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Atomic Research

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Marissa Smith

on 6 February 2018

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Transcript of Atomic Research

What is/makes up an atom?
An atom can be described as the basic unit of a chemical element and/or a source of nuclear energy.

It is consisted of protons, electrons, and neutrons.
Electrons: where they are located, how many are equal to a proton, and location/definition of valence electrons
- Electrons are found surrounding the nucleus consisting of protons and neutrons.
- approximately 2,000 electrons are equal to one proton
- A valence electron is an outer shell electron that is associated with an atom.
Atomic mass/number of an atom
The average atomic mass of an atom is approximately 35 amu. When calculating the atomic mass of anything, you multiply the fraction by the mass number of each isotope, then adding the two together.

The atomic number allows you to identify each element on the periodic table by the approximate number of protons in said element.
Components of a proton and the discovery of quarks

Components of a proton: Protons are consisted of three quarks, two up and one down.
Discovery of quarks: Quarks were discovered in 1968 by scientists. There are three quarks in each proton, held together by particles known as gluons.
Nucleus: What is it made of? Where is most of the mass of the atom located?
The nucleus is made up of a certain number of protons, neutrons, and electrons depending on the element/chemical.

Most of an atom's mass is centralized within the nucleus.
Proton: symbol and charge
Neutron: symbol and charge
Electron: symbol and charge
Proton: The symbol of a proton is + ; therefore meaning that the charge is positive.
Neutron: The neutron has no symbol, meaning that the charge coincides with it's name, ending up neutral instead of positive or negative.
Electron: The symbol of an electron is - ; therefore meaning that the charge is negative.
Atomic Research
Marissa Smith
1st period 2/6/2018

Ernest Rutherford
Atomic theory creation
"Gold foil" experiment explanation
Ernest Rutherford was a physicist originating from Nelson, New Zealand. His atomic theory consisted of the atom having a tiny and heavy nucleus. When conducting his "gold foil" experiment, Rutherford shot a beam of alpha particles at a sheet of gold foil. When the particles made contact with the foil, a few were deflected. Rutherford conducted the thought that this was caused by a tiny, dense nucleus.
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