2.1 Atoms and Their Structure
ObjectiveRelate historic experiments to the development of the modern model of the atom.Illustrate the modern model of the atom.Interpret the information available in an element block of the periodic table.
Early Ideas About Matter Our current model of the composition of
matter is based on hundreds of years of work.
About 2500 years ago, the Greek philosophers thought about the nature of matter and its composition.
They proposed that matter was composed of four fundamental elements…
And these were… Air Water Fire Earth
Greek Philosophers They also debated whether matter
could be divided into smaller and smaller pieces endlessly or whether there was an ultimate smallest particle that could no longer be divided.
They were excellent observers, but they did not test their theories with experiments.
Democritus, 460-370 B.C. Proposed that the world is made up a
empty space and tiny particles called atoms.
He thought that atoms were the smallest particles of matter and that different types of atoms exist for every type of matter.
Atomic Theory- matter is made up of fundamental particles called atoms.
Antoine Lavoisier (1743-1794) French chemist In 1782 he made
measurements of a chemical change in a sealed container.
Lavoisier’s Conclusion He observed that the mass of the reactants
before the chemical reaction were equal to the mass of the products after the reaction. In a sealed container 2.0 g of hydrogen gas reacted
with 16.0 g of oxygen gas to produce 18.0 g of water
Matter was neither created nor destroyed during a chemical reaction, but changed.
This became known as the law of conservation of matter
Law of Conservation of Mass
Joseph Proust Joseph Proust, French chemist September 26, 1754 – July 5, 1826
Proust’s Contribution Observed that the composition of water is
always 11% hydrogen and 89% oxygen by mass. Regardless of its source
He observed many other compounds and observed that the elements that composed the compounds were always in a certain proportion by mass. This is referred to as law of definite proportions.
John Dalton
Dalton’s Atomic Theory John Dalton (1766-1844), an
English schoolteacher and chemist Studied the experiments of
Lavoisier, Proust, and many others. Based on this he developed his
atomic theory.
Dalton’s Atomic Theory
1. All matter is made up of atoms.2. Atoms are indestructible and
cannot be divided into smaller particles(Atoms are indivisible)
3. All atoms of one element are exactly alike, but they are different from atoms of other elements.
Dalton’s Atomic Theory This gave chemist a model of the
particle nature of matter, but it also raised a lot of questions.
If all elements are made up of atoms then why are there so many different types of elements?
What makes one atom different from another?
Dalton’s Atomic Theory Experiments performed late in the
19th century began to explain the properties and behavior of substances
This was done by the discovery of three smaller particles. Protons, electrons and neutrons
Atomic Theory, Conservation of Matter and Recycling What happens to the stuff you
throw away? What happens to the atoms?
As you have already learned matter is neither created nor destroyed, so what happens.
What happens? When waste is incinerated or
buried the atoms may combine with oxygen and other substances to form new compounds.
The atoms are “recycled”
Recycling Recycling has become a part of life
now. Much of what you buy is either
recycled or can be recycled. We have found the advantage of
recycling materials and therefore atoms. We mimic what nature does and conserve our natural resources.
Hypotheses Hypothesis – testable prediction to
explain observations. Hypotheses are based on
observations. They can be proven correct or
incorrect by the experiments that are designed to test them.
Hypothesis
Theories Theory- an explanation based on
many observations and supported by the results of many experiments.
As scientists gather new information, a theory may be revised or replaced.
Theory
Laws Scientific Law – a fact of nature that is
observed so often that it is accepted as the truth.
Examples: Sun rises in the east
A law can generally be used to make predictions but does not explain why something happens.
Theories explain laws. One part of Dalton’s atomic theory explains why
the law of conservation of matter is true.
Review What is the difference between a
theory and a hypothesis? What is the Law of Conservation of
Mass?
The Discovery of Atomic Structure Dalton’s atomic theory was almost true. He assumed that atoms are the ultimate
particles of matter and can’t be broken up into smaller particles and that all atoms of the same element are identical.
His theory needed to be modified with the discovery of electrons, protons and neutrons.
The Electrons In 1897, JJ Thomson a British
physicist discovered that the solid ball of model was not accurate.
His experiments involved the use of a cathode ray.
Cathode Ray Composed of a vacuum tube At the end of the tube is a piece of metal
called on electrode which is connected to a metal terminal on the outside of the tube.
The electrode becomes electrically charged when connected to a high voltage.
When the electrode is charged rays travel in the tube from the negative electrode(the cathode) to the positive electrode (the anode)
Cathode Ray
Cathode Ray
Thomson’s Discovery What he found that the ray would bend
towards a positive charged plate and away from a negatively charged plate.
He concluded that the rays are composed of invisible negatively charged particles he called electrons
Electron – negatively-charged particle
Early Atomic Model The early atomic model was
referred to as the “plum pudding model”; you could more closely relate it to a chocolate chip cookie
Scientists believed that atoms were balls of positive charge with the negatively charged particles embedded in them.
Changes in the Atomic Model
Solid BallModel
Plum PuddingModel
Ernest Rutherford In 1909 he carried
out the first of the experiments that would reveal an arrangement far different from the “plum pudding” model
Rutherford’s Experiment Gold Foil Experiment He set up a lead-shielded box containing
polonium, which emitted a positively charged beam of alpha particles.
When the beam struck a sheet of gold foil, most of the particles passed straight through the foil
However, some of the particles from the beam were deflected. Some were only slightly deflected and some bounced straight back.
Gold Foil Experiment
Gold Foil Experiment
The Nuclear Model of the Atom Based on Rutherford’s work the team
devised a new model for the atom. Because some of the particles
bounced straight back they concluded that atoms must have a dense central core called the nucleus
Nucleus – a small, dense, positively charged central core of an atom
Nuclear Model
Changes in the Atomic Model
Solid BallModel
Plum PuddingModel
Nuclear Model
Atomic Model It was hard for people to grasp that atoms
contained a lot of empty space. When they looked at a rock, it was very
difficult to see how most of this object could be empty space.
If you were to enlarge an atom of hydrogen so the nucleus was the size of a golf ball, the electron would be a mile a way.
In one drop of water there is 6,500,000,000,000,000,000,000 (6.5 sextillion) atoms
Atomic Numbers and Masses The nucleus of an atom is composed
of protons and neutrons. Electrons move in the space around the nucleus.
Atomic Number – the number of protons in the nucleus of an atom. Every element has a unique atomic
number. Therefore, it is the number of protons that determines the identity of an element.
Atoms Protons - positively charged subatomic
particles. Neutrons – subatomic particle that does
not have a charge, it is neutral Atoms have no overall charge. Therefore the number of protons and
electrons must be equal. If you elements atomic number is 2
2 protons 2 electrons
Mass Number Mass number - the number of protons
and neutrons in the nucleus of an atom.
Isotope – atom of an element with a different number of neutrons and therefore a different mass number Ne-20 = neon 20(10 protons, 10 neutrons) Ne-21 = neon 21(10 protons, 11 neutrons)
Neon
Composition of Atoms You can
determine the composition of any element if you know the Atomic number Mass number
Atomic Mass Since elements have different isotopes
the atomic mass is the weighted average.
Located under the symbol on the periodic table.
You can use the atomic mass to determine the mass number of a element You take the atomic mass rounded up
Determining Atomic Mass
62.930 X 0.6917 = 43.52964.928 X 0.3083 = 20.017
43.529 + 20.017 = 63.546
Review What information does the atomic
number give us? How do we determine the number
of neutrons of any element? Who discovered the electron? What discovery did the Gold Foil
Experiment led to?
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