Untitled Flashcards Set

1. What is organic chemistry, and what does it primarily study?
   The study of carbon-containing compounds, including their structure, properties, and reactions.

2. Do all carbon-containing compounds qualify as organic? Provide examples.
   No, examples of inorganic carbon-containing compounds include CO₂ and carbonates.

3. What distinguishes the carbon-based structure of organic compounds from inorganic compounds?
   Organic compounds are primarily composed of carbon bonded to H, O, N, S, and other nonmetals, while inorganic compounds often involve metals and salts.

4. How does bonding differ between organic and inorganic compounds?
   Organic compounds have covalent bonding, whereas inorganic compounds usually have ionic bonding.

5. Why do organic compounds generally have lower melting and boiling points compared to inorganic compounds?
   Organic compounds have weaker intermolecular forces, while inorganic compounds have stronger ionic bonds.

6. Explain the solubility differences between organic and inorganic compounds.
   Organic compounds are soluble in nonpolar solvents but not in water, while inorganic compounds are typically water-soluble.

7. Why are organic compounds generally combustible, while many inorganic compounds are not?
   Organic compounds contain carbon and hydrogen, which burn easily, while inorganic compounds lack this structure.

8. What makes the structural diversity of organic compounds greater than that of inorganic compounds?
   Carbon can form chains, rings, and multiple bonds, creating a wide variety of structures.

9. What types of solvents are organic compounds typically soluble in? Why?
   Nonpolar solvents, because organic compounds are mostly nonpolar or weakly polar.

10. Why do inorganic compounds often conduct electricity, but organic compounds usually do not?
    Inorganic compounds have ions that allow electricity flow, while organic compounds lack free-moving charges.

11. What are the exceptions to the general rules of conductivity in organic compounds?
    Polymers and organic semiconductors can conduct electricity.

12. How does the reactivity of organic compounds depend on their functional groups? Provide an example.
    Functional groups like -OH (alcohol) or -COOH (acid) determine specific reactions, e.g., alcohols react with acids to form esters.

13. What are some exceptions to the combustibility of organic compounds and the non-combustibility of inorganic compounds?
    Carbonates are inorganic but decompose on heating; some halogenated organic compounds resist burning.

14. Why do inorganic compounds tend to have more predictable reactions compared to organic compounds?
    Their simpler structures and ionic nature make their reactions more straightforward.

15. What role do metals, salts, and nonmetals play in the structure of inorganic compounds?
    They form ionic compounds and lattices, giving stability and specific properties.

Organic Chemistry ETA Reviewer

(Final Destination Core)

(NAMING & DRAWING ARE NOT PART, STEP BY STEP PROCEDURE IS GIVEN BELOW)

Organic Chemistry

• Study of carbon-containing compounds

• All organic compounds contain carbon, but not all carbon-containing compounds are organic

Organic Compounds vs Inorganic Compounds

What makes carbon special?

Tetravalency 

Carbon has 4 valence electrons

• Electrons in the outermost of an atom

• Can form single, double, and triple bond with other carbon atoms 

Catenation

• Ability of carbon atoms to form long chains or rings by bonding with other carbon atoms

Bond Strength & Stability

C-C bond and C-H bond are very stable

• Due to their bond energies, making carbon-based compounds stable and durable under a wide range of conditions

Isomerism

• Same molecular formula = different structures or arrangements of atoms

Hybridization 

• Carbon’s ability to undergo hybridization allows it to form different types of bonds by mixing its s and p orbitals into new hybrid orbitals.

Variety of Functional Groups

• Carbon can form bonds with various functional groups like hydroxyl (-OH), carboxyl (-COOH), and amino (-NH₂)

Hydrocarbons

• Substances containing only carbon and hydrogen

Aliphatic / Acylic

• Hydrocarbons that have straight or branched chains of carbon atoms. They do not contain any rings.

Alicyclic

• Hydrocarbons that have a cyclic structure (carbon atoms are arranged in a ring)

Hydrocarbon

• Compounds consisting of C and H atoms

Alkanes

• single-bonded organic compounds can either be linear or branched follow the general formula CnH 2n+2

Cycloalkanes

• single-bonded organic compounds ring structure follow the general formula CnH 2n

Naming Alkanes & Cycloalkanes:

Functional Groups

• Functional groups are specific groups of atoms within molecules that determine the chemical properties of those molecules.

Alkanes and Combustion Reaction

Structure and Reactivity of Unsaturated Hydrocarbons

Unsaturated Hydrocarbons

• contain at least one double or triple bond, making them more reactive in certain types of reactions than alkanes. There are three major types:

Isomers

• compounds with the same molecular formula but different structures

Constitutional or Structural Isomers 

• same formula but different connectivity of atoms

Stereoisomers 

•  same connectivity but different spatial arrangement of atoms 

Addition Reactions of Alkenes 

• one of the most important types of reactions that alkenes undergo due to their carbon-carbon double bond, which is highly reactive

• the double bond becomes a single bond

Hydrogenation 

• REACTION: An alkene reacts with hydrogen gas (H2) in the presence of a metal catalyst (commonly platinum, palladium, or nickel)

Halogenation 

• REACTION: Alkenes react with halogens like chlorine (Cl₂) or bromine (Br₂) without a catalyst

Hydrohalogenation 

• REACTION: An alkene reacts with a hydrogen halide (like HCl, HBr, HI) 

• RESULT: The hydrogen atom attached to one carbon of the double bond, and the halogen attaches to the other carbon.

Hydrohalogenation  

• Follows the Markovnikov’s Rule 

• In asymmetrical alkenes, the hydrogen attaches to the carbon with more hydrogens (the “rich get richer” rule). 

Nomenclature of Alcohol 

•  Alcohols are named by changing the ending of the parent alkane name to -ol.

Nomenclature of Ethers

• characterized by an oxygen atom connected to two alkyl or aryl groups

Nomenclature of Alkyl Halides 

•  also called as haloalkanes 

•  compounds containing one or more halogen atoms (F, Cl, Br, I) bonded to an alkyl group

Nomenclature of Thiols 

• also known as mercaptans 

• organic compounds characterized by the presence of a sulfhydryl group (-SH) attached to a carbon atom

TIPS ON NAMING: 

(Starting point of naming is the highest substituent carbon)

BENZENE

CYCLOHEXANE

CYCLOHEXENE

EXTRA NAMINGS FOR ALKANES:

CYCLOPROPYL

NOTE: THE SUFFIX “PROPYL” IS USED IF THERE'S A BIGGER PARENT CHAIN THAN ITSELF

USE IF THERE IS 2 OR MORE OF THE SUBSTITUENT

1. Unique Properties of Carbon: Bonding and formation of multiple covalent bonds.

2. Physical and Chemical Properties: Solubility in polar/nonpolar solvents, boiling and melting points.

3. IUPAC Rules for Naming: Identifying parent chains, functional groups, and numbering substituents.

4. Naming Specific Classes: Alkanes, alkenes, alkynes, alcohols, ethers, thiols, and alkyl halides.

5. Types of Isomers: Structural (constitutional) isomers and stereoisomers (cis-trans and spatial arrangement).

6. Identification and Impact: Key functional groups (-OH, -SH, -COOH, ethers) and their effect on solubility and reactivity.

7. Properties and Classification: Alcohols (primary, secondary, tertiary) and thiols.

8. Combustion of Hydrocarbons: Complete vs. incomplete combustion and environmental impacts.

9. Addition Reactions: Markovnikov’s rule and tests for unsaturation (e.g., bromine test).

10. Benzene stability and aromaticity

11. Solubility and Polarity: Polar vs. nonpolar interactions and the role of functional groups.

12. Intermolecular Forces: Hydrogen bonding, dipole-dipole, and London dispersion forces.
    

Got it! Here's the updated and slightly more detailed version:  

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1. I can define organic chemistry.  

Organic chemistry is the study of carbon-containing compounds, including their structures, properties, reactions, and synthesis. These compounds often include hydrogen, oxygen, nitrogen, sulfur, and halogens.

2. I can describe the special nature of carbon.  

Carbon is unique because it can form four covalent bonds, allowing it to create stable single, double, and triple bonds. It can bond to itself, forming long chains or rings, and create complex structures with functional groups.

3. I can list the general characteristics of organic compounds.  

Organic compounds generally have covalent bonds, lower melting and boiling points compared to ionic compounds, and are often nonpolar or slightly polar. They tend to be soluble in nonpolar solvents but insoluble in water.

4. I can recognize the characteristic features of organic compounds.  

Organic compounds typically contain carbon-hydrogen bonds and may include functional groups such as alcohol (-OH), carbonyl (C=O), or carboxyl (-COOH). These functional groups define their chemical reactivity.

5. I can predict the shape around atoms in organic molecules.  

Using VSEPR theory (Valence Shell Electron Pair Repulsion), electron pairs around a central atom arrange to minimize repulsion. For example, four bonding groups form a tetrahedral shape, while three groups form a trigonal planar structure.

6. I can use shorthand methods to draw organic molecules.  

Shorthand methods like line-angle diagrams simplify structures by representing carbon atoms as vertices and bonds as lines, omitting hydrogen atoms bonded to carbons for clarity.

7. I can identify and draw acyclic alkanes and cycloalkanes.  

Acyclic alkanes are open-chain hydrocarbons with only single bonds, while cycloalkanes are ring-shaped alkanes. For example, propane is acyclic, while cyclopropane is a three-membered ring.

8. I can name alkanes using the IUPAC system of nomenclature.  

Identify the longest continuous carbon chain as the parent name, number the chain to give substituents the lowest possible numbers, and list substituents alphabetically with their positions.

9. I can identify constitutional isomers.  

Constitutional isomers have the same molecular formula but differ in the connectivity of atoms. For example, C₄H₁₀ includes both butane (a straight chain) and isobutane (a branched chain).

10. I can recognize the common functional groups and understand their importance.  

Functional groups, such as hydroxyl (-OH) in alcohols or carbonyl (C=O) in ketones, determine a molecule's reactivity, physical properties, and interactions in biological and chemical systems.

11. I can determine whether an organic compound is polar or nonpolar.  

Polarity depends on molecular shape and the electronegativity of atoms. Molecules with polar bonds and an asymmetrical shape are polar, while symmetrical molecules are often nonpolar.

12. I can determine solubility properties of organic compounds.  

Compounds with polar functional groups (e.g., -OH, -NH₂) dissolve in water, while nonpolar compounds (e.g., hydrocarbons) dissolve in organic solvents like hexane.

13. I can predict the physical properties of alkanes.  

Alkanes are nonpolar and have weak intermolecular forces (London dispersion), resulting in low melting and boiling points. These properties increase with molecular size and branching.

14. I can determine whether a vitamin is fat-soluble or water-soluble.  

Water-soluble vitamins (e.g., B and C) have many polar groups and form hydrogen bonds with water. Fat-soluble vitamins (e.g., A, D, E, K) are nonpolar and dissolve in lipids.

15. I can write equations for the complete and incomplete combustion of alkanes.  

Complete combustion (in excess oxygen) produces carbon dioxide (CO₂) and water (H₂O). Incomplete combustion (limited oxygen) produces carbon monoxide (CO) or soot (C).

16. I can identify the three major types of unsaturated hydrocarbons—alkenes, alkynes, and aromatic compounds.  

Alkenes have one or more double bonds, alkynes have one or more triple bonds, and aromatic compounds contain benzene or related ring structures with delocalized electrons.

17. I can name alkenes, alkynes, and substituted benzenes.  

For alkenes and alkynes, identify the longest chain containing the double or triple bond and number the chain to give the bond the lowest number. Substituents on benzene rings are named based on their positions (e.g., ortho, meta, para).

18. I can recognize the difference between constitutional isomers and stereoisomers, as well as identify cis and trans isomers.  

Constitutional isomers differ in connectivity, while stereoisomers have the same connectivity but differ in spatial arrangement. Cis isomers have groups on the same side, while trans isomers have groups on opposite sides.

19. I can predict the products of addition reactions of alkenes.  

In addition reactions, the π bond of an alkene breaks, and new atoms/groups (e.g., H₂, Br₂) add to the carbons, forming single bonds.

20. I can predict the products of reactions that follow Markovnikov’s rule.  

Markovnikov’s rule states that in addition of HX to an alkene, the hydrogen atom adds to the carbon with more hydrogens, and the halide adds to the more substituted carbon.

21. I can identify alcohols, ethers, alkyl halides, and thiols.  

Alcohols have an -OH group, ethers have an oxygen atom between two carbons (R-O-R), alkyl halides contain halogens, and thiols have a sulfur atom bonded to hydrogen (-SH).

22. I can classify alcohols and alkyl halides as 1°, 2°, or 3°.  

Alcohols and alkyl halides are classified based on the number of carbon atoms attached to the carbon bonded to the -OH or halogen. For example, 1° has one carbon attached, 2° has two, and 3° has three.

23. I can determine the properties of alcohols, ethers, alkyl halides, and thiols.  

Alcohols can form hydrogen bonds, making them more soluble and having higher boiling points. Ethers are less polar, alkyl halides vary depending on the halogen, and thiols are characterized by their strong odor and moderate polarity.