Traits Periodic Element

Traits Periodic Element Some of the periodic properties that will be discussed here are radius atom, energy ionization, electronegativity, affinity electron, characteristic metal, Andpoint melt as well as point boiling. a. Fingers Atom Fingers atom is distance from core atom until skin outermost. For for elements in the same group, the atomic radius decreases as the number goes down large because the number of shells an atom has increases, so skin outermost increasingly Far from core atom. 1 2 11 8 1 2 8 8 8 Na 8 1 18 2 19 K 8 2 37 Rb 8 1 18 18 55 Cs Picture 1. Fingers atoms of Elements Which a period elements in One group, from onto lower increasingly big. means they own fingers own amount skin Which The same. Will but, no atom Which The same also. The more to right location element, proton And electron Which owned increasingly Lots, so that tug core with electron increasingly strong. As a result, the outer electrons are pulled closer towards the nucleus. So, for elements in the same period, the atomic radius increases to the rightincreasingly small. 1 2 8 8 2 19 8 8 2 K Picture 2. Fingers atom elements in one period, In One from left to right increasingly valence small 3 2 20 8 7 18 Ca 2 31 8 18 Ga 35 Br group, configuration elements One group have amount electron The same And amount skin increase. As a result, the distance between the valence electrons and the nucleus increases, so that fingers atom in One group increasingly to lower increasingly big . So can concluded: 1) In One group, fingers atom increase big from on tolower. 2) In One period, fingers atom increasingly small from left to right. a. Ionization Energy Ionization energy is the energy required to release electron outermost something atom. Energy ionization This stated in unitkJ mol –1 . Elements Which group, energy ionization increasingly to lower gets smaller because the outermost electrons are farther from the nucleus (attractive force core increasingly weak), so that electron outermost increasingly easy released. Meanwhile, for elements in the same period, the attraction of the core increases right increasingly strong, so that energy ionization on generally increasinglyto right increasingly big. There is a number of exception Which need noticed. Group IIA, VA, And VIIIA it turns out have energy ionization Which very big, even more big than energy ionization element in adjacent right, namely IIIA and VIA. This happens because the elements of group IIA, VA, and VIIIA have relatively stable electron configurations, so that electron hard released. 2,500 He Periode 2 Periode 3 Ne Periode 4 Periode 5 Periode 6 Energi Ionisasi (kJ mol–1) 2,000 F Ar 1,500 N Kr P C Be B Xe Cl O H As As Ge Ga S Mg Si Al Li Ca Na K 0 10 18 Ga Rn I Te Sb Pb Sn Sr Tl In Ba Rb 1000 Po Lu Bi Ra Cs 36 54 Number Atom Picture 3. Connection energy ionization with number atom. 86 500 c. Electronegativity Electronegativity is the ability or tendency of a atom For catch or interesting electron from atom other. For example, fluorine has a tendency to attract electrons more strongly than hydrogen. So, can concluded that electronegativity fluorine more big than hydrogen. Draft electronegativity This First time submitted by Linus Pauling (1901 – 1994) on year 1932. Elements Which group, electronegativity increasingly to lower increasingly small because style pull core increasingly weak. Whereas elements Which a period, electronegativity increasingly to right increasingly big . Will but need remembered that group VIIIA No have electronegativity. This is because it already has 8 electrons in its shell outermost. So electronegativity biggest is at on group VIIA. Mark Electronegativity Elements IA 1 H 2,1 3 Li 1,0 11 Na VIIIA IIIA IVA VA VIA IIA 4 Be 1,5 12 Mg 0.9 1,2 IIIB IVB VB 19 20 21 22 23 K Ca Sc Ti V 0.8 1.01 1.3 1.5 1.6 37 38 39 40 41 Rb Sr Y Zr Nb 0.8 1.0 1,2 1.4 1.6 55 56 57 72 73 Cs Ba La Hf Ta 0.7 0.9 1.1 1.3 1.5 87 88 89 Fr0.7 Ra0.9 Air conditi oning 1.1 VIIIB VIB VIIB 24 Cr 1.6 42 Mo 1.8 74 W 1.7 25 MnFe 1.5 43 Tc 1.9 75 Re 1.9 26 _ 1.8 44 Ru 2.2 76 Os 2.2 IB 27 Co 1.8 45 Rh 2,2 77 Ir 2,2 28 Ni 1.8 46 Pd 2,2 78 Pt 2,2 5 B 2,0 6 C 2,5 7 N 3,0 8 O 3,5 13 Al 14 Sl 1.5 31 No 1.6 49 In 1.7 81 Tel 1.8 15 P 1.8 32 Ge 1.8 50 Sn 1.8 82 PB 1.8 16 S 2.1 33 US 2.0 51 SB 1.9 83 Ms 1.9 IIB 29 30 CuHZn _ 1.9 1.6 47 48 Ag Cd 1.9 1.7 79 80 Au Hg 2.4 1.9 2 He VIIA – 9 10 F Ne 4,0 – 17 18 Cl Ar 2.53.0 3435 SeBr 2,42.8 5253 TeI 2.12.5 8485 PoAt 2.02,2 – 36 Cr – 54 Xe – 86 Rn – d. Affinity Electron Affinity electron is energy Which join process addition1electron on One atom neutral in form gas, so that formedion charged –1 . Affinity electron Also stated in kJ mol –1 .Element Which own affinity electron marked negative, means have trend more big in absorb electronthan element Which affinity the electron marked positive. More and more negativemark affinity electron, so increasingly big trend element thein absorb electron (trend form ion negative). From characteristic This can concluded that: 1) Within a group, the electron affinity tends to decrease from on to lower. 2) In one period, the electron affinity tends to increase from left to right. 3) Except for alkaline earth elements and noble gases, all group elements main have affinity electron marked negative. Affinity electron biggest owned by group halogen. Affinity elektron Elements on Group Main Group Period HE 1 2 H –73 Li –60 IIA Be 240 IIIA B –27 IVA VA C N –122 0 VIA O –141 VIIA VIIIA He's 21 F Ne –328 29 3 4 5 6 Na –53 K –48 Rb –47 Cs –30 Mg 230 Ca 156 Sr 168 Ba 52 Al –44 No –30 In –30 Tel –30 Si –134 Ge –120 Sn –121 PB –110 P –72 US –77 SB –101 Ms –110 S Cl –200 –349 Se Br –195 –325 Te I –190 –295 Po At –180 –270 Ar 35 Cr 39 Xe 41 Rn 41 e. Characteristic Metal By chemistry, characteristic metal linked with electronegativity, that is trend let go electron form ion positive. So, characteristic metal depends on energy ionization. Reviewed from configuration electron, element- element metal tend release electron (own energy ionization Which small), whereas elements No metal tend catch electron (own electronegativity Which big). According to the trend of ionization energy and electron gatifan, so characteristic metal-nonmetal in periodic element is: 1) From left to right in one period, the metallic properties decrease, whereas characteristic nonmetal increase. 2) From top to bottom in a group, metallic properties increase, whereas characteristic nonmetal reduce. So, the metal elements are located at the bottom-left part of the system periodic element, whereas elements nonmetal located on part top right. The boundaries between metals and nonmetals in the periodic system are frequent depicted with ladder diagonal striped thick , so that element- elements around the border area between metals and nonmetals has both metallic and non-metallic properties. those elements called element metalloids . For example is boron And silicone. Besides That, characteristic metal Also relate with reactivity something element. Reactive It means easy react. Elements metal on system periodic element increasingly to lower the more reactive (more easy react) Because the more easy release electron. On the contrary, elements No metal on system periodic increasingly to lower increasingly not enough reactive (more hard react) Because the more hard catch electron. So, The most reactive metal elements are group IA (alkali metals) And element nonmetal Which most reactive is group VIIA (halogen). f. Point Melt And Point Boiling Based on the melting point and boiling point it can be concluded as following. 1) In One period, point liquid And point boiling go on from left to right until group IVA, then drops drastically. Liquid point and pointboiling Lowest owned by element group VIIIA. 2) In One group, it turns out There is two type trend: element- element group HE – IVA, point liquid And point boiling increasingly low fromtop to bottom; elements of groups VA – VIIIA, melting point and point he boiled increasingly tall.