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1. In life's hierarchy of organization, new properties emerge at each level as atoms are organized into molecules, organelles, cells, tissues, organs, systems, organisms, populations, communities, ecosystems, and the biosphere.
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This document provides a tutorial on writing cover letters. It discusses defining your personal brand, the purpose of cover letters, and key elements to include such as an opening paragraph, skills matching using the STARL method, and a closing statement. Formatting tips are also covered, such as including your name, the hiring manager's name if known, the company address, a reference line, and signatures. The tutorial emphasizes showing passion for the role and company through research and linking your experiences to the job requirements. Students are assigned to draft two cover letters for peer review.
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1. In life's hierarchy of organization, new properties emerge at each level as atoms are organized into molecules, organelles, cells, tissues, organs, systems, organisms, populations, communities, ecosystems, and the biosphere.
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This document discusses chemical equilibrium, including:
- The concept of equilibrium and how it applies to both physical and chemical processes.
- How to write expressions for the equilibrium constant (K) and what K represents in terms of reactant and product concentrations/pressures.
- Factors that can influence chemical equilibrium according to Le Chatelier's principle, including changes in concentration, pressure/volume, temperature, and adding a catalyst.
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This document discusses key concepts in chemical bonding including Lewis dot structures, ionic and covalent bonds, electronegativity, writing Lewis structures, formal charge, resonance structures, and exceptions to the octet rule. It provides Lewis dot symbols for common elements, defines ionic and covalent bonds, discusses how to write Lewis structures through a step-by-step process, and explains concepts like formal charge, resonance, and species that violate the octet rule. Tables and diagrams are included to further illustrate these important bonding concepts.
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1. N has an unpaired electron in its 2p orbital, so it is paramagnetic.
2. Mg, Na, and N all have their electrons paired, so they are diamagnetic.
3. Mn2+ has the electron configuration [Ar] 3d5, so it has 5 unpaired electrons.
4. Mn has the electron configuration [Ar] 3d5 4s2, so it has 3 unpaired electrons.
5. Fe2+ has the electron configuration [Ar] 3d6, so it has 4 unpaired electrons.
6. Fe3+ has the electron configuration [Ar] 3d5, so it has 5 unpaired electrons.
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This document summarizes key concepts relating to gases, including:
- The gas laws of Boyle, Charles, Avogadro, and combined gas law and how they relate pressure, volume, temperature, and moles of gas
- The ideal gas equation and how it incorporates these variables
- Standard temperature and pressure conditions for reporting gas measurements
- Gas density calculations using molar mass and gas stoichiometry problems
- Dalton's law of partial pressures which states that in a mixture of gases, the total pressure is equal to the sum of the partial pressures of the individual gases.
Chapter 3
Okay, here are the steps:
1) Convert the mass percentages to grams of each element in 100 g of the compound:
K: 24.75% = 24.75 g
Mn: 34.77% = 34.77 g
O: 40.51% = 40.51 g
2) Calculate the moles of each element:
K: 24.75 g / 39.10 g/mol (molar mass of K) = 0.634 mol
Mn: 34.77 g / 54.94 g/mol (molar mass of Mn) = 0.634 mol
O: 40.51 g / 16.00 g/mol (molar mass of O)
Chapter 2
This document provides information about naming ionic and molecular compounds. It discusses atomic number, mass number, and isotopes. It explains that ions are formed when atoms gain or lose electrons to become positively or negatively charged. The document outlines rules for writing chemical formulas, including ionic formulas which involve balancing charges between cations and anions. It also discusses naming conventions for ionic compounds based on metal cations and nonmetal anions. The document concludes by stating that molecular compounds consist of nonmetals and do not involve ion formation.
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The document summarizes key concepts in human reproduction and embryonic development. It describes asexual and sexual reproduction, the anatomy and functions of the male and female reproductive systems, gamete formation through meiosis, the hormonal regulation of the menstrual cycle, fertilization, cleavage and gastrulation in embryonic development.
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Chapter 3 [compatibility mode]
1. Monosaccharides are the simplest carbohydrates and include glucose and fructose. They have carbon skeletons of 3-7 carbons and are the main energy fuels for cellular work.
2. Cells form disaccharides by linking two monosaccharides together via dehydration reactions. Sucrose is an example of a disaccharide formed from glucose and fructose.
3. Polysaccharides are long chains of sugar units and include starch, glycogen, and cellulose. Starch is a glucose polymer stored in plants, while glycogen is a glucose polymer stored in animal cells for energy. Cellulose, composed of glucose, forms plant cell walls.
Chapter 5 the working cells [compatibility mode]
This document summarizes key points about cell membranes and cellular transport from Chapter 5 of a biology textbook. It discusses how membranes are composed of phospholipids and proteins arranged in a fluid mosaic structure. It describes different types of passive transport including diffusion, facilitated diffusion, and osmosis. Active transport requires energy in the form of ATP to move molecules against their concentration gradient. Large molecules are transported across membranes via exocytosis and endocytosis. The chapter emphasizes that ATP acts as the cell's energy currency, powering various types of cellular work through energy coupling reactions.
Chapter 22 gas exchange [compatibility mode]
This document discusses mechanisms of gas exchange in animals. It covers three main points:
1) Breathing involves exchanging carbon dioxide produced by cells for oxygen from the air through three phases: breathing, gas transport in blood, and exchange with tissues.
2) Animals exchange gases across moist surfaces like skin or specialized structures like gills, tracheal systems, or lungs.
3) In humans, air follows a branching path from nose to bronchi and bronchioles to reach alveoli in lungs where gas exchange occurs through diffusion across thin membranes.
Chapter 4
The document discusses concentration of solutions in terms of molarity. It defines molarity as moles of solute per liter of solution. It provides the key formula for calculating molarity given moles of solute and volume of solution. Examples are shown for calculating molarity, moles of solute, and volume of solution given different variables. Dilution of solutions is also discussed, where the number of moles of solute remains constant but volume changes upon addition of solvent.
Chapter 6 cell energy [compatibility mode]
Cellular respiration occurs in three main stages to harvest energy from glucose and produce ATP. Stage 1 is glycolysis in the cytoplasm, which oxidizes glucose to pyruvate and generates 2 ATP and 2 NADH. Stage 2 is the citric acid cycle in the mitochondria, which completes glucose oxidation and generates more NADH and FADH2. Stage 3 is oxidative phosphorylation in the inner mitochondrial membrane, where electrons are transferred through an electron transport chain to generate ATP through chemiosmosis. Fermentation enables some ATP production without oxygen through glycolysis alone.
Chapter 4 cell & tissues (1) [compatibility mode]
This document provides an overview of cell structures and their functions as seen through different types of microscopes. It begins by discussing the early observations of cells and development of cell theory. It then describes the light microscope and electron microscope and how each allows observation of different cell components. The document outlines the structural differences between prokaryotic and eukaryotic cells and describes several organelles found in eukaryotic cells including the nucleus, endoplasmic reticulum, ribosomes, and membranes. It explains how these structures work together and facilitates key cellular processes like manufacturing and transport.
Chapter 7 photosynthesis [compatibility mode]
Photosynthesis uses light energy, carbon dioxide and water to produce oxygen and glucose, which is the main food source for most living things. It occurs in two stages in the chloroplast. The light-dependent reactions use energy from sunlight to convert water to oxygen and produce ATP and NADPH. These products are then used in the light-independent Calvin cycle to reduce carbon dioxide and produce glucose from carbon dioxide absorbed from the atmosphere. Photosynthesis moderates global warming by absorbing carbon dioxide, a greenhouse gas, from the atmosphere.
Chapter 25: Excretion [compatibility mode]
This document summarizes key points from a chapter on thermoregulation and osmoregulation. It discusses how animals regulate their internal temperature and water balance through various physiological adaptations and mechanisms. Specifically, it covers how endothermic and ectothermic animals gain and lose heat, the categories of adaptations that help thermoregulation, and the challenges of osmoregulation for freshwater fish, saltwater fish and terrestrial animals. It also briefly outlines the processes of filtration, reabsorption, secretion and excretion involved in urine production by the kidneys.
Chapter 8: Genetics [compatibility mode]
The document summarizes key concepts from chapters 8 and 9 about cellular reproduction and Mendel's experiments with pea plants. It describes:
1) The two main types of reproduction - asexual, which produces identical offspring, and sexual, which involves inheritance from two parents and produces variations.
2) How prokaryotes reproduce through binary fission, and eukaryotes go through interphase and mitosis/cytokinesis. Meiosis reduces the chromosome number in gametes.
3) Gregor Mendel's experiments in the abbey garden that discovered genes are inherited as discrete factors and laid the foundations for genetics through studying traits in pea plants.
Chapter 21 nutrition and digestion [compatibility mode]
Chapter 21 nutrition and digestion [compatibility mode]kau_deanship of e-learning and distance education
The document summarizes key aspects of nutrition and digestion in animals. It discusses the four main stages of food processing - ingestion, digestion, absorption and elimination. It provides details on the digestive systems of different animal groups and focuses on the human digestive system. The human system consists of the alimentary canal and accessory glands. Food moves through the system via peristalsis and is broken down mechanically and chemically. Nutrients are then absorbed and transported to cells for energy production or storage. A balanced diet provides essential nutrients, fuels the body, and builds molecules.Viewers also liked (13)
Chapter 21 nutrition and digestion [compatibility mode]
Chapter 21 nutrition and digestion [compatibility mode]
More from kau_deanship of e-learning and distance education
Chapters 24,25
The document discusses organic chemistry topics including:
- Classes of organic compounds such as aliphatic hydrocarbons, aromatic hydrocarbons, and functional groups.
- Alkanes have the general formula CnH2n+2 and contain only single bonds. Cycloalkanes contain carbon atoms joined in rings.
- Alkenes contain carbon-carbon double bonds and have the general formula CnH2n. Alkynes contain carbon-carbon triple bonds and have the formula CnH2n-2.
- Aromatic compounds contain benzene rings, and their naming involves indicating substituted groups on the ring.
Chapter 15
This document discusses acids, bases, and pH. It defines acids as substances that produce hydrogen ions in water and bases as substances that produce hydroxide ions. pH is defined as the negative base-10 logarithm of the hydronium ion concentration and is a measure of acidity, with values below 7 indicating acidic solutions and above 7 indicating basic solutions. The autoionization of water is described by the ion product constant Kw, which relates the concentrations of hydronium and hydroxide ions in solution.
Chapter 14
This document discusses chemical equilibrium, including:
- The concept of equilibrium and how it applies to both physical and chemical processes.
- How to write expressions for the equilibrium constant (K) and what K represents in terms of reactant and product concentrations/pressures.
- Factors that can influence chemical equilibrium according to Le Chatelier's principle, including changes in concentration, pressure/volume, temperature, and adding a catalyst.
- Examples of using K expressions to calculate equilibrium concentrations and predict the direction reactions will shift to reestablish equilibrium when conditions change.
Chapter 9
This document discusses key concepts in chemical bonding including Lewis dot structures, ionic and covalent bonds, electronegativity, writing Lewis structures, formal charge, resonance structures, and exceptions to the octet rule. It provides Lewis dot symbols for common elements, defines ionic and covalent bonds, discusses how to write Lewis structures through a step-by-step process, and explains concepts like formal charge, resonance, and species that violate the octet rule. Tables and diagrams are included to further illustrate these important bonding concepts.
Chapter 8
This document discusses periodic trends in atomic and ionic properties, including:
- Atomic and ionic radii decrease across a period as effective nuclear charge increases. Radii increase down a group as principal quantum number increases.
- Ionization energies generally increase across a period as it becomes more difficult to remove electrons. Exceptions include group 2A and 5A having higher energies than 3A and 6A respectively within periods.
- Cations have smaller radii than their parent atoms as electrons are removed. Anions have larger radii as more electrons are gained. Isotectronic ions with more protons have smaller radii.
Chapter 7
1. N has an unpaired electron in its 2p orbital, so it is paramagnetic.
2. Mg, Na, and N all have their electrons paired, so they are diamagnetic.
3. Mn2+ has the electron configuration [Ar] 3d5, so it has 5 unpaired electrons.
4. Mn has the electron configuration [Ar] 3d5 4s2, so it has 3 unpaired electrons.
5. Fe2+ has the electron configuration [Ar] 3d6, so it has 4 unpaired electrons.
6. Fe3+ has the electron configuration [Ar] 3d5, so it has 5 unpaired electrons.
Chapter 5
This document summarizes key concepts relating to gases, including:
- The gas laws of Boyle, Charles, Avogadro, and combined gas law and how they relate pressure, volume, temperature, and moles of gas
- The ideal gas equation and how it incorporates these variables
- Standard temperature and pressure conditions for reporting gas measurements
- Gas density calculations using molar mass and gas stoichiometry problems
- Dalton's law of partial pressures which states that in a mixture of gases, the total pressure is equal to the sum of the partial pressures of the individual gases.
Chapter 3
Okay, here are the steps:
1) Convert the mass percentages to grams of each element in 100 g of the compound:
K: 24.75% = 24.75 g
Mn: 34.77% = 34.77 g
O: 40.51% = 40.51 g
2) Calculate the moles of each element:
K: 24.75 g / 39.10 g/mol (molar mass of K) = 0.634 mol
Mn: 34.77 g / 54.94 g/mol (molar mass of Mn) = 0.634 mol
O: 40.51 g / 16.00 g/mol (molar mass of O)
Chapter 2
This document provides information about naming ionic and molecular compounds. It discusses atomic number, mass number, and isotopes. It explains that ions are formed when atoms gain or lose electrons to become positively or negatively charged. The document outlines rules for writing chemical formulas, including ionic formulas which involve balancing charges between cations and anions. It also discusses naming conventions for ionic compounds based on metal cations and nonmetal anions. The document concludes by stating that molecular compounds consist of nonmetals and do not involve ion formation.
Chapter 1.powerpoint 1
This document discusses measurement units including the SI units, mass and weight, volume, and temperature scales. It provides information on the seven SI basic units, converting between units, derived units, common volume units like liters and milliliters, and temperature scales like Celsius, Kelvin and Fahrenheit. Examples are given for converting between units of length, mass, volume, density and temperature. The goal is for the reader to understand fundamental measurement units and conversions between unit systems.
Chapter 3.powerpoint
This document discusses mass relationships in chemical reactions, including:
1) Atomic mass, molecular mass, molar mass, and formula mass. It defines the mole and Avogadro's number.
2) Chemical equations and how they are used to represent chemical reactions by balancing the atoms on each side.
3) Calculations involving the amounts of reactants and products in chemical reactions, including limiting reagents.
Chapter 2.powerpoint
1) Atoms are made up of protons, neutrons, and electrons. The atomic number is the number of protons, and the mass number is the total number of protons and neutrons. Isotopes are atoms of the same element that differ in their number of neutrons.
2) Molecules are two or more atoms bonded together, while ions are atoms or groups of atoms with a positive or negative charge. Polyatomic ions and molecules contain more than one atom.
3) Chemical formulas indicate the composition of substances. Molecular formulas show exact atom counts, empirical formulas are the simplest whole number ratios, and ionic formulas result in an overall neutral charge. Nomenclature provides systematic names for compounds.
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