Chapter 6 Study Guide
The Periodic Table and Periodic Law
1. Explain how Mendeleev’s periodic table was in error. Arranging the elements by mass resulted
in several elements being placed in groups of elements with different properties
How was the error fixed? They were placed in order by increasing atomic number
2. How was Mendeleev’s periodic table organized?
In order of increasing atomic mass w/ columns with similar properties
3. What is the periodic law? Periodic repetition of chemical and physical properties of the
elements when they are arranged by increasing atomic number
4. Identify each of the following as a metal, nonmetal, or metalloid:
a. Oxygen
NM
b. Barium
M
c. Germanium M-oid
d. Iron
M
e. Neon
NM
f. Tungsten M
5. Describe the general characteristics of metals. Good conductors of heat & electricity,
malleable (pounded into thin sheets) , & ductile (drawn into wires
6. Match each numbered item on the right with the lettered item that is on the left.
1. Alkali metals b. Group 1
a. Group 18
2. Halogens
d. Group 17
b. Group 1
3. Alkaline earth metalsc. Group 2
c. Group 2
4. Noble gases a. Group 18
d. Group 17
7. A shiny solid element also is ductile. What side of the periodic table is it likely to be found? left
8. What are the general properties of a metalloid? Those of both metals and nonmetals
List 3 metalloids. Silicon, antimony & germanium
9. What is the purpose of the heavy stair-step line on the periodic table? Divides metals and
nonmetals
10. Give the chemical symbol of each of the following elements:
a. The two elements that are liquids are room temperature mercury and bromine
b. The noble gas with the greatest atomic mass radon
c. Any metal from group 14 tin or lead
d. Any inner transition metal any lanthanide or actinide
11. Explain why the radius of an atom cannot be measured directly.
Electron cloud based on
probability and does not have a clearly defined edge
12. Given any two elements within a group, is the element with the larger atomic number likely to
have a larger or smaller atomic radius than the other element?
larger
13. Which elements are characterized as having their d orbitals filled with electrons as you move
left-to-right across a period?
Transition metals
14. An element forms a negative ion when ionized. On what side of the periodic table is the
element located? right
15. Of the elements magnesium, calcium, and barium, which forms the ion with the largest radius?
Ba
The smallest? Mg
What periodic trend explains this? Ionic radius increases down a group
16. What is ionization energy? The energy required to remove an electron from a gaseous atom
17. Explain why each successive ionization of an electron requires a greater amount of energy?
The increase nuclear charge of each successive element produces an increased hold on the
valence electrons
18. Which group has the highest ionization energies? 17
19. Define an ion. Atom that has loss or gained 1 or more electrons and has a charge
20. Explain why atomic radii decrease as you move left-to-right across a period. Caused by the
increasing positive charge in the nucleus & principle energy level within periods remains the
same
21. Which element in each pair has the larger ionization energy?
a. Li, N
b. Kr, Ne
c. Cs, Li
22. Explain the octet rule. Atoms tend to gain, lose, or share electrons in order to acquire a full set
of eight valence electrons
23. How many valence electrons do elements in each of the following groups have?
a. Group 1
1
b. Group 18
8
c. Group 13 3
+
24. Na and Mg2+ ions each have ten electrons surrounding their nuclei. Which ion would you
expect to have the larger radius? Na+ Why? the size of the positive ions gradually decreases
25. Which element in each pair is more electronegative?
a. K, As
b. N, Sb
c. Sr, Be
26. An element is a brittle solid that does not conduct electricity well. Is the element a metal,
nonmetal, or metalloid?
27. Arrange the elements oxygen, sulfur, tellurium, and selenium in order of increasing atomic
radii. O, S, Se, Te Is your order an example of a group trend or a period trend? Group trend
ALSO NEED TO KNOW:
28. What is a group or family? columns
29. What is a period?
rows
st
30. Who created the 1 periodic table? Mendeleev How was it arranged? By increasing atomic
masses Who re-arranged it? Moseley How was it re-arranged? By increasing atomc #s
31. Names of the groups of elements for Group 1 (alkali metals), 2 (alkaline earth metals), 312 (transition metals), 17 ( halogens), and 18 (noble gases).
32. Where are the most reactive elements located? Groups 1 and 17
33. Where are the most unreactive elements located? Group 18
34. Characteristics of metals and non-metals. See Guided Reading Questions (GRQ)
35. What is ionization energy? See GRQ
36. What is electronegativity? See GRQ
37. What does the term periodic mean? See GRQ
38. Where is the d-block located? Transition metals What types of elements are in the dblock? Metals
39. Periodic trends in atomic radii and ionic radii. See GRQ
40. Periodic trends in ionization energy and electronegativity. See GRQ
41. How many electrons does it take for an element to have a “full” outer shell? 8
42. What is the law of octaves? See GRQ
43. What is the octet rule? See GRQ
44. What is and where are the representative elements? Elements in groups 1, 2, 13-18
45. What is an ion? See GRQ
46. What is and where are the transition elements? See # 38