1 acids and bases
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This document defines acids and bases, describing their properties and common examples. Acids produce hydrogen ions in water and taste sour, while bases produce hydroxide ions and feel slippery. Examples of strong acids include hydrochloric, sulfuric, and nitric acids, while examples of weak acids are acetic and carbonic acid. Strong bases like ammonia fully dissociate in water, whereas sodium hydroxide is an example of a weak base.
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Acids and bases ppt notes
The document discusses acids and bases, including their properties, examples of common acids and bases, and how strong vs. weak acids and bases are classified. Acids are sour, turn litmus red, and contain hydrogen ions. Bases are slippery, turn litmus blue, and contain hydroxide ions. Strong acids and bases have more hydrogen or hydroxide ions respectively and can be caustic.
Acid & bases
This document discusses acids, bases, indicators, and neutralization. It defines acids as substances with a pH below 7 that have a sour taste. It lists the three common acids used in labs as hydrochloric acid, sulfuric acid, and nitric acid. Alkalis are defined as sodium hydroxide, potassium hydroxide, and ammonia. Indicators change color depending on the type of solution, and there are universal indicators and lime indicators. Neutralization occurs when an acid and base cancel each other out through a reaction.
Class 7 chapter 5 Acids ,bases and Salts ppt 2
The document discusses neutralization reactions and their importance in daily life. It defines neutralization as the reaction between an acid and base to form a salt and water. An example reaction of hydrochloric acid and sodium hydroxide forming sodium chloride and water is provided. Neutralization reactions are important in relieving indigestion through antacids and reducing the itch of ant stings. Neutralization of acidic soil or factory waste is also discussed to prevent environmental damage.
Acids, bases, & salts
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7, forming H+ ions in solution, and neutralizing bases. Common acids include hydrochloric, sulfuric, nitric, acetic, carbonic, and phosphoric acids. Bases are defined as having a pH greater than 7, feeling slippery, and dissolving fats and oils. Common bases include sodium hydroxide, magnesium hydroxide, aluminum hydroxide, and ammonium hydroxide. Salts are formed from the reaction of acids and bases and are composed of the negative ion of an acid and positive ion of a base. A neutralization reaction produces a salt and water when an acid re
Acids, bases and salts
This document discusses acids, bases, indicators, and salts. It provides information on their properties, examples, uses, and how they are classified. Acids have a sour taste, react with metals and carbonates to produce gases, and turn litmus paper red. Bases have a bitter taste, feel slippery, and turn litmus paper blue. Common indicators, their color changes, and uses are described. Salts are the products of acid-base reactions and have properties like solubility and being hygroscopic.
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An acid is defined as a substance that yields hydrogen ions in water, while a base yields hydroxide ions. The Arrhenius theory defines acids and bases in terms of their dissociation in water, but it is limited to aqueous solutions and does not account for bases like ammonia without hydroxide groups. Lewis expanded the definitions to include any species that can accept or donate electron pairs. Acids and bases can be strong or weak depending on how fully they dissociate in water, yielding more or fewer hydrogen or hydroxide ions. A salt is formed when an acid is neutralized by a base through ionic bonding, and salts exist as neutral or acidic/basic depending on remaining hydrogen or hydroxide
Acid base notes
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Strong acids and bases completely ionize, while weak ones only partially ionize. Neutral substances have equal concentrations of hydrogen and hydroxide ions. When acids and bases are mixed, they neutralize to form salts and water through balanced chemical reactions. pH indicators can be used to determine if a solution is acidic, basic, or neutral.
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Acids and bases ppt notes
The document discusses acids and bases, including their properties, examples of common acids and bases, and how strong vs. weak acids and bases are classified. Acids are sour, turn litmus red, and contain hydrogen ions. Bases are slippery, turn litmus blue, and contain hydroxide ions. Strong acids and bases have more hydrogen or hydroxide ions respectively and can be caustic.
Acid & bases
This document discusses acids, bases, indicators, and neutralization. It defines acids as substances with a pH below 7 that have a sour taste. It lists the three common acids used in labs as hydrochloric acid, sulfuric acid, and nitric acid. Alkalis are defined as sodium hydroxide, potassium hydroxide, and ammonia. Indicators change color depending on the type of solution, and there are universal indicators and lime indicators. Neutralization occurs when an acid and base cancel each other out through a reaction.
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This document discusses acids, bases, indicators, and salts. It provides information on their properties, examples, uses, and how they are classified. Acids have a sour taste, react with metals and carbonates to produce gases, and turn litmus paper red. Bases have a bitter taste, feel slippery, and turn litmus paper blue. Common indicators, their color changes, and uses are described. Salts are the products of acid-base reactions and have properties like solubility and being hygroscopic.
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An acid is defined as a substance that yields hydrogen ions in water, while a base yields hydroxide ions. The Arrhenius theory defines acids and bases in terms of their dissociation in water, but it is limited to aqueous solutions and does not account for bases like ammonia without hydroxide groups. Lewis expanded the definitions to include any species that can accept or donate electron pairs. Acids and bases can be strong or weak depending on how fully they dissociate in water, yielding more or fewer hydrogen or hydroxide ions. A salt is formed when an acid is neutralized by a base through ionic bonding, and salts exist as neutral or acidic/basic depending on remaining hydrogen or hydroxide
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This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Strong acids and bases completely ionize, while weak ones only partially ionize. Neutral substances have equal concentrations of hydrogen and hydroxide ions. When acids and bases are mixed, they neutralize to form salts and water through balanced chemical reactions. pH indicators can be used to determine if a solution is acidic, basic, or neutral.
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Acids, bases, & salts
Acids have a pH below 7 and donate hydrogen ions in solution. They react with bases and metals. Common acids include hydrochloric acid and citric acid. Bases have a pH above 7 and accept hydrogen ions, feeling slippery. Common bases are sodium hydroxide and ammonia. When an acid and base react, they form a salt and water. Salts are neutral and composed of the ions of the original acid and base. The digestive system uses acids and bases to break down foods, with acid in the stomach and bases in the intestines.
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The document defines acids as substances that dissociate in water to produce hydrogen ions, and describes some of their key properties, such as sour taste and turning litmus red. It also discusses important acids like hydrochloric acid and sulfuric acid, and their common uses. Similarly, bases are defined as substances that dissociate to produce hydroxide ions in water. Important bases and their uses are also outlined, along with definitions and examples of salts.
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This document defines acids, bases, and salts. It states that acids are sour, turn litmus red, and release H+ ions, while bases are bitter, soapy, turn litmus blue and release OH- ions. Salts are formed through neutralization reactions between acids and bases. It provides examples of common acids, bases, and salts. It also discusses acid-base indicators and their color changes. The document further details chemical properties of acids and bases, the pH scale, and provides additional information on salt.
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This document defines acids and alkalis and provides their key properties. It states that acids produce hydrogen ions when dissolved in water and lists common acids like hydrochloric acid. It also notes that acids have a sour taste, turn litmus red, and have a pH below 7. Alkalis are defined as metal oxides or hydroxides soluble in water, with examples given. Alkalis are described as having a bitter taste, turning litmus blue, and having a pH above 7. The document outlines how both acids and alkalis react with other substances.
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Acids produce hydrogen ions in water and have sour tastes, while bases produce hydroxide ions in water and have bitter tastes. Common acids include citric acid and hydrochloric acid, while common bases include sodium hydroxide and ammonia. Strong acids and bases fully dissociate in water, while weak acids and bases only partially dissociate. The pH scale measures how acidic or basic a solution is. Neutralization is the reaction between an acid and base that produces water and a salt. Indicators change color to determine if a solution is acidic or basic.
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This document provides an introduction to acids, bases and salts. It discusses key concepts including:
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2) When acids and bases are mixed, a neutralization reaction occurs producing water and a salt.
3) Arrhenius defined acids as substances that release H+ ions in water and bases as those that release OH- ions. Bronsted-Lowry expanded this to include acids as proton donors and bases as proton acceptors.
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vinaykumarmaurya2005@gmail.com
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It is helpful for class 7 students . I hope you will like this . Thank you and do not forget to watch my other uploads.
Presentation1
This document defines acids and alkalis and provides their key properties. It states that acids produce hydrogen ions when dissolved in water and lists common acids like hydrochloric acid. It also notes that acids have a sour taste, turn litmus red, and have a pH below 7. Alkalis are defined as metal oxides or hydroxides soluble in water, with examples given. Alkalis are described as having a bitter taste, turning litmus blue, and having a pH above 7. The document outlines how both acids and alkalis react with other substances.
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This document discusses indicators, acids, bases, and the reactions between them. It provides examples of natural and synthetic acid-base indicators and how they change color with pH. Acids are defined as sour substances that turn litmus red and donate hydrogen ions in water, while bases are defined as bitter substances that turn litmus blue and accept hydrogen ions in water. Common strong acids and bases are listed. The document also summarizes several acid-base reactions including neutralization and reactions with metals, carbonates, and oxides. It discusses the pH scale and importance of pH in everyday life. In the end, it briefly discusses the preparation and uses of several common salts.
Chemicals from salts
Sodium chloride, or common salt, is an important raw material used to make many chemicals. When electricity is passed through a solution of salt water, it decomposes to form sodium hydroxide and chlorine in a process called the chlor-alkali process. Chlorine is used to make bleaching powder and sodium hydroxide is used to make baking soda. Baking soda, also known as sodium bicarbonate, is used to make baking powder and as an antacid. Washing soda, or sodium carbonate, can also be derived from salt and is used in glass, soap, and paper industries.
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Acids produce hydrogen ions in water and have sour tastes, while bases produce hydroxide ions in water and have bitter tastes. Common acids include citric acid and hydrochloric acid, while common bases include sodium hydroxide and ammonia. Strong acids and bases fully dissociate in water, while weak acids and bases only partially dissociate. The pH scale measures how acidic or basic a solution is. Neutralization is the reaction between an acid and base that produces water and a salt. Indicators change color to determine if a solution is acidic or basic.
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This document provides an introduction to acids, bases and salts. It discusses key concepts including:
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3) Arrhenius defined acids as substances that release H+ ions in water and bases as those that release OH- ions. Bronsted-Lowry expanded this to include acids as proton donors and bases as proton acceptors.
4) The pH scale is used to measure acidity/basicity, with acids having a pH <7 and bases
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This document discusses acids, bases and salts. It defines acids as substances that produce hydrogen ions in water, and classifies them as strong or weak based on how completely they ionize. Bases are defined as substances that produce hydroxide ions in water. Salts are formed when hydrogen ions in an acid are replaced by metal ions. The document also describes the reactions of acids with metals and carbonates, as well as the neutralization reaction between acids and bases to form water and a salt.
Hydrogen Bonding Powerpoint
1. Hydrogen bonding occurs when a hydrogen atom bonded to an electronegative atom like nitrogen, oxygen or fluorine interacts with another electronegative atom via electrostatic attraction between the hydrogen and the lone pair of electrons.
2. This leads to higher boiling points and enthalpies of vaporization for compounds that can form multiple hydrogen bonds like water. It also allows for the formation of structures like DNA base pairs and protein secondary structures.
3. Hydrogen bonding plays important roles in determining physical properties of compounds and enabling key biological molecules like DNA and proteins to form their functional three-dimensional structures.
Intermolecular forces
The document discusses different types of intermolecular forces including London dispersion forces, dipole-dipole forces, dipole-induced dipole forces, ion-dipole interactions, and hydrogen bonding. It provides examples of how these forces influence the properties of substances such as their melting and boiling points. Hydrogen bonding specifically is described as being an important intermolecular force that influences the properties of water, alcohols, and other polar molecules.
Acids and Bases
An acid is a substance that produces hydrogen ions in water and has a pH less than 7. Strong acids, like hydrochloric acid, are completely ionized in water, while weak acids like acetic acid only partially ionize. Acids react with metals to produce salts and hydrogen gas, with carbonates to produce salts, water and carbon dioxide gas, and with bases to produce salts and water. They have sour tastes and are corrosive.
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Similar to 1 acids and bases
Acids and bases
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Acids have a sour taste, turn litmus red, and react with metals and carbonates. Bases have a bitter taste, turn litmus blue, and react with acids to form salts and water. The document also discusses pH scale, uses of acids and bases, and how to classify different types of oxides such as acidic, basic, amphoteric, and neutral oxides based on their chemical properties.
Acids and bases ppt notes
The document discusses acids and bases, including their properties, examples of common acids and bases, and how strong vs. weak acids and bases are classified. Acids are sour, turn litmus red, and contain hydrogen ions. Bases are slippery, turn litmus blue, and contain hydroxide ions. Strong acids and bases have more hydrogen or hydroxide ions respectively and can be caustic.
Acids, bases, & salts
This document discusses acids, bases, and salts. It defines acids as having a pH less than 7 and forming H+ ions in solution, and bases as having a pH greater than 7 and forming OH- ions in solution. Acids are classified as weak or strong depending on how completely they ionize in water. Common acids include hydrochloric acid, sulfuric acid, and acetic acid. Bases are also classified as weak or strong. Common bases include sodium hydroxide, magnesium hydroxide, and ammonium hydroxide. A salt is formed when an acid and base react, consisting of the negative ion from the acid and positive ion from the base.
Lecture 19.1a- Acid/Base Properties
Acids taste sour and change the color of indicators. They produce hydrogen ions (H+) in water and can be strong or weak electrolytes. Bases taste bitter, feel slippery, and change indicator colors by producing hydroxide ions (OH-) in water. They can also be strong or weak electrolytes. According to the Arrhenius definition, acids dissociate to produce H+ ions and bases dissociate to produce OH- ions in water. When acids and bases are mixed, they neutralize through a reaction that produces water and an aqueous salt.
Acids And Alkali
This document discusses acids and alkalis. It defines acids as substances that produce hydrogen ions in water, and provides examples like hydrochloric acid. Acids have properties like a sour taste, turning litmus red, and reacting with metals and carbonates. Alkalis are defined as metal oxides or hydroxides soluble in water, with examples like sodium hydroxide. Alkalis have properties like a bitter taste, turning litmus blue, and reacting with acids. The document also describes how acids and alkalis neutralize each other to form salts and water.
NA_Lesson_01_Acids_and_Bases.pptx
This document provides information about acids and bases. It defines acids as substances that produce hydrogen ions in water, forming hydronium ions. It also defines bases as substances that produce hydroxide ions in water. The document lists some common acids and bases, and describes how they ionize or dissociate in water to produce ions. It notes characteristics of acids such as being corrosive and causing sour tastes, and characteristics of bases such as feeling slippery and tasting bitter.
Acids, bases, & salts
This document discusses acids, bases, and salts. It defines acids as compounds that produce hydrogen ions (H+) in water, have a pH below 7, and react with metals. Bases are defined as compounds that produce hydroxide ions (OH-) in water and have a pH above 7. Salts are neutral compounds formed by the reaction of acids and bases. Common acids and bases are listed, along with their uses. The pH scale and indicators are also explained.
Acids
Acids have several key properties: they taste sour, conduct electricity as electrolytes, and change the color of indicators like bromthymol blue from blue to yellow. When acids dissolve in water, they ionize by donating a hydrogen ion (H+), forming hydronium ions (H3O+) which allows them to conduct electricity. Common strong acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3) which fully ionize. Weaker acids like carbonic acid (H2CO3), boric acid (H3BO3), acetic acid (HC2H3O2), and citric acid (H3C6
Acid,base,and salt
This document discusses acids, bases, and salts. It defines acids as substances that release hydrogen ions in water and bases as substances that produce hydroxide ions in water. It explains that acids and bases neutralize through a reaction that produces a salt and water. Salts are usually solid crystals formed through neutralization reactions between acids and bases or other reactions like those between acid/base oxides or metals and acids. Common examples of acids, bases, and their properties are provided.
Acids and bases
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water and bases as substances that react with acids to form salts and water. It describes the chemical properties of acids and bases, including their tastes, pH levels, and ability to conduct electricity. Common acids like sulfuric acid and bases like sodium hydroxide are discussed along with their uses. The roles of water in producing hydrogen and hydroxide ions are explained. The pH scale is introduced as a measure of acidity and alkalinity. Strong and weak acids and bases are differentiated based on their ionization in water.
Acids and bases
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water and bases as substances that react with acids to form salts and water. It describes the chemical properties of acids and bases, including their tastes, pH levels, and ability to conduct electricity. Common acids like sulfuric acid and bases like sodium hydroxide are discussed along with their uses. The roles of water in producing hydrogen and hydroxide ions are explained. The pH scale is introduced as a measure of acidity and alkalinity. Strong and weak acids and bases are differentiated based on their ionization in water.
Acids and bases
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water and bases as substances that react with acids to form salts and water. It describes the chemical properties of acids and bases, including their tastes, pH levels, and ability to conduct electricity. Common acids like sulfuric acid and bases like sodium hydroxide are discussed along with their uses. The roles of water in producing hydrogen and hydroxide ions are explained. The pH scale is introduced as a measure of acidity and alkalinity. Strong and weak acids and bases are differentiated based on their ionization in water.
Acids and bases
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water and bases as substances that react with acids to form salts and water. It describes the chemical properties of acids and bases, including their tastes, pH levels, and ability to conduct electricity. Common acids like sulfuric acid and bases like sodium hydroxide are discussed along with their uses. The roles of water in producing hydrogen and hydroxide ions are explained. The pH scale is introduced as a measure of acidity and alkalinity. Strong and weak acids and bases are distinguished by their level of ionization in water.
ACIDS AND BASES
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water and bases as substances that react with acids to form salts and water. It describes the chemical properties of acids and bases, including their tastes, pH levels, and reactions. Common acids like sulfuric acid and carbonic acid and bases like sodium hydroxide and magnesium hydroxide are discussed along with their uses. The key roles of water in producing hydrogen and hydroxide ions are explained. The pH scale is introduced as a measure of acidity and alkalinity. Strong and weak acids and bases are differentiated based on their ionization in water.
AcidsBases.ppt
This document discusses acids and bases. It defines acids as hydrogen ion donors that have a pH lower than 7 and taste sour. Bases are defined as hydrogen ion acceptors that have a pH greater than 7 and taste bitter. It explains that strong acids and bases fully dissociate in solutions, while weak acids and bases only partially dissociate. Properties and reactions of acids and bases are provided such as their effects on indicators, reactions with metals and carbonates, and how acids neutralize bases through formation of water.
Intro acids and bases
This document defines acids and bases and their key characteristics. Acids release H+ ions in water and have sour tastes, while bases release OH- ions in water and feel slippery. Strong acids and bases fully dissociate in water, while weak ones only partially dissociate. Common strong acids include sulfuric acid and hydrochloric acid. When acids and bases react, they undergo a neutralization reaction where water and a salt are formed. Indicators are used to test whether a solution is acidic or basic. The pH scale measures the concentration of H+ ions, with lower pH indicating more H+ ions and higher pH less H+ ions.
Introacidsandbases 130416101155-phpapp02
This document defines acids and bases and their key characteristics. Acids release H+ ions in water and have sour tastes, react with metals, and contain hydrogen. Strong acids completely dissociate into H+ ions while weak acids only partially dissociate. Common strong acids include sulfuric acid and hydrochloric acid. Bases release OH- ions in water and usually taste bitter and feel slippery. Strong bases contain hydroxide ions and are also corrosive. When acids and bases react through neutralization, they form water and a salt like NaCl. The pH scale measures the concentration of H+ ions in a solution, with lower pH indicating more H+ ions.
GJ Acids Base X.pptx
Acids derive their name and sour taste from the Latin word "acidus" meaning sour. They contain acid compounds that donate hydrogen ions (H+) in water, causing a sour taste. Common acid-base indicators like litmus, turmeric, and red cabbage change color depending on whether a solution is acidic or basic. Acids react with metals and bases to produce salt and water in a neutralization reaction. The strength of acids and bases is measured on the pH scale, with values below 7 indicating acids and above 7 indicating bases.
Class-10-Chapter-01-Science-Chemistry-Acid bases and salts.ppsx
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Acids and bases
This document discusses acids and bases. It defines acids as substances that produce H+ ions in water and have a pH less than 7. Acids have properties such as turning litmus red and reacting with metals. Bases are defined as substances that produce OH- ions in water and have a pH greater than 7. They have properties such as turning litmus blue and reacting with acids to form salt and water. Strong acids and bases are fully dissociated in water while weak acids and bases are only partially dissociated. The document also discusses Bronsted-Lowry and Lewis acid-base theories.
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Class-10-Chapter-01-Science-Chemistry-Acid bases and salts.ppsx
Class-10-Chapter-01-Science-Chemistry-Acid bases and salts.ppsx
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This document provides a diagram labeling various anatomical features of an animal's internal organs and systems, including the location of the vomerine teeth, gullet, internal nares, glottis, maxillary teeth, vocal sacs, eye sockets, tympanic membrane, nictitating membrane, external naris, liver, fat bodies, small intestine, heart, gall bladder, lungs, kidneys, spleen, cloaca, mesentery, stomach, testis, urinary bladder, ovaries, oviduct, and their relative positions.
Chpt.3.1
1) Arthropods undergo either complete or incomplete metamorphosis. Complete metamorphosis involves four stages: egg, larva, pupa, and adult. Incomplete metamorphosis involves hatching from eggs as nymphs and molting into winged adults after several molts.
2) Animals exhibit one of three types of symmetry: asymmetry, radial symmetry, or bilateral symmetry. Radial and bilateral symmetry involve dividing the animal into mirror halves, while asymmetry does not.
3) Succession describes the process of ecological community change over time. There are two types: primary succession colonizes new bare rock and soilless sites, while secondary succession occurs on existing soil after a disturbance like
Chpt.2.3
This document summarizes the cycling of important materials like water, carbon, nitrogen, and phosphorus through ecosystems. It explains that while energy is lost at each trophic level, the sun replenishes it, and matter is recycled as nutrients move through organisms. The atoms that make up living things today have been on Earth since life began. It then provides more detailed explanations of the water, carbon, nitrogen, and phosphorus cycles.
Chpt.2.2
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Chpt.2.1
Ecology is the scientific study of the interactions between organisms and their environments. It reveals the interrelationships between living (biotic) and nonliving (abiotic) parts of the world. Key concepts in ecology include the biosphere, biotic factors, abiotic factors, levels of organization (organism, population, community, ecosystem, biome, biosphere), habitats, niches, and symbiosis (commensalism, mutualism, parasitism). Ecology combines information from various sciences to understand these relationships.
Chpt. 17.3- Domains and Kingdoms
The document discusses different systems for classifying life into kingdoms and domains. It describes the three domain system of Bacteria, Archaea and Eukarya. It also outlines the six kingdom system of Bacteria, Archaea, Protista, Plantae, Fungi and Animalia. Finally, it mentions the traditional five kingdom system of Monera, Protista, Plantae, Fungi and Animalia. It provides details about the defining characteristics of each domain and kingdom.
Chpt. 17.2 Modern Classification
Cladograms are branching diagrams that represent the proposed evolutionary history of a species or group, with closer branches indicating that organisms have more traits in common. They are a modern method of classification that shows evolutionary relationships rather than just taxonomic rankings.
Chpt. 17.1-History of Classification
Aristotle first classified organisms as either animals or plants, with plants grouped by size and animals by whether they had blood. Linnaeus broadened Aristotle's system and created the first formal taxonomy, grouping organisms into a binominal nomenclature with a genus and species name. The taxonomic categories from most specific to broad are species, genus, family, order, class, phylum, kingdom, and domain.
Chpt.15.2-Evidence of Change
There are several ways that scientists provide evidence of evolution, including comparative anatomy, comparative embryology, and fossils. Comparative anatomy looks at homologous and analogous structures between species, while comparative embryology examines similarities in development. Fossils provide direct evidence of extinct species and how they changed over time. Scientists use both relative dating of fossils layers and radioactive dating to determine the age of fossils and track changes in species. Adaptations like camouflage and mimicry help organisms survive and reproduce more successfully.
Chpt. 15.1
Charles Darwin developed the theory of evolution by natural selection based on his observations as a naturalist aboard the HMS Beagle in the 1830s. While visiting the Galapagos Islands, Darwin noticed that related but distinct animal species inhabited different islands. He later concluded that populations on the mainland evolved over generations as they adapted to their local environments, with better adapted traits being passed down. Darwin's theory proposed that natural selection drives evolution, as organisms better suited to their environment will survive and reproduce, passing on their favorable traits.
Chapter 11.3 notes
A karyotype is a micrograph that arranges homologous chromosome pairs in decreasing size order. It is used to study chromosomes stained during cell metaphase. Nondisjunction is a cell division error where sister chromatids do not separate properly, which can cause conditions like Down syndrome.
Chpt. 11.2 complex inheritance leftovers
Sickle-cell anemia is an autosomal recessive trait common in those with African and Mediterranean ancestry. It causes abnormally shaped red blood cells, impaired blood flow, tissue damage, and health issues. Sex is determined by the 23rd pair of chromosomes - females have XX and males have XY. The X chromosome carries many genes needed for development in both sexes. To compensate for having two X chromosomes, females inactivate one randomly. Sex-linked traits are on the X chromosome and are always expressed if recessive in females. Muscular dystrophy is an X-linked recessive disease. Polygenic traits like skin and eye color are influenced by two or more genes and result in a range of intermediate phenotypes.
Chapter 11.1 notes
This document summarizes several human genetic disorders including their inheritance patterns, symptoms, prevalence, and treatment options. Huntington's disease is an autosomal dominant neurological disorder with onset between 30-50 years of age that is always fatal. Cystic fibrosis is the most common lethal genetic disorder among white Americans, affecting the lungs and digestive system due to thick mucus production, with current treatments improving life expectancy. Tay-Sachs disease causes neurological deterioration and death by age 5 due to fatty acid accumulation in the brain.
Incomplete codominance multiple_alleles
The document discusses different patterns of inheritance beyond simple dominance:
1) Incomplete dominance, where the heterozygous phenotype is intermediate between the homozygous phenotypes. Examples include snapdragons and carnations.
2) Codominance, where both alleles are expressed in the heterozygote rather than blending. Examples include checkered chickens, roan horses, and variegated clover.
3) Multiple alleles, where more than two alleles control a trait. Examples include human blood types and coat colors in rabbits.
10.2 mendelian genetics
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Chapter 12.4 gene regulation & mutation
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Chapter 12.3 dna,rna and protein
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Chapter 12.2 dna replication
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