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28 Cards in this Set
- Front
- Back
Addition Reaction |
when double bonds are changed to single bonds (Fig 3.10), with the addition of H |
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Allotrope |
one of 2 or more forms of an element (eg, diamond and graphite) |
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Bond energy |
Strength of a bond, measured in joules |
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Condensed structure |
representative shorthand of atomic groups (103) |
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Delocalization |
alternating pattern of single and double bonds (Soccer ball) that allow electrons to spread out & diffuse over areas of alternation, common in carbon containing molecules and adds stability in Resonance stabilization) |
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Doping |
adding to semi-conducting elements in order to adjust their reactivity |
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Double bond |
pair of bonds, each containing 2 electrons for a total of 4 shared electrons |
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Electron dot structure |
sketch model indicating the position of all valence electrons in a molecule. |
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Electron pair geometry |
similar to Molecular Geometry but containing non-binding pairs which are not part of MG
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Electron pair geometry |
similar to Molecular Geometry but containing non-binding pairs which are not part of MG |
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Full structure |
long hand description of molecular structure |
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Joule |
electrical charge measurement |
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Line structure |
notation/sketch of molecule structure that simplify representation of H & C |
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Molecular geometry |
3D model of the repulsion of electrons
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Nanotube – |
cigar shaped Carbon cage. |
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Network solid |
solid with a extended system of repeated covalent bonds. Strong 3 dimensional network. |
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Nonbonding pair |
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Octet rule |
states that each atom needs 8electrons in its valence |
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Resonance stabilization |
the additional stability that comes from delocalization |
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Saturated Molecule |
Contains only single bonds and will not accept additional H (Hydrogen) |
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Semiconductor |
conducts in specific circumstances, like Silicone in light. Can be “doped” to alter/enhance reactivity. |
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Shortened structure |
shorthand for molecular structure, specifically of methyl groups, which tend to be organic. eg, -CH3instead of |
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Tetrahedron |
Pyramid like (4 point) carbon atom depiction |
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Triple bond |
triplet of bonds, each containing two electrons for a total of six electrons |
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Uniqueness principle |
regarding proximity of electrons to nucleus. Period 2 are small and have only a few, but very close electrons. |
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Unsaturated Molecule |
Containing one or more multiple bonds where Hydrogen (H) can be added to make multiple bonds into single bonds |
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VSEPR theory |
suggests that all atoms surrounding a central atom are trying to get away from each other. Repelling of electrons. |
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BONDING RULES FOR ELEMENTS IN UNCHARGED ORGANIC MOLECULES |
H---1 O---1 S---2 N---3 C---4 |