1. What do I study for the Chapter 11 Test on ?
Use your study guide, Ian, and blog resources

2. John Dalton and Joseph Thomson
Be able to list the Scientists and explain the scientist who have contributed to the development of Atomic Theory
John Dalton and Joseph Thomson
Dalton:
Stated that atoms were made up of tiny indivisible particles known as atoms.
Felt that compounds contained different types of atoms in definite ratios.
Most simple model and Did Not contain subatomic particles.
Thomson:
Created the Plum Pudding Model. He ran electricity through a cathode ray tube and saw a beam of particles. The rays were attracted to a positively charged object- bending toward the positively charged object. This was the first model with subatomic particles. These particles became known as electrons. The model displayed a solid sphere with scattered electrons.

3. Chapter 11 Section 1: Development of the Atomic Theory
Be able to list the Scientists and explain the scientist who have contributed to the development of Atomic Theory
Who is Rutherford?
Rutherford- Used the Gold Foil Experiment to prove that atoms were less dense that previously thought. He also proved there was a dense positive nucleus. His model shows us that the nucleus is in the center of the atom with electrons surrounding it.

4. What did Bohr do?
Bohr did not perform a specific experiment. His planetary model displayed an atom with specific orbital paths for the electrons. It also had different energy levels and protons made up the nucleus. Remember: you can only have up to 2 electrons( no more) in the first energy level, up to 8 ( no more) in the second level, and 18 ( no more) in the third level.

5. What is the difference between Bohr’s Model and Schrodinger’s Model of the atom?
Bohr felt that the atom did have specific orbital paths for the electrons as well as different energy levels.
In the Bohr model, the protons make up the nucleus.
Schrodinger stated that electrons were displayed in orbital regions but they did not follow any specific path or any certain position. Called his model Electron Cloud Model
Schrodinger’s electron cloud model displayed protons and neutrons in the nucleus.

6. Chapter 11 Section 2: Atomic Structure of the Atom
What is an Atom made of?
Matter is anything with Mass that takes up Space.
All matter is composed of small, fast moving particles called Atoms. Atoms can join together to form Molecules.
The atom is composed of subatomic particles that include the following:
Protons- have a POSITIVE charge and are found in the nucleus.
Neutrons- are also in the nucleus but have NO Charge!
Electrons- have a Negative charge and are found within the electron cloud that orbits the nucleus.
Remember: Electrons in the outer shells can move. All electrons in the outer shell are called VALENCE Electrons.
Normally in an atom the number of electrons within the electron cloud is equal to the number of protons in the nucleus. The positive and negative charges cancel each other out. Therefore, the atom is said to be electrically neutral. .

7. What Exactly is an ION?
  Valence Electrons can move on or off atoms.
Atoms can gain or lose electrons in the outer shell. Then they have a charge and are no longer neutral—the atom is now an ION
This gaining or losing of electrons happens when atoms form molecules

8. How can Atoms of the same type differ
How can Atoms of the same type differ? Atoms of the same element can be different from each other.
Atoms with the same number of protons and differing numbers of neutrons care called ISOTOPES
Proton number does not change!!!!!!!!!
The three naturally-occurring isotopes of hydrogen. The fact that each isotope has one proton makes them all variants of hydrogen: the identity of the isotope is given by the number of neutrons. From left to right, the isotopes are protium (1H) with zero neutrons, deuterium (2H) with one neutron, and tritium (3H) with two neutrons.

9. How do I find Atomic Number and Atomic Mass?
Atomic number is the NUMBER OF PROTONS
The atomic number of an atom is the same as the number of protons it has. For example, hydrogen has one proton and is atomic number 1. Each helium atom has two protons, so the element is atomic number 2. Simple, right?
Atomic Mass—average mass for all atoms including isotopes
Atomic Mass is the larger number on the cube—usually in decimal form. Round that number to find the MASS NUMBER which is also the number of protons and neutrons in an atom.
Protons and Neutrons have about the same mass each =1amu

10. Explain the forces in an Atom