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Chapt. 5-3
| Question | Answer |
|---|---|
| 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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