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Chemistry > Structure and bonding *DOUBLE AND TRIPLE* > Flashcards

Structure and bonding *DOUBLE AND TRIPLE* Flashcards

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1
Q

What are the three states of matter?

A

The three states of matter are solid, liquid and gas.

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2
Q

In which state are the particles arranged regularly?

A

Particles are arranged regularly in the solid state.

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3
Q

In which state do particles move quickly in all directions?

A

Particles move quickly in all directions in the gaseous state.

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4
Q

What state change happens when a substance melts?

A

When a substance melts it changes from solid to liquid.

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5
Q

What state change happens when a substance condenses?

A

When a substance condenses it changes from gas to liquid.

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6
Q

In general, which state of matter has particles with the highest energy?

A

Particles have highest energy in the gaseous state.

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7
Q

What is the melting point of water in 0C?

A

00C

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8
Q

What is the boiling point of water in 0C?

A

1000C

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9
Q

When a substance is melted, is energy transferred to or from the surroundings?

A

When a substance is melted, energy is transferred from the surroundings.

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10
Q

The melting point of sodium is 97.70C. What is the state of sodium at 25.00C?

A

Solid.

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11
Q

True or false - The temperature changes as a pure substance melts.

A

FALSE

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12
Q

True or false - When a substance melts, its particles move around and become less ordered.

A

TRUE

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13
Q

Is melting a physical process or a chemical process?

A

Melting is a physical process.

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14
Q

What do we call the change of state from a liquid to a gas?

A

The state change from liquid to gas is called evaporation.

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15
Q

What process takes place when a gas turns into a liquid?

A

The state change from gas to liquid is condensation.

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16
Q

What process takes place when a liquid is changing from a liquid to a gas throughout its volume (not just at its surface)?

A

Boiling.

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17
Q

What can link two atoms together?

A

A bond can link two atoms together.

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18
Q

Name the three types of strong chemical bonds.

A

The three types of strong chemical bonds are ionic, covalent and metallic.

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19
Q

What do ionic, covalent and metallic bonding all involve?

A

Ionic, covalent and metallic bonding all involve the transfer or sharing of outer shell electrons.

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20
Q

Describe ionic bonding

A

Ionic bonding occurs in compounds formed from metals combined with non-metals, where particles form oppositely charged ions by the transfer of outer shell electron/s.

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21
Q

Describe covalent bonding

A

Covalent bonding occurs in non-metallic elements and compounds of non-metals when outer shell electrons are shared.

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22
Q

Describe metallic bonding

A

Metallic bonding occurs in metallic elements and alloys and occurs when delocalised outer shell electrons are shared.

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23
Q

Which group of elements is stable and doesn’t form compounds easily?

A

Noble gases/group 0 elements are stable and don’t form compounds easily.

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24
Q

How is an element’s electron arrangement linked to its position in the periodic table?

A

Elements in the same group have the same number of electrons in their outer shell.

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25
Q

How do positive and negative charges affect each other?

A

Positive and negative charges attract each other.

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26
Q

Which sub-atomic particles of atoms take part in chemical reactions?

A

Electrons take part in chemical reactions.

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27
Q

What is an ion?

A

An atom that is charged because it has lost or gained one or more electrons

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28
Q

What happens when an ionic bond is formed?

A

One atom loses electrons to another atom to form oppositely charged ions that attract each other.

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29
Q

Which kinds of elements are usually involved in the formation of ionic bonds?

A

Metals and non-metals are involved in the formation of ionic bonds.

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30
Q

How is a positive ion formed and what is it called?

A

Positive ions are formed by the loss of electrons and are called cations.

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31
Q

How is a negative ion formed and what is it called?

A

Negative ions are formed by the gain of electrons and are called anions.

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32
Q

What are the forces called that hold ions together?

A

Forces that hold ions together are called electrostatic forces.

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33
Q

Why do atoms form ions?

A

Atoms form ions to become more stable.

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34
Q

When ions are formed by metals in groups 1 and 2 and non-metals in group 6 and 7, what does their electronic structure have in common?

A

The ions produced all have the stable electronic structure of a noble gas.

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35
Q

Explain why group 1 elements such as sodium and lithium form a 1+ ion.

A

Group 1 elements have one electron in their outer shell and lose it to become stable.

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36
Q

What are the charges on calcium, oxide and chloride ions?

A

Calcium = 2+, oxide = 2- and chlorine = 1-

37
Q

What structure of regularly repeating ions do ionic compounds form?

A

Ionic compounds form a giant structure of ions held together by electrostatic forces of attraction in a giant ionic lattice structure.

38
Q

What is the charge on the ions of elements in group 1 of the periodic table?

A

1+

39
Q

What is the charge on the ions of elements in group 6 of the periodic table?

A

2-

40
Q

What happens to the electrons in the outer shell of metal atoms when they form ions?

A

Electrons in the outer shell of metal atoms are lost when they form ions.

41
Q

What is the name of the ionic compound containing calcium and bromine only?

A

calcium bromide

42
Q

What is the name of the ionic compound containing potassium, chlorine and oxygen?

A

potassium chlorate

43
Q

What is a dot and cross diagram?

A

A dot and cross diagram is a drawing to show only the arrangement of the outer shell electrons of the atoms or ons in a substance.

44
Q

What is a ball and stick model?

A

A ball and stick model shows atoms (balls) bonded together (sticks), it is 2-D and does not show the shape of the molecule.

45
Q

What does a bond do in an element or compound?

A

A bond holds atoms together.

46
Q

What are electrostatic forces of attraction?

A

Electrostatic forces of attraction are attractions between positive and negative charges.

47
Q

Which part of an atom’s structure is most involved when two atoms react?

A

Electrons are the part of the atom’s structure involved when two atoms react.

48
Q

How many electrons are in the outer shell of the elements in groups 5, 6 and 7?

A

Group 5=5 outer shell electrons, group 6=6 outer shell electrons, and group 7=7 outer shell electrons.

49
Q

What kind of electron arrangement is most stable?

A

A complete/full outer shell of electrons is most stable (eg 2 for inner shell, 8 for 2nd and 3rd shells)

50
Q

What is the molecular formula of the very common compound formed between hydrogen and oxygen?

A

H2O

51
Q

How many more electrons does an oxygen atom need to get a complete outer shell?

A

An oxygen atom needs 2 electrons to get a complete outer shell.

52
Q

What are molecules?

A

Molecules are groups of atoms held together by covalent bonds.

53
Q

Which type of atoms are covalent bonds found between?

A

Covalent bonds are found between non-metal and non-metal atoms.

54
Q

What is a covalent bond?

A

A covalent bond is a shared pair of electrons.

55
Q

What happens to electrons between two atoms in a covalent bond?

A

Electrons are shared in a covalent bond.

56
Q

What kinds of elements usually form molecules?

A

Non-metals usually form molecules.

57
Q

What kinds of bonds are found in molecules?

A

Covalent bonds are found in molecules.

58
Q

What is the name of the type of bond formed by sharing electron pairs within molecules?

A

Covalent bonds are formed by sharing electron pairs in molecules.

59
Q

What term describes the number of atoms of each element bonded together in a molecule?

A

The molecular formula describes the number of atoms of each element bonded together in a molecule.

60
Q

In oxygen and carbon dioxide, the atoms share two pairs of electrons. How do we describe these bonds?

A

Double bonds are formed when atoms share two pairs of electrons.

61
Q

What is a polymer?

A

Polymers are many small reactive molecules that bond to each other to form long chains. The atoms are held together by covalent bonds and there are intermolecular forces between the polymer chains.

62
Q

What is the name of the force that holds molecules together in solids and liquids

A

Intermolecular forces hold molecules together in solids and liquids.

63
Q

How strong are the forces of attraction between molecules compared to the bonds within molecules?

A

The intermolecular forces of attraction between molecules are relatively weak in comparison to the bonds within molecules.

64
Q

Are simple molecules usually good conductors of electricity at room temperature?

A

Simple molecules are poor conductors of electricity because they have no free charged particles.

65
Q

What are intermolecular forces?

A

Intermolecular forces are forces of attraction between molecules.

66
Q

How does the strength of intermolecular forces change depending on the size of the molecule?

A

Intermolecular forces increase with the size of the molecules. (Thie means that larger molecules have higher melting and boiling points).

67
Q

What can you say about the formulae of small, simple molecules?

A

The formulae of small, simple molecules are fixed.

68
Q

What type of bonding is between the atoms in a molecule of water?

A

A molecule of water has covalent bonds between its atoms.

69
Q

What type of structure does water have?

A

Water has a simple molecular structure.

70
Q

What strength of forces are there between different molecules of water?

A

The forces between water molecules are weak.

71
Q

What type of structure do diamond and graphite have?

A

Diamond and graphite have giant covalent structures.

72
Q

What must be overcome to melt or boil giant covalent structures?

A

The strong covalent bonds must be overcome to melt or boil giant covalent structures.

73
Q

What does the term malleable mean?

A

Malleable means can be hammered or bent into a different shape.

74
Q

What type of bonding does copper have?

A

Copper has metallic bonding.

75
Q

What atoms does metallic bonding happen between?

A

Metallic bonding happens between atoms of metal and metal.

76
Q

What holds ions of metals together in a metallic bond?

A

Ions of metals are held together by a sea of delocalised electrons.

77
Q

Why can metals conduct electricity?

A

Electrons are free to move and carry charge.

78
Q

What is a metallic bond?

A

A metallic bond is the attraction between positive ions and delocalised electrons.

79
Q

What are the particles inside a metal?

A

Particles in a metal are metal ions surrounded by sea of electrons.

80
Q

Explain why metals are good conductors of electricity and heat.

A

Metals are good conductors of electricity because the delocalised electrons in the metal carry electrical charge through the metal. Metals are good conductors of thermal energy because energy is trnasferred by delocalised electrons.

81
Q

Why do ionic bonds have high melting and boiling points?

A

A large amount of energy is needed to break the many strong bonds in a giant ionic lattice.

82
Q

Can ionic compounds conduct electricity?

A

Ionic compounds cannot conduct electricity in the solid state. When melted or dissolved they can conduct because ions are free to move so charge can flow.

83
Q

Which forces are overcome when a covalent substance melts or boils?

A

The weak intermolecular forces are overcome when a substance melts or boils.

84
Q

Describe the structure and bonding of diamond.

A

In diamond, each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure, so diamond is hard, has a high melting point and does not conduct electricity.

85
Q

Describe the structure and bonding of graphite.

A

In graphite, each carbon atom forms 3 covalent bonds with three other carbon atoms, forming layers of hexagonal rings which have no covalent bonds between layers. One electron from each carbon atom is delocalised and therefore graphite is a good conductor.

86
Q

Describe the structure and bonding of an alloy.

A

Alloys are mixtures of two or more elements, at least one of which is a metal. The layers become distorted in alloys due to differently sized atoms of the different elements, making the alloy harder because it is less easy for the layers in a metal’s giant structure to slip over each other.

87
Q

What is graphene?

A

Graphene is a single layer of graphite. It is an excellent conductor of thermal energy and electricity, is low density and incredibly strong. These properties make it useful in electronics.

88
Q

What are fullerenes?

A

Fullerenes are molecules of carbon atoms with hollow shapes, formed from rings of 5, 6 or 7 carbon atoms eg buckminsterfullerene, C60.

89
Q

Give some uses of fullerenes.

A

Fullerenes can be used as lubricants or catalysts. Cylindrical fullerenes are used to reinforce composite materials for example in tennis rackets or in the electronics industry.

Chemistry (7 decks)

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