Chemistry, Chapters 3

Unit 2: Atomic Structure and Configuration

Unit Objectives Be able to describe Dalton’s atomic theory. Be able to describe how Thompson, Rutherford and

Bohr’s model of the atom and discoveries lead to the modern atomic theory

Be able to describe Rutherford’s “gold foil” experiment.

Be able to describe atoms in terms of their components: protons, neutrons and electrons.

Be able to describe and relate to Dalton’s theory the laws of conservation of matter, constant composition, and multiple proportions.

Be able to determine the electron configuration of the first twenty elements of the periodic table. Standards 2.1, 2.2, 2.3, 2.4

Key Vocabulary Atomic mass Atomic theory Avogradro’s constatn Law of definite proportion Law of multiple

proportions Mole Alpha particle Anode Atomic number Cathode Coulomb’s law Electron, neutron, proton

Isotope, Radioisotope Mass Number Electromagnetic

spectrum Electron configuration Excited state Ground state Hund’s rule Line-emission spectrum Orbital Pauli exclusion principle Quantum number Aufbau principle

Question of the Day

What is atomic theory?

Atomic Theory Law of Definite Proportions Law of Conservation of Mass Law of Multiple Proportions Dalton’s Atomic Theory Atomic Mass Mole and Avogadro’s Constant

Internal Structure of Atoms Subatomic Particles Nucleus Atomic Number Mass Number Coulomb’s law Isotopes

Electron Configuration Electromagnetic Spectrum

Line-emission spectrum Bohr: ground and excited state Quantum Number

n can be values 1-7 (higher the number, furthest from nucleus)

l can be values 0 to n-1. (0=s orbital, 1=p orbital, 2=d orbital, 3=f orbital)

m can be values based upon l l and m designate shapes and orientation of orbitals. Pauli exclusion principle Aufbau Principle Hund’s rule