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Chemistry H.W - Coggle Diagram
Chemistry H.W
Electronegativity
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The tendency of an atom to attract the shared electron much closer to it and it becomes electronegative
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Non-Metallic character
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Much harder for atoms that have greater atomic number to accept electrons as repelling force is greater and distance is greater
Metallic character decreases from left to right while non-metallic period increases down the period due to there being more nuclear force pulling on the electrons while nothing else changes
It increases down the period as most atoms towards the end of the period are able to attain stability by gaining electrons
Ionization energy
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Due to the electromagnetic force it can be told that elements with less electrons in their valence shell will be easier to ionize as the electromagnetic force is weaker
The more right the element is means that the amount of energy required will increase because the nuclear force will increase
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First Ionization energy is the energy required to take a electron from the atom and the second is when it is taken from a + atom
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Ionic Radius
Similar to Atomic Radius with the trends with the greater the period the greater the radius and the more you go right the smaller the atom gets
Cations have smaller ionic radius than the atom while anions have larger ionic radius because in cations the protons pull is more stronger and in anion the number of electrons are more which go further
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Atomic Radius
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Atomic Radius increases as periods increase due to the amount of orbits increasing and there is more distance between the nucleus and the furthest out electron
Atomic Radius decreases as you go among the groups due to the force of attraction increasing as more protons and electrons come into the atom
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