1. Introduction to Atoms Chapter 11 Material on Midterm

2. Where is it? How do we get information about items that we cannot see?

3. Section 1: Development of the Atomic Theory Objectives Describe some of the experiments that led to the current atomic theory Compare the different models of the atom Explain how the atomic theory has changed as scientists have discovered new information about the atom

4. Section 1: Development of the Atomic Theory The Beginning of Atomic Theory Democritus The particle that was so small it could not be ______ again The _______ Is the smallest particle into which an element can be divided and still be the same substance Means not able to be divided

5. Section 1: Development of the Atomic Theory The Beginning of Atomic Theory Democritus Challenged by _____________ Most believed him (even though he was wrong!)

6. Section 1: Development of the Atomic Theory Dalton’s Atomic Theory Based on Experiments Figured out that compounds are made of ___________ that are made of single ___________made of

7. Section 1: Development of the Atomic Theory Dalton’s Atomic Theory Based on Experiments Had three parts 1.All substances are made of ________. Atoms are small particles that cannot be created, divided, or destroyed 2.Atoms of the same element are exactly alike, and atoms of different elements are _____________ 3.Atoms join with other atoms to make _________ substances

8. Section 1: Development of the Atomic Theory

9. Thomson’s Discovery of Electrons Thomson used a device called a _______________ Determined that there are _________ particles inside of an atom

10. Section 1: Development of the Atomic Theory

11. _____________ are subatomic particles that have a negative charge Thomson created the _______ _________ model to show where the electrons go

12. Section 1: Development of the Atomic Theory Rutherford’s Atomic “Shooting Gallery” Rutherford wanted to test Thomson’s idea Had a sheet of gold foil (SUPER THIN) Had a detector on the outside Shot a beam of positive particles at it What he expected: all of the particles would just go ____________ _______________

13. Section 1: Development of the Atomic Theory

14. Rutherford’s Atomic “Shooting Gallery” What really happened Most went straight through (like he thought) Some got ________ at an angle A few bounced right back! “It was quite the most incredible event that has ever happened to me in my life. It was almost as if you fired a fifteen-inch shell into a piece of tissue paper and it came right back to you”

15. Section 1: Development of the Atomic Theory Where are the Electrons? Plum-pudding model was ______________! Rutherford realized that atoms were mostly ________ ______________mostly At the center is the _______________ The nucleus is an atom’s central region, which is made up of protons and neutrons __________ move around it

16. Section 1: Development of the Atomic Theory Bohr’s Electron Levels Bohr figured out electrons move around in ________ Like rungs on a ladder

17. Section 1: Development of the Atomic Theory Modern Atomic Theory …it’s complicatedcomplicated Schrodinger & Heisenberg and others helped Electrons ______ _______ move in paths that are very clear We cannot predict where electrons are ______ We’re likely to find them in electron _____, which are regions around the nucleus where electrons are likely to be found

18. Section 1: Development of the Atomic Theory Section Summary Please answer the objectives on your objective summary sheet 1.Describe some of the experiments that led to the current atomic theory 2.Compare the different models of the atom 3.Explain how the atomic theory has changed as scientists have discovered new information about the atom

19. Section 2: The Atom Objectives Describe the size of an atom Name and state information about the parts of an atom Describe the relationship between number of protons and neutrons and atomic number State how isotopes differ Describe and calculate atomic masses Describe the forces within an atom

20. Section 2: The Atom How small is an atom?

21. Section 2: The Atom 1 aluminum atom has a diameter of ___________________ cm How many atoms thick was our foil from chapter 1?

22. Section 2: The Atom What is an Atom made of? 3 major parts The ________ is the subatomic particle that has a positive charge and that is found in the nucleus of an atom The __________ is the subatomic particle that has no charge and that is found in the nucleus of an atom The _________ is the subatomic particle that has a negative charge and that is found in the electron cloud surrounding the atom

23. Section 2: The Atom

24. How big are these pieces VERY SMALL! Scientists came up with a special term for them The atomic mass unit is a unit of ____ the describes the mass of an atom or molecule Proton: ~1 amu Neutron: ~1amu Electron: ~_______________ amu

25. Section 2: The Atom An atom is normally _____________ Same number of protons and ___________ If an atom changes this ratio, it becomes an _________

26. Section 2: The Atom How do Atoms of Different Elements Differ? The atomic number is the number of _________ in the nucleus of an atom; the atomic number is the same for all atoms of an element An ________ is an atom that has the same number of protons/atomic number as other atoms of the same element but has a different number of neutrons (and this a different atomic mass) The __________ number is the sum of the protons and neutrons in an atom

27. Section 2: The Atom Subatomic particleLocationChargeKey feature ProtonNucleus__________________ ___________ ________NucleusNeutralIsotopes ElectronElectron cloud__________Charge

29. Section 2: The Atom Let’s do some practice! An atom has a mass number of 7. It’s atomic number is 3. What is… The number of protons? The number of neutrons? The number of electrons? The name of the element?

31. Section 2: The Atom Let’s do some practice! An atom has a mass number of 32. It’s atomic number is 16. What is… The number of protons? The number of neutrons? The number of electrons? The name of the element?

32. Section 2: The Atom Let’s do some practice! An atom has a mass number of 1. It’s atomic number is 1. What is… The number of protons? The number of neutrons? The number of electrons? The name of the element?

33. Section 2: The Atom Boron-10 5 protons 5 neutrons 5 electrons Atomic number: Mass number: Boron-11 5 protons 6 neutrons 5 electrons Atomic number: Mass number: Naming isotopes Remember, they are the SAME ELEMENT but differ in neutron number

34. Section 2: The Atom Calculating the mass of an element The atomic mass is not really a whole number The atomic mass is the mass of an atom expressed in __________ _________ ________ Hydrogen has an atomic mass of _______________ Where does this number come from?

35. Section 2: The Atom Calculating the Mass of an Element The atomic mass is a weighted average of the masses of all naturally occurring __________ of the element Takes into account that not all isotopes are found equally on earth

36. Section 2: The Atom Calculating the mass of an element There are two different isotopes of copper Copper-63 (69% of earth’s copper is this type) Copper-65 (31% of earth’s copper is this type Steps 1.Convert percentages into decimals 2.Multiple decimal value by atomic mass 3.Add these amounts together to find the mass

37. Section 2: The Atom Calculating the mass of an element There are two different isotopes of copper Copper-63 (69% of earth’s copper is this type) Copper-65 (31% of earth’s copper is this type Steps 1.Convert percentages into decimals 69%  0.69 31%  0.31

38. Section 2: The Atom Calculating the mass of an element There are two different isotopes of copper Copper-63 (69% of earth’s copper is this type) Copper-65 (31% of earth’s copper is this type Steps 2.Multiple decimal value by atomic mass (0.69 x 63) = 43.47 (0.31 x 65) = 20.15

39. Section 2: The Atom Calculating the mass of an element There are two different isotopes of copper Copper-63 (69% of earth’s copper is this type) Copper-65 (31% of earth’s copper is this type Steps 3.Add these amounts together to find the mass (43.47 + 20.15) = 63.62 amu

40. Section 2: The Atom You try! There are two different isotopes of chlorine Chlorine-35 (76% of earth’s chlorine is this type) Chlorine-37 (24% of earth’s chlorine is this type Steps 1.Convert percentages into decimals 2.Multiple decimal value by atomic mass 3.Add these amounts together to find the mass

41. Section 2: The Atom Forces in Atoms Four basic forces that are working even inside teeny atoms! ______________ __________ Strong Force Weak Force

43. Section 2: The Atom Section Summary Please answer the objectives on your objective summary sheet 1.Describe the size of an atom 2.Name and state information about the parts of an atom 3.Describe the relationship between number of protons and neutrons and atomic number 4.State how isotopes differ 5.Describe and calculate atomic masses 6.Describe the forces within an atom