Chemistry Over view.notebook November 12, 2014

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1 Science

2 Unit 2: Chemistry p What is chemistry? What is matter? How does chemistry affect our everyday life? How would you test to see if these common chemicals are present? O 2 CO 2 H 2 H 2 O Acids Bases 2

3 Pure Substances p Pure Substance All the particles of the substance are the same. There are two types: 1. Element A pure substance that can not be broken down into simpler substances. E.g. Oxygen gas, iron, diamond (pure carbon) 2. Compound A pure substance that is made up of two or more different elements in fixed proportions. E.g. Carbon dioxide has 1 atom of carbon for every 2 atoms of oxygen. 3

4 Pure Substances Most pure substances are compounds. E.g. water, stainless steel, wood 4

5 Chemical Properties p.173 Elements and compounds have a number of properties that make it possible to tell them apart. Physical property A characteristic of a substance. E.g. colour, state at room temperature, melting point. Chemical property Something you see when a substance changes to a new substance. 5

6 Chemical Properties Chemical properties are observable when two substances are mixed or reacted. E.g. When acid is mixed with baking soda a gas is produced. Chemical properties include a change in colour, odor, or solubility. *Combustibility *Reactivity 6

7 Questions What are the chemical and physical properties of iron? Water? 7

8 The Periodic Table There are about 109 different elements. These elements can be grouped together based on similar characteristics. E.g. gases can be grouped together. The grouping chemists use is called the periodic table of elements. One important feature of this table is the staircase line on the right. This separates metals (on the left) from non metals (on the right). Note that the large rectangle of elements on the bottom are also metals. 8

9 9

10 Organization of the table! 10

11 Question Is gold a metal or non metal? Is sulfur a metal or non metal? Is calcium a metal or non metal? 11

12 The Periodic Table Every atom is made up of protons (+), electrons ( ) and neutrons (neutral) Each element has two numbers. The top one is called the atomic number of the element. E.g. the atomic number of oxygen is 8. * atomic # = the number of protons and electrons The bottom number is the mass for each element atomic mass. E.g. the mass of oxygen is g/mol The number of nutrons = Atomic mass atomic # 12

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14 What is the atomic number, atomic mass, protons, electrons and neutrons for: Sodium Helium 14

15 The Periodic Table Because one atom of an element is very small, it would be hard to measure out just one atom. Therefore chemists use a set number of atoms when talking about the mass of an element. That number is the mole. The mole is big x One mole of oxygen is grams, which is much easier to measure out than a single atom of oxygen. (This is how we get the atomic mass) 15

16 Mass of compounds You can also calculate the mass of a compound using the peridic table State how many atoms and elements are in each of the following compounds: #Atoms H 2 O #ElementsWeight CO 2 H 2 O 2 CH 3 COOH Fe 16

17 Question How much does one mole of carbon weigh? How much does one mole of chlorine weigh? How much does CO2 weigh? How much does 2(NO4) weigh? 17

18 Types of Compounds Chemical compounds all have their own special properties. Based on these properties, compounds can be divided into 3 major groups: 1. Metallic compounds 2. Molecular compounds 3. Ionic compounds 18

19 1. Metallic compounds Compounds made by metal elements Properties of metals include: Shiny Conduct electricity Can be easily bent into new shapes Are solid at room temperature Dissolve in water ph = 7 Some examples are: FeCo (magnetic) Ag 3 Sn (in fillings) 19

20 2. Molecular compounds Compounds made by non metal elements Properties of molecules include: Do not conduct electricity Are solids, liquids or gases at room temperature If solid, they are white powders Some dissolve in water ph = 7 Some examples are: Sugar Water Oxygen gas 20

21 3. Ionic compounds Compounds made by metal and non metal elements Properties of ions include: Conduct electricity when dissolved in water Are solid crystals at room temperature Solids can be different colours ph = 1 14 Some examples are: NaCl (Table salt) Acetic Acid (Vinegar) Na 2 CO 3 (Baking Powder) 21

22 22

23 Ionic Compounds p Molecular compounds are made of non metal atoms that form covalent bonds. Metal and non metal atoms do not form covalent bonds. Instead they form ionic bonds. Ionic bonds exist between two or more charged atoms. The charge can be either positive or negative. An ionic compound is formed when the total charge on all the ions is zero. 23

24 Ionic Compounds E.g. Na + can form an ionic compound with Cl. The resultant solid crystal is called sodium chloride (table salt). Naming ionic compounds is easy. There is no change to the first ion name. The second ion will end in "ide," "ate," or "ite." The positive ion is written first and the negative ion, second. E.g. KF is potassium fluoride, not fluoride potassium. 24

25 Ionic Compounds In addition, there are no special prefixes used when there is more than one of the same ion present. E.g. AlI 3 is aluminum iodide, not aluminum triodide. 25

26 Polyatomic ions Some atoms like to stay together, and do not come apart Polyatomic compounds: are groups of atoms that tend to stay together and carry an overall ionic charge Eg. Nitrate ion: NO 3 These ions end with ite or ate Ionic compound: Metal + Non metal Polyotomic ions: Metal + Molecule ex: Na + NO3 = NaNO3 NaNO3 Some would call it: Sodium Nitrogen Oxide > WRONG Almost all compound have only 2 names So recieves a polyotomic name Sodium Nitrate 26

27 Polyatomic ion infosheet 27

28 Formulas for polyatomic ions Polyatomic ions will often exist in brackets Eg. Mg(OH) 2 If there are more than three atoms in a compound, it likely has a polyatomic ion Eg.CuSO 4 28

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31 Writing Formulas for Ionic Compounds Finding the formula is a little more complicated than naming ionic compounds Steps: Use the periodic table to find the two ions One will be positive ion (metal) and one negative ion(non metal) The overall charge of the compound must be neutral (zero charge). the overall positive charge must be equal to the overall negative charge. E.g. 1 Na + needs 1 Cl to be balanced, making NaCl. 31

32 Criss Cross method We can also use the criss cross method: Find the ions Bring the charge of the first ion down to the second and the charge of the second down to the first (Criss cross) Then check to see if they are in simplest form 32

33 Eg: 33

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35 Ionic compounds continued Look at iron on your periodic table of ions It has two ion options: It can be Fe 3+ or Fe 2+ When naming a compound that can be made of either ion we distinguish the ion used with a roman numeral. If Fe 3+ is used we would say: Iron(III) If Fe 2+ is used we would say: Iron(II) Iron (III) Bromide would be: Fe 3+ and Br Which would become: FeBr 3 Roman Numerals: 1 I 2 II 3 III 4 IV 5 V 6 VI 35

36 36

37 Naming Hydrates Sometimes compounds have molecules of water associated with them. This is called a hydrate Water is given a prefix based on the number of water molecules present. E.g. MgO 5H 2 O is magnesium oxide pentahydratẹ 37

38 Acids and Bases Acids and bases are special types of ionic compounds. Acids Compounds that dissolve in water to produce a hydrogen ion. E.g. HCl in water becomes H + and Cl The properties of acids include: Taste sour Conduct electricity Turn blue litmus paper red Use the unique state aqueous (aq) 38

39 Acids Acids can usually be identified by having a hydrogen atom at the beginning of the compound. E.g. HF, HCH 3 COO, H 2 SO 4 However some must just be memorized, as is the case with any compound containing the carbonate ion. E.g. CaCO 3 or Na 2 CO 3 39

40 Naming Acids There is a special way to name acids. 1. Name the compound as if it were an ionic compound. 2. Based on the ending of the ionic name rewrite the compound. if it ends in... name it... EndingNew compound ide hydro ic acid ate ic acid ite ous acid E.g. HCl Hydrogen chloride becomes hydrochloric acid. E.g. HClO 2 Hydrogen chlorite becomes chlorous acid. ***Specials*** 3. If the acid involves phosphorus, we keep the or. E.g. H 3 PO 4 is phosphoric acid, not phosphic acid. 4. If the acid involves sulfur, we keep the ur. E.g. H 2 SO 4 is sulfuric acid, not sulfic acid. 40

41 Bases are: Bases p Ionic compounds that dissolve in water to produce hydroxide (OH ) ion. E.g. NaOH in water gives Na + + OH 2. Ionic compounds that can accept a hydrogen ion. E.g. NH 3 + H 2 O NH OH Here NH 3 is a base. Bases are named the same way other ions are. E.g. NaOH is sodium hydroxide. 41

42 Bases Bases can usually be identified with an OH (hydroxide) group at the end. E.g NaOH, KOH, Ca(OH) 2 However some must be memorized, like ammonia (NH 3 ). The properties of bases include: Taste bitter Conduct electricity Turn red litmus paper blue Feel slippery 42

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46 Types of Chemical Reactions Chemical reactions When chemicals are mixed and produce new chemicals. The chemicals you start with are called reactants. The new chemicals produced are called products. Reactant + Reactant > Product(s) 46

47 Types of Chemical Reactions There are 7 types of chemical reactions we will deal with. For each there is a skeletal form. Eventually you will be able to complete chemical reactions when given word equations or the chemical symbols. 47

48 7 Types of Reactions We will say: E = element (Cu, C, F ect) C = compound (CuO 4, H 2 O, ec) 1. Synthesis Two atoms react to produce a compound. Skeletal form: E + E C or A + B > AB E.g. 4 Al + 3 O 2 > 2 Al 2 O 3 48

49 7 Types of Reactions 2. Decomposition A compound breaks apart into two elements. Skeletal form: C > E + E or AB A + B E.g. 2 NI3 > N2 + 3 I2 49

50 7 Types of Reactions 3. Single Displacement A compound and element react to produce a new compound and new element. Skeletal form: E + C > C + E or AB + C CB + A E.g. 2 AuI + Br 2 > 2 AuBr + I 2 50

51 7 Types of Reactions 4. Double Displacement Two compounds react to produce two new compounds. Skeletal form: C + C > C + C or AB + CD AD + CB E.g. 2 Fr2(SiO3) + GeCl4 > 4 FrCl + Ge(SiO3)2 51

52 7 Types of Reactions 5. Neutralization When an acid and a base are combined the resulting solution is neutral. This reaction produces water and a salt (ionic compound that is not an acid nor a base). Skeletal form: C + C > C + C (same as d displacemen But: Acid + Base Water + Salt E.g. HCl + Na(OH) > H(OH) + NaCl 52

53 7 Types of Reactions 6. Complete Combustion Burning compounds that are made of carbon and hydrogen. The only reaction to have an element and compound form two compunds Skeletal form: E + C > C + C or: Hydrocarbon + oxygen gas Carbon dioxide + water E.g. 2 C 12 H O 2 24 CO H 2 O The only thing that ever changes are the numbers of C and H 53

54 7 Types of Reactions 7. Incomplete Combustion p. 237 Similar to complete combustion except carbon monoxide is created because there is not enough oxygen. E.g. C 8 H O 2 6 CO H 2 O + CO + C 54

55 Chemical Reactions Chemical reactions can also be very helpful in the real world be releasing or absorbing heat Gasoline + O 2 > CO 2 + H heat Exothermic reaction: a reaction that releases energy Water (s) + Heat > Water (L) *actually a physical change Endothermic reaction: a reaction that absorbs energy 55

56 Chemical Reactions A chemical reaction is are used in every life situation from brushing your teeth to riding on a skidoo. Evidence of a chemical reaction: 1) formation of a gas from two liquids or a liquid and a solid. 2) formation of a solid (precipitate) from two liquids or a gas and a liquid. 3) unexpected color change. For example, mixing two colorless liquids and obtaining a color (not blue and yellow making green) 4) dissolving an insoluble solid (precipitate) in a solution. Note, the solution's solvent in this case will not dissolve the solid by itself. (what is added causes the reaction) * heat, and light are also good indications! 56

57 Balancing Chemical Reactions A chemical reaction is written like a math equation. Instead of an equal sign there is an arrow. Law of conservation of mass: In a chemical reaction, the total mass of the reactants is equal to the total mass of the products mass reactants = mass products We have to make sure that there are the exact same number of atoms on both sides of the arrow. 57

58 Balancing Chemical Reactions How many atoms of each element are present? Fe O 2 2 O 2 H 2 O 3 H 2 O Ca(OH) 2 Mg(NO 3 ) 2 2 Mg(NO 3 ) 2 # of atoms 58

59 Balancing Chemical Reactions E.g. When you put an electrical current through water, it can be decomposed into hydrogen and oxygen gas. H 2 O H 2 + O 2 We can t keep the reaction like this because both sides are not equal. Left Right 2 H 2 H 1 O 2 O So we need to put a 2 in front of the H 2 O That changes the number of Hydrogens so we have to balance them as well. H 2 O H 2 + O 2 59

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62 Strategy for balancing a combustion reaction Naming: Odd Hydrocarbon number - has a 1, 3, 5, 7, etc in it Always balance C first H second and O last! C 3 H 8 + O 2 > CO 2 + H 2 O balance the carbon atoms C 3 H 8 + O 2 > 3 CO 2 + H 2 O balance the hydrogen C 3 H 8 + O 2 > 3 CO H 2 O balance the the oxygen C 3 H O 2 > 3 CO H 2 O Balancing combustion reactions with an EVEN number of carbons. C 2 H 6 + O 2 > CO 2 + H 2 O place a 2 in front of the C 2 H 6 2 C 2 H 6 + O 2 > CO 2 + H 2 O Now balance the carbon 2 C 2 H 6 + O 2 > 4 CO 2 + H 2 O Balance the hydrogen 2 C 2 H 6 + O 2 > 4 CO H 2 O balance the oxygen 2 C 2 H O 2 > 4 CO H 2 O Done! 62

63 Predicting States In addition to balancing equations, you also will have to predict the states of the reactants and products. The state can be solid (s), liquid (l), gas (g), or aqueus (aq) which means dissolved in water. The elements or compounds we use will be at sea level and room temperature. We have to specify this because if the pressure or temperature changes, so can the state. 63

64 Predicting States In order to predict the state (at room temperature) of a particular chemical we must follow these rules: 1. Molecules States must be learned from experience. 2. Elements States can be determined from the periodic table (i.e. Hg, (l) group VIIA). 3. Hydrocarbons The state will be given in the reaction. 64

65 Predicting States 4. Acids All are aqueous (aq). 5. Bases Same state as if they were ions. 6. Ionic When used in synthesis or decomposition reactions, ions are always solids (s). 7. Ionic When used in single or double displacement reactions, we must use the solubility table. Solubility Table 65

66 Overall Predicting states 1. Molecules 2. Elements 3. Hydrocarbons 4. Acids 5. Bases 6. Ionic (Synthesis & Decomposition) 7. Ionic (Single & Double Displacement) 66

67 Solubility Table Try this: 67

68 Predicting Products Remember chemical reactions all look like this: Reactants Products If you look at each type of chemical reaction we use, you will notice each has unique reactants. Therefore we can predict what products will be made when we are given just the reactants. 68

69 1. Neutralization Skeletal form: Acid + Base Water + Salt E.g. HCl + NaOH 69

70 2. Synthesis Skeletal form: E + E C E.g. Al + O 2 70

71 3. Decomposition Skeletal form: C E + E E.g. NI 3 71

72 4. Single Displacement (Replacement) Skeletal form: C + E C + E E.g. AuI + Br 2 72

73 5. Double Displacement (Replacement) Skeletal form: C + C C + C Fr 2 (SiO 3 ) + GeCl 4 73

74 6. Complete Combustion Skeletal form: Hydrocarbon + oxygen gas Carbon dioxide gas + water vapor E.g. C 12 H 26 + O 2 74

75 Attachments 1206Attendance.xlsx

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