1.
I can discuss the historical developments leading to the atomic theory and analyze results of key scientists to determine their historical conclusions.
A.
Democritus (atomos)
B.
Dalton (atomic theory)
C.
Thomson (Plum pudding model of electrons)
D.
Rutherford (gold foil experiment)
2.
I can analyze an atomic model and correctly identify the subatomic particles and their charges.
A.
Define and give the charge of each: a.
Proton b. Neutron c. Electron
B.
Describe how the subatomic particles are arranged within the atom
C.
Compare the relative sizes of the subatomic particles
D.
Compare the relative charges of the subatomic particles
3.
I can distinguish between elements and isotopes.
1.
Define the following vocabulary terms (listed below).
2.
Identify the number of protons, neutrons, and electrons given atomic number, mass number, and charge (and vice versa).
3.
Contrast mass number and atomic mass.
A.
Calculate the atomic mass given the relative amounts of isotopes.
Learning Goal
I can discuss the historical developments leading to the atomic theory and analyze results of key scientists to determine their historical conclusions.
I can analyze an atomic model and correctly identify the subatomic particles and their charges.
I can distinguish between elements and their isotopes
C Level
Can match key historical scientists with their discoveries in chemistry.
Can list and identify subatomic particles and their relative charge, mass and location in the atom.
Can calculate the number of protons and neutrons in an element given isotope notation. Can list the number of protons and electrons given the element and the atomic charge.
B Level
Can explain the key discoveries in chemistry.
A Level
Can explain the key discoveries in chemistry and evaluate the errors present in these theories throughout chemistry history.
Can compare and contrast subatomic particles in terms of their relative charge, mass and location in the atom.
Can explain how atomic mass is different from mass number.
Can explain how these characteristic differences in subatomic properties affects the identity and behavior of an element.
Can calculate the atomic mass of an element given the relative amounts of isotopes.

1.
Atom
2.
Atomic Mass
3.
Atomic Mass Unit
4.
Atomic Number
5.
Atom Charge = 0
6.
Chemical Symbol
7.
Compound
8.
Electron
9.
Element
C Level:
1)Who developed the atomic theory?
10.
Isotope
11.
Isotope Notation
12.
Mass Number
13.
Molecule
14.
Neutron
15.
Nucleus
16.
Periodic Table
17.
Proton
18.
Subatomic Particle
2) What two subatomic particles are located in the nucleus?

3) An atom of nitrogen has an atomic number of 7 and a mass number of 13 with a charge of -3. How many protons, neutrons, and electrons does this atom have?
B Level:
4) How did the gold foil experiment help
Rutherford determine that the atom was primarily empty space but contained an extremely dense, positively charged nucleus?
5) What are two ways that neutrons and protons similar and what are two ways that they are different?
6) The mass number of an atom is always given as a whole number (ex. Mass number of a hydrogen atom = 1) but the atomic mass on the periodic table is usually listed as a decimal (ex. Atomic mass of hydrogen is 1.00794 amu). Explain why this difference exists.
A Level:
7) How will the addition of a proton affect the identify and chemical behavior of an element?
Addition of a neutron?
8) Two isotopes of gallium are naturally strong with gallium-69 occurring 63.11% and gallium-71 occurs at a rate of 39.89%. What is the atomic mass of gallium and why is it not just 70 – the average of the two mass numbers 69 and 71? Show math.
3