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LBCC Organic Chemistry > Chapter 1 Vocabulary > Flashcards

Chapter 1 Vocabulary Flashcards

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1
Q

Anti-bonding Molecular orbitals

A

A high-energy molecular orbital resulting from the destructive interference between atomic orbitals

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2
Q

Atomic orbital

A

A three-dimensional plot of ψ2 of a wavefunction. It is a region of space that can accommodate electron density.

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3
Q

Aufbau principle

A

A rule that determines the order in which orbitals are filled by electrons. Specifically, the lowest energy orbital is filled first.

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4
Q

Bent geometry

A

A geometric arrangement for three atoms connected to each other (such as H−O−H) in a nonlinear fashion.

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5
Q

Bonds

A

A strong force of attraction holding atoms together in a molecule or crystal, resulting from the sharing or transfer of electrons

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6
Q

Bonding Molecular orbitals

A

A low-energy molecular orbital resulting from the constructive interference between atomic orbitals.

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7
Q

Constitutional Isomers

A

Compounds that have the same molecular formula but differ in the way the atoms are connected.

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8
Q

Constructive interference

A

When two waves interact with each other in a way that produces a wave with a larger amplitude.

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9
Q

Covalent bond

A

A bond that results when two atoms share a pair of electrons.

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10
Q

Debye

A

A unit of measure for dipole moments, where 1 debye = 10 − 18 esu ⋅ cm.

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11
Q

Degenerate

A

Having the same energy.

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12
Q

Degenerate orbital

A

Orbitals that have the same energy.

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13
Q

Divalent

A

An element that forms two bonds, such as oxygen.

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14
Q

Dipole moment (µ)

A

The amount of partial charge (δ) on either end of a dipole multiplied by the distance of separation (d): μ = δ × d

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15
Q

Dipole-dipole interactions

A

The resulting net attraction between two dipoles.

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16
Q

Electron density

A

A term associated with the probability of finding an electron in a particular region of space.

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17
Q

Electrostatic potential maps

A

A three-dimensional, rainbow like image used to visualize partial charges (δ) in a compound.

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18
Q

Electronegativity

A

the degree to which an element tends to gain electrons and form negative ions in chemical reactions

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19
Q

Formal Charge

A

A charge associated with any atom that does not exhibit the appropriate number of valence electrons.

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20
Q

H. O. M. O.

A

The Highest Occupied Molecular Orbital.

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21
Q

Hund’s Rule

A

When considering electrons in atomic orbitals, a rule that states that one electron is placed in each degenerate orbital first, before electrons are paired up.

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22
Q

Hybridization

A

A mathematical procedure in which standard atomic orbitals are combined to form new, hybrid orbitals

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23
Q

Hydrogen bonding

A

A special type of dipole-dipole interaction that occurs between an electronegative atom and a hydrogen atom that is connected to an electronegative atom.

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24
Q

Hydrophilic

A

A polar group that has favorable interactions with water.

25
Q

Hydrophobic

A

A nonpolar group that does not have favorable interactions with water.

26
Q

Induction

A

The withdrawal of electron density that occurs when a bond is shared by two atoms of differing electronegativity.

27
Q

Ionic bond

A

A bond that results from the force of attraction between two oppositely charged ions.

28
Q

Lewis Structure

A

A drawing style in which the electrons take center stage.

29
Q

London Dispersion forces

A

Attractive forces between transient dipole moments, observed in alkanes.

30
Q

Lone Pair

A

A pair of unshared, or nonbonding, electrons.

31
Q

L. U. M. O.

A

The lowest unoccupied molecular orbital.

32
Q

Micelle

A

A group of molecules arranged in a sphere such that the surface of the sphere is comprised of polar groups, rendering the micelle water soluble.

33
Q

Molecular dipole moment

A

The vector sum of the individual dipole moments in a compound.

34
Q

Molecular orbitals

A

Orbitals associated with an entire molecule rather than an individual atom.

35
Q

Molecular orbital theory

A

A description of bonding in terms of molecular orbitals, which are orbitals associated with an entire molecule rather than an individual atom.

36
Q

Monovalent

A

An element that can form one bond (such as hydrogen).

37
Q

Nodes

A

In atomic and molecular orbitals, a location where the value of ψ is zero.

38
Q

Octet Rule

A

The observation that second-row elements (C, N, O, and F) will generally form the necessary number of bonds to achieve a full valence shell (eight electrons).

39
Q

Pauli Exclusion Principle

A

The rule that states that an atomic orbital or molecular orbital can accommodate a maximum of two electrons with opposite spin.

40
Q

Partial charge

A

(δ-) negative, (δ+) positive.

Charges created due to the asymmetric distribution of electrons in chemical bonds.

41
Q

Pi (π) bond

A

A bond formed from adjacent, overlapping p orbitals.

42
Q

Polar Covalent Bond

A

A bond in which the difference in electronegative values of the two atoms is between 0.5 and 1.7.

43
Q

Quantum mechanics

A

A mathematical description of an electron that incorporates its wavelike properties.

44
Q

Sigma (σ) bond

A

A bond that is characterized by circular symmetry with respect to the bond axis.

45
Q

sp-hybridized:

A

Atomic orbitals that are achieved by mathematically averaging one s orbital with only one p orbital to form 2 hybridized atomic orbitals.

46
Q

sp2 Hybridized orbital

A

Atomic orbitals that are achieved by mathematically averaging one s orbital with two p orbitals to form 3 hybridized atomic orbitals.

47
Q

sp3 Hybridization:

A

Atomic orbitals that are achieved by mathematically averaging one s orbital with three p orbitals to form 4 hybridized atomic orbitals.

48
Q

Steric number

A

The total of electron pairs (single bonds + lone pairs) for an atom in a compound.

49
Q

Tetrahedral

A

The geometry of an atom with four bonds separated from each other by 109.5°.

50
Q

Tetravalent

A

An element, such as carbon, that forms four bonds.

51
Q

Triagonal pyramidal

A

A geometry adopted by an atom that has one lone pair and a steric number of 4.

52
Q

Trigonal planar

A

A geometry adopted by an atom with a steric number of 3. All three groups lie in one plane and are separated by 120°.

53
Q

Trivalent

A

An element, such as nitrogen, that forms three bonds.

54
Q

Valence bond theory

A

A theory that treats a bond as the sharing of electrons that are associated with individual atoms, rather than being associated with the entire molecule.

55
Q

VESPR Theory

A

Valence shell electron pair repulsion theory, which can be used to predict the geometry around an atom.

56
Q

Wave equations (ψ)

A

Describes the total energy of an electron when in the vicinity of a proton.

57
Q

Wave functions

A

Solutions to wave equations (ψ) where ψ2 represents the probability of finding an electron in a particular location.

58
Q

Zeff

A

effective nuclear charge

LBCC Organic Chemistry (16 decks)

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