4.06 Periodic Table and Periodic...
Transcript of 4.06 Periodic Table and Periodic...
August 20171 4.06 Periodic Table and Periodic Trend
4.06 Periodic Table and Periodic Trends
Dr. Fred Omega GarcesChemistry 100, Miramar College
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The Periodic Table and the ElementsWhat is the periodic table ?What information is obtained from the table ?How can elemental properties be predicted base on the PT ?
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The Periodic TableA map of the building block of matter.
1IA
18VIIIA
11
H1.00797
2IIA Periodic Table 13
IIIA14IVA
15VA
16VIA
17VIIA
2He4.0026
23
Li6.939
4Be9.0122
5B10.811
6C
12.0112
7N
14.0067
8O
15.9994
9F
18.9984
10Ne20.179
311
Na22.9898
12Mg24.305
3IIIB
4IVB
5VB
6VIB
7VIIB
8 9VIIIB
10 11IB
12IIB
13Al26.9815
14Si28.086
15P
30.9738
16S32.064
17Cl35.453
18Ar39.948
419K39.102
20Ca40.08
21Sc44.956
22Ti47.90
23V50.942
24Cr51.996
25Mn54.9380
26Fe55.847
27Co58.9332
28Ni58.71
29Cu63.54
30Zn65.37
31Ga65.37
32Ge72.59
33As74.9216
34Se78.96
35Br79.909
36Kr83.80
537
Rb85.47
38Sr87.62
39Y88.905
40Zr91.22
41Nb92.906
42Mo95.94
43Tc[99]
44Ru101.07
45Rh102.905
46Pd106.4
47Ag107.870
48Cd112.40
49In114.82
50Sn118.69
51Sb121.75
52Te127.60
53I
126.904
54Xe131.30
655Cs132.905
56Ba137.34
57La138.91
72Hf178.49
73Ta180.948
74W183.85
75Re186.2
76Os190.2
77Ir192.2
78Pt195.09
79Au196.967
80Hg200.59
81Tl204.37
82Pb207.19
83Bi208.980
84Po[210]
85At[210]
86Rn[222]
787Fr[223]
88Ra[226]
89Ac[227]
104Ku[260]
105 106 107 108 109
http://www.chemsoc.org/viselements/pages/periodic_table.html
I like to refer to the periodic table as a map of the building block of matter. Consider the value of a map. A map of California for example shows you the terrain and geological information of California. According to the map, the east is the Sierra Nevada, the west is the Pacific Ocean, the north is Portland and south is Baja California. Like wise the periodic table provides valuable information. The PT shows family and periods. The southwest (lower-left) portion of the Periodic table are the most metallic while the northeast (upper-right) is the most nonmetallic. Other information about the periodic table will be describe in this chapter.
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Periodic Tablee- configuration from the periodic periodic table
B2p1
1IA
18VIIIA
1 2IIA
13IIIA
14IVA
15VA
16VIA
17VIIA
2
3 3IIIB
4IVB
5VB
6VIB
7VIIB
8 9VIIIB
10 11IB
12IIB
4
5
6
7
H1s1
Li2s1
Na3s1
K4s1
Rb5s1
Cs6s1
Fr7s1
Be2s2
Mg3s2
Ca4s2
Sr5s2
Ba6s2
Ra7s2
Sc3d1
Ti3d2
V3d3
Cr4s13d5
Mn3d5
Fe3d6
Co3d7
Ni3d8
Zn3d10
Cu4s13d10
B2p1
C2p2
N2p3
O2p4
F2p5
Ne2p6
He1s2
Al3p1
Ga4p1
In5p1
Tl6p1
Si3p2
Ge4p2
Sn5p2
Pb6p2
P3p3
As4p3
Sb5p3
Bi6p3
S3p4
Se4p4
Te5p4
Po6p4
Cl3p5
Be4p5
I5p5
At6p5
Ar3p6
Kr4p6
Xe5p6
Rn6p6
Y4d1
La5d1
Ac6d1
Cd4d10
Hg5d10
Ag5s14d10
Au6s15d10
Zr4d2
Hf5d2
Rf6d2
Nb4d3
Ta5d3
Db6d3
Mo5s14d5
W6s15d5
Sg7s16d5
Tc4d5
Re5d5
Bh6d5
Ru4d6
Os5d6
Hs6d6
Rh4d7
Ir5d7
Mt6d7
Ni4d8
Ni5d8
Electron configuration of an element is simply a listing of how many electrons are in each energy level of the atom for a particular element. The best way to determine of an element is to use the periodic table. In lecture notes 3.5, this was discussed.
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Periodic Table: electron behaviorThe periodic table can be classified by the behavior of their electrons
1IA
18VIIIA
1 2IIA
13IIIA
14IVA
15VA
16VIA
17VIIA
2
3 3IIIB
4IVB
5VB
6VIB
7VIIB
8 9VIIIB
10 11IB
12IIB
4
5
6
7
West (South) Mid-plains East (North)METALS
AlkaliAlkaline
Transition
METALLOID NON-METALSNoble gasHalogensCalcogens
These elementstend to give up
e- and formCATIONS
These elementswill give up e- or
accept e-
These elementstend to accepte- and formANIONS
It is important to note that when writing out the electron configuration for the elements, metals tend to have fewer electrons in their valence orbitals than nonmetals. When atoms try to attain the noble gas electron configuration, they tend to take the path of least resistance. Metals can attain a noble gas electron configuration more easily by losing electrons (therefore becoming cations) while nonmetals will attain a noble gas electron configuration by gaining electrons (therefore becoming anions).
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2. Trend in Atomic RadiusAtomic Radius: The size of at atomic specie is determine by the boundaries of the valence e-. Largest atomic species are those found in the southwest (SW) or bottom-left corner of the periodic table since these atoms have their valence electron found in a higher shell than the proceeding element above it in the periodic table. For example, elements with trends of increasing size goes, Li < Na , K < Rb for the Alkali family. For the chalcogen, the trend is O < S < Se < Te. Te has its valence electrons in the 5th shell and Se has its valence electrons in the 4th shell. Therefore, Te is bigger than O.
Across the periodic table, the atomic radius decreases. The smallest atoms are found in the northeast (NW) or top-right corner of the periodic table. This trend follows Z(effective), which means that for elements in the same period, the valence electrons are all found in the same shell. For a given period, elements to the right (east) of the periodic table have more protons than those to the left (west) of the periodic table. This effectively causes the electron cloud in the valence shell to contract towards the nucleus where they are attracted to the proton. Therefore, the atomic radius decreases across the periodic table. For the third period, the atomic radius essentially goes Al > Si > P > S > Cl > Ar. In this example, Chlorine is smaller than S because although Cl has 7 valence electrons found in the 3rd shell, these electrons are attracted by 17 protons. Sulfur on the other hand has six valence electrons attracted by only 16 protons. Seventeen protons attracting the valence electrons in chlorine is more effective in decreasing the atomic radius than sixteen protons of sulfur.
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3. Trend in Ionization PotentialIonization potential:
Ionization energy increases moving towards the NE corner or top-right corner of periodic table. The lowest ionization energy is towards the SW or bottom-left corner of the periodic table. The ionization energy is opposite the trend of atomic radii. This can be rationalize by thinking about the attraction of the valence electrons to the nucleus where the protons are located. For very small atoms, the valence electrons are closer to the protons and therefore the energy required to remove these valence electrons will be high. For larger atoms, the valence electrons are further away from the nucleus and therefore are not held as tightly. Larger atoms will have smaller ionization energy. There are some anomallies in this general trend that can be explained by how the electrons are arranged in the orbitals.
Exercise - In general the ionization energy increase when moving towards the non mental (right-top) portion of the periodic table. Why is it therefore that the ionization energy for oxygen (1314 kJ/mol is lower in energy than nitrogen 1402 kJ/mol, see table below
Ionization energy or potential energy is defined as the energy required to remove the valence electron from an atomic specie.
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4. Trend in Electron AffinityElectron Affinity:
Electron affinity is defined as the energy released (therefore the negative sign, see table) when an electron is added to the valence shell of an atom.
The electron affinity is most favorable toward NE or upper right corner of periodic table since these atoms will have the greatest tendency to attract electrons. Smaller atoms will have an affinity for electrons more effectively than large atoms. Going from right to left, B, C, N, O, and F, the electron affinity is increasingly negative. The anomallies in the trend, ie., nitrogen, due to the electron placement going into a half-filled p-orbitals.
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Periodic Table Live
http://www.chemeddl.org/resources/ptl/index.php
About Periodic Table Live!: Program that allows a broad range of information about the elements, their reactions, their properties, their structures, and their histories.
Required Components: Apple QuickTime is required to view videos on this site.Suggested Browsers: For the best user experience, we recommend one of the following browsers:
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Summary of TrendPeriodic Table and Periodic TrendsThe periodic table contains valuable information about all atoms responsible for matter in our universe. The
table can be thought of as a map in which information about physical characteristics and chemical behavior can be obtain. The table also organizes the elements in such a matter that trends in chemical behavior and physical properties can be realize. The following are easily obtain from the periodic table.
1. Electron Configuration2. Metallic Character
2. Atomic Radius: Largest toward SW corner of PT
3. Ionization Energy: Largest toward NE of PT
4. Electron Affinity: Most favorable NE of PT
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Summary
Periodic Table: Map of the Building block of matter
Type: Metal, metalloid and Nonmetal
Groupings: Representative or main, transition and
Lanthanide/Actanides
Family: Elements in the same column have similar chemical property because of similar valence electrons
Alkali, Alkaline, chalcogens, halogens, noble gases
Period: Elements in the same row have valence electrons in the same shell.