STUDENT SUPPLEMENT
www.rsc.org/eic
JULY 2009 • VOLUME 46 • NUMBER 4
Fluorescent
imaging
Looking inside
living cells
ISSN 0013-1350
GCSE science rethink
International review
Can assessment problems be
tackled by new criteria?
UK Research Councils and
chemists urged to talk more
ISSUE  JULY 
IN THIS
ISSUE
IONIC REALLY
Dead wood is abundant. Indeed
chemists are already looking to the
woody parts of plants that end up
as agricultural waste as potential
biofuels and as an alternative
source of industrial chemicals from
oil. But it’s not that easy, or is it?
Wood is made up of the
polysaccharides cellulose and
hemicellulose surrounded by the
highly branched polymer, lignin.
Lignin bonds to carbohydrates in
the plant, and crosslinks to the
polysaccharides. All in all, this is
what makes wood tough and
rigid. And herein lies the problem.
What chemists really want is the
lignin and cellulose separated.
Lignin can then be converted into
different products or used in
composite materials, such as
‘plastic wood’. Cellulose can be
used in advanced composites and
the synthesis of plastics, which
would provide a move away from
obtaining these materials from
oil-based chemicals. But
separating lignin from cellulose
and hemicellulose is an expensive,
energy-intensive process,
requiring high temperatures and
pressures. The process also uses
polluting chemicals such as
caustic soda and sodium sulfide.
JUPITERIMAGES
A  
Now chemists at Queen’s
University Belfast (QUB) have
discovered a greener way to
separate the chemicals that make
up wood. Reporting in the Royal
Star dust
Can chemists
unlock the
chemicals
from wood?
Chemists investigate the
mysteries of the cosmos
A day in the
life of…
Dan Clarke,
Advanced scientist
On-screen
chemistry
Society of Chemistry’s Green
chemistry journal, Professor Robin
Rogers and his colleagues describe
a process that involves dissolving
the wood in ‘ionic liquids’.
Ionic compounds are usually
high melting point solids, such as
sodium chloride. But in the late
1940s US chemists, Frank Hurley
and Tom Weir, when looking for a
quick way to electroplate
aluminium, discovered by mixing
and gently warming a powdered
organic salt – an alkylpyridinium
chloride – with aluminium
chloride, the powders reacted,
forming a clear, colourless liquid.
This was one of the first ‘ionic
liquids’.
Ionic liquids have some very
useful properties – they can
dissolve many different
compounds, they do not
evaporate, they are typically
non-combustible and can be
non-toxic, making them ideal
green solvents. In a crystalline
lattice like sodium chloride, the
ions behave like many apples
packed in a box. However, if bulky
organic anions replace the
chloride anions, these cannot pack
so neatly and it takes much less
energy to break the ions apart
– their lattice energy is low
enough to stop the mixture
crystallising and it remains liquid.
The QUB researchers found that
wood chips from both softwood
and hardwood trees, after mild
grinding to form a powder,
dissolved completely in their ionic
liquid – which comprises an
ethanoate anion – under mild
temperatures and low pressure.
The researchers then extracted the
cellulose and the lignin using
different propanone–water
mixtures, and recovered the ionic
liquid by distillation. ■
Download a pdf of this issue at: www.rsc.org/EiC
InfoChem_July 09..indd 1
Bungee jumping – with
a difference
Backyard
chemistry
Rainbow colours
Plus…
Prize puzzles
Editor
Kathryn Roberts
Assistant editor
James Berressem
Design and layout
Dale Dawson
Infochem is a supplement to Education
in Chemistry and is published
bi-monthly by the Royal Society of
Chemistry, Burlington House,
Piccadilly, London W1J 0BA, UK.
020-7437 8656, e-mail: [email protected]
www.rsc.org/Education/EiC/index.asp
© The Royal Society of Chemistry, 2009
Published in January and alternate
months. ISSN: 1752-0533
1
15/06/2009 16:51:59
   
ISSUE  JULY 
Some of the most fascinating discoveries in chemistry have taken place among distant
stars light years from Earth, in the clouds of cosmic dust and gas that separate these
far off worlds from our own. By attaching spectrometers to a telescope, scientists can
investigate the chemical cosmos, which may give clues to the origins of life on Earth.
T
he key to understanding
molecules in space lies in
the electromagnetic
spectrum. The 13th century
philosopher and Franciscan
friar Roger Bacon, also known as Doctor
Mirabilis, was the first scientist to recognise
that light, seemingly natural, white light from
the Sun produces a rainbow of colours – red,
orange, yellow, green, blue, indigo, and violet
– through a glass of water. Centuries later, in
1671, Sir Isaac Newton gave this rainbow its
modern name – the spectrum – after
carrying out sophisticated experiments with
sunlight and glass prisms, the basis of the
spectrometer.
A couple of centuries later, physicists
began to unravel the secrets of the visible
spectrum and beyond. They recognised, for
instance, that the spectrum represents a
range of energies. (The absorbed energy, ΔE,
is related to its frequency, ν, by the equation
ΔE = hν , where h is the Planck constant, and
the frequency of the absorbed or emitted
energy is inversely proportional to its
wavelength.) Red light has the least energy
(lowest frequency, and longest wavelength)
and violet has the most energy (highest
frequency and shortest wavelength).
The visible spectrum, however, is only a
very small part of the electromagnetic
spectrum, with infrared, microwaves, and
radio waves lying beyond the red end of the
visible spectrum and have gradually lower
energy. Ultraviolet, x-rays and gamma rays lie
beyond violet and have increasing energy.
NASA
Somewhere in a distant galaxy…
2
InfoChem_July 09..indd 2
S 
In the 19th century, scientists discovered that
light from distant stars when viewed through a
spectrometer does not produce a smooth
spectrum, but rather a series of ‘spectral lines’,
which are seen as bright or dark bands. The
positions of these lines in the spectrum
coincide with the absorption of energy by
different atoms and molecules (and thus
elements) in clouds of gas and dust lying
between the stars and the observer on Earth.
Each element has a characteristic spectral line.
Indeed, the elements helium, thallium, and
cerium were discovered on the basis of their
spectral lines.
There are now several analytical techniques
under the umbrella of spectroscopy that can
reveal structural details of molecules using
visible, infrared, or ultraviolet light. Shining the
light through a sample and recording how
much of the electromagnetic radiation is
absorbed at different energies (ie different
frequencies or wavelengths) on a spectrometer,
we can obtain information about an unknown
compound in the sample.
Molecules absorb energy from incident light
in different ways depending on their chemical
structure, the strength of their bonds, the
positions and mass of their atoms, and the
angles between those atoms. Molecules
vibrate, rotate, and bonds oscillate, depending
on the absorbed radiation. Characteristic
patterns of absorption are thus indicative not
only of particular elements, but also of different
bonds, or chemical groups or ions present in
the sample.
You may copy this page for use within schools
15/06/2009 16:52:16
 
Since it is impossible to collect a sample of
cosmic dust from a distant nebula and bring it
back to Earth for spectroscopic analysis, instead
space chemists use the light from stars lying
beyond the region of space they want to
sample as the source of electromagnetic
radiation. They use telescopes with
spectrometers attached to record the spectrum
of the material in the sample region.
DAVID A. HARDY/SCIENCE PHOTO LIBRARY; ISTOCKPHOTO
M 
Over several decades, scientists have recorded
the spectra of countless regions of space,
identifying elements, and simple and almost
ubiquitous small molecules such as hydrogen
(H2), water (H2O), methane (CH4), carbon
monoxide (CO), nitric oxide (NO), aluminium
monochloride (AlCl), iron oxide (FeO), and
ammonia (NH3), hydrogen cyanide (HCN),
carbonyl sulfide (OCS) , isocyanic acid (HNCO),
formaldehyde (H2CO), ketene (H2C2O), silane
(SiH4), ethanoic acid (CH3COOH), dimethyl
ether (CH3OCH3), and benzene (C6H6).
In all approximately 30 diatomic molecules
have been observed, 31 triatomic molecules, 18
species with four atoms, and 65 small
molecules with five or more atoms. There have
since been hints that much more complicated
molecules might be present in space and in
recent years researchers have begun to gather
evidence for the presence of such compounds.
In contrast, observers have found only rare
examples of charged molecules in space. One
of these, the hydronium ion (also known as
protonated water, H3O+), was first postulated by
Herbst and Kemplere in 1973 who went on to
identify the ion in 1986. The presence of such
ions in space is significant in that it suggests
that gas-phase reactions are taking place in
interstellar space, with the formation of
potentially complex molecules. The hydronium
ion is now known to be abundant in the
interstellar medium. It is found in diffuse and
dense molecular clouds as well as the plasma
tails of comets, such as Hale-Bopp.
In April 2008, scientists Arnaud
Belloche at the Max Planck Institute for
Radio Astronomy in Bonn, Germany,
Robin Garrod of the department of
astronomy, at Cornell University, US, and their
colleagues, detected a relatively complex
organic molecule, one that is closely related to
the amino acids used by all living things on
Earth to build proteins. This compound, amino
acetonitrile (NH2CH2CN), was observed using
a 30-metre radio telescope in Spain and two
radio interferometers, a type of spectrometer,
in France and Australia. The molecule is
present in vast quantities in a giant cloud of
gas near the centre of our Milky Way galaxy in
the constellation of Sagittarius, known as
‘Large Molecule Heimat’.
Finding such a molecule was an early hint of
more complicated finds to come from the
same team. In April this year, the scientists
published details of the discovery of ethyl
formate (C2H5OCHO) and n-propyl cyanide
(C3H7CN) in the Large Molecule Heimat. These
two compounds are more complex than amino
acetonitrile and scientists speculate that an
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InfoChem_July 09..indd 3
A dish with a view
amino acid might also be present among the
stars. Such a discovery, while expanding our
understanding of how chemical reactions can
take place in the rarefied clouds of gas and dust
in space, would also suggest that amino acids
might be more ubiquitous throughout the
cosmos than we had thought.
Indeed, if amino acids are present in space,
then some scientists have postulated that these
molecules may have been carried to Earth from
space through cometary or asteroid collisions
during our planet’s formative years.
Conceivably, interstellar amino acids might
have been the starting materials, the organic
seeds for life on Earth billions of years ago.
Scientists, however, have yet to find
spectroscopic, or any other kind of conclusive
evidence, for even the simplest amino acid,
glycine (NH2CH2COOH), in the interstellar
medium.
Spectral lines – elemental fingerprints

3
15/06/2009 16:52:34
“ 
   
…   ”
ISSUE  JULY 

S 
While finding complex molecules and,
ultimately, amino acids in interstellar space has
been the focus of many researchers for years,
other scientists are looking at starlight to try and
unravel the chemistry of the stars.
In 1985, chemist Harold Kroto had been
attempting to understand the observed spectra
of light from giant red stars and postulated that
some of the characteristics of the spectra of
these stars and the so-called diffuse interstellar
bands (DIBs) might result from the presence of
either very long chain-like carbon molecules or
polycyclic aromatic hydrocarbons containing
lots of carbon rings. Ultimately, Kroto’s team
working with colleagues in the US, suggested
that an all-carbon molecule composed of 60
carbon atoms and shaped like a football made
up of pentagons and hexagons might be the
culprit. They went on to discover the molecule
on Earth – buckminsterfullerene – but its
existence in space remains elusive.
Comets have a tale to tell…
The most recent theory on the interstellar bands
suggests that these might be down to element
helium rather than any complex carbon
molecule.
David Bradley
that’s chemistry
Simon Cotton, chemistry teacher at Uppingham School, looks at the molecules in our lives. In this issue: liquorice
Where does liquorice
come from?
occurs around the Mediterranean.
The plant was brought to the
British Isles in the Middle Ages,
and cultivated in areas such as
Pontefract in Yorkshire, where in
the mid-1700s local chemist
George Dunhill added sugar and
starch to liquorice extract to
JUPITERIMAGES X2;
It comes from the root of the
liquorice plant, Glycyrrhiza glabra,
which derives its name from the
Greek words glycys (sweet) and
rhiza (root). These roots grow one
metre down into the ground and
spread out up to six
metres. The sweet, black
liquorice extract is made
by harvesting the mature
roots, which are then
dried before being pulped
HOOC
and boiled in water. The
HO
HO
extract is concentrated by
HOOC
evaporation and on
O
HO
HO
cooling sets. This solid is
OH
beaten and rolled to form
the familiar black stick
liquorice.
How long has it been
eaten as a sweet?
The liquorice plant naturally
4
InfoChem_July 09..indd 4
HO
make the first liquorice sweets –
Pontefract cakes.
What makes liquorice
taste sweet?
Liquorice extract contains
glycyrrhizic acid (1). Comprising
two sugar molecules linked to a
steroid-like triterpenoid,
H3C COOH
this substance is 50
times sweeter than
CH3
sucrose. The chemical
acid. This chemical inhibits
O
CH3 H3C
H
also has medicinal
enzymes that metabolise lipid
properties.
compounds (prostaglandins)
H
CH3
released in the digestive system.
O
O
H
So
does
it
have
The build up of prostaglandins in
H3C CH3
O
turn inhibits gastric acid
medicinal uses?
Liquorice has been
secretion, which may be related
Triterpenoid
widely used in Chinese to its anti-ulcer action.
(1) Glycyrrhizic acid
medicine for hundreds
Another molecule found in
OH O
OH
of years as an
liquorice, the flavonoid
expectorant and to treat stomach β-hydroxy-DHP (2), targets and
complaints, such as ulcers. On
stops the growth of malignant
OH hydrolysis, glycyrrhizic acid yields cells in prostate and breast
(2) β-Hydroxy-DHP
the triterpenoid glycyrrhetinic
cancers. ■
You may copy this page for use within schools
15/06/2009 16:52:51
Jonathan Hare asks…
HANG TIME: could you use a hose
pipe to break a fall of 10 metres?
In the 1988 film Die hard we see Bruce Willis
escape his assailants by jumping off the top of a
tower with only a fire hose wrapped around his
waist to break his fall. To help us discover what
might happen to him we need to consider the
material properties of the hose pipe, but first we
need to do some calculations using a few basic
physics equations, to work out the forces on
Willis.
liberated when a very large firework goes off.
As Willis is brought to a standstill all this energy
has to be dissipated in the hose or in him. If this
happens only at the very end of his fall he will
experience a much greater force than if he is
brought to a stop over a longer braking distance.
To calculate the forces on Willis we rearrange
the equation:
Calculating the force
to get:
Looking at the clip it looks like Willis free falls
about two or three floors, ca 10 m, before the
hose brings him to a stop. From the equation:
s = ½gt2 (i)
E = F × d (iii)
F=E/d
where d is the braking distance.
Of hose pipes and stretching
Let us start by being kind to Willis. Let us say that
instead of a fire hose, he used a 5 m bungee rope,
and that this stretches another 5 m to bring him
to a gentle stop 10 m below. Bungee ropes are
made of many latex strands bundled together.
Because of the elasticity of the strands they can
t = √(2 × s/g)
absorb a great deal of the energy of a fall, making
= √(2 × 10/10) = √2
bungee jumps relatively safe. Using equation (iv)
we get a force on Willis of 7900 J/5 m = 1580 N
~ so t is about 1.5 s.
Using this value for t, we can work out how fast (Newton), equivalent to a weight of 158 kg, ie
about twice his weight – similar to the force on
(v) he will be falling just before the hose stops
your feet when you give someone a piggy back
him from the equation:
ride, which is acceptable.
v = g × t (ii)
In contrast, fire hose is made of woven nylon, a
–1
Thus v = 10 × 1.5 = 15 m s . Now if Willis’ body
masterpiece of chemical engineering. Hose pipe
mass (m) is about 70 kg we can work out his
can withstand pressures of up to 80 atmospheres
energy from:
(ca 8.1×106 Pa), pressures which, if the hose splits,
E = ½mv2
can brake brick walls. I tried putting a bin full of
water onto a 1 m piece of fire hose hanging from
= ½ × 70 × (15)2
a tree. It barely stretched 1 mm before the branch
= 7900 J
broke under the weight. So in the Die hard fall it’s
unlikely to stretch very much.
This is about the same amount of energy
where s is the distance he falls and g is the
acceleration due to gravity (ie ca 10 m s–2), we can
estimate how long (t) it will take him to fall this
distance by first rearranging the equation (i) so
that:
20TH CENTURY FOX/THE KOBAL COLLECTION
(iv)
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InfoChem_July 09..indd 5
Action hero should have done
the maths first…
Let’s say in Willis’ jump a 10 m fire hose
stretches 1 per cent ie 0.1 m. Equation (iv) now
gives F = 7900 J/0.1 m = 79000 N ... about 100
times his weight.
So what would happen to our action hero?
Talking through this one day with the actor and
presenter Robert Llewellyn he quite rightly
reflected, ‘I think there would be a Bruce and
somewhere else, a Willis’.
Dr Jonathan Hare, The CSC Centre, chemistry
department, University of Sussex, Brighton BN1
9ET (www.creative-science.org.uk/TV.html).
If you have come across a film or TV clip, or one from YouTube in
which chemistry is used to explain something, why not send it to
Jonathan Hare and find out if the science is correct (e-mail:
[email protected]). If we publish your question you will
receive a £20 HMV token.
5
15/06/2009 16:56:10
Dr Hal SoSabowSki preSentS experimentS you can Do on your own
Issue
MARCH
IN THIS ISSUE: layered liquids
In these experiments we are going to
exploit the different densities of some
liquids to make colourful effects.
Experiment 1
Oil and water do not mix. This is because
oil is non-polar and water is polar. Polar
compounds tend to dissolve in water but
not oil and vice versa. Hence the
expression ‘like dissolves like’.
MATERIALS & METHOD
You will need:
●
●
●
●
60 ml water;
60 ml vegetable oil;
food colouring;
a small glass; and cling film.
Pour the water into the glass. Add some
food colouring and mix. Now add the oil,
and note which layer is on top. Cover the
glass with cling film. While holding the
glass over a sink, shake it to mix the
liquids. Put the glass down and observe.
The density of a substance is the ratio of
its mass (weight) to its volume. The oil is
less dense than the water, so sits on top.
Experiment 2
This experiment examines the miscibility
and density of several liquids.
MATERIALS & METHOD
You will need:
●
●
●
●
●
60 ml dark corn syrup or honey;
60 ml dishwashing liquid; 60 ml water;
60 ml vegetable oil; 60 ml rubbing alcohol ;
tall glass and two glasses for mixing;
food colouring.
Pour enough syrup/honey to fill the glass
to about 1/6th of its height, taking care
not to get syrup on the side of the glass.
6
InfoChem_July 09..indd 6
Now tip the glass slightly and pour an
equal amount of the dishwashing liquid
slowly down the side of the glass. Does
the dishwashing liquid float on top of the
syrup or sink to the bottom?
Mix a few drops of food colouring with
water in one of the mixing cups. Colour
the rubbing alcohol a different colour in
another glass. Be careful to add the next
liquids very slowly. They are less viscous
and mix more easily than the previous
liquids. Tip the glass slightly, and add
slowly down the side of the glass the
coloured water, then the vegetable oil,
and finally the coloured rubbing alcohol.
The more dense liquids will rest at the
bottom, the less dense will sit at the top.
Stir up the liquids in the glass and watch
what happens to the layers.
Experiment 3
This is the ‘rainbow experiment’.
MATERIALS & METHOD
You will need:
●
●
●
●
240 ml water;
four different food colourings;
five tall glasses and a
tablespoon;
180 g of granulated sugar.
colouring to the first glass, yellow to the
second, green to the third, and blue to the
last glass.
Fill the remaining glass about a quarter
of the way with the blue sugar solution,
and carefully add the green solution. Do
this by putting a spoon in the glass, just
above the level of the blue solution.
Slowly pour the green solution onto the
spoon, raising the spoon to keep it just
above the level of the liquid, until the
glass is half full. Add the yellow solution,
and then the red one in the same manner.
The solutions should form layers since the
different proportion of sugars gives them
different densities.
HEALTH AND SAFETY
Food colouring and oil can stain clothing.
Alcohol is flammable so there must be no
naked flames in the vicinity when you are
doing the second experiment. ■
Acknowledgement: adapted by kind permission
of Professor Bassam Z. Shakhashiri, University of
Wisconsin–Madison.
In the first glass, add one
tablespoon of sugar, in the
second add two tablespoons
of sugar, three in the third
glass, and four in the last
glass. Then add three
tablespoons of water to each
glass and stir until the sugar is
dissolved. When the sugar is
completely dissolved, add two
or three drops of red food
You may copy this page for use within schools
15/06/2009 16:56:33
A     …
ADVANCED SCIENTIST:
Dan Clarke
Dan has spent the past 18 months working as an
advanced scientist for 3M Healthcare. He talks to
Rachel Bolton-King about his typical day.
3M is a global technology organisation with over 75,000 employees
working in various industries. Dan works in the healthcare division
and is part of a team of 15 staff in the inhalation drug delivery (IDD)
hardgoods R&D department based in Loughborough.
P 
Dan uses laboratory procedures developed in-house to test
prototype pressurised metered-dose inhalers (pMDIs) designed by
the IDD hardgoods design team for pharmaceutical customers. He
is currently working on two pMDI projects, both of which have been
running for five years. Most development projects take up to 10
years to complete before the product goes on sale.
Pressurised metered-dose inhalers comprise a pressurised aerosol
can containing the medication, a valve system to release a
controlled amount of drug, a dose counter to record the number of
doses remaining in the aerosol, and an outer plastic inhaler casing
called an actuator. Dan performs force tests, shot weight tests and
drop tests on all prototype pMDIs. In a force test, he uses a tensile
machine to apply a known increasing force to the aerosol can. This
test measures the force at which the pMDI fires a dose and is
PATHWAY TO SUCCESS
●
●
2008–present, advanced scientist, 3M
Healthcare, Loughborough
2006–08, scientist, 3M Healthcare,
Loughborough
2003–06, BSc chemistry (2.ii),
Loughborough University
2001–03, chemistry, physics and
psychology A-levels, St Michael’s Catholic
High School, Garston
●
●
You may copy this page for use within schools
InfoChem_July 09..indd 7
Dan Clarke
illustrated by a peak in
the force profile. Dan
fires the prototype 120 times, simulating the life of the aerosol, and
for each fire the force peak must be similar and of the correct
magnitude to show that the valve system is functioning properly.
To test shot weight Dan weighs the device before and after firing
and checks that a consistent dose is released during each fire. If a
more accurate analysis of the amount of active drug delivered is
required, he sends the pMDI to the analytical chemistry department
where the drug sample released in each fire is collected and
analysed using high-performance liquid chromatography (HPLC).
The drop test checks that the pMDI is robust and conforms to
international safety standards. Dan drops the device from one metre
to the ground three times to check it does not break. He then fires
the device to make sure a patient would still be able to receive a
dose. To see if any particles have broken off from the device, Dan
fires the device onto a filter, which he analyses using a microscope.
Dan records all his data in an Excel spreadsheet, which he uses to
generate graphs of the results to illustrate the product’s
performance and lifespan. These data are copied onto a shared
electronic database, which can be accessed,viewed and used by all
staff involved in the project. Every two weeks Dan attends a project
meeting to present, discuss and review all the work that he and
colleagues have done, and to propose any changes to the prototype
and plan the next trial stage or repeat previous testing.
Dan may also modify test procedures to accommodate any
modifications made to standard components in the pMDI. When
Dan develops a new procedure, he writes the method into the IT
system at 3M and his supervisor and head of department check the
procedure before it is published for use in project testing. As lab
supervisor Dan is responsible for ensuring equipment is calibrated.
Analytical balances are calibrated monthly by an external contractor
while other equipment is calibrated annually by the manufacturers.
M  
Dan enjoys his job because it is varied, unpredictable and, in
particular, satisfying because he is striving to develop products that
will improve people’s health and quality of life. ■
PhD student, Rachel Bolton-King was given a grant by Chemistry: the next
generation (C:TNG) to write this article in collaboration with Education in Chemistry.
7
15/06/2009 16:56:54
£50 OF HMV TOKENS TO BE WON!
FIND THE ELEMENT No. 9
Students are invited to solve Benchtalk’s Find the element puzzle,
contributed by Dr Simon Cotton of Uppingham School. Your task is
to complete the grid by identifying the nine elements using the
clues below.
ISSUE  JULY 
ACROSS
PRIZE WORDSEARCH No. 46
1. This metal forms an insoluble chloride.
Students are invited to find the 30 words/expressions associated with
sunscreen analysis hidden in this grid. Words read in any direction, but
are always in a straight line. Some letters may be used more than once.
When all the words are found, the unused letters, read in order, will spell
a further 12-letter word. Please send your answers to the Editor at the
usual address to arrive no later than Wednesday 5 August. First correct
answer out of the editor’s hat will receive a £20 HMV token.
2. This metal forms a carbonate that is a common mineral. On
heating the carbonate hard, it forms an oxide that is slightly
soluble in water, forming an alkaline solution.
3. Element that is a raw material in the contact process.
4. Inert gas sometimes used to provide the inert atmosphere
inside light bulbs.
5. This element forms a neutral oxide.
B
G
A
S
C
H
R
O
M
A
T
O
G
R
A
M
Y
6. This element turns blue litmus red, then bleaches it.
I
W
A
L
T
R
E
B
M
A
L
R
E
E
B
T
Y
7. This metal forms a white oxide, formula M2O3.
O
F
O
R
M
U
L
A
T
I
O
N
S
E
I
Q
R
8. Alkali metal with one electron in the third shell of the atom.
L
M
S
P
M
E
X
E
P
N
B
V
U
S
C
U
A
O
A
R
A
O
X
S
T
P
R
E
R
N
T
I
A
N
G
S
E
T
L
P
P
H
R
U
I
E
S
U
S
R
O
I
S
C
H
A
O
E
A
O
B
T
M
C
D
I
T
I
C
S
N
L
R
S
C
N
F
N
H
C
R
E
S
Z
T
A
P
A
E
I
U
T
O
I
U
G
V
E
N
O
C
A
L
E
C
N
T
R
R
L
L
S
I
U
E
T
M
U
T
E
C
N
G
Y
E
A
E
E
N
L
T
N
S
E
V
S
F
T
I
T
P
R
A
C
T
I
C
A
L
A
R
E
O
F
R
K
H
T
R
A
N
S
I
S
O
M
E
R
T
T
E
U
S
C
L
A
G
E
I
N
G
K
A
E
P
T
O
C
M
E
M
E
C
H
A
N
I
S
M
U
V
A
E
H
T
P
H
O
T
O
S
T
A
B
I
L
I
T
Y
S
P
S
P
E
C
T
R
O
P
H
O
T
O
M
E
T
E
R
AGEING
BEER LAMBERT LAW
BIOLOGICAL EFFECTS
CIS ISOMER
ETHANOL
EXPOSURE
FORMULATIONS
GAS CHROMATOGRAM
LIGHT
MASS SPECTRUM
MECHANISM
MOLARITY
PATHLENGTH
PEAK
PHOTOSTABILITY
PHOTOSTATIONARY
PRACTICAL
PROFILE
QUARTZ CUVETTES
SKIN CANCERS
SPECTRA
SPECTRAL INTENSITY
SPECTROPHOTOMETER
SUNBURN
SUNSCREEN
STUDENTS
TRANS ISOMER
UVA
UVB
UVC
1
2
8
InfoChem_July 09..indd 8
2
3
4
5
6
7
8
If you have found the correct eight elements, in 9 down you will have
generated the name of a metal found in the catalyst used in the contact
process for making sulfuric acid.
Please send you answers to: the Editor, Education in Chemistry, the
Royal Society of Chemistry, Burlington House, Piccadilly, London W1J
0BA, to arrive no later than Wednesday 5 August. First out of the editor’s
hat to have correctly completed the grid will receive a £30 HMV token.
1
2
May PRIZE WORDSEARCH No. 45 winner
The winner was Charlotte Taylor of Cowes High School, Isle of Wight.
The 11-letter word was THERAPEUTIC.
`
9
9
p o
p o
3
i
4
c a r b
5
z i
6
n i
7
f l u o r
8
a l
t a s s i u
s
t
r
o
n
t
i
u
m
i
a
o
n
c
r
n
m
l v e r
s s i u m
n
o g e n
e
i n i u m
Find the
element
no. 8
solutions
and winner
The winner was
Charlotte Wilkinson
from Wilberforce
College, Hull.
Download a pdf of this issue at: www.rsc.org/EiC
15/06/2009 16:57:15