Name: ________________________
Date: ___________
Block: _____
Atomic Structure and the Periodic Table Study Guide
1. What is an atom?
Smallest particle of an element that retains the properties of that element.
2. Complete the following chart about subatomic particles.
Name
Charge
Symbol
Location
Relative Mass
+
Proton
+
p
Nucleus
1 amu
Electron
e
Electron cloud
0
0
neutron
0
n
nucleus
1 amu
3. Draw an atom and label the subatomic particles.
4. Which subatomic particle is used to determine the identity of an element?
protons
5. Where is most of the mass of the atom? What particle(s) are in this area?
Nucleus; protons and neutrons
6. What is an atom called after it has gained or lost electrons? __ion_______________
7. What do you call an atom if it has more or less neutrons than normal? ___isotope_________
8. Label the information provided in the periodic table.
Atomic number
Symbol
Name
Atomic mass
9. From a box on the periodic table, how do you determine the number of protons, electrons, and
neutrons?
1) # p+ = _____atomic number______________________
2) # e- = _____number of protons______________________
3) # n0 = _____atomic mass – atomic number______________________
10. What does the atomic number represent? # protons in the nucleus
11. What does the atomic mass represent? # particles in the nucleus (protons & neutrons)
12. Use your knowledge of atomic calculations to complete the chart.
Element
Atomic #
Atomic Mass
# p+
# e-
# n0
Potassium
Sulfur
19
16
39
32
19
16
19
16
20
16
Hydrogen
Silver
Fluorine
1
47
9
1
108
19
1
47
9
1
47
9
0
61
10
13. If an atom has 43 electrons, 56 neutrons, & 43 protons, what is the approximate atomic mass?
What is the element? 56 amu + 43 amu = 99 amu
Technetium (Tc)
14. Calculate the correct number of p+, e-, and n0 for each isotope.
Complete Symbol
Atomic #
Atomic Mass
# p+
# e# n0
12
6
12
6
6
6
6 C
13
6
13
6
6
7
6 C
14
6
14
6
6
8
6 C
235
U
92
235
92
92
143
92
238
U
92
238
92
92
146
92
15. What term is used for electrons on the outermost electron shell or energy level? _valence___
16. The vertical columns on the periodic table are called ___groups________________.
17. Why do elements in the same column have similar properties? They have the same number of
valence electrons.
18. Match the correct name to each group number
1) _c__ Group 1
a. Rare Earth Metals
2) _h__ Group 2
b. Boron Family
3) _f__ Groups 3-12
c. Alkali Metals
4) _b__ Group 13
d. Nitrogen Family
5) _i__ Group 14
e. Halogens
6) _d__ Group 15
f. Transition Metals
7) _j__ Group 16
g. Noble Gases
8) _e__ Group 17
h. Alkaline Earth Metals
9) _g__ Group 18
i. Carbon Family
10) _a__ Two bottom rows of the
j. Oxygen Family
periodic table
19. The horizontal rows on the periodic table are called ___periods_________________.
20. What information does the row number, or period, give? Number of shells or orbitals
21. How many electrons will each energy level hold?
1st = _2__ 2nd = _8__ 3rd = _8__
22. What are the steps to drawing a Bohr model? Bohr model notes
23. What are the steps to drawing a Lewis dot structure? Lewis dot structure notes
24. Calculate the missing information and then draw the Bohr model and Lewis structure for each
element.
25. Answer the following questions about the elements in the previous question.
1) Which elements have a filled outermost shell? Ne, He
2) Which element would be most likely to lose an electron to become stable? Li
3) Which element would be most likely to gain an electron to become stable? Cl
4) Which elements are not likely to bond with other elements? Why? He and Ne full
valence shells
26. How many electrons do elements want in their valence shell to become stable? _8__
27. Complete the following table about ions.
Group Number
Valance eStable # of
e- Activity - # of
Charge of ion
valence ee-s lost or gained
formed
1
1
8
1 lost
+1
2
2
8
2 lost
+2
13
3
8
3 lost
+3
14
4
8
4 gained or lost
+/- 4
15
5
8
3 gained
-3
16
6
8
2 gained
-2
17
7
8
1 gained
-1
18
8
8
0 transferred
0