Term
| The atomic radius is affected by: |
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Definition
| the # of protons and shells |
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Definition
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Term
| As you go across the periodic table... |
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Definition
the number of protons in each element goes down, therefore the atomic radii get smaller |
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Term
| As you go down the periodic table... |
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Definition
shells are added to the atom making the radii larger |
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Term
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Definition
| The energy required to remove an electron from an atom: 500 kj/mol |
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Term
| Factors that affect the ionization energy of an atom |
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Definition
| # of valence electrons, protons, and shells (distance increases/shielding effect) |
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Term
| As you go across the periodic table, the ionization energy... |
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Definition
| goes up because you are adding more protons, therefore the attraction between the outermost electron and the protons is stronger, making it harder to pick off that electron |
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Term
| As you go down the periodic table, the ionization energy... |
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Definition
| goes down because you are adding more shells, making it easier to pull off the outermost electron because of shielding |
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Term
| Define the shielding effect |
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Definition
| when electrons shells block the outermost electron from the attraction of the protons in the nucleus |
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Term
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Definition
| The relative tendency of an atom to attract electrons to itself when it's bonded to another atom. |
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Term
| If the electronegativity difference between two atoms is... |
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Definition
| under 1.67, the bond is polar covalent, over 1.67, the bond is ionic, 0, the bond is pure covalent |
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