Everything you can feel is made of atoms! Chemistry!

Transcription

1 Name: Block: Sc10 Veenstra Everything you can feel is made of atoms Chemistry That the difference between atoms, ions, and molecules is caused by the difference in their structure and components The classification of substances as acids, bases, and salts, based on their characteristics, name, and formula The difference between organic and inorganic compounds Chemical reactions and the Law of conservation of mass How the rate of reaction is affected Radioactivity using modern atomic theory Our inquire into Everything you can feel is made of atoms will help us better understand: Vocabulary acids, alpha particle, atomic number, atoms, bases, beta particle, Bohr diagrams, bromothymol blue,catalyst, combustion, compounds, concentration, conservation of mass, covalent bonding, daughter isotope, decomposition, electron, fission, fusion, gamma radiation, half-life, indigo carmine, inorganic, ionic bonding, ions, isotope,lewis diagrams, light, litmus paper, mass number, methyl orange, molecules, neutralization (acid-base), neutron, organic, parent isotope, phenolphthalein, polyatomic, proton,radioactive decay, salts, single and double replacement, surface area, symbolic equations, synthesis, valence electron Note: If you lose this package it is your responsibility to print out a new copy from Ms. Veenstra s webpage: 1 of 20

2 Chapter 4 Learning Goal B D A E Reference 1. I can demonstrate knowledge of the three subatomic particles, their properties, and their location within the atom 2. I can define and give examples of ionic bonding and covalent bonding 3. I can with reference to elements 1 to 20 on the periodic table, draw and interpret Bohr models, including protons, neutrons, and electrons, of atoms (neutral), ions (charged), molecules - covalent bonding (e.g., O2, CH4 4. I can draw and interpret Lewis diagrams showing single bonds for simple ionic compounds and covalent molecules, and distinguish between lone pairs and bonding pairs of electrons in molecules 5. I can use the periodic table and a list of ions (including polyatomic ions)to name and write chemical formulae for common ionic compounds, using appropriate terminology 6. I can convert names to formulae and formulae to names for covalent compounds, using prefixes up to deca Chapter 4.1 Chapter 4.1 Chapter 4.1 Chapter 4.1 Chapter 4.2 Chapter I can define and explain the law of conservation of mass Chapter I can represent chemical reactions and the conservation of atoms using molecular models 9. I can write and balance (using the lowest whole number coefficients) chemical equations from formulae, word equations, or descriptions of experiments My estimate based on quizzes and assignments: LG = Mark = % Chapter 4.3 Chapter 4.3 "#$%%$%#& '"(")*+$%#&,--*.+)$/0"1& 23".+)456& Does not demonstrate a basic understanding of concepts. Demonstrates a basic understanding of concepts. Assign by Ms. V LG = Mark = % Demonstrates a solid understanding of concepts. Test result: % Demonstrates a complete and deep understanding of concepts && "#$%%$%#& '"(")*+$%#&,--*.+)$/0"1& 23".+)456& 72992:&;:,'2&& "#"$" %&""#""%" %'""#""(&""#""(""#""('" )"&""#")""#"")'" <2:=2>9,;2&& *" +*",-" --".*".-" /*" /-" 0*" 0-" 1*" 1-" 2**" 2 of 20

3 PART I: ATOM SCREEN Chapter 4.1 Atomic Theory Lab 4.1: Building an Atom (PhET simulation) 1. Go to the website: phet.colorado.edu. Click on HTML5 simulations on top right of screen and choose the Build an Atom simulation ( simulation/build-an-atom) 2. Explore the Build an Atom simulation with your group. As you explore, talk about what you find. List two things your group observed in the simulation. a. b. 2. Click on the + sign for each of the boxes (element name, net charge and mass number) to view changes as you change the number of particles in the atom. 3. What particle(s) are found in the centre of the atom? 4. Play until you discover which particle(s) determine(s) the name of the element you build. 5. What is the name of the following atoms? a. An atom with 3 protons and 4 neutrons: b. An atom with 2 protons and 4 neutrons: c. An atom with 4 protons and 4 neutrons: 6. Play with the simulation to discover which particles affect the charge of an atom or ion. 7. Fill in the blanks below to show your results: a. Neutral atoms have the same number of protons and electrons. b. Positive ions have protons than electrons. c. Negative ions have protons than electrons. 3 of 20

4 8. Develop a relationship (in the form of a single sentence or equation) that can predict the charge of the atom/ion based on the number and types of particle. 9. Play with the simulation to discover what affects the mass number of your atom or ion. a. What is a rule for determining the mass number of an atom or ion? 10. Fill in the blanks below to show your understanding of charge and mass: a. Protons have a mass of amu and a charge of. b. Neutrons have a mass of amu and a charge of. c. Electrons have a mass of nearly amu and a charge of. 11. Practice applying your understanding by playing 1 st and 2 nd levels on the game screen. PART II: SYMBOL SCREEN 1. Using the Symbol readout box, figure out which particles affect each component of the atomic symbol and how the value of the numbers is determined. d ca b Position in symbol box Term to describe this information Particle used to determine this a Element symbol protons How the value is determined # of p will identify the element b c d Ion charge Atomic number Mass number 3. Practice applying your understanding by playing the 3 rd and 4 th game levels. Play until you can get all the questions correct on the 4 th level. Fill in the information here for your last screen of the 4 th game level: protons neutrons electrons Finish Worksheet 4.1 Atomic Theory 4 of 20

5 Chapter 4.1 Bohr Models Notes Electron shells (orbitals, E levels) 1st shell holds only Valence shell: 2nd shell hold 3rd shell holds Valence electrons: 4th shell holds Example: Sodium Atom Shortcomings of model? Advantages of model? Stable: Unstable: Atoms will tend to gain or lose e- in order to become stable ION vs ATOM IMPORTANT NOTE: Protons are locked in the nucleus so the positive charge can t change...positive ions come from atoms that have lost e-, NOT from gaining protons Example Single e - in valence shell Unstable gain 7 or lose 1 e -? 5 of 20

6 4.1 Bohr Model Compounds Notes Forming Compounds Atoms wants to be stable (have a full valence shell). Atoms can become stable by 1. - metals tend to and become (called ) - non-metals tend to and become (called ) 2. A. Ionic Compounds Ionic bonds are formed between positive ions and negative ions. Generally, this is a metal (+) and a non-metal (-) ion. For example, lithium and oxygen form an ionic bond in the compound Li 2 O. Covalent Compounds Covalent bonds are formed between two or more non-metals. Electrons are shared between atoms. For example, hydrogen and fluoride form a covalent bond in the compound HF. Ionic vs. Covalent NOTE: Metals are found 6 of 20

7 Lewis Structures 4.1 Lewis diagram Notes Lewis diagrams illustrate chemical bonding by showing only an atom s valence electrons and the chemical symbol. Example Draw Lewis structure for Ca, a chlorine ion and a beryllium ion. NOTE: Square brackets are placed around each ion and the charge is added outside the bracket. Ionic Compounds Beryllium and chlorine can form an ionic compound: Let s try CaO: Covalent Compounds Lewis diagrams can also represent covalent bonds. The shared pairs of electrons are usually drawn as a straight line. Example: HF H2O Bonding e - : Lone pairs: 7 of 20

8 4.2 Type I Ionic Compounds (metal + non-metal) - contain a metal and a nonmetal - the metal that is present only forms one type of cation (only one charge in the periodic table). - Both the metal and the non-metal form ions, which is why it is called an ionic compound. 1) From the following list, cross out those compounds that do NOT belong in the category for Type I binary ionic compounds. NaCl FeCl2 CaCl2 TiO2 MgO AlBr3 KCl K2S BeF2 Cu2O3 AgCl Zn3N2 Formula and name examples for Type I ionic compounds: KI = potassium iodide BaO = barium oxide ZnF2 = zinc fluoride Na2S = sodium sulfide Ag3N = silver nitride BeCl2 = beryllium chloride 2) What type of element is always listed first (metal or nonmetal)? second? 3) Is the name of the first element in the compound different from the element? (yes/no) 4) What is the common ending for all the names? 5) In zinc fluoride, there are 2 fluoride atoms, are they indicated in the name? (yes/no) 6) What is the charge on the zinc ion? 7) What is the charge on the fluoride ion? 8) Why do you need one zinc ion and two fluoride ions for the formula for zinc fluoride? 9) Why do you need two sodium ions for every sulfide ion in sodium sulfide? 10) As a team, determine the rules for naming type I ionic compound when given the formula. 11) As a team, determine the rules for writing the formula for a type I ionic compound when given the name. 12) Name each of the type I ionic compounds listed in question 1. Finish Q on Worksheet 4.2 A + B 8 of 20

9 4.2 Type II Ionic Compounds (transition metal +non-metal) - contain a metal and a non-metal - the metal that is present here can form more than one type of cation (blank in the periodic table above) - both the metal and the nonmetal form ions, and it is still called an ionic compound. 1) From the following list, cross out those compounds that do NOT belong in the category for Type II ionic compounds. AlP FeCl2 Ag2O VBr5 CoS SnF2 K3N SrF2 CuBr AuCl3 ZnO HgS Formula and name examples for Type II ionic compounds: Fe2O3 = iron(iii) oxide FeO = iron(ii) oxide CuS = copper(ii) sulfide CuCl = copper(i) chloride MnO2 = manganese(iv) oxide MnCl2 = manganese(ii) chloride 2) What type of element is always listed first (metal or nonmetal)? second? 3) Is the name of the first element in the compound different from the element? (yes/no) 4) What is the common ending for the nonmetal portion of the names? 5) In the compound FeO, what is the charge on iron? 6) In the compound Fe2O3, what is the charge on iron? 7) What does the Roman number after the metal name represent? 8) As a team, determine the rules for naming type II ionic compound when given the formula. 11) As a team, determine the rules for writing the formula for a type II ionic compound when given the name. 12) Name each of the type II ionic compounds listed in Question 1 of Type II section. Finish Q on Worksheet 4.2 A + B 9 of 20

10 4.2 Compounds Containing Polyatomic Ions Polyatomic ions are ions that as a group have a set charge. Polyatomic ions are usually recognized in a formula by the grouping of more than one nonmetal elements after a metal. Your book has a table listing polyatomic ions. Use p. 5 in the data booklet to fill in the following table with the appropriate names/formulas of the polyatomic ions. Name Formula Name Formula ammonium chlorite nitrite CH 3 COO NO 3 CrO 4 2 OH 2 SO 3 Use your knowledge of Type I and Type II metals as well as the appropriate polyatomic name/ formula to fill in the following table. cyanide Check your work: Are the compound formulas you filled into the table above neutral in charge? Do all type II metals in the table above have their charge indicated by either a Roman numeral? Are all type I metals listed without a Roman numeral? Finish Q on Worksheet 4.2 A + B carbonate Name Cation Anion Formula aluminium hydroxide iron(ii) nitrate calcium sulfite ammonium nitrate OH KCN Cu(NO 10 of 20

11 4.2 Covalent compounds (non-metal and non-metal) Compounds that do not contain metals have covalent bonds instead of ionic bonds. A covalent bond is formed by sharing one or more pairs of electrons. The pair of electrons is shared by both atoms. For example, in forming H2, each hydrogen atom contributes one electron to the single bond. 1) From the following list, cross out those compounds that do NOT belong in the category for binary compounds containing only nonmetals or metalloids. CCl4 AlCl3 CO SeF6 SiO2 SrI2 P4O10TiO2 SeO3 IrCl ZrO2 N2O5 Formula and name examples for covalent compounds: CO2 = carbon dioxide H2O = dihydrogen monoxide P4S10 = tetraphosphorus decasulfide NO = nitrogen monoxide IF5 = iodine pentafluoride BF3 = boron trifluoride 2) Which element is listed first in the name? 3) Is the name of the first element in the compound different from the element? (yes/no) 4) What is the common ending for all the names? 5) What do the prefixes (di-, mono-, penta-, tri-) in the names above mean? 6) Is the prefix mono- used when there is only one atom of the first element? (yes/no) 7) Is the prefix mono- used when there is one atom of the second element? (yes/no) 8) As a team, determine the rules for naming covalent compound when given the formula. 8) Name each of the covalent compounds listed above. Finish Worksheet 4.2 C + D Covalent Compounds 11 of 20

12 NOMENCLATURE REVIEW 1. Type 1 ionic compounds: metal (only one possible charge) + nonmetal Name: metal written firstand -ide ending example: Formula: *balance charges example: 2. Type 2 ionic compounds: transition metal (two or more possible charges) + non-metal * include roman numerals in the name example: 3. Poly atomic ions: includes ions with 2 or more elements example: *have different endings, such as ite and ate *exceptions: Cyanide (CN - ), hydroxide (OH - ), bisulfide (HS - ) 4. Hydrogen: Some areas of common confusion concerning hydrogen are listed below: HBr hydrogen bromide NaOH sodium hydroxide NaH sodium hydride 5. Covalent Compounds: 2 nonmetals together *no balancing of charges *use prefixes (what you see is what you get) *no roman numerals example: 6. Elements: *Diatomic gases: I2 Br2 Cl2 F2 O2 N2 H2 pneumonic: "I Bring Clay For Our New House (or 7" plus one) * Monoatomic elements: All other elements (Na, K, Fe, etc.) 12 of 20

13 Chemical Equation: Word equation: Chapter 4.3 Chemical Equations Notes Symbolic equation: Skeleton Equation reactants Balanced Equation coefficient subscript products States of Matter: 4.3 Law of conservation of mass notes 4.3 Law of conservation of atoms notes 13 of 20

14 Chapter 4.3 Lab The Mass of Reactants and Products Question: In a chemical reaction, will the reactants weigh the same as the products? Background: In this experiment, we investigate two chemical reactions. 1. The reaction between calcium chloride and sodium carbonate: calcium chloride + sodium carbonate calcium carbonate + sodium chloride CaCl2 + Na2CO3 CaCO3 + NaCl 2. The reaction of vinegar (the chemical name for vinegar is acetic acid) and baking soda (the chemical name for baking soda is sodium bicarbonate): baking soda + vinegar carbon dioxide + water + sodium acetate NaHCO3 +HC2H3O2 CO2 + H2O + NaC2H3O2 We will use this experiment to find out if the reactants weigh the same as the products. Pre-lab questions: 1. How do you know that a chemical reaction have occurred? 2. What do you think happens to the mass in a chemical reaction? Materials: 2 beakers sodium carbonate (Na2CO3) Balance Baking Soda (NaHCO3) calcium chloride(cacl2) Vinegar (CH3COOH) Procedure/Data/Observations: 1. Put on safety goggles. Part 1 2. Add approximately 10 ml of calcium chloride to one beaker and 10 ml of sodium carbonate to another beaker. 14 of 20

15 3. Record the mass of the two beaker. Mass of reactants: 4. Add the content of one beaker to the other beaker. Record your observations: (Change in colour, temperature, formation of bubbles or similar) 5. Record the mass of the two beakers again. Mass of products: 6. Rinse the beakers. Part 2 7. Add approximately 10 ml of vinegar to one beaker and 1 tsp of baking soda to another beaker. 8. Record the mass of the two beaker. Mass of reactants: 9. Add the vinegar to the baking soda. Record your observations: (Change in colour, temperature, formation of bubbles or similar) 10.Record the mass of the two beakers again. Mass of products: 11.Rinse the beakers. Analysis: 1. How did you know that reactions occurred? 2. In part 1 did the mass of the reactants equal the mass of the products? 3. What is the law of conservation of mass? How does it relate to this experiment? 4. In part 2, did the mass of the reactants equal the mass of the products? 5. In part 2, was mass destroyed? 15 of 20

16 4.3 Conservation of Atoms Activity 1. Pick up a bag of blocks from Ms. Veenstra. 2. Record the colours symbolizing the following atoms (as written on the note in the bag): Na = H = C = O = 3. Make block models of the two reactants in the chemical reaction represented below. NaHCO3 +HC2H3O2 CO2 + H2O + NaC2H3O2 4. Make a simplified drawing of the reactants in the table below (include colour) Number of the different atoms in the reactants Na = H = C = O = Number of the different atoms in the products Na = H = C = O = 5. Count the number of different atoms in the all of the reactants and add it to the bo:om right of the table. 5. Rearrange the blocks to represent the products in the chemical reaction. Make a simplified drawing in the table. 6. Count the number of different atoms in the all of the products and add it to the bottom right of the table. Questions: 1. What does a block represent? 2. What does a collection of blocks represent? 3. What can you say about the number of blocks before and after the reaction? 4. What is the law of conservation of atoms and how is it related to this activity? 16 of 20

17 insert balancing equation activity 17 of 20

18 insert balancing activity 18 of 20

19 4.3 Balancing Notes Counting atoms Mg3(PO4)2 2Ca(NO2)2 Balancing Basics If a chemical reaction is, then mass, atoms and charge are The number of each atom is the same on both sides of the arrow. Balance by placing in front of each compound. Tips for Balancing Balance first and last Balance hydrogen and oxygen You can often treat polyatomic ions, such as SO3 2-, as a unit If an equation is balanced by using half a molecule (1/2O2), you must double all the coefficients to get whole numbers. Examples: AlBr 3 + K 2 SO 4 KBr + Al 2 (SO 4 ) 3 C4H10 + O2 CO2 + H2O 19 of 20

20 4.3 Tips for changing word equations to symbolic equations Memorize the following: methane = ammonia = water = The following elements are diatomic (they come in pairs when NOT in a compound) H2, N2, O2, F2, Cl2, Br2, I2 All other elements are not diatomic and no subscripted is used. Eg. Pb, Na, V Example: iron(iii) oxide + hydrogen water + iron sodium phosphate + calcium hydroxide sodium hydroxide + calcium phosphate 20 of 20