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Chapt. 5-3

QuestionAnswer
Difficult to determine size: small, energy level changes two identical chem. bonded and then / number of protons affecting valence Atomic Radii
Atomic Radii decreases to the right due to increased positive charge in nucleus, pulls in Period Trends
Radius increases as you move down GA smaller due to force moving horizontally Group trends
Electrons can be removed froma n atoms if enough energy is supplied (kicking) A+ energy---> A+ + E A+= ion of elements with a positive charge A+ energy---> Ionization
Element with a single positive charge Ion
energy required to remove an electron from it's neutral state Measurements made in gas phase Larger atomic # = less energy Noble gas config= LOTS Of energy D and f block increase across a period, increase down a group Ionization Energy
Energy change that occurs when an electron is acquired by a neutral atom Most atoms release energy when acquiring, others must be forced to gain by using energy Electron affinity
Adding a second electron to a negative ion is difficult All second electron affinities are positive Adding electrons to negative ions
positive ion decrease of electrons smaller cloud, pulled in cation
negative Ion addition of electrons larger cloud, less pull anion
electrons available to be lost, gained, or shared when forming chemicals compounds determines properties Group #-10 for the number of valence electrons Valence electrons
Measure the ability of an atoms in a chem. compound to attract electrons form another compound atom In relation to F Number below on table Not common because of partially filled s-sublevels Electronegativity
Radii decreases along f-block period F-block properties
Created by: jenniferbauer
 

 



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