Chemistry. - Many philosophers concluded that matter was composed of things such as earth, -Democritus: -Aristotle: -Dalton:
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1 Chemistry Made by Saleem Abu-Tayeh Chapter 4 - Many philosophers concluded that matter was composed of things such as earth, water, air, and fire. It was also commonly accepted that matter could be endlessly divided into smaller and smaller pieces. -Democritus: Wast he first person to propose the idea that matter was not infinitely divisible. He believed matter was made up of tiny individual particles called atoms. He believed that atoms could not be created, destroyed, or further divided. -Aristotle: He rejected the notion of atoms because it did not agree with his own ideas about nature. Atoms moved through empty Space, NOT. -Dalton: elements involved in those reactions. He was able to use experiments to determine the mass ratios of the -Law of conversation of mass states that mass is conserved any process, such as a chemical reaction. -Dalton s atomic theory easily 1
2 explains that the conservation of mass in chemical reactions it he result of the separation, combination, or rearrangement of atoms-atoms that are not created, destroyed, or divided in the process. - Atoms of the same element can have slightly different masses. - Section 1 Review: Democritus was the first person to propose the existence of atoms. According to Democritus, atoms are solid, homogenous, and indivisible. Aristotle did not believe in the existence of atoms. John Danton s atomic theory is based on numerous scientific experiments. - Smallest particle of an element that retains the properties of element is called an atom. - Atoms can be views using Scanning tunneling microscope (STM). - The cathode-ray tube and Sir William Crookes: A green flash was produced by some form of radiation striking a zinc-slide coating that had been applied to he end of the tube. This ray, originating from the cathode and traveling to the anode, was called a cathode ray. The accidental discovery of the cathode ray led to the invention of the TV. Cathode rays were a dream of charged particles. The particles carried a negative charge. (The exact value of the negative charge was not known.) Negatively charge particles that are part of all forms of matter are now known as electrons. - Charge-to mass ratio: 2
3 Thomson was able to determine the charge-to-mass ratio of the charged particle. Thomson concluded that the mass of the charged particle was much less than that of a hydrogen atom, the lightest known atom. - The oil-drop experiment and the charge of an electron: Robert Milikan determined the charge of an electron using the oil-drop apparatus. He was able to determine the magnitude of the charge on each drop increased in discrete amounts and determined that the smallest common denominator was 1.602*10^-19, he identified this numbers as the charge of the electron. A single electron carries a charge of 1-. -Mass of an electron is 1/1840 -JJ Thomson proper a model of the atom that became known as the plum pudding model. -In 1911, Ernest Rutherford began to study how positively charged alpha particles interacted with solid matter. -Rutherford concluded that the plum pudding model was incorrect because it could not explain the results of the gold foil experiment. - He calculated that ann atom consisted mostly of empty space through which the electrons move. - He also concluded that almost all of the atom s positive charge and almost all of its was were contained in a tiny, dense region int he center of the atom, which he called the nucleus. - A proton is a subatomic particle carrying a charge equal to but opposite of an election; that is, a proton has a charge of 1+. 3
4 -A neutron is a subatomic particle that has a mass nearly equal to that of a proton, but it carries no electric charge. -Section 2 Review: An atom is the smallest parties of an element that maintains the properties of that element. Electrons have a 1- charge, proton have a 1+ charge, and neutron have no charge. An atom consist mostly of empty space surrounding the nucleus. -Atomic number: The number of protons in an atom. -Atoms with the same number of protons but different numbers of neutrons are called isotopes. -The mass number is the sum of the atomic number and neutron in the nucleus. - Atomic mass unit (amu) is defined as one-twelfth the mass of a carbon-12 atoms. 4
5 - Atomic mass of an element is the weighted average mass of the isotopes of that element. 5
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