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Chapter 4 The Effects of Chemical Reactions. • Introduction to Chemical Reactions. - Chemical reaction: a process in which one or more substances change into one or more new substances. - Clues that a chemical reaction has occurred : 1. Color change Example: two colorless aqueous solutions mix together to produce a bright yellow precipitate. 2. A precipitate (solid) is formed when mixing two solutions together. 3. Gas formation. Bubbles of gas (effervescence) are produced when mixing substances together (solid – liquid or aqueous – aqueous ….) 4. Heat is produced. - Chemical reactions are described by using word equations or chemical equations. - Chemical equations need to be balanced when written because it shows the correct proportions (amounts) of chemicals in a reaction. - A balanced chemical equation has equal number of atoms of each element in the reactants (left hand side) and the products (right hand side). - Exercise: Balance the following equations. a) KClO3→KCl + O2 b) Na2O + H2O NaOH c) Cu + AgNO3 Cu(NO3)2 + Ag d) C3H7OH + O2 CO2 + H2O • Synthesis and Decomposition Reactions. Synthesis: Two or more substances (elements and / or compounds) combine to form one larger compound. General pattern: A + B → C Examples: N2 + 3 H2 → 2 NH3 CaO + CO2 → CaCO3 2 P + 3 Cl2 → 2 PCl3 Decomposition: This is opposite to synthesis; that is, one large compound breaks down (decomposes) into 2 or more simpler substances. Example: 2 KClO3 → 2 KCl + 3 O2 General pattern: R → S + T Remark: Usually decomposition happens due to heat or electricity. - Predicting the product of decomposition or synthesis reactions. 2 AlCl3 (s) → 2 Al (s) + 3 Cl2 (g) Zn (s) + S (s) → ZnS (s) 2 Zn (s) + O2 (g) → 2 ZnO(s) - Single Displacement (Replacement) Reactions. Definition: A reaction in which an element displaces (replaces) another element in a compound, producing a new compound and a new element. General pattern: A + BC → AC + B Example: Mg (s) + CuSO4 (aq) → MgSO4 (aq) + Cu (s) Zn (s) + 2 AgNO3 (aq) → Zn(NO3)2 (aq) + 2 Ag (s) Fe (s) + MgCl2 (aq) → no reaction. Remark: The element that displaces the other element in a compound must be more reactive (active) than that element, otherwise no reaction takes place. In the general pattern above, A should be more reactive than B for the reaction to proceed. The following reactivity (activity) series lists the chemical strength (reactivity) of the metals in order from the more reactive to the less reactive. KPlease stop calling my amazing zebra in the long Nahungry class. sorry !! Ca Mg Al Zn Fe Sn Pb H Cu Ag Examples of single displacement reactions : 2 Al (s) + 3 CuSO4 (aq) → Al2(SO4)3 (aq) + 3 Cu (s) Sn (s) + Zn(NO3)2 (aq) → no reaction Exercise: Complete and balance the following equations. If there is no reaction occurring write no reaction. a) 2 Al (s) + 6 HCl (aq) → 2 AlCl3 (aq) + 3 H2 (g) b) Cu (s) + H2SO4 (aq) → no reaction c) 2 AlCl3 (aq) + 3 Ca (s) → 3 CaCl2 (aq) + 2 Al (s) d) Mg (s) + 2 HNO3 (aq) → Mg(NO3)2 (aq) + H2(g) - Reactivity of halogens decreases down the group. F2> Cl2> Br2> I2 The reactions taking place for the halogens or their compounds are in solution (aqueous) Examples: Cl2 (aq) + 2 KBr (aq) → 2 KCl (aq) + Br2 (l) Cl2 (aq) + NaF (aq) → no reaction. Exercise: F2 (aq) + 2 LiCl (aq) → 2 LiF (aq) + Cl2 (g) I2 (aq) + NaCl (aq) → no reaction • Double displacement reactions. - Definition: A reaction in which two compounds mix together and an exchange of ions (elements) occurs which results in the formation of 2 new compounds. - General pattern: AB + CD → AD + CB - Solubility: the amount of solute that dissolves in a given amount of solvent at a given temperature. - When we say a substance is soluble, it means it dissolves in water; whereas if it is insoluble it means it doesn’t dissolve in water. - The compound in a reaction that is soluble is in aqueous (aq) phase, whereas the compound which is insoluble is in the solid state (s). - The solid which is formed in a double displacement reaction is called the precipitate and it is insoluble. - Solubility rules (used in double displacement reactions). 1. All alkali metal ions and ammonium ion (NH4+) are soluble. 2. All nitrates (NO3-) are soluble. 3. All sulfates (SO4-2) are solubleexceptwith Ba+2 , Pb+2 , Ca+2 , Sr+2 , Ag+ . 4. All chlorides, bromides and iodides(Cl-, Br-, I-) aresolubleexcept with Ag+ , Pb+2 , Hg+, Cu+ 5. All OH- are insolubleexceptwith rule 1, and Ba+2 and Sr+2 . 6. All oxides (O2-), sulfides (S2-), sulfites (SO32-), carbonates (CO32-), phosphates (PO43-) are insoluble except with rule 1 Remark: If all compounds formed in a double displacement reaction are soluble (aqueous) then no reaction takes place. Exercise: State whether each of the following compounds is soluble or insoluble ? Na2SO4 : Fe(NO3)2: LiOH: ZnSO4: PbBr2: BaSO4: Mg(OH)2: PbO: NH4Cl: Na2S: Cu(OH)2: KF: Exercise: Complete and balance the following chemical equations: - KNO3 (aq) + NaCl (aq) → - LiCl (aq) + AgNO3 (aq) → - Zn (s) + FeSO4 (aq) → - NaOH (aq) + CuCl2 (aq) → - ZnCl2 (aq) + Na3PO4 (aq) → - Pb(NO3)2 (aq) + K2S (aq) → • Net ionic equation: a chemical equation which shows ONLY the ions that are involved in the formation of the precipitate (solid). Examples: Pb+2 (aq) + S-2 (aq) → PbS (s) Ag+ (aq) + Cl- (aq) → AgCl (s) Cu+2 (aq) + 2 OH- (aq) → Cu(OH)2 (s) • Full ionic equation: an equation which shows All the ions in the soluble (aqueous compounds) in both reactants and products. Example: - 2 NaOH (aq) + CuCl2 (aq) → 2 NaCl (aq) + Cu(OH)2 (s) 2 Na+ (aq) + 2 OH- (aq) + Cu+2 (aq) + 2 Cl- (aq) → 2 Na+ (aq) + 2 Cl- (aq) + Cu(OH)2 (s) - 3 ZnCl2 (aq) + 2 Na3PO4 (aq) → Zn3(PO4)2 (s) + 6 NaCl (aq) Full ionicequation: 3 Zn+2(aq) + 6 Cl-(aq) + 6 Na+ (aq) + 2 PO4-3 (aq) → Zn3(PO4)2 (s) + 6 Na+ (aq) + 6 Cl- (aq) Net ionic equation: 3 Zn+2 (aq) + 2 PO4-3 (aq) → Zn3(PO4)2 (s) Exercise: Complete and balance the following equation, then write full ionic and net ionic equations for the reaction. Pb(NO3)2 (aq) + 2 NaI (aq) → Full ionic equation: Net ionic equation: Spectator ions: the ions that are not involved in the formation of the precipitate (solid). Note that the spectator ions appear on both sides of the full ionic equation. For example, in the above reaction, Na+ (sodium ions) and NO3- (nitrate ions) are the spectator ions. Exercise: Complete and balance the following equation, then write the net ionic equation and identify the spectator ions. BaCl2 (aq) + K2SO4 (aq) → Net ionic equation: Ba+2 (aq) + SO4-2 (aq) → Spectator ions: - Combustion reaction is a special type of (synthesis) reaction in which the substance reacts with (burns in) oxygen. Examples: C(s) + O2(g) → CO2(g) • Production of gases (lab scale): 1. CO2 2. SO2 3. H2 4. H2S (hydrogen sulfide) 5. NH3 (ammonia) General pattern of the chemical reactions to produce the above gases: 1. Metal carbonate + acid → CO2 Example: Na2CO3 (aq) + 2 HCl (aq) → 2 NaCl(aq) + CO2(g) + H2O(l) 2. Metal sulfite + acid → SO2 K2SO3 (aq) + 2 HCl (aq) → 2 KCl(aq) + SO2(g) + H2O(l) 3. Metal + acid → H2 Remark: This is a single displacement reaction therefore the metal used in the reaction should be higher in the reactivity series than hydrogen. Zn (s) + 2 HCl (aq) → ZnCl2 (aq) + H2(g) 4. Metal sulfide + acid → H2S Na2S (aq) + 2 HCl (aq) → 2 NaCl (aq) + H2S (g) 5. Ammonium compound + base (alkaline solution) → NH3 NH4Cl (aq) + NaOH (aq) → NaCl (aq) + NH3 (g) + H2O (l) Exercise: Write the net ionic equations for each of the above 5 reactions. Answers 1. 2 H+ (aq) + CO3-2(aq) → CO2(g) + H2O (l) 2. 2 H+ (aq) + SO3-2(aq) → SO2(g) + H2O (l) 3. Zn(s) + 2 H+(aq) → Zn+2(aq) + H2(g) 4. 2H+ (aq) + S-2 (aq) → H2S (g)
Updated 42d ago
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Know the relationship between molecular weight and rate of diffusion The rate of diffusion is inversely proportional to the molecular weight Small weight-fast diffusion; heavy weight-slow diffusion Identify RBC’s in various solution and determine tonicity Tonicity - the ability of an extracellular solution to make water move into or out of a cell by osmosis If a cell is placed in a hypertonic solution, there will be a net flow of water out of the cell, and the cell will lose volume (shrink). A solution will be hypertonic to a cell if its solute concentration is higher than that inside the cell, and the solutes cannot cross the membrane. If a cell is placed in a hypotonic solution, there will be a net flow of water into the cell, the cell will gain volume (bigger). If the solute concentration outside the cell is lower than inside the cell, then solutes cannot cross the membrane, then the solution is hypotonic to the cell. If a cell is placed in an isotonic solution, there will be no set flow of water into or out of the cell, and the cell’s volume will remain stable. If the solute concentration outside the cell is the same as inside the cell, and the solutes cannot cross the membrane, the solution is isotonic to the cell. Homeostatic feedback loop for respiratory rate, heart rate and temperature Respiratory Rate: Stimulus : The level of carbon dioxide (CO2) in the blood increases (often due to exercise or hypoventilation) . Receptors: Chemoreceptors in the medulla oblongata, carotid arteries, and aortic arch detect changes in blood pH and CO2 levels Control Center: The medulla oblongata processes this information Effectors: Respiratory muscles (diaphragm and intercostal) adjust breathing rate and depth Response: Increased respiratory rate removes CO2 and increases O2 intake, restoring normal pH and gas levels. Heart Rate: Stimulus : Changes in blood pressure, O2, CO2, or pH levels Receptors: Baroreceptors (detect blood pressure changes) in the carotid sinus and aortic arch; chemoreceptors monitor blood chemistry Control Center: The medulla oblongata (cardiac center) processes signals Effectors : The autonomic nervous system (ANS) adjusts heart rate through the sympathetic nervous system (increases heart rate) or parasympathetic nervous system (decreases heart rate) Response : Heart rate increases during low O2 or low blood pressure (to circulate oxygen) and decreases when homeostasis is restored. Temperature Regulation Stimulus: Changes in body temperature (hyperthermia or hypothermia) Receptors: Thermoreceptors in the skin and hypothalamus detect temperature fluctuations. Control Center: The hypothalamus processes this information and signals effectors Effectors and Responses: If too hot: Blood vessels dilate (vasodilation) to release heat, and sweat glands produce sweat for cooling If too cold: Blood vessels constrict (vasoconstriction) to retain heat, and shivering generates warmth. Steps of a generic homeostatic feedback loop Stimulus : A change in the internal or external environment that disrupts homeostasis (eg. temperature change, pH levels, blood sugar levels) Sensor (Receptor) : Specialized cells or receptors detect the change and send information to the control center. Control Center (Integrator): Often the brain or endocrine glands, this component processes the information from the sensors and determines the appropriate response to restore balance. Effector: This component carries out the response to the stimulus as dictated by the control center. Effectors can be muscles or glands that help to counteract the change. Response: The action taken by the effectors to restore homeostasis. This could involve increasing or decreasing a physiological process (e.g. sweating to cool down or shivering to warm up) Feedback: The results of the response are monitored. If homeostasis is restored, the system maintains its state; if not, the loop may repeat, continuing to adjust until balance is achieved. How to evaluate data to determine the set point, error, and disturbance Identify the set point The set point is the optimal level or range that the system aims to maintain. To determine the set point: Gather baseline data: Collect data over a period to understand the normal range for the variable in question (e.g. body temp., BP, blood glucose levels) Analyze Trends: Look for patterns in the data to identify the average or median value that represents the stable condition of the system. Consult Literature: Reference established physiological norms or previous studies to confirm the typical set point for the variable. Assess Disturbance A disturbance is any factor or event that causes a deviation from the set point. To evaluate disturbances: Identify External and Internal Factors: Analyze the data for any external influences (e.g. environmental changes, dietary habits) or internal changes (e.g. illness, stress) that might have impacted the variable. Quantity Disturbance: Measure the magnitude and duration of the disturbance. This can be done by comparing the data points during the disturbance against the established set point. Monitor Changes: Track how the system responds to disturbances over time to assess their impact on maintaining homeostasis. WBC types and normal distribution values/ abnormal values and what those values indicate (infections/diseases) (Never Let Monkeys Eat Bananas) Neutrophils (50-70%) - First responders to infections, especially bacterial. High levels indicate bacterial infections, inflammation, or stress. Low levels can indicate bone marrow disorders or severe infections. Lymphocytes (20-40%) - Include B cells and T cells, important for immunity. High levels can suggest viral infections or leukemia, while low levels might indicate immune deficiency. Monocytes (2-8%) - Help with cleaning up dead cells and fighting infections. High levels can be linked to chronic infections or autoimmune diseases. Eosinophils (1-4%) - Involved in allergic reactions and fighting parasites. Elevated levels may indicate allergies or parasitic infections. Basophils (0.5-1%) - Release histamine during allergic reactions. High levels might be see in allergic conditions or blood disorders. Normal WBC Count Total WBC Count: 4000-11000 cells per microliter of blood (varies slightly by lab) Leukocytosis (High WBC): Can indicate infection, inflammation, stress, or leukemia Leukopenia (Low WBC): Can result from bone marrow disorders, viral infections, or autoimmune diseases Neutrophils: Banded vs Segmented Neutrophils are the most abundant type of white blood cells and play a crucial role in fighting infections. They exist in different stages of maturation: Banded Neutrophils (“Bands”) - Immature Neutrophils Appearance: Have a curved, unsegmented nucleus (band-shaped) Normal Range: 0-6% of total WBC count (~0-700/uL) Clinical Significance: Increased Bands (Bandemia) -> Indicates an acute bacterial infection or severe stress (e.g. sepsis). The bone marrow releases immature neutrophils in response to infection. Low Bands -> Not clinically significant unless the total WBC count is low, which could suggest bone marrow suppression. Segmented Neutrophils (“Segs”) - Mature Neutrophils Appearance: Have a segmented nucleus with 2-5 lobes Normal Range: 50-70% of total WBC count (~2500-7000/uL) Clinical Significance: High Segs (Neutrophilia) -> Suggests bacterial infections, stress, chronic inflammation, or leukemia Low Segs (Neutropenia) ->Can be caused by viral infections, bone marrow disorders, chemotherapy, or autoimmune diseases. Discuss the stages of cell cycle/mitosis-which stages are longest/shortest The cell cycle is a series of events that cells go through to grow and divide. It consists of two main phases: Interphase (Longest Phase) – Preparation for division Mitosis (Shortest Phase) – Actual cell division Stages of the Cell Cycle Interphase (90% of the Cell Cycle – Longest Phase) Interphase is the period of cell growth and DNA replication. It has three subphases: G1 Phase (Gap 1) The cell grows, produces proteins, and prepares for DNA replication. Longest variable phase; some cells may stay here indefinitely (e.g., neurons in G0 phase). S Phase (Synthesis) DNA replication occurs, ensuring each daughter cell gets a complete genome. Takes about 6-8 hours in human cells. G2 Phase (Gap 2) The cell prepares for mitosis by producing proteins and organelles. Shorter than G1 but still significant in length. Mitosis: Prophase, Metaphase, Anaphase, Telophase Know proportional and inversely proportional relationships Direct (Proportional) Relationship When two quantities increase or decrease together at a constant rate, they are directly proportional. Inversely Proportional When one variable increases, the other decreases proportionally. Know relationship between molecular weight and rate of diffusion The rate of diffusion of a substance is inversely proportional to the square root of its molecular weight. Lighter molecules diffuse faster Heavier molecules diffuse slower due to greater mass. Know relationship between filtration rate and pressure of fluid or weight of fluid Filtration rate is directly proportional to the pressure or weight of the fluid driving the filtration process. Higher pressure → Higher filtration rate Lower pressure → Lower filtration rate Know why men and women blood values are different The differences in blood values between men and women are due to biological, hormonal, and physiological factors
Updated 44d ago
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