Atom Booklet
- 1. Today in Science You will Need: 1)Pencil, Colored Pencils, Highlighters or Markers 2)Atom Booklet Directions– 1 page 2 sides- Bookshelf 3)4 pieces of white unlined paper– Bookshelf
- 2. Reminder 1)Update Log #3 2)End of Quarter is this Wednesday– if you have missing assignments you want to turn in they must be turned in by Wed. 3)Test #2 Corrections + Parent Signature – Due Wednesday
- 3. 1) Materials Managers – Pick up a stapler from front table. 2) Folding and Stapling the Book 3) Label pages according to Sample Booklet 4) Page six Element = DO NOT CHOOSE Platinum 5) Page six and seven need CHARTS – can be done as “T” Tables
- 4. Topic: Atom Booklet Information Do we understand everything????
- 5. Democritus 400 BC • 1st idea of “atoms” Greece - stated that all matter is made up • Believed all matter is made of atoms. He also stated that atoms are up of tiny particles separated eternal and invisible and so small that they can’t be divided, by space and they entirely fill up the space they’re • Named particles “atomos” in which means indivisible. Lavoisier 1789 • Founder of modern chemistry France - provided the formula for the conservation of matter • 1st carefully controlled in chemical reactions, and also distinguished experiments providing between an element and a compound evidence to the Law of Conservation of Mass
- 6. Dalton 1766-1844 1st MODERN Atomic Theory (pg 165) 1.All matter made up of tiny England - formed the 1st atomic theory, which states that all matter is composed of indivisible particles called atoms tiny, indestructible particles called atoms that are all alike and have the same atomic weight. 2.Atoms of the same element have identical properties 3.Atoms of different elements have different properties 4.Atoms combine in a specific ratio to form compounds 5.A specific compound is always made up of atoms in a specific proportion.
- 7. Thomson 1897 Plum Pudding Model (pg 166) 1.Negative particles scrambled into the “dough” of the positive particles. England - discovered the electron and developed the plum- pudding model of the atom. Rutherford 1898 Gold Foil Experiment (pg 167) England - used the results of his gold-foil experiment to state that 1.Atoms are mostly empty space all the mass of an atom was in a small 2.All the Mass of an atom is in the positively-charged ball at the center of positively charged ball in the the atom. center of the structure.
- 8. Bohr 1922 Denmark - stated that “Planetary” atom model (pg 169) the electrons moved 1.Believed the atom structure was like our around the nucleus in successively large solar system: nucleus in the middle like orbits. He also presented the Bohr the sun and the electrons orbiting like the atomic model which planets. stated that atoms absorb or emit radiation only when the electrons abruptly jump between allowed, or stationary, states. Schrödinger (Schroedinger ) Wave Mechanic Model 1930 Austria - introduced the Shroedinger Equation, a 1.Planetary model was too specific wave equation that describes the form of the 2.Rather: electrons vibrate around the probability waves that govern the motion of outside of the nucleus- can only small particles and how these waves are altered predict where they are most like to be by external influences. 3.QUARKS – protons, neutrons and electrons made up of some of these smaller particles. 4.http://library.thinkquest.org/05aug/01087/quarks.html
- 9. Basic Atomic Structure Today scientists agree on the three basic subatomic particles that make up all atoms. Bohr Model for Lithium (not to scale) Electron = 3 (pg 172) P= 3 + N = 3 0 Where is most of the mass in the NUCLEUS Atom? Where is most of the volume in the Outside the Nucleus; Electron Atom? Cloud
- 10. Nucleus • Contains protons(+) and Neutrons (0) • Holds most of the mass of the atom • Very small compared to the entire size of the atom • Most dense part of the atom Electron • Negatively charged subatomic particle • Found outside the nucleus in the electron cloud • Smallest particle; mass = 1/1836th of the atom
- 11. Proton • Positively charged subatomic particle • Found in the nucleus • Mass = 1 amu (atomic mass unit) • # of protons in an atom IDENTIFIES the atom (which element) • # of protons in the nucleus of an atom called the atomic number Neutron • Zero charge • Mass = 1 amu • Do NOT affect the identity of the atom • Found in the nucleus • Same atom of an element can have varying amounts of neutrons (isotope) • Adding the total number of protons & neutrons = Atomic Mass Number http://www.sawyerscience.com/Units/unit2/atoms_compounds.html
- 12. All atoms found on the • Neutral – same # of protons(+) and Periodic Table are # of electrons(-) Isotope • Atoms of the same element with (pg 176) same number of protons and different number of neutrons. nucleus nucleus Proton Hydrogen has 3 natural occurring ISOTOPES: Protiu nucleus Deuteriu Protium, Deuterium and m m Tritium are Neutro All ROGEN have n l HYD use al Tritium a bec oton. r 1p
- 13. Atomic MASS • On the Periodic Table represents a weighted average of the mass of all naturally occurring isotopes of each element. (based on mass and abundance of each isotope). • When atoms gain or lose electrons IONS they become charged. (number of protons (+) and electrons (-) particles are NOT EQUAL)
- 14. How do we know if an element is a metal, 1. Metalloids – are in green boxes nonmetal or metalloid? 2. Nonmetals – are in yellow boxes 3. Metals – are in blue boxes Look on pg. 196-197 Go to the Hyperlink in Learning How can I find the Bohr Point for this week. Model for my Element? It should read BOHR MODEL and have a picture of a globe next to it.
- 15. Homework 1)Atom Booklet– Due by Thursday at the end of class 2)Test #2 Corrected & Signed by Parents on the Front – Due Wednesday Have you noticed HOW the periodic table and the Atomic Structure are RELATED?