Review for Periodic Table and Chemical Bonding TEST
Chapters 3-4 Key
1. From the Periodic Table, know how to determine the number of protons, neutrons, and electrons in an atom.
Atomic # = # of protons & # of electrons (A.P.E.)
Atomic mass – Atomic # = # nuetrons
2. Where are the metals, nonmetals, and semiconductors (metalloids) located on the periodic table?
Metals are left of the “staircase.” Nonmetals are right of the “staircase.” Metalloids are touching the
“staircase”, except for Aluminum.
3. Predict the arrangement of electrons within energy levels and determine the number of valence electrons.
What do you look for? How do you determine?
2 e- on 1st level, 8 e- on 2nd level, 8 e- on 3rd level. Number of valence e- is related to the group
number on the Periodic Table.
4. Determine the oxidation number and number of valence electrons of an element from location on periodic
table. (list group # and the corresponding oxidation # and # of valence electrons)
# of valence eGive or Gain
Oxidation #
Group 1
1
Give 1
+1
Group 2
2
Give 2
+2
Group 13
3
Give 3
+3
Group 14
4
Give 4 or Gain 4
+4 or -4
Group 15
5
Gain 3
-3
Group 16
6
Gain 2
-2
Group 17
7
Gain 1
-1
Group 18
8
Has Stable Octet
0
5. Compare and contrast and an element vs. a compound.
Elements are atoms of the all same type. Compounds have 2 or more elements.
6. Count the number and type of atoms in chemical formulas.
Ex:
NaCl
Na = 1
Cl =1
HSO4
H=1
S=1
O=4
MgBr2
Mg = 1
Br = 2
P2O5
P=2
O=5
Ba3(PO4)2
Ba =3
P=2
O=8
7. Distinguish between a compound, an element, and an ion
Ex:
KCl
Pb
Al+3
F-1
C6H12O6
Ionic
element
ion (charged atom) ion
compound
8. Use subscripts in a chemical formula to make the charges of ions cancel out in a compound.
Ex:
Al__ Cl__
C__F__
Si__O__
AlCl3
CF4
SiO2
9. Identify if a compound’s bond is ionic or covalent or both (with a polyatomic) based on elements involved.
Ex:
MgBr2
H2O
Li2SO4
KF
Cl2
Ionic
covalent
both
ionic
covalent
10. Predict if elements will form ionic or covalent bonds, based on the elements involved.
Ex: K + Cl
C+H+O
Mg + S
H + NO3
Ionic
covalent
ionic
covalent
11. Bohr Models (draw and label) be able to show transfer/movement of electrons. Which is ionic? Covalent?
Covalent Bonds
Ionic Bond
12. Why do ionic compounds that result from combining Group 2 and Group 16 elements have a 1:1 ratio?
Group 2 have 2 valence electrons to donate to a Group 16 element that needs 2 valence e- to become
stable
13. Elements in which group number are most likely to react with potassium (K)? What is this group’s special
name?
Group 17 (or halogens) because they need one more valence electron to become stable
14. The elements of which group on the periodic table are most resistant to forming compounds?
Group 18 or Nobel Gasses already have a stable octet.
15. Name 3 elements that have bonding characteristics similar to oxygen.
Oxygen is in Group 16, so Sulfur, Selenium, Tellurium, and Polonium
16. Name 3 elements that are most likely to donate one electron.
Group 1 metals (alkali metals) have one electron to donate, so Li, Na, K, Rb, Cs, and Fr
17. According to the periodic table, which elements will form an ion with a –2 charge?
Group 16 elements form -2 ions, so O, S, Se, Te, Po
Circle the correct options to make the statement true.
18. Elements in Group 16 of the periodic table usually gain / lose 1, 2, 3 electrons.
19. Elements in Group 17 of the periodic table usually gain / lose 1, 2, 3 electrons.
20. Elements in Group 1 of the periodic table usually gain / lose 1, 2, 3 electrons.
21. Elements in Group 2 of the periodic table usually gain / lose 1, 2, 3 electrons.
Short Answer. Answer each question in complete sentences
22. Elements from which groups will more readily bond and why?
Group 1 elements (+1) bond regularly with Group 17 elements (-1) because they make stable
compounds in a 1:1 ratio.
Group 2 elements (+2) bond regularly with Group 16 elements (-2) because they make stable
compounds in a 1:1 ratio.
23. How do ionic and covalent bonds differ?
Ionic bonds are formed after a metal has donated its valence electrons to a nonmetal. This creates
and attractive force between the (+) cation and the (-) anion. Covalent bonds form when nonmetals
share pairs of electrons between them.