1. The Periodic Table
Chapter 6

2. Mendeleev’s Periodic Table
Arranged the elements in the periodic table in order of increasing mass
Mendeleev’s Periodic Table

3. Modern Periodic Table elements are arranged in order of increasing atomic number Groups = columns 1-18 elements have similar properties Periods = rows 1-7 equal to the principal energy level
The Periodic Law

5. Period →
Group ↓

6. Three ways to classify elements
Elements can be classified into metals, nonmetals, and semimetals.
Elements can also be classified into groups or families.
You should be able to do both.
Semimetals

7. Properties of Metals
Metals are good conductors of heat and electricity.
They are shiny and lustrous.
Metals can be pounded into thin sheets (malleable) and drawn into wires (ductile).
Metals do not hold onto their valence electrons very well. They have low electronegativity.

12. Properties of Nonmetals
Nonmetals are poor conductors of heat and electricity.
Exception: graphite is a good conductor.
Nonmetals are brittle. If you hit them with a hammer, they shatter and turn to powder.
Good examples of nonmetals are sulfur, carbon, and all the gases.

13. More on Nonmetals The seven diatomic molecules are all nonmetals.
Remember that hydrogen is a nonmetal even though it is located on the left side of the table with the metals.
Nonmetals strongly attract their electrons. They have high electronegativity values and therefore form negative ions.
Br2I2N2Cl2H2O2F2

14. Semimetals Si
These elements have properties that are in- between those of the metals and nonmetals.
They are very important for making transistors and computer chips.
Silicon (Si), germanium (Ge), and tellurium (Te) are shown.
Different books include polonium (Po) and leave out astatine (At). Te Ge

15. Semimetals are also called metalloids.

17. METALS Metals and Nonmetals Nonmetals Metalloids H He Li Be B C N O F1 He 2 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2
Nonmetals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4
METALS Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5
Metalloids Cs 55 Ba 56 He 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 6 * Fr 87 Ra 88 Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109 7 W La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm
100 Md
101 No
102 Lr
103

18. decreases increases Reference Table Periodic Table Trends:
1. Across a period, metallic character →
Why?
More electrons in outer shells
Less tendency to lose electrons
2. Down a group, metallic character →
Electrons are in outer shells further from the nucleus
Greater tendency to lose electrons
decreases
increases

19. Which of these sets of elements have similar physical and chemical properties?
oxygen, nitrogen, carbon, boron
strontium, magnesium, calcium, beryllium
nitrogen, neon, nickel, fluorine
Name 2 elements that have properties similar to those of the element sodium.
Any other Group 1 element:
Lithium, Potassium, Rubidium, Cesium, Francium

20. Metallic Review Metal Metalloid Nonmetal Metal
Identify each element as a metal, nonmetal or metalloid
Gold -
Silicon -
Sulfur -
Barium -
Metal
Metalloid
Nonmetal
Metal

21. Identify each property below as more characteristic of a metal or a nonmetal
Brittle -
Malleable -
Poor conductor of electricity -
Shiny -
Tend to gain electrons -
In which pair of elements are the chemical properties of the elements most similar?
sodium and chlorine
nitrogen and phosphorus
boron and oxygen
Nonmetal
Metal
Nonmetal
Metal
Nonmetal

22. Classifying the Elements
Alkali Metals –
Alkaline Earth Metals –
Halogens –
Noble Gases –
Representative Elements –
Transition Elements –
Group 1 (1A)
Group 2 (2A)
Group 17 (7A)
Group 18 (8A) Inert gases
Groups 1,2 and 13-17
All Groups 3-12 (B)

24. Label your Reference Periodic Table…1 18 H 1 He 2 1 2 13 14 15 16 17 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 3 4 5 6 7 8 9 10 11 12 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Cs 55 Ba 56 He 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 6 * Fr 87 Ra 88 Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109 7 W La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm
100 Md
101 No
102 Lr
103

25. Classifying Review Which of the following are transition metals? Cu SrCd Au Al Ge Co

26. Periodic Trends Trends in Atomic Size Trends in Ionization Energy
Trends in Ionic Size
Trends in Electronegativity

27. Trends in Atomic Size
Atomic Radius – one half of the distance between the nuclei of two atoms of the same element

28. Trends in Atomic Size Found on table S Group Trends in Atomic Size
From top to bottom the size trends increases
Why?
The number of shells (rings) increases
Valence electrons get shielded from the nuclear pull
Period Trends in Atomic Size
From left to right the size trends decreases
The size of the rings stay the same
The number of protons increase and pull from nucleus is strong

29. Trends in Atomic Size

30. Sample Exercise
Which element in each pair has atoms with a larger atomic radius?
or lithium
or magnesium
Carbon or
or oxygen
Arrange these elements in order of decreasing atomic size: sulfur, chlorine, aluminum, and sodium.
Sodium
Strontium
germanium
Selenium
Sodium  Aluminum  Sulfur  Chlorine

31. ions
Form when electrons are transferred between atoms An ion with a positive charge (lost electrons) is called a An ion with a negative charge (gained electrons) is called an Ionization Energy - the energy required to remove an electron from an atom
cation
anion

33. Ionization Energy Found on table S
The ability to become a positive charge
Group Trends in Ionization Energy
From top to bottom IE decreases (easier to take away e-)
Why?
More layers of shells (rings)
Nucleus is too weak to pull in valence
Period Trends in Ionization Energy
From left to right IE increases
Same amount of shells (rings)
Nuclear pull increases, ring becomes smaller

34. Ionization Energy This is the energy needed to remove an electron.
It is easier to remove an electron from a larger atom because the electron is farther from the nucleus and feels less attraction.

35. Ionization energy Practice
Which element in each pair has a greater first ionization energy?
Lithium or
or strontium
Cesium or
Arrange the following groups of elements in order of increasing ionization energy.
Be, Mg, Sr
Bi, Cs, Ba
Na, Al, S
boron
Magnesium
aluminum
Sr  Mg  Be
Cs,  Ba  Bi
Na  Al  S

36. Trends in ionic Size Ion – When an atom loses or gains electrons
Cation
When an atom loses an electron (becomes positive)
Radius becomes smaller than the original atom
Why?
There is less repulsion between the electrons.
Anion
When an atom gains an electron (gains electron)
Radius becomes bigger than the original atom
There is more repulsion between electrons

38. Trends in ionic Size Practice
Which particle has the larger radius in each atom/ion pair?
or Na+
S or
I or
or Al3+
In each pair, which ion is larger?
or Mg2+
Cl- or
or Cu2+ Na
S2- I- Al
Ca 2+
P3-
Cu+

39. Trends in Electronegativity
The ability of an atom to attract an electron Found on table S Group Trends in Electronegativity From top to bottom; electronegativity values decrease Why? More atomic shells (rings) Weaker nuclear pull Periodic Trends in Electronegativity From left to right; electronegativity values increase Shells (rings) stay the same Stronger nuclear pull

41. Trends in Electronegativity Practice
Which element in each pair has a higher electronegativity value?
Cl or
C or
or Ne
or Ca
Which element in each pair has a greater attraction for electrons?
Ca or
O or
H or
K or F N Mg As O F O S

42. Periodic Property
Across a Period
Down a Group
Metallic Character
Decreases
Increases
Atomic radius
Ionization energy
Ion Size
Electronegativity