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15 Cards in this Set
- Front
- Back
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Why are the ionization energies of the Noble Gases so high? |
Noble gases have a complete outer main energy level and are very stable. They would require lots of energy to remove an electron |
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Explain the trend in Atomic Radius as you go down a group. |
As you go down a group the atomic radius increases b/c atoms are adding in main energy levels. |
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Why does Ionization energy increase with decreasing atomic radius? |
Smaller atoms gave a stronger attraction between the nucleus and valence electrons, so they have higher ionization energy. |
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Define Electronegativity |
A measure of the ability of an atom in a chemical compound to attract electrons. |
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Define Ionization energy |
The energy required to remove one electron from a neutral atom of an element. |
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Define Atomic Radius |
1/2 the distance between the nuclei of identical atoms that are bonded together (Atomic Size) |
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What group are the Alkali Metals located in and what is their description? |
- Group 1 |
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What group are the Alkaline Earth Metals located in and what is their description? |
- group 2 - |
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What group are the Transition Metals located in and what is their description? |
- whole d block |
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What group are the Lanthanides and Actinides located in and what is their description? |
- Lanthanides are located in the 1st row of the F Block - Actinides are located in the 2 row of the F Block |
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What group are the Metalloids located in and what is their description? |
- B, Si, Ge, As, Sb, Te |
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What group are the Halogens located in and what is their description? |
- Group 17 |
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What group are the Noble Gases located in and what is their description? |
- Group 18 |
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What group are the Metals located in and what is their description? |
- Group 1-16 |
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What group are the Non-Metals located in and what is their description? |
- Group 14-18 |
