Results for "Sodium"

Lecture 22 - Sodium Balance

Lecture 4: Sodium and Water Balance II

Lecture 3: Sodium and Water Balance

4. Metals and Non-metals Learning Objectives By the end of the lesson, you will be able to: ☑ distinguish between metals and non-metals ☑ describe the physical and chemical properties of metals and non-metals ☑ list the uses of some metals and non-metals MINERALS AND ORES You have learnt that all materials Here is the exact text from the image:are made up of basic substances called elements, and that elements cannot be split into simpler substances by chemical methods. There are 118 known elements. Sodium, zinc, gold, mercury, iron, lead, barium and tin (metals); and hydrogen, oxygen, carbon, sulphur, chlorine, boron, neon and radon (non-metals) are some examples. Only certain unreactive elements are found free in nature. Others occur in combined states as minerals. A mineral is a solid inorganic substance that is found in nature. A mineral deposit that can be mined and from which an element or compound can be obtained profitably is known as an ore. Elements can be broadly classified into two groups—metals and non-metals. Table 4.1 Some common ores Fig. 4.1 Some common ores a. Bauxite (aluminium) b. Malachite (copper) c. Haematite (iron) d. Galena (lead) e. Apatite (phosphorus) f. Quartz (silicon) -- --- METALS All except 20 of the known elements are metals. Most metals are reactive; they combine with other elements in nature, such as oxygen and sulphur, and occur as oxides, sulphides and carbonates. Only a few unreactive metals like gold, silver and platinum are found as free metals in the Earth's crust. Physical Properties of Metals Metals are solids at room temperature, except mercury, which is a liquid at room temperature (Fig. 4.2(a)). They are generally hard and strong, with a few exceptions such as sodium and potassium, which are soft and can be easily cut with a knife (Fig. 4.2(b)). They have a metallic lustre (shine), especially when freshly cut. They have high melting and boiling points, with a few exceptions like sodium, potassium and mercury. They are good conductors of heat and electricity. Silver and copper are the best conductors of electricity, followed by gold and aluminium. Metals are sonorous. They produce a ringing sound when struck. Most metals have high tensile strength. They can take heavy loads without breaking. They are malleable. Metals, with exceptions like sodium and potassium, can be beaten into thin sheets and foils. They are ductile. Metals, with exception like sodium and potassium, can be drawn into wires. Most metals have high density. However, sodium and potassium have low density and float on water. Fig. 4.2 Special metals a. Mercury b. Sodium --- Chemical Properties of Metals Reaction with oxygen Metals react with oxygen under different conditions to form basic oxides. These basic oxides react with water to form bases. Sodium and potassium react vigorously with oxygen at room temperature. 4Na + O_2 \rightarrow 2Na_2O To prevent this oxidation, sodium and potassium are stored under kerosene. Magnesium reacts with oxygen only when ignited. It burns with a dazzling bright flame and forms a white powder of magnesium oxide. 2Mg + O_2 \rightarrow 2MgO Copper and iron react with oxygen only when heated to a very high temperature. 2Cu + O_2 \rightarrow 2CuO --- --- Reaction with water Metals react with water to form hydroxides or oxides, along with hydrogen. Different metals react at different temperatures. Sodium, potassium, and calcium react with cold water to form hydroxides. 2Na + 2H_2O \rightarrow 2NaOH + H_2 Magnesium Reacts with steam or hot water to form magnesium oxide. Mg + H_2O \rightarrow MgO + H_2 Aluminium Forms an oxide too, but this oxide forms a protective covering over the metal and prevents further reactions. 2Al + 3H_2O \rightarrow Al_2O_3 + 3H_2 Zinc Reacts only with steam. Zn + H_2O \rightarrow ZnO + H_2 Iron Reacts with steam when heated strongly. 2Fe + 3H_2O \rightarrow Fe_3O_4 + 3H_2 Copper, gold, silver, and platinum do not react with water at all. --- Activity 4.1 Teacher Demonstration Aim: To study the reaction of metals with water. [Caution: This activity should be demonstrated by the teacher, and students should stand away from the table.] Materials required: Two 200 mL beakers Pieces of sodium and calcium Forceps Knife Litmus papers Water Method: 1. Fill each beaker with 100 mL of water. 2. Using forceps and a knife, cut a small piece of sodium. 3. Dry it on a tissue paper and drop it into one of the beakers. 4. Repeat the same procedure with calcium. 5. Test the water in both the beakers with red and blue litmus papers. Observations and Conclusions: Sodium reacts vigorously and may explode. A gas is also released. The reaction with calcium is quick, though not as vigorous as that with sodium. In both cases, the red litmus paper turns blue, showing that the solutions are bases. --- Reaction with dilute acids Most metals react with dilute acids to form their salts and liberate hydrogen gas. The reaction with reactive metals like sodium, potassium, and calcium is violent. Magnesium, aluminium, zinc, and iron do not react violently. Mg + 2HCl \rightarrow MgCl_2 + H_2 Copper, silver, gold, and platinum do not react with dilute acids. --- Reaction with bases Only some metals such as aluminium and zinc react with strong bases like sodium hydroxide to liberate hydrogen gas. Zn + 2NaOH \rightarrow Na_2ZnO_2 + H_2 --- Activity 4.2 Aim: To study the reaction of metals with dilute hydrochloric acid. Materials required: Sandpaper Six test tubes Dilute hydrochloric acid Strips of magnesium, zinc, iron, tin, lead, and copper Method: 1. Clean the metal strips with sandpaper. 2. Add dilute hydrochloric acid to the six test tubes. 3. Insert a strip of metal into each test tube. Observe if any bubbles are formed in the test tubes. If no bubbles are seen, warm them gently in a beaker of hot water. 4. Observe the speed at which gas is generated. This gives an idea of the speed of the reaction. 5. Classify the metals in order of their reactivity with dilute hydrochloric acid. [Caution: Acids are corrosive and should be handled carefully.] --- Activity 4.3 Aim: To study the reaction of metals with bases. Materials required: Small piece of zinc Beaker Sodium hydroxide Method: 1. Prepare warm sodium hydroxide or caustic soda solution. 2. Drop the piece of zinc into it. Observations and Conclusions: You will notice that zinc reacts with sodium hydroxide to liberate hydrogen gas. Observations on Metals with Dilute Acids Metals like sodium, potassium, and calcium react violently with dilute acids to liberate hydrogen gas. Magnesium, aluminium, zinc, and iron also displace hydrogen from dilute acids, but the reaction is not violent. Metals such as copper, silver, gold, and platinum do not displace hydrogen from dilute acids. --- Activity Series of Metals The activity series of metals is the arrangement of metals in decreasing order of reactivity. The series in the book shows reactivity decreasing from top to bottom. Potassium is the most reactive metal while gold is the least reactive. --- Displacement of a Metal by Other Metals A more reactive metal displaces a less reactive metal from its compounds in an aqueous solution. Some examples: Mg + CuSO_4 \rightarrow MgSO_4 + Cu Zn + FeSO_4 \rightarrow ZnSO_4 + Fe Iron can displace copper from copper sulphate solution (as shown in Activity 4.4). The solution turns green, and reddish-brown copper deposits on the iron nail. Copper cannot displace iron from iron sulphate solution, showing that copper is less reactive than iron. Cu + FeSO_4 \rightarrow \text{No reaction} Question: What do you think will happen if you place a silver spoon in copper sulphate solution? --- Activity 4.4 - Displacement Reaction Aim: To study a displacement reaction. Materials Required: Test tube Iron nail Copper sulphate solution Method: 1. Fill the test tube with copper sulphate solution (blue in colour). 2. Place the clean iron nail in the solution. Observations and Conclusions: After about an hour, the solution changes to green, and a reddish-brown deposit is formed on the iron nail. --- Corrosion of Metals Corrosion is the destruction or damage of a material due to chemical reaction. Rusting of iron happens when iron is exposed to moist air, forming a reddish-brown layer of rust. Rust is iron oxide, which eventually flakes off, damaging the object. Definition written on the page: "Slow eating of a metal’s surface due to oxidation is called corrosion of metals." --Observations on Metals with Dilute Acids Metals like sodium, potassium, and calcium react violently with dilute acids to liberate hydrogen gas. Magnesium, aluminium, zinc, and iron also displace hydrogen from dilute acids, but the reaction is not violent. Metals such as copper, silver, gold, and platinum do not displace hydrogen from dilute acids. --- Activity Series of Metals The activity series of metals is the arrangement of metals in decreasing order of reactivity. The series in the book shows reactivity decreasing from top to bottom. Potassium is the most reactive metal while gold is the least reactive. --- Displacement of a Metal by Other Metals A more reactive metal displaces a less reactive metal from its compounds in an aqueous solution. Some examples: Mg + CuSO_4 \rightarrow MgSO_4 + Cu Zn + FeSO_4 \rightarrow ZnSO_4 + Fe Iron can displace copper from copper sulphate solution (as shown in Activity 4.4). The solution turns green, and reddish-brown copper deposits on the iron nail. Copper cannot displace iron from iron sulphate solution, showing that copper is less reactive than iron. Cu + FeSO_4 \rightarrow \text{No reaction} Question: What do you think will happen if you place a silver spoon in copper sulphate solution? --- Activity 4.4 - Displacement Reaction Aim: To study a displacement reaction. Materials Required: Test tube Iron nail Copper sulphate solution Method: 1. Fill the test tube with copper sulphate solution (blue in colour). 2. Place the clean iron nail in the solution. Observations and Conclusions: After about an hour, the solution changes to green, and a reddish-brown deposit is formed on the iron nail. --- Corrosion of Metals Corrosion is the destruction or damage of a material due to chemical reaction. Rusting of iron happens when iron is exposed to moist air, forming a reddish-brown layer of rust. Rust is iron oxide, which eventually flakes off, damaging the object. Definition written on the page: "Slow eating of a metal’s surface due to oxidation is called corrosion of metals." Uses of Metals (Continued) Aluminium Used in high-voltage electric lines. Alloys like duralumin and magnalium are used in aircraft and automobile bodies. Used for making aluminium foil and cooking utensils. Copper Good conductor of electricity → Used in electrical wires, cables, motors, and transformers. Good conductor of heat → Used in the bottoms of stainless steel vessels. Zinc Used to make corrosion-resistant galvanised iron (GI) pipes and sheets. Used as an electrode in dry cells. Other Metals Gold and silver → Used in jewellery. Lead → Used in electrodes of lead storage batteries (used in automobiles and inverters). Chromium → Used for electroplating iron to give a shiny, corrosion-resistant finish. --- Looking Back (True/False Statements) 1. Gold, silver, and platinum are found in the Earth’s crust as free metals. → True 2. Most metals are solids that are soft. → False 3. Metals such as zinc and magnesium react with dilute acids to liberate oxygen. → False 4. A less reactive metal displaces a more reactive metal from its aqueous solution. → False 5. The chemical name of rust is zinc oxide. → False (Rust is Fe₂O₃.xH₂O) 6. Coating zinc objects with iron is called galvanising. → False (Galvanising is coating iron with zinc) Non-Metals Physical Properties of Non-Metals Exist as gases or solids at room temperature (except bromine, which is liquid). Not as hard as metals (except diamond, which is very hard). Low tensile strength and low density. Low melting and boiling points (except graphite). Not sonorous (do not produce a ringing sound). Not malleable or ductile (cannot be beaten into sheets or drawn into wires). Do not have lustre (except iodine and graphite). Bad conductors of heat and electricity (except graphite, and silicon under specific conditions). --Chemical Properties of Non-Metals Reaction with Water Most non-metals do not react with water. Highly reactive non-metals (e.g., phosphorus) catch fire in air, so they are stored in water. Fluorine, chlorine, and bromine react with water to form acids. Reaction with Oxygen Non-metals react with oxygen to form acidic or neutral oxides. Carbon and sulfur react with oxygen to form acidic oxides, which dissolve in water to form acids. Some oxides (e.g., CO, N₂O) are neutral and do not form acids. Examples: Carbon + Oxygen → Carbon Dioxide (CO₂) CO₂ + Water → Carbonic Acid (H₂CO₃) Sulfur + Oxygen → Sulfur Dioxide (SO₂) SO₂ + Water → Sulfurous Acid (H₂SO₃) Reaction with Acids Unlike metals, non-metals do not replace hydrogen in acids. Silicon reacts with hydrofluoric acid (HF). --Uses of Non-Metals Hydrogen Used in the manufacture of ammonia and industrial chemicals. Used in vanaspati (a cooking oil). Oxygen Used in breathing support systems in hospitals. Used with other gases in equipment to weld metals. Sulphur Used in the manufacture of sulphuric acid, sulphur dioxide gas, and other industrial chemicals. Used to make pesticides for agriculture. Used in vulcanising rubber (making it harder) and in gunpowder. Nitrogen Used in the manufacture of ammonia and nitrogenous fertilisers like ammonium nitrate and ammonium sulphate. Used as an inert gas in processed food packaging to prevent rancidity. Silicon Used in making semiconductors for microchips. Silicates (oxides of silicon) are used in making glass. Other Non-Metals Phosphorus: Used in making fertilisers (superphosphates). Chlorine: Used for disinfecting drinking water. Argon: Used in welding stainless steel and filling electric bulbs. Helium: Used in balloons for meteorological observations. Neon: Used in fluorescent lights for advertisement displays

PHOSPHORUS, SODIUM, AND POTASSIUM

Cation tests (aqueous sodium hydroxide)

You place a RBC (0.9%) into a 5% sugar solution. Which statement below is false? The RBC is hypotonic to the 5% solution Which is an example of a sensor in a negative homeostatic feedback loop? Chemoreceptor in carotid body For membrane fluidity experiment, the part of the experiment that actually validated that the membrane was fluid was: The labeled antibodies of the human and mouse intermixing An example of primary active transport would be a protein requiring ATP to transport sodium ions across the plasma membrane. True If a red blood cell is put in a solution and it hemolyzes, then the solution is considered to be: Hypotonic If your body temperature goes too high you can denature enzymes in your body. True What does an integrator do in a homeostatic pathway? Measures the signal coming in to a set point and send a signal out to the body Which of the following represents stages of the cell division (mitosis) in the proper sequence? Prophase, metaphase, anaphase, telophase Which is not true for proteins? They are comprised of mostly cellulose What would be a disturbance for blood glucose homeostasis (normal blood glucose set point = 77mg/dL)? A permanent decrease in insulin production from the Islets of Langerhans Dr. Bio measures your total cholesterol and he reports back to you that your level is 300 mg/ 100 ml of plasma. You do what? Eat more oatmeal and flax to increase your HDL level. How do you make an unsaturated fatty acid? Perform a dehydration synthesis reaction on a saturated fatty acid Which is false for antioxidants? They speed up reactions in your body Which molecules do not dissolve in water? Non-polar Which molecule requires a transport protein to get through the plasma membrane (either channel or carrier protein)? Two of the answers are correct Interphase is considered to be part of normal cell division (mitosis). False What is the function of ATP? All of the answers are correct What are the three kinds of lipids? Triglycerides, phospholipids, and steroids When glycerol combines with 3 fatty acids to form a triglyceride (fat), which of the following chemical reactions has occurred? Dehydration Synthesis How can you alter a protein’s shape? More than one answer is correct If a red blood cell is put into a solution and it maintains its shape, then the solution is considered to be: Isotonic Which molecule requires some type of transport protein to get through the plasma membrane? Sodium Ion Cofactors are molecules that activate enzymes. Which is not a cofactor? Mercury The nitrogenous bases found in DNA have complementary paring. Which pair is correct? C-G Which is not true for meiosis? Results in a gamete that is 2N In the diagram below the two solutions are separated by a semi permeable membrane. In which direction will net movement of water occur? From side A to side B Which is not a component of a DNA molecule: Ribose Sugar Phospholipids are similar to fatty acids except for? Phospholipids have a phosphate group Which is not true for cells? They allow diffusion of all molecules If you combine a molecule of glucose and fructose, which statement is true? You have formed sucrose Which is true for enzymes? Activity will increase until the enzyme becomes saturated What method would you use to get glucose into a cell along/down it’s concentration gradient (from high to low)? Facilitated Diffusion Which is not considered an integrator in a negative homeostatic feedback loop? Pancreas Which phase of the cell cycle is where cytokinesis takes place? Telophase What vitamin do we produce by sitting in the sun; it aids in calcium absorption from the small intestine? Vitamin D Why is it important to think about ion dissociation in the body? All the above In what order do you use macromolecules for fuel? Carbohydrates, lipids, proteins Which is false for cholesterol? It can dissolve in water/blood You place a RBC (0.9%) into a 0.5% sugar solution. Which statement below is false? The RBC is hypertonic to the 0.5% solution Which is not a membrane protein function? Protein synthesis Ingesting (eating) excess hydrophilic vitamins, such as vitamin C, results in excess vitamin C being stored in your tissues. False Diffusion is: The movement of molecules from an area of high molecular concentration to an area of low molecular concentration across a selectively-permeable membrane The hormone responsible for glucose uptake/removal from the blood is: Insulin What method would you use to get sodium ions into a cell against sodium’s concentration gradient (from low to high concentration)? Active Transport Which phase of the cell cycle is where the cell is functioning normally or doing its job? Interphase Evidence for mitochondria once being bacteria that our cells engulfed is: It has it’s own DNA Ionic molecules (ie NA+, K+) can diffuse straight through the plasma membrane. True What is the difference between cis and trans fatty acids? Cis fatty acids have hydrogens on the same side of the carbon double bond and trans fatty acids do not Cofactors are molecules that activate enzymes. Where do we get cofactors from? Vitamins found in fruits and vegetables RNA has what nitrogenous base in place of thymine? Uracil Large polar molecules (ie glucose) can diffuse straight through the plasma membrane? False Which lipoprotein is comprised of more protein and less cholesterol so it scavenges for cholesterol in the blood? High density lipoprotein A normal human being has 46 chromosomes (23 pairs/2N/diploid) in each somatic cell (body cell). True The three main compounds digested by the digestive system are? Fats, carbohydrates, and proteins Meiosis is the process in which our sex cells go from 46 chromosomes to 23 single chromosomes. True The effector in any negative feedback loop is usually: An organ/tissue If a red blood cell is put into a solution and it crenates (shrinks), then the solution is considered to be: Hypertonic Which statement is false for glycogen? It is a disaccharide Enzymes aid in digestion by? Lowering the energy required to break food apart Nonpolar molecules (ie CO2) can diffuse straight through the plasma membrane

Please wait outside until I let you in, and put all your stuff at the back just like we've done about 20 times already this semester. Okay? Or this semester and last, and you will be just fine. Now your lecture exam too is 90 marks big. It is 90 multiple choice questions. Okay. It is going to be on cardiovascular disorders, urinary system, fluid balance, Okay. So let's start talking about them. First of all, okay, you need to know the difference between a myocardial infarct, ischemic attack, a congestive heart failure, and angina pectorals. You need to know what a low level inflammatory response that develops over time where the endothelium is damaged due to the aging or prolonged hypertension, where LDLs accumulate, and the endothelium is repaired with collagen is called. That might take you a long time to read. Okay? But it is a good question. Okay? You need to know now be really, really clear on these. Okay? You absolutely need to know the difference between right ventricular hypertrophy and left ventricular hypertrophy and what they cause. Because there's two questions on here, and so far, this one hasn't been done very well. Okay? Make sure you understand what right ventricular hypertrophy leads to and you understand what left ventricular hypertrophy leads to. Now the original term, congestive heart failure, that refers to left ventricular hypertrophy leading to backup in the lungs. K? You need to know what arteries or vessels are used in bypass surgery. You need to know what a mini stroke is. Okay? You need to know the difference between thrombus and ballast occlusion and arthroma. You need to know what is a restriction in blood supply generally due to factors in the blood vessels with resultant damage or dysfunction of tissue. You need to know, what are the consequences of an aging cardiovascular system. And then I I've got a matching question for you. You need to match the basic function of the proximal convoluted tubule, the glomerulus, and the peri colic duct. And then two of my favorite questions. Are you ready? Okay. You have to find out which of the following is the best explanation for why the cells of the proximal convoluted tubule contain so many microclonary. Oh, isn't that lovely? Okay. And then the other one you need to know is you need to find the best explanation for the microvilli on the apical surface of the proximal convoluted tubules. So don't get that one wrong because we've talked about microvilli about a bazillion times. Okay? This picture is gonna be on there, folks. Okay? This is the picture of the of the nephron from your textbook. Okay. You need to label things like glomerulus glomerulus afferent arteriole collecting duct nephron move. Okay. Where do you find the granular cells? Okay. The difference between the medulla and the cortex. Make sure you know all of those things. I'll read you this one. This is a good question too. Hydrostatic pressure is the primary driving force of plasma through the filtration membrane into the capsular space. All the publicly following statements reflects why hydrostatic pressure is so high in the glomerular capillaries. Select the one statement that does not explain the high pressure within the glomerular capillaries. So you need to know why glomerular capillary pressure is higher than the rest of the capillaries in the body. You need to know how or why cells or transport proteins are prevented from moving through how yeah. What drives reabsorption of organic nutrients in the proximal condylated tubule? Who drives thus? You need to know the mechanism that establishes the medullary osmotic gradient the The functional and structural unit of the kidneys is what? The g force pushing the blood and solids out of the blood across the filtration membrane is what? Okay. The macular densities cells do what? Function in angiotensin two is to do what? What is, specific gravity or density? Okay. If you talk about the specific gravity or density of urine, how is it different from water? You need to actually, this is just one question, but it should be a pretty simple one. Okay? You need to place the following and correct sequence from the formation of a drop of urine to its elimination of the body. And so you have to go through from well, I'll just read it to you. Major calyx, minor calyx, nephron, urethra, ureter, and collecting that. So you need to put those in order from start to finish. Okay? What would happen if the capsular hydrostatic pressure were increased above normal? You need to know what would happen. Reabsorption of bilevels of glucose and amino acids in the filtrate is accomplished. The 44 more. Okay. So you need to match to their definition. All of your hypo and hypers. Make sure you have some under control. Okay? And then you need to match possible causes. So there's possible causes of respiratory alkalosis, metabolic alkalosis, metabolic acidosis, and respiratory acidosis. Respiratory alkalosis, metabolic alkalosis, metabolic acidosis, and respiratory acidosis. There are possible causes for those four things. You need to match the disorder to the cause. Okay? And then you need to know, the body's motor volume is mostly tied to the level of then I have a couple of clinical correlation questions for you, but they are multiple choice this time. So something happened to Jane. You have to tell me what's happening to Jane. Okay? Now whereas sodium is mainly found in the extracellular fluid, most is found in intracellular systems are. Okay. Which of the following is not a likely source of hydrogen ions in blood plasma, so there's a few types in the tablets, so make sure you know which ones are going to produce acids and which ones aren't. And then Annie had something happen to her as well. Across capillary walls is what? Regulation of potassium balance is what? Now Dave Dave did something silly. Okay? Dave ran a marathon. Okay? And then Dave did something even more silly afterwards. I want you to tell me what happened to Dave. And in addition to that, Nancy is having a panic attack. So I want you to tell me what's happening to Nancy in terms of respiratory aesophosis and respiratory aldosterone. Okay. If thyroid and parathyroid glands were surgically removed, which of the following would go out of balance without replacement therapy? Falling arterial blood pressure holds which? An illness, Doug. Doug has severe diarrhea. Okay. And, is accompanying the loss of bicarbonate or secretions. So how is Doug gonna compensate for that for Doug? Okay. You need to know what the medical term for kidney stones is. You need to know what happens, or what could cause the passage of proteins, red blood cells, and white blood cells into the urine. You need to know how to solve prostatic enlargement, and, you need to know what the presence of white blood cells in urine is called and what is causing it. Okay? And then there's a picture of the lymphatic of the lymph node. Okay. You need to label the lymph node picture. And then you there is going to be a matching question on lymphatic structures, so you need to know what happens in the spleen, the lymph nodes, the thoracic duct, the lymph, and the pyre patches. There's a list, a small short list. Okay? So in other words, you're going to need to know what is classified as a lymphoid organ and what does not. Okay? So make sure you know what your lymphoid organs are. You need to know the pathway of lymph. So it starts in lymph capillaries. Where does it end? Make sure you know all the steps along the way. And then you need to know the functions of the spleen. What did what does the spleen do? And that is it for an example

1. Hyperemesis Gravidarum/ Pernicious Vomiting Definition: Excessive nausea and vomiting during pregnancy, extending beyond week 12 or causing dehydration, ketonuria, and significant weight loss within the first 12 weeks. Incidence: 1 in 200-300 women Cause: Unknown, but may be associated with increased thyroid function and Helicobacter pylori infection. Signs and Symptoms: • Decreased urine output • Weight loss • Ketonuria • Dry mucous membranes • Poor skin turgor • Elevated hematocrit • Decreased sodium, potassium, and chloride levels • Polyneuritis (in some cases) Assessment: • Hemoglobin: Elevated hematocrit concentration (hemoconcentration) due to inability to retain fluids. • Electrolytes: Decreased sodium, potassium, and chloride levels due to low intake. • Acid-base Balance: Hypokalemic alkalosis (severe vomiting, prolonged period). • Neurological Examination: Polyneuritis due to B vitamin deficiency. Effects (if left untreated): • Intrauterine Growth Restriction (IUGR): Dehydration and inability to provide nutrients for fetal growth. • Preterm birth: Due to complications caused by the condition. • Prolonged hospitalization/home care: Resulting in social isolation. Therapeutic Management: • Fluid and Electrolyte Management: Monitor input and output, blood chemistry to prevent dehydration. • Nutritional Support: Withhold oral food and fluids (usually) and administer total parenteral nutrition (TPN). • Intravenous Fluid Replacement: 3000 ml Ringer's lactate with added vitamin B to increase hydration. • Antiemetic Medication: Metoclopramide (Reglan) to control vomiting. 2. Ectopic Pregnancy Definition: Implantation of a fertilized egg outside the uterine cavity (ovary, cervix, fallopian tube - most common). Incidence: Second most frequent cause of bleeding during the first trimester. Causes: • Obstruction of the fallopian tube: ◦ Adhesions (from previous infection like chronic salpingitis or pelvic inflammatory disease). ◦ Congenital malformations. ◦ Scars from tubal surgery. ◦ Uterine tumor pressing on the proximal end of the tube. ◦ Current use of an intrauterine device (IUD). Signs and Symptoms: • Missed period/amenorrhea. • Positive hCG test. • Sharp, stabbing pain in the lower abdominal quadrants and pelvic pain (at time of rupture). • Scant vaginal spotting/bleeding. • Rigid abdomen (from peritoneal irritation). • Leukocytosis (increased WBC count due to trauma). • Decreased blood pressure and increased pulse rate (signs of shock). • Cullen's sign (bluish tinge around the umbilicus). • Tender mass palpable in the cul-de-sac of Douglas (vaginal exam). • Falling hCG or serum progesterone level (suggesting the pregnancy has ended). • No gestational sac on ultrasound. Therapeutic Management: • Non-ruptured Ectopic Pregnancy: Oral administration of methotrexate followed by leucovorin. • Ruptured Ectopic Pregnancy (emergency): Laparoscopy to ligate bleeding vessels and remove or repair the damaged fallopian tube. 3. Hydatidiform Mole (H-mole)/ Gestational Trophoblastic Disease/ Molar Pregnancy Definition: A gestational anomaly of the placenta consisting of a bunch of clear vesicles resembling grapes. This neoplasm is formed from the swelling of the chorionic villi, resulting from a fertilized egg whose nucleus is lost, and the sperm nucleus duplicates, producing a diploid number 46XX. Incidence: Approximately 1 in every 1500 pregnancies. Risk Factors: • Low socioeconomic group (decreased protein intake). • Women under 18 or over 35 years old. • Women of Asian heritage. • Receiving clomiphene citrate (Clomid) for induced ovulation. Types of Molar Growth: • Complete/Classic H-mole: All trophoblastic villi swell and become cystic. No embryonic or fetal tissue present. High risk for malignancy. • Partial/Incomplete H-mole: Some of the villi form normally. Presence of fetal or embryonic tissue. Low risk for malignancy. Signs and Symptoms: • Uterus expands faster than normal. • No fetal heart sounds heard. • Serum or urine test for hCG strongly positive. • Early signs of preeclampsia. • Vaginal bleeding (dark-brown spotting or profuse fresh flow). • Discharge of fluid-filled vesicles. Diagnosis: • Ultrasound. • Chest x-ray (lung metastasis). • Amniocentesis (no fluid). • Hysteroscopy (via cervix). Management: • Evacuation of the mole: Dilation and curettage (D&C). • Blood transfusion. • Hysterectomy (in some cases). • Monitoring hCG levels: Every 2 weeks until normal. • Contraception: Reliable method for 12 months to prevent confusion with a new pregnancy. 4. Premature Cervical Dilatation/ Incompetent Cervix Definition: Premature dilation of the cervix, usually occurring around week 20, when the fetus is too immature to survive. Incidence: About 1% of pregnancies. Causes: • Increased maternal age. • Congenital structural defects. • Trauma to the cervix (cone biopsy, repeated D&C). Signs and Symptoms: • Painless dilation of the cervix. • Pink-stained vaginal discharge. • Increased pelvic pressure. • Rupture of membranes and discharge of amniotic fluid. Therapeutic Management: • Cervical cerclage: Surgical procedure to prevent loss of the child due to premature dilation. • Bed rest: After cerclage surgery, to decrease pressure on the sutures. 5. Abortion Definition: Termination of pregnancy before the fetus is viable (400-500 grams or 20-24 weeks gestation). Types of Abortion: • Spontaneous Abortion: Pregnancy interruption due to natural causes. ◦ Threatened: Mild cramping, vaginal spotting. ◦ Inevitable/Imminent: Profuse bleeding, uterine contractions, cervical dilation. ◦ Complete: All products of conception expelled spontaneously. ◦ Incomplete: Part of the conceptus expelled, some retained in the uterus. ◦ Missed: Fetus dies in utero but is not expelled. ◦ Habitual: 3 or more consecutive spontaneous abortions. • Induced Abortion: Deliberate termination of pregnancy in a controlled setting. Complications of Abortion: • Hemorrhage. • Infection (endometritis, parametritis, peritonitis, thrombophlebitis, septicemia). Management: • Bed rest. • Emotional support. • Sedation. • D&C: Surgical removal of retained products of conception. • Antibiotics. • Blood transfusion. 6. Placenta Previa Definition: The placenta is implanted in the lower uterine segment, covering the cervical os, obstructing the birth canal. Incidence: 5 per 1000 pregnancies. Signs and Symptoms: • Abrupt, painless vaginal bleeding (bright red). • Bleeding may stop or slow after the initial hemorrhage, but continue as spotting. Types: • Total: Placenta completely obstructs the cervical os. • Partial: Placenta partially obstructs the cervical os. • Marginal: Placenta edge approaches the cervical os. • Low-lying: Placenta implanted in the lower rather than the upper portion of the uterus. Therapeutic Management: • Immediate Care: Bed rest in a side-lying position. • Assessment: Monitor vital signs, bleeding, and fetal heart sounds. • Intravenous Therapy: Fluid replacement with large gauge catheter. • Delivery: Vaginal birth (safe for infant if previa is less than 30%). Cesarean section (safest for both mother and infant if previa is over 30%). 7. Abruptio Placenta/ Premature Separation of Placenta/ Accidental Hemorrhage/ Placental Abruption Definition: Separation of a normally implanted placenta after the 20th week of pregnancy, before birth of the fetus. Incidence: Most frequent cause of perinatal death. Causes: • Unknown. • Predisposing Factors: ◦ High parity. ◦ Advanced maternal age. ◦ Short umbilical cord. ◦ Chronic hypertensive disease. ◦ PIH. ◦ Trauma (automobile accident, intimate partner abuse). ◦ Cocaine or cigarette use. ◦ Thrombophilitic conditions (autoimmune antibodies). Classification: • Total/Complete: Concealed hemorrhage. • Partial: Concealed or apparent hemorrhage. Signs and Symptoms: • Sharp, stabbing pain in the uterine fundus. • Contractions accompanied by pain. • Uterine tenderness on palpation. • Heavy vaginal bleeding (may be concealed). • Signs of shock. • Tense, rigid uterus. • Disseminated Intravascular Coagulation (DIC). Therapeutic Management: • Fluid Replacement: IV fluids. • Oxygen: Limit fetal hypoxia. • Fetal Monitoring: External fetal heart rate monitoring. • Fibrinogen Determination: IV fibrinogen or cryoprecipitate. • Lateral Position: Prevent pressure on the vena cava. • Delivery: CS is the method of choice if birth is not imminent. 8. Premature Rupture of Membranes Definition: Rupture of the fetal membranes with loss of amniotic fluid during pregnancy before 37 weeks. Incidence: 5%-10% of pregnancies. Causes: • Unknown. • Associated with: Infection of the membranes (chorioamnionitis), vaginal infections (gonorrhea, streptococcus B, Chlamydia). Signs and Symptoms: • Sudden gush of clear fluid from the vagina with continued minimal leakage. • Nitrazine paper test: Amniotic fluid turns the paper blue (alkaline), urine remains yellow (acidic). • Microscopic examination: Amniotic fluid shows ferning, urine does not. • Ultrasound: Assess amniotic fluid index. • Signs of infection (increased WBC count, C-reactive protein, temperature, tenderness, odorous vaginal discharge). Therapeutic Management: • Bed Rest: To prevent further leakage and risk of infection. • Corticosteroids: To hasten fetal lung maturity. • Prophylactic Antibiotics: To reduce risk of infection. • Intravenous Penicillin/Ampicillin: If (+) for streptococcus B. • Induction of Labor: If fetus is mature and labor does not begin within 24 hours. 9. Pregnancy-Induced Hypertension (PIH)/ Toxemia Definition: Vasospasm occurring in both small and large arteries during pregnancy, causing elevated blood pressure, proteinuria, and edema. Incidence: Rarely occurs before 20 weeks of pregnancy. Risk Factors: • Multiple pregnancy. • Primiparas younger than 20 or older than 40. • Low socioeconomic background. • Five or more pregnancies. • Hydramnios. • Underlying diseases (heart disease, diabetes). • Rh incompatibility. • History of H-mole. Categories: • Gestational Hypertension: Blood pressure 140/90 or greater, without proteinuria or edema. • Preeclampsia: Blood pressure 140/90 or greater, with proteinuria and edema. • Eclampsia: Seizures or coma accompanied by preeclampsia. Therapeutic Management: • Preeclampsia: Bed rest, balanced diet, left lateral position. • Severe Preeclampsia: Hospitalization, diazepam, hydralazine, magnesium sulfate. • Eclampsia: Magnesium sulfate, diazepam, oxygen therapy, left lateral position

Ch 2 Chemical Compounds and Bondings Chemical bond: force of attraction between 2 atoms or 2 ions. There are 2 main types of chemical bonds: 1. Ionic bond: a bond between a metallic atom (metal) and a non-metallic atom (non-metal) in which there is a complete transfer of electrons from the metal to the non-metal. The compound which is formed is called an ionic compound. Ex.: NaCl , MgCl2, Al2O3 To write the formula of an ionic compound we use the criss-cross method (we down cross multiply the charges without the sign, only the numbers of the charges) Remark: if the charges are the same then they cancel each other in the formula so there will be one atom of the metal and one atom of the non-metal in the compound. Exercise: Write the formula of the compound which is formed between the following elements, and name each compound. a) Rb and S: b) Ca and Se: c) Al and Br: d) Na and N: - Draw a Bohr diagram to show the transfer of electrons (loss / gain) in an ionic compound. Example: Na2O (sodium oxide) Remark: The ionic bond is also described as an electrostatic force of attraction between a positive ion and a negative ion (eg: Na+ Cl- ). 2. Covalent bond: a bond between a non-metal and another non-metal in which there is a sharing of electrons between the non-metallic atoms. The compound that is formed is called a covalent or molecular compound. Molecule: 2 or more atoms (non-metallic) bonded together; the atoms can be of the same element such as O2 or of different elements such as HCl, CH4, H2O,….. We show the sharing of electrons between non-metallic atoms by using the Lewis diagram. In addition we can make intersecting circles for the atoms to show the sharing. Reminder: Lewis diagram of an atom shows only the valence electrons of that atom. Most of the atoms follow the octet rule (there are very few exceptions), that is each atom will have eight electrons in the valence shell (same as noble gases) except hydrogen will have 2 electrons after sharing (same as helium). Remark: 2 electrons that are not bonded to any other atom is called a lone pair (non-bonding pair) of electrons. Exercise: Draw lewis diagrams to show the sharing of electrons in each of the following compounds: 1. NF3 2. CH4 3. CO2 4. CCl4 5. CH2O Remark:In drawing Lewis structure, we show the bonds between the atoms and we also show all lone pairs (if present) on any atom. - Naming molecular compounds: 1: mono 2: di 3: tri 4: tetra 5: penta 6: hexa 7: hepta 8: octa 9: nona 10:deca Example: PCl5 : phosphorus pentachloride Remark: If the first element contains only one atom we don’t write mono before it; If the second element contains only one atom we have to write mono before it. Ex.: NO : nitrogen monoxide CO: carbon monoxide Exercise: Fill in the table below Name Chemical Formula diphosphorus pentoxide SO3 CO Aluminum sulfide Al2S3 SF6 Calcium oxide Lithium nitride Li3N Remark: If the compound contains a transition metal, then we have to mention the type of charge of the transition metal by inserting a roman numeral in brackets (I, II, III, IV ….) after the symbol of the transition metal. Example: Name the following compounds: - FeCl2 : Iron (II) chloride - Cu(NO3)2 : Copper (II) nitrate Remark: There are few transition metals that have only one type of charge such as zinc, nickel, and silver; in this case no roman numeral is required. Zinc : Zn+2 Silver: Ag+ Nickel: Ni+2 - ZnSO4 : zinc sulfate - AgNO3 : silver nitrate - CuSO4 : copper (II) sulfate - Co(NO3)3 : cobalt (III) nitrate Exercise: Write the formula of the following compounds. Calcium phosphate: Iron(III) hydroxide: Sodium hydroxide: Manganese(II) hydroxide: Barium sulfate: Zinc carbonate: Ammonium nitrate: Remark: We must enclose the polyatomic ion in brackets if the number after it is more than 1. Note: If the polyatomic ion that ends with the prefix –ate decreases by one oxygen atom then the prefix changes to -ite. If the prefix ending with – ite decreases by one oxygen atom then we precede the prefix by hypo, whereas if the prefix ending with – ate increases by one oxygen atom then we precede the prefix by per. Example: ClO3- is called chlorate; if we reduce one oxygen atom then the ion becomes ClO2- and is called chlorite, however if we increase by one oxygen atom then the ion becomes ClO4- and is called perchlorate; and if the chlorite is reduced by one oxygen atom then the ion becomes ClO- and is called hypochlorite. Exercise: Name the following compounds: K2SO3 : NaNO2 : Mg(ClO4)2 : LiBrO2 : - Comparison Table between ionic and covalent (molecular) compounds: property Ionic Compounds Covalent Compounds State (at room temperature) solids Solids, liquids or gases Melting point and boiling point Very high Usually low Involvement of electrons Loss and gain (transfer) of electrons Sharing of electrons Electric conductivity When dissolved in water (in solution) , electric conductivity is high

QC Lab - Experiment 2: Preparation and Standardization of 1N Sodium Hydroxide Solution

Experiment 2 - Introduction; Order of Reaction + Reaction of Sodium thiosulfate and Hydrochloric acid

Maintaining sodium ion gradient by the loop of Henle

NMT 215 Lecture 5 & 6 (sodium pertech and skeletal imaging)

sodium imbalance

Sodium & Potassium

Sodium Potassium Pump

Lab 3: Renal Physiology, Water and Sodium Balance

sodium hydroxide solution tests (testing for metal ions)

Sodium, Chloride, and Dehydrated States