4.2 Structure of the Nuclear Atom > Chapter 4 Atomic Structure. 4.2 Structure of the Nuclear Atom. 4.1 Defining the Atom
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1 Chapter 4 Atomic Structure 4.1 Defining the Atom 4.2 Structure of the Nuclear Atom 4.3 Distinguishing Among Atoms 1
2 CHEMISTRY & YOU How did scientists determine the structures that are inside an atom? Doctors often use X-rays to see bones and other structures that cannot be seen through your skin. Scientists use many methods to see inside an atom. 2
3 Subatomic Particles Much of Dalton s atomic theory is accepted today. One important change, however, is that atoms are now known to be divisible. They can be broken down into even smaller, more fundamental particles, called subatomic particles. Three kinds of subatomic particles are electrons, protons, and neutrons. 3
4 Subatomic Particles Electrons In 1897, the English physicist J. J. Thomson ( ) discovered the electron. Electrons are negatively charged subatomic particles. 4
5 Subatomic Particles Electrons One electrode, the anode became positively charged. The other electrode, the cathode, became negatively charged. The result was a glowing beam, or cathode ray, that traveled from the cathode to the anode. 5
6 Subatomic Particles Electrons Thomson found that a cathode ray is deflected by electrically charged metal plates. A positively charged plate attracts the cathode ray, while a negatively charged plate repels it. 6
7 Subatomic Particles Electrons Thompson knew that opposite charges attract and like charges repel, so he hypothesized that a cathode ray is a stream of tiny negatively charged particles moving at high speed. Thompson called these particles corpuscles. Later they were named electrons. 7
8 Subatomic Particles Electrons A cathode ray can also be deflected by a magnet. 8
9 Electrons Subatomic Particles To test his hypothesis, Thompson set up an experiment to measure the ratio of an electron s charge to its mass. He found this ratio to be constant. Also, the charge-to-mass ratio of electrons did not depend on the kind of gas in the cathode-ray tube or the type of metal used for the electrodes. 9
10 Subatomic Particles Electrons Thompson concluded that electrons are a component of the atoms of all elements. 10
11 Subatomic Particles Electrons The U.S. physicist Robert A. Millikan ( ) carried out experiments to find the quantity of an electron s charge. In his oil-drop experiment, Millikan suspended negatively charged oil droplets between two charged plates. He then changed the voltage on the plates to see how this affected the droplets rate of fall. 11
12 Subatomic Particles Electrons The U.S. physicist Robert A. Millikan ( ) carried out experiments to find the quantity of an electron s charge. From his data, he found that the charge on each oil droplet was a multiple of coulomb, meaning this must be the charge of an electron. 12
13 Subatomic Particles Electrons The U.S. physicist Robert A. Millikan ( ) carried out experiments to find the quantity of an electron s charge. Using this charge and Thomson s charge-to-mass ratio of an electron, Millikan calculated an electron s mass. Millikan s values for electron charge and mass are similar to those accepted today. An electron has one unit of negative charge, and its mass is 1/1840 the mass of a hydrogen atom. 13
14 Subatomic Particles Protons and Neutrons If cathode rays are electrons given off by atoms, what remains of the atoms that have lost the electrons? For example, after a hydrogen atom (the lightest kind of atom) loses an electron, what is left? You can think through this problem using four simple ideas about matter and electric charges. 14
15 Subatomic Particles Protons and Neutrons You can think through this problem using four simple ideas about matter and electric charges. 1. Atoms have no net electric charge; they are electrically neutral. 2. Electric charges are carried by particles of matter. 3. Electric charges always exist in whole-number multiples of a single basic unit; that is, there are no fractions of charges. 4. When a given number of negatively charged particles combines with an equal number of positively charged particles, an electrically neutral particle is formed. 15
16 Subatomic Particles Protons and Neutrons It follows that a particle with one unit of positive charge should remain when a typical hydrogen atom loses an electron. 16
17 Subatomic Particles Protons and Neutrons In 1886, Eugen Goldstein ( ) observed a cathode-ray tube and found rays traveling in the direction opposite to that of the cathode rays. He concluded that they were composed of positive particles. Such positively charged subatomic particles are called protons. 17
18 Subatomic Particles Protons and Neutrons In 1932, the English physicist James Chadwick ( ) confirmed the existence of yet another subatomic particle: the neutron. Neutrons are subatomic particles with no charge but with a mass nearly equal to that of a proton. Although protons and neutrons are extremely small, theoretical physicists believe that they are composed of yet smaller subnuclear particles called quarks. 18
19 Interpret Data The table below summarizes the properties of these subatomic particles. Properties of Subatomic Particles Particle Symbol Relative charge Relative mass (mass of proton = 1) Actual mass (g) Electron e 1 1/ Proton p Neutron n
20 What evidence did Thompson have that led him to conclude the cathode ray was a stream of tiny negatively charged particles? The ray was attracted to a metal plate with positive electric charge, and Thompson knew that opposite charges attract and like charges repel. 20
21 When subatomic particles were discovered, scientists wondered how the particles were put together in an atom. 21
22 When subatomic particles were discovered, scientists wondered how the particles were put together in an atom. Most scientists including J. J. Thompson thought it likely that the electrons were evenly distributed throughout an atom filled uniformly with positively charged material. 22
23 When subatomic particles were discovered, scientists wondered how the particles were put together in an atom. Most scientists including J. J. Thompson thought it likely that the electrons were evenly distributed throughout an atom filled uniformly with positively charged material. In Thomson s atomic model, known as the plum-pudding model, electrons were stuck into a lump of positive charge, similar to raisins stuck in dough. 23
24 The Atomic Nucleus This model of the atom turned out to be short-lived, however, due to the work of a former student of Thomson, Ernest Rutherford ( ). Born in New Zealand, Rutherford was awarded the Nobel Prize for Chemistry in His portrait appears on the New Zealand $100 bill. 24
25 The Atomic Nucleus Rutherford s Gold-Foil Experiment In 1911, Rutherford and his co-workers wanted to test the existing plum-pudding model of atomic structure. They devised the gold-foil experiment. Their test used alpha particles, which are helium atoms that have lost their two electrons and have a double positive charge because of the two remaining protons. 25
26 The Atomic Nucleus Rutherford s Gold-Foil Experiment In the experiment, a narrow beam of alpha particles was directed at a very thin sheet of gold. 26
27 The Atomic Nucleus Rutherford s Gold-Foil Experiment In the experiment, a narrow beam of alpha particles was directed at a very thin sheet of gold. According to the prevailing theory, the alpha particles should have passed easily through the gold, with only a slight deflection due to the positive charge thought to be spread out in the gold atoms. 27
28 The Atomic Nucleus Rutherford s Gold-Foil Experiment Rutherford s results were that most alpha particles went straight through, or were slightly deflected. 28
29 The Atomic Nucleus Rutherford s Gold-Foil Experiment Rutherford s results were that most alpha particles went straight through, or were slightly deflected. What was surprising is that a small fraction of the alpha particles bounced off the gold foil at very large angles. Some even bounced straight back toward the source. 29
30 CHEMISTRY & YOU How did scientists see inside an atom to determine the structures that are inside an atom? Scientists determined the structures inside an atom by observing how the atom interacted with particles with known properties, like negatively charged electrons or positively charged alpha particles. 30
31 The Atomic Nucleus The Rutherford Atomic Model Based on his experimental results, Rutherford suggested a new theory of the atom. He proposed that the atom is mostly empty space. Thus explaining the lack of deflection of most of the alpha particles. 31
32 The Atomic Nucleus The Rutherford Atomic Model Based on his experimental results, Rutherford suggested a new theory of the atom. He concluded that all the positive charge and almost all of the mass are concentrated in a small region that has enough positive charge to account for the great deflection of some of the alpha particles. 32
33 The Atomic Nucleus The Rutherford Atomic Model The Rutherford atomic model is known as the nuclear atom. In the nuclear atom, the protons and neutrons are located in the positively charged nucleus. The electrons are distributed around the nucleus and occupy almost all the volume of the atom. 33
34 The Atomic Nucleus The Rutherford Atomic Model According to this model, the nucleus is tiny and densely packed compared with the atom as a whole. If an atom were the size of a football stadium, the nucleus would be about the size of a marble. 34
35 The Atomic Nucleus The Rutherford Atomic Model Rutherford s model turned out to be incomplete. The Rutherford atomic model had to be revised in order to explain the chemical properties of elements. 35
36 What evidence from Rutherford s Gold-Foil experiment disproves J.J. Thompson s plumpudding model? Rutherford observed that most of the particles passed through the foil with no deflection, and a small fraction were deflected at large angles or reflected directly back. If the plum-pudding model was true, most alpha particles would have been deflected at small angles by the evenly-spaced electrons. 36
37 Key Concepts Three kinds of subatomic particles are electrons, protons, and neutrons. In the nuclear atom, the protons and neutrons are located in the nucleus. The electrons are distributed around the nucleus and occupy almost all the volume of the atom. 37
38 Glossary Terms electron: a negatively charged subatomic particle cathode ray: a stream of electrons produced at the negative electrode (cathode) of a tube containing a gas at low pressure proton: a positively charged subatomic particle found in the nucleus of an atom neutron: a subatomic particle with no charge and a mass of 1 amu; found in the nucleus of an atom nucleus: the tiny, dense central portion of an atom, composed of protons and neutrons 38
39 BIG IDEA Electrons and the Structure of Atoms Atoms have positively-charged protons and neutral neutrons inside a nucleus, and negatively-charged electrons outside the nucleus. 39
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