1.1 Atomic Structure

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35 Terms

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Ancient greek model of the atom

Atoms are tiny solid spheres which cannot be divided

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JJ Thompson

Discovered the electron and developed the "plum-pudding" model of the atom

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Plum pudding model of the atom

atoms are balls of positive charge with negative electrons embedded in it

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Rutherford, Geiger, and Marsden

carried out alpha particle scattering experiment and developed the nuclear model of the atom

<p>carried out alpha particle scattering experiment and developed the nuclear model of the atom</p>
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Alpha particle scattering experiment

Fired alpha particles at a thin sheet of gold foil.

<p>Fired alpha particles at a thin sheet of gold foil.</p>
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Observations of the alpha particle scattering experiment

Most of the alpha particles went straight through the atom, a few bounced back

<p>Most of the alpha particles went straight through the atom, a few bounced back</p>
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Conclusions of the alpha particle scattering experiment

Most of the atom is empty space except for a tiny positive nucleus

<p>Most of the atom is empty space except for a tiny positive nucleus</p>
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Nuclear model of the Atom

Atoms are made of a small positive nucleus orbited by negative electrons.

<p>Atoms are made of a small positive nucleus orbited by negative electrons.</p>
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Niels Bohr

Suggested that electrons orbit the nucleus at specific distances

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James Chadwick

Carried out experiments which provided evidence of neutrons

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Relative mass of protons, neutrons and electrons

1, 1, 1/1840

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Relative charge of protons, neutrons and electrons

+1, 0, -1

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Why are atoms neutral?

same number of positive protons as negative electrons

<p>same number of positive protons as negative electrons</p>
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Atomic number

the number of protons in the nucleus of an atom

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Locations of subatomic particles

Protons/ neutrons- Nucleus

Electrons- Orbiting shells surrounding nucleus

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Proton

has a positive charge, defines the type of atom and that is found in the nucleus

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mass number (atomic mass)

number of protons + number of neutrons

<p>number of protons + number of neutrons</p>
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Average atomic radius

0.1 nm (1 Ă— 10-10 m)

<p>0.1 nm (1 Ă— 10<sup>-10</sup> m)</p>
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Average radius of an atomic nucleus

10,000 times smaller than an atom (1 x 10-14 m)

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Relative atomic mass

weighted average mass of an atom of an element

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Relative atomic mass formula

(atomic mass*percentage abundance)+(atomic mass*percentage abundance)/(total percentage abundance)

<p>(atomic mass*percentage abundance)+(atomic mass*percentage abundance)/(total percentage abundance)</p>
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Shells can hold

2, 8, 8 electrons

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No of shells =

Period on the periodic table

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What are valence electrons?

Outer shell electrons which are involved in reactions

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No of valence electrons =

Group number on the periodic table

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Hydrogen electron structure

1

<p>1</p>
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Nitrogen electron structure

2,5

<p>2,5</p>
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Argon electron structure

2,8,8

<p>2,8,8</p>
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Potassium electron structure

2,8,8,1

<p>2,8,8,1</p>
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Calcium electron structure

2,8,8,2

<p>2,8,8,2</p>
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Aluminium electron structure

2,8,3

<p>2,8,3</p>
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Magnesium electron structure

2,8,2

<p>2,8,2</p>
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Oxygen electron structure

2,6

<p>2,6</p>
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Fluorine electron structure

2,7

<p>2,7</p>
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Carbon electron structure

2,4

<p>2,4</p>