1. Atomic Structure
A History of the Atom
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2. Atomic Structure
By the late 1800’s scientist were convinced that atoms were the fundamental units of which all matter is composed.
They soon learned that the atom was not indivisible.
Atoms are composed are smaller (subatomic) particles: proton, neutron, and electron
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3. Atoms
An atom is the smallest particle of an element that retains the properties of that element.
Atoms are extremely small. One gram of Pb (lead) has
2.9 x 1021 atoms.
Compare that to the Earth’s population which is about
4 x 109 people.
So…….where did the idea of atoms come from?
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4. Atoms
The idea of atoms were first suggested by an ancient Greek citizen named Democritus.
The word “atom” comes from the
Greek language:
Atomos = Indivisible
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5. Atoms
It wasn’t until the late 1700’s that chemist were able to relate chemical changes to events at the level of individual atoms.
At that time, an English chemist and physicist named John Dalton ( ) first stated his atomic theory.
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6. Atoms: Daltons Atomic Theory
1-All elements are composed of tiny indivisible particles
called atoms.
2-Atoms of the same element are identical. The atoms of
any one element are different from atoms of another
element.
3- Atoms of different elements can combine in simple
whole number ratios to form compounds.
4 – Chemical reactions occur when atoms are separated,
joined or rearranged. However, atoms of one
element are not changed into atoms of another
element by a chemical reaction.
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7. Atoms of “A” Atoms of “B” Mixture of Compound of “A” and “B” Molecules made
from “A” and “B”
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8. Electrons, Protons, and Neutrons
*Electrons are negatively charged subatomic particles.
*They were primarily the interest of electricians rather than chemist.
*These scientists (i.e. electricians) studied the flow of gases in an enclosed tube…at low pressure. The tube had two metal plates at each end. One of the plates held a positive charge and the other a negative charge. When high voltage was applied, the gas inside the tube glowed.
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10. The device they used is called a cathode ray tube.
The glowing beam inside the tube is called a cathode ray.
Electrons (which are negatively charged are attracted to the positive plate) hence electrons travel from the negative cathode toward the positive anode.
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11. An English physicist named
Sir Joseph J. Thomson ( ) experimented with Cathode rays.
In 1897, he found that cathode rays could be deflected by a magnet or
an electrically charged
plate place within or near
the Cathode ray tube.
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12. Cathode rays are a collection of very small negatively charged
particles.
He called these particles
Electrons.
He found out the following:
J.J. Thomson
The mass of an electron is lighter than a hydrogen atom.
No matter what gas was used in the cathode ray tube or the type of metal used for electrodes within the tube…cathode rays are ALWAYS made of electrons.
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13. J.J. Thomson believed electrons exisited in ALL atoms!
His model of the atom became known as the “plum pudding” model of the atom!
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14. Answer: It would exist as a bare proton.
Hydrogen Atom
Q: If atoms are electrically neutral, what would happen to a hydrogen atom if it lost it’s only electron?
Answer: It would exist as a bare proton.
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15. A single proton is 1840 x heavier than an electron.
Hydrogen Atom
A single proton is 1840 x heavier than an electron.
A proton carries a single positive charge.
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16. confirmed the existence of yet another subatomic particle:
In 1932 the physicist, James
Chadwick (1891 – 1974)
confirmed the existence of yet
another subatomic particle:
the neutron.
* Neutrons are subatomic particles with NO charge.
* They reside with protons in the nucleus.
The mass of a neutron is nearly equal to the mass of a
proton!
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17. The fundamental building blocks of an atom are:
At this point, the fundamental building blocks of an atom were in existence!
The fundamental building blocks of an atom are:
Protons, neutrons, and
electrons.
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18. In 1886, Eugen Goldstein observed rays traveling in the opposite direction of the cathode ray. This occurred when used a cathode with holes in it.
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19. He later called these rays, “Canal Rays”
He later called these rays, “Canal Rays”. Later, the canal rays were found to be made up of positively
charged particles.
Eugen Goldstein
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20. If the cathode ray tube contained Hydrogen gas, then the canal rays were made up of bare protons!
Eugen Goldstein
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21. Properties of Subatomic Particles
Symbol
Relative
Electrical
Charge
Approximate
Mass
(amu)
Actual
(grams)
Electron e- 1-
1/1840
9.11 x 10-28
Proton p+ 1+ 1
1.67 x 10-24
Neutron n0
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22. Click the link below to view Rutherford’s now famous
The discovery of the nucleus (which houses protons and neutrons) is credited to
Ernest Rutherford.
Click the link below to view
Rutherford’s now famous
“Gold Foil Experiment”.
Click Here to see Rutherford’s Gold Foil Experiment
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23. The Structure of the Atom
The nucleus of an atom is composed of ____________ and _____________.
protons
neutrons
The nucleus has a ___________ charge and occupies a very small part of the volume of an atom.
positive
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
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24. Atomic Number
The atomic number of an element
is the number of protons in the nucleus of an atom for that element.
Since atoms are electrically neutral, the number of protons in the nucleus of an atom must equal the number of electrons orbiting the nucleus
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
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25. Atomic Number
Q: Element Carbon is atomic number 6. How many protons and electrons are in a carbon atom?
6 p+ and 6 e-
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Answer: ______________________________
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26. Sodium Atomic Number Q: The atomic number of an element is 11.
What is the element?
Sodium
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Answer: ______________________________
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27. REVIEW Who am I ? Democritus
I’m the first to develop the concept of atoms. I am a Greek philosopher.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Democritus
Answer: ______________________________
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28. REVIEW Who am I ? John Dalton
I developed an early atomic theory that stated atoms can combine with each other to form new compounds.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Answer: ______________________________
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29. REVIEW Who am I ? J.J. Thomson
I “coined” the term “electrons” and designed the “plum pudding” model of the atom.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Answer: ______________________________
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30. REVIEW Who am I ? James Chadwick
I am an English physicist who discovered the neutron.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Answer: ______________________________
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31. REVIEW Who am I ? Ernest Rutherford
I designed a simple experiment known as the gold foil experiment. I am credited with the discovery of the nucleus.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Answer: ______________________________
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32. REVIEW Who am I ? Neils Bohr I developed what is known
as the “planetary model”
of the atom.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Answer: ______________________________
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33. REVIEW What is the term used to describe the number
of protons in the nucleus
of an atom?
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Atomic Number
Answer: ______________________________
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34. REVIEW Which subatomic particle is negatively charged and orbits the
nucleus of an atom?
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
The electron
Answer: ______________________________
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35. REVIEW Which subatomic particle has no charge and is usually found in
the nucleus of an atom?
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
The neutron
Answer: ______________________________
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36. REVIEW Which subatomic particle has a positive
charge and is found in the
nucleus of an atom?
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
The proton
Answer: ______________________________
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37. Mass Number Most of the mass of an atom is concentrated in the
nucleus.
The mass number is the total
number of protons and
neutrons in the nucleus.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
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38. Using a periodic chart, complete the chart below:
Atomic Mass Number Number Number Symbol
number number of of of
protons neutrons electrons 7 14 7 7 7 N 9 19 9 10 9 F 19 39 19 20 19 K 27 59 27 32 27 Co
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39. Great Job! Now let’s continue our lesson… End of Review
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
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40. Isotopes Isotopes are atoms! They belong to the same element!
Because they belong to the same element they have the same number of protons…..BUT
they have a different number of neutrons
Greek: Isotopos = the same place
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Atoms that have the same number of protons but a different number of neutrons are called Isotopes.
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41. Isotopes Atoms of the same element Same Number of Protons
Different Number of Neutrons
6 p+
6 p+
6 p+
6 n0
7 n0
8 n0
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
6 e-
6 e-
6 e-
Carbon-12
Carbon-13
Carbon-14
98.89%
1.10%
.01%
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42. C Symbols for Isotopes 12 6 Mass Number Atomic Number 6 p+ 6 n0 6 e-
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Atomic
Number
6 e- 6
Carbon-12
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43. O O O 8 16 8 17 8 18 Check your Understanding Oxygen – 16 Oxygen – 17
Write the symbol for the following isotopes.
Oxygen – 16
Oxygen – 17
Oxygen – 18 O 8 16 O 8 17 O 8 18
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
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44. N 18 7 Check your Understanding 11 Neutrons
Determine the number of neutrons in Nitrogen-18. 18
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom. 7
11 Neutrons
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45. Atomic Mass
The atomic mass of an element is an “average” of many numbers. That’s why it doesn’t appear as a “whole number” on the periodic chart.
Atomic Mass is defined as the weighted average of the masses of the isotopes of that element.
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
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46. Atomic Mass Example Problem:
Element X has two natural isotopes. The isotope with a mass number of 10 has a natural abundance of 20%. The isotope with a mass number of 11 has a relative abundance of 80%. Estimate the average atomic mass for the element from these figures. What is the true identity of element X?
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
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47. Atomic Mass 11X 11 amu x .80 = 8.8 amu Total 10.8 amu
Example Problem Solution:
10X amu x = amu
11X amu x = amu
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
Total amu
The average atomic mass of element X is 10.8 amu. Element X is Boron. Boron also has an
atomic number of 5
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48. Atomic Mass
Hydrogen has three naturally occurring isotopes.
Since most of the hydrogen atoms found in nature are Hydrogen-1 isotopes, the average atomic mass of Hydrogen calculates to be
amu.
1 p+
1 p+
1 p+
0 n0
1 n0
2 n0
Even before neutrons were discovered scientist wondered how electrons and protons were positioned within the atom.
1 e-
1 e-
1 e-
Hydrogen-1
Hydrogen-2
Hydrogen-3
Deuterium
Tritium