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In this installment on the history of atom theory, physics professor (and my dad) Dean Zollman discusses how Ernest Rutherford and his teams experimented to see whether atoms were more like plum pudding or a planet with moons.—Kim

By Dean Zollman

Dean ZollmanThe scientific models of the atom that we considered last month are quite different from one another. Of course, all of them are attempts to describe objects that we cannot see. So, early 20th century scientists needed to find some indirect method to probe the atom. Some indirect evidence about the atom such as the light emitted from them was available. But all of models explained these observations about equally well or equally badly. A creative new approach was needed.

Hans Geiger

Hans Geiger (public domain via Wikimedia)

We have already met the person who would provide that creativity—Ernest Rutherford, who had named alpha and beta radiation. You might remember that Rutherford grew up in New Zealand and came to England to be the graduate student of J.J. Thomson. He did his early work on emissions from the nucleus at McGill University in Canada. He returned to England to become a professor at the University of Manchester. Rutherford’s predecessor Arthur Schuster (1851-1934) had hired an outstanding experimenter, Hans Geiger (1882-1945). Geiger became Rutherford’s assistant and built a very fruitful collaboration.

Rutherford worked in a different mode than most scientists of his or earlier times. Instead of working in relative isolation with at most a few assistants, he assembled teams of scientists, many with doctorates. These teams would conduct research under Rutherford’s direction. This mode of doing science anticipated the modern team approaches by 50-60 years.

Ernest Rutherford in his laboratory

Ernest Rutherford in his laboratory, about 1905 (used under Creative Commons Attribution 4.0 International via Wikimedia Commons).

At McGill, Rutherford had focused much of his energy on investigating the changes in elements that emitted radioactive particles. In Manchester, he switched to investigations about the objects that were being emitted, particularly alpha particles.

One of the first issues that he tackled was the nature of alpha particles. From previous work, Rutherford suspected that alpha emissions were similar to helium atoms. However, he was a very thorough scientist and wanted to confirm his suspicions before publishing the results. Working with Thomas Royds (1884-1955) in 1908, he collected alpha particles in a sealed container. They then passed an electric spark through the container.

The light that was emitted was the same as the spectrum of helium. This experiment was sufficient proof for Rutherford to state publicly that alpha particles were helium atoms. From previous work, he knew that the alpha particles had positive electrical charge. So, alpha particles were helium atoms with a positive charge. (He did not know then that the alpha particles were just the nucleus of helium. He had not yet discovered the nucleus.)

Dark Rooms and Gas-Filled Tubes

Rutherford and Geiger began working on ways to detect the alpha particles. William Crookes (1832-1919) had noticed that when alpha particles struck zinc sulfide a very small flash of light was emitted. This phenomenon was verified by Julius Elster (1854-1920) and Hans Geitel (1865-1923). The process is somewhat similar to the way old-style TVs create pictures.

In the TV, electrons hit the screen and cause light to be emitted. However, the light that was emitted from the impact of a single alpha particle with the zinc sulfide was extremely dim. Rutherford and Geiger devised a scheme so that the light could be seen and the number of alpha particles striking the screen could be counted.

Before starting the counting process, the experimenter would sit in a completely dark room for about 20 minutes. Once the eyes had adjusted to the darkness, the experimenter would look through a microscope at a small area of the zinc sulfide screen and wait to see a blip of light. With this extremely tedious procedure, the experimenter could count for only a short time before fatigue set in.

A second method involved a gas filled tube with a voltage on two wires. The voltage was sufficiently high that it would almost cause a spark. When an alpha particle passed through the gas, it would create a spark, which could be registered on a meter. This instrument would be later developed into the Geiger-Muller counter. In some of these counters, a speaker would click with each alpha particle. These clicking Geiger counters appear in many 1950s science fiction movies.

 Inside a Geiger-Mueller tube

The basic function inside a Geiger-Mueller tube: the cathode is negative; the anode, positive. When ionizing radiation such as an alpha particle enters the tube, a spark occurs and is counted (used under the Creative Commons Attribution-Share Alike 3.0 Unported licence via Wikimedia).

Like Scattering Table Tennis Balls

With all of this data about the alpha particle, Rutherford had enough information to use it to probe the atom. He knew the mass and the electric charge. He also knew how to measure where an alpha particle was.

Using it as a probe was simple in concept but somewhat complex in practice. He could not see an atom or an alpha particle. But he could direct the alpha particle toward some matter. Then he could detect where the alpha particle went after it passed through the matter. By looking at any change in the particle’s direction, he could use the physical principles related to change in motion and electrical interactions to surmise what had happened inside the matter. That is: what type of interaction the alpha particle had with the atoms of the material that it went through or near.

When I introduce this concept in a class, I hide an object behind a screen. Then, I shoot table tennis balls at it. The students are challenged to determine as much as they can by looking at how the balls bounce off the object. This process is called a scattering experiment because we are trying to learn something about an object by looking at how small particles bounce off (or scatter from) it. Doing it with alpha particles is now called Rutherford scattering.

For detecting the location of the alpha particles after the scattering, counting small blips of light was the more accurate method. He arranged a radioactive source of alpha particles behind a lead shield with a small hole in it. Alpha particles could pass through the hole but not the rest of the lead. So, a small beam of alpha particles was available to collide with something. Rutherford chose to direct the beam at a very thin foil of gold. He would then have a student look at a zinc sulfide screen through a microscope.

The student who got to perform this experiment was Ernest Marsden (1889-1970). By varying the angle at which Marsden observed the screen he could see how the gold atom caused the alpha particles to change their direction. This drawing indicates how the actual apparatus may have looked.

Experimental apparatus used by Marsden and Geiger

The experimental apparatus used by Marsden and Geiger. The zinc sulfide screen is on the inside end of the microscope. The microscope could be moved to look at different angles relative to the incoming beam of alpha particles (by Kurzon, licensed under the Creative Commons Attribution-Share Alike 3.0 Unported via Wikimedia).

The diagram below shows the basic idea in a schematic form. The alpha particles come in toward the gold foil. After they pass through the foil, they may be moving in a different direction than when they entered. By moving the microscope around the foil, Marsden could count how many came off at each angle.

Experimental arrangement for probing the atom

The experimental arrangement for probing the atom (by Kurzon, licensed under the Creative Commons Attribution-Share Alike 3.0 Unported via Wikimedia).

Differing Recollections about Motivation But…

At this time the prevailing model of the atom was the “plum pudding” model that we discussed last time. Because the electrons and positive charges were somewhat uniformly distributed in the model, Rutherford’s expectation was that the alpha particles would travel through the gold with some small changes in their motion. For a while, Marsden looked for the small deviations from the incoming path. Most of the alpha particles were deflected through small angles; a large fraction were not deflected at all.

At some point, a decision was made to have Marsden look for big changes in the motion. Much later, Rutherford recalled that he needed something for Marsden to do so he said to Geiger, “Why not let him see if any alpha particles can be scattered through a large angle?” This statement sounds a little like “We need to find something to keep Marsden out of the pubs and in the lab.”

Ernest Marsden

Ernest Marsden, 1921 (by S P Andrew Ltd. public domain, via Wikimedia Commons)

Marsden remembered the story differently. He recalled, “Rutherford had been thinking over the matter, and he turned to me and said: ‘See if you can get some effect of alpha-particles directly reflected from a metal surface.”’ Independently of who said what, Marsden looked for very large changes in the alpha particles motion. He not only found something; he changed the way scientists think about matter!

To Rutherford this result was astounding. He said later, “It was quite the most incredible event that has ever happened to me in my life. It was almost as incredible as if you fired a 15-inch shell at a piece of tissue paper and it came back and hit you.”

Geiger and Marsden published a paper in June 1909 describing their results. However, at that time they could not explain their observations. Rutherford spent much time trying to understand how the atom must be constructed to give such a strange result. He worked toward a solid mathematical model which could explain the large scattering that they saw. Not until December of 1910 did Rutherford feel that he understood. His reasoning included:

  • The alpha particle has a relatively small mass; it is being occasionally deflected in the opposite direction that it was moving. Thus, these particles are interacting with something much bigger than they are. (Like a baseball bouncing off a wall.)
  • Because they are coming back, they are being repelled. The object that must have the same type of charge as the alpha particle. It must be positive. (Like charges repel.)
  • Most of the alpha particles are going through undeflected. So most of them interact with nothing. Thus, most of the gold foil is really empty space.

The diagram below shows Rutherford’s conclusion and compares it with the result that would have been expected with the Thomson plum pudding model of the atom. To view a simulation of these two models with Rutherford scattering go to PhET.

 

Diagram of atom models

The left side shows the result expected for the Thomson model; the right side is Rutherford’s conclusion about how the atom must look based on his experiment (By Kurzon, licensed under the Creative Commons Attribution-Share Alike 3.0 Unported license via Wikimedia).

Using a combination of Newton’s Laws of Motion and Coulomb’s Law for interactions among electrical charges, a Rutherford scattering equation can predict results for this type of experiment.

The net conclusion was that the atom had a very small, positively charged center (now called the nucleus). Most of the mass of the atom is located in this nucleus. Because overall the atom has no electrical charge, electrons must be outside the nucleus. Further, because most of the alpha particles passed through the gold unchanged, the distance between atoms must be large in comparison to the size of the nucleus. Matter seems to be mostly empty space.

So, this one experiment changed the way that scientists thought about matter. Instead of being a somewhat uniform “glob” of positive and negative charges, it was a concentrated massive positive charge surrounded by some very light electrons.

But there was a big problem. Why was this atom stable? Positives attract negatives. Further, acceleration charges radiate energy. Why does the electron not just spiral into the nucleus? We know that it does not because we exist. A possible explanation would be forthcoming. However, before we can try to understand that explanation, we need to go back to about 1900 and pick up another thread of reasoning about the nature of light. We will start that thread next time.

Dean Zollman is university distinguished professor of physics at Kansas State University where he has been a faculty member for more than 40 years. During his career he has received four major awards — the American Association of Physics Teachers’ Oersted Medal (2014), the National Science Foundation Director’s Award for Distinguished Teacher Scholars (2004), the Carnegie Foundation for the Advancement of Teaching Doctoral University Professor of the Year (1996), and AAPT’s Robert A. Millikan Medal (1995). His present research concentrates on the teaching and learning of physics and on science teacher preparation.

Previously

What Are Things Made of? Depends on When You Ask.

Ancient Greeks Were the First to Hypothesize Atoms

The Poetry of Atoms

Atom Theory in Ancient India

Religion, Science Clashed over Atoms

Medieval Arabic Scholarship Might Have Preserved Scientific Knowledge

Rediscovering a Roman Poet – and Atom Theory – Centuries Later

Reconciling Atom Theory with Religion

Did Atom Theory Play a Role in Galileo’s Trouble with the Inquisition?

Did Gifted Scientist’s Belief in Atoms Led to His Obscurity?

Does Atom Theory Apply to the Earthly and the Divine?

A Duchess Inspired by Atoms

Separating Atoms from Atheism

Isaac Newton: 300 Years Ahead of His Time

Issac Newton and the Philosopher’s Stone

When Chemistry and Physics Split

Redefining Elements

Mme Lavoisier: Partner in Science, Partner in Life

With Atoms, Proportionality and Simplicity Rule

Despite Evidence of Atoms, 19th Century Skeptics Didn’t Budge

Mission of the First International Scientific Conference: Clear up Confusion

Rivalry over the First Periodic Table

The Puzzle of Dark Lines amid Rainbow Colors

The Colorful Signature of Each Element

Light Waves by the Numbers

Even Scientific Dead Ends Can Contribute to Knowledge

Discovery of the Electron Took Decades and Multiple Scientists

‘Wonders of the X-ray’

The Accidental Discovery of Radioactivity

Marie Curie: A Determined Scientist

Pierre and Marie Curie Extract Radium – and Pay a High Price

Scientists Delve into Radioactivity and Make Their Own Discoveries

The First Attempts to Visualize Atoms

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