1. 8 th Grade SOL Chemistry Review

2. In order to meet this standard, it is expected that students will  describe the particle theory of matter.  describe how to determine whether a substance is an element, compound, or mixture.

3. Matter is anything that has mass and occupies space. All matter is made up of small particles called atoms. Matter can exist as a solid, a liquid, a gas, or plasma.

4. Matter can exist as a solid, a liquid, a gas, or plasma. describe the properties of solids, liquids, gases, and plasma. Plasma

5. distinguish between physical properties (i.e., shape, density, solubility, odor, melting point, boiling point, and color) and chemical properties (i.e., acidity, basicity, combustibility, and reactivity).

7. Properties: are characteristics Physical properties describe a substance. Chemical properties describe how a substance will react to something else.

8. find the mass and volume of substances and calculate and compare their densities.

9. Mass Volume Density The amount of matter in a substance. The amount of space an object or substance occupies: V=LxWxH Mass of a substance per unit volume: D= M/ V

10. define compounds as inorganic or organic. (All organic compounds contain carbon). Organic compounds contain Carbon Inorganic compounds do not contain Carbon

11.  analyze the pH of a solution and classify it as acidic, basic, or neutral.

13.  describe what a salt is and explain how salts form.  When an acid and a base mix in equal amounts to neutralize each other a salt and water is formed.  HCl + NaOH ----  NaCl + H 2 O Hydrochloric Acid + sodium hydroxide yields Sodium chloride and Water.

14. determine the identity of an unknown substance by comparing its properties to those of known substances. The major categories are metals, nonmetals, metalloids, you may also be asked about acids, bases and salts.

15. Metals: Most are solids, have a luster, are good conductors and are malleable and ductile. They are located on the left side of the Periodic table. Mercury is a liquid at room temperature. Nonmetals: may be solids liquids or gases, most are dull and brittle. They are good insulators and are located on the right side of the periodic table. Bromine is a liquid all others are solids or gasses

16. Metalloids are located along a stair step line between the metals and nonmetals. Some are semiconductors: conduct electricity under certain conditions, Can act like metals or nonmetals. Acids are sour and react with metals to form hydrogen gas. Turn blue litmus paper red. Bases: are bitter and slippery to the touch, they turn red litmus paper blue.

17. http://www.periodni.com/download/periodic_table-color.png

18.  design an investigation from a testable question related to physical and chemical properties of matter. The investigation may be a complete experimental design or may focus on systematic observation, description, measurement, and/or data collection and analysis. (Students should be able to use the inquiry skills represented in PS.1 and LS.1 to compose a clear hypothesis, create an organized data table, identify variables and constants, record data correctly, We did an activity with unknown substances and you tested the properties to determine the properties and identity of the substances.

19. construct appropriate graphs, analyze data, and draw reasonable conclusions.) http://img.sparknotes.com/content/testprep/bookimgs/sat2/chemistry/ 0003/sat117002_0507.gif

20. https://www.youtube.com/watch?v=uuGBzQDbOXI http://www.bbc.co.uk/bitesize/intermediate2/mathematics/images/200/108 _bitesize_intermediate2_mathematics_bargraph_table_crisps.png

22. In order to meet this standard, it is expected that students will describe the historical development of the concept of the atom and the contributions of Dalton, Thomson, Rutherford, Bohr and other scientists (Schrödinger). differentiate among the three basic particles in the atom (proton, neutron, and electron) and their charges, relative masses, and locations. compare the Bohr atomic model to the electron cloud model with respect to its ability to represent accurately the three- dimensional structure of the atom.

23. Stated that matter in the form pf Elements was made of particles called atoms. Atoms cannot be divided or destroyed Atoms of the same element are alike in mass and atoms of different elements are different in mass. Elements combine in predictable ratios.

24. Thomson proved that atoms give off electrons. He reasoned that the atom must also have positive charges to balance out the negative charges. The Electrons are scattered through it like raisins in a muffin.

25. His experiment found that alpha particles struck a thin piece of gold foil passed through the foil except a few that bounced off sideways. He reasoned that most of the atom is empty space. A small part of an atom is solid and has a positive charge and he called this the nucleus. Electrons have a negative charge and move around the nucleus like planets in the solar system.

26. He said Electrons move around the nucleus in orbits he called energy levels. The lower their energy the closer they are to the nucleus Higher energy electrons are further from the nucleus.

27. The modern model is based upon calculations made by Edwin Schrodinger. According to this model electrons exist in an area around the nucleus called a “cloud”. An electron may be found anywhere in the Cloud. This model explains how substances have color, release heat, or give off radiation.

28. http://www.scienceclarified.com/images/uesc_02_img0063.jpg

29. In order to meet this standard, it is expected that students will use the periodic table to obtain the following information about the atom of an element: symbol atomic number atomic mass state of matter at room temperature number of outer energy level (valence) electrons. describe the organization of the periodic table in terms of atomic number metals, metalloids, and nonmetals groups/families vs. periods.

30. Atomic Number Atomic Mass Element Symbol

31. http://f.tqn.com/y/chemistry/1/S/X/u/PeriodicTableNaturalState.jpg

32. http://images.tutorcircle.com/cms/images/44/periodic-table-with-valence-elelectrons.png Remember the transition elements can have valences of 1-4 denoted by roman numerals “Iron IV”

33. http://adesanjaya.com/images/periodic%20table/periodic-table- families/periodic-table-family-names-and-groups960-x-720-97-kb-jpeg-x.jpg

34. recognize that an atom’s identity is related to the number of protons in its nucleus. categorize a given element as metal, nonmetal, or metalloid. given a chemical formula of a compound, identify the elements and the number of atoms of each that comprise the compound. recognize that the number of electrons in the outermost energy level determines an element’s chemical properties or chemical reactivity. describe the difference between ionic and covalent bonding. predict what kind of bond (ionic or covalent) will likely form when metals and nonmetals are chemically combined.

35. http://www.vias.org/physics/img/bk4_fehlendes_bild_02.png

36. https://d2gne97vdumgn3.cloudfront.net/api/file/9MpYatkxTeefvOaQoNl9

37. Given a chemical formula of a compound, identify the elements and the number of atoms of each that comprise the compound. Chemical Formula: NaHCO 3 Sodium 1, hydrogen 1, Carbon 1, Oxygen 2.

38. recognize that the number of electrons in the outermost energy level determines an element’s chemical properties or chemical reactivity. Fewer the outer electrons the more reactive the element is Elements with eight electrons in their outer level are not reactive.

39. Describe the difference between ionic and covalent bonding. Ionic bonding: Occurs between metals and nonmetals. Involves a transfer of electrons. Covalent bonding occurs between two nonmetals. Elements share electrons

40. predict what kind of bond (ionic or covalent) will likely form when metals and nonmetals are chemically combined. Electronegativity (EN)is a measure of the attraction of an atom for an electron. The higher the electronegativity the greater the attraction of that atom for an electron. The electronegativity scale goes from 0 to 4.0 (for fluorine). One way to predict whether a bond is ionic or covalent is to look how far apart the two atoms forming the bonds are in the periodic table. If one atom is of the far left (Group 1 or 2) and the other is on the far right (Group 5, 6, or 7), then the atoms will have large differences in EN and will form an ionic bond. Most other pairs of atoms are close enough in EN to form covalent bonds. For example, any two atoms in the main group elements (Groups 3, 4, 5, 6, 7), will usually form a covalent bond.

43. The student will investigate and understand changes in matter and the relationship of these changes to the Law of Conservation of Matter /Energy. a) physical changes; b) chemical changes; and c) nuclear reactions. compare and contrast physical, chemical, and nuclear changes. identify the reactants and products in a given chemical equation formula. design an investigation that illustrates physical and chemical changes. given chemical formulas, write and balance simple chemical equations. analyze experimental data to determine whether it supports the Law of Conservation of Mass. recognize that some types of chemical reactions require continuous input of energy (endothermic) and others release energy (exothermic). describe, in simple terms, the processes that release nuclear energy (i.e., nuclear fission and nuclear fusion). Create a simple diagram to summarize and compare and contrast these two types of nuclear energy. evaluate the positive and negative effects of using nuclear energy.

44. Physical changes do not change what the substance is. Change in color, size, shape, state,

45. New substances are formed.

47. identify the reactants and products in a given chemical equation formula.

48. given chemical formulas, write and balance simple chemical equations.

49. analyze experimental data to determine whether it supports the Law of Conservation of Mass.

50. recognize that some types of chemical reactions require continuous input of energy (endothermic) and others release energy (exothermic).

51. describe, in simple terms, the processes that release nuclear energy (i.e., nuclear fission and nuclear fusion). Create a simple diagram to summarize and compare and contrast these two types of nuclear energy. Fusion: takes place in the sun.

52. Fission: used in nuclear reactors.

53. evaluate the positive and negative effects of using nuclear energy. Clean cheap energy Nuclear plants can be environmentally disastrous if a melt down occurs. Nuclear waste stays reactive for thousands of years and must be stored in a safe place.