SCIENCE GATEWAY

1. SCIENCE GATEWAY CHEMISTRY REVIEW

2. MATTER PHASES PROPERTIES CHANGES

3. Chemical and Physical Key Terms • Atom – Smallest unit of matter having all the characteristics of a certain element.

4. Ion –charged particle

5. Molecule – Two or more atoms of the same substance.

6. Law of Conservation of Matter – Matter cannot be created or destroyed

7. States of Matter – solid, liquid, gas are the 3 common states of matter. (There are 2 others.)

8. Physical Properties – Such as color, size, shape.

9. Physical Changes – Do not alter the chemical makeup of a substance, such as cutting.

10. Chemical Properties – Such as acidity, interactions, structure. (tomatoes were once thought to be poisonous. Why?)

11. Chemical Changes – Do alter the chemical makeup, such as burning.

12. More Key Terms • Intermolecular Attraction – Two or more molecules attracting one another.

13. SOLIDS molecules are closely packed together. strong intermolecular attraction intermolecular space is limited. not compressible most dense (exception is water.) Three phases of matter

14. LIQUIDS molecules not closely packed. less intermolecular attraction molecules able to move around more intermolecular space are not compressible Phases of matter

15. GASES molecules far apart weak intermolecular attraction molecules are free to move around more intermolecular space easily compressible least dense of 3 phases Phases of matter

16. quick quiz – 3 phases of matter closely 1-molecules in solids are ________ packed together. 2-solids have a strong _____________ ___________. 3-solids are the most dense except for ___________. 4-the molecules in liquids have ______ intermolecular attraction than solids. 5-the molecules in liquids can move around _________ than the molecules in solids. 6-liquids take the ____________ of their container. intermolecular attraction water less more freely shape

17. quick quiz – 3 phases of matter(continued) 7 - in ________ the molecules are farthest apart. 8 - gases have ______ intermolecular attraction. 9 - gases are the least ______ of all three phases. 10- in a gas, molecules move around _________. liquids weak dense most freely

18. PHYSICAL don’t involve changes in composition can be qualitative or quantitative temperature color odor size; density melting, boiling, freezing points CHEMICAL observed when composition of a substance changes describe ability to react or decompose rust on iron ability to burn instability of a substance Physical and chemical properties

19. X X X X X X X X X X X

20. X X X X X X

21. Law of conservation of mass (matter) ~~In a chemical change~~ matter is neither created or destroyed! (atoms do not appear/disappear)

22. Quick quiz – Properties, Changes and Conservation changes 1 - Physical properties do not involve _________ in composition. 2 - Physical properties can be qualitative or _________. 3 - a _______ property can only be observed if there has been a change in substance. 4 - a chemical property describes a substance’s ability to react or ____________. 5 - Name 2 examples of a physical property and 2 examples of a chemical property/change. 6 - State the law of conservation of matter. quantitative chemical decompose Matter is neither created or destroyed

23. gateway practice paragraph *write about what you have learned It’s time to build a campfire outside to roast some hot dogs for your picnic. You have matches and wood. What else do you need to: -get and keep the fire burning? -put the fire out? -explain which state of matter each of these two products are and describe characteristics of each. As this fire burns, describe what kind of change you are observing. *clue – think change in substance / what is this new substance?

24. SCIENCE GATEWAY CHEMISTRY REVIEW

25. ATOMIC STRUCTUREAND BONDING

26. Atomic Structure and Bonding Key Terms • Element – Substance made up of only one type of atom. • Compound – Atoms of different elements are chemically held together • Subatomic Particles – Particles that make up atoms. • Atomic Number – Number of Protons only.

27. More Key Terms • Valence Electron – Electron on the outermost energy level. • Lewis Dot Structure – Model to display valence electrons. • Periodic Table – Systematic chart of the elements and (some of) their characteristics • Mass Number - Protons plus neutrons in an atom.

28. More More Key Terms • Atomic Mass Unit – 1 AMU = 1.661x10-24 kg • Proton – Positively charged subatomic particle located in the nucleus • Neutron – Uncharged subatomic particle located in the nucleus • Families (groups) – A column on the periodic table.

29. More More More Key Terms • Element Symbol – Abbreviation for elements’ names on the periodic table. • Electron – Negatively charged subatomic particle located in orbit around the nucleus. • Period – Rows of the periodic table.

30. More More More Key Terms • Ionic Bonding – Ions of opposite charge held together due to electric fields. • Isotope – Elements with different number of neutrons than usual. • Covalent Bonding – Atoms bonded by their valence electrons.

31. 5 11 5 6 5 16 32 16 16 16 7 14 7 7 7 17 35 17 18 17 6 12 6 6 6 13 28 13 15 13 53 128 53 75 53 15 31 15 16 15 18 40 18 22 18

32. Ionic bonding -electrons are either gained or lost by atoms -occurs between metals and nonmetals metals lose electrons - nonmetals gain electrons -creates ions – positive (fewer electrons) or negative (more electrons) -strong bonds; usually solid; high melting and boiling points -atoms want complete, full outer shells to be happy! magic number is 8! (exception: H and He each need 2.)

33. Ionic bonding

34. common ionic bonds • NaCl sodium chloride – table salt • CuSO4 copper sulfate (treats algae growth in pools) • NaHCO3 baking soda

35. covalent bonding • electrons are shared between atoms • neither atom has a charge • intermolecular forces between molecules are weak, and have lower melting and boiling points; tend to be liquids and gases at room temperature; if solid - can form crystals • common covalent compounds: water, sugar, hydrocarbons

36. Covalent bonds

37. quick quiz –Ionic bonding gained 1-in ionic bonding electrons are either or . lost Metals nonmetals 2- lose electrons and gain electrons. fewer 3-a positive ions has electrons and a negative ion has electrons. more Ionic 4- bonds are strong, usually solid, and have melting and boiling points. high 5-the magic number of valence electrons needed by all but two atoms is . eight Table salt, baking soda. 6-name two common ionic bonds.

38. Quick quiz –Covalent bonding shared 2-neither atom has a __________. 1-in a covalent bond, electrons are _______. charge 3-intermolecular forces _______________ are weak. between molecules 4-covalent bonds have ___ melting and ___ points. low low 5-covalent bonds are usually found in these two states of matter: Liquids and gases water 6-two common covalent compounds are ______ and _______. sugar

39. Atomic Bonding 2. Choose the type of bonding (covalent or ionic) that will form between the following atoms. 1. Sodium and Chlorine 2. Carbon and Oxygen 3. Magnesium and Nitrogen 4. Fluorine and Fluorine 5. Barium and Oxygen ionic covalent ionic covalent ionic

40. subatomic particles • Proton -same as atomic number - located inside nucleus - mass of 1 amu -positive charge

41. subatomic particles Neutron -located inside nucleus -mass of 1amu -has no charge; neutral -to find number of neutrons: mass # - atomic #

42. Subatomic particles Electron -orbits around nucleus -mass much less than 1 amu -negative charge Valence electron -outer shell electron - is involved in chemical bonding

43. quick quiz – subatomic particles proton 1-the positive particle is the ______________. 2-the negative particle is the ______________. electron 3-the neutral particle is the _______________. neutron 4-the proton is the same as the ________ number. atomic 5-the two particles located inside the nucleus are the _________ and the ________. Each of these particles have a mass of ______________. proton neutron 1 amu

44. quick quiz – subatomic particles (continued) 6-the electron _______ the nucleus. orbits valence shell 7-the _________ electrons are the outer _____ electrons and are involved in _______ bonding. covalent 8-to find the number of neutrons in an atom you subtract the ________ number from the _________ number. atomic mass

45. Atomic Number -number used to arrange periodic table -increase left to right -same as number of protons and electrons in a neutral atom Mass Number -sum of the protons and neutrons in nucleus of an atom numbers

46. electron arrangement • electrons orbit the nucleus in energy levels. • outermost electrons involved in bonding process – valence electrons • Lewis dot structure – shows number of valence electrons of an element and how these electrons are shared so that elements can bond.

47. 2. Discuss the differences between ionic and covalent bonding. • In ionic bonding, electrons are given from one atom to another forming a strong bond. These are formed between metals and non-metals. • Covalent bonding involves the sharing of electrons, it is a weaker bond formed between non-metals.

48. Lewis dot structures Show how the row of elements act like jigsaw puzzle pieces…

49. quick quiz – Numbers and Electron Arrangement atomic number left right 1-The ___________ ____ is used to arrange the periodic table as it increases from ____ to _____. protons 2-the atomic number is the same as the number of ____ . mass 3-the _____ number is the sum of protons and neutrons inside the ________. nucleus valence 4-the outermost electrons are the ________ electrons and they orbit the nucleus in _________ levels. energy Lewis Dot Structure 5-A shows the number of valence electrons and how they are shared in the process between elements. bonding

50. gateway practice paragraph • write about what you have learned! Compare and contrast the two types of bonding. How are they similar? How are they different? - name each type of bond - which subatomic particle is involved in the process - how it is arranged in each type of bond - name one compound formed by each type of bond. *clue – think valence and what atoms need to be happy