Objectives for Unit 2 packet.
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Date: __________
Explain the laws of conservation of mass, definite proportions, and multiple proportions.
Summarize the essential points of Dalton’s atomic theory and explain how it accounted
for all of the above laws.
Summarize the observed properties of cathode rays that led to the discovery of the
electron.
Describe Thomson’s model of the atom.
Describe Rutherford’s famous gold foil experiment and interpret the results of the
experiment.
Describe Rutherford’s model of the atom.
Describe (briefly) Bohr’s model of the atom.*
List the characteristics of the subatomic particles: protons, neutrons, and electrons.
Define atom.
Explain what isotopes are.
Define atomic number and mass number.
Given the identity of a nuclide, determine how many protons, neutrons, and electrons it
has.
Interpret notation for nuclides (e.g., C-14 or 146C).
Define nuclear charge.
Use the periodic table to determine the correct number of protons and electrons in a
neutral atom.
Define the terms ion, cation, anion.* How is an ion made?*
Calculate the number of neutrons, protons, and electrons in ions of specific nuclides.
Calculate average atomic mass of an element, given the masses and abundances of its
naturally occurring isotopes.
Know that one mole is defined as the number of atoms in exactly 12 grams of pure C-12.
Know Avogadro’s number. Understand that this number was determined experimentally
after the mole was defined in terms of a mass of carbon-12.
Determine the gram atomic mass (or molar mass or formula mass) of an element using
the periodic table.
Explain the concept of a relative mass scale.
Know the standard for the atomic mass unit.
Explain the differences between atomic number, mass number, atomic mass, and average
atomic mass.
Define molar mass.
Understand the relationship between mole, molar mass, and Avogadro’s number.
Convert between mass in grams, amount in moles, and number of atoms for elements.