Unit 4 2014 ppt sound
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This document discusses the basics of sound waves. It explains that sound waves are caused by vibrations, requiring a medium like air, liquid or solid to transfer energy. It describes how compression and rarefaction of molecules transfers sound waves. Frequency determines pitch, with higher frequencies being higher pitched. Amplitude determines loudness, with greater amplitude being louder. Graphs can show the displacement over time of sound waves to represent characteristics like frequency and amplitude. The speed of sound depends on the medium and temperature.
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Here are the key steps:
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Approaching:
fo = 1000(1 + v/343)
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1.3 velocity
1) Acceleration is a measure of how quickly velocity changes. It can represent a change in speed, direction, or both.
2) The slope of a velocity-time graph represents acceleration. The area under the graph represents displacement.
3) For objects experiencing uniform acceleration, displacement can be calculated using: s = ut + (1/2)at^2
1.2 displacement and position vs time graphs
1) Displacement is defined as the straight line path between an object's initial and final positions, representing the change in position. It is not necessarily the same as the total distance travelled.
2) Victor's displacement is calculated as his final position (2km North of Starbucks) minus his initial position (3km South of Starbucks), equaling 5km North.
3) A position-time graph shows an object's position over time. The slope of the line between any two points represents the average velocity during that time interval.
1.1 vectors
1) Vectors are quantities that have both magnitude and direction, unlike scalars which only have magnitude. Common vector quantities include force, velocity, and displacement.
2) Vectors can be described by their magnitude, direction, and reference frame. Direction is measured in degrees from the x-axis.
3) Vector operations like addition, subtraction, multiplication and division can be performed graphically or using components and trigonometry. Parallel vectors can be added/subtracted algebraically but others require using components.
4) To add vectors using components, each vector is broken into x and y components using trigonometry. The x and y components can then be added separately and combined to find the overall resultant vector.
2016 topic 5.2 hess's law
1. Hess's law states that the overall enthalpy change of a chemical process is independent of the path taken.
2. The document uses the reaction of sodium hydroxide and hydrochloric acid to illustrate Hess's law. It shows that the enthalpy change of the direct reaction is equal to the sum of the enthalpy changes for the stepwise reactions.
3. Representing the reactions on an enthalpy level diagram and enthalpy cycle confirms that Hess's law applies, with the enthalpy change for the overall reaction being the sum of the enthalpy changes for the individual steps.
2016 topic 5.1 measuring energy changes
This document provides an overview of exothermic and endothermic reactions, calorimetry, and how to calculate enthalpy changes. The key points are:
- Exothermic reactions release heat while endothermic reactions absorb heat.
- Enthalpy change (ΔH) is the quantity of heat released or absorbed during a chemical reaction.
- Calorimetry experiments allow calculation of ΔH by measuring the temperature change of a reaction mixture.
- Sample problems demonstrate how to use calorimetry data like mass changes and temperature differences to calculate the enthalpy change for a reaction.
2016 topic 4.5 bonding - metallic
Metallic bonding involves a lattice of positive metal ions surrounded by delocalized electrons that form a negative "electron cloud". This electron cloud binds the positively charged ions together and is responsible for metals' properties. Metals exhibit high electrical conductivity because the mobile electron cloud allows electrons to move freely throughout the structure. The strength of metallic bonding depends on electron density and ionic radius - greater electron density and smaller ionic radius lead to stronger bonding and higher melting points. Alloys are mixtures of metals designed to enhance properties like strength, corrosion resistance, magnetism, and ductility.
2016 topic 4.2 bonding - covalent
This document provides an overview of ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged ion and another atom gains those electrons to become a negatively charged ion. For example, in sodium chloride, sodium atoms lose electrons to form Na+ ions and chloride atoms gain electrons to form Cl- ions. The oppositely charged ions are then held together by electrostatic forces in a repeating crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity in solid form but do conduct when molten or dissolved in water as the ions become mobile.
Unit 4 2014 ppt wave characteristics
The document summarizes key concepts about waves, including:
1) Waves can be classified as mechanical or electromagnetic depending on whether they require a medium to travel. Mechanical waves include sound and water waves while electromagnetic waves include radio and light waves.
2) Waves can be transverse, with oscillations perpendicular to the direction of travel, or longitudinal, with oscillations parallel to the direction of travel.
3) Key wave properties include frequency, wavelength, period, amplitude, and speed. The speed of a wave depends on properties of the medium and can be calculated from the wavelength and period.
2016 topic 01 part 1
This document discusses quantitative chemistry concepts including the mole, Avogadro's constant, molar mass, and using moles to calculate the number of particles and mass of substances. Some key points covered are:
- A mole is a unit used to count fundamental particles and represents 6.02x1023 particles.
- The mole allows converting between large numbers of particles and more manageable units like grams.
- Molar mass relates the mass of a sample of a substance to the number of moles it contains.
- Problems use molar mass to calculate moles, particles, or mass given any two of those quantities.
Chemistry 1 - Atomic Structure
- Atoms consist of a nucleus containing protons and neutrons surrounded by electrons in orbitals.
- The atomic number is the number of protons, which identifies the element. The mass number is the total number of protons and neutrons.
- Isotopes are atoms of the same element with different numbers of neutrons. The relative atomic mass takes into account the natural abundance of isotopes.
2016 Topic 2: Electron Configuration
This document discusses electron configuration and how it is described using quantum numbers. It explains the main concepts like energy shells (n), subshells (s, p, d, f), orbitals and how electrons fill these according to the Aufbau principle and Hund's rule. Examples are provided to show the electron configurations of elements like hydrogen, helium, lithium and how the configurations change as the atomic number increases. Practice problems are included at the end to determine configurations of additional elements.
2016 Topic 2: Atomic Structure
This document discusses atomic structure and properties. It begins by reviewing the basic atomic model including protons, neutrons, and electrons. It then discusses atomic number, mass number, isotopes, ions, and electron configuration. The document also covers average atomic mass and mass spectrometry. It concludes by discussing the Bohr model of the atom and how this helped explain emission spectra of elements. In summary, the key topics covered are the fundamental particles of atoms, atomic notation, isotopes, ions, electron configuration, and early atomic structure models.
2016 topic 0 - oxidation and reduction (INTRODUCTION)
The document discusses oxidation and reduction reactions. It defines oxidation as the loss of electrons or an increase in oxidation state, and reduction as the gain of electrons or a decrease in oxidation state. Redox reactions involve both oxidation and reduction occurring simultaneously. Oxidation states can be used to identify what is oxidized and reduced in a reaction. The document provides examples of calculating oxidation states in various compounds and ions using rules like the sum of oxidation states equaling the overall charge.
2016 topic 0 - elements & periodic table
- An element is a substance composed of a single type of atom that cannot be broken down further. A compound is a substance made of two or more elements chemically bonded together.
- Elements can exist as individual atoms, molecules of two bonded atoms, or giant molecular or network structures made of many bonded atoms like metals. Elements are categorized as metals, nonmetals, or metalloids based on their physical and chemical properties.
Introduction to elements & periodic table
- An element is a substance composed of a single type of atom that cannot be broken down further. A compound is a substance made of two or more elements chemically bonded together.
- Elements can exist as individual atoms, molecules of two bonded atoms, or giant molecular or network structures made of many bonded atoms like metals. Elements are categorized as metals, nonmetals, or metalloids based on their physical and chemical properties.
Topic 20 6 stereoisomers
This document provides an overview of organic chemistry topics related to stereoisomers, including:
1) It defines structural isomers and stereoisomers as different types of isomers, and provides examples to illustrate each type.
2) It discusses the importance of stereochemistry in fields like biochemistry, medicine, and studying reaction mechanisms.
3) It explains key concepts around chiral centers, configurations, enantiomers, and how these relate to a molecule's ability to rotate plane-polarized light and be optically active.
Topic 20 4 condensation reactions
This document discusses organic chemistry topics including condensation reactions which combine two smaller molecules to form one larger molecule with the elimination of a small molecule like water. It provides examples of esterification reactions forming esters and amide formation, as well as condensation polymerization reactions that form polymers from monomers with functional groups undergoing condensation. Specific examples discussed include the formation of terylene, nylon 6,6, and polypeptides from amino acid monomers.
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Unit 4 2014 ppt sound
- 1. Sound Physics Power Points Physics I Mr. Young www.pedagogics.ca
- 2. Basic facts about sound waves: Sound waves are caused by vibrations. The source of all sound waves is a vibrating object. For example: a speaker cone, a guitar string, a drum skin, an air column in a trumpet. Sound waves are longitudinal. Sound waves are mechanical waves. They require a medium to transfer energy. Sound can travel through solids, liquids and gases.
- 3. Sound waves are caused by vibrations When a tuning fork is struck, the tines vibrate back and forth. Each vibration compresses the surrounding air molecules together (high pressure). Air is elastic. As the compression expands, adjacent molecules are compressed. In this way sound waves travel through the medium. rarefaction l compression Sound waves are longitudinal Molecules vibrate parallel to energy transfer.
- 4. Sound waves are mechanical waves
- 5. Sound waves are mechanical waves Sound relies on the vibration of particles to transfer the energy of the sound wave. If there are no particles, there is no sound! Bell in Jar Demo - Video
- 6. Frequency of Sound Waves The frequency of a sound wave is described as the pitch of a sound. The higher the frequency of the vibrating source, the higher the pitch. Humans can hear sounds in the range of 20 Hz to 20 kHz. Dogs and other animals can perceive higher frequencies (why you can’t hear a dog whistle.
- 7. Amplitude of Sound Waves The amplitude of a sound wave is perceived as the loudness of a sound. The greater the amplitude of the vibrating source, the more energy the sound wave has and your hear a louder noise. Loudness is measured in decibels (dB). It is a logarithmic scale. 10 times more energy gives a +10 dB increase in loudness.
- 8. Graphical Representations of Sound Waves A microphone can be used with a data logger to create a graphical representation of a sound wave. A displacement-time graph for a sound wave shows the frequency and amplitude of vibration of the wave. Time is measured on the x-axis and the y-axis is representative of displacement.
- 9. Graphical Representations of Sound Waves Example 1 – Showing high pitch (frequency) http://onlinetonegenerator.com/
- 10. Graphical Representations of Sound Waves Example 2 – Showing low pitch (frequency)
- 11. Graphical Representations of Sound Waves Showing loudness
- 12. Graphical Representations of Sound Waves Musical instruments do not produce pure tones. The wave form is still distinguishable in this recorder sound wave pattern.
- 13. Speed of Sound The speed of sound depends on the medium that it is traveling through. In general: Vsolid > vliquid > vgas Specific properties of the medium will also affect the speed. For example, the speed of sound is slower in cold air than in warm air. Why is this?
- 14. Speed of Sound The speed of sound in still air can be determined by the following equation: v = 331 + 0.6T m/s Where T is the temperature in Celsius. When we discuss speed in Mach numbers (example Mach 1.4) we are referring to how fast one is traveling relative to the speed of sound. Mach 1.4 is slower on a cold day than on a warm one.