Fatty Acids and Lipids Lecture Review

These flashcards cover key concepts related to fatty acids, lipids, and their roles in health as discussed in the lecture.

Omega Three Fatty Acids

Essential fatty acids that are important for reducing inflammation and can be found in flax seeds and fish.

Omega Six Fatty Acids

Fatty acids that are often consumed in excess in the typical diet, linked to increased inflammation.

Saturated Fat

Fat that is solid at room temperature; contains no double bonds between carbon atoms.

Unsaturated Fat

Fat that is liquid at room temperature; characterized by one or more double bonds in the fatty acid chains.

Triacylglycerols (Triglycerides)

The simplest form of lipids made from glycerol and three fatty acids, used for energy storage.

Hydrocarbon

An organic compound consisting entirely of hydrogen and carbon.

Emulsification

The process of mixing two immiscible liquids, such as fat and water, facilitated by bile salts.

Metastasis

The spread of cancer cells from the original tumor to other parts of the body.

Monounsaturated Fat

Fats that contain one double bond in their fatty acid chains.

Polyunsaturated Fat

Fats that contain multiple double bonds in their fatty acid chains, also known as PUFAs.

Cis and Trans Fats

Cis fats have hydrogen atoms on the same side of the double bond; trans fats have hydrogens on opposite sides, which can be detrimental to health.

Arachidonic Acid

A type of polyunsaturated fatty acid important in cellular signaling.

Bile Salts

Derivatives of sterols that help emulsify fats in the digestive process.

Lipase

An enzyme that breaks down lipids into smaller molecules for absorption.

Omega Three Fatty Acids

Essential fatty acids that are important for reducing inflammation and can be found in flax seeds and fish.

Omega Six Fatty Acids

Fatty acids that are often consumed in excess in the typical diet, linked to increased inflammation.

Saturated Fat

Fat that is solid at room temperature; contains no double bonds between carbon atoms.

Unsaturated Fat

Fat that is liquid at room temperature; characterized by one or more double bonds in the fatty acid chains.

Triacylglycerols (Triglycerides)

The simplest form of lipids made from glycerol and three fatty acids, used for energy storage.

Hydrocarbon

An organic compound consisting entirely of hydrogen and carbon.

Emulsification

The process of mixing two immiscible liquids, such as fat and water, facilitated by bile salts.

Metastasis

The spread of cancer cells from the original tumor to other parts of the body.

Monounsaturated Fat

Fats that contain one double bond in their fatty acid chains.

Polyunsaturated Fat

Fats that contain multiple double bonds in their fatty acid chains, also known as PUFAs.

Cis and Trans Fats

Cis fats have hydrogen atoms on the same side of the double bond; trans fats have hydrogens on opposite sides, which can be detrimental to health.

Arachidonic Acid

A type of polyunsaturated fatty acid important in cellular signaling.

Bile Salts

Derivatives of sterols that help emulsify fats in the digestive process.

Lipase

An enzyme that breaks down lipids into smaller molecules for absorption.

Arrhenius Acid

A substance that produces H^⁺ ions in water. Example: HCl
ightarrow H^⁺ + Cl^⁻

Arrhenius Base

A substance that produces OH^⁻ ions in water. Example: NaOH
ightarrow Na^⁺ + OH^⁻

Brønsted–Lowry Acid

An H^⁺ donor.

Brønsted–Lowry Base

An H^⁺ acceptor.

Conjugate Base (Acid-Base pairs)

Formed when an acid donates an H^⁺ ion.

Conjugate Acid (Acid-Base pairs)

Formed when a base accepts an H^⁺ ion.

Acid-Base Conjugate Example

In the reaction HF + H₂O \rightleftharpoons H₃O^⁺ + F^⁻, HF is the acid, H₂O is the base, H₃O^⁺ is the conjugate acid, and F^⁻ is the conjugate base.

Cation

A positively charged ion (e.g., Na^⁺, K^⁺, NH₄^⁺).

Anion

A negatively charged ion (e.g., Cl^⁻, SO₄^{2⁻}, NO₃^⁻).

Salt (Chemistry)

An ionic compound formed from the reaction of an acid and a base. Example: HCl + NaOH
ightarrow NaCl + H₂O, where NaCl is the salt.

Dissociation of Ionic Compound

When an ionic compound splits into its constituent ions in water. Example: CaCl₂
ightarrow Ca^{2⁺} + 2 Cl^⁻

Single Reaction Arrow (→)

Indicates a reaction that goes to completion, typical for strong acids/bases.

Double Reaction Arrow (⇌)

Indicates an equilibrium reaction, typical for weak acids/bases.

Binary Acid Naming

For acids composed of hydrogen and one other element, named "Hydro-" + root of element + "-ic acid." Example: HCl is hydrochloric acid.

Oxyacid Naming (-ate ending)

For oxyacids where the polyatomic ion ends in "-ate," the acid name ends in "-ic acid." Example: HNO₃ is nitric acid.

Oxyacid Naming (-ite ending)

For oxyacids where the polyatomic ion ends in "-ite," the acid name ends in "-ous acid." Example: HNO₂ is nitrous acid.

pH calculation

pH = -log[H^⁺]

pOH calculation

pOH = -log[OH^⁻]

pH + pOH relationship

pH + pOH = 14

Autoionization of Water Constant (K_w)

[H^⁺][OH^⁻] = 1 \times 10^{⁻¹⁴} at 25°C.

Acidic Solution (pH)

A solution with pH < 7

Neutral Solution (pH)

A solution with pH = 7

Basic Solution (pH)

A solution with pH > 7

Finding [H⁺] from pH

If pH = x, then [H^⁺] = 10^{⁻x}. For example, if pH = 3, then [H^⁺] = 10^{⁻³}.

Dilution Equation

Used for volume and concentration problems: C₁V₁ = C₂V₂

pKa relationship to Ka

pKa = -log(Ka)

Strength of Acid and pKa

A smaller pKa indicates a stronger acid.

Henderson–Hasselbalch Equation

pH = pKa + log(\frac{[A^⁻]}{[HA]})

Titrant

A solution of known molarity (M), typically found in the burette during a titration.

Analyte

A solution of unknown molarity (M), typically found in the flask during a titration.

Equivalence Point (Titration)

The point in a titration where the moles of acid exactly equal the moles of base.

Titration Equation (monoprotic)

For monoprotic acids: M₁V₁ = M₂V₂

Titration Equation (polyprotic)

For polyprotic acids: n₁M₁V₁ = n₂M₂V₂, where n is the number of H^⁺ or OH^⁻ ions.

Titration Experimental Steps (summary)

Rinse burette with titrant, fill burette, add analyte + indicator to flask, slowly add titrant while swirling, stop when color change persists for 30 seconds, use total volume added for calculations.

Alpha (α) Radiation

Consists of a helium nucleus (^4_2He); has low penetration and can be blocked by paper.

Beta (β) Radiation

Consists of an electron; has medium penetration.

Gamma (γ) Radiation

High-energy electromagnetic radiation (light); has deep penetration.

Atomic Number (Z)

The number of protons in an atom's nucleus.

Mass Number (A)

The total number of protons and neutrons in an atom's nucleus (A = protons + neutrons).

Balancing Nuclear Equations (principles)

Conserve both the mass number and the atomic number on both sides of the equation. Example: ^{238}{92}U \rightarrow ^42He + ^{234}_{90}Th

Half-Life Equation

N = N₀(½)^{t/t{½}} (where N is remaining amount, N₀ is initial amount, t is time, and t{½} is half-life).

Nuclear Fission

The process of splitting a heavy atomic nucleus into two or more lighter nuclei, used in nuclear power plants.

Nuclear Fusion

The process of combining two light atomic nuclei to form a heavier nucleus, occurring in the sun and stars.

Organic Compound (definition)

Mostly consists of C–H bonds (e.g., drugs, fuels, plastics).

Inorganic Compound (definition)

Generally involves metals, salts, and ionic compounds, lacking extensive C–H bonding.

Alcohol Functional Group

Contains an –OH group.

Amine Functional Group

Contains an –NH₂ group.

Carboxylic Acid Functional Group

Contains a –COOH group.

Ketone Functional Group

Contains a carbonyl group (C=O) within the carbon chain.

Aldehyde Functional Group

Contains a carbonyl group (C=O) at the end of a carbon chain.

Ester Functional Group

Contains a –COO– group.

Ether Functional Group

Contains an –O– group bridging two carbon chains.

Alkene Functional Group

Contains a carbon-carbon double bond (C=C).

Alkyne Functional Group

Contains a carbon-carbon triple bond (C \equiv C).

Aromatic Functional Group

Specifically refers to a benzene ring.

Alkane

Hydrocarbons containing only single bonds between carbon atoms (C–C); considered saturated. Naming ends with "-ane".

Alkene

Hydrocarbons containing one or more double bonds between carbon atoms (C=C); considered unsaturated. Naming ends with "-ene".

Branched Chain (Organic)

A carbon chain with substituents coming off the main chain.

Linear Chain (Organic)

A continuous chain of carbon atoms without substituents.

Skeletal Structure (Organic Chemistry)

A simplified representation where ends and bends represent carbon atoms, and hydrogens are implied unless written.