C. Sifat Logam dan Non Logam serta Sifat Keperiodikan unsur Kimia

 The student can dicrimination metal and non metal properties.  The student can explain few elements metalloid.  The student can explain the atomic radius signification.  The student can explain in the same group the atomic radius.  The student can explain in the same period the atomic radius.

 The students can explain the electron affinity signification.  The student can explain in the same group the electron affinity.  The student can explain in the same period the electron affinity.  The student can explain the ionization potential signification.  The student can explain in the same group the ionization potential.  The student can explain in the same period the ionization potential.

Elements are classified as:  Metals  Nonmetals  Metalloids

 Good conductors of heat and electricity  Shiny; High melting points  Malleable (bends easily)  Ductile (can be made into wires)  Found on the LEFT of the periodic table  Not brittle  Mostly on solid form, except for mercury which has liquid form.

 Dull  Brittle (hard/ easily broken)  Found on the RIGHT of the periodic table

Nonmetals Brittle Do not conduct electricity

 Has properties of both metals and nonmetals  Found touching the dark, zig-zag line  Metalloid means “metal-like”  Boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium(Te), polonium (Po), astatine (At).

 The electron configuration of atom can be used to determine an atom position in periodic table. Group number = valence electron Period number = number of shell filled with electron Example : 35 Br Konfigurasi elektronnya Elektron valensinya : 7Golongan VIIA Jumlah kulit : 4Perioda : 4

What are semiconductors used in?

 Atomic radius is the distance between outermost electron to the nuclei of the atom.  In the same group the atomic radius increases from up to bottom  In contrary, the atomic radius within the same period, from left to right, is generally decreasing.

H 37 He 54 Li 15 6 Be 105 B 91 C 77 N 71 O 60 F 67 Ne 80 Na 18 6 Mg 160 Al 14 3 Si 117 P 111 S 10 4 Cl 99 Ar 96 K 23 1 Ca 197 Sc 16 1 Ti 15 4 V 131 Cr 12 5 M n 118 Fe 125 Co 12 5 Ni 12 4 Cu 128 Zn 13 3 Ga 12 3 Ge 122 As 116 Se 115 Br 114 Kr 99 Rb 24 3 Sr 215 Y 18 0 Zr 16 1 Nb 147 Mo 13 6 Tc 13 5 Ru 132 Rh 13 2 Pd 13 8 Ag 144 Cd 14 9 In 15 1 Sn 140 Sb 14 5 Te 13 9 I 138 Xe 10 9 Cs 26 5 Ba 210 Hf 15 4 Ta 143 W 13 7 Re 13 8 Os 134 Ir 13 6 Pt 13 9 Au 144 Hg 14 7 Tl 18 9 Pb 175 Bi 15 5 Po 16 7 At 145 Rn La 18 7 Ce 183 Pr 18 2 Nd 18 1 Pm 181 Sm 18 0 Eu 19 9 Gd 179 Tb 17 6 Dy 17 5 Ho 174 Er 17 3 T m 17 3 Yb 194 Lu 17 2 Atomic Radius (pm) 1pm=1x m

 Electron affinity is the released used energy by an atom in gas form, after it accepts an electron.  For example when chlorine gas accepts an electron to from negative ion, it releases energy, Cl2(g) + 2e 2Cl - the energy change associated with the addition of an electron to a gaseous atom.

 In the same period from left to right, affinity has increasing tendency.  In the same group, from bottom to up, affinity has increasing tendency

 Ionization potential is defined as the minimum energy required for ionizing an isolated gaseous atom to produce positive ion. Na (g) Na + + e

 The ionization potential in the same period from left to right has increasing tendency.  In the same group from up to bottom, the ionization potential has decreasing tendency.

 The tendency of every element for attracting is defferent.  This value is called electronegativity  Whithin the same period, the trend shows ascending pattern form left to right.  Whithin the same group, from up to bottom, it shows descending pattern.

H 2.1 Li 1.0 Be 1.5 Na 0.9 Mg 1.2 Al 1.0 K 0.8 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0 Al 1.5 Si 1.8 P 2.1 S 2.5 Cl 3.0 Ne - Ar - He - Increase in electronegativity Decrease

m.p./ o C Atomic number C Si He Ne Ar Ca

H -259 Li 180 Be 1280 Na 97.8 Mg 650 Ca 850 K 63.7 B 2300 C 3730 N -210 O -218 F -220 Al 660 Si 1410 P 44.2 S 119 Cl -101 Ne -249 Ar -189 He -270 Unit: o C Increase