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Chemistry > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

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1
Q

There are about ……. different elements

A

100

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2
Q

an element consists of

A

all the same atoms

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3
Q

define compound

A

Compounds contain two or more elements chemically combined in
fixed proportions

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4
Q

do compounds have similar or different properties to the elements their made of ?

A

usually totally different properties

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5
Q

Compounds can only be separated into elements by ……………….

A

chemical reactions

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6
Q

define mixture

A

A mixture consists of two or more elements or compounds not
chemically combined together.

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7
Q

Mixtures can be separated by

A

physical processes/ techniques

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8
Q

give 5 examples of physical processes of separation

A

filtration,
crystallisation,
simple distillation,
fractional distillation
chromatography

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9
Q

define molecule

A

a molecule has ANY element chemically combined
eg Ca(OH) 2 this is a compound AND a molecule
Cl2 is a molecule

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10
Q

how many atoms of each in this compound ? Ca(OH)2

A

1 Ca
2 O
2 H

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11
Q

physical separation techniques are used to separate …………… they cant be used to separate the ………….. in a ……………..

A

physical separation techniques are used to separate mixtures they cant be used to separate the elements in a compound

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12
Q

what is filtration used to separate

A

insoluble solid from liquid

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13
Q

what does (aq) mean

A

aqueous, dissolved in water

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14
Q

how do you filter
what do you need to filter

A

get filter paper and funnel and beaker
pour solution through filter paper and funnel
insoluble solid left in filter paper
liquid left in beaker

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15
Q

what is crystalisation used for

A

separate a soluble solid from a liquid

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16
Q

describe the process of crystallisation

A

heat solution in beaker till solvent evaporates
Crystals of the solid left in beaker
pour/ filter excess solvent
dry crystals in oven / pat with filter paper

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17
Q

what is simple distillation used for

A

simple distillation used for separating a solid from liquid if we want to keep the liquid

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18
Q

2 stages of simple distillation

A

evaporate liquid by heating
condense vapour by cooling

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19
Q

process of simple distillation (4 steps)

A
  1. place solution ( liquid + solid ) in conical flask
    flask connected to glass tube which is surrounded by condenser
  2. heat solution till liquid evaporates
  3. vapour passes through condenser
    ( condenser kept cold by circulation of water around it )
  4. condensed liquid collected in beaker
  5. crystals in flask and liquid in beaker
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20
Q

what can simple distillation be used for and a con of this

A

to produce drinking water from sea water
requires a great deal of energy

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21
Q

what is fractional distillation used for

A

separating a mixture of different liquids with different boiling points

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22
Q

how is the set up for fractional distilation different to the set up for simple distillation

A

the flask containing mixture is connected to a fractionating column (long column with hundreds of glass beads)

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23
Q

process of fractional distillation

A

. gently heat mixture
. both liquids start to evaporate
(lowest bp evaporate easier)
. mixture of two vapours making way up
fractionating column
. vapours hit fractionating column, they condense + drip back into flask and evaporate again
. repeated evaporation and condensation increases amount of lower b.p chemical in fractionating column
.warm vapours past column and reach thermometer (temp of thermometer rises)
-mixture passing thermometer has more of low b.p vapour
-vapours pass into condenser and becomes a liquid.
(still a mix of two chemicals)
-temp of thermometer reaches boiling point of lower bp chemical and stops rising
-swap to new flask, now much more lower bp chemical is evaporating and condesing into flask -(Higher bp chemical isnt evaporating or condensing much)
-we get our first pure sample of low bp chemical
-Temp of thermometer rises again-
mixture of vapour condenses into beaker(more high bp then low)
- when temp is constant, swap to new beaker- relatively pure sample of high bp chemical is collecteted

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24
Q

what does chromatography do

A

separate substances based on different solubilities

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25
Q

how can chromotography be used to find out which pens contain a mix / one colour

A

draw pencil line on chromatography paper - near bottom
put dot of first colour on pencil line and dot of second next
place bottom of paper in solvent
solvent makes its way up paper dissolves ink in coloured dots
ink is carried up paper as well

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26
Q

what is the stationary phase

A

the paper, it does not move

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27
Q

what is the mobile phase

A

solvent is the mobile phase as it moves

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28
Q

how to tell if a dye is pure

A

a pure compound will produce a single spot in all solvents

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29
Q

how to tell if a dye is a mixture

A

compounds in a mixture may separate into different spots depending on the solvent used

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30
Q

why does paper chromatography work

A

different substances have different solubilities . A more soluble substance travels further up the paper than a substance that is less soluble. That way we can seperate substances based on solubility

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31
Q

why do we draw our staring line in pencil

A

if we drew line in pen, pen ink would move up the paper, with the solvent

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32
Q

how do you measure distance moved by chemical

A

from pencil line to centre of spot

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33
Q

Rf value =

A

distance moved by substance / distance moved by solvent

no unit…

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34
Q

how to identify an unknown substance

A

workout Rf value and compare to datatbase
if 1+ substances have this Rf value than compare it in other solvents

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35
Q

in chromatography, what would you do if different substances have the same rf value

A

repeat with different solvent

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36
Q

Before the discovery of the electron, atoms were thought to be …………………

A

tiny spheres that could not be divided

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37
Q

The plum pudding model suggested that the atom is a ……………………..

A

ball of positive charge with negative electrons embedded in it.

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38
Q

the discovery of which subatomic particle led to the plum pudding model

A

The discovery of the electron led to the plum pudding model of the
atom

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39
Q

what did the discovery of electrons show?

A

that atoms are not solid spheres and can be divided into smaller parts and have internal structure

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40
Q

why was the alpha scattering experiment carried out

A

to check if the plum pudding model was correct

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41
Q

how was alpha scattering experiment carried out?

A

1 alpha particles ( w/ positive charge) fired at piece of gold foil -few atoms thick
2 expected particles to travel through foil
3 some alpha particles bounced back / some deflected

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42
Q

why were particles deflected, bounced back , go straight through

A

alpha particles with + charge repelled by + charge in centre of atom
bounced back, directly striked nucleus
straight through, went through empty space

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43
Q

most of the particles went through foil- what did this show…..
some particles deflected showed…

A

most of atom is empty space
centre of atom has + charge

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44
Q

what model replaces the plum pudding model

A

the nuclear model

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45
Q

what conclusion did the results from the Alpha scattering experiment lead to ?
3 points

A

. the mass of an atom and + charge is concentrated at the centre
(nucleus)
. atom mainly empty space

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46
Q

describe nuclear model

A

most of atom is empty
positive nucleus
cloud of electron surround nucleus

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47
Q

how was the nuclear model adjusted

A

electrons orbit the nucleus at specific distances

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48
Q

who adjusted the nuclear model

A

Neil Bohr

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49
Q

Bohr said electrons orbit at fixed distances. why was this accepted

A

his work agreed with the results of experiments by other scientists

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50
Q

how was the electron shell (bohr) model different to the nuclear model

A

it showed electrons orbiting in shells, fixed energy levels

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51
Q

what was discovered after energy shells

A

the proton

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52
Q

Further experiments provided evidence that the ……….. contained …… particles called ……..

A

Further experiments provided evidence that the nucleus contained smaller particles called protons

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53
Q

who discovered neutrons in the nucleus

A

James chadwick

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54
Q

The experimental work of……. ……….. provided the evidence
to show the existence of …… within the nucleus. This was
about … ….years after the nucleus became an accepted scientific
idea.

A

The experimental work of James Chadwick provided the evidence
to show the existence of neutrons within the nucleus. This was
about 20 years after the nucleus became an accepted scientific
idea.

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55
Q

why do atoms have no overall charge

A

same number of protons and electrons

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56
Q

charges of:
electron
proton
neutron

A

electron -1
proton +1
neutron 0

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57
Q

what is the atomic number

A

number of protons

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58
Q

All atoms of a particular element have …… number of
protons

A

. All atoms of a particular element have the same number of
protons

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59
Q

radius of an atom

A

0.1 nm

(1 x 10 to ^-10 m)

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60
Q

radius of atom in metres

A

1 x 10 to the power of -10 metres

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61
Q

radius of nucleus

A

less than 1/ 10 000 of atoms radius

1x 10 to the power of -14 metres

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62
Q

mass of
electron
proton
neutron

A

electron very small
proton 1
neutron 1

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63
Q

what is mass number

A

sum of Protons and Neutrons

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64
Q

which number is mass/ atomic number?

   23 Na 
  11
A

atomic = 11
smaller number
mass= 23
larger number

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65
Q

is atomic number the smaller or larger number

A

smaller

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66
Q

to work out neutrons…

A

mass number- atomic number

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67
Q

what is an isotope

A

atom of same element with different neutron number

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68
Q

what are ions

A

atom with an overall charge
lost or gained electrons

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69
Q

The relative atomic mass of an element is an…………value that
takes account of the…….. of the……. of the element

A

The relative atomic mass of an element is an average value that
takes account of the abundance of the isotopes of the element

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70
Q

what does a different mass number mean

A

different neutron number

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71
Q

equation for relative atomic mass

A

(mass of isotope1 x % of isotope 1)
+
(mass of isotope2 x % of isotope 2)
divided by 100

72
Q

how many electrons in each shell

A

2
8
8
18

73
Q

what does the outer electron number tell you about element in the table

A

group number

74
Q

The elements in the periodic table are arranged in order of ………. number

A

The elements in the periodic table are arranged in order of atomic
(proton) number

75
Q

why is it called periodic table

A

elements with similiar properties occur at regular intervals

76
Q

group 1 consists of?

A

highly reactive metals
eg lithium
sodium
potassium

77
Q

group 7 consist of ?

A

highly reactive non metals
fluorine
chlorine
bromine

78
Q

why do elements in same group have similar chemical properties?

A

because Elements in the same group in the periodic table have the same number of electrons in their outer shell

79
Q

Before the discovery of protons, neutrons and electrons,how were elements arranged

A

in order of atomic weights

80
Q

problems of earlier periodic tables x 2

A

incomplete
some elements placed in inappropriate groups if strict order of atomic weights followed.

81
Q

what did mandeleev arrange periodic table by

A

increasing atomic weight

82
Q

Mendeleev overcame some of the problems by…..

A

leaving gaps for undiscovered elements
sometimes changed the order based on atomic weights

83
Q

why did mandeleev switch the order of specific elemts

A

so they fitted the pattern of other elements in the same group

84
Q

what was surprising about madeleevs periodic table- why was table accepted

A

mandeleev predicted properties of undiscovered elements
Elements with these properties were discovered and filled the gaps.

85
Q

differences between mandeleevs table and modern one

A

modern- arranged by atomic number (protons)
modern- has group 0 (not all discovered when madeleev made his table).

86
Q

why was ordering by atomic weight not always correct

A

due to isotopes ( different neutron no.)

87
Q

are noble gases reactive or unreactive

A

unreactive

88
Q

why are noble gases unreactive

A

They are unreactive and do not easily form molecules
because their atoms have stable arrangements of electrons.

89
Q

which noble gas has 2 electrons

A

helium

90
Q

what INCREASES down EVERY group

A

atomic mass

91
Q

what happens to boiling points down gr 0

A

b.p increases down group 0

92
Q

describe the b.p of noble gases

A

lower than room temp (as they’re gases)

93
Q

are most of the elements metals or non metals

A

metals

94
Q

where are the metals found on the table

A

to the left and centre

(to remember this- think that most of the world is left handed…)

95
Q

where are non metals found on periodic table?

A

right

96
Q

what groups are highly reactive metals

A

group 1 and 2

97
Q

transitional metals are generally more or less reactive than group 1 and 2 metals?

A

less

98
Q

describe what happens when a metal reacts- in terms of electrons
why does this happen
what is the end result

A

lose electrons
to achieve full outer energy level
have electronic structure as noble gas

99
Q

Elements that react to form ………. ions are metals.
Elements that form ……… ions are non metals

A

Elements that react to form positive ions are metals.
Elements that do not form positive ions are non-metals.

100
Q

why do metals form + ions

A

Metals LOSE electrons

101
Q

how do you show an element has become an ion

A

Square brackets
charge on right corner
[ Li ] +

102
Q

name for group 1 metals

A

alkali metals

103
Q

how many outer electrons do group 1 metals have

A

1

104
Q

are group 1 metals hard or soft

A

soft

105
Q

describe the reaction of group 1 metals with oxygen

A

react rapidly with oxygen

106
Q

what happens to reactivity down group 1

A

reactivity increases down group 1

107
Q

all group 1 metals react similarly with oxygen. why

A

because they all have 1 outer electron

108
Q

complete and balance
Li + O¬2 =
group 1 reacting with oxygen molecule

A

4Li + O¬2= 2 Li¬2O

1 O needs 2 Li
O¬2 needs 4 Li
2 Li¬2O is produced

109
Q

what does 1 chlorine molecule
and 1 oxygen molecule contain

A

chlorine molecule =2 chlorine atoms
oxygen molecule= 2 oxygen atoms
(Cl2, O2)

110
Q

describe reaction of group 1 metals with chlorine and oxygen

A

react rapidly

111
Q

complete and balance
Na + Cl =
group 1 and group 7

A

2Na + Cl¬2= 2 NaCl

because Cl is diatomic.
we must use 2 Cl so we also use 2 Na

112
Q

complete and balance
Na + O¬2 =
group 1 and oxygen molecule (group 6)

A

4Na + O¬2 = 2 Na¬2O

113
Q

alkali metal + oxygen =

A

alkali metal + oxygen = metal oxide

114
Q

alkali metal + chlorine =

A

alkali metal + chlorine = metal chloride

115
Q

elements that react to form ……. …….. are metals

A

positive ions

116
Q

what is an ion

A

an atom with a different electron number

117
Q

a group 1 metal reacts with oxygen in the air
eg
sodium + oxygen. what is formed

A

sodium oxide

118
Q

4Li + O2 =
(Li is group 1, O is group 6)

A

2 Li¬2O

119
Q

write balanced equation for sodium and one molecule of oxygen

A

4Na + O2 = 2 Na¬2O
the first 2 applies to all of the elements

120
Q

what happens when lithium is added to water
x4

A

reacts rapidly
effervescence-fizzing
gas produced
water turns alkaline

121
Q

what happens when sodium is added to water
x4 and 1 comparison to other group 1 elements

A

reacts very rapidly
effervescence
gas produced
water turns alkaline
reacts more rapidly than lithium

122
Q

what happens when potassium is added to water
x4 and 1 comparison to other group 1 elements

A

reacts extremely rapidly
effervescence
gas produced
water turns alkaline
reacts more rapidly then lithium and sodium

123
Q

write word equation for lithium and water

A

lithium and water= lithium hydroxide and hydrogen

124
Q

why does the universal indicator in the water turn purple when group 1 elements are added

A

products of group 1 metal and water = group 1 hydroxide + hydrogen
(eg lithium hydroxide and hydrogen)
a group 1 hydroxide is an alkali
( regardless of what group 1 it is )

125
Q

why do we see effervescence when a group 1 element is added to water

A

(products of group 1 metal and water = group 1 hydroxide + hydrogen)
Hydrogen is formed and hydrogen is a gas so we see bubbling

126
Q

write balanced chemical equation for li + H2O

A

(could be: Li + H2O = LiOH + H2
but H isn’t balanced
so: )
2Li + 2H¬2O= 2 LiOH + H2

127
Q

write balanced chemical equation for Na + H2O

A

2Na + 2H2O= 2NaOH + H2

128
Q

write balanced chemical equation for K + H2O

A

2K + 2H2O= 2KOH + H2

129
Q

what are the products made when the first 3 group 1 metals are added to water

A

lithium hydroxide and hydrogen
sodium hydroxide and hydrogen
potassium hydroxide and hydrogen

130
Q

name first three group 1 elements going down the group

A

lithium
sodium
potassium

131
Q

down group 1 you have:
lithium
sodium
potassium
what can you say about the size of these atoms going down the group

A

size of atoms increase down group, they have increasing electron number

132
Q

why does reactivity increase down group 1
5 points

A

-down group, size of atom increases
-there is greater distance btwn + nucleus and -outer electron
- outer electron also shielded from nucleus by internal energy levels
-this means outer electron less attracted to nucleus
- so outer electron easier to lose and element is more reactive

133
Q

what are group 7 elements called

A

halogens

134
Q

if 2 group 7 elements are reacted together they will form….

A

a molecule with 2 atoms joined by a covalent bond

135
Q

describe how a covalent bond is made when 2 group 7 elements react together

A

they overlap their outer energy levels
then
share a pair of electrons

136
Q

F-F is a covalent bond
what has been formed

A

fluorine molecule

137
Q

what elements are diatomic

A

group 7
oxygen
hydrogen
nitrogen

138
Q

what happens to melting point and boiling point and relative molecular mass of group 7 elements down group

A

increases down group

139
Q

what is room temp

A

20 degrees

140
Q

bromine is a liquid at room temp
relate this to its melting and boiling points

A

bromine melting point is below 20 degrees
but bromine boiling point is above 20 degrees

141
Q

fluorine and chlorine are gas at room temp
relate this to their boiling point

A

their boiling point is lower than 20 degrees

142
Q

iodine is a solid at room temp
relate this to its melting point and boiling point

A

iodine’s melting & boiling point is higher than 20*

143
Q

the RMM increases down group 7
(relative molecular mass)
explain what this means in 5 words

A

molecules get bigger down group

144
Q

are halogens metals or non metals

A

non metals

145
Q

what kind of bond would atoms of the same group 7 elements form together. eg 2 fluorine atoms.

A

a single covalent bond

146
Q

what do group 7 elements form when they react with OTHER NON -metal atoms

A

covalent compounds

147
Q

in fractional distillation , what might we have to do if liquids have similar boiling points

A

carry out several rounds of fractional distillation

148
Q

why do gr 7 atoms from covalent compounds with other non metal atoms

A

covalent- because as the atoms are non-metal, they each want to gain electrons

compound- because its atoms of Different element chemically joined

149
Q

halogen + non metal atom=
eg chlorine and hydrogen

A

covalent compound
eg hydrogen chloride

150
Q

what do group 7 elements form when they react with metals

A

ionic compounds

151
Q

Li + Cl =
(gr1 metal) (gr7 non-metal)
what ions are formed

A

Cl-
Li+

152
Q

how do you remember that gr 7 reacting with a metal = ionic compounds

A

it would be ionic because its a bond between a metal and non metal
and a compound because its 2 different elements

153
Q

when halogens form 1-ions, how do their names change.
give an example

A

the -ine turns into -ide
eg fluorine turns to fluoride

154
Q

what happens to reactivity down group 7

A

reactivity decreases down group 7

155
Q

describe what the relative atomic mass is in your own words.
you can use the example of chlorine

A

isotopes of chlorine have different mass numbers (they have a different neutron number so their weight changes)
there are two main isotopes of chlorine. they have a weight of 35 and 37
to decide what mass number of chlorine should go on the table, scientists worked out the relative atomic mass by using the equation.
they took into account how common each isotope is (the abundance)

156
Q

what is the negative electron attracted to

A

the + charge of the nucleus

157
Q

what happens to the halogens when they react with metals

A

they gain an electron

158
Q

why does reactivity decrease down group 7 halogens
5 points

A

further down the group:
-greater distance between outer energy level and nucleus
-more internal electrons shield the outer energy electrons from positive charged nucleus
-less attraction between outer electrons and nucleus
-harder for elements lower down to attract an electron to its outer energy level
-so they are less reactive than elements higher in group 7

159
Q

what happens when:
sodium bromide + fluorine

A

fluorine more reactive than bromine
fluorine can push out the bromine-
a displacement reaction happens

160
Q

complete word equation
sodium bromide + fluorine =

  • fluorine is the first element in group 7
    -bromine is the third element in group 7
A

sodium fluoride + bromine

161
Q

A more reactive halogen can displace a less reactive halogen from
an aqueous solution of its salt.

give example of ‘an aqueous solution of its salt’ for different group 7 elements
fluorine
chlorine
bromine
iodine
astatine

A

sodium fluoride
sodium chloride
sodium bromide
sodium iodide

162
Q

potassium iodide + chlorine =

group 7 elements down the column:
fluorine
chlorine
bromine
iodine
astatine

A

potassium chloride + iodine

  • chlorine is more reactive then iodine so it displaces iodine*
163
Q

A more reactive halogen can displace a less reactive halogen from what

A

aqueous solution of its salt.

164
Q

what have we done to make sodium bromide an aqueous solution

A

dissolved it in water

165
Q

where on the table are nonmetals found

A

right hand side

166
Q

here are transitional metals found on table

A

central part

167
Q

5 main properties of alkali metals

A

soft
low melting point
low density
react rapidly
form +1 ion

168
Q

name three substances alkali metals react very rapidly with

A

oxygen
chlorine
water

169
Q

what group are alkali metals

A

group 1

170
Q

7 properties of transition metals

A

hard+ strong
high melting points
high density
less reactive than group 1
form ions with different charges
form coloured compounds
can be used as catalysts

171
Q

where in the table are metals found

A

left hand side

172
Q

lithium chloride + bromine=

group 7 elements down the column:
fluorine
chlorine
bromine
iodine
astatine

A

lithium chloride+ bromine

*bromine is less reactive than chlorine so it doesn’t displace *

173
Q

give an example of a transition element that can form a coloured compound and the colour

A

iron (lll) oxide - red
manganese (ll) chloride - pink
chromium (lll) chloride - purple

174
Q

compare the properties of group 1 alkali metals and transition metals
7 points

A

ALKALI’S:
soft
low melting point
low density
react rapidly
form +1 ion
TRANSITION METALS:
hard/strong
high melting point
high density
less reactive
form ions with different charges
-coloured compounds
-used as catalysts

175
Q

what ionic charges can iron form

A

Fe 2+
Fe 3+

Chemistry (18 decks)

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