Download Chapter 6 Study Guide

Name:______________________________________________________Date:________Period:________
Study Guide: Periodic Table
1. What is periodic law?
2. How did Moseley improve upon Mendeleev’s periodic table?
3. Label the following periodic table with the group numbers (both overall numbers AND
the main group element numbers. i.e., the boron family is overall group 13 but 3A for
main group elements).
4. Identify each element as a metal, nonmetal, or metalloid.
a. Fluorine (F): _________________________________________________
b. Germanium (Ge):_____________________________________________
c. Zinc (Zn):___________________________________________________
d. Phosphorous (P): _____________________________________________
e. Lithium (Li):_________________________________________________
5. Give two examples of elements in each group and write the number of valence
electrons.
a. Alkali Metals:________________________________________________________
b. Alkaline Earth Metals: _______________________________________________
c. Transition Metals:____________________________________________________
d. Halogens:___________________________________________________________
e. Noble Gases:_______________________________________________________
6. Write the symbol for the elements in the following locations.
a. period 3, Group IIIA _____________________________________________
b. period 1, Group VIIIA ____________________________________________
c. period 4, Group IIA ______________________________________________
d. period 6, Group VA ______________________________________________
7. How many Valence electrons are in each group of the main group elements?
8. Find the Element
Write the symbol of the element or elements that fit each description
a. A halogen in period 3
b. The inner transition metal with the lowest atomic number
c. A metal in group 5A
d. All the transition metals with an atomic number that is a multiple of 5
e. The electron configuration ends with 4s2
9. Why do elements in the same family generally have similar properties?
10.What trend in atomic radius occurs down a group on the periodic table? What causes
this trend?
11. What is the trend in atomic radius across a period in the periodic table? What causes
this trend?
12.Circle the atom in each pair that has the largest atomic radius.
a. Al or B
d. O or F
b. Na or Al
e. Br or Cl
c. S or O
f. Mg or Ca
Name:______________________________________________________Date:________Period:________
13. Define ionization energy.
14.What trend in ionization energy occurs down a group on the periodic table? What
causes this trend?
15. What is the trend in ionization energy across a period in the periodic table? What
causes this trend?
16. Circle the atom in each pair that has the greater ionization energy.
a. Li or Be
d. P or Ar
b. Ca or Ba
e. Cl or Si
c. Na or K
f. Li or K
17.How does ionization energy affect the trend in reactivity in the alkali metals and the
alkaline earth metals?
18. Define electronegativity.
19.What is the trend in electronegativity down a group on the periodic table? What
causes this trend?
20.What is the trend in electronegativity across a period on the periodic table? What
causes this trend?
21. Circle the atom in each pair that has the greater electronegativity.
a. Ca or Ga
d. Ba or Sr
b. Br or As
e. Cl or S
c. Li or O
f. O or S
22. How does electronegativity affect the trend in reactivity in the halogens?
The code letters A to Z have been assigned to the first 26 elements in the periodic table. The code letters do
not represent the chemical symbols, nor have the letters been assigned in alphabetical order.
These letters are presented in groups and your assignment is to arrange these elements in the proper periodic
form, according to the information given pertaining to certain members of the group.
The best way to start is to find which group each family belongs, and then arrange the elements within the
group. The following elements belong together in groups:
NDG
WASO
BRL
QTJ
HUM
ZPY
EVFX
KIC
The following clues are given
1. M has a total of 8 electrons
2. W’s electron configuration of1s22s22p63s23p6
3. S is a noble gas
4. R is an alkaline earth metal
5. X has an electronegativity less than V
6. D has the smallest atomic mass in its group
7. S only has electrons in the 1s orbital
8. L is an alkaline earth metal
9. Z is a halogen
10. U has an ionization lower than H A has more
neutrons than O
1A
2A
3A
4A
N
11. I has one more proton than B
12. K is a metal
13. T has the smallest atomic radius in its group
14. E is a gas
15. Atom F contains 11 electrons
16. J is a metalloid
17. R has an atomic number smaller than B but
larger than L
18. P has the smallest radius in its family
19. Z has higher ionization energy than Y
5A
6A
7A
8A
Name:________________________________________________Date:____________Hour:___________