Lesson 1.1: A Whole Field Dedicated to Carbon

Lesson 1.1: A whole field dedicated to carbon Importance of Chemical Safety: ●​ In Canada, workplaces exposed to hazardous chemicals require WHMIS (Workplace Hazardous Materials Information System) training. ●​ Even if your job isn't directly related to chemistry, you may still work with hazardous materials. Key Elements of WHMIS: ●​ Hazard Classification: Identifying hazardous materials. ●​ Cautionary Labeling: Labels with symbols and information on safe handling. ●​ Material Safety Data Sheets (MSDS): Provides details about chemicals, including hazards and safety precautions. ●​ Worker Education & Training: Ensures all employees are knowledgeable about potential chemical hazards. MSDS Requirements (9 categories in Canada): 1.​ 2.​ 3.​ 4.​ 5.​ 6.​ 7.​ 8.​ 9.​ Product Information: Product name, manufacturer info, and emergency contacts. Hazardous Ingredients: List of harmful ingredients. Physical Data: State (solid, liquid, gas), color, odor, etc. Fire/Explosion Hazard Data: Information about flammability. Reactivity Data: Stability and reactions with other substances. Toxicological Properties: Health effects (e.g., carcinogenicity). Preventive Measures: Safety precautions (e.g., protective clothing). First Aid Measures: Instructions in case of exposure. Preparation Information: Who prepared the MSDS and when. WHMIS LabelsComponents: 1.​ 2.​ 3.​ 4.​ 5.​ Pictogram: Symbol representing the hazard. Signal Word: Alerts to hazard level ("Danger" or "Warning"). Hazard Statement: Description of the product's hazard (e.g., "Fatal if swallowed"). Product Identifier: Name of the chemical. Precautionary Statement: Instructions on how to minimize hazards (e.g., "Wear gloves"). ●​ Language Requirements: Labels must be bilingual (English and French). Common Chemical Hazards ●​ Properties of Organic Compounds: ○​ Flammability: Ability to ignite. ○​ Combustibility: Can catch fire or explode. ○​ Volatility: Tendency to evaporate quickly. ●​ Safe Handling: Always check WHMIS labels and MSDS for safety precautions. Plastics and Environmental Concerns ●​ Plastic Use: Plastics are used in various industries, from healthcare (e.g., heart valves, blood bags) to everyday items (e.g., bottles, packaging). ●​ Environmental Impact: Plastic waste is a major concern: ○​ Only 11% of plastic waste in Canada is recycled. ○​ Millions of tons of plastic enter the oceans annually, causing harm to wildlife. ●​ Polyethylene: A commonly used plastic made from carbon and hydrogen atoms. Organic Chemistry and Organic Compounds ●​ Definition: Organic chemistry involves the study of carbon-based compounds, which can be naturally occurring or synthetically created. ●​ Applications: Found in pharmaceuticals, textiles, plastics, perfumes, cleaners, etc. ●​ Why Carbon?: ○​ Bonding Ability: Carbon can form long chains, and multiple bonds (single, double, triple). ○​ Versatility: Can form chains, branched chains, or rings. ○​ High Bonding Capacity: Carbon can bond with a variety of other elements, forming complex molecules. Review and Safety Practices ●​ Familiarity with WHMIS Symbols: Always know the symbols and procedures for handling hazardous materials. ●​ Safety Clothing: Depending on the chemical, wear gloves, goggles, or aprons to protect yourself. ●​ Chemical Spill Response: Be prepared with a clear understanding of the steps to safely manage chemical spills. LESSON 1.2 Organic compounds can be represented in three main ways: ●​ Complete Structural Formulas ●​ Condensed Structural Formulas ●​ Line Diagrams (Skeletal Formulas) Complete Structural Formulas ●​ Definition: Shows all atoms in the compound and the bonds between them. ●​ Bond Representation: ○​ Single bond: Dashed line (—). ○​ Double bond: Double dashed line (=). ○​ Triple bond: Triple dashed line (≡). ●​ Example: ○​ Ethane (C2H6) complete structural formula: H—C—C—H. Condensed Structural Formulas ●​ Definition: A more compact representation where bonds aren't shown, and groups of atoms are written together. ●​ How It Works: ○​ Similar atoms bound to a carbon are grouped and represented using subscripts. ○​ Identical repeating units are put in brackets and repeated with subscripts. ●​ Example: ○​ Pentane (C5H12) complete structural formula: CH3(CH2)3CH3. ○​ Condensed structural formula: CH3(CH2)3CH3. Line Diagrams (Skeletal Formulas) ●​ Definition: Simplified way to represent organic compounds where carbon and hydrogen are implied: ○​ Carbon atoms are represented at the ends or intersections of lines. ○​ Hydrogen is implied, with the maximum number of hydrogen atoms needed to satisfy carbon’s 4 bonds. ●​ Bond Representation: ○​ Single bond: Single line (—). ○​ Double bond: Double line (=). ○​ Triple bond: Triple line (≡). ●​ Example: ○​ Butane (C4H10): CH3(CH2)2CH3 → Line diagram: A zig-zag chain of four lines. ○​ 2-Butanol (C4H10O): CH3CH(OH)CH2CH3 → Line diagram: A zig-zag chain with an OH group on the second carbon. Naming Alkanes (CnH2n+2) ●​ Definition: Alkanes are hydrocarbons that contain only single bonds between carbon atoms. ●​ General Formula: CnH2n+2, where n is the number of carbon atoms in the molecule. ●​ Examples: ○​ Methane (CH4), Ethane (C2H6), Propane (C3H8), Butane (C4H10), Hexane (C6H14). ●​ Naming Convention: ○​ Prefix (indicates the number of carbon atoms) + Suffix "-ane" (indicates single bonds). ○​ Prefix Table: ■​ Meth-: 1 carbon ■​ Eth-: 2 carbons ■​ Prop-: 3 carbons ■​ But-: 4 carbons ■​ Pent-: 5 carbons ■​ Hex-: 6 carbons ■​ Hept-: 7 carbons ■​ Oct-: 8 carbons ■​ Non-: 9 carbons ■​ Dec-: 10 carbons Naming Alkanes with Substituent Groups ●​ Substituent Group: A group of atoms that branches off the main carbon chain (e.g., a methyl group - CH3). ●​ Steps for Naming: ○​ Step 1: Count the longest continuous chain of carbon atoms to determine the base name. ○​ Step 2: Identify the substituent group (e.g., methyl = CH3). ○​ Step 3: Determine the position of the substituent by numbering the carbon chain. Number the chain so that substituents get the lowest possible number. ○​ Step 4: Combine the substituent's position and the base name. ●​ Example: ○​ A methyl group attached to the second carbon of pentane (C5H12). ○​ Name: 2-Methylpentane. Alkanes with Multiple Substituent Groups ●​ When More Than One Substituent: ○​ If there are multiple substituent groups (e.g., two methyl groups), use the prefixes di-, tri-, etc., to indicate how many there are. ○​ Substituent positions are numbered based on their position on the main chain. ●​ Example: ○​ 2,3-Dimethylbutane: Two methyl groups attached to the second and third carbons of a butane molecule. Practice Steps for Naming Alkanes ●​ Step-by-Step Naming: ○​ Find the Longest Carbon Chain. ○​ Identify the Substituent Groups. ○​ Number the Carbon Chain so the substituents get the lowest numbers. ○​ Write the Name by combining the substituents and the base name of the alkane. ○​ Example: ■​ C6H12: Longest chain is hexane. ■​ Substituent: A methyl group on carbon 2. ■​ Name: 2-Methylhexane. ●​ Multiple Substituents: When there are multiple substituent groups of the same type, use prefixes like di-, tri-, etc. to indicate how many there are (e.g., dimethyl for two methyl groups). ●​ Ensure Low Numbering: Always number the chain so that the substituents have the lowest possible numbers. Lesson 1.3 Description: Hydrocarbons that are saturated are alkanes. Hydrocarbons that are unsaturated are alkenes, alkynes, or aromatics. ●​ A saturated hydrocarbon has only single bonds to any atom and therefore the maximum number of hydrogens attached possible. ●​ An unsaturated hydrocarbon has one or more double or triple bonds between carbon atoms or is cyclic in nature, reducing the number of hydrogen atoms attached. These dietary fats have been associated with the current global obesity epidemic, and an increase in diseases such as type-2 diabetes and heart disease. Most fats are an essential component of a healthy diet and part of a group of key biological molecules, they are an essential component of a healthy diet and part of a group of key biological molecules, called lipids, that are necessary for a wide variety of biological functions including the production of hormones and energy storage. Lipids As a large and diverse group, a hallmark of lipids is that: ●​ They tend to be made up of mostly hydrocarbons. ●​ They are generally insoluble in water. Fats, oils, waxes, steroids and phospholipids are just several subtypes of the broader lipid macromolecule group. In particular, fats, also known as triacylglycerols or triglycerides, consist of a glycerol backbone and a fatty acid tail. The glycerol is a small organic molecule with three hydroxyl (-OH) groups, while the fatty acid tails consist of a large hydrocarbon chain attached to a functional group known as a carboxyl. Fatty acids Both saturated and unsaturated fatty acids are made up predominantly of carbon and hydrogen and have a glycerol group. Saturated fatty acids contain only single bonds, while unsaturated fatty acids contain one or more double bonds. You should have noticed that saturated fatty acids contain only single bonds, having the maximum number of hydrogen atoms possible bonded to the carbon skeleton. In comparison, unsaturated fatty acids contain a double bond. In some cases, this double bond can cause a kink in the fatty acid tail, which has significant implications for the behaviour of these molecules. The following tables outline the melting points of a variety of unsaturated and saturated fatty acids. Press the following tabs to know more. Alkenes are hydrocarbons that have at least one double bond in them. The general format for an alkene with only one double bond is CnH2n. 1.​ How many carbons are in the longest chain? When determining the number of carbons on the longest chain, you need to make sure you include the double bond between the two carbons. In this case, there are five carbons, so this is some type of pentene. 2.​ Where is the double bond located? When determining which side of the chain to start from, you need to number the carbons so that the double bond gets the lowest number combination. In our example, the carbons involved in the double bond are carbons 2 and 3. If you were to number the chain in reverse, then the carbons involved in the double bond would be 3 and 4. 3.​ Where are the substitutes and where are they located? There are no substituents in our compound, so this step can be skipped. 4.​ Assemble the name: This compound would be named 2-pentene, or more accurately, pent-2-ene. While it is not incorrect to have the number occur at the beginning of the name, it is considered more precise to have the number associated with the -ene ending so that there is no confusion as to what the number is referring to. Alkynes are hydrocarbons which have a triple bond between two or more carbons. The ending for an alkyne is -yne. Just like alkenes, you need to ensure that the triple bond has the priority when numbering the longest chain. However, if a molecule contains both a double and a triple bond, the carbon chain is numbered so that the first multiple bond gets the lower number. When examining an alkyne that is drawn as a line diagram, be careful when counting the carbons. Remember, wherever a line ends, there is a carbon represented there. Isomers Structural isomers: Recall from a previous learning activity that a structural isomer is one where you have the same number of atoms but they are connected to each other differently. We can also have structural isomers of alkenes, simply by moving around the double bond, or other atoms within the molecule. Geometric isomers In addition to structural isomers, alkenes also have geometric isomers. In a geometric isomer, the atoms are attached in identical ways, however the geometrical orientation of the atoms relative to each other changes. This occurs because in an alkene, the double bond prevents the atoms from being able to rotate. As a result, the relative position of atoms on either side of the double bond is static, whereas in an alkane, the relative position of atoms is constantly changing because of the rotation about the bond. Consider the following two structures in Diagram 1 and Diagram 2. How are they different? 1.​ What is the priority of atoms attached to the carbons in the double bond? Start by identifying the atoms that are attached to the carbons involved in the double bond. Assign those atoms a priority based on their atomic number. The atom with the larger atomic number gets the priority. In the following images, you can check how we have identified which atoms have the priority. 2.​ What is the location of the high-priority atoms? Once you’ve identified the priority on each side, we then compare where the two high-priority atoms are located relative to each other. When they are across from each other (i.e. on opposite sides of the double bond), we use the letter “E” to indicate this. When they are beside each other (i.e. on the same side as the double bond), we use the letter “Z” to indicate this. 3.​ Lesson 1.4: A group that gives function - functional group Alcohols ●​ Each alcohol has an OH group attached to a carbon. ●​ OH indicates that it is an alcohol. ○​ Can be said that any carbon chain that has OH functional group is an alcohol. ●​ When naming alcohols is used the suffix “ol” ●​ To name an alcohol follow: ○​ First number the chain. (Hint: see which side gives the lowest number) ○​ Will put the lowest number. ■​ Example it is 1-ol ○​ Because it’s three carbons long, it is used the prefix “prop” ○​ And because it is made of single bonds, it is used “an” ■​ Therefore, the name is: “propan-1-ol” Aldehydes ●​ Are classified by the presence of carbon with a double bonded oxygen. ●​ Than functional group is known as carbonyl group ●​ In aldehyde carbonyl always occurs on a terminal carbon. ○​ Meaning that a carbon that is the beginning or the end of a chain. ○​ The carbon chain can be of any side but with the carbonyl group attached at the end. ●​ When aldehydes is named , the suffix “al” is used to indicate it is aldehyde. ●​ We do not identify the number for the carbon because it occurs at the end. ○​ Therefore it is used by default “al” and is understood that carbonyl is on the first carbon of the chain. ●​ To name an aldehyde follow: ○​ First identify the longest carbon chain. (Hint:used the lowest number to assign it to the functional group). ○​ Example: It is made with 4 carbons and made up of a single carbons. ■​ Therefore, this is a butane compound. ■​ And because it’s an aldehyde, it is added “al” at the end. ●​ Therefore is named: “butanal” Lesson 1.5: Drawing compounds ●​ Atoms are held by bonds to form compounds. Example: H2O ●​ There are 3 types of compounds: polar covalent, non-polar covalent and ionic bonds. ●​ Organic compounds have different physical properties (i.e. room temperature, clour, solubility…). ○​ This is based on the atoms organization that makes the compound. To understand this is necessary to know: ■​ How are atoms arranged? ■​ How does that arrangement affect the shape of the compound? ■​ How does that shape influence these properties? ●​ It can be drawn as a charged and neutral compound wit lewis structure.