1. Atomic Structure

2. What are the 3 major parts of an atom?

3. What are the 3 major parts of an atom?
Proton
Neutron
Electron

4. Draw a diagram showing the location of each part of the atom.

5. Draw a diagram showing the location of each part of the atom.

6. Draw a diagram showing the location of each part of the atom.

7. Draw a diagram showing the charges of each part of the atom.

8. Draw a Diagram of an Atom

9. Draw a diagram showing the charges of each part of the atom.

10. Describe Proton

11. Describe Proton
Protons are positively charged particles found in the atomic nucleus. Protons were discovered by our friend Ernest Rutherford..
Experiments done in the late 1960's and early 1970's showed that protons are made from other particles called quarks.

12. Describe Neutron

13. Describe Neutron
Neutrons are uncharged particles found in the atomic nucleus. Neutrons were discovered by James Chadwick in 1932.
Experiments done in the late 1960's and early 1970's showed that neutrons are made from other particles called quarks.

14. Describe Electron

15. Describe Electron
Electrons are negatively charged particles that surround the atom's nucleus. Electrons were discovered by J. J. Thomson in 1897.
Electrons determine properties of the atom. Chemical reactions involve sharing or exchanging electrons.

16. What is the Electron Cloud Model? Diagram 1:

17. What is the Electron Cloud Model? Diagram 2:

18. What is the Electron Cloud Model?
Model of the atom pictures the electrons moving around the nucleus in a region called an electron cloud.
The electron cloud is a cloud of varying density surrounding the nucleus. The varying density shows where an electron is more or less likely to be. Atoms with electrons in higher energy levels have additional electron clouds of different shapes that also show where those electrons are likely to be.

19. Numbers used to describe Elements
Atomic Number
Mass Number
Isotopes
Atomic Mass
Ions

20. Atomic Number
Atomic number correlates to the top number you see most of the times on the periodic table
# of protons in an element’s atom’s nucleus

21. Isotope
Atoms that have the same number of protons but different numbers of neutrons
React the same as regular element, & have same amount of protons & electrons

22. Describe Isotope Example:

23. Mass Number
This is the added number of the amount of neutrons and electrons
Do not confuse this with atomic mass, which we will get to in a bit.
This is the number you see in front of an element in superscript when written
238U
This leads to isotopes

24. Atomic Mass
When atoms of an element have more or less neutrons in their nuclei, they obviously weigh differently.
Atomic mass is the average mass of an element as it occurs in nature
Scale based

25. Finding Atomic Mass
You take the amount of each isotope and multiply it by its %, then add the product
Example

26. Ions We will talk about ions more when we get into the next chapter
For now, know electrons
Makes your overall sample positive or negative – changes charge

27. Types of ions
When you add electrons to a sample of atoms– negative = anion: pronounced an ion
When you take electrons away for a sample – positive = cation: pronounced cat ion