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Science 10 Unit A: A1.1 Unit A: Energy and Matter in Chemical Change Energy and Matter in Chemical Change Introduction Read pages: 6-11 WHMIS o Workplace Hazardous Materials Information System o There are three components to the WHMIS system: ___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________ WHMIS Symbols: 1 Science 10 A1.2 Unit A: Energy and Matter in Chemical Change Properties and classification of matter Read pages: 12-17 Physical Properties Describe the physical appearance and composition of a substance: They include: Chemical Properties Describe how a substance will react chemically with another substance. They include: Pure Substance Are only made up of one type of particle, all particles are identical. Elements ____________________________________________________________________________ Are listed on the periodic table. Eg. _________________________________________________________ Compounds ____________________________________________________________________________ Eg. CO2 – carbon dioxide ___________________________ _______________________________ 2 Science 10 Unit A: Energy and Matter in Chemical Change Mixtures _______________________________________________________________________________________ _______________________________________________________________________________________ Solution Is uniform throughout, cannot see the different particles. Eg. ____________________________________________________________________ Mechanical Mixture You can see the different particles. Eg. ____________________________________________________________________ Suspension Is a mixture when the particles have different states. Eg. ____________________________________________________________________ Colloid Is like a suspension but it is not easy to separate the parts. Eg. ____________________________________________________________________ 3 Science 10 Unit A: Energy and Matter in Chemical Change Chemical Reactions The following are signs that a chemical reaction has occurred: 1. 2. 3. 4. 5. Assignment: Check and Reflect Page 17: Questions 1 - 9 4 Science 10 Unit A: Energy and Matter in Chemical Change Student Worksheet: Classification of Matter 5 Science 10 A1.3 Unit A: Energy and Matter in Chemical Change 6 Atomic Models Read pages: 18-25 Aristotle [400 BC – 1500 AD] Thought that all matter is made up of only four elements: o ___________________________________________________ o all of matter is some combination of these four elements Alchemy [1500 AD] In the 1500’s many scientists were________________________________________________ ________________________________________________________________________________________ While they were not able to create gold they did discover many useful properties of matter such as: o density o boiling point o melting point o separation techniques Dalton [1766-1844] Developed the _____________________________________________________________ o All matter is made up of tiny particles called atoms. o The atom is the smallest particle of matter and cannot be divided. o The atoms of an element are all identical in size and mass. o Atoms of different elements have different properties. o Different atoms combine together in specific ratios to form new substances. Eg H2O Science 10 Unit A: Energy and Matter in Chemical Change 7 JJ Thomson [1890s] Developed the ____________________________________________ o Studied the properties of cathode rays. o Discovered the electron. o Within the atom there exists tiny negative particles called electrons, the rest of the atom is a positive fluid sphere. Ernest Rutherford [1908] Rutherford did the gold foil scattering experiment. _________________________________________________ o The atom has a small positive, dense nucleus. o Most of the matter is found in the nucleus. o The negative electrons orbit the nucleus like planets orbit the sun. Neils Bohr Bohr studied the bright lines in the visible spectrum of hydrogen. Bohr created a theory where ___________________________________________________ __________________________________________________________ o Electrons can occupy only specific orbits. o Each orbital can only hold a certain number of electrons. o For an electron to occupy an orbital it must has a specific amount of energy (energy level). Quantum Mechanical In today’s model of the atom ___________________________________________________ ___________________________________ o We have the greatest probability of locating electrons in certain regions around the atom. o Depending on how many electrons an atom has and which energy level the electron is in then that electron can be found in a certain cloud formation. o The electron can exist as a particle and as a wave at the same time. Check and Reflect: 4 – 8 A1.R Section 1 Review page 25 page 27 Science 10 A2.1 Unit A: Energy and Matter in Chemical Change Atomic Structure Read pages 28-38 Elements Are made up of only one type of atom. Metals Properties include: Non-metals Properties include: Metalloids Properties include: 8 Science 10 Unit A: Energy and Matter in Chemical Change 9 The Period Table All of the elements have been organized onto the periodic table of elements. The elements are organized into rows and columns _____________________________ _________________________________________________________________________________________ Groups Elements are placed into _________________________________________. Elements in the same group/family have the same physical and chemical properties. i. ____________________________________ - Group IA - Very reactive metals - Li, Na, K, Rb, Cs, Fr ii. _____________________________________ - Group IIA - Reactive metals - Be, Mg, Ca, Sr, Ba, Ra iii. _____________________________________ - Group VIIA - Very reactive non-metals - F, Cl, Br, I, At iv. _____________________________________ - Group VIIIA - These elements are non-reactive - They do not form ions or compounds - He, Ne, Ar, Kr, Xe, Rn Periods Elements are placed into rows. Elements in the same row all have the same number of orbits and energy levels. Eg. Li, Be, B, C, N, O, F, Ne Science 10 Unit A: Energy and Matter in Chemical Change 10 Subatomic Particles The atom is made up of three types of subatomic particles: Particle Proton Neutron electron Symbol Charge Mass 1.67 x 10-27 kg 1.67 x 10-27 kg 9.11 x 10-31 kg Location atomic mass number atomic number 52.00 24 Cr Atomic Mass Number ____________________________________________________________. Is the mass of 1 mole of atoms. Atomic Number ____________________________________________________________. The number of electrons is equal to the number of protons in one atom. Example: Chromium Protons: Electrons: Neutrons: ___________ ___________ ____________________ Ru _______________ _______________ _______________________ Science 10 Unit A: Energy and Matter in Chemical Change 11 Formation of Ions Atoms of the same element will always have the same number of protons. When an atom _________________________________________ it will become an ion. Metals Will form _________________________________ They _____________________________________ electrons from the outer orbit Non-metals Will form _____________________________ They _______________________________ to gain extra electrons Science 10 Unit A: Energy and Matter in Chemical Change 12 Octet Rule o Atoms strive to have _______________________ in their outermost orbit. o Atoms will give away or steal electrons until it has a complete and stable outer orbital. o The number of electrons in the outer orbital is called ___________________ _________________________________ o The number of electrons an atom will gain or lose to reach a stable orbit is called the _______________________________. o Example: o Sodium Valance electrons: _________ valance number: ___________________________ ion: _______________ o Chlorine Valance electrons: _________ Valance number: ___________________________ Ion: _________________ Lewis Dot Structures o A Lewis diagram is a model where the valance electrons are drawn as dots around the atom. o This model shows ___________________________________________________________ ________________________________________________________________________________ o Examples: o Science 10 Unit A: Energy and Matter in Chemical Change 13 How Ions Form Compounds o When atoms combine to form an ionic compound the _______________________ _____________________________________________________________________________________ o One ion will become positive and the other ion will become negative. o Each atom ends up with a complete outer orbit with 8 electrons each. Examples: 1. Complete the following for each atom Atom Atomic Number 1st orbit 2nd orbit 3rd orbit Valance # Ion Na N Cl 2. For each of the following draw the Lewis dot structure and write the atom as an ion: a. Li b. S Check and Reflect: 1 – 12 page 39 Science 10 A2.2 Unit A: Energy and Matter in Chemical Change 14 Naming Ionic and Molecular Compounds Read pages: 40-49 Ionic Compounds o An ionic compound is formed when ___________________________________________ _____________________________________________________________________________________ o An ionic compound is formed because the metal ion becomes positive and the non-metal ion becomes negative so they _________________________________ ____________________________. Ionic Compound Formulas o For two atoms to form an ionic compound there must be __________________ _____________________________ between the negative ions and the positive ions. 1. Write the correct formula for the ionic compound. a. Li F b. Ca 2 Cl c. K O2 d. Al 3 S 2 Science 10 Unit A: Energy and Matter in Chemical Change Naming Ionic Compounds o {metal} {non-metal} + “ide” o Example: o Sodium + chlorine ______________________________ 2. Name each compound above in #1. 3. Write the formula given the name a. lithium oxide b. strontium chloride Assignment: Worksheet A2.2: Ionic Compounds Worksheet #1 - simple ionic compounds Multivalent Elements o Some metals have the ability to form __________________________________________ ________________________________. o These elements are usually the transitional-earth metals. o Examples: o Iron (II): Fe2+, iron (III): Fe3+ o Copper (I): Cu+, Copper (II): Cu2+ 4. Write the equation for each of the following a. Iron (III) oxide b. Copper (II) bromide 5. Given the formula write the correct chemical name: a. CrO b. Co2S3 15 Science 10 Unit A: Energy and Matter in Chemical Change 16 Polyatomic Ions o A polyatomic ion is made up of ______________________________________. o Polyatomic ions can combine in ______________________________. o Suffixes “ite” has fewer atoms of an atom “ate” has more atoms of an element Sulfite: ___________ Sulfate: ___________ o Compounds containing polyatomic ions follow the same balancing rules as all other ionic compounds. o Naming polyatomic compounds: {metal} + {polyatomic ion} the name of the polyatomic ion does not change (it has been married once already) Example: Calcium carbonate 1. Write the correct chemical formula for the following: a. sodium sulfite b. magnesium nitrate c. ammonium sulfide Assignment: Ionic Compounds Worksheet #2 Science 10 Unit A: Energy and Matter in Chemical Change 17 Molecular Compounds o A molecular compound is created when _________________________________________ __________________________________. o When non-metal atoms form molecules they must ______________________________, they form _________________________________. By sharing electrons the outer orbits still have _______________________________. o Science 10 Unit A: Energy and Matter in Chemical Change 18 o Because non-metals atoms ______________________________ the same two elements they ________________________________________ (we cannot predict the ratio in a molecular compound) o To name molecular compounds we use a prefix system for naming. o Examples: a. SO, ______________________________ b. SO2, ______________________________ c. SO3, ____________________________________________________________ d. SO4, ____________________________________________________________ e. P3O5, ____________________________________________________________ o A number of molecular compounds have common names: Name Formula H2O(l) CO2(g) C6H12O6(s) C12H22O11(s) CH4(g) NH3(g) H2O2(l) C3H8(g) Molecular elements o Many of the non-metal elements exist in molecular form: Element Formula Hydrogen Nitrogen Oxygen Fluorine Chloride Bromine Iodine Phosphorus Sulfur Ozone Assignment: Molecular Compounds Worksheet #2 Check and Reflect: 1 – 11 page 50 Science 10 A2.3 Unit A: Energy and Matter in Chemical Change 19 Properties of Ionic and Molecular Compounds Read pages 51-60 Properties of ionic compounds o o o o o o o o o an ionic compound is also referred to as “a salt” Solubility of Ionic Compounds o some ionic compounds are more soluble than others o a substance that dissolves well is considered very soluble o an ionic compound that is soluble in a solution is written as ___________________, a an ionic compound that is not soluble will be written as ______________________ Solubility Table Ion Very Soluble Group 1 NH4+ H3O+ (H+) All Slightly None Soluble ClO3- CH3COONO3ClO4- ClBrI- SO42- S2- OH- PO43SO32CO32- All Most Most Most Only with: Group 1 Group 2 NH4+ Only with: Group 1 NH4+ None Only with: Ag+ Hg+ Only with: Ag+ Pb2+ Hg+ Cu+ Tl+ Only with: Ca2+ Sr2+ Ba2+ Ra2+ Pb2+ Ag+ Most Only with: Group 1 NH4+ Sr2+ Ba2+ Tl+ Most Most Science 10 Unit A: Energy and Matter in Chemical Change 20 Examples: 1. Which of the following compounds will most likely dissolve in water? a. NaNH4 b. LiCl c. CaS d. KOH e. AgCl f. CaSO4 g. Cu(OH)2 Properties of Molecular Compounds o Molecular compounds are compounds made up of ___________________________ _____________________________________________ o The non-metal atoms are held together by ________________________________, the atoms share electrons which make a _____________________________________. o The attraction between neighboring molecules is weak so ___________________ __________________________________________ o Molecular compounds can also make crystalline structures that crumble easily. o Molecular compounds _______________________________________________ because they are made up of non-metal atoms. Special Properties of Water o ______________________________________, one side is slightly positive and the other side is slightly negative. o The molecules form an electrostatic attraction to each other. o Water has the following properties: _________________________, water molecules are attracted to other water molecules _________________________, water molecules are attracted to other molecules _________________________________, because of cohesion water makes a strong surface force _________________________________, water can crawl up a straw or edge of a container because of adhesion Conducts heat __________________________________ Specific heat capacity Science 10 Unit A: Energy and Matter in Chemical Change 21 Phases of Water (Ice) o Ice (solid) is less dense than the liquid form of water because of the molecular formation of water, ordered molecular structure o _________________________________________________________________________________ __________________________________________ o Water (lakes) freezes from the top down. Assignment: Check and Reflect: 1 – 9 Page 61 Science 10 A2.4 Unit A: Energy and Matter in Chemical Change 22 Acids and Bases Read pages 62-68 Properties of Acids o o o o o o Properties of Bases o o o o o o ph Scale o pH is an indication of the ________________________________________ in a solution o the higher the concentration of H+ ions the stronger the acid, the higher the pH acids: _________________ neutral _________________ bases: _________________ Science 10 Unit A: Energy and Matter in Chemical Change 23 Indicators o an acid-base indicator is a chemical that is used to determine if a solution is ________________________________________ o an indicator ________________________________________________________________________ o different indicators will change colour for different pH ranges: o universal indicator is a mixture of several indicators that change colour as the pH changes to different ranges Naming Acids o acids are named based on the non-metal anion in the compound Anion “ide” “ite” “ate” Compound name Hydrogen (anion)-ide Hydrogen (anion)-ite Hydrogen (anion)-ate Acid name Hydro (anion)-ic acid (anion)-ic acid (anion)-ous acid Examples: Formula HS(aq) H2SO3(aq) H2SO4(aq) Compound Common Acid name Hydrogen sulfide Hydrogen sulfite Hydrogen sulfate IUPAC naming system for acids: [International Union of Pure and Applied Chemistry] Formula HS(aq) H2SO3(aq) H2SO4(aq) Compound IUPAC name Hydrogen sulfide Hydrogen sulfite Hydrogen sulfate 1. Name the following acids: a. H3N(aq) b. HNO2(aq) c. HNO3(aq) d. H3PO4(aq) Assignment: Worksheet – A2.4 Naming acids Science 10 Unit A: Energy and Matter in Chemical Change 24 Bases o Most bases contain an __________________________________ o Bases _____________________________________ because they react with oils and grease o Some common bases: Base NaOH(aq) NH4OH(aq) Mg(OH)2(aq) Name Common name Sodium hydroxide Ammonium hydroxide Magnesium hydroxide Use Acids and Bases in Your Body o Our bodies contain a variety of substances each substance has a specific pH: Saliva – 6.4 Blood – 7.35 Stomach – (1-2) Small intestine – 8.5 Large intestine – (5.5-7.0) Urine – 6.4 o It is important that our bodies maintain this pH balance o ______________________________, is a substance that helps to maintain a pH level in a solution, it resists change in pH Acids and Bases in the Home o acids and bases serve a variety of functions in our homes o some typical acids are: o _________________________________________________________________________ o some typical bases are: o _________________________________________________________________________ Science 10 Unit A: Energy and Matter in Chemical Change Neutralization o a type of chemical reaction where ______________________________________________ _____________________________________________________is called a neutralization o the products of a neutralization reaction are always: _____________+_______________--> ____________________+______________________ HClaq NaOH aq H 2Ol NaClaq o carbon dioxide is produced only when one of the compounds contain the carbonate molecule o eg vinegar + baking soda Assignment: Check & Reflect 25 Science 10 A2.5 Unit A: Energy and Matter in Chemical Change 26 Our Chemical Society Read pages: 70-75 Issues Related to Chemicals o some chemicals are hazardous because of: ____________________________________________________________ how they are produced ________________________________________________________________________________ their effect on the ecosystem Environmental Effects o some chemicals are harmful because of how they effect components within the environment o some harmful chemicals ____________________________________________________________ ____________________________________________ o CFC’s chlorofluorocarbons come from Freon used in __________________________________________________ can stay in the atmosphere for up to 50 years _________________________________________, the ozone helps to protect the Earth from harmful UV, and X-Rays from the sun o Greenhouse gases (________________________) most of the greenhouse gases come from the _____________________________ ______________________________ levels of greenhouse gases in our atmosphere are increasing the greenhouse gases are trapping in heat and the temperatures around the Earth are increasing o Acid Precipitation other products of the combustion of fossil fuels are ____________________ ________________________________________________________ particulates enter the Earth’s atmosphere and return in the form of _____________________________________________ ______________________________________________________________________________ _________________________________ Science 10 Unit A: Energy and Matter in Chemical Change 27 Health Concerns o Many people use chemical substances for recreational purposes o Some of these chemicals are ____________________________________________ o Some of these chemicals _____________________________________ o Alcohol (CH3CH2OH(l)) alcohol is considered a drug because of its effects on the body excessive amounts can __________________________________________________ ______________________________________________________________________ repeated use can lead to physical and psychological dependence, ______________________________________________ o Nicotine and tobacco products __________________________________________________________________________ The use of tobacco products have been related to high incidences of cancer Benzene o Benzene is a hazardous chemical that is both toxic and flammable o Many products are made using benzene ________________________________________________________________ o Benzene is a regulated chemical so there are strict regulations about its transportation and storage o Because of its toxic effects any ____________________________________________________ is hazardous Workers must take specific steps for protection, WHMIS Chemistry Related Careers o Because we use so many different chemicals there are many careers that involve chemistry: Chemical engineers Chemistry teachers ___________________________________________ ___________________________________________________________ Cosmetics Household product design o Almost each person works or interacts with chemicals everyday Food and cooking _____________________________________________ Gas and transportation _____________________________________________ Manufactured products A2.R Section 2 Review AQ.2 Quiz 2 pages 76-77 Science 10 A3.1 Unit A: Energy and Matter in Chemical Change Examples of Chemical Change Read pages: 79-85 During a chemical reaction a ___________________________________________________________ _____________________________________________________________ Example: Methane + oxygen water + carbon dioxide + (energy) ____________________ _______________________________ Showing States in a Chemical Formula o In some chemical reactions the products may be in the form of a _______________ or in the form of a ____________________________ o The symbol (aq) means that in solution the compound will ________________________________________. o In any chemical equation it is important that you show the state of each element or compound in the reaction o Examples CH 4(g) O2(g) H 2O(g) CO2(g) energy CaC2(s) H 2O(l ) Ca OH 2(s) C2 H 2(g) Which compounds are gases? Which compounds are solid? Which compounds are liquid? Which of these was an element? 28 Science 10 Unit A: Energy and Matter in Chemical Change 29 Energy Changes o ____________________________________________________________________________________ _________________________________________. Phase Change o When a substance changes state there is a characteristic change in energy that occurs. o In a pure substance the phase changes (_____________________________________________________________) o In a mixture there are a variety of phase changes. Exothermic Reaction o Release energy usually in the form of __________________________________ o The energy of the products is ____________________ than the energy of the reactants. (______________________________________________________________) o Example: CH 4(g) O2(g) H 2O(g) CO2(g) energy Endothermic Reaction o Energy is absorbed from the surrounding environment, usually __________________________________________________________________ o The energy of the products is________________________ than the energy of the reactants. (___________________________________________________) o Example: Ba OH 2(s) NH 4 SCN Ba SCN 2(aq) NH 4OH(aq) Biochemical Reactions o Two important biochemical reactions are: o Cellular Respiration This is how living organisms (cells) get energy from glucose. Is an __________________________________________. o Photosynthesis This is how plants get energy from the sun. Is an ___________________________________________. Science 10 Unit A: Energy and Matter in Chemical Change 30 Evidence of a Chemical Reaction o In all chemical reactions a new substance is produced that has its own characteristic properties. o Indicators of a chemical change: Conservation of Mass o Mass is conserved in all chemical reactions. o In all chemical reactions ______________________________________________________ the mass of the reactants. o Example: o 2AgNO3(aq) Cu(s) Cu NO3 2(aq) 2Ag(s ) (33.98g) Assignment (6.36g) (______________) Check and Reflect: 1 – 11 (21.57g) P. 85 Science 10 A3.2 Unit A: Energy and Matter in Chemical Change 31 Writing Chemical Equations Read pages: 86-89 Chemical Equations o a word equation describes the reactants and products of a chemical reaction ____________________________ o a chemical equation _______________________________________________________________ to identify the reactants and products in a chemical reaction o a chemical equation is more useful because: o _____________________________________________________________________________ o _____________________________________________________________ Example: Word equation Silver nitrate + copper copper nitrate + silver Chemical equation Practice: Write the following as a chemical equation: 1. potassium + oxygen potassium oxide 2. scandium + nitrite scandium nitrite 3. sulfur + oxygen sulfate Worksheet: A3.2 Writing chemical equations Science 10 Unit A: Energy and Matter in Chemical Change 32 Balancing Chemical Equations o in all chemical reactions mass is conserved so we ______________________________ _____________________________________ for each element in the reactants and in the products o it is important that we balance any chemical equation that we write Examples: Balance each of the following chemical equations a. Na(s) + b. H2(g) + O2(g) c. N2(g) + H2(g) d. Na(s) + H2O(l) NaOH(aq) + e. CH4(g) + O2(g) H2O(g) + f. Pb(s) + NaCl(s) H2O(l) NH3(g) H3PO4(aq) H2(g) + g. AgNO3(aq) + Worksheet Cl2(g) H2(g) CO2(g) Pb3(PO4)2(s) CuSO4(aq) Ag2SO4(s) + Cu(NO3)2(aq) A 3.2 Balancing Chemical Equations Check & reflect 6–9 p. 90 Science 10 A3.3 Unit A: Energy and Matter in Chemical Change 33 Five Common Chemical Reactions Read pages: 91-105 There are five common types of Chemical Reactions: I. Formation Reaction (Synthesis) o During a formation reaction two or more elements __________________________ _____________________________________________________ o A formation reaction is also referred to as a __________________________________. o Many formation reactions are ____________________________, that is heat is given off during the reaction. A + B AB Example: magnesium + oxygen magnesium oxide Practice: Complete the reaction by writing the product, write the chemical equation, then balance. 1. aluminum + chlorine 2. carbon + hydrogen methane Text: Practice problems: Skill Practice: 2, 3, 4 1, 2, 3 p. 92, 93 p. 93 Science 10 II. Unit A: Energy and Matter in Chemical Change 34 Decomposition o During a decomposition reaction __________________________________________ into its component elements. o Many decomposition reactions are ____________________________, that means that energy must be added to the reaction to break apart the existing chemical bonds. AB A + B Example: Water + energy (electricity) hydrogen + oxygen Practice: 1. calcium oxide 2. aluminum sulfide Text Practice problems: 5 p. 94 Science 10 III. Unit A: Energy and Matter in Chemical Change Hydrocarbon Combustion o During a combustion reaction a __________________________________________ _______________________________________________________________________________ _________________________________________________ o Combustion reactions are _________________________________. o The potential energy of the reactants is higher than the energy of the products so during the reaction heat energy was released. Example Methane + oxygen carbon dioxide + water + (energy) Practice: 1. propane C3H8(g) + oxygen 2. glucose + oxygen Text: Practice Problem: 6 p. 95 35 Science 10 Unit A: Energy and Matter in Chemical Change 36 Solubility of Ionic Compounds o some ionic compounds are more soluble than others o a ionic compound that ___________________________________________________________ _____________________________________________________________________________________ o an ionic compound that is soluble in a solution is written as __________________, a an ionic compound that is not soluble will be written as _____________________, it will form a ____________________________ Solubility Table Ion Very Soluble Slightly Soluble Group 1 NH4+ H 3O + (H+) All ClO3NO3ClO4- CH3COO- ClBrI- SO42- S2- OH- PO43SO32CO32- All Most Most Most Only with: Group 1 Group 2 NH4+ Only with: Group 1 NH4+ None None Only with: Ag+ Hg+ Only with: Ag+ Pb2+ Hg+ Cu+ Tl+ Only with: Ca2+ Sr2+ Ba2+ Ra2+ Pb2+ Ag+ Most Only with: Group 1 NH4+ Sr2+ Ba2+ Tl+ Most Most Examples: Which of the following compounds are very soluble and which are slightly soluble? a. NaNH4 b. LiCl c. CaS d. KOH e. AgCl f. CaSO4 g. Cu(OH)2 Science 10 IV. Unit A: Energy and Matter in Chemical Change 37 Single Replacement o During a single replacement reaction an ionic compound reacts with another element, the chemical bond in the compound breaks apart and then ______________________________________________ _______________________________________________________________ o The other two ions will have a ____________________________________ (bond) this is why they combine to form a different compound. A + BC B + AC D + BC C + BD Example: Sodium chloride + silver silver chloride + sodium Practice: Complete the word equation and predict the products. Write the appropriate chemical equation, indicate if a precipitate is formed. Balance the equation. 1. Lithium sulfate + calcium 2. Chlorine + copper I bromide Text: Skill practice: 1 – 4 p. 97 Science 10 V. Unit A: Energy and Matter in Chemical Change 38 Double Replacement o During a double replacement reaction two ionic compounds in a solution will combine and then _________________________________________________________ ___________________________________________________________________________________ o One pair of ions will have a _______________________________________ (bond) this is why a different compound is formed. o Quite often a _________________________________________ as a result of a double replacement reaction. AB(aq) + CD(aq) AD(s) + CB(aq) Example: sodium chloride + silver nitrate sodium nitrate + silver chloride Practice: Complete the word equation and predict the products. Write the appropriate chemical equation, indicate if a precipitate is formed. Balance the equation. 1. Text: Assignment: Potassium iodide + silver nitrate Practice problem: 9, 10, 11, 12 p. 100 – 105 Worksheet A 3.3 Reaction Types Check and Reflect: 1 – 8 p. 106 Science 10 A3.4 Unit A: Energy and Matter in Chemical Change The Mole 39 Read pages: 107-111 Avogadro’s Number o The quantity that chemists use to measure _______________________________________ is present in a sample is called the _______________________________ o The number of atoms or particles in one mole is Avogadro’s Number o 1 mole = ____________________________________ Atomic Mass o the atomic mass of an element is the mass of 1 mole of atoms of that element that is the mass of 6.02 x 1023 atoms. o For example: o 6.02 x 1023 atoms of Carbon weigh: __________________ o 6.02 x 1023 atoms of Oxygen weigh: __________________ Where did the atomic masses of all of the elements come from? o By looking at how atoms combine to form compounds scientists were able to find the atomic masses of all of the elements as they were _____________________ __________________________________________________. o Today’s periodic table is based on _____________________________________________ o After finding the atomic numbers and the atomic masses ____________________ then created the _______________________________________. Finding the Atomic Mass of a Compound o The atomic mass of 1 mole of a compound will be the sum of the atomic masses of each of the elements in the compound. o ________________________________________________________________________________________ o Example: what is the atomic mass of one mole of a. H2O(l): 2 H + 1 O = 2(1.01) + 1 (16.00) = 18.02 g/mol b. CO2(g) : c. Na3PO4(s): d. Ca(NO3)2(s): 1C+2O= Science 10 Unit A: Energy and Matter in Chemical Change Converting Moles to Grams (mass) mn M m n M Examples: m n M mass (g) moles molar mass Find the mass of a. 3 moles of NaCl(s) b. 2 Fe2SO4(s) c. 4.5 Zn(NO2)2(s) Converting Grams (mass) to Moles Examples: a. How many moles are there for each compound given the mass. 65.0 g of: NaOH(s) 1 mole: NaOH(s) = 40.00 g n Text: A3.R AR b. 348.75 g of: CoSO4(s) c. 880.10 g of: Cr(NO3)2(s) Practice Problems: 13 – 20 Check & Reflect: 1 – 11 Section Three Review Unit A Review m 60.0g 1.5 mol M 40.00g p . 108, 109 p. 112 p. 113 p. 117-121 40