Types of energy notes
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This document contains information about a roller coaster problem and energy transfers in various systems. It begins by stating that the weight (Wt) of the roller coaster is 50N. It then lists 7 problems about finding different forms of energy (potential, kinetic, mechanical) at various points (A, B, C) in the roller coaster's path. The document also discusses energy transfers that occur in systems like light bulbs, the human body during digestion, and hairdryers. It defines and provides examples of different forms of energy, such as mechanical, electrical, nuclear, chemical, sound, light, and thermal energy.
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Energy types notes 2010
Here are the answers to your thermal energy questions:
- Thermal energy is kinetic energy, as it is the energy of particles moving.
- If you touch something with faster moving particles than your skin, it would feel hot to the touch. Heat would flow from the object into your skin.
- If an object has more thermal energy than its surroundings, heat will flow from the object into the cooler surroundings until both reach thermal equilibrium (the same temperature). The object will cool down as it transfers heat.
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The document discusses Sommerfeld's free electron model of metallic conduction. It explains that in this model, each free electron inside a metal experiences both an attractive electrostatic force from the positive ions and a repulsive force from other electrons. The model also assumes the positive ion lattice produces a uniform attractive potential field for electrons. The potential field must be periodic to match the crystal structure of the solid metal. The model provides explanations for electrical conductivity, heat capacity, and thermal conductivity of metals but fails to account for differences between conductor and insulator behaviors.
ELECTRONEGATIVITY
Pauling was the first to propose a scale of electronegativity in 1932 based on the difference in the measured energy of an AB bond and the expected energy of a purely covalent AB bond. Mulliken suggested an approach to electronegativity in 1934 based on ionization enthalpy and electron affinity, defining electronegativity as the arithmetic mean of ionization energy and electron affinity. Electronegativity is influenced by factors such as charge on the atom, hybridization state, ionization energy, electron affinity, and effective nuclear charge. It is used to determine bond polarity, percent ionic character, and enthalpy of formation.
Bohr's model
1) Bohr's atomic model successfully explained the hydrogen spectrum by postulating that electrons revolve in definite orbits called energy levels without radiating energy.
2) The radius, energy, and frequency of radiation emitted by electrons in different orbits were derived based on Bohr's model.
3) Bohr's model showed that electrons can jump between discrete energy levels, emitting or absorbing photons of specific frequencies corresponding to the energy differences between levels.
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Energy types notes 2010
Here are the answers to your thermal energy questions:
- Thermal energy is kinetic energy, as it is the energy of particles moving.
- If you touch something with faster moving particles than your skin, it would feel hot to the touch. Heat would flow from the object into your skin.
- If an object has more thermal energy than its surroundings, heat will flow from the object into the cooler surroundings until both reach thermal equilibrium (the same temperature). The object will cool down as it transfers heat.
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The document discusses Sommerfeld's free electron model of metallic conduction. It explains that in this model, each free electron inside a metal experiences both an attractive electrostatic force from the positive ions and a repulsive force from other electrons. The model also assumes the positive ion lattice produces a uniform attractive potential field for electrons. The potential field must be periodic to match the crystal structure of the solid metal. The model provides explanations for electrical conductivity, heat capacity, and thermal conductivity of metals but fails to account for differences between conductor and insulator behaviors.
ELECTRONEGATIVITY
Pauling was the first to propose a scale of electronegativity in 1932 based on the difference in the measured energy of an AB bond and the expected energy of a purely covalent AB bond. Mulliken suggested an approach to electronegativity in 1934 based on ionization enthalpy and electron affinity, defining electronegativity as the arithmetic mean of ionization energy and electron affinity. Electronegativity is influenced by factors such as charge on the atom, hybridization state, ionization energy, electron affinity, and effective nuclear charge. It is used to determine bond polarity, percent ionic character, and enthalpy of formation.
Bohr's model
1) Bohr's atomic model successfully explained the hydrogen spectrum by postulating that electrons revolve in definite orbits called energy levels without radiating energy.
2) The radius, energy, and frequency of radiation emitted by electrons in different orbits were derived based on Bohr's model.
3) Bohr's model showed that electrons can jump between discrete energy levels, emitting or absorbing photons of specific frequencies corresponding to the energy differences between levels.
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Atomic nucleus and radioactivity
Radiation is emitted from radioactive materials as a result of their capacity for radioactivity. There are three main types of radiation: alpha particles, which have a large mass and short range; beta particles, which are electrons; and gamma rays, which are high-energy electromagnetic radiation that travels at the speed of light. Radioactive atoms become unstable due to an excess of energy or mass in their nucleus, which can be caused by changes in the number, arrangement, or energy of nucleons. Unstable atoms seek stability through radioactive decay and emission of radiation until the nuclear forces are balanced.
Ionization potential and electron affinity
1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
Nuclear Structure
In 1909, Rutherford performed the Gold Foil Experiment and suggested the following characteristics of the atom:
It consists of a small core, or nucleus, that contains most of the mass of the atom
This nucleus is made up of particles called protons, which have a positive charge
The protons are surrounded by negatively charged electrons, but most of the atom is actually empty space.
In 1913, Bohor proposed the Atomic Model, which suggests that electrons travel around the nucleus of an atom in orbits or definite paths.
Atom consists of a tiny nucleus.
Each orbit has fixed energy that is quantatized.
The energy is emitted or absorb only when an electron jumps from one orbit to another.
Electron can revolve in orbits of fixed angular momentum mvr.
Liquid Drop Model
The nuclei of all elements are considered to be behave like a liquid drop of incompressible liquid of very high density.
In an equilibrium state the nuclei of atoms remain spherically symmetric under the action of strong attractive nuclear forces just like the drop of a liquid which is spherical due to surface tension.
The density of a nucleus is independent of its
size just like the density of liquid which is also
independent of its size.
The protons and neutrons of the nucleus move about
within a spherical enclosure called the nuclear
potential barrier just like the movement of the
molecules of a liquid within a spherical drop of liquid.
. The binding energy per nucleon of a nucleus is constant
Binding Energy
The binding energy, BE, of a nucleus is a measure of the strong force and represents the energy required to separate the nucleus into its constituents protons and neutrons;
Greater the binding energy, the more stable the nucleus.
Volume
The volume of the nucleus is directly proportional to the total number of nucleons present in it.
Density
The density of the nucleus is nearly constant.
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Video link:
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4.3 Notes
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Electron affinity
Electron affinity is the energy released when an electron is added to an isolated gaseous atom. Electron affinity increases with increasing atomic number and decreasing size, as effective nuclear charge increases. Electron affinity decreases with increasing size and number of electron shells, as effective nuclear charge decreases. Electron affinity also increases with greater effective nuclear charge and decreases with greater screening effects and stability of half or completely filled orbitals.
Elementary particles
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Basic Atomic structure
1. Atoms are the basic building blocks of matter and consist of a small, dense nucleus surrounded by electrons.
2. Rutherford's gold foil experiment in 1911 showed that the atom has a small, dense nucleus containing positively charged protons and uncharged neutrons.
3. Niels Bohr proposed his model of the atom in 1913 in which electrons orbit the nucleus in fixed shells at specific energy levels, explaining atomic spectra.
The Nuclear Atom
1. Atoms consist of a dense central nucleus orbited by much smaller electrons.
2. Geiger and Marsden's alpha particle scattering experiments showed that positive charge in atoms is concentrated in a small central nucleus, rather than spread uniformly.
3. Isotopes of an element have the same number of protons but different numbers of neutrons.
Bohr model and electron configuration
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- The quantum mechanical treatment of the H2+ molecular ion involves solving the Schrodinger equation as a three-body problem involving the two nuclei and one electron.
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Fundamental particles of an atom.
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(2) Energy quantization described by Planck's equation.
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Energy types
Here are the steps to solve the roller coaster energy problems:
1. PE at point A = mgh = (20 kg)(10 m/s^2)(250 m) = 50,000 J
2. KE at point A = 0 J (velocity is 0 m/s at the top)
3. ME at point A = PE + KE = 50,000 J + 0 J = 50,000 J
4. KE at point B = 1/2mv^2 = 1/2(20 kg)(200 m/s)^2 = 40,000 J
5. ME at point C = ME is conserved. ME at point A was 50,000 J.
6. PE at
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1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
Nuclear Structure
In 1909, Rutherford performed the Gold Foil Experiment and suggested the following characteristics of the atom:
It consists of a small core, or nucleus, that contains most of the mass of the atom
This nucleus is made up of particles called protons, which have a positive charge
The protons are surrounded by negatively charged electrons, but most of the atom is actually empty space.
In 1913, Bohor proposed the Atomic Model, which suggests that electrons travel around the nucleus of an atom in orbits or definite paths.
Atom consists of a tiny nucleus.
Each orbit has fixed energy that is quantatized.
The energy is emitted or absorb only when an electron jumps from one orbit to another.
Electron can revolve in orbits of fixed angular momentum mvr.
Liquid Drop Model
The nuclei of all elements are considered to be behave like a liquid drop of incompressible liquid of very high density.
In an equilibrium state the nuclei of atoms remain spherically symmetric under the action of strong attractive nuclear forces just like the drop of a liquid which is spherical due to surface tension.
The density of a nucleus is independent of its
size just like the density of liquid which is also
independent of its size.
The protons and neutrons of the nucleus move about
within a spherical enclosure called the nuclear
potential barrier just like the movement of the
molecules of a liquid within a spherical drop of liquid.
. The binding energy per nucleon of a nucleus is constant
Binding Energy
The binding energy, BE, of a nucleus is a measure of the strong force and represents the energy required to separate the nucleus into its constituents protons and neutrons;
Greater the binding energy, the more stable the nucleus.
Volume
The volume of the nucleus is directly proportional to the total number of nucleons present in it.
Density
The density of the nucleus is nearly constant.
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This document contains 15 important theory questions about Rutherford's alpha particle scattering experiment, Rutherford's model of the atom, its limitations, Bohr's model of the hydrogen atom, Bohr's postulates, expressions for the stationary and kinetic energy levels of an electron in the hydrogen atom, the energy level diagram for hydrogen showing different emission series, and definitions of terms like Rydberg constant, excitation potential, and ionization potential. The questions are related to key experiments and models in the development of atomic structure and spectra.
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Video link:
https://youtu.be/C-xhuw9ZN6U
4.3 Notes
Bohr's model of the atom proposed that electrons orbit the nucleus in fixed orbits and absorb or emit discrete amounts of energy when changing orbits. Later evidence showed electrons exist as a probabilistic electron cloud rather than fixed orbits. Atomic orbitals represent regions where electrons are most likely found and electrons occupy orbitals according to their electron configuration, which arranges them in the lowest energy state.
Periodic trends detailed edit
Periodic Trends
This document discusses several periodic trends including ionization energy, electronegativity, atomic radius, and ionic radius. It notes that ionization energy generally decreases down a group and increases left to right in a period as the nuclear charge increases. Electronegativity also typically increases left to right and decreases down a group. Atomic radius decreases left to right in a period as the nuclear charge increases but increases down a group as the principal energy level increases. Ionic radius trends are similar, with positive ion size decreasing left to right and both positive and negative ion size increasing down a group.
Electron affinity
Electron affinity is the energy released when an electron is added to an isolated gaseous atom. Electron affinity increases with increasing atomic number and decreasing size, as effective nuclear charge increases. Electron affinity decreases with increasing size and number of electron shells, as effective nuclear charge decreases. Electron affinity also increases with greater effective nuclear charge and decreases with greater screening effects and stability of half or completely filled orbitals.
Elementary particles
This document provides an overview of elementary particles, including their classification and properties. It discusses baryons such as protons and neutrons, as well as leptons like electrons and photons. Mesons like pions and kaons are also introduced. The document explains that all particles have corresponding antiparticles and explores conservation laws like parity, charge conjugation, and CPT symmetry. Overall, the document serves as a high-level introduction to the fundamental constituents of matter.
Basic Atomic structure
1. Atoms are the basic building blocks of matter and consist of a small, dense nucleus surrounded by electrons.
2. Rutherford's gold foil experiment in 1911 showed that the atom has a small, dense nucleus containing positively charged protons and uncharged neutrons.
3. Niels Bohr proposed his model of the atom in 1913 in which electrons orbit the nucleus in fixed shells at specific energy levels, explaining atomic spectra.
The Nuclear Atom
1. Atoms consist of a dense central nucleus orbited by much smaller electrons.
2. Geiger and Marsden's alpha particle scattering experiments showed that positive charge in atoms is concentrated in a small central nucleus, rather than spread uniformly.
3. Isotopes of an element have the same number of protons but different numbers of neutrons.
Bohr model and electron configuration
Bohr's model proposed that electrons orbit the nucleus in fixed, quantized energy levels. Later models, like the quantum mechanical model, provided a more accurate description of electron behavior. Electrons fill atomic orbitals according to specific rules, building up the electron configuration of elements in a predictable order based on energy levels. Exceptions occur when half or completely filled orbitals result in a lower energy configuration. Practice filling electron configurations to understand these patterns.
Class15 diatomic molecules - 11th march 2022
- Molecules form when atoms bond together through attractive forces between oppositely charged ions or through quantum mechanical effects in the case of two similar atoms bonding.
- The quantum mechanical treatment of the H2+ molecular ion involves solving the Schrodinger equation as a three-body problem involving the two nuclei and one electron.
- Approximations can be made by treating the nuclei as fixed at some internuclear distance and solving the equation for the electron motion. This yields energy levels that depend on the internuclear separation.
Fundamental particles of an atom.
By 1932, only electrons, protons, and photons were known elementary particles. The discovery of the neutron by Chadwick in 1932 raised the number to four. Later discoveries found that atoms are made of protons, neutrons, and electrons, and that protons and neutrons consist of even smaller particles called quarks. A variety of other elementary particles like pions, muons, and neutrinos were also discovered. Experiments using particle accelerators helped reveal the subatomic structure of matter and uncovered many new fundamental particles and forces.
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The document summarizes key topics in the chapter on nuclear physics, including:
1) The structure and properties of the nucleus, including its composition of protons and neutrons.
2) The discovery of the neutron by James Chadwick in 1932, which helped explain nuclear structure.
3) The strong and weak nuclear forces that bind nucleons together in the nucleus.
Bohar atomic model
This document discusses the structure of atoms based on experimental evidence. It describes experiments scattering charged particles and emitting/absorbing radiation that provided information about atomic structure. This evidence was used to develop atomic models, though models are simplifications and may not explain all properties. Atoms are very small, stable due to balanced internal forces, and electrically neutral even though they contain electrons.
Periodic property ppt
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This document discusses the key principles of quantum physics including:
(1) The wave-particle duality of microparticles like electrons described by de Broglie's equation.
(2) Energy quantization described by Planck's equation.
(3) Heisenberg's uncertainty principle.
It describes how Schrodinger's equation is used to model the wave-like behavior of electrons in solids. The energy and behavior of electrons is quantized based on solutions to Schrodinger's equation under different boundary conditions, such as electrons confined in a potential well or interacting with a potential barrier. Quantum theory was needed to fully explain properties of electrons in solids and failures of classical free electron theory
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Here are the steps to solve the roller coaster energy problems:
1. PE at point A = mgh = (20 kg)(10 m/s^2)(250 m) = 50,000 J
2. KE at point A = 0 J (velocity is 0 m/s at the top)
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3) When sufficient energy is given to an electron, it can be removed from its orbit or energy level. Removing an electron upsets the atom's balance and results in ionization, which plays a role in
Energy
The document discusses different forms of energy including mechanical, heat, chemical, electromagnetic, and nuclear energy. It explains kinetic energy as the energy of motion and potential energy as stored energy. Examples are given of energy conversions between different forms, such as chemical energy being converted to heat and mechanical energy in car engines. The law of conservation of energy is introduced, which states that energy cannot be created or destroyed, only changed from one form to another.
Basics of energy conversion and solar cell working
A change from one form of energy to another is called energy conversion.
Most forms of energy can be converted into any other form
Matter and antimatter
The document discusses fundamental particles and forces. It explains that every particle has an antiparticle with opposite charge that acts as a mirror image. The four fundamental forces - gravitational, electromagnetic, weak nuclear, and strong nuclear forces - are carried by exchange particles that produce attractive or repulsive forces over different ranges. The strong nuclear force mediated by gluons has the shortest range but is the strongest force binding quarks and nucleons together in the nucleus.
23 p.10.1 forms of energy ppt (1) (1)
There are six basic forms of energy: mechanical, electrical, heat, light, sound, and chemical energy. Mechanical energy includes potential energy, which is stored energy due to an object's position, and kinetic energy, which is energy of motion. Potential energy can be gravitational or elastic. Electrical energy comes from the movement of charged particles and can be transformed into other forms of energy. Heat energy is how hot or cold an object is and is transferred between objects. Light and sound energies are forms of wave energy that travel away from their sources. Chemical energy is stored energy due to molecular arrangements.
Forms of energy
Energy exists in various forms including heat, light, sound, electrical, chemical, nuclear, and mechanical. These forms of energy can be transformed from one to another, though transformations come with losses. Heat is the most easily lost form of energy and the form most easily transformed from and to other forms. Chemical energy is stored in chemical compounds and released through chemical reactions, powering living things and being harnessed from fuels. Nuclear energy is stored in atomic nuclei and can be released through fission or fusion to generate electricity. Mechanical energy exists as kinetic or potential energy and comes from natural sources like wind and water. Energy transformations power modern technologies and daily activities but always follow the law of conservation of energy.
Unit 2: Matter and energy
The document discusses energy and its various forms. It defines energy as the capacity to do work or produce heat. Energy cannot be created or destroyed, only transformed from one form to another. There are various types of material systems depending on how energy and matter can be exchanged. Energy exists in many forms including mechanical, thermal, chemical, electrical, electromagnetic, nuclear, and internal. Energy can be transferred or converted between these different forms.
EF
Work is done when a force causes an object to move in the direction of the force. There are different forms of energy including kinetic energy from motion, potential energy from stored or elevated positions, and chemical and nuclear energy from atomic structures. Power is defined as the rate at which work is done or energy is converted over time. The document provides definitions and formulas for calculating work, energy, power, and other energy fundamentals.
Energy and work
it is a 9 and 10 th presentation its good for people and i can wet you will get a1 if you download from here.
ENERGY-TRANSFORAMATION by jaspher-3.pptx
This document describes an elementary classroom lesson on energy transformation. It includes the content standards which are that students demonstrate understanding of how energy is transformed. The performance standards are that students appreciate the transformation of energy. Examples are given of how sound, heat, light and electricity can be transformed. Activities are described where students explore energy transformations involving a clock, electric fan, jogging, and a flashlight to demonstrate chemical to light energy transformation. Students are asked to identify energy transformations and explain why energy needs to be transformed to usable forms.
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Measurement 2011
Make any changes or
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improve it.
2. Share your graphic organizer
with a partner and have them
provide feedback. Make any
final changes based on the
feedback.
Heat notes abbreviated
Fossil fuels are nonrenewable sources of energy that were formed from the remains of ancient plants and animals. They get their energy from the sun, which was originally stored by organisms that lived millions of years ago. Common examples of fossil fuels include coal, oil, and natural gas. This document also discusses temperature, thermal energy, and different temperature scales including Fahrenheit, Celsius, and Kelvin, noting that Kelvin scale defines absolute zero as the lowest possible temperature.
What is energy2010
1. Energy is the ability to do work or cause change. Work is done when a force causes an object to move, and is measured in Joules.
2. Kinetic energy depends on an object's mass and speed, and is calculated as KE=1/2mv^2. Potential energy depends on an object's mass and height, and is calculated as PE=mgh.
3. Mechanical energy is the total of an object's kinetic and potential energies, or ME=KE+PE. As an object moves, its kinetic energy increases as its potential energy decreases, keeping the total mechanical energy constant.
Intro to Energy
The document discusses energy and how it was used in the past compared to today. It prompts the reader to list what they know about energy and what they want to learn. It then asks the reader to define energy and provide 10 everyday ways they use energy. The document discusses how ancestors lived without modern conveniences like light bulbs, cars, and air conditioners. It prompts the reader to think about whether ancestors required energy in their daily activities. The reader is then asked to read a story about life 100 years ago and discuss differences in energy usage between the past and present. Finally, the document prompts the reader to draw an illustration showing the relationship between energy and work and explain their drawing.
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Mammals, birds, reptiles, amphibians, and fish are the five classes of vertebrates. Mammals are warm-blooded and nurse their young, while birds are also warm-blooded but lay eggs. Reptiles, amphibians, and fish are cold-blooded and many reproduce by laying eggs, though some amphibians hatch as larvae.
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Frogs are amphibians that undergo metamorphosis from tadpole to adult. They have bilateral symmetry with internal organs and systems that allow for movement on land or water. A frog's form and functions, such as its ability to leap and catch insects, are well-suited to its environment and lifestyle.
Mammals notes
Birds and reptiles can be compared and contrasted using a Venn diagram. Some key differences are that birds are endothermic and have feathers for insulation, while reptiles are ectothermic and have scales. Both lay eggs but birds care for their young after hatching while most reptiles do not provide parental care.
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Birds have adaptations for flight including feathers and hollow, lightweight bones. They lay amniotic eggs and maintain a high body temperature through endothermy, panting to cool off and eating frequently. Birds also have a four-chambered heart and double-looped circulatory system.
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This document discusses the characteristics and adaptations of reptiles. It notes that reptiles and amphibians both share characteristics with chordates. Reptiles have developed adaptations to live on land such as dry scales, thick skin, and amniotic eggs to prevent water loss. Their circulatory system includes a three-chambered heart and double-looped circulatory system. Reptiles are ectothermic and must rely on external heat sources to regulate their body temperature.
Reptile and bird notes
Fish and amphibians share characteristics with all chordates, such as having a notochord and dorsal nerve cord. Reptiles evolved adaptations like scales, thick skin, and amniotic eggs to prevent water loss and live on land. Reptiles have three-chambered hearts and double-looped circulatory systems, and are ectothermic, maintaining their body temperature through their surroundings. Birds further adapted for land with feathers for flight, thin hollow bones, and the ability to regulate their own high body temperatures through panting and a high metabolism.
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This document contains a series of slides from a frog dissection guide. It lists and numbers various external and internal structures of frogs such as the mouth parts, internal organs, and reproductive systems of male and female frogs. The slides provide labels for anatomical structures like the ventricle, auricle, liver, gallbladder, intestines, kidneys, testes, ovaries and more.
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Frog dissection is a common biology lab activity where students examine the internal anatomy of frogs. The purpose is for students to learn frog anatomy through direct observation of organs like the heart, lungs, stomach and intestines. This document likely contains diagrams and pictures to help guide students through the dissection process and identify internal structures.
Amphibians notes
Amphibians are vertebrates that breathe through lungs and thin, moist skin. They have a three-chambered heart and double-loop circulatory system that is more efficient than the single-loop system of fish. Amphibians go through a metamorphosis where tadpoles with tails and gills transform into adults without tails that use lungs to breathe on land. There are three main groups of amphibians: frogs and toads, salamanders, and caecilians.
Fish notes
1. Vertebrates share four key characteristics: a notochord, hollow nerve cord, pharyngeal gill pouches, and a tail.
2. Fish are the largest and simplest group of vertebrates. They are ectothermic, have fins and scales, and a lateral line.
3. Fish have a closed circulatory system with two heart chambers that pumps blood to the gills and body for gas exchange.
Crayfish conclusion
Crayfish are advanced arthropods that belong to the phylum Arthropoda. They have a segmented body adapted for movement, digestion, and survival. Their form fits their function, with organs and symmetry suited to their lifestyle in waterways.
Crayfish dissection diagrams
This document contains diagrams and descriptions of the external and internal anatomy of a crayfish. It identifies and describes key external structures like the cephalothorax, abdomen, appendages, eyes and sensory organs. Internally, it outlines the location of organs like the heart, hepatopancreas gland, stomach and nerve cord. Descriptions are provided of both male and female reproductive structures and swimming appendages.
Arthropoda & echinodermata notes
Arthropods are the most successful group of animals on Earth, making up over 75% of all animal life. They have a segmented body, jointed appendages, a hard exoskeleton that many molt to shed and grow, and undergo complete metamorphosis from egg to adult. Arthropods have bilateral symmetry, organs and systems, eat a wide variety of foods, and reproduce sexually. They are found globally in nearly all environments.
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The document provides information about mollusks and annelids. It notes that mollusks are one of the most diverse animal groups, have a radula and live in various habitats. Their body plans include bivalves, gastropods and cephalopods. Annelids are segmented worms that fertilize soil, have a closed circulatory system and brain, and move by creeping along using muscles.
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Flatworms and cnidarians share some basic characteristics like having simple tissue organization but differ in key aspects like flatworms having bilateral symmetry and a digestive system while cnidarians do not. Some flatworms like tapeworms are parasitic and can infect humans, causing illnesses if meat or water is ingested that contains the parasite larvae. Roundworms also infect many humans and include parasites like hookworms that burrow into the skin and travel to the bloodstream, feeding on blood.
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Types of energy notes
- 1. Wt=50N 1. What is the KE at point A? Why? 2. What is the PE at point A? 3. What is the ME at point A? 4. What is the height at point B? 5. What is the height at point C?
- 2. 1. What is heat? 2. How does thermal energy play a role in the Law of Conservation of Energy?
- 3. Roller Coaster Energy Problems HT=250 m WT=200N HT=20 m WT=200N M=20kg V=200m/s 1. Find the PE at point A. 2. Find the KE at point A. Answer the 3. Find the ME at point A. problems on 4. Find the KE at point B. the left on your sheet under the 5. What is the ME at point C? roller coaster 6. Find the PE at point C. picture. 7. Find the KE at point C.
- 4. 1. Describe the energy transfers that occur in a light bulb. 2. Describe the energy transfers that occur when the body is powered by food.
- 5. 1. Describe the energy transfers in a hairdryer. 2. What is the difference between renewable and nonrenewable energy resources?
- 6. Forms Explanation Example Total energy of Mechanical motion and position Total kinetic energy Thermal of particles Energy stored in Chemical rearranging atoms
- 7. Energy of moving Electrical electrons Energy of vibrating Sound particles Vibrations of electrically Light charged particles Energy in the nucleus of Nuclear an atom
- 8. 1. Mechanical Energy total energy of motion and position ME=KE + PE
- 9. 2. Electrical Energy the energy of moving electrons Like charges repel and + + Opposite charges attract + -
- 10. The Power of Electricity ๏ Can be turned into other kinds of energy ๏ Can do work ๏ Hairdryer converts electric to thermal ๏ Alarm clock converts electric to sound and light
- 11. 3. Nuclear Energy the energy of the nucleus of an atom ๏ Fission ๏ Fusion
- 12. The Sun ๏Giant nuclear fusion reactor ๏Ultimate source of energy for our planet
- 13. 4. Chemical Energy the energy of rearranging atoms ๏ Is photosynthesis endothermic or exothermic? ๏ Is respiration endothermic or exothermic?
- 14. 5. Sound Energy the energy of vibrating particles -caused by vibrations & carried through a substance.
- 15. 6. Light Energy the vibrations of electrically charged particles Called PHOTONS ๏
- 16. The EM Spectrum ๏ Visible light is one portion of the Electromagnetic Spectrum. ๏ All of these waves are energy- filled waves. ๏ Insects, like bees, see shorter wavelengths than humans. What type of EM waves do they see? WATCH IT! - prism
- 17. Possibilities of Light Light rays move away from their source in straight lines. When they hit something, they are either Absorbed Reflected Refracted (stopped) (bounced off) (bent) WATCH IT! - Mirror
- 18. Sound & Light: Alike, but Different Sound Light *vibration *does NOT *needs a medium need a medium *longitudinal *transverse
- 19. 7. Thermal Energy the total kinetic energy of the particles ๏ more thermal energy = faster moving particles ๏ less thermal energy = slower moving particles
- 20. Thermal Energy vs. Heat Heat is the transfer of energy between objects that are at different temperatures.
- 21. Three Kinds of Heat Conduction Convection Radiation (touch) (current) (rays) Hot Cold Common