Download Chapter 6 Review Name Period _____ Know the history

Chapter 6 Review
Name _______________________
Period _____
 Know the history/development of the periodic table.
1. Who first published the classification of the elements that is the basis of our periodic
table today?
Mendeleev
2. By what property did Mendeleev arrange the elements?
By Atomic Mass
3. By what property did Moseley suggest the periodic table be arranged?
By Atomic number
4. What is the periodic law?
The Periodic Table is arranged by increasing atomic number, and thus shows mutliple
repeating patterns are evident without fail
 Know the layout/arrangement of the periodic table.
5. What is a period? How many are there in the periodic table?
The rows of the Periodic Table, 7
6. What is a group? How many are there in the periodic table?
The columns or families of the PT, 18 (8 representative
7. State the number of valence electrons in an atom of:
a. Sulfur
____6__
b. Calcium
___2___
c. Chlorine
____7__
d. Arsenic
_____5_
8. Write the name of the element that is found in the following periods and groups:
a. Period 2, Group 2A Beryllium__________
b. Period 4, Group 8A
____Krypton_________________
c. Period 6, Group 4A _________Lead____________
9. Which of the following pairs of elements belong to the same period?
a. Na and Cl
b. Na and Li
c. Na and Cu
d. Na and Ne
10. Which of the following pairs of elements belong to the same group?
a. H and He
b. Li and Be
c. C and Pb
d. Ga and Ge
Chapter 6 Review
Name _______________________
Period _____
11. How does an element’s period number relate to the number of the energy levels of its
valence electrons?
Representative element – equal to
Transition Metals- one more (n-1)
12. Would you expect Strontium to be, chemically, more similar to calcium or rubidium? Why?
Calcium
13. What are the Group 1A elements called?
Akali metals
14. What are the Group 2A elements called?
Akaline earth metals
15. What are the Group 7A elements called?
Halogens
16. What are the Group 8A elements called?
Noble gases
17. Why do all the members of a group have similar properties?
They contain the same number of valence electrons
18. Where, generally, are the metals located on the periodic table?
To the left of the staircase
19. Where, generally, are the nonmetals located on the periodic table?
To the right of the staircase
20. List some properties of metals.
High luster, ductile, malleable, good conductor of heat and electricity
21. List some properties of nonmetals.
Poor conductor of heat and electricity, brittle EXCEPT carbon
22. What kinds of properties do metalloids have?
Contain properties of both metals and nonmetals depending on the conditions
 Know the trend for atomic radius.
23. Within a group, what happens to the atomic radius as you go down a group? Why?
The atomic radius increases because, as you go down a group the energy level increases
24. Within a period, what happens to the atomic radius? Why?
Chapter 6 Review
Name _______________________
Period _____
The atomic radius decreases, as you go across a period the valence electrons increase,
causing a larger interaction with the nucleus
25. What is the shielding affect?
The electrons that are in between the valence shell and the nucleus shield
 Know the trend for ionic radius.
26. What is the charge of a cation?
Increases across the period, same for each group
27. How are neutral atoms made into cations?
They lose electrons in their outter shell
28. What is the charge of an anion?
Negative, increases across a period and reamin the same going down
29. How are neutral atoms made into anions?
They gain electrons to fill their valence shell
30. Metals usually form what type of ions?
Cations
31. Nonmetals usually form what type of ions?
Anions
32. When an atom becomes an anion, what happens to its radius? Why?
With the addition of an electron the repulsion between the electrons increases increasing
the size of the ion.
33. When an atom becomes a cation, what happens to its radius? Why?
As an atom loses an electron the repulsion decreases
34. For each of the following pairs, circle the atom or ion having the larger radius.
a. S or O
c. Na+1 or Na
e. S-2 or S
b. Ca or Ca+2
d. Na or K
f. F
or F-1
 Know the trend for ionization energy.
35. What is ionization energy?
The energy required to knock off an electron
36. Which is higher: 1st Ionization energy or 2nd Ionization energy?
37. What is the general trend of ionization energy as you go across a period? Why?
Chapter 6 Review
Name _______________________
Period _____
Increases, as you go across a period the number of valence electrons increase the more
“resistant” the atom is to give up an electron.
38. What is the general trend of ionization energy as you go down a group? Why?
Decreases as you go down a group. Shielding is increased the nucleus has less effect on
valence electrons
 Know the trend for electronegativity.
39. What is electronegativity?
The affinity for an atom to “pick up” an electron
40. What is the general trend of electronegativity as you go down a group?
Decreases
41. What is the general trend of electronegativity as you go across a period?
Increases