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

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
Define an ion
charged particles formed by atom gaining or losing electron
26
Define diffusion (2)
movement of particles through a liquid or gas movement of particles from an area of high concentration to an area of low concentration
27
Determinants of rate of diffusion (2)
molecular mass - larger molecular mass is slower vacuum - faster as no other particles to collide with
28
Define a chemical reaction (2)
reaction which occurs when 2 or more substances react to form a new substance difficult to reverse/irreversible
29
Define a physical change (3)
involve a change of state no new substance is made easily reversible
30
Name indicators of chemical reaction (4)
colour change gas produced solid formed temperature change
31
Name reversible reactions (2)
Hydrated copper(II) sulfate crystals <-> Anhydrous copper(II) sulfate + Water Hydrated cobalt(II) chloride <-> Anhydrous cobalt(II) chloride + Water
32
Colour change from hydrated copper sulfate crystals to anhydrous copper sulfate
blue crystals to white powder
33
Colour change from hydrated cobalt chloride crystals to anhydrous cobalt chloride
pink crystals to blue
34
Define an element
a substance which contains only one type of atom
35
Word equation of Hydrated copper(II) sulfate crystals <-> Anhydrous copper(II) sulfate + Water
CuSO4 5H2O(s) -> CuSO4(s) + 5H2O(l)
36
Chemical equation of Hydrated cobalt(II) chloride <-> Anhydrous cobalt(II) chloride + Water
CoCl2 6H2O(s) -> CoCl2(s) + 6H2O(l)
37
Define mixture
contains elements and compounds not chemically joined together
38
Properties of metals (7)
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)
39
Properties of non-metals (4)
dull poor conductors (heat and electricity) low melting and boiling points brittle (breaks easily)
40
Exceptions to metal and non-metal properties (4)
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
41
Define metalloids
elements that exhibit characters of both non-metals and metals
42
Define alloys
substances formed when metals mix with other elements
43
Examples of alloys (3)
steel bronze brass
44
Define a solution
mixture formed when one substance dissolves fully into another
45
Define solute
substance that is dissolved
46
Define solvent
substance which does the dissolving
47
Define concentration of a solution (2)
amount of solute dissolved in certain volume can be expressed as number of moles of solute in one decimetre cubed of solution
48
What 3 sub-atomic particles are in an atom (3)
proton neutron electron
49
Name of centre of atom
nucleus
50
Features of protons (3)
found in nucleus have a positive charge (+1) have relative mass of 1 atomic mass unit (amu)
51
Features of electrons (3)
found in electron shells orbiting nucleus have negative charge (-1) have relative mass of 1/2000
52
Features of neutrons (3)
found in nucleus of atom have no charge and are neutral (0) have relative mass of 1 amu
53
What is the charge of atoms (2)
atoms have no charge (neutral) number of protons equal to number of electrons
54
What does nuclide notation show (3)
element symbol proton/atomic number nucleon (mass) number
55
What does proton/atomic number show
number of protons an atom has
56
What happens to proton/atomic number when you move from left to right across a period
proton/atomic number increases
57
Define periodicity
trend that can be seen in periodic table
58
What does nucleon/mass number show
number of protons and neutrons an atom has
59
What is most of an atom
empty space
60
How are electrons arranged (4)
arranged in shells first shell holds 2 electrons 2nd shell holds 8 electrons 3rd shell holds 8 electrons
61
Features of noble gases (2)
full outer electron shell are stable as electron shell full
62
Name of outer electrons
valence electrons
63
What do elements in the same group have and why (2)
similar chemical properties due to same number of valence electrons
64
What happens to the number of electrons as we move along a period
number of electrons in outer shell increases
65
Define an isotope
atoms of same element with same atomic number but different mass number due to different neutron number
66
Properties of Isotopes
have same chemical properties as they have same number of valence electrons
67
What is the charge of an atom which has lost electrons
positive charge
68
Which atoms tend to lose electrons
metals
69
What is the charge of an atom which has gained electrons
negative charge
70
Define cations
positive ions
71
Define anions
negative ions
72
Which substances will an ionic bond form between (2)
metal non-metal
73
How do ions form (3)
metal atoms give electrons to non-metal atoms both atoms are stable charged particles atoms attracted as they are oppositely charged
74
Define an ionic bond
electrostatic force of attraction between oppositely charged ions
75
Name given to pattern which ionic compounds are organised in
ionic lattice
76
Ionic lattice structure
ion surrounded by ions of opposite charge
77
Define oxidation
when an atom/ion loses electrons
78
Define reduction
when an atom/ion gains electrons
79
Define electricity
flow of charged particles (ions or electrons)
80
In metals and graphite which part of the atom moves and carries an electric current
outer electrons of atoms (delocalised electrons) which can move and carry current
81
Define an electrolyte
molten substance or solution that conducts
82
At which states do metals conduct (2)
solid liquid
83
Can non-metals and covalent substances (except graphite) conduct electricity
no
84
Features of ionic substances (5)
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
What determines strength of ionic bond
greater charge greater strength
86
When will a covalent bond form with
non-metals
87
Define a covalent bond
pair of electrons shared by two atoms
88
Define a diatomic molecule
molecule made up of 2 atoms bonded together
89
Define triatomic molecule
molecule made up of 3 atoms bonded together
90
Example of triatomic molecule
H2O
91
Define valency
number of bonds an element needs to form
92
Group 1 valency
1
93
Group 2 valency
2
94
Group 3 valency
3
95
Group 4 valency
4
96
Group 5 valency
3
97
Group 6 valency
2
98
Group 7 valency
1
99
Group 8 valency
0
100
How is a covalent bond held together (3)
positively charged protons in the nucleus negatively charged electrons in shared area electrons and protons attracted as opposites attract
101
Define macromolecules
molecules that contain large number of atoms
102
Define allotropes
different forms of same element
103
2 giant covalent structures of carbon
diamond graphite
104
Diamond structure (3)
carbon atoms arranged in tetrahedral structure carbon bonded to 4 other carbon atoms held together by strong covalent bonds
105
Graphite structure (3)
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
Properties of diamond (3)
strong covalent bonds high melting point - lots of energy needed to break strong bonds between atoms hard substance
107
Properties of graphite (4)
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
Can diamond conduct electricity
no
109
Can graphite conduct electricity
yes
110
Why is graphite able to conduct electricity (2)
has delocalised electrons (electron left from not having 4th bond) electron is free to move and allows conduction
111
Examples of macromolecules (3)
silicon (IV) oxide diamond graphite
112
Number of covalent bonds for silicon (IV) oxide
4
113
Melting and boiling point of covalent bonds
low melting and boiling points
114
Why do covalent bonds have low melting and boiling points (2)
covalent bonds (intramolecular forces) not broken when substance melted or boiled much weaker forces of attraction (intermolecular forces) broken
115
Define volatility
how easily substances vaporise
116
What are covalent bonds said to be
volatile since they have low melting and boiling points
117
Do covalent substances conduct electricity why? (3)
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
Are covalent substances insoluble or soluble in water
insoluble
119
Melting and boiling points of giant covalent structures
high melting and boiling points
120
Structure of giant covalent structures (2)
have strong covalent bonds - no weak
121
Why do giant covalent bonds have high melting and boiling points (2)
every strong covalent bond must be broken hence require lots of energy

Chemistry (3 decks)

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