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1)Explain how different observations and experiments led to changes in the atomic model.
2)Describe the properties and locations of protons, neutrons, and electrons in an atom.
3)Explain what the mass number and atomic number identify about an atom.
4)Use mass and atomic number to determine the number of each subatomic particle in an atom.
5)Identify the differences between isotopes of an element.
6)Calculate the weighted average mass of an element when given the percent abundance and mass of its isotopes.
7)Describe the mole and its use in chemistry calculations.
8)Use the mole, Avogadro’s number, and molar mass in dimensional analysis calculations.
9)Describe observations that led to the Bohr and quantum models of the atom.
10)Explain how line spectra are used to identify elements and what they indicate about atoms.
11)Explain properties of waves and how these properties apply to the quantum model.
12)Describe your observations, calculations, and conclusions from the virtual lab.
13)Represent electron arrangements using electron configuration, orbital notation, shorthand notation, and Lewis dot notation.
14)Describe the quantum model of an atom in terms of energy levels, sublevels, and orbitals.
15)Use quantum numbers to represent the locations of electrons.
16)Apply the rules and limitations of each quantum number to identify possible and impossible quantum number sets.

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Hagrid
Describe the changes in the atomic model over time.
The existence of atoms began to be accepted around 1910 when many theories called upon the fact that atoms most exist (for example the work of Boltzmann trying to explain entropy, died 1906).
At that time atoms were seen as tiny small ball like objects, all matter was composed of. the models have been advanced ever since. Key names that are worth looking up are J. J. Thomson, Rutherford, Bohr and de Broglie.

Explain how different observations and experiments led to changes in the atomic model.
Many of the models that the men above proposed were created upon what they saw from their experiments. An example is that Niels Bohr wanted to explain the spectral lines in hydrogen, introducing the energy shells are quantized.

de Broglie saw that we could calculate wavelengths for particles with a certain velocity, introducing the particle wave duality.

Rutherford suggested that electrons are orbiting the nucleus like planets.

Thomson that there was a "electronsness" surrounding a positive core.

They can all be explain more deeply, but this is just introductory.