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Paper1- Chemistry > Topic 1- Atomic structure and the Periodic Table > Flashcards

Topic 1- Atomic structure and the Periodic Table Flashcards

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1
Q

what is the electronic structure when filling outer shells

A

2.8.8…..

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2
Q

what does 2.8.8 mean

A

the maximum number of electrons that fit in each outer shell

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3
Q

why do elements react

A

in order to fill out their outer shells

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4
Q

what is the electron configuration of sodium, Na

A

2.8.1
they have 11 electrons

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5
Q

what is the electron configuration of calcium, Ca

A

2.8.8.2
they have 20 electrons

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6
Q

what is fractional distillation used for

A

to separate a mixture of liquids

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7
Q

why can the mixture be separated using fractional distillation

A

because they have very different melting points

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8
Q

what do you use to condense the liquid in fractional distillation

A

a fractionating column

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9
Q

how do you do fractional distillation

A
  1. put the mixture in a flask and stick a fractionating column on top the heat it
  2. when the liquid with the lowest boiling point starts to evaporate it reaches the top of the column
    3.it will condense and collect in a test tube
  3. raise the temperature until the next liquid is ready
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10
Q

which liquid will evaporate first in fractional distillation

A

liquid with lowest boiling point

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11
Q

as the first liquid evaporates, what happens if other liquids start to aswell in fractional distillation

A

liquids with higher boiling points might also start to evaporate but the column is cooler towards the top so they will condense again

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12
Q

what is crystallisation used to separate

A

soluble solids from solutions

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13
Q

how do you carry our crystallisation

A
  1. pour the solution into an evaporating dish and gently heat the solution(becomes more concentrated as it evaporates)
  2. once some has evaporated or when you start to see crystals start to form, remove the dish from the heat and leave it cool
  3. the salt should start to form crystals as it becomes insoluble in the highly concentrated solution
  4. filter the crystals out of the solution and leave them to dry
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14
Q

what happens when the solution starts to evaporate

A

the solution becomes more concentrated

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15
Q

how do you do evapoartion

A
  1. pour the solution into an evaporating dish
  2. slowly heat the solution. the solvent will evaporate and the solution will get more concenrtated
  3. crystals will start to form
  4. keep heating the evaporating dish until all you have left are dry crystals
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16
Q

what is evaporation used for

A

separate a soluble salt from a solution

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17
Q

what does filtration separate

A

insoluble solids from solutions

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18
Q

what happens in filtration

A

when the solution is poured, the solid gets trapped in the filter paper and the liquid goes through

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19
Q

what is simple distillation used for

A

to separate out solutions

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20
Q

how does simple distillation work

A
  1. the solution is heated. the liquid with the lowest boiling point evaporates first
  2. the vapour is then cooled, condensed and is collected
  3. the rest of the solution is left
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21
Q

what is the problem with simple distillation

A

it only works with to separate liquids with very different boiling points- if boiling point goes higher they will mix again

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22
Q

what is an example of how simple distillation is used

A

to get pure water from sea water

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23
Q

what is the difference between simple and fractional distillation

A
  • simple only separates one fraction(Liquid) but fractional separates multiple
  • fractional uses a fractionating column
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24
Q

what is rock salt

A

a simple mixture of salt and sand

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25
Q

what 4 things do you do to separate rock salt

A
  1. grinding
  2. dissolving
  3. filtering
    4.evaporating
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26
Q

how do you separate rock salt

A
  1. GRINDING grind the mixture to make sure salt crystals are small, so will dissolve easily
  2. DISSOLVING put the mixture in water and stir. the salt will dissolve the sand wont
  3. FILTERING filter the mixture. the sand will collect in the paper. the salt passes through as part of the solution
  4. EVAPORATING evaporate the water from the salt so it forms dry crystals (or crystallisation if you want big ones)
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27
Q

what is a mixture

A

two or more element or compounds not chemically bonded together

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28
Q

what happens to the chemical properties of the substances in a mixture

A

the chemical properties of each substance in the mixture is unchanged

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29
Q

how do you separate a mixture

A

using physical methods

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30
Q

are mixtures easily separated

A

yes

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31
Q

what does soluble mean

A

can be dissolved(a solid)

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32
Q

what is an example of a soluable substance

A

sugar, salt

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33
Q

what does insoluble mean

A

does not dissolve

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34
Q

what is an example of insoluble substances

A

sand

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35
Q

what does miscible mean

A

liquids that dissolve in each other

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36
Q

what is residue

A

solid collected in the filter paper

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37
Q

what is the filtrate

A

liquid/solution that runs through the filter

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38
Q

what is immiscible

A

not soluble, don’t mix

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39
Q

what does chromatography separate

A

separates mixtures(dyes in ink)

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40
Q

how do you set up a chromatography

A

take a piece of filter paper and draw a pencil line near the bottom
place a dot of ink on the line

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41
Q

how do you do chromatography

A
  1. place the prepared filter paper in the solvent(water)
  2. as the solvent travels up the paper, it drags the different dyes with it, more soluble dyes work best
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42
Q

in chromatography, what happens to soluble dyes

A

it will travel quicker and further

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43
Q

what is the end result of the chromatography called

A

a chromatogram

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44
Q

what is an ion

A

an atom with a charge(gained or lost electron)

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45
Q

what is the ion for each group

A

1= +
2= +2
3=+3
4= don’t make ions
5=3-
6= 2-
7= -
0= already stable- don’t make ions

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46
Q

what is the ion of sodium, Na

A

Na +

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47
Q

what is the ion for sodium electron configuration

A

[2.8]+
11 electrons

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48
Q

when balancing equations, what must ALWAYS be the same

A

same number of atoms on both sides

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49
Q

what does a formula show

A

what atoms are in a substance

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50
Q

which side of a formula are the reactants on?
Products?

A

reactants- left
products- right

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51
Q

ethane +oxygen —> carbon dioxide + water
which are Products?
reactants?

A

products- carbon dioxide, water
Reactants- ethane, oxygen

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52
Q

what is the law of conservation of mass

A

total mass of products formed is ALWAYS equal to the total mass of reactants

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53
Q

what is an isotope

A

atoms of the same element with a different number of NEUTRONS and the same number of PROTONS

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54
Q

what is the only thing that affects what an element is

A

the atomic number

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55
Q

Isotopes have the same —– number but different —— numbers

A

isotopes have the same atomic number but different mass numbers

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56
Q

what are the chemical properties of isotopes

A
  • isotopes of an element have the same chemical properties because electron arrangement is the same
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57
Q

what are the physical properties of an isotope

A

isotope of an element have different masses due to having more or less neutrons in the nucleus

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58
Q

what is an atom

A

the smallest part of an element

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59
Q

what is an element

A

a substance with only one type of atom

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60
Q

what is a compound

A

substance with 2 or more elements chemically bonded

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61
Q

what are the vertical columns called ^

A

groups

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62
Q

what are the horizontal rows called >

A

periods

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63
Q

what subatomic particles are found in the nucleus

A

protons and neutrons

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64
Q

what subatomic particles are on the outside in shells

A

electrons

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65
Q

what is the radius of a nucleus

A

1x10 ^-14

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66
Q

what does the nucleus contain

A

protons and neutrons

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67
Q

where is the nucleus located

A

in the centre of the atom

68
Q

what is the charge of the nucleus

A

positive charge due to protons

69
Q

where is the mass of the atom concentrated

A

in the middle

70
Q

how many electrons and protons are in an atom

A

the same

71
Q

what is the charge of an atom? why?

A

neutral- they have the same number of proton and electrons and have opposite charges so cancel out

72
Q

where are electrons in an atom

A

move around the neutron in electron shells

73
Q

23
Na
11
which one is the mass number

A

the top one

74
Q

what is the mass number

A

total number of protons and neutrons

75
Q

23
Na
11
which is the atomic number

A

the bottom one

76
Q

what is the atomic number

A

how many protons there are

77
Q

what is the relative charge of the neutron

A

0

78
Q

what is the relative charge of the proton

A

+1

79
Q

what is the relative charge of the electron

A

-1

80
Q

what is the relative mass of the neutron

A

1 mass unit

81
Q

what is the relative mass of the electron

A

virtually no mass
1/1840 mu

82
Q

what is the relative mass of the proton

A

1 Mass unit (MU)

83
Q

how do you find the number of protons

A

atomic number

84
Q

how do you find the number of neurons

A

mass number- proton number

85
Q

how do you find the number of electrons

A

number of protons

86
Q

what happens during a chemical reaction

A

always involve the formation of one or more new substances and often involve a detectable energy change

87
Q

how can compounds be represented

A

by formula

88
Q

what is the radius of an atom

A

0.1 NM
or 1x10^-10

89
Q

how is the modern periodic table laid out

A

in order of increasing atomic number

90
Q

because of how the modern periodic table is laid out what does it mean

A

there are repeating patterns in their properties

91
Q

where are metals found on the periodic table

A

left

92
Q

where are the non metals found on the periodic table

A

right

93
Q

what are the vertical columns called

A

groups

94
Q

what are the horizontal rows called

A

periods

95
Q

what does the group number tell you

A

how many electrons there are in there outer shells

96
Q

what do the groups in the periodic table allow you to do

A

you can predict properties of other elements in that group e.g group 1 metals all react in similar ways

97
Q

what are the group 0 elements known as

A

noble gases

98
Q

are the noble gases (group 0) reactive

A

no they are unreactive

99
Q

why are the noble gases unreactive

A

they are unreactive because they have a full outer shell- 8

100
Q

what does inert mean

A

don’t react at all

101
Q

what is different between helium and the rest of the noble gases

A

it only has 2 in its outer shell- but it still has a full outer shell

102
Q

what are the trends of group 0 elements (noble gases)

A
  • increase in boiling point down the group
  • increase in relative atomic mass down the group
103
Q

why does the boiling point increase down the group in group 0 elements

A

due to an increase in the number of electrons in each atom leading to greater intermolecular forces which need to be overcome

104
Q

ESQ- neon is gas at 25 ‘C. Predict what state helium is at at this temperature

A
  • helium is higher on the periodic table so has a lower Boiling point
  • must be a gas
105
Q

what are the group 0 elements at room temperature

A

colourless gases

106
Q

are the group 0 elements flammable

A

non- flammable

107
Q

what are the group 7 elements called

A

the halogens

108
Q

why do the group 7 elements react similarly

A

they all have 7 electrons in their outer shells

109
Q

are the group 7 elements metals or non metals?

A

non metals

110
Q

what do the group 7 elements consist of

A

molecules made of pairs of atoms

111
Q

what are the trends of group 7 elements

A
  • melting point, boiling point and relative atomic mass increase down the group
  • the reactivity decreases down the group
112
Q

why does the reactivity decrease down the group of the group 7 elements

A

it is harder to gain extra electrons because the outer shells are further from the nucleus so it cannot easily gain an electron

113
Q

how can the halogens also get a full outer shell

A

the atoms can share electrons via covalent bonding with other non metals to achieve full outer shells

114
Q

what is it called when nonmetals react with metals

A

ionic bonding

115
Q

—— reactive Halogens will ——- —– reactive ones from an ——- solution of its —–

A

more reactive halogens will displace less reactive ones from an aqueous solution of its salts

116
Q

what is formed when the halogens react

A

compounds that all have simple molecular structures

117
Q

what is the difference between group 1 metals and transition metals

A
  • group 1 metals are much more reactive- react more vigorously with water, oxygen
  • much less dense, strong and hard than transition metals
  • group 1 metals have lower melting points
118
Q

what happens when group 1 elements react with water

A

they react vigorously to produce hydrogen gas and metal hydroxide

119
Q

what is produced when a group 1 element reacts with water

A

hydrogen gas and metal hydroxide

120
Q

what is the equation for a reaction between a group 1 element and water

A

metal + water —> metal hydroxide +hydrogen

121
Q

what happens down the group when group 1 elements react with water

A
  • the lower down the group the more vigorous the reaction
  • the amount of energy given out by the reaction increases
122
Q

what happens when group 1 elements react when heated with chlorine

A

vigorously react when heated with chlorine gas to form white metal chloride salts

123
Q

what is the equation for the reaction between group 1 elements and chlorine

A

metal+ chlorine –> metal chloride

124
Q

what happens down the group when group 1 metals react with chlorine

A
  • the reaction increases and becomes more vigorous
125
Q

what is produced when group 1 elements react with oxygen

A

metal oxide

126
Q

what does lithium produce when reacting with oxygen

A

lithium oxide

127
Q

what does sodium produce when reacting with oxygen

A

sodium oxide and sodium peroxide

128
Q

what does potassium produce when reacting with oxygen

A

potassium peroxide and potassium superoxide

129
Q

what are group 1 elements also known as

A

alkali metals

130
Q

how many electrons are in the alkali metals outer shells

A

1

131
Q

what are the properties of the alkali metals(group 1)

A
  • soft
  • have low density
  • the first 3 in the group are less dense than water
132
Q

what does it mean if the alkali metals have 1 electron in their outer shell

A
  • they are very reactive
  • have similar properties
133
Q

what are the trends down the group for the alkali metals

A
  • increases in reactivity
  • lower melting and boiling points
  • higher relative atomic mass
134
Q

why does the reactivity increase down the group in the alkali metals

A

outer electron is more easily lost as attraction between nucleus and electrons decrease - more shielding because there is more shells

135
Q

what are the transition metals found on the periodic table

A

in the centre between group 2 and 3

136
Q

what are the physical properties of the transition metals

A

typical metal- dense, strong, shiny, conduct

137
Q

do the transition metals all have similar properties

A

yes

138
Q

what are the chemical properties of the transition metals

A
  • useful as catalysts
  • make colourful compounds
  • ions with different charges
139
Q

what are catalysts

A

speed up reactions

140
Q

how do you work our relative atomic mass

A

(isotope abundance x mass number)
/sum of abundance(all isoptopes)

141
Q

ESQ 14 13 12
C C C
1% 3% 96%
what is the relative atomic mass

A

(14x1)+(13x3)+(12x96)/100

= 12.05

142
Q

what is a metal

A

element that reacts to form positive ions

143
Q

what is a non metal

A

elements that do not react to form positive ions

144
Q

why do metals form positive ions

A

there is not much energy needed to remove the electrons so it is feasible for the elements to react to form positive ions with full outer shells

145
Q

why do non metals not form positive ions

A

it is far more feasible for them to either share or gain electrons to get a full outer shell, it is harder to remove electrons

146
Q

what are the physical properties of metals

A
  • strong- malleable, ductile(can be wires)
  • great at conducting heat and electricity
  • high boiling and melting points
147
Q

why do metals have similar physical properties

A

all metals have metallic bonding which cause them to have similar

148
Q

what are the physical properties of non metals

A
  • dull looking and more brittle
  • don’t conduct electricity generally
  • often lower density
  • aren’t always solid at room temperature
149
Q

what was the order of the discovery of the subatomic particles

A
  1. electrons- JJ Thompson
  2. nucleus- Rutherford
  3. protons
  4. neutrons- Chadwick
150
Q

what was the first model of the atom

A

plum pudding model

151
Q

who created the plum pudding model

A

JJ Thompson

152
Q

what is the plum pudding model

A

suggested the atom is a ball of positive charge with negative electrons embedded in it randomly

153
Q

who created the nuclear model

A

Rutherford

153
Q

who did the alpha particle scattering experiment

A

Geiger and Marsden(students of Rutherford

154
Q

what was the alpha particle experiment

A
  • they took a piece of gold foil and fired alpha particles at it. most particles passed through but a few were reflected by the centre and small number were repelled back to source
155
Q

what did the alpha particle experiment conclude

A
  • the mass of the atom was concentrated at the centre(nucleus) and it was charged
  • rest of the atom was empty space
156
Q

how did Niels Bohr alter the nuclear model

A

suggested that electrons orbit the nucleus at specific distances

157
Q

what did experiments lead to after Niels Bohr

A

the idea that the positive charge of any nucleus could be subdivided into smaller particles, called protons

158
Q

what did the experimental work of Chadwick find

A

the existence of neutrons in the nucleus- 20 years after the nucleus was accepted

159
Q

how did Dalton order the periodic table

A

elements by weight

160
Q

how did newlands order the periodic table

A

ordered the elements into columns of order of atomic mass, in rows of 8, patterns didnt always work

161
Q

how did moseley order the periodic table

A

by atomic number

162
Q

what is the order of scientists who altered the periodic table

A
  1. Dalton
  2. Newland
  3. Mendeleev
  4. Moseley
163
Q

how did Mendeleev alter the periodic table

A

left gaps for elements that he thought had not been discovered and in some places changed the order based on atomic weight
- the elements with properties predicted by Mendeleev were discovered and filled the gaps

164
Q

how did scientist try to order the elements before the discovery of the protons

A

in order of atomic number

165
Q

what was wrong with the early periodic table

A

was incomplete, some elements were placed in inappropriate groups if the order of atomic weights were followed

166
Q

what is the modern periodic table based on

A

Mendeleev’s ideas plus new elements

Paper1- Chemistry (3 decks)

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