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The Periodic Table
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The Periodic Table
Table of Contents
1.0 The Periodic Table......................................................................................................... 3
1.1 History.......................................................................................................................... 3
1.2 Description of the Modern Periodic Table........................................................... 3
1.3 Classification of Elements......................................................................................... 4
1.4 Atomic Number and Mass Number........................................................................ 9
2.0 Some Periodic Properties of Elements...................................................................10
2.1 The Sizes of Atoms..................................................................................................10
2.2 Ionic Radius ...............................................................................................................12
2.3 Ionization Energy......................................................................................................12
2.4 Electron Affinity........................................................................................................13
2.5 Metallic Character....................................................................................................14
3.0 Quiz................................................................................................................................. 15
The Periodic Table 2
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1.0 The Periodic Table
1.1 History
Dmitri Mendeleev and Lothar Meyer independently proposed in 1869 the periodic law. This law
states that when the elements are arranged in order of increasing atomic mass, certain sets of
properties recur periodically. Many scientists during the time of Mendeleev and Meyer have
attempted to come up with a systematic arrangement of the elements. Mendeleev succeeded
where others failed for two reasons. First, Mendeleev left blank spaces in his table for undiscovered
elements. Second, he corrected previously erroneous atomic mass values. Two of the atomic mass
values he corrected were those of indium and uranium. The blanks in the periodic table that
Mendeleev created came at atomic masses 44, 68, 72, and 100. He predicted that the blanks are
those of the elements that were soon to be discovered. Shortly after the appearance of his 1871
periodic table, two of the elements Mendeleev predicted were discovered. In Mendeleev’s table,
similar elements fall in the same vertical groups. The properties of these elements changed
gradually from top to bottom in a group.
1.2 Description of the Modern Periodic Table
The modern periodic table arranges the elements in 18 groups, called the “long” form. The vertical
arrangement of elements is called a group or family. The horizontal row of elements is called a
period. A group number is located at the top of the periodic table while the period number is on
the left. The first two groups (groups 1 and 2) in the periodic table are known as the s-block. The
last six groups (groups 13 to 18) belong to the p-block. Together, the s-block and the p-block
constitute the main group elements. Elements in the inner lower box (groups 3 to 12) of the
periodic table are known as the transition elements or the d-block. The f-block elements are the
elements extracted from the periodic table. They are the two rows of elements below the main
periodic table. The upper row is known as the lanthanides. They belong to period 7. Elements in
the lower row are called the actinides. They belong to period 8. Together the actinides and the
lanthanides are called the inner transition metals. The group and period numbers aid in the location
and classification of elements. For example, the element in group 2 and period 4 is calcium. The
element in group 17 and period 2 is the highly reactive halogen fluorine.
3 The Periodic Table
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The Modern Periodic Table
Group → 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
↓ Period
1 1 2
H He
2 3 4 5 6 7 8 9 10
Li Be B C N O F Ne
3 11 12 13 14 15 16 17 18
Na Mg Al Si P S Cl Ar
4 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
5 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
6 55 56 * 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
7 87 88 ** 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Uub Uut Uuq Uup Uuh Uus Uuo
8 119 120
Uue Ubn
Lanthanides 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Actinides 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103
Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Atomic numbers of solids are in black. Those of liquids are in blue, and those of gases are in red.
1.3 Classification of Elements
The elements are classified as metals, nonmetals, and metalloids. The periodic table is divided by a
zigzag line on the right portion. On top of this zigzag line are the elements boron (B), silicon (Si),
arsenic (As) and tellurium (Te). Under the zigzag line, you will find aluminum (Al), germanium (Ge),
antimony (Sb), and polonium (Po). Elements in olive green colored blocks are the metalloids. To
the left of the zigzag line are the metals. To the right are the nonmetals. Most metals are good
conductors of heat and electricity. They are also malleable and ductile. They have moderate to high
melting points. In general, nonmetals are non-conductors of heat and electricity. They are usually
The Periodic Table 4
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