Chapter 3 The Atom. HISTORY OF THE ATOM NOTES BLACK CIRCLE ACTIVITY Day One and Day Two.

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Presentation transcript:

Chapter 3 The Atom

HISTORY OF THE ATOM NOTES BLACK CIRCLE ACTIVITY Day One and Day Two

Black Circles You and your partner will be given a black circle. Within the black circle is a ball and some barrier Your job is to figure out what shape the barrier is….

The Greek Philosophers Democritus Greek Philosopher Nature must be small particles which were indivisible Aristotle Greek Philosopher Matter was continuous Table (chop forever)

John Dalton 1.Matter = particles with definite size & mass 2. All atoms that make up an element have the same mass.

John Dalton 3. Atoms of 2 different elements have different masses. 4. Atoms come together in definite ratios to form compounds. H 2 O

Thomson Studied the Cathode Ray Tubes Rays appear on phosphorescent screen when an electrical current is sent through Atoms are neutral How could the magnet affect these particles? Must be smaller positive and negative particles

J.J. Thomson

Rutherford Gold Foil Experiment What did he expect? – Majority of particles to hit straight across opening

What actually happened? Most went through Few particles hit foil and bounced back

Conclusions from the Gold Foil Experiment 1.Atom is mostly empty space 2.Mass is concentrated in the center 3.Nucleus is positive

RUTHERFORD MARBLE ACTIVITY Day Three

Rutherford: Measuring what you cannot see

LAB WRITE-UP REVIEW FOR QUIZ Day Four

Dalton 1.What is the name of his theory? 2.What are elements made of? 3.An atom of hydrogen and an atom of carbon are ________ 4.What are compounds made of?

J.J. Thomson 1.What did Thomson discover? 2.What is the charge of an electron?

Rutherford 1.What is the charge of an alpha particle? 2.Why is Rutherford’s experiment called the gold foil experiment? 3.How did he know the atom was mostly empty space?

Rutherford 4. What happened to the alpha particles as they hit the gold foil? 5. How did he know that the nucleus was positively charged?

LECTURE: NUCLIDE SYMBOLS QUIZ: HISTORY OF ATOMIC STRUCTURE Day Five

Structure of the Atom Proton – Nucleus – Positive Charged Neutron – Nucleus – Neutrally charged Electron – Outside the nucleus – Negatively charged

Nuclide Symbols Atomic Number Mass Number

Nuclide Symbol Write the nuclide symbol for a potassium atom that has 21 neutrons.

Lets Try a Few Write the Nuclide Symbols A lithium atom with 4 neutrons A sulfur atom with 15 neutrons

Assignment Page 20 – Practice Problems: Writing Nuclide Symbols First Four

LECTURE: NUCLIDE SYMBOLS & ISOTOPES Day Six

Nuclide Symbols Mass Number Atomic Number

Lets Try a Few!! Write the nuclide symbols for the following: – Copper- 64 – A Sulfur with has 17 neutrons – Potassium- 39

Isotopes Atoms of the same number of protons but different number of neutrons

Assignment Page 20 and 21

Day Seven LECTURE: NUCLIDE SYMBOLS AND IONS

Nuclide Symbols

Nuclide Symbols for Ions What is an ion? – An ion is a charged particle It could be positive or negative What does that do to the number of protons, electrons, and neutrons?

Example 40 K +1, Determine the number of protons, neutrons, and electrons.

Lets Try a Few! Determine the number of electrons, protons, and neutrons in the following: 81 Br N -3

Radioactivity Three types of Radioactivity – Alpha – Beta – Gamma

Assignment Page 22 – Complete the first table

NUCLIDE SYMBOLS/ RADIOACTIVITY PRE-LAB FLAME TEST Day Eight

Radioactivity Three types of Radioactivity – Alpha – Beta – Gamma

Example

Properties of Electrons Most of the atom’s mass is made up of ______ Most of the atom’s volume is made up of _____ Found in __________

Properties of Electrons The closer the electron is to the nucleus the less energy it has

Ground vs. Excited States Ground State Close to nucleus as possible Excited State – Electrons receive energy move farther away – Release E to drop back down to ground state (LIGHT) – Light can be seen in different colors – Elements can be identified by observing the colors it releases

Assignment Radioactivity Worksheet

FLAME TEST REVIEW FOR NUCLIDE AND RADIOACTIVITY QUIZ Day Nine

QUIZ: NUCLIDE AND RADIOACTIVITY LAB WRITE-UP Day Ten

ELECTRON CONFIGURATION Day Eleven

Locating/Mapping Electrons Energy Levels (n) – Higher the n farther away from the nucleus – More Energy Sublevels – Number of sublevels is related to the energy level – N=1 : 1 sublevel, N=2: 2 sublevels – N= 3 : ? Sublevels, N=4 : ???, N= 5: ???

Shapes and Orbitals Orbital: – Most probable location of the electrons – Each orbital can hold a maximum of 2 electrons Shapes – 4 different orbitals that have four different shapes – s, p, d, f

Lets try to summarize this: (Page 28) Sublevels (Symbol) # of orbitals # of electrons in EACH orbital TOTAL # of electrons possible in sublevel s p d f

ELECTRON CONFIGURATION Day Twelve

Lets try to summarize this: (Page 28) Sublevels (Symbol) # of orbitals # of electrons in EACH orbital TOTAL # of electrons possible in sublevel s p d f

Lets dig a little deeper: (Page 28) Energy Level (n) # of Sublev els Type of sublevels # of electrons possible in each orbital Total # of electrons possible in Energy Level

So how do we “map” out the location of the electrons? Aufbau Principle: – Electrons will always fill up an atom from lowest to highest energy CARBON

Assignment Page 29 – Oxygen, Boron, Helium, Sulfur, Magnesium

ELECTRON CONFIGURATION Day Thirteen

What about the bigger elements? Potassium

1s 2s2p 3s3p3d 4s4p4d4f 5s5p5d5f 6s6p6d6f 7s7p7d7f

Assignment Page 30 – #1-10

QUIZ: ELECTRON CONFIGURATION MODEL OF THE ATOM Day Fourteen

REVIEW FOR TEST MODEL OF THE ATOM Day Fifteen

TEST Day Sixteen