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7 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Atomic Radius |
The distance between the center of the atom to the valence shell. |
The weird one |
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Trend of Atomic Radius |
Increases from right to left because more electrons( and protons) are put into same subshell. Increase in protons increases postive charge making electrons pull closer and atomic radius to decrease. Increases down a family because more electrons are added to higher energy level( more shells) and electrons are futher. |
Subshells, Electron pull, Atomic radius increase and decrease |
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Electron Affinity |
Energy either absorbed or released during additon of electron to neutral atom. If energy is needed to add an electron the ion will be unstable and loose the electron. If energy is released the Ion will be stable. |
Energy absorbtion |
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Electron Affinity Trend |
Increases from left to right because more energy is needed to gain electrons. Increases up a group because energy is released when electron is added. Higher electron affinity equals higher reaction. |
Release and Gain. Metals have low affinty. High negative equals high affinty and reactive |
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Ionization Energy |
Energy it takes to overcome the attractive force of the (positive) nucleus. |
to pull electron from the neutral atom |
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Ionization Energy trend |
Increases up because number of orbits increase and valence is further from nucleus. decrease across (left to right) because + and - increase and atoms don't want to give up electons. Atoms that give away electrons easily have low ionization and are usually on the left side. |
Noble gases have the highest |
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Electronegativity |
Measures attracting ability. High number= high attractions. Non metals have higher. Non metals=pure. |
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