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| Effectice Nuclear Charge is the key to |
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| predicting periodic trends, higher the charge, the more pull to the nucleus |
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| ions that have same number of electrons |
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| If all aoms are isoelectronic, the smallest in ionic radii is |
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| the one with most protons |
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| It is hard for Na to go from level 1 to level 2 because |
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| it has a full valence shell and is very hard to pull one off |
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| Ionization Energy increases |
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| Ionization energy increases across a period becuase |
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| ENC is higher so the electrons hold on tighter! |
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| Electron affinity process is likely to occur if the atom is |
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| Larger value of electron affinity = |
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| more energy given off= more stable |
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| change in energy when an electron is added to a gaseous atom to form an anion |
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| EA becomes less negative as you |
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| move down a group bc higher effective nuclear charge, less shielding, closer to nucleus! |
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| Higher Electron Affinity = more likely to |
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| Electronegativity is the measure of |
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| relative tendency of an atom to attract itself when chemically combined with another element |
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| Noble gases aren't very electronegative becuase |
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| they don't want any more electrons |
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| Electronegativy is measured on ___ scale |
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| anions of the compound are larger in ionic radii than |
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| nonmetal to nonmetal bonding |
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| which typically loses electrons? |
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| naming a covalent bond you give it |
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| prefixes like mono di tri tetra |
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| crystal lattice energy is always |
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| crystal lattice energy is the energy change |
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accompanying the formation of one
mole of formula units in the crystalline state
from constituent particles in the gaseous state. |
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| angular mg can only be formed from |
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| trigonal bipyramidal with 4 bonded pairs molecular geometry is |
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| octrahedral with 3 bonded pairs molecular geometry is |
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