Cambridge IGCSE™

* 1 6 8 3 2 9 8 6 6 6 *

CO-ORDINATED SCIENCES 0654/43

Paper 4 Theory (Extended) October/November 2022

2 hours

You must answer on the question paper.

No additional materials are needed.

INSTRUCTIONS
● Answer all questions.
● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
● Write your name, centre number and candidate number in the boxes at the top of the page.
● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
● Do not write on any bar codes.
● You may use a calculator.
● You should show all your working and use appropriate units.

INFORMATION
● The total mark for this paper is 120.
● The number of marks for each question or part question is shown in brackets [ ].
● The Periodic Table is printed in the question paper.

This document has 32 pages. Any blank pages are indicated.

DC (LK/CT) 302056/6
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1 (a) Gills are the gas exchange surface in fish.

Fig. 1.1 is a photograph of gills in fish.

Fig. 1.1

Gills have adaptive features for gas exchange.

Use your scientific knowledge and Fig. 1.1 to suggest two of these adaptive features.

1 ................................................................................................................................................

2 ................................................................................................................................................
[2]

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(b) Table 1.1 shows the composition of some gases in inspired and expired air.

Table 1.1

gas

percentage of oxygen percentage of carbon dioxide

inspired air 21 0.004

expired air 16 4

(i) Use Table 1.1 to calculate the difference in percentage of oxygen between inspired and
expired air.

................................................................................................................................. % [1]

(ii) Explain the difference in percentage of oxygen between inspired and expired air that is
shown in Table 1.1.

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [2]

(iii) State one difference in composition between inspired and expired air that is not shown
in Table 1.1.

...........................................................................................................................................

..................................................................................................................................... [1]

(c) Red blood cells have adaptive features for the efficient transport of oxygen.

State two of these features.

1 ................................................................................................................................................

2 ................................................................................................................................................
[2]

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(d) Lung cancer is a disease caused by smoking.

(i) Place ticks (3) to show two other diseases caused by smoking.

chronic obstructive pulmonary disease (COPD)

coronary heart disease

kwashiorkor

marasmus

scurvy

[2]

(ii) State the name of the component in tobacco smoke that causes cancer.

..................................................................................................................................... [1]

(iii) Describe how the goblet cells, mucus and ciliated cells protect the gas exchange system
from some of the particles in tobacco smoke.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [3]

[Total: 14]

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2 (a) A student investigates two liquid fuels, A and B, to find out which fuel releases most energy.

Fig. 2.1 shows the apparatus used. 1.5 g of each fuel is burned completely.

thermometer

copper can

100 g water

spirit burner
1.5 g of liquid fuel

Fig. 2.1

Table 2.1 shows the student’s results.

Table 2.1

temperature of temperature of temperature

fuel water at start water at end change
/ °C / °C / °C
A 16 25 9
B 16 34 18

(i) Describe how the results show which fuel releases the most energy.

...........................................................................................................................................

..................................................................................................................................... [1]

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(ii) Fig. 2.2 is the equation representing the complete combustion of ethanol.

H H O H
O
H C C O H + 3 2 C + 3 O
O
H H O H

Fig. 2.2

This reaction is exothermic.

Place a tick (3) in the box next to the correct explanation of an exothermic reaction.

More energy is given out by bond breaking

than is taken in by bond making.

More energy is given out by bond making

than is taken in by bond breaking.

More bonds are broken than are made.

More energy is taken in by bond breaking

than is given out by bond making.
[1]

(b) Fig. 2.3 shows the energy level diagram for an exothermic reaction.

200

reactants
150
energy / kJ
100

products
50

progress of reaction

Fig. 2.3

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(i) Use Fig. 2.3 to calculate the energy given out in the reaction.

energy given out = .................................................... kJ [1]

(ii) Use Fig. 2.3 to calculate the activation energy for the reaction.

activation energy = .................................................... kJ [1]

(c) Ethanol can be made by

• the catalytic addition of steam to ethene

• fermentation.

(i) Construct the balanced symbol equation for the addition of steam to ethene to make
ethanol, C2H5OH.

.................................. + .................................. .................................. [2]

(ii) Describe how ethanol is made by fermentation.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [3]

[Total: 9]

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3 Fig. 3.1 shows a man in a canoe on a lake.

The combined mass of the man and the canoe is 120 kg.

Fig. 3.1

(a) The canoe moves at a speed of 4.0 m / s.

(i) Calculate the kinetic energy of the man and the canoe.

kinetic energy = ...................................................... J [2]

(ii) The canoe takes 5.0 s to slow down to a speed of 0.5 m / s.

Calculate the constant deceleration of the canoe.

deceleration = ................................................ m / s2 [3]

(iii) On Fig. 3.2 draw a speed–time graph to show the canoe’s deceleration.

4.0

3.5

3.0

2.5

speed
2.0
m/s
1.5

1.0

0.5

0
0 1 2 3 4 5
time / s

Fig. 3.2
[1]
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(b) The canoe exerts a pressure of 0.5 kPa on the surface of the water.

Calculate the area of canoe in contact with the surface of the water.

The gravitational field strength, g, is 10 N / kg.

area = .................................................... m2 [3]

(c) Fig. 3.3 shows water waves on the surface of the lake.

Fig. 3.3

(i) On Fig. 3.3, draw a double headed arrow (↕ or ↔) to show the wavelength of the wave.
[1]

(ii) Use the words below to complete the sentences about waves.

You can use each word once, more than once or not at all.

compression energy force longitudinal matter perpendicular

parallel rarefaction transverse

Waves transfer ...................................... without transferring ...................................... .

A water wave is an example of a ...................................... wave.

In a water wave the oscillations are ...................................... to the direction of the wave.
[2]

[Total: 12]

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4 (a) A student investigates the effect of light intensity on the rate of photosynthesis in an aquatic
plant. The plant is placed in a beaker of water containing an excess of carbon dioxide.

A lamp is placed 10 cm away from the beaker of water.

The student counts the number of oxygen bubbles produced by the aquatic plant in one
minute.

The lamp is then moved increasing distances away from the beaker to decrease the light
intensity.

The number of oxygen bubbles produced is directly proportional to the rate of photosynthesis.

Table 4.1 shows the results.

Table 4.1

distance of lamp from the aquatic plant number of oxygen bubbles produced per
/ cm minute
10 37
20 37
30 36
40 32
50 25
60 15
70 6
80 1

(i) Use Table 4.1 to describe the effect of light intensity on the rate of photosynthesis.

Include data in your answer.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [2]

(ii) State why an excess of carbon dioxide is provided for the aquatic plant during this
investigation.

...........................................................................................................................................

..................................................................................................................................... [1]

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(b) Complete the sentences to explain how a lack of magnesium affects plant growth.

Magnesium is required for the synthesis of .............................................. .

This substance transfers light energy into .............................................. energy for the
synthesis of carbohydrates.

A deficiency of magnesium ions causes the leaves to turn .............................................. .

[3]

(c) Nitrate ions are required for the synthesis of amino acids.

State the name of the class of large molecules made from amino acids.

............................................................................................................................................. [1]

[Total: 7]

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5 This question is about metals.

(a) Potassium is a metal in Group I of the Periodic Table.

Fig. 5.1 shows the electronic structure of three elements.

A B C

Fig. 5.1

(i) State which diagram A, B or C, shows the electronic structure of a Group I metal.

..................................................................................................................................... [1]

(ii) A student wants to confirm that a compound contains potassium.

The student uses a flame test.

State what the student observes if the compound contains potassium.

..................................................................................................................................... [1]

(b) Iron is a transition element.

Iron(II) sulfate contains iron(II) ions, Fe2+.

Sodium hydroxide solution is used to test for iron(II) ions.

The iron(II) ions react with OH– ions from the sodium hydroxide solution. A precipitate of
iron(II) hydroxide, Fe(OH)2, is made.

(i) State the colour of the precipitate of iron(II) hydroxide.

..................................................................................................................................... [1]

(ii) Construct the balanced ionic equation for the formation of Fe(OH)2. Include state
symbols.

..................................................................................................................................... [2]

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(c) Magnesium reacts with oxygen to make magnesium oxide.

(i) Fig. 5.2 shows the electronic structure of a magnesium atom.

The proton number (atomic number) of magnesium is 12.

Fig. 5.2

Draw a diagram to show the electronic structure of an oxygen atom.

The proton number (atomic number) of oxygen is 8.

[1]

(ii) When magnesium reacts with oxygen, magnesium ions and oxide ions are made.
Fig. 5.3 shows the electronic structure of an oxide ion.

2–

Fig. 5.3

Draw a diagram to show the electronic structure of a magnesium ion.

[2]

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(iii) Explain why magnesium oxide has a high melting point.

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [2]

(d) Potassium oxide is also an ionic compound.

Potassium ions, K+, combine with oxide ions, O2–, to form potassium oxide.

Determine the formula of potassium oxide.

............................................................................................................................................. [1]

[Total: 11]

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6 Fig. 6.1 shows a marble staircase made up of 17 steps.

Fig. 6.1

(a) Fig. 6.2 shows the dimensions of one of the marble steps which has a mass of 72 kg.

0.16 m

0.20 m

0.90 m

Fig. 6.2

(i) Calculate the density of the marble step.

density = .............................................. kg / m3 [3]

(ii) On a hot, sunny day the marble step expands.

Suggest what happens to the density of the marble step when it expands.

..................................................................................................................................... [1]

(iii) Explain, in terms of particle movement, why the marble expands.

...........................................................................................................................................

..................................................................................................................................... [1]

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(b) (i) On a hot, sunny day the marble steps feel cold because of conduction.

Describe the process of conduction in marble.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [2]

(ii) Explain why conduction causes the marble to feel cold.

...........................................................................................................................................

..................................................................................................................................... [1]

[Total: 8]

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7 (a) Yeast produces carbon dioxide during anaerobic respiration.

A scientist adds 2 g of yeast to 250 cm3 of glucose solution and leaves the mixture for
10 days.

Each day, at the same time, he records the volume of carbon dioxide produced in one hour.

Fig. 7.1 shows the results.

40

35

30

25
volume of
carbon dioxide
produced in 20
one hour / cm3
15

10

0
0 2 4 6 8 10
time / days

Fig. 7.1

(i) Use Fig. 7.1 to identify the day with the greatest rate of anaerobic respiration.

..................................................................................................................................... [1]

(ii) Explain why the volume of carbon dioxide decreases as shown in Fig. 7.1.

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [2]

(b) The investigation is repeated with boiled yeast.

Explain with reference to enzymes why no carbon dioxide is produced.

...................................................................................................................................................

...................................................................................................................................................

...................................................................................................................................................

............................................................................................................................................. [3]

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(c) Table 7.1 shows some products of different types of respiration.

Complete Table 7.1 by placing ticks (3) to show the correct products of each type of
respiration.

One has been done for you.

Table 7.1

products of respiration

type of respiration carbon dioxide water lactic acid

aerobic in humans

anaerobic in
humans

anaerobic in yeast 3

[3]

(d) Substances enter and leave a yeast cell by diffusion.

A student writes an incorrect definition of diffusion.

Circle the two words that are not correct.

‘Diffusion is the total movement of particles from a region of their higher concentration

to a region of their lower concentration up a concentration gradient, as a result of their

random movement.’
[2]

[Total: 11]

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8 (a) Water must be treated so that it is safe to drink.

Draw lines to link each stage in the water treatment process to the reason why it is used.

stage reason

kills microbes

filtration

allows larger solid particles to settle out

chlorination

traps finer particles using sand

[2]

(b) Water can be tested to identify some of the chemicals in it.

A scientist tests a sample of water from a river with acidified aqueous silver nitrate and also
with acidified aqueous barium chloride.

Table 8.1 shows the results.

Table 8.1

with acidified with acidified

test aqueous silver aqueous barium
nitrate chloride
result cream precipitate white precipitate

The scientist thinks that the water contains both chloride and sulfate ions.

State whether the scientist is correct.

Explain your answer.

...................................................................................................................................................

...................................................................................................................................................

............................................................................................................................................. [2]

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(c) Barium chloride, BaCl 2, reacts with sodium sulfate, Na2SO4.

Barium sulfate, BaSO4, and sodium chloride, NaCl, are made.

Construct the balanced symbol equation for this reaction.

............................................................................................................................................. [2]

(d) Carbon dioxide dissolves in rainwater to make the water weakly acidic.

Suggest the pH of the rainwater produced.

pH = ......................................................... [1]

(e) The atoms in carbon dioxide, CO2, are bonded by sharing electrons.

Fig. 8.1 shows some dot-and-cross diagrams.

O C O O C O

A B

O C O O C O

C D

Fig. 8.1

(i) State which diagram A, B, C or D, shows the arrangement of the outer shell electrons in
carbon dioxide.

diagram = ......................................................... [1]

(ii) State the name of this type of bonding that holds the atoms together in carbon dioxide.

..................................................................................................................................... [1]

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(f) Complete the following sentences about some of the problems caused by carbon dioxide.

Choose words from the list. Each word or phrase may be used once, more than once or not
at all.

climate change greenhouse oxidation

noble rusting

Carbon dioxide is a ................................................ gas.

Increased concentrations of carbon dioxide in the atmosphere

contribute to ................................................ .
[2]

[Total: 11]

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9 Fig. 9.1 shows the equipment used by a teacher to demonstrate the properties of ionising radiation
to a group of students. They are using a source which emits β-particles.

radiation detector counter

019

source emitting β-particles

Fig. 9.1

(a) The radioactive source can be moved further away from the radiation detector. The teacher
measures the distance between the source and the radiation detector and records the count
rate using the laptop.

Fig. 9.2 shows the results plotted as a graph.

200

150

counts per minute

100

50

0
0 10 20 30 40 50
distance / cm

Fig. 9.2

(i) Describe the trend shown in Fig. 9.2.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [2]

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(ii) Use Fig. 9.2 to explain why the teacher tells the students to stand at least 2 m away from
the radioactive source for their own safety.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [2]

(iii) The teacher replaces the radioactive source with one which only emits α-particles.

The source which only emits α-particles also measures a count rate of 200 per minute at
a distance of 0 m.

On Fig. 9.2, draw a line to show the results the teacher obtains when using the source
which emits only α-particles.
[2]

(b) Fig. 9.3 shows the information sticker on the laptop.

power input = 65 W

potential difference = 19.5 V

Fig. 9.3

(i) The laptop has an efficiency of 80%.

Calculate the useful power output of the laptop.

power = ..................................................... W [2]

(ii) Power for the laptop comes from a 230 V supply through a device in the charger which
changes the potential difference to 19.5 V.

State the name of this device.

..................................................................................................................................... [1]

[Total: 9]

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10 (a) Albinism is a condition that results in a lack of colour in the skin causing a very pale
appearance.

The allele for albinism is recessive, a.

The allele for no albinism is dominant, A.

Fig. 10.1 is a pedigree diagram showing the inheritance of albinism.

Key no albinism albinism

male

Q
female

Fig. 10.1

The boxes on the left represent person P and person Q as shown in Fig. 10.1.

The boxes on the right complete statements about person P and person Q.

Draw two lines from person P and two lines from person Q to make four correct statements.

has a heterozygous genotype.

Person P has albinism.

has a homozygous recessive

genotype.

has the genotype AA.

Person Q
is male.

is female without albinism.

[4]

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(b) Alleles are passed to offspring during sexual reproduction.

The sex cell in human males is sperm.

(i) State the name of the sex cell in human females.

..................................................................................................................................... [1]

(ii) State the number of chromosomes in one human sperm cell.

..................................................................................................................................... [1]

(iii) State the number of sex chromosomes in a body cell of a human male.

..................................................................................................................................... [1]

(iv) State the number of parents required for asexual reproduction.

..................................................................................................................................... [1]

[Total: 8]

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11 Diamond is one form of carbon.

(a) (i) State the name of another form of carbon.

..................................................................................................................................... [1]

(ii) Diamond is used in cutting tools such as those shown in Fig. 11.1.

Fig. 11.1

State why diamond is used.

...........................................................................................................................................

..................................................................................................................................... [1]

(b) Silicon dioxide, SiO2, has a similar structure to diamond.

Fig. 11.2 shows the structure of silicon dioxide.

silicon atoms
oxygen atoms

Fig. 11.2

Describe the structure and bonding in silicon dioxide.

Use Fig. 11.2 to help you.

...................................................................................................................................................

...................................................................................................................................................

............................................................................................................................................. [2]

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(c) One of the isotopes of carbon is called carbon-12 and the other is called carbon-14.

Table 11.1 shows some information about carbon-12.

Complete the table for carbon-14.

Table 11.1

number of number of
number of protons
neutrons electrons

carbon-12 6 6 6

carbon-14

[1]

(d) Relative atomic mass, Ar , is defined in terms of a carbon atom.

Complete the definition of relative atomic mass.

Choose words from the list. Each word may be used once, more than once or not at all.

average compound density

element formula mass

Relative atomic mass is the ................................... mass of naturally

occurring atoms of an ................................... on a scale where the 12 C atom has a

................................... of exactly 12 units.

[3]

(e) Calculate the number of moles in 0.6 g of carbon.

[Ar : C, 12;]

moles = ......................................................... [1]

[Total: 9]

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12 Fig. 12.1 shows a circuit containing two resistors connected in parallel with a 9.0 V battery.

9.0 V

12.0 Ω

6.0 Ω

Fig. 12.1

(a) (i) Calculate the total resistance of the circuit shown in Fig. 12.1.

total resistance = ..................................................... Ω [2]

(ii) Calculate the current passing through the 6.0 Ω resistor.

current = ...................................................... A [2]

(b) The 9.0 V battery is connected in series with a lamp, a variable resistor and a switch.

(i) Draw a circuit diagram showing a 9.0 V battery connected in series with a lamp, a variable
resistor and a switch.

[2]

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(ii) The variable resistor is used to change the voltage across and the current in the lamp.

On Fig. 12.2, sketch a graph showing the current-voltage characteristic of a filament

lamp.

current

voltage

Fig. 12.2
[1]

(c) Fig. 12.3 shows a circuit containing a thermistor and a lamp in series with an ammeter.
A voltmeter is connected in parallel across the thermistor.

9.0 V

Fig. 12.3

(i) Describe what happens to the readings on the ammeter and voltmeter when the
temperature of the thermistor increases.

Use the words increases, decreases or stays the same.

Each word may be used once, more than once or not at all.

ammeter ....................................................................................

voltmeter ....................................................................................
[1]

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(ii) Explain why the brightness of the lamp changes as the temperature of the thermistor
increases.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [3]

[Total: 11]

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© UCLES 2022 0654/43/O/N/22

 The Periodic Table of Elements
Group
I II III IV V VI VII VIII

© UCLES 2022
1 2

H He
hydrogen helium
Key 1 4
3 4 atomic number 5 6 7 8 9 10

Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
7 9 relative atomic mass 11 12 14 16 19 20
11 12 13 14 15 16 17 18

Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
23 24 27 28 31 32 35.5 40
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
32

85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131
55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
lanthanoids

0654/43/O/N/22
Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – –
87 88 89–103 104 105 106 107 108 109 110 111 112 114 116
actinoids
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv
francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium flerovium livermorium
– – – – – – – – – – – – –

57 58 59 60 61 62 63 64 65 66 67 68 69 70 71
lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
139 140 141 144 – 150 152 157 159 163 165 167 169 173 175
89 90 91 92 93 94 95 96 97 98 99 100 101 102 103
actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
– 232 231 238 – – – – – – – – – – –

The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).