2. Learning objectives:
After completing this unit of study, you should be able to:
An element’s location on the periodic table gives an indication of its physical and chemical properties.
Elements on the Periodic Table are arranged in order of increasing atomic number.
Elements are classified as metals, nonmetals and metalloids based on their properties and location on the periodic table.
Groups 1, 2, and have the same number of valence electrons in the group, and therefore have similar chemical properties. Helium is the exception to this.
Each group shows trends in atomic radius, ionic radius, Electronegativity, first ionization energy, and metallic and nonmetallic properties.
Each period shows trends in atomic radius, Electronegativity, first ionization energy, and metallic and nonmetallic properties.
When an element becomes an anion by gaining electrons, the radius increases.
When an element becomes a cation by losing electrons, the radius decreases.
Some elements exist as two or more forms in the same phase due to differences in molecular or crystal structures, and therefore have different chemical and physical properties. These are called Allotropes. Carbon has the allotropes coal, graphite, diamond, and fullerenes. Oxygen has the allotropes O2 & O3.

3. Learning Guide 1: P.T. Basics
Dimitri Mendeleev organized the 1st periodic table by atomic mass.
Mosley re-organized the periodic table by atomic number.
This was better because there are places on the periodic table that mass goes down, but atomic number ALWAYS INCREASES BY 1.
Modern Periodic Law states that elements are organized by atomic number, and properties are determined by number of valence electrons.

4. Learning Guide 1: P.T. Basics
Atomic Mass Oxidation States (charge) Symbol Atomic Number Electron Configuration

5. Learning Guide 1: P.T. Basics
6. A PERIOD is a horizontal row on the periodic table. 7. All elements in a period have valence electrons in the same ring. 8. The number of valence electrons go up by one as you go cross a period.

6. Metals, Metalloids & Nonmetals:

7. Learning Guide 1: P.T. Basics
9. Metals are located to the left and below the staircase line. 10. Nonmetals are located to the right and above the staircase line. 11. Metalloids (Semimetals) are located bordering the staircase line.

8. States of Matter at RT

9. Learning Guide 1: P.T. Basics
12. The majority of the elements are SOLID at room temperature. 13. There are 2 elements that are liquids at room temperature: Bromine (Br) & Mercury (Hg). 14. The gases at room temperature are : Hydrogen (H), Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn), Flourine (F), Oxygen (O), Nitrogen (N), Chlorine (Cl)

10. Learning Guide 1: P.T. Basics
15. A GROUP is a vertical column on the periodic table. 16. Another name for a group is a family. 17. All elements of a group have the same number of valence electrons. 18. All members of a group have similar reactivity.

11. Learning Guide 1: P.T. Basics
Symbol
Name
Atomic #
Period
Group Pb
Potassium 45
Iron 3 17

12. Complete chemdo 1

14. Metals, Metalloids & Nonmetals:

15. METAL
NONMETAL
Located to the left & below the staircase line
Located to the right above the staircase line
Solid ( except Hg(l) )
Luster (shiny)
Malleable ( flattens)
Ductile (wire)
Conducts electricity
Conducts heat
Hi density
Soft
Solid, liquid or gas
Dull
Brittle
Hard
Don’t conduct electricity
Don’t conduct heat
Loses electrons
Gains electrons
Form cations ( + ion)
Form anion (- ion)
Ions smaller than atom
Ions bigger than atom
Good conductor of heat & electricity
Poor conductor of heat & electricity
Lo Ionization Energy
Hi Ionization Energy
Lo Electronegativity
Hi Electronegativity
Most active metal lower left
Most active nonmetal upper right

16. Learning Guide 2: M/NM/SM
Nonmetal ions are larger than the atoms from which they are formed from because they gain electrons.
Metal ions are smaller than the atoms from which they from because they lose electons.

17. Learning Guide 2: M/NM/SM
3. Transition metals are located in groups 3-12.
4,,The transition metals have multiple (more than one) oxidation states.
4. 2 unique characteristics are multiple oxidation states and colored solutions in water.

18. Learning Guide 2: M/NM/SM
5. Metalloids are elements that have properties of both metals and nonmetals. 6. Metalloids border the staircase line.

19. Learning Guide 2: M/NM/SM
7. Noble gases are found in group They are unique because they do not react with other elements (they are snobs).

20. Learning Guide 2: M/NM/SM
9. Allotope: elements that exist as two or more forms in the same phase due to differences in molecular or crystal structures, and therefore have different chemical and physical properties.
10. a. Carbon (C) has the allotropes coal, graphite, diamond, and fullerenes.
b. Oxygen has the allotropes O2 & O3. Phosphorus has 3 allotropes

21. Allotropes of Carbon:

22. Metals, Metalloids & Nonmetals:

23. Metals, Metalloids & Nonmetals:

24. to left and below staircase line 2/3 of elements border staircase line
Property
METAL
SEMIMETAL
NONMETAL
LOCATION
 to left and below staircase line
2/3 of elements
 border staircase line
To right & above staircase line 
1/3 of elements
LUSTER – SHINY?
 yes
maybe
 no, dull
CONDUCTIVE OF
HEAT & ELECTRICITY?
Maybe no
MALLEABLE – can bend without breaking?
No, hard & brittle
PHYSICAL STATE at RT?
 solid, except Hg(l)
 solid
solid, liquid & gas
Important examples:
 Cu, Au, Ag, Pt
B, Ge, Si, Sb, Te, At
F, C, N, O, Cl… 
# OF
VALENCE ELECTRONS
 1, 2, 3,
 3, 4,,5
 5, 6, ,7
TENDENCY TO LOSE OR TO GAIN ELECTRONS?
 tend to lose e- forming cations, getting smalller
Can gain or lose
 tend to gain e- , forming anions, getting larger
GENERAL ATOMIC
STRUCTURE
 less than 4 valence electrons
Around 4 valence electrons 
 more than 4 valence electrons
Are IE & EN high or low?
Low
Medium
High

25. Metal & Nonmetal LAB METALS NONMETALS Luster: shiny Mostly solid Soft:
Malleable – can flatten easily
Ductile – can be a wire
Conducts heat & electricity
(Cu wire , Ag & Au jewelry)
Reactive
( bubbles w/ HCl, darkens w/ CuCl2)
Dull (not shiny)
Can be solid or liquid or gas
Hard & Brittle
( crushes to a powder easily)
Does NOT conduct
Does NOT react

26. Which elements that you tested were METALS?
LIST: Support:

27. Which elements that you tested were NONMETALS?
LIST: Support:

28. Which elements that you tested were METALLOIDS?
LIST: Support:

30. Complete chemdo 2

31. Groups/Families of the Periodic Table

32. Nuclear Charge The charge of the nucleus
The number of protons = atomic number
Greater nuclear charge means greater attraction of nucleus on the electrons
Means smaller radius, harder to lose e- (IE)
easier to gain e- (e-neg)

33. Shielding
Kernel electrons interfere with the nuclear attraction for valence electrons.
More energy levels mean that it is easier to remove an e- and harder to gain an e-, because protons are shielded by the kernel e- in between them.

34. Ionization Energy
The amount of energy needed to remove the outermost electron.
More IE = harder to remove an electron
Less IE = easier to remove an electron

35. Learning Guide 3: Trends in Groups & Families
nuclear charge 4. As you go left to right across a period, nuclear charge increases, electrons are stronger attracted and more energy is required to remove them

36. Learning Guide 3: Trends in Groups & Families
nuclear charge
5. As you go top to bottom down a group, valence elevtrons are farther from the nuclesu and it is easier energy is required to remove them

37. Atomic Radius
DEF: ½ the distance between 2 atoms OR THE RADIUS OF AN ATOM

38. Learning Guide 3: Trends in Groups & Families
7. As you go left to right across a period atomic radius decreases. 8. As nuclear charge increases as you go left to right across a period, the number of protons increase, pulling tighter on electrons and making the radius smaller.

39. Learning Guide 3: Trends in Groups & Families
9. Shielding effect across a period is constant because balance electrons are in the same energy level in the same period.
Li Be B C N O F Ne
e- config:
Across a period sheilding has NO EFFECT!!

40. Learning Guide 3: Trends in Groups & Families
10. As you go top to bottom down a group atomic radius increases. 11. The number of occupied energy levels increases as you go top to bottom down a group. 12. Shielding causes atomic size to INCREASE as atomic number increases down a group.

41. Learning Guide 3: Trends in Groups & Families
13. ION: a charged part of an atom, resulting from the loss or gain of an electron. 14. Ionic Radius: LOSS of electron  ion is SMALLER than atom GAIN of electron  ion is BIGGER than atom

42. Learning Guide 3: Trends in Groups & Families
15. Metals tend to lose electrons to form an ion with a radius that is smaller than the atom. 16. Nonmetals tend to gain electrons to form an ion with a radius that is larger than the atom.

43. Learning Guide 3: Trends in Groups & Families
17. Electronegativity: A measure of how easily an atom gain gain (attract) electrons. Bigger EN number: easier to gain LOOK ON REF. TABLE S!!!!!!!! 18. Flourine has highest EN value of Francium has lowest EN of 0.7

44. Remember ionic radius???
When an atom forms an ION that is POSITIVE, the IONIC RADIUS is LESS THAN ATOMIC RADIUS, because it LOSES ELECTRONS
When an atom forms an ION that is NEGATIVE, the IONIC RADIUS is BIGGER THAN ATOMIC RADIUS, because it GAINS ELECTRONS

45. Bohr models of 3Li, 9F, 87Fr

46. Pg notepacket:
Atomic Radius – distance from nucleus to valence electron
Ionization Energy: energy required to remove the outermost electron
Electronegativity – a measure of ability to gain an electron

47. Periodicity: FOLLOWS A PATTERN
There are general trends in properties as you move left to right across a period.
There are general trends in properties as you move top to bottom down a group.

48. Periodic Trend in Number of Valence Electrons

49. Periodic Trend in Number of Valence Electrons
1.) What is the trend in valence electron number as you go from left to right across any period on the table? 2.) What is the trend in the valence electron number as you go down any group from top to bottom? 3.) What is the trend in the number of energy levels as you go down any group from top to bottom? 4.) Use your answers to #2 & 3 to write a statement explaining the relationship between number of valence electrons and the number of energy levels.

50. Periodic Trend in Atomic Radius

51. Periodic Trend in Atomic Radius
1.) What is the trend in atomic radii as you go from left to right across any period on the table? 2.) What is the trend in the number of protons (nuclear charge) as you go from left to right across any period on the table? 3.) Use your answers to #1 & 2 to write a statement explaining the relationship between atomic radii and nuclear charge (# of protons). 4.) What is the trend in atomic radii as you go down any group from top to bottom? 5.) What is the trend in the number of energy levels as you go down any group from top to bottom? 6.) Use your answers to #4 & 5 to write a statement explaining the relationship between atomic radii and the number of energy levels.

52. Ionization Energy: energy required to remove the outermost electron

53. Periodic Trend in Ionization Energy
1.) What is the trend in ionization energy as you go from left to right across any period on the table? 2.) What is the trend in the number of protons (nuclear charge) as you go from left to right across any period on the table? 3.) Use your answers to #1 & 2 to write a statement explaining the relationship between ionization energy and nuclear charge (# of protons). 4.) What is the trend in ionization energy as you go down any group from top to bottom? 5.) What is the trend in the number of energy levels as you go down any group from top to bottom? 6.) Define shielding: 7.) Use your answers to #4 & 5 to write a statement explaining the shielding effect on onization energy .

54. Electronegativity – a measure of ability to gain an electron

55. Periodic Trend in Electronegativity

56. Periodic Trend in Electronegativity
1.) What is the trend in electronegativity as you go from left to right across any period on the table? 2.) What is the trend in the number of protons (nuclear charge)as you go from left to right across any period on the table? 3.) Use your answers to #1 & 2 to write a statement explaining the relationship between electronegativity and nuclear charge (# of protons). 4.) What is the trend in electronegativity as you go down any group from top to bottom? 5.) What is the trend in the number of energy levels and shielding as you go down any group from top to bottom? 6.) Use your answers to #4 & 5 to write a statement explaining the shielding effect of number of energy levels on electronegativity.

57. Periodic Trend in Melting and Boiling Points
Graph Title: Periodic Trend in Melting Point and Boiling Point
Y-axis: start at -300, end at 4800, each “bold” line increases by 300. Label: TEMPERATURE (oC)
X-axis: _______ start at 0, end at 20, each “bold” line increases by Label: Atomic Number

58. Chem Do 3 graph
Y-axis: start at 50, increase by 10, stop at 220 X-axis : start at 10, count by .5, stop at 18 Be sure to * write a good title (1pt) * label each axis (1 pt each) * make a key describing the colors (1 pt)

59. Chem Do 3b graphs
#6: “Trend in atomic radius down group 2” Y-axis: start at 100, increase by 10, stop at 270 X-axis : start at 0, count by 5, stop at 90 #7: “Trend in ionization energy down group 1” Y-axis: start at 200, increase by 100, stop at 1800

60. Complete chemdos 3a & 3b

61. Periodic Properties of Elements

62. Alkali Metals
Location: group 1 Characteristic Elements: Na, K, Rb, Cs, Fr Reactivity: most active metals (Fr is THE most active metal), never found free in nature, electrolysis of fused salts. lo IE & electronegativity lose e-, IR<AR

63. Alkaline Earth Metals
Location: group 2 Characteristic Elements: Be, Mg, Ca, Sr, Ba, Ra Reactivity: very hi, but less than group 1. Also never found free in nature, electrolysis of fused salts lo IE & electronegativity lose e-, IR<AR

64. Transition Metals
Location: groups 3-12 Characteristic Elements: Fe, Cu, Cr, Au, Ag, Pt, Pb, Mn, Co… Special Characteristics: hard solids with hi MP, less reactive than groups 1 & 2 multiple oxidation states due to more than one energy level being filled at a time cause: colored solutions in water

65. Why do transition metals produce colored solutions?
MULTIPLE OXIDATION STATES! Look at: Fe Cr Ni Cu

66. Alloy
Def: solid mixture of metals (homogeneous mixture, ratio can vary) Examples: brass – mixture of zinc & copper bronze – copper & tin sterling silver – silver & copper

67. Halogens
Location: group 17 Characteristic Elements: F, Cl, Br, I, At Reactivity: most reactive NONMETALS, Also never found free in nature, electrolysis of fused salts or chemically hi IE & electronegativity (F is highest of 4.0) gain e-, IR>AR Exhibit all 3 states of matter (F & Cl (g), Br (l), I & At (s))

68. Noble Gases
Location: group 18 Characteristic Elements: He, Ne, Ar, Kr, Xe, Rn Reactivity: monatomic because full valence shell of 8 e- (He is full w/ 2 e-) therefore, do not react exception: Xe & Ar w/ F BP increases with increasing size

69. Use the next slide to label the blank periodic table found on page 18 of your packet.
Label the name of and color the group(s) as follows:
ALKALI METALS - RED
ALKALINE EARTH METALS – ORANGE
TRANSITION METALS – YELLOW
METALLOIDS-GREEN
HALOGENS- BLUE
NOBLE GASES - PURPLE

70. Groups/Families of the Periodic Table

71. Learning Guide 4: Families of Elements
The metals in group 1 are called alkali metals.
The metals in group 2 are called alkaline earth metals.
Group 1 and 2 metals easily lose electrons and they are never found free in nature.
Elements in group 1 & 2 have low IE & low EN.
Elements in group 1 form ions with a +1 charge and elements in group 2 form ions with a -1 charge.

72. Learning Guide 4: Families of Elements
6. Reactivity increases as you go down the groups 1 & 2 top to bottom.
7.The most reactive metal is Fr (Francium).
8. Metallic character increases as you go down groups 14,15, 16. (nonmetal  metalliodmetal)
9. The nonmetals in groups 14, 15, 16 are C, N, P, O, S, Se.
10. The metalliods in groups 14, 15, 16 are Si, Ge, As, Sb, Te, Po.

73. Learning Guide 4: Families of Elements
11. The metals in groups 14, 15, 16 are Sn, Pb, Bi, Po.
12. Group 17 elements are called halogens.
13. Group 17 is special because it has all three states of matter: solid (I, At), liquid (Br) and gas (F, Cl.
14. The most reactive element of group 17 is F (flourine).

74. Learning Guide 4: Families of Elements
15. Group 18 elements are called noble gases.
16. Oops 
17. Because they don’t react with other elements – they are snobs.
18. Elements in the same group/family have similar chemical properties because they have the same number of valence electrons.

75. Learning Guide 4: Families of Elements
19. The number of valence electrons is important because they are the electrons that are involved in forming bonds.
20. Each unpaired electron is a bonding site.
21. When determining similar reactivity and trends, elements within the same group will react the same, due to the same number of valence electrons.

76. Learning Guide 4: Families of Elements
For example:
a.) if Na (group 1) & Cl (group 17) react to form NaCl
Then K (group 1) & Cl (group 17) will form KCl

77. Learning Guide 4: Families of Elements
For example:
a.) if Mg (group 2) & Cl (group 17) react to form MgCl2
Then Ca (group 2) & Cl (group 17) will form CaCl2

78. Complete chemdo 4

79. Reactivity of Metals Demo (pg 21)

80. Physical properties of group IA & IIA metals
Complete the following data table by making observations about the physical appearance of the metals shown by the instructor. Include luster(shine), hardness or softness, reaction with air.
Physical properties of group IA & IIA metals
IA (1) IIA (2) Na Mg K Ca

81. Observe the reactions of each metal as the instructor places it in water. Record your observations below.

83. Video demos of alkali metals
Video of sodium in water Video if potassium in water Video of Cesium in water Video of Francium in water

84. Learning Guide 5: Reactivity
As you look down a group the electron configuration gains one more number (ring).
As you look down a group the number of valence electrons stays the same.
Elements in the same group have similar chemicals properties because they have the same number of valence electrons.

85. Learning Guide 5: Reactivity
4. As you go down a group the elements may change from nonmetal metalloid  metal.
5. The metallic characteristics increase as you go down a group.
6. As you go left to right metallic characteristics decrease.
7. Hydrogen may not be considered a member of group 1 because it can also acts as a nonmetal in group 17.

86. Learning Guide 5: Reactivity
8. Hydrogen can have +1 or -1
oxidation states.
9. Group 1 is named alkali metals.
10. Group 2 is named alkaline earth metals.
11. Group 1 & 2 elements are characterized by low electronegativity and high reactivity.
12. Group 1 is more reactive than group 2.

87. Learning Guide 5: Reactivity
13. Groups 14, 15, 16 progress from
nonmetal  metalloid metal.
14. Group 17 is named halogens.
15. Group 17 is the only group
that contains solid, liquid and gas. 
16. Group 17elements are characterized
by high EN and high IE.

88. Learning Guide 5: Reactivity
17. Since small nonpolar molecules are held in solid and liquid phases by weak forces, BP & MP increase as the number of electrons increase.
18. Groups 1, 2, & 17 are never found free in nature because they are too reactive. They will react with anything in the air quickly.
19. They are reduced to their free state by electrolysis: zap them w/ lots of electricity!!

89. Learning Guide 5: Reactivity
20. Group 18 elements were once called the inert gas group because they do not react with other elements, due to a gull valance shell of 8 electrons. They are now called noble gases.
21. The trend in BP going down group 18 is increasing
(look it up on ref. table S: He BP = 4K
Rn Bp =211 K

90. Complete Chemdo 5

91. Never found free in nature: groups 1, 2, 17 Colored ions due to multiple oxidation states: transition metals Strongest Metal: Fr Strongest Nonmetal: F Liquids at RT: Hg & Br

92. Periodic Table Review
Trends across a period L  R, due to increased nuclear charge (val. e- in same energy level) pulling valance electrons closer/tighter
Decreased AR, Increased IE & EN
Trends down a group (top  bottom), due to shielding: more energy levels between nucleus and valence electrons
Increased AR, Decreased IE & EN