Lentz/Wolfe
Chapter 3 Guided Notes
Symbols for the Elements (3.2)
ElementCan be broken down into:
# Naturally Occurring Elements:
# Man-Made Elements:
Element names come from:
Element Symbols:
First letter:
Second letter:
Dalton’s Atomic Theory (3.3)
Dalton, John:
Dalton’s Theory explains:
1.
2.
3.
4.
5.
Formulas of Compounds (3.4)
CompoundCompounds ALWAYS contain:
Chemical Formula:
Chemical formulas include:
Rules for writing Formulas:
1.
2.
3.
Structure of the Atom (3.5)
Thomson’s Experiment:
This experiment identified:
Thomson also knew:
Thomson, William:
Plum Pudding Model: atom thought of as
Pudding is _____charge
Electrons _____charge
Rutherford, Ernest:
Rutherford’s Experiment:
Main Area of Interest:
Rutherford’s Conclusions:
Nuclear Atom
Nucleus
Proton
Neutron
Introduction to the Modern Concept of Atomic Structure (3.6)
What has been learned since then?
Nucleus:
Protons:
Electrons:
Isotopes (3.7)
Isotope:
Atomic Number:
Mass Number:
Introduction to the Periodic Table (3.8)
Periodic Table:
8
O
Oxygen
16.00
Arranged:
Groups:
Alkali Metals
Alkaline earth Metals:
Halogens
Noble Gases
Transition Metals
Metals
Nonmetals
Metalloids
Semimetals
Natural States of the Elements (3.9)
Most elements are:
This means:
Diatomic Molecules:
Some elements that form diatomic molecules:
Allotropes
Ions (3.10)
Ion:
Produced when:
*Ions are never formed by:
Cation:
Produced when:
How named?
Anion:
Produced when:
Ion charges and the Periodic Table (color and label appropriately)
Compounds that Contain Ions (3.11)
Chemists think that Chemical compounds contain ions because:
NaCl example:
Ionic Compounds:
Must have a net charge of _____
If a compound contains ions, then:
1.
2.