1. Atomic Structure

2. To discuss the evolution of the atomic model
Aim 1
To discuss the evolution of the atomic model

3. basic building block of matter/single unit of an element
Atom
basic building block of matter/single unit of an element
cannot be broken down chemically

4. Dalton (1808)- Father of the atomic theory
All matter is made up of small particles called atoms
2. Atoms of the same element are identical

5. 3. Atoms of different elements are different 4
3. Atoms of different elements are different 4. Atoms cannot be broken down

6. 5. Atoms of different elements combine in simple whole-number ratios to form chemical compounds
6. In chemical reactions, atoms are rearranged (combined OR separated)

7. ****CANNONBALL THEORY/MODEL****
Representation
****CANNONBALL THEORY/MODEL****

8. Thomson
1. Discovered SUBATOMIC PARTICLE called the ELECTRON 2. Concluded that electrons are SMALL and NEGATIVELY CHARGED

9. **** PLUM PUDDING THEORY/MODEL****
Representation
**** PLUM PUDDING THEORY/MODEL****

10. Video

11. Rutherford
Conducted the GOLD FOIL EXPERIMENT where he BOMBARDED a thin piece of GOLD FOIL with POSITIVE PARTICLES

12. 2. Expected all particles to pass straight through foil
2. Expected all particles to pass straight through foil. Most passed through, but some were severely deflected.

13. 3. He concluded that because most of the atoms went through that the atom was MOSTLY EMPTY SPACE and that because some of them were deflected, that the atom has a DENSE, POSITIVELY CHARGED CENTER called the nucleus!

14. Diagram of Experiment

15. LED TO…
****** NUCLEAR THEORY/MODEL******

16. NEILS BOHR (1913) Bohring!
Electrons travel AROUND the nucleus in well-defined (FIXED) paths called ORBITS
Each electron has a unique amount of energy: higher # shell=more energy. This is its fingerprint.

17. Representation

18. Wave-Mechanical/Cloud Model
Electrons have distinct amounts of energy and move in areas called ORBITALS
MANY SCIENTISTS have contributed to this theory

19. Orbitals
an area of HIGH PROBABILITY for finding an ELECTRON (not a circular path)
Electrons DO NOT TRAVEL IN FIXED PATHS

20. Representation: Generally called Fuzzy Cloud

21. To understand the vocabulary of the periodic table!
Aim 2
To understand the vocabulary of the periodic table!

22. VOCABULARY (OF THE PERIODIC TABLE)
Element Symbol = the letter(s) used to
identify an element
Only one letter will be capitalized

23. Atomic # = the number
of protons in EVERY
ATOM of the element
NEVER CHANGES!!!

24. Atomic Mass = AVG.
mass of all the isotopes
of an element

25. Electron configuration = number of
Oxidation #’s = possible
charges an atom of an
element can have
Electron configuration = number of
electrons in each energy level; add the
numbers to get the total # of electrons

27. Subatomic Particles Subatomic Particle Charge Relative Mass Location
Symbol
How to Calculate
Proton
Neutron
Electron

28. Practice Symbol Protons Neutrons Electrons Atomic Number Mass Number
Nuclear Symbol
Cl-35
C-12
Ar-40
O-16

29. Aim 3
To calculate the average atomic mass using all isotopes of a given element

30. Isotopes?
ISOTOPE = atoms of the same element with different mass #’s; same atomic #

31. Nuclide: a way to express an isotope
Nuclide: a way to express an isotope. It must include the identity of the element AND MASS Examples: Carbon-14 OR 14 C 6

32. EXAMPLE 1: ISOTOPES OF CARBON (C-12, C-13, & C-14)

33. EXAMPLE 2: ISOTOPES OF URANIUM (U-238, U-240)

34. Aim 4
To draw Bohr diagrams to represent the size of an atom and to locate electrons

35. bohr
BOHR DIAGRAMS (one method for expressing electron location in an atom or ion); ALL ELECTRONS MUST be drawn  BOHRing

36. practice

37. The last number in the electron configuration
Valence electrons
Valence electrons are electrons found in the outermost shell or orbital of an atom
The last number in the electron configuration

38. Inner electrons (all non valence electrons)
Kernel electrons
Inner electrons (all non valence electrons)

39. Practice
Chlorine Nitrogen Potassium Sodium

40. To draw electron dot diagrams to predict behaviors of an atom.
Aim 5
To draw electron dot diagrams to predict behaviors of an atom.

41. Lewis (Electron) dot diagrams
Lewis Electron Dot Diagrams: Only illustrate VALENCE ELECTRON CONFIGURATION

42. rules
1. Write the element’s symbol 2. Retrieve electron configuration from Periodic Table. The last number in the configuration is the NUMBER OF VALENCE ELECTRONS

43. Aim 6
To differentiate between atoms and ions in order to determine the chemical properties of matter.

44. ATOMS (NEUTRAL) VS. IONS (CHARGED)
Vocabulary Term
Definition
Example/Diagram
Atom
Ion (aNion)
Ion (ca+ion)