Ionic Radius Ionic Radius
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SOR1 Ionic Radius Ionic Radius How do I remember this????? The more electrons that are lost, the greater the reduction in size. Li+1 Be+2 protons 3 protons 4 electrons 2 electrons 2 Which ion is smaller? Ionic Radius How do I remember this??? The more electrons that are gained, the greater the increase in size. P-3 S-2 protons 15 protons 16 electrons 18 electrons 18 Which ion is smaller? Ionization Energy Ionization Energy – energy needed to remove outermost e- Ionization Energy Group Trend – As you go down a column , ionization energy decreases As you go down, atomic size is increasing (less attraction), so easier to remove an e- Periodic Trend – As you go across a period (L to R), ionization energy increases As you go L to R, atomic size is decreasing (more attraction), so more difficult to remove an e- (also, metals want to lose e-, but nonmetals do not) Electronegativity Electronegativity- tendency of an atom to attract e- Electronegativity Trend Group Trend – As you go down a column, electronegativity decreases As you go down, atomic size is increasing , so less attraction to its own e- and other atom’s e- Periodic Trend – As you go across a period (L to R), electronegativity increases As you go L to R, atomic size is decreasing, so there is more attraction to its own e- and other atom’s e- Oxides Generally can be prepared by direct combination of elements with oxygen slowly at room temperature Oxidation number of the oxides 1) The oxidation number of elements in its oxides corresponds to the number of electrons used for bonding . 2) The maximum oxidation number is the same as the group number to the total number of outermost electrons used for bonding 3) Oxidation numbers of elements for their oxides are always positive - oxygen are more electronegative 4) P and S show several oxidation numbers as - has energetically available 3d subshells - for expansion of octet Достарыңызбен бөлісу:
