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Definition
| Schrodinger discovered that each of these corresponds to a different mathematical description of the electron wave. |
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Term
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| A wave function (psi). In terms of probability (psi^2) of finding an electron at some point relative to the nucleus, as the volume inside the boundary surface of an atom, or the region in space where the probability of finding an electron is high. |
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| The solutions to arithmetic expressions that express the energy of an electron in an atom. |
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| The quantum number n of an electron that describes its energy level. An electron with n = 1 must be an s electron; one with n = 2 has s and p states available. |
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| The surface that encloses the region where the probability of finding an electron is high (90-95%). |
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| One of the four quantum numbers that describe an electron. An electron may have either of two different spin quantum numbers, + 1/2 or - 1/2. |
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| Pauli Exclusion Principal |
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Definition
| No two electrons can have the same set of four quantum numbers. An equivalent expression is that only two electrons can occupy the same orbital, and only when they have opposite spins. |
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Definition
| A plane drawn through an orbital where the algebraic sign of a wave function changes. The probability of finding an electron at a node is zero. |
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Definition
| When two orbitals are of equal energy, they are populated by electrons so that each is half-filled before either one is doubly occupied. |
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Definition
| The outermost electrons of an atom. For second-row elements these are the 2s and 2p electrons. The number of these is equal to the number of the element's group number. |
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Definition
| The maximum number of electrons in the ___________ for period 2 elements is 8. |
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Definition
| Amount of energy required to remove an electron from some species. |
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Definition
| Energy change associated with the capture of an electron by an atom |
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Term
| Electrostatic/Coulombic attractions |
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Definition
Attractive forces between two oppositiely charged particles.
aka ionic bond |
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Term
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Definition
| Chemical bond between oppositely charged particles that results from the electrostastic attraction between them |
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Term
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Definition
| For a substance A:B, the energy required to break the bond between A and B so that each retains one of the electrons in the bond |
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Definition
| A shared electron pair bond in which the electrons are drawn more closely to one of the bonded atoms than the other |
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Definition
| A measure of the ability of an atom to attract the electrons in a covalent bond toward itself. Flourine is the most electronegative element. |
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Term
| Electronegative/electropositive |
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Definition
___________ element attracts electrons.
___________ element donates them. |
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Term
| Electrostatic potential map |
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Definition
| The charge distribution in a molecule represented by mapping the interaction energy of a point positive charge with the molecule's electric field on the van der Waals surface. |
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Definition
| No polarization of electron distribution. |
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Definition
| The dipole moment of a bond between two atoms. |
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Definition
| Product of the attractive force between two opposite charges and the distance between them. This has the symbol (mew) and is measured in Debye units (D). |
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Definition
| Unit used for measuring dipole moments. 1 D = 1 X 10 ^ -18 esu*cm |
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Definition
| Order in which a molecule's atoms are connected. Synonymous with constitution |
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Definition
| Different compounds that have the same molecular formula. |
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Definition
| Isomers that differ in respect to the order in which the atoms are connected. Butane and isobutane are examples. |
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Term
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Definition
| Isomers with the same constitution but that differ in respect to the arrangement between the orbitals of the electron donor and acceptor. |
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Term
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Definition
| Same as constitutional isomer. |
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Term
| Condensed structural formulas |
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Definition
| Structural formula in which subscripts are used to indicate replicated atoms or groups. |
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Term
| Bond-line formulas/Carbon skeleton diagrams |
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Definition
| Formula in which connections between carbons are shown but individual carbons and hydrogens are not. |
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Term
| Contributing structures/Resonance hybrid |
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Definition
| The various resonance structures that can be written for a molecule. |
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Term
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Definition
Lewis formulas show electrons as ________.
Shared between two atoms in a covalent bond or unshared electrons belonging to a single atom. |
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Term
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Definition
| Association of an electron with more than one atom. The simplest example is the shared electron pair or covalent bond. This is important in conjugated pi electron systems, where an electron may be associated with several carbon atoms. |
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Term
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Definition
| 4 bonds at an angle of 109.5 |
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Term
| Strong acids/strong bases |
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Definition
An acid that is stronger than H30+
A base that is stronger than HO- |
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Term
| Oxonium ion/hydronium ion |
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Definition
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Definition
| An electronic effect transmitted by successive polarization of the sigma bonds within a molecule or ion. |
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Definition
| Chemical reaction in which an atom or a group of a molecule is replaced by a different atom or group. |
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Definition
| An atom or ion that has an unshared electron pair which can be used to form a bond to carbon. These are Lewis bases. |
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