Chem change
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This document discusses chemical and physical changes in matter. It defines chemical properties as those that describe a substance's ability to change into a different substance through a chemical reaction. Physical properties can be observed without a chemical change. Chemical changes result in new substances, while physical changes only alter the form or appearance. Evidence of a chemical change includes a change in properties or energy, with energy either absorbed or released. Chemical equations are used to represent chemical reactions and their reactants and products. The mass of reactants and products is conserved in any chemical change.
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The Matterjacobo durango echeverri
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This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.More from MrsKendall (20)
Forces in fluids
Forces in fluidsMrsKendall
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This document discusses various principles related to forces in fluids. It explains that pressure relates to force over an area and is greater the deeper one is in a fluid. Objects will float if their density is less than the fluid and sink if greater. Buoyancy creates an upward force opposing gravity. Archimedes' principle states buoyant force equals weight of displaced fluid. Pascal's principle explains how pressure changes in confined fluids are transmitted equally. Bernoulli's principle describes decreasing pressure as fluid speed increases.Newtons laws
Newtons lawsMrsKendall
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Newton's first law states that an object at rest stays at rest and an object in motion stays in motion with the same speed and in the same direction unless acted upon by an unbalanced force. Newton's second law states that acceleration depends on the net force acting on an object and its mass. Newton's third law states that for every action there is an equal and opposite reaction. Momentum is the product of an object's mass and velocity, and the law of conservation of momentum states that the total momentum of a system remains constant unless an outside force acts on it.Energy
EnergyMrsKendall
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Energy is the ability to do work or cause change. There are two main types of energy: kinetic energy, which is the energy of motion, and potential energy, which is stored energy due to an object's position or shape. The law of conservation of energy states that energy cannot be created or destroyed, but can change forms.Motion etc
Motion etcMrsKendall
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This document defines and explains key concepts related to motion, speed, velocity, and acceleration in physics. It defines motion as the changing distance between objects based on a reference point. Speed is defined as the distance traveled over time, while velocity includes both speed and direction of motion. Acceleration is defined as the rate of change of velocity over time, which can refer to increasing or decreasing speed or changing direction. Examples and calculations are provided for each term.Notes galaxies
Notes galaxiesMrsKendall
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This document discusses different types of galaxies. Galaxies are massive systems of stars, dust and gas held together by gravity, and usually have a central bulge containing a supermassive black hole. The main types are spiral galaxies with arms radiating from a central bulge, barred spiral galaxies with a bar through the center, elliptical galaxies in an elliptical shape, and irregular galaxies with no defined shape. The Milky Way is described as a barred spiral galaxy over 120,000 light years in diameter containing between 100-400 billion stars. It has a massive black hole in the center, around 4 million times the sun's mass. The closest galaxy to the Milky Way is the Andromeda galaxy, around 2.5 million light yearsNotes nebula starlife
Notes nebula starlifeMrsKendall
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The document summarizes the life cycle of stars from their birth in nebulae through their evolution into red giants, white dwarfs, neutron stars, or black holes. It explains that stars produce light through nuclear fusion, where hydrogen fuses into helium. Nebulae are large clouds of dust and gas where stars are born as gravity causes material to collapse and form protostars at the center.Star Classification
Star ClassificationMrsKendall
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Stars are large balls of ionized gas held together by gravity that emit energy through nuclear reactions. They are classified based on size, temperature, and brightness. Size categories include super giants, red giants, main sequence, white dwarfs, and neutron stars. Temperature determines color, from red (coolest) to blue (hottest). Brightness depends on both a star's intrinsic luminosity and its distance from Earth. Spectrographs are used to analyze starlight and determine properties like chemical composition, temperature, and distance.Asteroids, comets, meteors
Asteroids, comets, meteorsMrsKendall
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Asteroids are rocky objects that orbit the sun and are smaller than planets. Comets are made of ice and dust with elongated orbits around the sun, forming tails as they near the sun. Meteors enter Earth's atmosphere as meteorites and appear as "shooting stars", transitioning from meteoroid to meteor to meteorite. While both appear as streaks of light, comets remain stationary while meteors quickly streak across the sky.Keplers laws
Keplers lawsMrsKendall
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Early Greek astronomers believed in a geocentric model of the universe, with Earth at the center. Ptolemy hypothesized that planets moved in circular orbits around Earth. Nicolaus Copernicus later developed a heliocentric model placing the Sun at the center. Johannes Kepler analyzed astronomical data collected by Tycho Brahe, leading Kepler to discover his three laws: 1) planetary orbits are ellipses rather than circles, 2) planets move faster when closer to the Sun and slower when farther, and 3) the squares of planetary orbit periods are proportional to the cubes of their average distances from the Sun.Keplers laws
Keplers lawsMrsKendall
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The document discusses the history of models of the solar system from ancient Greek astronomers to Johannes Kepler. It describes how Greeks originally believed in a geocentric model with the Earth at the center, which was later supported by Ptolemy. Copernicus then developed the heliocentric model of the sun at the center. Galileo's observations of Jupiter's moons and use of the telescope supported this model. Tycho Brahe and Kepler collected extensive observational data, allowing Kepler to develop his three laws: planets orbit in ellipses, their speed changes as they revolve with closer planets moving faster, and their orbital period relates to their average distance from the sun.Notes on our solar system
Notes on our solar systemMrsKendall
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Our solar system contains 1 sun, 8 planets, 5 dwarf planets, and over 170 moons. The planets are divided into two groups - terrestrial planets which are small and rocky, and gas giants which are much larger and composed primarily of hydrogen and helium. Terrestrial planets include Mercury, Venus, Earth, and Mars. Gas giants include Jupiter, Saturn, Uranus, and Neptune. Dwarf planets such as Ceres and Pluto have not cleared their orbital path. Pluto was reclassified as a dwarf planet after astronomers discovered other similar objects in the Kuiper belt.Sun, Earth, Moon System
Sun, Earth, Moon SystemMrsKendall
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This document discusses the relationships between planets, moons, and other celestial bodies. It explains that the Moon orbits the Earth and is considered our natural satellite. A satellite revolves around a planet. Lunar eclipses occur when the Moon passes behind Earth into its shadow, while solar eclipses happen when the Moon passes between Earth and the Sun. The Moon's phases are caused by varying amounts of sunlight reflecting off its surface due to its orbit around Earth. Tides are also influenced by the Moon's gravity, with high and low tides occurring regularly due to the positions of the Moon and Sun relative to Earth.Notes revolution rotation
Notes revolution rotationMrsKendall
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This document provides an overview of key astronomy concepts including:
- The structures of the solar system such as the sun, planets, and moons.
- Key terms like axis of rotation, period of rotation, period of revolution, and ellipses that describe planetary motion.
- Distances in our solar system measured in Astronomical Units and on a galactic scale using light years.
- How the tilt of the Earth on its axis and its revolution around the sun cause the seasons.
- The equinoxes in March and September when day and night are equal length and the solstices in June and December when the sun is farthest from the equator.CHONPS (basic o-chem intro)
CHONPS (basic o-chem intro)MrsKendall
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Carbon plays a central role in living organisms due to its ability to combine with itself and other elements in many ways. Organic compounds contain carbon and were originally thought to only relate to living things, but are now known to exist more broadly. Polymers are long chains of molecules formed when monomers link together repeatedly through chemical bonds, and include both synthetic materials like plastics as well as natural polymers like proteins, DNA, and silk that make up living things.Acids bases
Acids basesMrsKendall
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The document discusses acids, bases and the pH scale. It explains that the pH scale ranges from 0-14 and measures the concentration of hydrogen ions in a solution. Acids have a pH below 7 and contain hydrogen ions, while bases have a pH above 7 and contain hydroxide ions. A pH of 7 is neutral. The document also provides examples of common acids and bases, their properties, and some of their uses.Balancing equations
Balancing equationsMrsKendall
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The document discusses how to balance chemical equations by ensuring the total number of atoms on both sides of the equation are equal. It explains that coefficients are used to represent the number of molecules in a reaction, while subscripts indicate the number of atoms in a molecule. The steps to balance an equation are to: 1) Write the unbalanced equation, 2) Count the atoms on each side, 3) Use coefficients to make the atoms equal on both sides. Examples are provided to demonstrate balancing equations through adjusting coefficients and verifying the balanced atoms.Periodic table
Periodic tableMrsKendall
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The document summarizes the history and organization of the periodic table. It describes how Mendeleev organized the first periodic table based on atomic mass and properties, and how the modern table is organized by atomic number. The periodic table is divided into periods and groups; elements in the same group have similar properties. The document also defines metals, nonmetals, semimetals, and inert gases, and provides examples of their characteristic properties.Metallic bonds
Metallic bondsMrsKendall
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Metallic bonds form when metal atoms come together and their valence electrons move freely around the atomic nuclei, creating a "sea of electrons" that positively charged metal ions are suspended within. This bond structure allows metals to be malleable, ductile, shiny, electrically conductive, and thermally conductive. Alloys are mixtures of metals that are generally stronger than their pure metal components due to metallic bonding between different kinds of metal atoms.Covalent bonds
Covalent bondsMrsKendall
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Covalent bonds form when atoms share electrons to gain a full outer shell. Atoms that form covalent bonds, like hydrogen and oxygen in water, share electrons so that neutral molecules are created. Covalent bonds generally occur between nonmetals and result in molecules with low melting and boiling points that do not conduct electricity well.Ionic bonds
Ionic bondsMrsKendall
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Ionic bonds form between metal and nonmetal atoms when the metals donate electrons to the nonmetals, becoming positively charged cations while the nonmetals accept electrons and become negatively charged anions. The oppositely charged ions are then attracted to each other, bonding ionically. When ionic compounds form, the charges balance out according to the formula. For example, two chloride (Cl-) ions with a charge of -1 each will balance out one magnesium (Mg2+) ion with a charge of +2, written as MgCl2. Ionic compounds form hard, brittle solids with high melting points and conduct electricity when dissolved in water.Chem change
- 1. Chemical Change Observing, Describing, Controlling
- 2. Observing Chemical Change • Matter can be described in two ways: – Chemical properties – Physical properties
- 3. Observing Chemical Change • Chemical Properties: The characteristics of a substance that describes it’s ability to change into a different substance. – EXAMPLE: In our magnesium lab, we lit the magnesium on fire, watched it burn as it reacted with the oxygen in the air. This was its chemical property: flammability.
- 4. Observing Chemical Change • Physical Properties: a characteristic of a substance that can be observed without changing the substance into something new. – EXAMPLE: Frozen water (ice) melts at 0 degrees Celsius. The tops of the tables in this room are black and 4.5ft long.
- 5. Observing Chemical Change • Like the properties of matter, the changes it undergoes can be: – Physical Changes OR – Chemical Changes
- 6. Observing Chemical Change • Physical Changes: Any change that alters the form, shape, or appearance of a substance but does not change it into a new substance. – EXAMPLE: If I were to toss fresh berries into a blender and make a fruit smoothie- it would still be fruit, just mashed into smaller pieces.
- 7. Observing Chemical Change • Chemical Changes: a change that a substance undergoes where a totally new substance is the result. – EXAMPLE: In the magnesium lab, we burned magnesium and after it’s chemical change the result was magnesium oxide. It was no longer metal!!
- 8. Observing Chemical Change • During a chemical change you have: – Reactants: the substance that is being changed. – Products: the new substance formed as a result of the chemical reaction.
- 9. Observing Chemical Change • REMEMBER: in order for a chemical reaction to have occurred- bonds must be broken and new bonds must be made!!!
- 10. Observing Chemical Change • EVIDENCE that a CHEMICAL REACTION has occurred: – Change in properties – Change in energy
- 11. Observing Chemical Change • Change in properties: color change, a solid forms (precipitate), formation of gas, and texture change. • CAUTION!! Sometimes physical changes make it SEEM like a chemical change has occurred. Really THINK about the changes.
- 12. Observing Chemical Change • Change in Energy: During chemical changes, energy is either absorbed or released. – Endothermic reactions (heat enters) – Exothermic reactions (heat exits) • (remember those words…??)
- 13. Describing Chemical Changes • Chemical equations are used to show/explain a chemical reaction. – This shows the reactants and products of a reaction – They show the substances you start with, on the left and the new substances on the right separated by an arrow.
- 14. Describing Chemical Changes • Generic formula looks like: Reactant + Reactant ---> Product + Product
- 15. Conservation of Mass (matter) • During Chemical reactions, atoms cannot be created OR destroyed. • The total mass of the reactants must equal the total mass of the products.
- 16. Conservation of Mass (matter) • In a chemical reaction, the number of atoms stays the same- they are just rearranged. Therefore, the number of atoms in the reactants are the same as the number of atoms in the products.
- 17. Open and Closed System • Sometimes it’s hard to understand where the matter comes from in a reaction. • Matter can either come from an… – Open System or a… – Closed System
- 18. Open and Closed System • Open System: Matter can enter from or exit into the surroundings during a reaction. • Closed System: Matter cannot enter or leave during the reaction.