Upload
thomas-gaines
View
222
Download
2
Embed Size (px)
Citation preview
Honors ChemistryChapter 3
Atomic Structure
I. Dalton’s TheoryPart 1 - elements are composed of tiny particles
called atoms.
Part 2 - Atoms from the same element are identical.
Part 3 - Atoms are neither created nor destroyed in a chemical reaction.
(just a new order with new bonds)
Part 4 - A given compound has the same relative numbers and kinds of atoms.
*water is always H2O
II. Discovering Atomic StructureA. Faraday (1839)
1. -atoms contain particles that have electrical charges
B. Franklin
1. Tests electricity
And proved that…
III. The ElectronA. Cathode Ray Tube JJ Thomson (1896)
- Led to the discovery of the electron and itsbasic charge.
B. Millikan (1909)
1. Determined the charge and mass of a single electron.
2. 1 electron = 2000 times lighter than an H atom
IV. The Proton and NucleusA. Gold Foil Experiment (Rutherford 1909)
-determined nucleus (positive charge)
Assign: 3.1• Read 3.3 and draw a picture of Cl-35 and Cl-
37 with the correct number of protons, electrons, and neutrons.
V. Structure of the Atom
Particle Type Charge Relative Mass
Electron (cloud) 1- 0
Proton (nucleus) 1+ 1
Neutron (nucleus) 0 1
VI. Terminology and the P.T.
A. Atomic Number - # of protons in an atoms
1. top number
2. gives clue to the number of electrons
B. Mass Number – the # of protons and neutrons
1. always rounded
C. Ions – atom that has gained or lost electron(s)
1. Ex: Ca 20
Ca2+ ___
2. Can be positive or negative18
D. Isotopes – atoms that have different numbers of neutrons.
1. or… H-1, H-2, H-3
E. Atomic Mass – the average of all isotopes of a certain element.
Element Symbol Atomic # Mass ## of
electrons# of
neutrons# of
protons
Carbon
13
65
Fe3+
O2-
10 12
32 18
8 6
C 6 12 6 6 6
Aluminum Al 27 13 14 13