4.02 Atomic Models

1. Click on Dalton's statements and a pop up will show you which 2 statements were proven false. 4.02 Atomic Models • Can you list all five statements of Dalton’s atomic theory? • And tell which 2 have been proven false? • 1. • 2. • 3. • 4. • 5. • Can you describe the work of Thompson? • What equipment did he use in his experiment? • What charge did he find in an atom? • What did his atom look like?What is his model commonly called? • Can you describe the work of Rutherford? • What was his experiment? • What was the results of his experiment? • Which subatomic particle did he discover? • Can you describe the work of Bohr? • Where did he think electrons are found? • What does Bohr’s model resemble? • What is the new field of study he inspired? • How is an electron cloud part of the current atomic model? Electrons travel as ______in the _________ ________that surrounds the____________. This answer is in 4.02- Click on Text Version of the video from Thomson to Today.

2. 4.02 Atomic Models Which 2 of Dalton’s statements have been proven false? • All matter is made of atoms. • All atoms of a given element are the same. • Different elements are made up of different atoms. • Atoms cannot be divided into smaller pieces. • Atoms of different elements combine in whole number ratios to make compounds.

3. 4.02 Atomic Models • Can you describe the work of Thompson? What equipment did he use in his experiment? • a. gold foil • b. cathode ray • c. electron microscope What charge did he find in an atom? • a. positive proton • b. negative electron • c. neutral atom What did his atom look like?What is his model commonly called? • a. plum pudding • b. solar system • c. helix

4. 4.02 Atomic Models • Can you describe the work of Rutherford? What was his experiment? • a. used a cathode ray tube • b. shot alpha particles into gold • c. used electrically charged plates What was the results of his experiment? • a. All of the particles were deflected. • b. Most of the particles went through the foil, but some were deflected. • c. All of the particles went through the foil. Which subatomic particle did he discover? • a. proton • b. electron • c. neutron

5. 4.02 Atomic Models • Can you describe the work of Bohr? Where did he think electrons are found? • a. in every part of the atom • b. in the nucleus • c. orbiting around the nucleus What does Bohr’s model resemble? • a. solar system • b. helix • c. plum pudding What is the new field of study he inspired? • a. Quantum Mechanics • b. Particle Physics • c. Classical Physics

6. 4.02 Atomic Models • How is an electron cloud part of the current atomic model? Electrons travel as ______in the _________ ________that surrounds the____________. A. waves B. orbits C. electron D. nucleus E. cloud

7. 4.03 Introduction to the Periodic Table Metalshave these properties…. 1. Ductility 3. Conductivity A. ductileA. good conductors of heat and electricity B. not ductile B. mod. conductors of heat and electricity C. poor conductors of heat and electricity 2. Luster 4. Phase A. metallic luster A. solid at roomtemp. B. moderate metallic luster B. gasses at room temp. C. no metallic luster C. solids or gasses at room temp.

8. 4.03 Introduction to the Periodic Table Non-Metalshave these properties…. 1. Ductility 3. Conductivity A. ductileA. good conductors of heat and electricity B. not ductileB. mod. conductors of heat and electricity C. poor conductors of heat and electricity 2. Luster 4. Phase A. metallic luster A. solid at room temp. B. moderate metallic luster B. gasses at room temp. C. no metallic luster C. solids or gasses at room temp.

9. 4.03 Introduction to the Periodic Table Metalloidshave these properties…. 1. Ductility 3. Conductivity A. ductileA. good conductors of heat and electricity B. not ductileB. mod. conductors of heat and electricity C. poor conductors of heat and electricity 2. Luster 4. Phase A. metallic luster A. solid at room temp. B. moderate metallic luster B. gasses at room temp. C. no metallic luster C. solids or gasses at room temp.

10. 4.03 Introduction to the Periodic Table What does it mean for a substance to be a semi-conductor? • A. it has properties half-way between metals and non-metals • B. it is only half of a material • C. it is a poor conductor of electricity Why are they so important to the technology industry?

11. 4.04 Using the Periodic Table a. atomic b. atomic mass c. protons d. neutrons e. electrons

12. 4.04 Using the Periodic Table atomic protons electrons a. atomic b. atomic mass c. protons d. neutrons e. electrons

13. 4.04 Using the Periodic Table atomic protons electrons atomic mass atomic atomic mass neutrons row column

14. Elements, Compounds and Mixtures with Mrs. Greer

15. Matter Scientists classify matter based on their composition and how the matter can be separated into its basic components. There are pure substances and mixtures. • Pure Substances= definite composition throughout and cannot be separated by physical means. • Elements • Compounds • Mixtures= do not have a definite composition and can be separated by physical means. • Homogeneous Mixtures • Heterogeneous Mixtures

17. Elements- • A pure substance that cannot be broken down any further by physical or chemical means. • Elements are made up of only 1 type of atom. • There are more than 100 known elements and they are listed on the Periodic Table. A helium atom.

18. Examples of Elements

20. Compounds • Two or more elements that combine chemically. • Maintain a definite composition. • Can be separated by chemical means (ie. Electrolysis, combustion, and oxidation) • Divided into 2 categories: • Ionic Compounds • Covalent Compounds

21. Ionic Compounds Ionic bonds are created when a metal and a nonmetal combine. It is chemical bond that results from an electrostatic attraction that occurs when metal atoms lose electrons to nonmetal atoms. The metal atom gives its electrons to the nonmetal atom. An example would be table salt, NaCl, which is sodium chloride. The metal atom (sodium –Na) gives its electrons to the nonmetal atom (chlorine-Cl). Sodium bicarbonate is found in Baking Soda. Magnesium sulfate is found in Epsom Salt. Calcium carbonate is found in chalk and antacids • Properties of ionic compounds • High melting and boiling points • Solids • Contains positive and negative ions • Strong force of attraction between particles • Separate into charged particles in water to give a solution that conducts electricity • Brittle

22. Covalent Compounds Covalent bonds are created when two or more nonmetals combine. It is a chemical bond that is formed by the sharing of electrons between atoms. An example would be H2O, water. Two nonmetal atoms of hydrogen share their electrons with a nonmetal atom of oxygen. Covalent bonds are also called molecules. Rubber Sugar • Properties of covalent compounds • Lower melting and boiling points (often liquids or gases at • room temperature • Solids, liquids, and gases • Neutral molecules • Weaker forces of attraction between molecules • Remains the same molecule in water, therefore does not • conduct electricity • Soft, not brittle Isopropyl Alcohol Ammonia

23. Mixtures • A mixture is two or more elements or compounds that • are blended without combining chemically. • Each part of the matter in a mixture has its own • identity (properties). • Mixtures can be separated using physical or • mechanical means. • There are 2 types of mixtures: • - Heterogeneous mixtures • - Homogeneous mixtures

24. Heterogeneous Mixtures The substances in this kind of a mixture are not spread out evenly, not uniform. Heterogeneous mixtures can be separated by physical means.

25. Homogeneous Mixtures The substances in a homogeneous mixture are spread evenly throughout, uniform. This kind of mixture is called a solution. Solution- a homogeneous mixture in which one substance (the solute) is dissolved in another substance (the solvent). Water is known as the universal solvent. Lemonade- Lemonade mix (solute) dissolved into water (solvent). Bronze- Tin (solute) dissolved into copper (solvent). Saltwater- Salt (solute) dissolved into water (solvent).

27. How much have we learned? • Quiz • Jeopardy

28. PRACTICE Classify each of the following as a: solution, heterogeneous mixture, element or compound. *A mixture that is uniform throughout - solution *Alloys are an example - solution *Marble is an example - heterogeneous mixture *Aluminum is an example - element *Sodium chloride is an example - compound *A pure substance that can be broken down by chemical means - compound *Sand and water is an example - heterogeneous mixture *A pure substance that cannot be broken down - element *Air is an example - solution *Carbon is an example - element *A mixture that is not uniform throughout - heterogeneous mixture *Carbon monoxide is an example – compound

29. What are examples of Physical Properties?

30. Physical Properties *Color When you observe the color of an object, you are observing a physical property. *Shape The shape of a sample of matter can be observed and even changed without changing the identity of the material. Ripping or folding a piece of paper does not stop it from being paper. *Phase/State The phase (solid, liquid, or gas) of a substance is a physical property that can be observed without changing the identity of the matter. *Density This ratio of mass per volume is a physical property that does not depend on the size of the sample. You will be learning more about this physical property in a later lesson.

31. Physical Properties Mass The measure (in grams or pounds) of the amount of matter in an object is definitely a physical property. *Volume The amount of space occupied by an object is a physical property that can be measured in units like liters or cubic centimeters.

32. Physical Properties *Ductility The ability to be pulled or stretched to make a wire is a physical property of metals. *Melting Point The temperature at which a solid becomes a liquid is a physical property unique to each type of matter. *Malleability The ability to be shaped, dented, or extended by beating with a hammer or rolling is another physical property of metals. Have you ever bent a metal spoon or put a dent in the door of a car?

33. Intensive and ExtensiveProperties

34. 4.08 Physical Properties - Extensive and Intensive Physical Properties *Extensive Physical Properties *An extensive physical property depends on the amount of matter present in the sample. Such properties include mass, length, shape, and volume. These measurements will change depending on how large or small the sample of matter. *Intensive Physical Properties An intensive physical property does not depend on the amount of matter present in the sample. Such properties include melting point, boiling point, density, ductility, malleability, and color. These properties will not change for a given type of matter regardless of the sample size.

35. 4.09 Weight vs Mass • *Weight -is a measure of Earth’s gravitational attraction for matter. This means that weight is affected by both the amount of matter in the object and the amount of gravity pulling on the object. This is why the weight of an object changes on different planets. • *Mass -is a measure of the quantity, or amount, of matter in an object. This means that the more matter there is in an object, the greater its mass. Mass is not affected by gravity. This is why the mass of an object does not change on different planets. • *Formula • weight = mass x gravity

36. 4.10 Density • *Density is: • *A ratio of mass per unit volume; or mass divided by volume. • *An intensive physical property that is used to help identify an element or compound. • *A property that is most commonly measured in the units: g/mL, g/cm3, or g/L.

38. States of Matter • 1. • 2. • 3. • 4.

39. States of Matter

40. States of Matter

41. States of Matter

42. Advanced States of Matter • Plasma- is a collection of charged particles that respond strongly to electromagnetic fields, taking the form of gas-like clouds or ion beams.

43. Advanced States of Matter • Plasmas are found in: • Fluorescent lights. • Plasma TVs, which are made up of tiny fluorescent lights (in the pixels). • Lightning. • Auroras, which are an atmospheric phenomenon of bands of light sometimes seen in the sky at the polar regions. Examples include the Northern Lights and Southern Lights. • The sun and stars. • Nebulae. • Interstellar space.

44. Physical Changes

45. Physical Changes • A physical change is any change in the property of matter that does not change the make up of the substance. • In a physical change, the chemical make up of a substance does not change. The only thing that changes is a physical property such as: • Color • Shape • Phase (solid, liquid, or gas) • Size

46. Chemical Changes

47. 5.03 Chemical Changes • A chemical change is a change one or more substances undergo when they become new or different substances. Another name for a chemical change is a chemical reaction. • Fireworks are an example of chemical change. The light, sound, and color are all signs that a chemical change is occurring

48. Chemical Changes • When a chemical change or reaction occurs: • The substances at the end of the reaction have different properties than the original substances. • The chemical bonds holding atoms together as compounds are broken. • New chemical bonds are formed, resulting in new chemical compounds.

49. Chemical Changes • Some easily observed changes strongly suggest that a chemical change has occurred. • Color change • Bubbling or fizzing • Light or heat production • Production of gases or solids • Odor production

50. Endothermic and Exothermic Reactions