liquid cools down

energy from the liquid is transferred to the surroundings and so it won’t have enough energy to overcome the forces of attraction between the bonds/particles and it will freeze into a solid fixing the particles in place

50
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what are the limitations of the particle model

particles aren’t solid since atoms are mostly empty space

many particles aren’t spherical

51
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what is an ion?

a charged particle formed by the gain or loss of electrons

52
New cards

all metals ____ electrons to become _____ly charged ions

lose, positive

53
New cards

all non metals ____ electrons to become ____ly charged ions

gain, negative

54
New cards

what is ionic bonding?

transfer of electrons from a metal to a non metal to form a positively charged metal ion and a negatively charged non metal ion

55
New cards

what holds ionic compounds together?

the positive and negative charges are held together by the strong electrostatic forces of attraction that act in all directions

56
New cards

what are the structures of ionic compounds?

they are composed of 100s of ions both positive and negative, held together by strong electrostatic forces, this forms 3D structures called a giant lattice structure

57
New cards

how can ionic compounds be represented?

using a ball and stick diagram

58
New cards

what are the properties of ionic compounds?

- can only conduct electricity when melted or dissolved in water as the ions are free to move/ flow and are no longer fixed

- very high melting point as lots of energy is needed to overcome the electrostatic forces of attraction

59
New cards

how does metallic bonding work?

each metal atom donates its outer electron to become a positively charged ion and these electrons are free to move creating a sea of electrons. The metallic bond is the electrostatic force of attraction between these positive metal ions and the negative electrons. This holds the metal together in a regular lattice structure

60
New cards

what are alloys?

a mixture of two or more elements containing at least one metal

61
New cards

why are alloys stronger than regular metals?

the different sized atoms disrupt the regular structure/causes distorted layers so the layers can no longer slide over each other so it’s stronger

62
New cards

why do metals with a greater number of outer electrons have a higher melting point?

This is due to the increased positive charge on the metal ion and the increased number of electrons that are delocalised, resulting in stronger bonding.

63
New cards

how do metals conduct electricity

their outer electrons of each metal atom are delocalised so they are free to flow within the structure and carry charge

64
New cards

what is covalent bonding?

a shared pair of electrons between two non metal atoms

65
New cards

what are polymers?

long chains made up of large repeating units called monomers

66
New cards

are polymers solid at room temperature?

yes as the molecules are really big, so the intermolecular forces add up to be quite strong, however most polymers melt easily as the intermolecular forces remain less strong than the chemical bonds

67
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do covalent structures conduct electricity? explain your answer

no as they have no free electrons and they don’t have any charged particles( except graphite)

68
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why do simple covalent structures have a low melting point?

because they have small molecules causing them to have weak intermolecular forces so little energy is needed to overcome these

69
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do giant covalent structures have intermolecular forces?

no as it’s just one giant molecule

70
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why do giant covalent structures have high melting points?

because it takes a lot of energy to break all the strong covalent bonds between the atoms in the structure

71
New cards

what are allotropes?

different structural forms of the same element in the same physical state

72
New cards

what are the allotropes of carbon?

- diamond

- graphite

- graphene

- buckminsterfullerene

73
New cards

what is the structure of diamond?

each carbon atom is covalently bonded to 4 other carbon atoms

74
New cards

what are the properties of diamond?

- can’t conduct electricity as it has no free electrons or ions

- high melting point

- strong

75
New cards

what is the structure of graphite?

each carbon atom is covalently bonded to three others, the atoms are arranged in hexagons that form flat sheets that form layers on top of each other

76
New cards

what are the properties of graphite?

- slippery

- can conduct electricity

- high melting point

77
New cards

why is graphite slippery?

they have layers that are held together by weak intermolecular forces as there are no covalent bonds between them so they can slide over each other making graphite soft and be used in pencil lead

78
New cards

why can graphite conduct electricity?

because each carbon atom is only bonded to three others, and carbon can make 4 covalent bonds, so there’s a carbon atom that isn’t bonded, so there’s a delocalised electron that is free to flow and carry charge through the structure and conduct electricity

79
New cards

what is graphene?

a singular layer of graphite

80
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how are fullerenes such as nanotubes made?

made by bending sheets of graphene

81
New cards

what are fullerenes?

molecules of carbon with hollow shapes

82
New cards

what is buckminsterfullerene?

C60 first fullerene to be discovered, spherical

83
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uses of fullerenes

- industrial catalysts (spherical)

- transporting drugs into the body (spherical)

- electronics (cylindrical)

- strengthening materials eg. in tennis rackets

- lubricants (spherical)

84
New cards

what are the uses of nanoparticles

- silver nanoparticles have antibacterial properties so we can infuse them into surgical masks and wound dressings as they are lightweight as well

- catalysts due to their high surface area: volume ratio

- conducting electricity

- deodrants

- sunscreens

85
New cards

what are the issues with using nanoparticles

- the use of nanoparticles is in ealry stages so we don’t know its long term effects on the human body ( if used in sunscreams for example)

- we don’t know if they damage the environment when they’re disposed of

- they aren’t easily disposed of

86
New cards

what are the advantages of a dot and cross diagram?

- useful for illustrating the transfer of electrons

- indicates from which atom the bonding electrons come from

87
New cards

what are the disadvantages of a dot and cross diagram?

- doesn’t indicate the relative sizes of atoms

- doesn’t illustrate the 3D arrangements of the atoms and electron shells

88
New cards

what are the advantages of a ball and stick model?

- useful for illustrating the arrangement of atoms in 3D space

- useful for visualizing the shape of a molecule

89
New cards

what are the disadvantages of a ball and stick model?

- doesn’t show movement of electrons

- gives no information about the forces of attraction between the ions

- the atoms are placed far apart from each other, which in reality is not the case as the gaps between the atoms are much smaller

90
New cards

what are the advantages of 2D models?

- , shows what atoms are in a molecule and how they’re connected

- simpler versions of the ball and stick model

91
New cards

what are the disadvantages of 2D models?

- fails to illustrate the relative sizes of the atoms and bonds

- can’t give you an idea of the shape of a molecule and what it looks like in 3D space

92
New cards

describe the structure of a solid

strong forces of attraction holds the particles close together to form a regular lattice structure

definite shape and volume

can’t be compressed

strong forces of attraction

93
New cards

what happens when a solid is heated

particles gain kinetic energy and vibrate more weakening the bonds between them until the melting point is reached and the particles gain enough energy to break free of their bonds

—>liquid

94
New cards

describe the structure of a liquid

free to move

shape can flow to fit a container

definite volume

weak forces of attraction

95
New cards

what happens when a liquid is heated

the particles gain more kinetic energy and move around faster/vibrate and slide over each other weakening the forces between them until boiling point is reached and the bonds are broken and the liquid evaporates into a gas

96
New cards

describe the strucuture of a gas

free to move

no definite shape or volume

very weak forces of attraction

constantly move with random motion

97
New cards

what happens when a gas is heated

if it’s in an expandable container the gas will expand

if it’s in a fixed container the pressure will increase

98
New cards

what happens when a gas is cooled down

won’t have enough energy to overcome bonds as energy is transferred to the surroundings so bonds will form again and it will condense into a liquid

99
New cards

what happens when a liquid cools down

energy from the liquid is transferred to the surroundings and so it won’t have enough energy to overcome the forces of attraction between the bonds/particles and it will freeze into a solid fixing the particles in place

100
New cards

what are the limitations of the particle model

particles aren’t solid since atoms are mostly empty space

many particles aren’t spherical