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Learn about matter, its properties, physical and chemical changes, and the difference between pure substances and mixtures. Explore the states of matter and the changes in energy that occur during these states. Understand the basics of energy transformation and temperature measurement.
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Matter- anything that has mass and takes up space. Matter makes up the materials around you. Mass- the amount of matter in an object. Even air has mass. Weight- the measure of gravitational force on an object. * The standard scientific unit for weight is grams. 100 grams = approx. 1 N on Earth. (1 N is about 0.25 lbs.) Volume- the amount of space that an object takes up. Density- The amount of mass in a volume.
Water displacement to find volume: 52 mL -50 mL= 2 mL or 2 cm³ 5.8 mL -4.8 mL= 1 mL or 1 cm³
Pg. 14 Do the Math: Calculate: Obsidian is another type of igneous rock. What is the density of a piece of obsidian that has a mass of 239.2 g and a volume of 92 cm³? Formula: D=m/V D= 239.2 g / 92 cm³ D= 2.6 g/cm³
Pg 15 Do the Math: Calculate: A rhyolite rock has a volume of 9.5 mL. The density of the rock is 2.6 g/cm³. What is the mass of the rock? Formula: m= D•V m= 2.6g/cm³ • 9.5mL m= 24.7 g
Physical property- characteristics that do not involve a chemical change *Write the common physical properties found on pages 24-25 in your notes Chemical Property- property of matter that describes a substance’s ability to participate in a chemical reaction.
Module HUnit 1: MatterLesson 3: Physical and Chemical Changes
Physical Change- Chemical Change- Law of Conservation of Mass- states that in ordinary physical and chemical changes, mass is not created or destroyed, only transformed into different substances. Bubbles are formed, substance does NOT change Physical Odor produced Change in energy Chemical Chemical Change in energy Change in color Substance does NOT change Physical
Atoms- the smallest unit of an element that maintains the properties of that element Element- made of one or more element of the same kind of atom Compound- made from different kinds of atoms, held together with chemical bonds. These compounds have different properties than the single elements they are made from. Mixture- a combination of elements and compounds, that are NOT chemically bonded.
Pure Substance- A sample of matter, either a single element or a compound, that has definite chemical and physical properties What is the difference between a
Energy is gained Energy is lost
Melting Evaporation Flow of energy during changes of state.
Specific Latent Heat- the heat required to convert a solid to a liquid, or a liquid into a vapor, without a change in temperature.
Unit 1 TEST Review How do you find volume of an odd shaped item? Place the item in a graduated cylinder and measure the amount of displaced water What tools do you need to determine the density of an item? You will need a graduated cylinder What are Physical Changes? Changes that can be observed without a change it the identity of the substance (magnetism, solubility, malleability) What are Chemical Changes? Changes the substance (example: cooking meat) How are Chemical and Physical changes alike? Both obey the law of conservation of mass Different? Physical: changes the way it may look, Chemical: changes the substance What are the chemical properties of water? Water reacts with metal Law of Conservation of Mass: Mass cannot be created or destroyed, only changed.
Pure Substance: includes elements and compounds Mixture: the parts keep their own properties Solution: allows light to pass through Example of a solution: salt water Suspension: looks cloudy, you may see tiny particle floating in it. Example of a suspension: sandy water Use the Law of Conversation of Mass to explain melting. although it may appear that you have less substance, the liquid has only changed from a solid to a liquid, the mass remains the same. sublimation? Same theory as melting, except the fluid goes from a solid to a gas without a change in mass Properties of a solid: has a definite shape What happens to the temperature during evaporation? It remains the same
States of Matter: melting – A solid becomes a liquid Freezing- A liquid becomes a solid Boiling- A liquid becomes a gas (throughout) Evaporation- A liquid becomes a gas (on the surface) Condensation- A gas becomes a liquid Sublimation- A solid becomes a gas deposition- A gas becomes a solid
Energy- the ability to cause change (always measured in Joules “J”) Energy Transformation- anytime energy changes from one form to another. Law of Conservation of Energy- states that energy cannot be created or destroyed, only changed.
Kinetic Theory of Matter- states that the particles that make up matter are constantly in motion. The average kinetic energy of those moving particles is how temperature is measured.
Temperature- measures the average kinetic energy in in an object. Degree(°)- units of the temperature scale. Thermometer- instrument to measure temperature.
Thermal Energy- the kinetic energy of all particles in an object Heat- energy transferred from hot objects to cold objects Calorie (cal.)- the amount of energy needed to raise the temperature of 1 g of water 1 °C. Conduction- transfer of heat through direct touch Conductor- a material that transfers heat very well Insulator- a material that reduces or prevents the transfer of heat Convection- movement of matter due to differences in density. Radiation- transfer of energy as electromagnetic waves.
Renewable Both Nonrenewable Resources replaced by nature at the same rate or faster than they are used up. Cannot be replaced, reused, or reproduced as fast as it is used. Finite amount that can run out. Resources used by humans to transform stored energy into useful forms of energy.
Unit 2 TEST Review potential energy- stored energy kinetic energy- energy of motion What causes an object to have more or less kinetic energy? Mass KE= ½ m•v² types of energy-
thermal energy- heat transfers from an object of higher temperature to an object of lower temperature renewable energy- Resources replaced as they are used up. nonrenewable energy- Cannot be reproduced as fast as it is used. Finite amount that can run out. calorie- the amount of energy needed to raise the temperature of 1 g of water 1 °C. (incorrect on test) How do the particles react at different temperatures? Particles have less energy at lower temperatures What type of energy do we mostly use in the USA? Fossil fuels
Have a basic understanding of temperature in degrees Celsius and **Kelvin
**Know types of heat transfer **Conductor **Insulator **Radiation
Module HUnit 3: Atoms and the Periodic TableLesson 1: The Atom
Atom- The smallest particle into which and element can be divided and still be the same element Electrons- (-)negatively charged particles 0u Nucleus- (+) small dense center that is surrounded by moving electrons. Proton- (+) positively charged particles in the nucleus (protons and electrons are ALWAYS =) Neutrons- neutral particles in the nucleus. Electron Cloud- region around the nucleus where current theory believes electrons may be found
Mass Number- total number of protons and neutrons in the nucleus https://www.youtube.com/watch?v=JjozjUCsSaU&t=357s Atomic Number- the number of protons in the nucleus (# of protons = # of electrons)
Module HUnit 3: Atoms and the Periodic TableLesson 2: The Periodic Table
