Atomic Structure/Periodic Table Study Guide
Science Standards are in italics.
Atomic Structure
SC-HS-1.1.2: Students will understand that the atom’s nucleus is composed of protons and neutrons that
are much more massive than electrons. When an element has atoms that differ in the number of
neutrons, these atoms are called different isotopes of the element.
Parts of the atom:
1. Define:
A. Atom
B. Proton
C. Neutron
D. Electron
E. Nucleus
F. Electron Cloud
2. Complete the following table:
Particle
Proton
Neutron
Electron
Electrical Charge
Mass
Location
3. The number of _____________________ determines which element an atom is.
4. Rutherford conducted experiments in which he beamed electrons at gold foil. Based on the results, he
determined that most of the mass of an atom is located in the _____________________.
5. Most of the volume of an atom is composed of the ______________________.
6. What is the radius of an atom? _______________________________________________________
Properties of an atom:
1. Define the following:
A. Atomic Number
B. Atomic Mass
2. Label the different parts of the squares in the periodic table. You must be able to read your periodic
table and find this information for any given element!!
Hydrogen
1
H
1.008
3. Complete the following table. You will need to be able to do this for any given element!
Element
Symbol
Atomic
Number
Atomic Mass # of Protons
# of
neutrons
# of
electrons
Carbon
Nitrogen
Neon
Magnesium
Silver
Radon
Mercury
4. If an element has atomic number 16, how many protons does it have? ____________________
5. If an element has atomic mass 65 and atomic number 30, how many neutrons does it have? ________
6. All atoms of the same element have the same number of ___________________.
Isotopes
1. Define
A. Isotope
B. Average Atomic Mass
2. As the mass number of an element increases, the number of protons __________________ and the
number of neutrons ___________________.
3. If an element has 1 proton, 1 electron, and 1 neutron, what is its atomic number? _________ Atomic
mass? ___________
Atomic Models
SC-H-STM-U-1: Students will understand that the configuration of atoms in a molecule determines the
molecule’s properties.
1. Define
A. orbital
B. valence electron
Bohr Model
1. Where are electrons located in the Bohr model? ___________________
2. List the number of electrons needed to fill each electron level:
1st level _____
2nd level _____
3rd level _____
4th level _____
3. Draw the Bohr model for the following elements. Include the number of protons, neutrons, and the
elemental symbol in the nucleus. You must be able to do this for any given element!!
Hydrogen
Carbon
Oxygen
Aluminum
Chlorine
Argon
Lewis Structures (Electron dot diagrams)
1. Draw the Lewis structures for the following elements.
H
H
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
2. You must be able to draw the Lewis structure for the elements based on where they are located on
the periodic table. Draw the following Lewis structures
Rb
As
Kr
Bi
Po
Pb
At
Ra.
Electron Configurations (Atomic Orbitals)
1. Describe the Heisenburg Principle.
2. What is an orbital?
3. The orbital occupied by the hydrogen electron is called _________________.
4. How many electrons can fit in each of the following orbitals? S ____
P ____
D ____
F _____
5. As you go from a 1s orbital to a 2s orbital, you ________________ in energy level.
6. List the orbitals in order. (You may draw the chart that we used in class and then list them.)
7. Write the electron configuration for the following elements. You must be able to do this for any given
element!
B: ______________________________________________________________________________
S: _______________________________________________________________________________
As: ______________________________________________________________________________
Cl: _______________________________________________________________________________
Xe: __________________________________________________________________________________
8. Identify the elements based on their electron configuration. You must be able to do this for any given
element!
A) 1s2 2s2 2p6 3s2 3p6 4s2 3d6 ______________________________
B) 1s2 2s2 2p4 ______________________________
C) 1s2 2s2 2p6 3s2 3p6 4s1 ______________________________
Periodic Table
SC-HS-1.1.1: Students will classify or make generalizations about elements from data of observed
patterns in atomic structure and/or position on the periodic table. The periodic table is a consequence of
the repeating patterns of outermost electrons.
HS-PS1-1: Use the periodic table as a model to predict the relative properties of elements based on the
patters on electrons in the outermost energy level of atoms.
Define the following terms:
A) periodic table
B) atomic radius
C) ionization energy
D) reactivity
E) electronegativity
F) metals
G) nonmetals
H) metalloids
I) period
J) group
Periodic Trends
1. How are the elements arranged on the periodic table?
2. What is the periodic law?
3. Describe the elements in the following groups: (be able to locate and identify these on the periodic
table)
A. Alkali metals
B. alkaline earth metals
C. halogens
D. noble gasses
E. transitional metals
4. How are elements in the same group similar?
5. How are elements in the same row similar?
6. Complete the following table. Describe and explain how each characteristic trends on the periodic
table. You need to understand these trends and be able to answer questions relating to these trends!
Characteristic
Across Table
Down Table
Explanation
Atomic Radius
Ionization Energy
Reactivity
Electronegativity
7. Compare metals, nonmetals, and metalloids. Be able to locate each on the periodic table.