Chapt. 5-3
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Difficult to determine size: small, energy level changes two identical chem. bonded and then / number of protons affecting valence | Atomic Radii
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| Atomic Radii decreases to the right due to increased positive charge in nucleus, pulls in | Period Trends
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| Radius increases as you move down GA smaller due to force moving horizontally | Group trends
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| 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
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| Element with a single positive charge | Ion
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| 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
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| 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
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| Adding a second electron to a negative ion is difficult All second electron affinities are positive | Adding electrons to negative ions
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| positive ion decrease of electrons smaller cloud, pulled in | cation
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| negative Ion addition of electrons larger cloud, less pull | anion
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| electrons available to be lost, gained, or shared when forming chemicals compounds determines properties Group #-10 for the number of valence electrons | Valence electrons
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| 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
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| Radii decreases along f-block period | F-block properties
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Created by:
jenniferbauer
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