CHEMISTRY 11

CHEMISTRY 11

LEARNING OUTCOMES

Chemistry 11 is an introductory course that focuses on the principles and theories of Chemistry. It is designed to help students understand some of the basic processes that occur in the natural environment and the role of chemistry in our everyday lives. Basic skills in Science are also developed further as students prepare for future courses in the Sciences.

A. Introduction to Chemistry

Lab Safety

· list the safety and protective equipment available in the laboratory

· describe how and when to use each piece of equipment

· indicate on a school map the location of the nearest fire alarm and appropriate fire exits

· list sources of first‑aid assistance other than the classroom teacher

· describe common chemistry laboratory hazards

· describe the appropriate procedure or technique for dealing with particular hazards

· produce a list of general rules of safe laboratory conduct

· display a conscious safety attitude in the laboratory

Matter and Its Changes

· define matter

· describe chemistry as the science concerned with the properties, composition, and behavior of matter

· describe and give examples of a variety of forms and properties that matter can exhibit

· distinguish between observation and interpretation

· describe the types of changes that may be observed when matter is heated, combined, or separated

· differentiate between physical and chemical changes

· classify a substance as solid, liquid, or gas, and describe its different properties

· define boiling point, freezing point, and melting point

· describe the simple molecular motions and arrangements for solids, liquids, and gases

· relate the heat changes that occur during phase changes to changes in molecular motions and arrangements

B. Atoms, Molecules, and Ions

Classification

· describe a substance as having a set of unique and identifiable properties

· classify a given material as an element, compound, or mixture, using the properties of the material

· describe several ways that substances may be separated from one another

· relate the observable properties and characteristics of elements, compounds, and mixtures to the concept of atoms and molecules

· define atom, molecule, and ion

Nomenclature

· write chemical symbols for elements and formulae for ions from appropriate charts

· name the ionic compound from a formula, and write the formula given a name

· name the covalent compound from a formula using the prefix naming system, and write the formula given a name

· predict the formulae of covalent compounds given the formula of another compound containing elements in the same family (families)

· write the names and formulae for some common acids

Measurement and Communication

· use SI units and their accepted alternatives in chemistry

· demonstrate skills in measuring mass, volume (liquid), and temperature

· describe the imprecise nature of all measurements

· determine the number of significant figures in a measured quantity and relate to the uncertainty

· round off calculated results to the appropriate number of significant figures

· correctly determine the unit of a derived quantity

· state the acceptability of numerical results of a lab experiment with regard to the uncertainty of the results

· communicate results and data in clear and understandable forms

C. Mole Concept

Introduction

· explain the relative nature of atomic mass

· identify the unit for counting atoms, molecules, or ions as the mole

· define the mole

· determine the molar mass of an element or compound

· perform calculations relating the number of particles, moles, and mass

Molar Volume of Gases

· state Avogadro's hypothesis

· determine experimentally the molar volume of a gas at room temperature and pressure

· state the molar volume of a gas at STP

· calculate the moles or mass of a gas from a given volume at STP or vice versa

Percent Composition

· compare and contrast molecular and empirical formulae

· determine the percent composition by mass from the formula of a compound

· determine the empirical formula for the compound from the percent composition by mass

· determine the molecular formula from the molecular mass and empirical formula

Molarity

· describe molarity (mol/L or M) as a measure of molar concentration

· prepare a standard solution

· perform calculations relating mass (or moles) of solute, volume of solution, and molarity

· calculate the resulting concentration when a given volume of a standard solution is diluted with water to a given volume

D. Chemical Reactions

Introduction

· define reactants and products

· observe and record changes that occur during a chemical reaction

· describe chemical reactions in terms of the rearrangement of the atoms as bonds are broken and new bonds are formed

· gather experimental data that lead to the law of conservation of mass

· apply the law of conservation of mass to a formula equation of a reaction to demonstrate that atoms are conserved in the reaction

· balance formula equations of several chemical reactions

· use subscripts to represent solids, liquids, gases, and aqueous solutions

· classify, predict products, and write balanced equations for the following types of chemical reactions:

· define exothermic and endothermic reactions

· classify reactions as exothermic or endothermic based on experimental observations

· relate energy changes to bond breaking and formation

· write equations for chemical reactions including the energy term

Stoichiometry

· relate the coefficients in a balanced equation to the relative number of molecules or moles (the mole ratio) of reactants and products in the chemical reaction

· perform calculations involving reactions using any of the following:

o number of molecules

o moles

o mass

o gas volume at STP

o solution concentration and volume

· perform calculations involving limiting reagent

E. Atomic Theory

Introduction

· describe early models of the atom

· describe the relative position, mass, and charge for a proton, neutron, and electron

· identify the atomic number for an element, using a table

· calculate the number of protons and electrons in an atom or ion

· define isotope and explain it in terms of atomic structure

· calculate the number of neutrons, protons, and electrons for an atom or ion of an isotope given the mass number of the isotope and the charge of the ion

· calculate the average atomic mass from isotopic data

· describe a simple electron arrangement for the first 20 elements

Periodic Table

· classify elements as metal, non‑metal, or metalloid and locate them on the periodic table

· describe the similarities and trends among elements using such properties as: melting point, ionization energy, atomic radius, chemical reactivity, ion charge, conductivity

· distinguish the ordering of elements in early periodic tables (based on atomic mass) from the ordering of elements in the modern periodic table (based on atomic number)

· identify the following families of elements: alkali metals, alkaline earth metals, halogens, noble gases

· describe some properties of the alkali metals, alkaline earth metals, halogens, and noble gases

· relate noble gas stability to electron arrangement within the atom

· predict the probable electron gain or loss for elements in columns 1, 2, 13, 15, 16, and 17 to attain stability

· relate the observed charge of monatomic ions of metals and non‑metals to numbers of electrons lost or gained

· predict the characteristics of elements knowing the characteristics of another element in that family

· predict the metallic character of an element based upon its position in the table

Chemical Bonding

· define covalent and ionic bonding

· define valence electrons

· demonstrate a knowledge that bonding involves valence electrons

· draw an electron dot diagram for an atom

· identify from a chemical formula the probable type of bond (ionic or covalent)

· draw electron dot diagrams and structural formulae for simple molecules and ions and deduce molecular formulae

F. Solution Chemistry

Introduction

· define solution as a homogeneous mixture

· classify a solution as a system distinct from a pure solid, liquid, or gas

· identify the solute and the solvent as the components of a solution

· describe the causes of molecular polarity

· categorize various common solvents as polar and non‑polar

· on the basis of observations, make deductions concerning the solubility of polar and non‑polar solutes in polar and non‑polar solvents

· use lab observations to describe the relative conductivity of several solutes in aqueous solution

· summarize the results of a conductivity experiment as to the types of solute that conduct electricity when dissolved in water

· propose a mechanism that explains the conductivity of soluble salts in water

· write dissociation or ionization equations for several substances that dissolve to give conducting solutions

· calculate the molarity of each ion in a salt solution given the molarity of the solution

· calculate the concentration of ions resulting when two solutions of known concentration and volume are mixed (assuming no reaction)

G. Organic Chemistry

Introduction

· identify the multiple bonding character of carbon atoms

· identify carbon as the backbone of organic chemistry

· relate organic chemistry to products such as plastics, fuels, pharmaceutical drugs, pesticides, insecticides, solvents, synthetics

· identify major sources of organic compounds

· describe a specific industrial application of organic chemistry

Hydrocarbons

· define hydrocarbon, alkane, alkene, alkyne, cyclic, and aromatic as they relate to organic compounds

· classify a hydrocarbon as either saturated or unsaturated

· compare the geometry of single, double, and triple bonds between two carbon atoms

· compare the rotational ability in single, double, and triple bonds

· name and draw structures of alkanes, alkenes, and alkynes up to C₁₀

· recognize and name the substituent groups methyl, ethyl, fluoro, chloro, bromo, and iodo

· name and draw structures of simple substituted alkanes to C₁₀

· identify cis‑ or trans‑isomers of alkenes

· draw a structure of a benzene ring

Functional Groups

· describe the term functional group and relate it to classes of compounds

· identify a compound as an alcohol, aldehyde, ketone, ether, organic acid, ester, amine, or amide when given a structural diagram

· name and draw structures for simple alcohols

· describe how an ester can be prepared through the reaction of an alcohol and an organic acid and how it can be detected (by its aroma)