Chemistry Chapter 4
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| Dalton's Atomic Theory Part 1 | 1. All matter is made of small particles called atoms
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| Dalton's Atomic Theory Part 2 | 2. All atoms in an element are identical
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| Dalton's Atomic Theory Part 3 | 3. Atoms cannot be created, divided, or destroyed
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| Dalton's Atomic Theory Part 4 | 4. Different atoms combine to make compounds
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| Dalton's Atomic Theory Part 5 | 5. Chemical reaction-atoms are separated or combined
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| Democritus's Ideas Part 1 | 1. Matter is composed of empty space through which atoms move.
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| Democritus's Ideas Part 2 | 2. Atoms are solid, homogeneous, indestructible, and indivisible.
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| Democritus's Ideas Part 3 | 3. Different kinds of atoms have different sizes and shapes.
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| Democritus's Ideas Part 4 | 4. The differing properties of matter are due to the size, shape, and movement of atoms.
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| Democritus's Ideas Part 5 | 5. Apparent changes in matter result from changes in the groupings of atoms and not from changes in the atoms themselves.
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| Atom | The smallest particle of an element that retains the properties of the element.
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| Cathode Ray | A ray of radiation that originates from the cathode and travels to the anode of a cathode ray tube.
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| Electron | Negatively charged particles that are part of all forms of matter.
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| Nucleus | A small, positively charged, dense center of an atom that contains protons and neutrons. It is surrounded by empty space through which electrons move.
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| Proton | A subatomic particle in the nucleus with a 1+ charge
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| Neutron | A neutral subatomic particle in the nucleus with the same mass as the protons
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| Atomic Number | The number of protons in an atom. This determines what element it is. It is the number above the symbol on a periodic table and determines where it is on the periodic table.
atomic number=number of protons=number of neutrons
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| Isotope | Atoms with the same number of protons, but different number of neutrons.
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| Mass Number | Sum of protons and neutrons in a nucleus.
The number is added after the element's name to distinguish which isotope it is.
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| Atomic Mass Unit (amu) | One-twelfth the mass of a carbon-12 atom
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| Atomic Mass | The weighted average mass of the isotopes of that element
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| Cathode Ray Tube Experiment-process | A tube is filled with low pressure gas. An electrode at each end is attached to a battery. Light flashes from the cathode ray
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| Cathode Ray Tube Experiment-results | 1. Particles of the ray are in all matter
2.Cathode rays are streams of charged particles
3. These particles carry a negative charge
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| J.J. Thompson | Discovered the existence of subatomic particles using cathode ray tube experiments.
Plum Pudding Model
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| Robert Millikan | Determined each electron was 1- charge and calculated an electron's mass
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| Plum Pudding Model | Negatively charged electrons were distributed thought a uniform positive charge.
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| Ernest Rutherford | Used gold foil experiment to disprove the plum pudding model.
Discovered the nucleus.
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| Gold Foil Experiment-process | A beam of alpha particles is aimed at a gold foil. A zinc sulfide screen surrounds the foil and marks where the alpha particles hit.
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| Gold Foil Experiment-results | Some alpha particles deflected at large angles.
Nuclear Atom Model developed
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| Nuclear Atom Model | Most of an atoms is electrons moving rapidly through empty space surrounding a nucleus and are held to the atom by their attraction to the positively charged nucleus.
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| James Chadwick | Discovered neutrons
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| Subatomic Particles | Electrons, protons, and neutrons that make up all atoms
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| Calculate number of protons | atomic number = number of protons = number of electrons
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| Calculate number of electrons | atomic number = number of protons = number of electrons
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| Calculate number of neutrons | Mass number - atomic number = number of neutrons
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| Mass of an Electron | .000549 amu
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| Mass of a Proton | 1.007 amu
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| Mass of a Neuton | 1.008 amu
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| Oil Drop Experiment-results | determined the charge of an electron
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| Rutherford's Proton Experiment | Gold Foil Experiment
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| Chadwick's Neutron Experiment | Using scatter measurements
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