Atoms, Elements and Compounds and The Particulate Nature of Matter Flashcards

1
Q

Name the states of matter (3)

A

solids

liquids

gases

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2
Q

State symbol of solid

A

s

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3
Q

State symbol of liquid

A

l

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4
Q

State symbol of gas

A

g

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5
Q

Define a particle

A

simplest and smallest unit of matter

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6
Q

Define atoms

A

simplest particles that make up everything

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7
Q

Define compounds

A

two or more types of atoms chemically joined together

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8
Q

Define a property

A

characteristic of something

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9
Q

Which state of matter has a fixed shape

A

solid

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10
Q

Which state of matter has a fixed volume (2)

A

solid

liquid

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11
Q

Which state of matter flows (2)

A

liquid

gas

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12
Q

Particle arrangement of solid (3)

A

packed tightly together

has strong forces of attraction holding particles together

particles only vibrate on the spot

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13
Q

Particle arrangement of liquid (4)

A

packed tightly together

particles have strong forces of attraction

particles can move over one another

liquids take shape of their container

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14
Q

Particle arrangement of gas (3)

A

spaced far apart

particles move about freely

spread to fill container they are in

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15
Q

Which states cannot be compressed and why (3)

A

solids

liquids

particles already packed together

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16
Q

Which state can be compressed and why (2)

A

gas

particles are spread out

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17
Q

Define melting point

A

temperature of substance when it changes from solid to liquid

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18
Q

Define boiling point

A

temperature of substance when it changes from liquid to a gas

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19
Q

Process of change from solid to liquid

A

melting

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20
Q

Process of change from liquid to gas

A

boiling

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21
Q

Process of change from gas to liquid

A

condensing

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22
Q

Process of change from liquid to solid

A

freezing

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23
Q

How process of evaporation works (4)

A

liquid particles have some particles which move faster

faster particles have more kinetic energy

hence they have enough energy to escape liquid surface as gas

not all particles evaporate as boiling point not reached

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24
Q

Define molecules

A

particles of atoms joined together by covalent bonds

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25
Q

Define an ion

A

charged particles formed by atom gaining or losing electron

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26
Q

Define diffusion (2)

A

movement of particles through a liquid or gas

movement of particles from an area of high concentration to an area of low concentration

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27
Q

Determinants of rate of diffusion (2)

A

molecular mass - larger molecular mass is slower

vacuum - faster as no other particles to collide with

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28
Q

Define a chemical reaction (2)

A

reaction which occurs when 2 or more substances react to form a new substance

difficult to reverse/irreversible

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29
Q

Define a physical change (3)

A

involve a change of state

no new substance is made

easily reversible

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30
Q

Name indicators of chemical reaction (4)

A

colour change

gas produced

solid formed

temperature change

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31
Q

Name reversible reactions (2)

A

Hydrated copper(II) sulfate crystals <-> Anhydrous copper(II) sulfate + Water

Hydrated cobalt(II) chloride <-> Anhydrous cobalt(II) chloride + Water

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32
Q

Colour change from hydrated copper sulfate crystals to anhydrous copper sulfate

A

blue crystals to white powder

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33
Q

Colour change from hydrated cobalt chloride crystals to anhydrous cobalt chloride

A

pink crystals to blue

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34
Q

Define an element

A

a substance which contains only one type of atom

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35
Q

Word equation of Hydrated copper(II) sulfate crystals <-> Anhydrous copper(II) sulfate + Water

A

CuSO4 5H2O(s) -> CuSO4(s) + 5H2O(l)

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36
Q

Chemical equation of Hydrated cobalt(II) chloride <-> Anhydrous cobalt(II) chloride + Water

A

CoCl2 6H2O(s) -> CoCl2(s) + 6H2O(l)

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37
Q

Define mixture

A

contains elements and compounds not chemically joined together

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38
Q

Properties of metals (7)

A

shiny/lustrous

good conductors (heat and electricity)

high melting and boiling points

high tensile strength

sonorous (rings when struck)

ductile (can be stretched into wire)

malleable (can be beaten into shape)

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39
Q

Properties of non-metals (4)

A

dull

poor conductors (heat and electricity)

low melting and boiling points

brittle (breaks easily)

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40
Q

Exceptions to metal and non-metal properties (4)

A

carbon and silicon have high melting points

carbon in form of graphite conducts electricity

mercury has low melting point

alkali metals are soft, have low melting points, not sonorous

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41
Q

Define metalloids

A

elements that exhibit characters of both non-metals and metals

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42
Q

Define alloys

A

substances formed when metals mix with other elements

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43
Q

Examples of alloys (3)

A

steel

bronze

brass

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44
Q

Define a solution

A

mixture formed when one substance dissolves fully into another

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45
Q

Define solute

A

substance that is dissolved

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46
Q

Define solvent

A

substance which does the dissolving

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47
Q

Define concentration of a solution (2)

A

amount of solute dissolved in certain volume

can be expressed as number of moles of solute in one decimetre cubed of solution

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48
Q

What 3 sub-atomic particles are in an atom (3)

A

proton

neutron

electron

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49
Q

Name of centre of atom

A

nucleus

50
Q

Features of protons (3)

A

found in nucleus

have a positive charge (+1)

have relative mass of 1 atomic mass unit (amu)

51
Q

Features of electrons (3)

A

found in electron shells orbiting nucleus

have negative charge (-1)

have relative mass of 1/2000

52
Q

Features of neutrons (3)

A

found in nucleus of atom

have no charge and are neutral (0)

have relative mass of 1 amu

53
Q

What is the charge of atoms (2)

A

atoms have no charge (neutral)

number of protons equal to number of electrons

54
Q

What does nuclide notation show (3)

A

element symbol

proton/atomic number

nucleon (mass) number

55
Q

What does proton/atomic number show

A

number of protons an atom has

56
Q

What happens to proton/atomic number when you move from left to right across a period

A

proton/atomic number increases

57
Q

Define periodicity

A

trend that can be seen in periodic table

58
Q

What does nucleon/mass number show

A

number of protons and neutrons an atom has

59
Q

What is most of an atom

A

empty space

60
Q

How are electrons arranged (4)

A

arranged in shells

first shell holds 2 electrons

2nd shell holds 8 electrons

3rd shell holds 8 electrons

61
Q

Features of noble gases (2)

A

full outer electron shell

are stable as electron shell full

62
Q

Name of outer electrons

A

valence electrons

63
Q

What do elements in the same group have and why (2)

A

similar chemical properties

due to same number of valence electrons

64
Q

What happens to the number of electrons as we move along a period

A

number of electrons in outer shell increases

65
Q

Define an isotope

A

atoms of same element with same atomic number but different mass number due to different neutron number

66
Q

Properties of Isotopes

A

have same chemical properties as they have same number of valence electrons

67
Q

What is the charge of an atom which has lost electrons

A

positive charge

68
Q

Which atoms tend to lose electrons

A

metals

69
Q

What is the charge of an atom which has gained electrons

A

negative charge

70
Q

Define cations

A

positive ions

71
Q

Define anions

A

negative ions

72
Q

Which substances will an ionic bond form between (2)

A

metal

non-metal

73
Q

How do ions form (3)

A

metal atoms give electrons to non-metal atoms

both atoms are stable charged particles

atoms attracted as they are oppositely charged

74
Q

Define an ionic bond

A

electrostatic force of attraction between oppositely charged ions

75
Q

Name given to pattern which ionic compounds are organised in

A

ionic lattice

76
Q

Ionic lattice structure

A

ion surrounded by ions of opposite charge

77
Q

Define oxidation

A

when an atom/ion loses electrons

78
Q

Define reduction

A

when an atom/ion gains electrons

79
Q

Define electricity

A

flow of charged particles (ions or electrons)

80
Q

In metals and graphite which part of the atom moves and carries an electric current

A

outer electrons of atoms (delocalised electrons) which can move and carry current

81
Q

Define an electrolyte

A

molten substance or solution that conducts

82
Q

At which states do metals conduct (2)

A

solid

liquid

83
Q

Can non-metals and covalent substances (except graphite) conduct electricity

A

no

84
Q

Features of ionic substances (5)

A

hard crystals - strong attraction between positive and negative ions

high melting points - lot of energy needed to overcome forces of attraction between ions

dissolves in water - water forms electrostatic attractions with ions and “pluck” them off lattice

does not conduct when solid - electrons held tightly in lattice and cannot move

conducts when molten/solution - lattice breaks and ions free to move

85
Q

What determines strength of ionic bond

A

greater charge greater strength

86
Q

When will a covalent bond form with

A

non-metals

87
Q

Define a covalent bond

A

pair of electrons shared by two atoms

88
Q

Define a diatomic molecule

A

molecule made up of 2 atoms bonded together

89
Q

Define triatomic molecule

A

molecule made up of 3 atoms bonded together

90
Q

Example of triatomic molecule

A

H2O

91
Q

Define valency

A

number of bonds an element needs to form

92
Q

Group 1 valency

A

1

93
Q

Group 2 valency

A

2

94
Q

Group 3 valency

A

3

95
Q

Group 4 valency

A

4

96
Q

Group 5 valency

A

3

97
Q

Group 6 valency

A

2

98
Q

Group 7 valency

A

1

99
Q

Group 8 valency

A

0

100
Q

How is a covalent bond held together (3)

A

positively charged protons in the nucleus

negatively charged electrons in shared area

electrons and protons attracted as opposites attract

101
Q

Define macromolecules

A

molecules that contain large number of atoms

102
Q

Define allotropes

A

different forms of same element

103
Q

2 giant covalent structures of carbon

A

diamond

graphite

104
Q

Diamond structure (3)

A

carbon atoms arranged in tetrahedral structure

carbon bonded to 4 other carbon atoms

held together by strong covalent bonds

105
Q

Graphite structure (3)

A

carbon atoms in hexagonal shape in layers

each carbon atom bonds to 3 other carbon atoms

layers held together by weak intermolecular forces of attraction

106
Q

Properties of diamond (3)

A

strong covalent bonds

high melting point - lots of energy needed to break strong bonds between atoms

hard substance

107
Q

Properties of graphite (4)

A

strong bonds between atoms

weak intermolecular forces between layers

weak IMFs cause layers to slide over each other

is flaky and can be used as lubricant

108
Q

Can diamond conduct electricity

A

no

109
Q

Can graphite conduct electricity

A

yes

110
Q

Why is graphite able to conduct electricity (2)

A

has delocalised electrons (electron left from not having 4th bond)

electron is free to move and allows conduction

111
Q

Examples of macromolecules (3)

A

silicon (IV) oxide

diamond

graphite

112
Q

Number of covalent bonds for silicon (IV) oxide

A

4

113
Q

Melting and boiling point of covalent bonds

A

low melting and boiling points

114
Q

Why do covalent bonds have low melting and boiling points (2)

A

covalent bonds (intramolecular forces) not broken when substance melted or boiled

much weaker forces of attraction (intermolecular forces) broken

115
Q

Define volatility

A

how easily substances vaporise

116
Q

What are covalent bonds said to be

A

volatile since they have low melting and boiling points

117
Q

Do covalent substances conduct electricity why? (3)

A

do not conduct electricity as no free electrons to carry charge

do not have ions

exceptions - some covalent substances will form ions when dissolved in water

118
Q

Are covalent substances insoluble or soluble in water

A

insoluble

119
Q

Melting and boiling points of giant covalent structures

A

high melting and boiling points

120
Q

Structure of giant covalent structures (2)

A

have strong covalent bonds - no weak

121
Q

Why do giant covalent bonds have high melting and boiling points (2)

A

every strong covalent bond must be broken

hence require lots of energy