ORGANIC CHEMISTRT

REVIEWER

Branch of chemistry that deals with carbon-containing compounds except carbonates, bicarbonates, cyanides and oxides

ORGANIC CHEMISTRY

from the term organisms

ORGANIC

a German chemist, disproved the “Vitalism” theory which states that all organic compounds come from living things. He was able to isolate urea from an inorganic compound, ammonium cyanate

Friedrich Wohler

heated inorganic compound ammonium cyanate produced urea

Wöhler synthesis

AKA Carbamide

UREA (CH4N2O)

In what year Friedrich Wohler disproved the “Vitalism” theory which states that all organic compounds come from living things. He was able to isolate urea from an inorganic compound, ammonium cyanate?

1828

states that organic compounds cannot be produced from inorganic compounds or molecules, instead it can only produced on living organism or part of a living organism

THEORY OF VITALISM OR VITAL FORCE THEORY

is metabolized by CHON

UREA

is metabolized to produce urea

ORNITHINE

TRUE OR FALSE

Carbon is able to form 6 covalent bonds (6 valence electrons) with other carbon or other elements

FALSE

Carbon is able to form 4 covalent bonds (4 valence electrons) with other carbon or other elements

TRUE OR FALSECarbon atoms have the ability to bond to each other to form long chains or rings

TRUE

Carbon atoms link together to form chains of varying length, branched chains and rings of different sizes

Ability to catenate

capability of an atom in forming stable bonds with itself

CATENATION

Fundamental building blocks of all substances

ELEMENTS

Smallest particle of an element

ATOM

number of protons in nucleus

ATOMIC NUMBER (Z)

number of protons +neutrons

MASS NUMBER (A)

generally neutral consisting of a nucleus surrounded by electrons that are equal in number to the protons of the nucleus

ATOM

Neutral subatomic particle

NEUTRON

Positively charged subatomic particle (+1charge)

PROTON

Negatively charged subatomic particle(-1 charge)

ELECTRON

Center region of an atom

NUCLEUS

Atoms of the same element with different numbers of neutrons and thus different mass number (A)

ISOTOPES

AKA WAVE FUNCTION or ELECTRON CLOUD

ORBITALS

In each orbitals, it can hold 2 electrons

ORBITALS

TRUE OR FALSE

Region of space where there is a certain probability of finding an electron

TRUE

are in fixed distances from the nucleus of an atom, where electrons may be found

ENERGY LEVELS

TRUE OR FALSE

For different kinds of orbitals, electrons are based on those H+ atom

TRUE

TRUE OR FALSE

Each shell contains subshells known as atomic orbitals

TRUE

Each shell contains subshells known as atomic orbitals.

Electrons are said to occupy orbitals in an atom

S and P orbitals are the most common in organic and biological chemistry.

DISTRIBUTION OF ORBITALS WITHIN SHELLS

States that electrons fill lower-energy atomic orbitals before filling higher-energy ones

AUFBAU PRINCIPLE

For degenerate orbitals, electrons fill the orbitals singly before they pair up

HUND’S RULE

Maximum of 2 electrons can occupy the same orbital only if they have opposite spins

PAULI’S EXCLUSION PRINCIPLE

Impossible to predict/ accurately determine the particle’s velocity (position & momentum

HEISENBERG’S UNCCERTAINTY PRINCIPLE

Symbolic notation of the manner in which the electrons of its atoms are distributed over different atomic orbitals

ELECTRON CONFIGURATION

Favorable process because it always leads to lowered energy and increased stability

CHEMICAL BONDING

Joining of two atoms in a stable arrangement

CHEMICAL BONDING

Summary of where the electrons are around a nucleus

ELECTRON CONFIGURATION

atoms react in a way that achieve valence shell of eight valence electrons

OCTET RULE

Hydrogen and helium may have no more than two electrons in their valence shells

DUET RULE

TRUE OR FALSE

Under Duet Rule, it only need to satisfy 1 electrons to become stable

FALSE

it needs to satisfy 2 electrons to become stable

Atom may lose or gain enough electrons to acquire a completely filled valence shell

IONIC BOND

the tendency among atoms of group 1A(alkali-metals)-7A(halogen) elements to react in ways that achieve an outer shell of eight valence electrons

OCTET RULE - FORMATION OF IONS

bearing a negative charge, gain electrons

ANIONS

bearing a positive charge, lose electrons

CATIONS

Pair of valence electrons that are not used for bonding

LONE PAIR

Lone-pair electrons or non-bonding electrons

COVALENT BONDING

Simplified representation of valence e-

LEWIS STRUCTUR

Each shared electron is represented by line between the atom symbols

KEKULE STRUCTURE

Associated with any atom that does not exhibit the appropriate number of valence electrons

FORMAL CHARGE

Measure of the ability of an atom to attract electrons

ELECTRONEGATIVITY

TRUE OR FALSE

Electronegativity from top to bottom, increases

FALSE

Electronegativity from top to bottom, decreases

TRUE OR FALSE

Electronegativity from left to right across the period, increases

TRUE

Withdrawal of electrons towards a highly electronegative atom which causes the formation of partial charges

INDUCTION

It can formed partial positive and partial negative charges

INDUCTION

Shorthand ways of writing structures

DRAWING CHEMICAL STRUCTURES

C-H and C-C and single bonds aren’t shown but understood

CONDENSED STRUCTURES

A property that does not affect the chemical identity of a compound/p>

PHYSICAL PROPERTIES

GIVE THE FACTORS AFFECTING THE PHYSICAL PROPERTIESOFORGCMPDS

Structure of Functional Group

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Molecules having a polar functional group have a higher BP than others with a non-polar functional group of similar molecular masses

Can be observed and measured without changing a compound’s composition of matter

PHYSICAL PROPERTIES

TRUE OR FALSE

Aldehydes and Ketones both have carbonyl group or compound

TRUE

BP and density lower than its straight-chain isomer

Molecules with branched chains

Molecules with higher molecular masses have higher MP,BP, and density

Length of Carbon chains

If the solvent is polar, like water, then a smaller hydrocarbon component and/or more charged, hydrogen bonding, and other polar groups will tend to increase the solubility

SOLUBILIY

TRUE OR FALSE

Any functional group that can donate a hydrogen bond to water will significantly contribute to water solubility

TRUE

TRUE OR FALSE

Anything with a charged group (eg. ammonium, carboxylate, phosphate) is almost certainly water soluble, unless it has large polar group, in which case it will most likely be soluble in the form of micelles, like a soap or detergent

FALSE

Anything with a charged group (eg. ammonium, carboxylate, phosphate) is almost certainly water soluble, unless it has large nonpolar group, in which case it will most likely be soluble in the form of micelles, like a soap or detergent

TRUE OR FALSE

Any functional group that can only accept a hydrogen bond from water (eg. ketones, aldehydes, ethers) will have a somewhat larger but still significant effect on water solubility

FALSE

Any functional group that can only accept a hydrogen bond from water (eg. ketones, aldehydes, ethers) will have a somewhat smaller but still significant effect on water solubility

Melting and boiling are processes in which non-covalent interactions between identical molecules in a pure sample are disrupted

Boiling Point and Melting Point

TRUE OR FALSE

The stronger the non-covalent interactions, the more energy that is required, in the form of heat, to break them apart

TRUE

it y is the ability to dissolve into a solvent is dependent on IMFs

SOLUBILITY

The physical properties of molecules are in part dependent on the type's of intermolecular forces (IMF) present

INTERMOLECULAR FORCES

are the types of forces that holds the atoms together within a molecule

INTRAMOLECULAR FORCES

A complex interaction that includes dipole- dipole, as well as orbital interactions and the transfer of electron density between molecules

Hydrogen bondi

These are generally weaker than H-bonding, ranging from about 5-10 kJ/mol

Dipole-dipole

Occur primarily between OH, NH and FH. The more EN the atom the stronger the interaction. (The atom H is attached to usually has a lone pair of e -)

Hydrogen bonding

Hydrogen bonding

dispersion forces arise from the movement of electrons within a molecule

Van der Waals

Common to polar molecules because they have permanent dipole that are formed due to the differences in the electronegativities

Dipole-dipole

These “induced” dipole moments are very brief as they disappear when the electrons move to new locations within the molecule, so they forces are very brief and weak, only2-5kJ/mol

Van der Waals

The strength of the IMFs depend on the amount of contact between the molecules, especially for dispersion forces. Hence, the shape of the molecule can affect the surface area of contact, long thin molecules have more surface in contact than spherical molecules

STRUCTURAL EFFECTS ON IMFs

A chemical reaction is accompanied by breaking of some bond sand by making of some others

CHEMICAL PROPERTIES

Define as the detailed knowledge of the steps involved in a process in which the reactant molecules change into products

REACTION MECHANISM

During bond breaking or bond fission, the two shared electrons can be distributed equally or unequally between the two bonded atoms

REACTION MECHANISM

A chemical reaction occurs when one substance is converted into another substance(s)

CHEMICAL PROPERTIES

species formed after homolytic fission; are neutral but reactive species having an unpaired electron and these can also initiate a chemical reaction; are important intermediates in organic chemistry

FREE RADICALS

The fission of a covalent bond with equal sharing of bonding electrons

HOMOLYTIC FISSION

This type of bond fission results in the formation of ions. The ion which has a positive charge on the carbon atom, is known as the carbonium ion or a carbocation. On the other hand, an ion with a negative charge on the carbon atom is known as the carbanion

HETEROLYTIC FISSION

an elimination reaction is characterized by the removal of a small molecule from adjacent carbon atoms and the formation of a double bond

ELIMINATION

Unsaturated hydrocarbons such as alkenes and alkynes are extremely reactive towards a wide variety of reagents. The carbon-carbon double bond (–C=C–) of an alkene contains two types of bonds. In alkynes, three carbon-carbon bonds

ADDITION

two or more molecules are combined to generate a bigger one

ADDUCT

proceeds with a fundamental change in the hydrocarbon skeleton of the molecule and during this reaction, an atom or group migrates from one position to another

MOLECULAR REARRANGEMENTS

these are compounds with the same molecular formula and same molecular weight but different structural formula, this differ in physical and chemical properties

ISOMERS

a substitution reaction involves the displacement of one atom or group in a molecule by another atom or group. Aliphatic compounds undergo nucleophilic substitution reactions

SUBSTITUTION

The charged species obtained by the heterolytic fission initiate chemical reactions and they are classified as electrophiles and nucleophiles

HETEROLYTIC FISSION

is negatively charged or electron rich neutral species, however, in chemical reaction, they seek a positive center (nucleus of an atom)

NUCLEOPHILES

contain at least one asymmetric, or chiral, carbon atom

OPTICAL ISOMERS

mixture with equal amounts or dextro & levo isomers, optically inactive or cannot rotate plane polarized light

RACEMIC MIXTURE

Carbons that have four non-identical substituents around it

CHIRAL

Arises from compounds having the same molecular formula but different orientation of atoms that belongs to a molecule in a 3 dimensional

STEREOISOMERISM

Three main groups under Stereoisomerism

Optical Isomers

Geometric Isomers

Conformational Isomers