20366665
Descripción
Fichas por kadyn drummond, actualizado hace más de 1 año
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Creado por kadyn drummond
hace más de 4 años
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| Pregunta | Respuesta |
| Atomic Radius across a period | There is a decrease in atomic radii as you move left to right across a period this is due to the increase of nuclear charge and an increase in the number of electrons. |
| Atomic Radius down a group | Atomic radii increases as you move down a group due to an increase in the number of mainshells and an increase in shielding effect. |
| Ionic Radius across a period | Ionic Radius decreases across a period to group 15 where it increases and then it decreases again. |
| Ionic Radius down a group | Ionic Radius increases down a group due to more mainshells of electrons and increase in shielding effect. |
| Ionization Energy across a period | Ionization Energy increases across a period due to an increase in nuclear charge and a smaller radius. |
| Ionization Energy down a group | Ionization Energy decreases down a group because the electrons are farther from the nucleus causing a greater shielding effect. |
| Electronegativity across a period | Electronegativity increases across a period due to an increase in nuclear charge and the decrease in atomic radius, the nucleus has a greater pull on the nucleus. |
| Electronegativity down a group | Electronegativity decreases down a group due to an increase in the mainshells and increase in shielding effect, the pull of the nucleus on the electrons is lessened. |
| Electron Affinity across a period | Electron Affinity increases across a period because of the increase in nuclear charge and the smaller radius makes it easier to pull an electron into the valence shell. |
| Electron Affinity down a group | Electron Affinity decreases down a group because the valence shell is farther away from the nucleus and there is more shielding effect. |
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