Power Notes   Atomic Structure -Day 2
Upcoming SlideShare
Loading in...5

Like this? Share it with your network


Power Notes Atomic Structure -Day 2






Total Views
Views on SlideShare
Embed Views



2 Embeds 98

https://www.learningpoint.org 91
https://learningpoint.org 7



Upload Details

Uploaded via as Microsoft PowerPoint

Usage Rights

© All Rights Reserved

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
Post Comment
Edit your comment

Power Notes Atomic Structure -Day 2 Presentation Transcript

  • 1. Today in ScienceYou will Need:2)Pencil, Colored Pencils, Highlighters orMarkers3)Power Notes – Atomic Structure– 2 page 4sides- Picked up yesterday(Wed.)4)Signed Progress Notice– Due NOW
  • 2. Quick Writes will not be grade for points but for participation and honesty.3. You are allowed to use your brain, any notes, labs or worksheets we have done in class.4. You may not use your textbook or interactive reader.5. You will have 10 minutes to complete as many questions as possible.6. With a colored pencil, you will grade
  • 3. 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 P= 3 + N = 3 0Where is most of the mass in the NUCLEUSAtom?Where is most of the volume in the Outside the Nucleus; ElectronAtom? Cloud
  • 4. 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 atomElectron • Negatively charged subatomic particle • Found outside the nucleus in the electron cloud • Smallest particle; mass = 1/1836th of the atom
  • 5. 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 Numberhttp://www.sawyerscience.com/Units/unit2/atoms_compounds.html
  • 6. All atoms found on the • Neutral – same # of protons(+) andPeriodic Table are # of electrons(-)Isotope • Atoms of the same element with same number of protons and different number of neutrons. nucleus nucleus ProtonHydrogen has 3 naturaloccurring ISOTOPES:Protium, Deuterium and Protium nucleus DeuteriumTritium are Neutro All ROGEN have n l HYD use al Tritium a bec oton. r 1 p
  • 7. 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 electronsIONS they become charged. (number of protons (+) and electrons (-) particles are NOT EQUAL)REVIEW & REFLECT + -
  • 8. Coloring the Periodic • Outline each box in the followingTable way: 3. Metalloids – in BLUE 4. Nonmetals – in ORANGE*Textbook pg 196-197 – Use the 5. Metals – in GREENkey
  • 9. Homework 1)Power Notes– Due Monday –Date Change (There is time to work in class tomorrow)Do You see HOW the periodic tableand the Atomic Structure areRELATED?