Term
| Max electrons in each orbital |
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Definition
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Term
| At equilibrium, the Gibbs free energy of the phases are _____. |
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Definition
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Term
For a spontaneous process the change in the
Gibbs free energy is ____ |
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Definition
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Term
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Definition
1. Ionic
2. Covalent
3. Metallic |
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Term
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Definition
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Term
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Definition
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Term
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Definition
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Term
| As the electronegativity difference increases, the % ionic character ___. |
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Definition
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Term
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Definition
| The energy required to lose an electron from a neutral atom. |
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Term
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Definition
| The energy given off when a neutral atom attracts an electron to become a negative ion. |
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Term
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Definition
| The ability of an atom in a molecule to draw bonding electrons to itself. |
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Term
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Definition
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Term
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Definition
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Term
| Delocalized electrons (which is what metallic bonds have) |
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Definition
| Electrons in a molecule, ion or solid metal that are not associated with a single atom or a covalent bond. |
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Term
| On Bond-Force Curve, steeper curve ___ bondings and ___ Young's Modulus. |
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Definition
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Term
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Definition
| The minimum size that must be formed by atoms or molecules clustering together |
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Term
| Change in electronegativity from ionic to covalent occurs at what number? |
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Definition
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Term
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Definition
1. van der Waals
2. Hydrogen |
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Term
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Definition
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Term
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Definition
Permanent dipole
Form whenever hydrogen bonds with strong electronegative atoms |
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Term
| For the critical radius ratio, do anions need to touch each other? |
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Definition
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Term
| Arrhenius Equation Formula |
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Definition
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Term
| The asymmetry in the bond energy curve is related to the ______ of the material. |
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Definition
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Term
| Which quantum number contributes to magnetic properties? |
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Definition
| Magnetic spin and angular momentum |
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Term
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Definition
| The tendency of matter to change in shape, area, and volume in response to a change in temperature, through heat transfer. |
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Term
| Deep energy trough, ____ thermal expansion. |
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Definition
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