1. Chapter 3 Atoms and Elements

2. Understanding the Macroscopic World
The connection between the microscopic atom and the macroscopic element is the key to understanding the chemical world.

3. Atoms An atom is the smallest identifiable unit of an element.
Similarities and differences on the atomic scale correlate with similarities and differences on the macroscopic scale.

4. Atoms

5. Protons Determine the Element
The atomic number, Z, represents the number of protons in the nucleus of an atom.
The charge of a proton is assigned numerical value of +1.
Protons constitute a significant part of the mass of an atom.
Mass of a proton is 1.0 amu

6. Chemical Symbols
Symbols are an abbreviation of the chemical name which can be based on:
The English name for the element: hydrogen  H
The Greek or Latin name: ferrum (iron)  Fe
Their place of discovery: europium  Eu
The scientist honored by the naming: curium  Cm

7. Periodic Table of Elements

8. Electrons
A neutral atom has as many electrons outside its nucleus as protons within its nucleus.
The opposing charges of protons and electrons hold electrons within a spherical region surrounding the nucleus.
Atoms can lose and gain one or more electrons.

9. Determining Protons and Electrons

10. Neutrons
Neutrons are almost as massive as protons but carry no electrical charge.
The number of neutrons in the atoms of an element can vary resulting in ISOTOPES.
Can be naturally occurring or man-made
The sum of neutrons and protons in an atom is called the mass number of the atom.

11. Atomic Mass
Atomic masses listed on the periodic table are weighted averages of the masses of each naturally occurring isotope for that element.
Silver has two naturally occurring isotopes. One has a mass of about 107 amu and the other has a mass of about 109 amu.
Silver -107 has an abundance in nature of 51.84%.
Silver -109 has an abundance in nature of 48.16%.

12. Atomic Mass Calculate the average atomic mass of silver.
Silver has two naturally occurring isotopes.
One has a mass of amu (abundance in nature of 51.84%.)
The other has a mass of amu (abundance in nature of 48.16%.)
amu ( ) = amu
amu (0.4816) = amu
amu

13. Molar Mass Calculate the Molar Mass of Calcium carbonate
The mass of one mole of a compound.
Calcium carbonate
Chemical Formula  CaCO3
Calcium grams X 1 mole = grams
Carbon grams X 1 mole = grams
Oxygen grams X 3 moles = grams
grams

14. Periodic Law
Mendeleev listed the known elements in order of increasing atomic mass, grouping those with similar properties.
He noticed that certain similar properties would recur in a periodic fashion.
His tabulation is the precursor to our modern periodic table.

15. Mendeleev and the Periodic Table
Proposed that elements would be discovered to fill in gaps in the table.
Proposed that some measured atomic masses were in error.
Summarized a large number of observations
The underlying reasons for periodic behavior were as yet unknown
The Bohr model and the quantum mechanical model were needed to explain the observations.

16. The Bohr Model
This is a MODEL of the atom that links electron behavior (microscopic) to the periodic law (macroscopic).

17. Bohr Diagrams/Electron Configurations
Based on the behavior of electrons as particles
Electron orbits
Specified with n, the orbit’s quantum number
Fixed energies
Fixed radii
Maximum number of electrons based on n
This model is an oversimplification (as are most models).
Atoms with full outer orbits are extremely stable.
Atoms with outer orbits that are not full are unstable and will undergo chemical reactions attempting to fill the outer orbit.

18. The Quantum Mechanical Model
Based on the behavior of electrons as waves
Replace Bohr’s orbits with orbitals, a representation of electron location as the probability of finding it in a certain region of space.
Orbitals are grouped into shells and fill similarly to Bohr’s orbits.

19. Determinism and Quantum Mechanics
Specifics of orbital filling are beyond the scope of this text…BUT
The statistical nature of the quantum mechanical model rocked the scientific establishment.
An indeterminate universe
Both models are useful even though Bohr’s, by experiment, has been shown to be invalid.

20. Families of Elements Also called groups
Based on outer electron configurations
Vertical columns
Alkali metals
Alkaline earth metals
Chalcogens
Halogens
Noble gases

21. Element Families

22. Metals, Nonmetals, and Metalloids

23. Molecular Elements
Some elements occur as diatomic molecules.

24. The Mole Concept Counting particles as small as atoms is impractical.
The mole concept allows us to relate the mass of a sample of an element to the number of atoms within it.
The unit of comparison is called a mole and corresponds to x 1023.

25. Avogadro’s Number
Determined such that the numerical value of the atomic mass of an element in amu is equal to the molar mass of that element in grams per mole.
These relationships of grams, moles, and atoms can be used as conversion factors.

26. Chapter Summary Molecular Concept Atomic Number and Mass Number
Isotopes
Molar Mass
Bohr Model
Quantum Mechanical Model
Orbitals
Societal Impact
Chemical processes that cause change are caused by changes in atoms or molecules.
Pollution results from “misplaced” atoms. Atoms that are not where they are supposed to be located.
Models are used to describe nature.