1. Ms. Pici 2016-2017, Iroquois Central Schools
Atomic Structure
Ms. Pici , Iroquois Central Schools

2. Objectives
Students will explain that atoms are the smallest unit of an element and are composed of subatomic particles.
Students will analyze models of the scientific theory of atoms.
Students will analyze models and describe the motion of particles in solids, liquids, and/or gasses.

3.
Pick up bill Nye video sheet
Hand out tests to see grade we will go over after everyone has taken them 9th period
IF YOU WERE ABSENT FRIDAY YOU MUST TAKE YOUR UNIT TEST 9TH PERIOD TODAY NO EXCEPTIONS
White board: What do you think an atom looks like? What is it made of? What do atoms make up? Explain this through a rap, picture, or through written expression.

4. Atoms….What are they anyway???
On your white board with your partner, brainstorm what you think an atom is. Feel free to draw a picture, write a song, or anything that allows you to express your ideas!
Essential Questions: How and why has the Atomic Theory changed over time? How can we describe the molecular motion of the states of matter?

5. Bill Nye Video- Atoms
Pick up and fill out the worksheet while watching the Bill Nye video.

6. 1-18-17 Take out bill nye video Pick up worksheets
Due date for collage is next Tuesday, !!!!

7. How small are atoms?

8. 1-19-17 Take out homework to be checked and we will go over
Get into your collage groups take out your sheet for the collage
Homework is tweet #15

9.
Work on scientist collage

10. Atoms
Matter is anything that takes up space and has mass. All matter is made of atoms.
Atoms are the basic building blocks of matter. They make up everything around us; Your desk, the board, your body, everything is made of atoms!
Atoms are too small to see without powerful microscopes.

11. Atomic Structure
There are two basic components in every atom: Electron Cloud Nucleus

12. Atomic Theory
Because we can not see atoms, we use models to teach and learn about atoms.
The atomic theory has changed over time as new technologies have become available.
Remember: Scientific knowledge builds on past research and experimentation.

13. Atomic Theory Timeline
Scientist
Information
Model
Democritus
From:
(Greece)
-make up everything
-”small invisible” –”atomos”

14. Atomic Theory Timeline
Scientist
Information
Model
John Dalton
From:
England
All matter is made of atoms. Atoms are too small to see, indivisible and indestructible. All atoms of a given element are identical. Can be combined

15. Atomic Theory Timeline
Scientist
Information
Model
J.J Thompson
From: England
Discovered the negative electron, and predicted that there also must be a positive particle to hold the electrons in place.
Discovered the electron cathode ray

16. Atomic Theory Timeline
Scientist
Information
Model
Ernest Rutherford
From: New Zealand
Discovered the nucleus of an atom and named the positive particles in the nucleus “protons”. Concluded that electrons are scattered in empty space around the nucleus.
Golf foil

17. Atomic Theory Timeline
Scientist
Information
Model
Niels Bohr
From: Denmark
Electrons orbit the nucleus in definite paths and around the nucleus
Neutrons

18. Atomic Theory Timeline
Scientist
Information
Model
Neils Bohr
Concluded that electrons are located in planet-like orbits around the nucleus in certain energy levels.

19. Scientist Information Model
(Many Scientists!)
The Modern Atomic Theory
Erwin Schrodinger
Electrons do not orbit the nucleus in neat planet-like orbits but move at high speeds in an electron cloud around the nucleus.

20. Think-Pair-Share!
Take a minute to read the essential question as I read it aloud: “How and why has the Atomic Theory changed over time?” After you have jotted down your notes in the space on your guided notes, exchange your thoughts with your partner. We will have share- outs and discuss the answer.

21. Subatomic Particles Three subatomic particles make up every atom:
Charge
Location
Proton
Positive (+)
Nucleus or “Core”
Neutron
No Charge (0)
Electron
Negative (-)
Electron Cloud

22. Subatomic Particles Electron Cloud: Electrons orbit the nucleus.
Nucleus or “Core”:
Protons and Neutrons are found in the nucleus.

23.
Additional video resource:

24. number of electrons = number of protons
ATOMIC STRUCTURE 4
Atomic mass He
the number of protons and
neutrons in an atom
Symbol (1 or 2 letters), first letter is always capital 2
Atomic number
the number of protons in an atom
number of electrons = number of protons

25. The mass number tells you….
Protons and neutrons
Can find it because …..
Larger in volume (value)

26. The atomic number tells you…
Protons and electrons
Can find it because….
Smaller in value

27. Symbol tells you….
Element name
Can find it because of
Letters

28. Other important info…
In a neutral atom, the number of protons (+) is equal to the number of electrons (-).
The number of neutrons is found by using the formula mass #- Atomic number= # of neutron s

29. Practice 32 S 16

30. Practice PRACTICE ATOMIC NUMBER = 16 MASS NUMBER = 32
PROTONS = 16 ELECTRONS = 16
NEUTRONS = 16 (SHOW WORK) 32 S 16

31. Using the periodic table

41. How to determine an isotope

43. Carbon 12

44. Carbon 12 ATOMIC NUMBER = 6 MASS NUMBER = 12 PROTONS = 6 ELECTRONS = 6
NEUTRONS = 6

45. Carbon 14

46. Carbon 14 ATOMIC NUMBER = 6 MASS NUMBER = 14 PROTONS = 6 ELECTRONS = 6
NEUTRONS = 8

47. What element is this? Carbon (C)
How do you know? Because the atomic number is 6.
What qualities are the same for both diagrams? Atomic number, protons, electrons
What qualities are different in the diagrams? Neutrons and mass number

48. DEFINE ISOTOPE: An atom of the same element with a different mass number (# of neutrons).
Name an isotope and tell what it is used for. Carbon 14 is used to date fossils (Dead stuff).

49. (Tritium is released during nuclear weapons tests.)
DRAW THE ATOMIC STRUCTURE FOR HYDROGEN, THEN DRAW ITS
ISOTOPE TRITIUM WITH A MASS # OF 3.
(Tritium is released during nuclear weapons tests.)

50. Hydrogen

51. Tritium

52. Energy Levels DEFINE ENERGY LEVEL: A place where electrons are found.
Give 4 synonyms for energy level: orbits clouds
rings shells
Each energy level can only hold a certain number of electrons before it becomes full.
The rule is to use the formula 2N², where N is the number of the level.

53. ENERGY
LEVEL #
2N²
MAXIMUM # OF ELECTRONS 1
2(1)² 2
2(2)² 8 3
2(3)² 18 4
2(4)² 32 5
2(5)² 50

54. K
a# = 19
m# = 39
p = 19
e- = 19
n = 20 Ca
a# = 20
m# = 40
p = 20
e- = 20 Na
a# = 11
m# = 23
p = 11
e- = 11
n = 12
Dot Diagram:
1. look at valence (outermost) shell
2. Draw symbol
3. Draw dots to equal valence electrons
around to represent a clock.