1. PERIODIC TABLE
Kenneth E. Schnobrich

2. Li Atomic Mass Oxidation State Atomic Number Electron Configuration 3
6.941 +1
Atomic Number 3
1s22s1 or 2-1
Electron Configuration

3. GROUPS H Li Na K Rb VERTICAL COLUMNS - • Alkali Metals
• Alkaline Earth Metals
• Transition Elements
• Chalcogens
• Halogens
• Inert (Noble) Gases 1 2
3-12 16 17 18 Li Na K Rb

4. PERIODS 1s22s1 1s22s2 1s22s22p1 1s22s22p2 1s22s22p3
HORIZONTAL ROWS - the Period Number indicates the Principal Energy Level that is filling as we move from left to right. Li Be B C N O F Ne

5. PERIODS
2-1
2-2
2-3
2-4
2-5
2-6
2-7
2-8
HORIZONTAL ROWS - the Period Number indicates the Principal Energy Level that is filling as we move from left to right. Li Be B C N O F Ne

6. METALS
METALLOIDS
NONMETALS
INERT GASES

7. Atomic Radius
Table S*
DECREASES
*NYS Reference Tables for Chemistry

8. COVALENT RADII - PERIOD 2

9. Atomic Radius
INCREASES

10. COVALENT RADII - GROUP IA

11. Types of Atomic Radii
Covalent Radius - effective distance from the center of the nucleus to the outer valence shell in a covalent or coordinate covalent bond.
Van der Waals Radius - half the closest distance between two nonbonded atoms.

12. Metals +
Loss of electrons -
Nonmetals
Gain of electrons

13. IONIZATION ENERGY ELECTRONEGATIVITY
Definitions
Ionization Energy – the amount of energy (usually in kilojoules) needed to remove the most loosely bound electron from a gaseous atom of an element.
Electronegativity – the attractive force that an atom has for an electron(s) during the formation of a chemical bond. (no units are assigned)

14. Ionization Energy & Electronegativity
“PROPERTIES OF SELECTED ELEMENTS”
Table S
First Ionization
Energy (kJ/mol) Na
496
0.9
Electronegativity

15. Ionization Energy
INCREASES

16. General Trend Across a Period

17. Ionization Energy
DECREASES

18. General Trend Down a Group

19. General Trend Down a Group

20. ELECTRONEGATIVITY DECREASES Table S*
*NYS Reference Tables for Chemistry

21. Electronegativities of Group IA

22. Electronegativity Across a Period
INCREASES

23. Electronegativities for Period 2

24. REACTIVITY
REACTIVITY
INCREASES
REACTIVITY
INCREASES

25. Transition Elements
Multiple Oxidation States
Form Colored Compounds
Incomplete Inner “d” Sublevels

26. TYPICAL QUESTIONS

27. The Most active metals are in Group -
1 (IA)
15 (VA)
13 (IIIA)
17 (VIIA)

28. The elements known as Alkali metals are found in Group
1 (IA)
2 (IIA)
13 (IIIA)
17 (VIIA)

29. What is the total number of electrons found in the valence shell of an Alkaline Earth element in the ground state 1 2 3 4

30. As the elements in Group IIA are considered from top to bottom, the # of electrons in the 2s subshell
increases
decreases
remains the same

31. Which group contains atoms that form +1 ions having an inert gas configuration?
1 (IA)
11 (IB)
17 (VIIA)
7 (VIIB)

32. Which Group 17(VIIA) elements listed below has the greatest nuclear charge?F Cl Br I

33. Which element is most likely to form a compound with Kr?
Fluorine
Chlorine
Bromine
Iodine

34. Which group on the Periodic Table contains solid, liquid, and gaseous elements at room temperature?
2 (IIA)
16 (VIA)
17 (VIIA)

35. Which represents the correct order of activity for the Group VIIA(17) elements?
Br > I > F > Cl
F > Cl > Br > I
I > Br > Cl > F
F > Br > Cl > I

36. If the elements are considered from top to bottom in Group 16(VIA), the number of electrons in the outermost shell will?
decrease
increase
remain the same

37. Which Group contains and element that is a liquid at room temperature?
2 (IIA)
11 (IB)
12 (IIB)

38. Which element has the greatest tendency to gain electrons?Se S O
USE CHART S

39. When atoms of the elements in Group 18 (0) are compared in order from top to bottom, the attractions between atoms?
increases and the boiling point decreases
decreases and the boiling point increases
increases and the boiling point increases
decreases and the boiling point decreases

40. In the ground state, an atom of which element in Period 3 has the most loosely bound electron?Si Na S Ar
USE CHART S

41. Which Period contains elements that are all gases at STP?1 2 3 4

42. Considered in succession, the elements in Period 2 of the Periodic Table show a decrease in atomic radius with increasing atomic charge increases?
nuclear charge increases
# of PEL increases
number of neutrons decreases
# of protons increases

43. Which represents the electron configuration of a metalloid in the ground state?
2-3
2-5
2-8-5
2-8-6

44. In a given Period of the Periodic Table, the element with the lowest first ionization energy is always?
an Alkaline Earth Metal
an Alkali Metal
a Halogen
an Inert Gas
USE CHART S

45. As one goes from Li to F in Period 2 of the Periodic Table, the atomic radius of the elements?
decreases
increases
remains the same
USE CHART S

46. An element in which electrons from more than one energy level may be involved in bond formation?
potassium
calcium
copper
zinc

47. Which element can form more than one binary compound with chlorine?
potassium
calcium
iron
zinc

48. A pure compound is blue in color. It is most likely a compound of?
sodium
lithium
calcium
copper

49. Which is the electron configuration of a transition element in the ground state?
2-8-8 Ar Ca Zn Kr