1 / 22

Matter and Energy

Matter and Energy. Matter. Matter is anything that has mass and volume Two forms of matter Pure Substances Mixtures. Pure substances. Uniform composition The same throughout the sample Two Types Elements Compounds. Elements. Simplest form of matter Cannot breakdown

ronan-hood
Download Presentation

Matter and Energy

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Matter and Energy

  2. Matter • Matter is anything that has mass and volume • Two forms of matter • Pure Substances • Mixtures

  3. Pure substances • Uniform composition • The same throughout the sample • Two Types • Elements • Compounds

  4. Elements • Simplest form of matter • Cannot breakdown • Smallest part called atom • Represented using a capital letter or capital letter and lower case letter

  5. compound • Two or more elements chemically joined in a specific ratio • Can be broken down • Decomposed • Properties of the compound are different than the elements that make it up

  6. mixture • Two or more substances physically joined in any ratio • Keep the properties of the components of the mixture • Two types • Heterogeneous • Homogeneous

  7. Heterogeneous Homogeneous Visible difference between components (parts) No visible differences between components (parts) Called a solution Represented using (aq) aqueous

  8. Properties of matter • Physical Properties • Properties that can be observed without changing the substance • Chemical Properties • Properties that show how a substance reacts (changes)

  9. Energy • Energy is the driving force behind change • Cannot be created or destroyed • Does change its form • Sound • Chemical • Radiant (light) • Electrical • Atomic (nuclear) • Mechanical • Thermal (heat)

  10. Two types of energy • Kinetic • Energy of motion • Potential • Stored energy

  11. Measurements involving energy • Temperature • Average kinetic energy of particles • Measured using a thermometer (unit: degrees) • Fahrenheit • Celsius • Kelvin • To convert • °F to °C -- use °C = 5/9( °F - 32) • °C to ° F -- use °F = 9/5°C + 32 • °C to K -- use K = °C + 273 • K to °C– use K = °C + 273

  12. Measurements involving energy • Calorimetry • Measures the actual energy (q) in a system • Related to mass (m), specific heat capacity (C) and temperature change (∆T) • Measured using a calorimeter (unit: joules) • To calculate energy use • q = m C ∆T • q = m Hfusion • q = m Hvaporization

  13. Cwater = 4.18J/g °C Hfus= 334J/g Hvap = 2260J/g • How many joules are required to heat 40g water at 30°C to 70°C? q = m C ∆T q = 40g x 4.18J/g°C x 40°C q = 6688J • 5000J were added to 30g water at 25°C. What is the new temperature? q = m C ∆T 5000J = 30g x 4.18J/g°C x ∆T 5000 = 125.4 x ∆T ∆T = 39.9 ~ 40 T new= 25 + 40 T new= 65°C • How many joules are needed to melt 100g ice at 0°C q = m Hfus q = 100g x 334J/g q = 33400J

  14. Phases of Matter • Solids • Liquids • Gases

  15. Solids • Matter that has specific shape and specific volume • Atoms closely packed together • Cannot be compressed

  16. Liquids • Matter that has a specific volume but takes the shape of the container • Atoms are close but have some space between them • Cannot be compressed • Can be poured

  17. Gases • Matter that takes the shape and volume of the container • Atoms have free space between them • Compressible • Can be poured

  18. Phase Changes If energy is added… • Melting • Solid to liquid • Boiling • Liquid to gas • Sublimation • Solid to gas

  19. Phase Changes If energy is removed… • Freezing • Liquid to solid • Condensing • Gas to liquid • Deposition • Gas to solid

  20. Phase Diagram Heating Curve for a Substance boiling gas melting liquid solid

  21. Phase Diagram Heating Curve for a Substance potential kinetic potential kinetic kinetic

  22. condensing freezing

More Related