2. Chemistry Unit Notes Science 10 PIB Science 10 PIB

3. Basic Vocabulary  Matter: Anything that has mass and volume  Mass: Amount of matter in an object  Volume: Amount of space an object takes up

4. More Vocabulary  Atoms: Smallest particle of an element that has all the properties of matter: –Protons- particles in the nucleus with positive charge –Electrons- particles orbiting around nucleus with negative charge –Neutrons- particles in the nucleus with no charge  Elements: Simplest form of a pure substance  Compounds: Two or more elements chemically combined to form a new substance

5. More Vocabulary A mixture is a physical combination of two or more kinds of matter. A mixture is a physical combination of two or more kinds of matter. A homogeneous mixture is one where the components are blended together so well that it looks like just one substance e.g. salt water or grape juice. Aka a solution A homogeneous mixture is one where the components are blended together so well that it looks like just one substance e.g. salt water or grape juice. Aka a solution A heterogeneous mixture is one where the different components retain their identity and are clearly visible e.g. iron filings and salt. A heterogeneous mixture is one where the different components retain their identity and are clearly visible e.g. iron filings and salt.

6. More Vocabulary A pure substance has a definite composition which remains the same in response to physical changes. E.g. copper, water with nothing dissolved in it, nitrogen, gold etc. A pure substance has a definite composition which remains the same in response to physical changes. E.g. copper, water with nothing dissolved in it, nitrogen, gold etc. Pure substances can be classified into elements and compounds. An element cannot be chemically separated into simpler substances whereas a compound can be separated chemically. Pure substances can be classified into elements and compounds. An element cannot be chemically separated into simpler substances whereas a compound can be separated chemically.

7. Chemical vs. Physical Change –Physical Change: A change that can occur without changing the identity of the substance. –Ex. Solid, Liquid, Gas (Phase change) –Chemical Change: Process by which a substance becomes a new and different substance –Ex. Fire

8. Sub-Atomic Particles Part of Atom ChargeLocationMass/Size Electron - negative outside nucleus.0006 amu (too little to count) Proton + positive inside nucleus 1 amu Neutron no charge inside nucleus 1 amu

9. Periodic Table

10. Using the Periodic Table Atomic Number Atomic Number –Equal to # protons = # electrons –Periodic Table is arranged by this number Symbol Symbol –“Shorthand” for the element – Note 2 nd letter is always lowercase Atomic Mass Number Atomic Mass Number –Total AVERAGE mass of Protons + Neutrons + Electrons 17 Cl 35.5

11. Electron Energy Levels Electrons are arranged in “Shells” around nucleus in predictable locations Electrons are arranged in “Shells” around nucleus in predictable locations Fill “seats” closest to nucleus first (concert – best seats) Fill “seats” closest to nucleus first (concert – best seats) “Seats” available “Seats” available –Shell #12 electrons –Shell #28 electrons –Shell #38 electrons –Shell #4 18 electrons –Shell #5 18 electrons –Shell #632 electrons Ex. Carbon has 6 total electrons so… Ex. Carbon has 6 total electrons so… Two electrons on first energy level Four electrons on second energy level Question: Could we fit more electrons on the second energy level if there were more electrons in carbon??

12. Atomic Structure 17 Cl 35.5 Total Mass of Nucleus 36 - 17 = 18 neutrons Element Name Chlorine Total # of protons and electrons (in a neutral atom) 17 protons in nucleus 17 electrons orbiting nucleus Notice: electrons follow energy level rules from previous slide. (Round Atomic Mass)

13. Atomic Mass – Fractions? Look at Chlorine (atomic number 17) Look at Chlorine (atomic number 17) Atomic mass of 35.5? I dont’ get it! Atomic mass of 35.5? I dont’ get it! Where does the 35.5 come from? Where does the 35.5 come from? –0.5 protons? 0.5 neutrons?  No Atomic Mass = average number of protons and neutrons in nature Atomic Mass = average number of protons and neutrons in nature

14. More Practice Determine the name, number of protons, neutrons and electrons for each element shown and draw… Determine the name, number of protons, neutrons and electrons for each element shown and draw… 15 P 31 8 O 16 26 Fe 56

15. Isotopes An isotope is a variation of an element (same protons) but can have diff. # of neutrons An isotope is a variation of an element (same protons) but can have diff. # of neutrons Ex: carbon (atomic mass = 12.011) Ex: carbon (atomic mass = 12.011) –Carbon (14) and carbon (12) exist in nature

16. Ions Change in electrons which gives an atom a charge (+ or -) Change in electrons which gives an atom a charge (+ or -) You can only add or subtract electrons! (protons don’t change) You can only add or subtract electrons! (protons don’t change) –Ex. Count the number of electrons below… Carbon ion (-1 charge) 7 electrons (-) 6 protons (+) Carbon ion (+1 charge) 5 electrons (-) 6 protons (+) Neutral Carbon 6 electrons (-) 6 protons (+)

17. Valence Electrons An electron on the outermost energy shell of an atom An electron on the outermost energy shell of an atom Important to understand because this is a key factor in how atoms will BOND with each other Important to understand because this is a key factor in how atoms will BOND with each other Octet rule – stable atom will have 8 electrons in that outer shell Octet rule – stable atom will have 8 electrons in that outer shell Practice – Valence # of Practice – Valence # of –Chlorine? –Neon? –Nitrogen? –Oxygen?

18. Electron Dot Diagrams a diagram that represents the # of valence electrons in an atom of an element. a diagram that represents the # of valence electrons in an atom of an element. The amount of electrons is displayed by dots around the symbol of the element. The amount of electrons is displayed by dots around the symbol of the element. Ex. Ex. http://www.fordhamprep.org/gcurran/sho/sho/le ssons/lesson38.htm http://www.fordhamprep.org/gcurran/sho/sho/le ssons/lesson38.htm http://www.fordhamprep.org/gcurran/sho/sho/le ssons/lesson38.htm http://www.fordhamprep.org/gcurran/sho/sho/le ssons/lesson38.htm

19. Types of Chemical Bonds Ionic- Two elements bond by transferring electrons to create ions that attract together (+ is attracted to - after an electron is transferred) Ionic- Two elements bond by transferring electrons to create ions that attract together (+ is attracted to - after an electron is transferred) Covalent- Two elements bond by sharing electrons (strongest bond type) Covalent- Two elements bond by sharing electrons (strongest bond type) Metallic- Two metals bond and form a “common electron cloud”. This is a cluster of shared electrons (weakest bond type) Metallic- Two metals bond and form a “common electron cloud”. This is a cluster of shared electrons (weakest bond type)

20. Examples of Bonding http://www.youtube.com/watch?v=xTx_DWboEVs http://www.youtube.com/watch?v=1wpDicW_MQQ http://www.youtube.com/watch?v=QqjcCvzWwww http://lc.brooklyn.cuny.edu/smarttutor/core3_22/Bonds.html

21. Predicting Bonds Ionic Bond = metal to non-metal Ionic Bond = metal to non-metal Covalent = non-metal to non-metal Covalent = non-metal to non-metal Metallic = metal to metal Metallic = metal to metal Do you understand why? HINT: the numbers at the top of the table indicate the # of valence electrons for each column

22. Oxidation Numbers Oxidation numbers are assigned to each element Oxidation numbers are assigned to each element They represent a predicted “charge” of an atom/ion when it bonds with another element. They represent a predicted “charge” of an atom/ion when it bonds with another element.  (tells us if the atom would prefer give or take electrons, and how many). They help us to predict what compounds will form when two elements get together. They help us to predict what compounds will form when two elements get together. Oxidation numbers are labeled like this: Oxidation numbers are labeled like this:  Na 1+  O 2-

23. How to Use Oxidation Numbers Oxidation Number indicates the number of electrons lost, gained or shared when bonding with other atoms. Ex. Na wants to lose an electron. If an electron is lost, it becomes a +1 charge SO: oxidation number for Na = 1+ Ex. Cl wants to gain an electron. If an electron is gained, it becomes a -1 charge SO: oxidation number for Cl = 1-

24. Oxidation Numbers Each column going down the periodic table has elements with the same oxidation number. Each column going down the periodic table has elements with the same oxidation number.

25. Label the oxidation numbers on your periodic table at the top of each column as shown here: Label the oxidation numbers on your periodic table at the top of each column as shown here: 1+ 2+ 3+ 4 (+/-) 3- 2- 1- 0

26. Rules for using oxidation numbers to create compounds 1.Positive ions can only bond with negative ions and vice versa 2. The sum of the oxidation numbers of the atoms in a compound must be zero (the key is to stay balanced) 3. If the oxidation numbers are not equal to zero, then you must add additional elements until they balance at zero. 4. When writing a formula the symbol of the Positive (+) element is followed by the symbol of the negative (-) element.

27. Examples of Forming Compounds Ex. Na (+1) + Cl (-1) = NaCl Are these oxidation numbers already equal to zero? If so, you don’t need to add any extra elements to combine them into a compound, so the answer is simply NaCl Ex. H (+1) + O (-2) = H 2 O How many +1 would you need to balance the -2 to zero? Since you need 2 atoms of the 1+ to balance the 2- to zero the resulting compound would be H 2 O In other words: to combine H with O, you MUST have 2 H to balance the oxidation numbers to zero 2+ and 2- = ZERO Ex. Al (+3) + S (-2) = Al 2 S 3 This one is tricky…we are not even close to balancing + and - to zero. Because of this we must have more than one Al and more than one S in our final equation. By using 2 Aluminums instead of just1 we would have 6+ By using 3 sulfers instead of just 1 we would have 6- Since these are now equal to zero, we combine 2 Aluminums and 3 Sulfers to make Al 2 S 3

28. Chemical Reactions Chemical Reaction: a process in which the physical and chemical properties of the original substance change as new substances with different physical and chemical properties are formed Chemical Reaction: a process in which the physical and chemical properties of the original substance change as new substances with different physical and chemical properties are formed

29. Chemical Reaction Basics H 2 + O 2 --> H 2 O Reactants- substance that enters into a reaction Products- substance that is produced by a chemical reaction ReactantsProducts

30. Evidence of Chemical Change  EPOCH is an acronym that stands for evidence that a chemical reaction has occurred. – Effervescence (bubbles and/or gives off gas) – Effervescence (bubbles and/or gives off gas) – Precipitate (solid crystals form) – Precipitate (solid crystals form) – Odor (change of smell is detected) – Odor (change of smell is detected) – Color change – Color change – Heat (reaction either heats up or cools down) – Heat (reaction either heats up or cools down)  Does sighting evidence of a chemical reaction mean that a chemical reaction has undoubtedly taken place? E P O C H

31. Types of Reactions Romance Chemistry :) Synthesis- Marriage/Dating A + B = AB Decomposition- Divorce/Breakup AB= A + B Single-Replacement- Dance Cut In A + BC = AC + B Double-Replacement- Dancing couples switch partners. AB + CD = AC + BD

32. Cartoon Chemistry This is an example of synthesis

33. Cartoon Chemistry This is an example of a decomposition

34. Cartoon Chemistry This is an example of a single replacement

35. Cartoon Chemistry This is an example of a double replacement

36. Reaction Types Review… Match each chemical reaction with one of the reaction types on your chemical cartoons. Match each chemical reaction with one of the reaction types on your chemical cartoons. –Zn + 2HCl  H 2 + ZnCl 2 –N 2 + 3H 2  2NH 3 –2KI + Pb(NO 3 ) 2  2KNO 3 + PbI 2 –2MgCl  Mg 2 + Cl 2

37. Conservation of Mass Atoms cannot be created or destroyed in a chemical reaction. Atoms cannot be created or destroyed in a chemical reaction. What goes in must come out. What goes in must come out. So we must balance equations to conserve mass. So we must balance equations to conserve mass.

38. Balancing Equations Rules: Rules: –We can not add or subtract subscripts from either side of the equation –We can only add coefficients to the front of each compound Ex. 2H 2 + O 2 --> 2H 2 O Ex. 2H 2 + O 2 --> 2H 2 O H = 4 H = 4 H = 4 H = 4 O=2 O = 2 O=2 O = 2 Before must match After Before must match After See “Balancing Act” worksheet for more examples…

39. Solution Chemistry  Mixtures: Matter that consists of two or more substances mixed but not chemically combined  Solutions: Homogeneous Mixture in which one substance is dissolved into another  Solute = Substance that gets dissolved (ex. Kool-Aid powder)  Solvent = Substance that does the dissolving (ex. Water)  Acid: Compound with a pH below 7 that tastes sour and is a proton donor.  Ex. Citrus foods  Base: Compound with a pH above 7 that tastes bitter and is a proton acceptor  Ex. Cleaning Products (soap)

40. Acids and Bases - Solutions can be acidic or basic - Acids and Bases have unique properties when dissolved in water -Acids = sour taste -Bases = bitter taste - Indicators are substances that change color when mixed with a solution, which helps to determine if a substance is an acid or a base. (pH paper, Litmus paper, cabbage juice)

41. Acids Proton donors (H+) Proton donors (H+) Acids contain hydrogen and produce positive ions (H+) when dissolved in water Acids contain hydrogen and produce positive ions (H+) when dissolved in water Acids = good electrolytes Acids = good electrolytes Examples of acids: Examples of acids: –Lemon Juice –Citric Acid –Carbonic Acid –HCl

42. Bases Proton acceptors Proton acceptors Bases contain hydroxide ions (OH-) when mixed with water. Bases contain hydroxide ions (OH-) when mixed with water. Bases = weak electrolytes Bases = weak electrolytes Examples of bases: Examples of bases: –Ammonia –Soap –Bleach (chlorine)

43. Combining Acids and Bases -Mixing acids and bases is a balancing act. (like a teeter-totter) (like a teeter-totter) Acid + Base = neutral (water and salt)

44. Combining Acids and Bases EXAMPLE: Acid + Base = neutral (water and salt) H+ + OH-  HOH + Salt H+ + OH-  HOH + Salt Acid Base water Acid Base water Ex. HCl + NaOH  H 2 O + NaCl

45. Measuring Acids and Bases pH scale- used to measure the acidity of a solution. pH scale- used to measure the acidity of a solution. Measure pH with indicators Measure pH with indicators pH scale goes from 0 – 14 pH scale goes from 0 – 14 0 = very acidic 0 = very acidic 14 = very basic 14 = very basic 7 = neutral 7 = neutral

46. Acids and Bases