Chapter 4 – Chemical Foundations: Elements, Atoms, and Ions
General Chapter Outline
Elements & Symbols
Dalton’s Atomic Theory
Law of Constant Composition
Law of Conservation of Matter
Formulas of Compounds
Atomic Structure
 Protons
 Neutrons
 Electrons
 Nucleus
 Atomic Number (Z)
 Mass Number (A)
JJ Thompson
William Thompson
Gold Foil Experiment – Rutherford
Isotopes (Names, Symbols, Percent Abundance Problems)
Periodic Table
Metals
Nonmetals
Metalloids
Alkali Metals
Alkaline Earth Metals
Transition Metals
Inner Transition Metals: Lanthanide Series, Actinide Series
Halogens
Noble gases
Natural States of the Elements
 Diatomic Elements (H, O, Cl, Br, F, I, N)
Allotropes
Ions
 Cation
 Anion
 Monatomic Ions
 Polyatomic Ions (the BIG 5)
 Trends on the Periodic Table
Ionic Compounds
 Electrolytes (when molten or dissolved in water)
 High Melting and Boiling Points
Textbook Homework Problems: (1, 2, 9, 10, 19, 21, 22, 24, 25, 29, 35, 37, 39,
45, 47, 51, 53, 63, 64, 67, 69, 73, 75, 77, 83)
Questions and Problems
1) Know the symbols and proper spellings for the elements on your list.
2) Outline how the atomic theory has progressed since the time of the early Greek
philosophers. Be sure to include Dalton’s Atomic Theory, the Plum Pudding
Model, and Rutherford’s Gold Foil Experiment.
3) What are the three subatomic particles? Indicate the relative charge and relative
mass of each of these particles. Where are each located within an atom? What
purpose does each particle serve?
4) What are isotopes?
5) Define atomic number and mass number?
6) How many protons, neutrons and electrons are in each of the following
atoms/ions?
a) Calcium – 41
b) Tin – 119
c) 50Cr2+
d) 79Br17) Naturally occurring sulfur has an average atomic mass of 32.066amu and
consists of two isotopes, 32S and 34S. If their respective atomic masses are
31.972amu and 33.968amu, calculate the relative abundance of each isotope.
8) Describe the periodic table of elements.
a) How are the elements arranged in the table?
b) Why are the elements are arranged into vertical groups?
c) What general area contains the metallic elements? Nonmetallic elements?
d) Give the locations of the following: noble gases, transition metals, alkali
metals, lanthanide series, alkaline earth metals, halogens, nonmetals,
actinide series, metals, representative elements, metalloids, inner-transition
metals, and the staircase line.
9) List the physical properties of metals and nonmetals.
10) Define: ion, cation, anion, monatomic ion, polyatomic ion
11) How is a cation formed? How is an anion formed?
12) Does the nucleus change when an atom is converted to an ion? Explain.
13) How is the periodic table used to predict what ion an element’s atoms will form?
14) Write formulas for the ionic compounds that will form between the following
pairs of elements.
a) lithium and oxygen
______________
b) magnesium and nitrogen
______________
c) aluminum and bromine
______________
d) calcium and sulfur
______________
15) Write names for the following ionic compounds.
a) KF
_______________________________
b) Ba3P2
_______________________________
c) Na2S
_______________________________
d) SrI2
_______________________________
16) List three properties that are representative of ionic compounds.
17) List the seven diatomic elements.
BONUS: List the BIG 5 polyatomic ions (names and formulas)