Atomic Basics Work
Part A: The Periodic Table
1. Label the information provided in the periodic table.
2.
3.
4.
5.
NAME:___________________________HR:_________
What does the atomic number represent? _________________________________________________________
What does the atomic mass represent?___________________________________________________________
How would you determine the number of neutrons in an atom?________________________________________
Use your knowledge of atomic calculation to complete the chart.
Common
Element
Atomic
Atomic Mass
Protons
Neutrons
Electrons
Name
Number
Li
P
____
35
Ni
K
____
47
H
Part B: Atomic Structure
6. Label the following atom.
7. Draw an atom that has five protons, six neutrons and five total electrons. Label the protons, neutrons, and the
electrons with their charge as well as their location. What is the name of this element?____________________
8. Use your knowledge of Atomic Structure to fill out the following table.
Element Atomic
# of
# of
# of
# of
#of
#
Protons Electrons Electrons
Electrons
Electrons
in 1st Shell in 2nd Shell in 3rd Shell
H
# of
Valence
Electrons
Type of
Ion
Formed
Mass
#
# of
Neutrons
He
Li
Be
B
C
N
O
F
Ne
9. A carbon atom has 4 electrons in its highest energy level. How many hydrogen atoms could become bonded to a
single hydrogen atom?________________
a. Oxygen atom? _________________
10.
11. Using your knowledge of neutral atoms, ions and isotopes fill in the table below.
Element Atomic Mass
# of
# of
# of
Isotope, Ion,
How do you know?
#
#
C
6
C
6
14
He
2
4
H
1
H
Li
N
Protons Neutrons
electrons
6
6
Neutral
1
Neutral
1
3
Neutral Atom
0
7
14
Neutral
Part C: Bonding
12. Use the following terms to label the structures shown in each of the diagrams: electron, nucleus, neutral atom,
positive ion, negative ion, ionic bond, covalent bond, molecule. Some terms may be used twice or not at all.
Sodium (Na)
Chlorine (Cl)
Sodium Chloride (NaCl)
13. Use the following terms to label the structures shown in each of the diagrams: electron, nucleus, neutral atom,
positive ion, negative ion, ionic bond, covalent bond, molecule. Some terms may be used twice or not at all.
Chlorine (Cl2)
14. How is an ion different than a neutral atom?
15. Describe what happens with the electrons in the following bond types:
a. Covalent Bond:
b. Ionic Bonds:
Part D: Chemical Reactions
16. A number of chemical reactions are described below. In the spaces provided, identify the reactant(s) and the
product(s). Then write an equation for each reaction.
a. A sodium ion (Na+) reacts with a chlorine ion (CL-) to form the compound sodium chloride (NaCl).
Reactant(s):______________________________________
Product(s):_______________________________________
Equation(s):______________________________________
b. Magnesium oxide (MgO) is produced when a magnesium ion (Mg2-) reacts with an oxygen ion (O2-).
Reactant(s):______________________________________
Product(s):_______________________________________
Equation(s):______________________________________
c. Nitrogen (N2) and hydrogen (H2) form ammonia (NH3).
Reactant(s):______________________________________
Product(s):_______________________________________
Equation(s):______________________________________
d. Carbonic acid (H2CO3) breaks down to form water (H2O) and carbon dioxide (CO2).
Reactant(s):______________________________________
Product(s):_______________________________________
Equation(s):______________________________________
e. When it is burned, natural gas (CH4) combines with oxygen gas (O2) to produce carbon dioxide (CO2) and
water (H2O).
Reactant(s):______________________________________
Product(s):_______________________________________
Equation(s):______________________________________
17. In a molecule of 2C6H12O6:
a. How many molecules are present?___________
b. How many different elements are present?____________
c. How many atoms of each element are present?_________________
i. Carbon:_________
ii. Hydrogen:_________
iii. Oxygen:_________
d. How many total atoms are there?____________