Atomic Theory: Early Models of the Atom:
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1 Atomic Theory: Our next job in Chemistry 11 is to learn about what matter is made of. After we have done this, we can start to understand why matter behaves the way it does. Everything that has volume and mass is made up of atoms. The ONLY difference between different substances is the differences in the atoms. We will come back to this idea after we find out what makes each atom different. Early Models of the Atom: 1/ Democritus: (Greek Philosopher 450 B.C.) Proposed that all matter was made up of tiny indivisible particles he called ATOMOS. Aristotle disagreed because he said that if this were true, wouldn t everything fall apart in a windstorm? 2/ John Dalton: (British School Teacher 1803) Studied other people s experiments. Came up with the ATOMIC THEORY OF MATTER: o Each element is composed of small particles called atoms. o All atoms of a given element are identical, but they differ from those of any other element. o Atoms can neither be created nor destroyed. o A given compound always has the same relative numbers and kinds of atoms. His model is called the BILLIARD BALL MODEL. Question: if they are like billiard balls, how can atoms of one element behave differently than another?
2 3/ Faraday: (English Chemist 1839) Did a huge amount of experiments. Discovered that atoms have electrical energy. Benjamin Franklin: came up with the idea of positive and negative charge. 4/ J. J. Thomson: (English Physicist 1896) Studied Cathode Ray Tubes (they used to be in old TV s). CRT are tubes with very little air in them and allow an electrical current to pass through (have a positive and negative end). When an electrical current is applied to a gas inside the tube, it creates a beam of particles. Thomson placed a magnet near this beam and found that the beam bent TOWARDS THE POSITIVE END OF THE MAGNET. From this experiment, he concluded that the beam was made up of particles of negative charge, which he called ELECTRONS. His model is called the PLUM PUDDING or BLUEBERRY MUFFIN MODEL.
3 5/ Henri Bequerel: (French Physicist 1896) Discovered radioactivity when he left a chunk of uranium in a drawer with undeveloped film. The radiation caused an image of the uranium chunk to be created. 5a) The Curie s Sidebar: Radioactive Particles Particle Symbol Charge Mass Penetrating Ability Alpha Beta Gamma 6/ Ernest Rutherford: (New Zealand Physicist 1900 s) Studied Radioactivity. The radioactive particles were alpha particles. He aimed and shot alpha particles at a sheet of gold foil that was pounded so flat it was a couple of atoms thick. His experiment was surrounded by a screen that would show the radioactive particles. Most particles: Some particles:
4 A couple of particles: His model is called the PLANETARY MODEL. 7/ Others: Bohr: studied the hydrogen atom and furthered our knowledge of electron structure. De Broglie: studied the wave nature of light and furthered our knowledge of electron structure. Schrodinger: also furthered our knowledge of electron structure. The Current Understanding of the Atom: * There are subatomic particles: protons, electrons, and neutrons. Protons: (p)
5 THE NUMBER OF PROTONS IN THE NUCLEUS DETERMINES THE IDENTITY OF THE ELEMENT (because only that element has that atomic number) Neutrons: (n) WHEN THE NUMBER OF NEUTRONS IS DIFFERENT, THEY ARE CALLED ISOTOPES. Question: What property of the atom will change if the number of neutrons changes? The mass number:
6 * Electrons weigh essentially nothing (9.11 x g). This means that all the mass of the atom is in the nucleus from the protons and neutrons (each weighing 1). * Therefore, in order to calculate the mass number of an atom we just add the number of protons and neutrons together (mass number = p + n) * Isotopes require that we learn a unique symbol notation to write the elements, but we need to take time out to learn all of the ways. 1/ The Periodic Table Notation - almost always the periodic table symbol is written like this: 2/ Element Symbol Notation:
7 3/ Isotope Symbol Notation because they are all the same element, the atomic number is not written: Sometimes they are written Hydrogen-1, Hydrogen-2, and Hydrogen-3. * But wait a minute!!!!! If the mass of the atom is just the number of protons and neutrons is equal to the mass of the atom, what is up with those numbers in the periodic table!!!!! * The masses listed in the periodic table are: * In order to understand where this number comes from we need to know about what is called a weighted average. An example of this is the average numbers of siblings in this class. * In order to calculate the AVERAGE ATOMIC MASS of a element, we need to know how many of each isotope we have.
8 Ex: The Isotopes of Boron * The numbers of each isotope is given as a percent abundance. What that means is that if we had 100 atoms of that element, that many would be expected to that isotope (remember that a percentage is a number out of 100) Ex: The Isotopes of Oxygen Try One: Calculate the average atomic mass for Chlorine
9 Would you expect the average atomic mass for Uranium to be closer to 235 or 238? Why? * In order to pick out the mass number vs. the average atomic mass: the mass number is a whole number and is p + n, while the average atomic mass is not a whole number and is from the periodic table. Electrons: (e - ) What property of the atom will change if the number of electrons is different? A negatively charged atom: A positively charged atom: ******* REMEMBER: it is only the number of electrons that changes when an ion is created. If the number of protons changes, it would no longer be the same element.
10 ******** When electrons are removed, the atom becomes: ******** When electrons are added, the atom becomes: Ex: Sulphur Now, to wrap it all up into one neat little package: Ex: 235 U # of protons? mass number or average atomic mass? # of electrons? # of neutrons?
11 Ex: Mg 2+ # of protons? mass number or average atomic mass? # of neutrons? # of electrons? atomic number? Ex: element has 32 protons and 35 electrons element symbol? charge? anion, cation or atom? # of neutrons? Mass number or average atomic mass?
12
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