Ochem

Front 1

Vital Force

Back 1

Thought to be the reason organic compounds could not be synthesized in a lab

Front 2

Organic Chemistry

Back 2

The study of carbon compounds

Front 3

Carbon

Back 3

Group 4A element that can share 4 valence electrons and form 4 covalent bonds

Front 4

Atom Structure

Back 4

Made of a positively charged nucleus surrounded by negatively charged electron cloud

Front 5

Atom diameter

Back 5

2 × 10 ^-10 or 200 picometers (pm)

Front 6

Angstrom

Back 6

represents the unit Aº= 10^-10 m or 100 picometer

Front 7

Atomic number (Z)

Back 7

the number of protons in the atom's nucleus; the same for all atoms of a given element

Front 8

Mass Number (A)

Back 8

The sum of protons & neutrons

Front 9

Isotopes

Back 9

Atoms of the same element that have a different number of neutrons ( different Mass numbers)

Front 10

Atomic mass ( atomic weight)

Back 10

Weighted average mass of an element the naturally occurring isotopes

Front 11

Quantum Mechanics

Back 11

Describe the electron energies and locations by a wave equation (orbital,)

Front 12

Orbital (triton)

Back 12

The wave function in quantum mechanics; a plot of these describes where electron most likely to be. Each can hold 2 electrons

Front 13

S & P Orbital

Back 13

Most important orbitals in organic and biological chemistry

Front 14

How many kinds of orbitals for electrons in hydrongen atom

Back 14

There are four orbitals s, p, d, f

Front 15

Shell (n)

Back 15

Groupings of orbitals that vary in size and energy. Correspond to the periods on the table

Front 16

1st Shell (1s)

Back 16

This shell has only one s orbital

Capacity 2 electrons

Front 17

2nd Shell (2s)

Back 17

This shell contains one s orbital (2s)x1 and p orbitals (2p)x3

Capacity is 8 electrons

Front 18

3rd Shell

Back 18

This shell has one s orbital (3s) x1, p orbitals (3p) x3, and d orbitals (3d) ×5

Capacity 18 electrons

Front 19

P orbitals

Back 19

Each shell has three of these orbitals of equal energy and separated by an area of zero electron density, a node

Front 20

Node

Back 20

An area of zero electron density in a p orbital

Front 21

Ground State Electron Configuration

Back 21

Rule of atomic structure lowest energy arrangement of atom lists orbitals occupied by electrons

Front 22

Aufbau Principle

Back 22

The first rule of electron config: the "build-up"- lowest energy orbitals fill first

Front 23

Pauli Exclusion Principle

Back 23

Rule 2 of electron config: only two electrons of opposite spin can occupy an orbital to have unique wave equations

Front 24

Hund's Rule

Back 24

Rule 3 of electron config: if two or more empty orbitals of equal energy are available electrons occupy each with spins parallel until all orbitals have one electron

Front 25

Kekulé and Couper

Back 25

Each observed that carbon always has 4 bonds

Front 26

Tetrahedral Carbon Atom

Back 26

Front 27

Chemical Bonding Theory

Back 27

Atoms form bonds because compound are more stable than separate atoms

Front 28

Covalent bond

Back 28

The bond organic compounds get from sharing electrons

Front 29

Ionic bonds

Back 29

This type of bond results from electron transfers (btwn metal &nm)

Difference in EN > 2

Front 30

Kekulé Structures

Back 30

Line bond structures: the line rep a 2 electron covalent bond

Front 31

Lewis Structure

Back 31

Electron dot structures where each dot rep one valence electron

Front 32

Nitrogen

Back 32

This element has 5 valence electrons (2s^2) ( 2p^3) but forms only 3 bonds NH3

Front 33

Oxygen

Back 33

Has 6 valence electrons 2s2 2p4 but forms only two bonds H2O

Front 34

Molecular Geom- Linear

Back 34

Ax2 @180º

Front 35

Molecular Geom- Bent

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AX2E @ 120º

Front 36

Molecular Geom- Triangular Planar

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AX3 @120º

Front 37

Molecular Geom- Tetrahedral

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AX4 @109.5º

Front 38

Molecular Geom- Trigonal Pyramidal

Back 38

AX3E @ 107º

Front 39

Molecular Geom- Angular Bent

Back 39

AX2E2 @ 104.5º

Front 40

Lone pairs

Back 40

Another term for valence electrons not used in bonding (nonbonding electrons)

Front 41

Valence Bonding Theory

Back 41

This theory states that atoms in a covalent bond share electron density through the overlapping of their valence Atomic orbitals

Front 42

2SP2 Hybridization

Back 42

AX2

Front 43

3SP2 Hybridization

Back 43

AX3

AX2E

Front 44

4SP3 Hybridization

Back 44

AX4

AX3E

AX2E2

Front 45

Tetrahedral

Back 45

109.5º. AX4

Front 46

Bent

Back 46

120º. AX2E

Front 47

Linear

Back 47

180º AX2

Front 48

Trigonal pyramid

Back 48

107º AX3E

Front 49

Angular Bent

Back 49

104.5º. AX2E2

Front 50

Sigma Bond

Back 50

Single Bond created by overlapping of s or p orbitals during hybridization

Front 51

Major Resonance Structure

Back 51

The major resonance structure is one with the maximum number of atoms with zero formal charge and also one in which negative formal charges are on more electronegative atoms.

Front 52

ELECTRON DOMAIN GEOMETRY

Back 52

The electron pairs around a central atom (A) in a Lewis structure arrange themselves so as to minimize the electrostatic repulsions among the them. The resulting arrangement is called ...

Front 53

MOLECULAR GEOMETRY

Back 53

If we ignore the lone pairs, the arrangement of bond pairs result in geometry is called ____ and that is the shape of the molecule.

Front 54

Bond Angle

Back 54

The angle between bond pairs in a molecular geometric shape

Front 55

Molecular Orbital (MO) Theory

Back 55

Bonds result from combination of atomic orbitals to give molecular orbitals which belong to the entire molecule

Front 56

Sigma Bond

Back 56

A single bond formed by head-on interaction in a circular cross-section due to s or p overlap

*in Diatomic molecules*

Front 57

Pi Bond

Back 57

A bond that forms bc of parallel overlap of singly occupied p orbital

*polyatomic molecules* need this bond for hybridization

Front 58

Hybridization

Back 58

This occurs by the sharing of orbitals to form bonds in polyatomic molecules

Front 59

Degenerate Orbital

Back 59

Another term for hybrid orbital. Meaning energy level will be closer to the p

Front 60

Single bonds

Back 60

These bonds are long (1sigma)

Front 61

Double bonds

Back 61

This bond consists of 1 sigma + 1 pi bond

Front 62

Triple bond

Back 62

Short bond that contains 1sigma +2 pi bonds

Front 63

Polar covalent bonds

Back 63

Form when Bonding electrons are attracted more strongly by one atom than the other

*think north and south pole*

Front 64

Electronegativity (EN)

Back 64

Intrinsic ability of an atom to attract the shared electrons in a covalent bond

Difference in this produce bond polarity

Front 65

Nonpolar Covalent Bond

Back 65

Bond that forms btwn atoms with the same or very similar EN

EN < 0.4

Front 66

Inductive Effect

Back 66

Shifting of electrons in a bond response to EN of nearby atoms

Front 67

Polar covalent bonds

Back 67

Bond btwn atom with a a low EN to one that is high

EN >0.5

Front 68

Dipole

Back 68

When an arrow shows which atom is more EN

Front 69

Dipole moment

Back 69

Net molecular polarity due to the difference in the summed charges

*n/a in symmetrical molecules bc they have one in opposite directions which cancels out" ie) benzene, ethane, methane, co2

Front 70

Dipolar

Back 70

A term used to describe a neutral molecule whose central atoms have bith a positive and negative charge

Front 71

Arrhenius Acid

Back 71

Examines behaviors in water

H is released in water

Front 72

Arrhenius base

Back 72

In water these bases increase in OH

Front 73

Brönstead Acid

Back 73

Acids are proton (H+) donors

These molecules have H attached to a more EN atom

Front 74

Brönstead Base

Back 74

Bases are H+ acceptors

EN atoms w/ lone pairs

Front 75

Lewis Acid

Back 75

Acids are on e (electrophile)

Front 76

Lewis Base

Back 76

Bases are e rich (nucleophile)

Base Bonus

Front 77

Carboxl group

Back 77

Front 78

Hydroxl group

Back 78

Front 79

Carbonyl group

Back 79

Front 80

Aromatic hydrocarbon (Arene) [Benzene Ring ]

Back 80

Front 81

Benze nomenclature

Back 81

-yl benzene

Front 82

Thiol group

Back 82

Front 83

Amine group (-amine)

Back 83

Front 84

Imine group ( -imine)

Back 84

Front 85

Nitrile group (-nitril)

Back 85

Front 86

Akyl halide group (-oyl halide)

Back 86

Front 87

Amide group (-amide)

Back 87

Front 88

Ester (-ethyl, -oate)

Back 88

Front 89

Carboxylic acid (- oic acid)

Back 89

Front 90

Acid anhydride (-oic anhydride)

Back 90

Front 91

Ketone (-one)

Back 91

Front 92

Aldehyde (-al)

Back 92

Front 93

Haloalkane (halo-)

Back 93

Front 94

Ether (-oxy, -ane)

Back 94

Front 95

Alcohol (-ol)

Back 95

Front 96

Alkene group (-ene) *hydrocarbon*

Back 96

Hint 96

Hc dbl bond

Front 97

Alkyne group (-yne) *hydrocarbon*

Back 97

Hint 97

hc triple bond

Front 98

Alkanes *hydrocarbon*

Back 98

Not a functional group

Hint 98

hc single bond

Front 99

Azo compound (azo-)

Back 99

Front 100

Isocyanate (-yl isocyanate)

Back 100

Front 101

Amino group

Back 101

Front 102

Phosphate group

Back 102

Front 103

Sulfhydrl

Back 103

Front 104

Methyl group

Back 104

Front 105

Steriochemistry

Back 105

The branch of chemistry concerned with the 3D arrangement of atoms and molecules and the effects on its chemical reactions

Front 106

Constitutional isomer

Back 106

Molecules with the same molecular formula but with atoms connected to each other in different ways

Front 107

Stereoisomer

Back 107

Molecules with the same atom connectivity but with different orientations of those atoms in space

Front 108

Conformation

Back 108

Different arrangement of atoms resulting from Bond rotation

Front 109

Steric strain

Back 109

Repulsive interaction occurring between atoms that are forced closer together than their atomic radii allow

Front 110

Alkyl Alphabetical Order

Back 110

butyl

sec-butyl

t-butyl

ethyl

isobutyl

Isopropyl

methyl

propyl

Front 111

Staggered (Anti) conformation

Back 111

Mot stable conformation

All 6 C-H are far away (180º)

Front 112

Eclipsed (Gauche) conformation

Back 112

Least stable conformation

All 6 C-H are close =60º