1. Atoms Unit 3 Introduction to the Atom History of the Atom+ -

2. Some of the First Discussions about the Atom….
Democritus (400 BC) named the atom, which means indivisible, and said it was the smallest particle and could not be broken down.
He was pretty much correct in that if you did break the atom down, it wouldn’t be that “element” any more. But he wasn’t aware that the atom was made up of particles.
IN OTHER WORDS: Gold is an element. The smallest part of gold that is STILL gold is an atom.

3. Greeks Philosophers Continue the Discussion and Disagree
Aristotle (350 BC) believed matter could always be broken down into smaller and smaller parts.
And this is true to a certain extent… but eventually you come to the small basic particles that can no longer be broken apart.
In other words: You CAN break an atom of gold down into its parts… protons, electrons and neutrons, however, it wouldn’t be gold anymore.

4. His ideas are now called the Atomic Theory of Matter
Dalton's Atomic Theory
In 1808, John Dalton proposed that elements were composed of atoms & that only whole numbers of atoms can combine to form compounds
His ideas are now called the Atomic Theory of Matter
Dalton’s Atomic Theory ( AD) was widely accepted but not totally correct

5. Dalton’s Atomic Theory
All matter is composed of atoms. THIS IS TRUE
Atoms of the same kind of elements are identical; atoms of different elements are different from each other. THIS IS PARTLY TRUE
ELEMENT 1
ELEMENT 2
ELEMENT 3
ELEMENT 4
Dalton’s Atomic Theory

6. Atoms can’t be changed, created, or destroyed. THIS IS PARTLY TRUE
You can make compounds out of combinations of different atoms THIS IS TRUE
Chemical reactions are rearranging or recombining atoms THIS IS TRUE + +

7. Atomic Theory Not all of Dalton’s claims were true
Atoms CAN be divided into even smaller particles (Protons, electrons, neutrons)
Some elements have atoms that have different masses. (ISOTOPES)
Atomic Theory

8. Atomic Theory Dalton’s Atomic Theory of Matter has been modified.
What remains is…
All matter is composed of atoms
Atoms of any one element differ in properties from atoms of another element
Atomic Theory

9. In the 1800’s it was determined that atoms are actually composed of several basic types of smaller particles
It’s the number and arrangement of these particles that determine the atom’s chemical properties.
A new definition of an atom is the one we use today: The smallest particle of an element that retains the chemical properties of that original element.
Atomic Theory

10. Plum Pudding Model
JJ Thomson’s cathode ray tube experiment in the late 1800s showed that atoms had smaller parts, called negative corpuscles; he developed the “plum pudding model.”
The plum pudding model showed electrons (the plums) mixed in together with protons (the cake batter)

11. Negative particles embedded in a sphere of positive plasma-like matter.
THINK…
Chocolate Chip Cookie

12. Scientists still didn’t really understand how the particles were put together in an atom.
This was a difficult question to resolve, given how tiny atoms are. They didn’t have GOOGLE to find out the answer!
Most thought it likely that the atom resembled Thomson’s model
Atomic Structure

13. Rutherford’s gold foil experiment
In 1911, Ernest Rutherford showed:
1) atoms had a hard, dense, positively charged nucleus where most of the mass resided.
2) negatively charged electrons outside the nucleus, and that the atom was actually mostly empty space.

14. Rutherford Model (not to proportion)

15. Bohr Model of the Atom
Neils Bohr put electrons into different energy levels or shells.
(This model is not correct either… electrons do not travel in orbits or paths like the model suggests)

16. Modern Day Theory (Electron Cloud Theory)
The Modern Theory suggests that electrons are located somewhere in a cloud.

17. 2) Atoms of different elements have different numbers of protons.
Basic and important facts to remember: 1) All atoms contain the same basic parts (protons, neutrons, electrons)
2) Atoms of different elements have different numbers of protons.
The Periodic Table lists atoms in consecutive order by their Atomic Number
The atomic number is directly related to the number of protons in the nucleus of each atom of that element

18. Atoms have: A nucleus small, dense part of the atom
consists of protons and neutrons
An electron cloud
large part of the atom that is empty space except for the electrons that are moving very fast and very randomly around the nucleus
Nucleus
Electron Cloud

19. The total number of protons & neutrons determines the mass of the atom
Called the “Mass Number” (atomic mass is the averaged mass of the isotopes and is given on the periodic table. Simply round the atomic mass to get the mass number)
A Carbon atom, has 6 protons and 6 neutrons, so its mass number is 12
If you know the atomic number & mass number of an atom of any element, you can determine the atom’s composition and the number of neutrons.

20. The Proton The protons are what give the atom its charge (+)
They add mass to the atom as well. Each proton is equal to one AMU (atomic mass unit)
The number of protons in an atom determines what element it is.
The atomic number signifies the number of protons
Protons are held together in the nucleus by the “Strong Force” otherwise they would repel each other.

21. The Neutron The neutron adds mass (1 amu) to an atom but has NO charge
Atoms of the same elements are identical due to the number of protons, but there can be different numbers of neutrons (we call those isotopes)
To find the number of neutrons, subtract the atomic number from the mass number.

22. Electrons
Electrons have almost no mass, and we DO NOT count their mass.
Located outside the nucleus in the electron cloud (aka: shells, orbitals, energy levels) moving at incredibly high speeds.
Electrons have a negative (-) charge.
Electrons found in the outermost shells of the atom are responsible for chemical reactions. Electrons have different amounts of energy depending what energy level they are at.
Electrons can be removed and added to atoms quite easily, unlike protons.

23. Subatomic Particles Particle Symbol Charge Relative Mass
Electron e
Proton p
Neutron n

24. Location of Subatomic Particles
10-13 cm
electrons
protons
neutrons
10-8 cm
nucleus

25. in an atom and determines what element it is
Atomic Number
Counts the number
of protons
in an atom and determines what element it is

26. Atomic Number on the Periodic Table11 Na
Atomic Number
Symbol
The symbol represents the element. RULE: The first letter is always capitalized, and IF there is a second letter, it is lower case.

27. All atoms of an element have the same number of protons11 Na
11 protons
Sodium

28. Atomic Mass on the Periodic Table11 Na
22.99
Atomic Number
Symbol
Atomic Mass
Atomic mass is the weighted average mass of all the atomic masses of the isotopes of that atom. That is why there is a decimal.

29. Mass Number Counts the number of protons and neutrons in an atom
(note: Atomic Mass is different from Mass Number. On your periodic table of elements, the atomic mass is usually given and you need to round it to the nearest whole number to use to figure Neutrons)

30. Atomic Notation atomic number 11
Shows the mass number and atomic number
Gives the symbol of the element
mass number
23 Na sodium-23
atomic number 11

31. Number of Electrons An atom is neutral when no charge is indicated.
The net charge is zero
Remember: Atomic number = Number of protons
and therefore….
Number of protons = Number of electrons when the atom is neutral.

32. Subatomic Particles Showing the P E N
O P Zn
8 p p+ 30 p+
8 e e- 30 e-
8 n 16 n 35 n

33. Isotopes
Atoms with the same number of protons, but different numbers of neutrons.
Atoms of the same element (same atomic number) with different mass numbers
Isotopes of chlorine
35Cl 37Cl
chlorine chlorine - 37

34. Learning Check
Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of these carbon atoms.
12C C 14C
#p _______ _______ _______
#e _______ _______ _______
#n _______ _______ _______

35. Solution
12C C 14C #p #e #n