Making a Silver-Halide Photogram — When Chemistry Becomes a Photograph
There is something almost magical about watching a photograph appear in a tray of developer.
A blank sheet of photographic paper goes into the liquid. For a few seconds, apparently nothing happens. Then faint grey shapes begin to emerge. Shadows deepen. Edges become clearer. Within a minute or two, an image that simply was not visible before is sitting in front of you.
Of course, it is not magic.
It is chemistry.
And for students who have grown up in a world where taking a photograph means tapping a screen and seeing the result instantly, traditional black-and-white photography provides a wonderful opportunity to connect chemistry, physics, history and technology in one very memorable practical investigation.
I would begin with something extremely simple: a silver-halide photogram.
Then I would take the experiment much further.
I can get an old 35 mm camera out of the cupboard, load it with black-and-white film, let students take photographs and then actually process the film. Instead of an image appearing instantly on a screen, they can watch the entire photographic process unfold in front of them.
The final moment — unrolling the processed film and seeing those tiny negatives for the first time — is particularly satisfying.
For much of the twentieth century, this was how an enormous proportion of family photographs, school photographs, newspaper photographs and scientific images were made.
The smartphone camera may be astonishingly sophisticated, but there is a great deal of science hidden by that convenience.
Traditional photography allows us to uncover it again.
What Is a Photogram?
A photogram is one of the simplest photographs it is possible to make because you do not actually need a camera.
Instead, objects are placed directly onto light-sensitive photographic paper.
The paper is briefly exposed to light and then processed using photographic chemicals.
Where light reaches the paper strongly, the finished image becomes dark.
Where an opaque object blocks the light, the paper remains comparatively light.
Translucent objects produce shades of grey.
The result can be surprisingly beautiful.
Leaves, feathers, mesh, keys, electronic components, pieces of lace, laboratory glassware and even water droplets can create fascinating images.
But behind those shapes lies some excellent chemistry.
The Chemistry Begins with a Precipitate
Traditional photographic materials contain microscopic crystals of silver halides suspended in a gelatin emulsion.
Common examples include silver bromide and silver chloride.
Silver bromide can be formed by precipitation when silver ions meet bromide ions:
Ag+ + Br- -> AgBr(s)
Silver bromide forms a pale cream precipitate.
This gives us a useful introductory experiment before we even touch the photographic paper.
Under appropriate laboratory conditions, students can observe a small-scale precipitation reaction involving silver ions and halide ions and then investigate what happens when the precipitate is exposed to light.
That gives us our first clue about why silver compounds became so important in photography.
They are light sensitive.
Why Does Silver Bromide Respond to Light?
Silver bromide crystals consist of silver ions and bromide ions arranged within a crystal lattice.
When light of sufficient energy is absorbed by the crystal, electrons can become available and ultimately allow tiny quantities of silver ions to be converted into metallic silver.
In simplified terms:
Ag+ + e- -> Ag
Only a tiny amount of metallic silver is initially produced.
There is not enough for us to see a photograph.
Instead, the exposure creates what photographers call a latent image.
The photograph is already encoded into the photographic material, but it remains invisible.
This is one of the ideas I particularly like discussing with students.
An image can exist even though you cannot yet see it.
That is a wonderfully strange concept.
The Developer Reveals the Hidden Image
The job of the photographic developer is to turn that invisible latent image into something we can see.
A developer contains reducing agents.
The tiny regions created by exposure to light encourage further reduction of silver ions within the exposed silver-halide crystals.
More metallic silver is produced.
And metallic silver is dark.
The more exposure a region receives, the greater the eventual density of metallic silver produced during development.
So the image begins to appear.
ILFORD describes conventional black-and-white film in essentially these terms: light creates a latent image within silver-halide crystals, and development amplifies that extremely small initial change into visible grains of metallic silver. Ilford Photo
This is a lovely example of chemistry being used as an amplification process.
A very small photochemical change eventually produces a macroscopic image that our eyes can see.
Watching the Photograph Appear
This is the moment students tend to remember.
The exposed paper goes into the developer.
Initially it looks blank.
Then something happens.
Perhaps the outline of a key appears.
Then the veins of a leaf.
Then areas that were completely exposed become increasingly dark.
It is particularly effective if students have previously only experienced digital photography.
A digital photograph appears instantly because enormously complicated electronics are doing the processing invisibly.
With silver-halide photography, much of the process happens physically in front of you.
You can watch chemistry creating the image.
But Development Cannot Simply Continue
If we left the photographic paper in active developer indefinitely, the image would continue changing.
Traditional processing therefore separates the stages carefully.
A typical black-and-white sequence is:
- development;
- stop bath or rinse;
- fixing;
- washing;
- drying.
ILFORD's own technical guidance describes film processing as development, stop bath, fixing, washing, wetting-agent rinse and drying, with temperature, timing and agitation important for consistent results. Ilford Photo
This gives students another useful lesson.
Good experimental science is not simply about putting chemicals together.
It is about controlling variables.
Time matters.
Temperature matters.
Concentration matters.
Agitation matters.
And reproducibility matters.
The Fixer Performs a Completely Different Job
Development produces metallic silver in those crystals associated with the latent image.
But a problem remains.
Large amounts of unexposed silver halide are still present.
If we simply took the photograph into daylight at this stage, those remaining light-sensitive crystals would react and the photograph would gradually darken.
We therefore need to remove them.
That is the job of the fixer.
Traditional fixing agents contain thiosulphate ions, usually using sodium thiosulphate or ammonium thiosulphate.
A simplified representation is:
AgBr + 2S2O3^2- -> [Ag(S2O3)2]^3- + Br-
The important point is that the insoluble silver halide is converted into a soluble silver-thiosulphate complex which can be removed from the photographic material.
The metallic silver forming the image remains.
ILFORD similarly describes fixation as the removal of residual silver halide while leaving metallic silver behind to form the permanent image. Ilford Photo
Now the photograph can safely be exposed to ordinary light.
The image has been fixed.
That familiar photographic word therefore has a very literal chemical meaning.
A First Practical: Make a Photogram
For a first session I would keep things deliberately simple.
Students can choose several objects with different optical properties.
For example:
- a metal key;
- a leaf;
- a feather;
- a piece of netting;
- a glass slide;
- a translucent plastic object;
- a spring;
- wire;
- a small electronic circuit board;
- pieces of laboratory apparatus.
Under suitable darkroom or safelight conditions, arrange them directly on black-and-white photographic paper.
Expose the arrangement to light for a controlled period.
Then develop, stop, fix and wash the paper according to the photographic paper and chemical manufacturers' instructions.
Suddenly we have something worth investigating rather than merely demonstrating.
Turn the Photogram into a Proper Experiment
There are many variables that students could investigate.
For example, keep everything else constant and change the exposure time.
Try a series such as:
1 second
2 seconds
4 seconds
8 seconds
16 seconds
The exact useful times will depend on the light source, distance and photographic material, so an initial test strip is much better science than simply guessing the "correct" exposure.
Students can compare the resulting density.
Does doubling exposure time double the apparent darkness?
Probably not in any simple visual sense.
And that opens another discussion about photographic response, density and logarithmic scales.
Investigating Distance
Move the light source farther from the photographic paper.
What happens?
Now photography connects with physics.
For an approximately point-like source, illumination is related to distance through the inverse-square relationship:
intensity proportional to 1 / distance^2
Double the distance and, under idealised conditions, the intensity falls to approximately one quarter.
The experiment suddenly connects photochemistry with GCSE and A-level physics.
Opaque, Transparent and Translucent
A photogram can also become a simple investigation of light transmission.
An opaque metal washer may block almost all the light.
Clear glass might transmit most of it.
Frosted plastic scatters the light.
Coloured transparent materials may behave differently depending upon the spectral sensitivity of the photographic paper.
Rather than treating the photograph simply as artwork, students can ask:
What can we infer about an object's interaction with light from the image it produces?
That is a much more scientific question.
Then Bring Out the 35 mm Camera
The photogram establishes the basic principle.
Now comes the part I particularly enjoy.
I can take an old 35 mm camera out of the cupboard.
For many students, even loading the film may be unfamiliar.
Open the back.
Place in the film cassette.
Pull the film leader across.
Engage it with the take-up mechanism.
Close the camera.
Advance the film.
Suddenly photography becomes mechanical as well as chemical.
There is no LCD screen.
There is no instant review.
There is no delete button.
You have perhaps 24 or 36 exposures.
You actually have to think before pressing the shutter.
A Camera Is Really Just Controlling Light
Once the mystery is removed, the basic photographic camera is beautifully simple.
The lens forms an image.
The aperture controls how much light can enter.
The shutter controls how long that light reaches the film.
The film records the image.
That allows us to introduce another basic photographic relationship:
exposure approximately depends on light intensity x exposure time
Photography becomes a practical demonstration of optics.
Students can investigate:
- aperture;
- shutter speed;
- focus;
- depth of field;
- motion blur;
- focal length;
- exposure.
Things that are largely automated by a smartphone become visible decisions again.
The Strange Experience of Not Knowing Whether the Photograph Worked
This is something younger photographers have almost completely lost.
Take a photograph digitally and you immediately inspect it.
Was it sharp?
Was the exposure correct?
Did somebody blink?
With film, you do not know.
You press the shutter and move on.
The image exists as a latent chemical change inside the film cassette, but there is nothing yet to inspect.
Only when the film has been developed do you discover what you actually captured.
That delay changes the way you take photographs.
It encourages thought before exposure rather than correction afterwards.
Processing the Film
After the photographs have been taken, the film must be processed.
This provides another wonderful moment.
The film has to be removed from its cassette and loaded onto a processing reel in complete darkness or inside a changing bag.
Once the light-tight processing tank is closed, the rest of the process can normally be carried out in ordinary room light.
Developer is added.
The film is agitated according to the chosen process.
Development is stopped.
The film is fixed.
Then it is washed.
Temperature control matters because photographic development is a chemical reaction and its rate varies with temperature. ILFORD specifically notes the dependence of development on temperature and pH. Ilford Photo
Again, what looks like photography has become experimental chemistry.
And Then Comes the Reveal
Eventually the tank opens.
The film is carefully removed from the spiral.
And there they are.
Tiny photographs.
Except that they look completely wrong.
The bright sky appears dark.
Dark clothing may appear pale.
Light and dark are reversed.
The students are looking at a negative.
For somebody who has only known digital photography, physically holding a strip of 35 mm negatives can be surprisingly fascinating.
The negative is not merely an old-fashioned curiosity.
It reveals how the entire photographic system works.
A bright part of the original scene exposes the film strongly and eventually produces a dense region containing more metallic silver.
A dark part of the scene gives less exposure and produces a more transparent region.
When we subsequently use the negative to make a print, that relationship is reversed again.
The final photograph looks normal.
From Negative to Positive Print
Now we can complete the journey.
Place the negative in an enlarger.
Project its image onto photographic paper.
Adjust focus and enlargement.
Expose the paper.
Then once again:
developer...
the image appears...
stop...
fix...
wash...
dry.
We have gone from:
real scene -> camera -> latent image -> negative -> projected image -> photographic paper -> positive print
That entire chain is enormously instructive.
A modern phone compresses all of this into perhaps a fraction of a second.
The old process allows students to see every stage.
A Contact Sheet Makes an Excellent Teaching Tool
Before making individual enlargements, I would also show students how a contact sheet works.
Place strips of negatives directly against photographic paper beneath glass.
Expose the whole sheet.
Process it.
You then have miniature positive versions of every frame.
This was once an important part of photographic workflow.
The photographer could inspect the contact sheet and decide which frames were worth enlarging.
It also teaches something interesting about selection.
A photographer might take 36 photographs but print only three.
That is another contrast with the modern habit of accumulating thousands of nearly identical digital images.
Why Black-and-White Photography Is Perfect for Teaching Chemistry
Colour photography is scientifically fascinating, but it introduces several additional layers of complexity.
Black-and-white silver photography exposes the essential chemistry far more clearly.
We can follow silver through the whole process.
Begin with:
Ag+
Form:
AgBr
Expose it to light.
Create a latent image.
Develop exposed crystals.
Produce:
Ag metal
Remove unwanted AgBr during fixation.
What remains is an image made largely from microscopic particles of metallic silver.
The photograph is therefore not simply a picture.
It is a chemical object.
There Is Also a Valuable Environmental Discussion
Once we start processing photographic materials, another question becomes important:
What happens to the chemistry afterwards?
Used photographic fixer can contain silver compounds and should not simply be treated as though it were harmless water. ILFORD technical information for photographic processing notes silver in waste fixer streams. Ilford Photo
That creates an opportunity to discuss:
- chemical waste;
- heavy-metal recovery;
- laboratory responsibility;
- recycling;
- safe storage;
- why disposal instructions matter.
This is exactly the sort of broader scientific thinking I want students to develop.
An experiment does not finish simply because we have obtained our result.
We are also responsible for the materials we have used.
Safety Matters
Traditional photography is perfectly capable of being an excellent teaching practical, but it should still be treated as laboratory chemistry.
I would use commercial photographic developer and fixer according to their current instructions and safety data, with appropriate eye protection, gloves where specified, good ventilation and separate labelled equipment.
Silver nitrate used for introductory precipitation experiments requires particular care because it can damage eyes, irritate tissue and produce persistent stains.
Photographic chemistry should never be placed in drinks bottles or unlabelled containers.
And silver-containing waste should be collected and disposed of appropriately rather than casually poured away.
Students should see good chemical practice as part of the experiment, not as an inconvenience added to it.
What Could Students Actually Investigate?
Once the basic technique is working, the possibilities expand enormously.
A photogram could become an investigation into exposure time.
Film could be used to explore shutter speed and motion.
Different apertures could demonstrate depth of field.
A test strip could investigate photographic-paper exposure.
Negatives could be compared for different camera settings.
Students could measure optical density.
They could investigate developer temperature.
They could compare fresh and ageing chemistry.
They could examine film grain under magnification.
They could even compare a film image with a modern digital sensor image of exactly the same scene.
Suddenly one old camera has become a gateway into:
chemistry, optics, electronics, materials science, imaging, measurement, art and technological history.
From Silver Grains to Silicon Pixels
The final stage of the lesson should probably bring us back to the device almost every student has in their pocket.
A smartphone camera does not normally use silver halide.
Its sensor contains millions of photosensitive semiconductor elements.
Photons still have to be detected.
Light still carries the information.
Lenses still have to form an image.
Exposure still matters.
But the method of recording that information has changed dramatically.
In the traditional camera:
light -> chemical change
In a modern digital camera:
light -> electrical signal -> numerical data
That is an extraordinary technological transition.
And it happened within living memory.
"Was Every Photograph Really Made Like This?"
I sometimes tell students that this is how photographs used to be made.
It is worth adding a little historical precision.
Photography has used many processes during its history: daguerreotypes, wet-plate collodion, glass negatives, silver-gelatin materials, colour films and numerous specialist processes.
For example, the daguerreotype used a silver-coated copper plate sensitised with silver halides rather than modern roll film. National Science and Media Museum blog
But for a large part of the twentieth century, silver-halide film and photographic paper were the dominant technology behind ordinary photography.
The family snapshot.
The school photograph.
The holiday photograph.
The wedding album.
News photography.
Scientific photography.
The rolls of film sent away in envelopes and returned days later as prints.
For students who have never known anything except instant digital images, that world can seem surprisingly remote.
Yet it is not ancient history at all.
One Photograph, Several Sciences
This is exactly the sort of experiment I enjoy because it refuses to stay neatly inside one subject.
The precipitation reaction is chemistry.
The photosensitivity is photochemistry.
Development involves reduction.
Fixing involves complex ions and solubility.
The lens introduces optics.
Exposure brings in intensity and time.
The camera introduces engineering.
Film grain leads into materials science.
The history of photography introduces technological change.
And the final print becomes art.
That is much closer to real science than treating every topic as though it belongs in its own isolated chapter of a textbook.
The Photograph Appearing in the Tray Is Still Special
There are faster ways to make a photograph.
There are easier ways.
There are certainly cheaper ways if you already own a smartphone.
But very few are as educational.
I can explain silver ions, precipitation, reduction, lenses, shutter speeds and negatives on a whiteboard.
Students may understand them perfectly well.
But putting a supposedly blank sheet of photographic paper into developer and watching an image slowly emerge is different.
Then taking an old 35 mm camera, processing the film and holding the still-wet strip of negatives up to the light completes the story.
For a few moments, students experience photography not as an app, but as a scientific process.
And perhaps the most important question is no longer:
"What photograph did we take?"
It becomes:
"How did light and chemistry manage to make an image at all?"
That is a much more interesting question.
