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Questions and Answers
The rule that states electrons fill subshells of the lowest available energy is known as the ______ Rule.
The rule that states electrons fill subshells of the lowest available energy is known as the ______ Rule.
Aufbau
A ______ pair refers to a pair of valence electrons that are not shared with another atom.
A ______ pair refers to a pair of valence electrons that are not shared with another atom.
lone
Carbon typically forms ______ covalent bonds.
Carbon typically forms ______ covalent bonds.
4
Different classes of organic compounds can be demonstrated, such as ______, alkenes, and alkynes.
Different classes of organic compounds can be demonstrated, such as ______, alkenes, and alkynes.
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The principles of ______ are essential for understanding the spatial arrangement of atoms in a molecule.
The principles of ______ are essential for understanding the spatial arrangement of atoms in a molecule.
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Compounds constructed of strong covalent bonds are more stable than compounds incorporating one or more relatively weak ______.
Compounds constructed of strong covalent bonds are more stable than compounds incorporating one or more relatively weak ______.
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The distribution of electrons at sites of reaction is affected by electronic ______.
The distribution of electrons at sites of reaction is affected by electronic ______.
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When atoms are crowded together, van der Waals repulsions produce an unfavorable steric ______.
When atoms are crowded together, van der Waals repulsions produce an unfavorable steric ______.
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The solvent selected for a given reaction may exert a strong ______ on its course.
The solvent selected for a given reaction may exert a strong ______ on its course.
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A full head arrow indicates complete movement or shift of an ______ pair.
A full head arrow indicates complete movement or shift of an ______ pair.
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Molecules with ______ pairs of electrons can have various shapes such as tetrahedral, trigonal, and linear.
Molecules with ______ pairs of electrons can have various shapes such as tetrahedral, trigonal, and linear.
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The bond angles in a tetrahedral configuration are approximately ______ degrees.
The bond angles in a tetrahedral configuration are approximately ______ degrees.
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Isomers are different compounds that have the same ______ formula.
Isomers are different compounds that have the same ______ formula.
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Resonance involves the delocalization of ______ electrons within certain molecules.
Resonance involves the delocalization of ______ electrons within certain molecules.
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A primary carbon is one that is bonded to no more than ______ other carbon atom.
A primary carbon is one that is bonded to no more than ______ other carbon atom.
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The hydrogen bond is weaker than an ordinary covalent bond but stronger than ______ interactions.
The hydrogen bond is weaker than an ordinary covalent bond but stronger than ______ interactions.
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Dipole–dipole forces are attractive forces between the positive end of one ______ molecule and the negative end of another.
Dipole–dipole forces are attractive forces between the positive end of one ______ molecule and the negative end of another.
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Ethyl alcohol has a higher boiling point than dimethyl ether due to the presence of strong ______ bonds.
Ethyl alcohol has a higher boiling point than dimethyl ether due to the presence of strong ______ bonds.
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In dimethyl ether, the intermolecular forces are weaker dipole–dipole interactions and do not include ______.
In dimethyl ether, the intermolecular forces are weaker dipole–dipole interactions and do not include ______.
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Many organic compounds, especially ______ and other hydrocarbons, are nearly insoluble in water.
Many organic compounds, especially ______ and other hydrocarbons, are nearly insoluble in water.
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Organic compounds that are water soluble, such as ethanol and ______, generally have hydrogen bond acceptor and donor groups.
Organic compounds that are water soluble, such as ethanol and ______, generally have hydrogen bond acceptor and donor groups.
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A chemical ______ is the transformation of the reactants into the reaction products.
A chemical ______ is the transformation of the reactants into the reaction products.
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In a reaction, the ______ refers to the organic compound undergoing change.
In a reaction, the ______ refers to the organic compound undergoing change.
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The final result of a chemical reaction is referred to as the ______.
The final result of a chemical reaction is referred to as the ______.
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In an addition reaction, the number of ______ in the substrate molecule increases.
In an addition reaction, the number of ______ in the substrate molecule increases.
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If the number of hydrogen atoms bonded to a carbon ______, that carbon has been oxidized.
If the number of hydrogen atoms bonded to a carbon ______, that carbon has been oxidized.
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Arrowheads must direct towards an electron deficient species which may be a positive charge or the positive end of a polarized ______
Arrowheads must direct towards an electron deficient species which may be a positive charge or the positive end of a polarized ______
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The products of bond breaking are not stable and cannot be isolated for prolonged ______
The products of bond breaking are not stable and cannot be isolated for prolonged ______
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An electron deficient atom or molecule that has an affinity for an electron pair is known as an ______
An electron deficient atom or molecule that has an affinity for an electron pair is known as an ______
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An atom or molecule that has an electron pair that may be donated in bonding to an electrophile is called a ______
An atom or molecule that has an electron pair that may be donated in bonding to an electrophile is called a ______
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Hybridization is the term applied to the mixing electrons of atomic unequivalent orbitals to generate a set of new equivalent ______ orbitals.
Hybridization is the term applied to the mixing electrons of atomic unequivalent orbitals to generate a set of new equivalent ______ orbitals.
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SP3 hybridization involves the mixing of the electron in 2S with three electrons of 2P to produce four ______ hybrid orbitals.
SP3 hybridization involves the mixing of the electron in 2S with three electrons of 2P to produce four ______ hybrid orbitals.
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Carbon radicals have only seven valence electrons and are considered electron ______.
Carbon radicals have only seven valence electrons and are considered electron ______.
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Examples of nucleophiles include substances like R-NH2 and ______-OH.
Examples of nucleophiles include substances like R-NH2 and ______-OH.
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Ethylene molecule contains a C=C and has ______ geometry.
Ethylene molecule contains a C=C and has ______ geometry.
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In sp2 hybridization, only 2Px and 2Py orbitals combine with the 2S orbital while the 2Pz orbital remains ______.
In sp2 hybridization, only 2Px and 2Py orbitals combine with the 2S orbital while the 2Pz orbital remains ______.
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Acetylene molecule has a ______ geometry, containing a carbon-carbon triple bond.
Acetylene molecule has a ______ geometry, containing a carbon-carbon triple bond.
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The total number of ______ bonds formed by the unhybridized 2Py and 2Pz orbitals in acetylene is two.
The total number of ______ bonds formed by the unhybridized 2Py and 2Pz orbitals in acetylene is two.
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A compound having a bond angle of 180° is an ______.
A compound having a bond angle of 180° is an ______.
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What type of chemical bonding will be found in ______ oxide?
What type of chemical bonding will be found in ______ oxide?
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The total number of tertiary ______ found in the compound is [4].
The total number of tertiary ______ found in the compound is [4].
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Which among the following compounds cannot form ______ bond?
Which among the following compounds cannot form ______ bond?
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Study Notes
Pharmaceutical Organic Chemistry I PC101 - Introduction
- Course name: Pharmaceutical Organic Chemistry I PC101
- Instructor: Mona S. El-Zoghbi, Ph.D. Pharm. Sc.
- Contact: [email protected]
Intended Learning Outcomes (ILOs)
- Students will be able to recognize several organic terms.
- Students will be able to identify different types of chemical bonds.
- Students will be able to recognize different classes of organic compounds and their IUPAC names,
- Students will be able to explain alkanes, alkenes, alkynes, and alkyl halides including nomenclature, physical and chemical properties, and reactions.
- Students will be able to classify different reaction mechanisms.
- Students will be able to describe fundamental principles and applications of stereochemistry, stereo-dynamics, hydroxyl, and carbonyl compounds.
- Students will be able to recognize principles of aromaticity and benzenoid compounds.
Quiz Questions
- The Pauli Exclusion rule states electrons fill subshells of lowest available energy, then higher energy.
- Fluorine is a monovalent atom.
- Carbon forms four covalent bonds.
Lone Pairs
- Lone pairs are pairs of valence electrons not shared with another atom.
- They are found in the outermost electron shell of atoms.
Molecular Shapes
- Molecular shape/configuration is an important property.
Shapes of Molecules Without Lone Pairs
- Tetrahedral: 4 bonding groups, 109.5° bond angles
- Trigonal: 3 bonding groups, 120° bond angles
- Linear: 2 bonding groups, 180° bond angle
Isomers
- Isomers are different compounds with the same molecular formula.
- Example isomers of C5H12 are: pentane, 2-methylbutane, 2,2-dimethylpropane.
Structural Formulas for C4H10O Isomers
- Various structural formulas are shown for C4H10O.
Resonance
- Describes delocalized pi electrons in molecules or polyatomic ions where bonding cannot be represented by a single structure.
- The double-headed arrow represents resonance.
Different Groups of Carbon Atoms
- Primary (1°): bonded to 1 other carbon.
- Secondary (2°): bonded to 2 other carbons.
- Tertiary (3°): bonded to 3 other carbons.
- Quaternary (4°): bonded to 4 other carbons.
Intermolecular Forces
- Atoms/molecules are weakly attracted to each other.
- Weak forces called van der Waals attraction forces exist.
- Without them, all matter would be gaseous.
Dipole-Dipole Attraction
- Attracive forces between the positive end of a polar molecule to the negative end of another polar molecule.
Hydrogen Bonding
- Electrostatic attraction between a hydrogen (H) and electronegative atoms (N, O, F) and another adjacent atom bearing a lone pair of electrons.
- Hydrogen bonding is stronger than dipole-dipole forces but weaker than covalent bonding.
Hydrogen Bonding Accounts
- Ethyl alcohol has a much higher boiling point (78.5°C) than dimethyl ether (24.9°C) due to hydrogen bonding.
Solubility of Organic Compounds in Water
- Many organic compounds (alkane etc) are nearly insoluble in water
- Organic compounds that are water-soluble such as ethanol and acetone usually contain hydrogen bond acceptors or donors
Chemical Reactions
- A transformation of reactants into reaction products
- A reactant is an organic compound undergoing change.
- A product is the final result of the chemical reaction
- Reaction conditions (temperature, pressure, catalysts, solvent) optimize the reaction.
- Catalysts accelerate the reaction rate without being consumed.
Classes of Organic Chemical Reactions
- Addition: the number of σ-bonds increases, usually at the expense of π-bonds.
- Elimination: the number of σ-bonds decreases, and new π-bonds are created.
- Substitution: one atom or group is replaced by another.
- Rearrangement: generates an isomer; the number of bonds does not change.
Mechanism of Organic Reactions
- Detailed description of structural/bonding changes.
- Involve curved arrows for understanding bond breaking/formation.
- Full head arrow indicates electron pair movement.
- Half head arrow indicates single electron movement.
Homolysis vs Heterolysis
- Homolysis: a covalent bond breaks, each fragment receives one electron.
- Heterolysis: a covalent bond breaks, both electrons stay with one fragment.
Reaction Mechanism - General Overview
- Curved arrows are used in drawing mechanisms.
Reactive Intermediates
- Charged: Carbocation, Carbanion
- Uncharged: Radical, Carbene
Electrophiles and Nucleophiles
- Electrphile: Electron-deficient atom/molecule attracted to electron-rich species.
- Nucleophile: Electron-rich atom/molecule attracted to electron-deficient species.
Hybridization
- Combining atomic orbitals to create hybrid orbitals.
- SP3 hybridization: Found in CH₄, tetrahedral geometry.
- SP2 hybridization: Found in C₂H₄, planar geometry; double bonds are formed from sideway overlapping of unhybridized orbitals.
- SP hybridization: Found in C₂H₂; linear geometry; triple bonds are formed from sideway overlapping of unhybridized orbitals.
Practice Exercises
- Various exercises and quiz questions that appear throughout, are included.
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Description
Test your knowledge on the fundamentals of Pharmaceutical Organic Chemistry I. This quiz covers essential concepts such as chemical bonds, organic compounds, IUPAC naming, reaction mechanisms, and stereochemistry. Perfect for students looking to solidify their understanding of organic chemistry principles.
