Skills, Stoich,
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Meas, Labreference IB objective numbers)
(# in parentheses
RXNS
Describe Gas tests for hydrogen/oxygen/carbon dioxide
M
e Define and give examples of random uncertainties and systematic errors (11.1.1)
a
s Use the correct number of significant figures to report experimental and calculated values (11.1.5)
u
r express random uncertainties as an uncertainty range +/- (11.1.4)
e
m Calculate uncertainties in processed data and state as absolute or % (11.2.1/2)
e
n State the results of calculations with the appropriate number of significant figures (11.1.5)
t
distinguish between precision and accuracy (11.1.2)
R Write equations describing chemical reactions using appropriate symbols when all reactants and products are given (1.3.1/3)
e
a Balance an equation when given the formulas for the reactants and products
c
t Identify a reaction as a combination, decomposition, single-replacement, double-replacement, or combustion
i
o Predict the products of any of the 5 reaction types
n
s Use the solubility rules or tables to identify the precipitate in a reaction
Calculate the molar mass of a compound (1.2.2)
Convert between moles, mass, molecules, ions, electrons, atoms, concentration, formula units and liters (of gas at STP or of
M
a solution with a given concentration) of a substance (1.1.2/1.2.3/1.4.5)
o
l Distinguish between the terms solute, solvent, solution, and concentration (1.5.1)
e
s Complete calculations using the ideal gas law (1.4.7)
Convert between concentration, mass of solute and volume of solution (1.5.2)
Use a balanced equation to convert moles, gas volume, mass, concentration or particles of a reactant/product into moles, gas
volume, mass, concentration or particles of a reactant/product
S
t identify the mole ratio or any two species in a balanced equation (1.3.2)
o
i identify the limiting and excess reagents (1.4.2)
c
h calculate theoretical yields from chemical equations (1.4.1)
.
solve % yield problems when given the experimental yield(1.4.3)
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Atomic Structure and thenumbers)
(# in parentheses reference IB objective
PT
find the number of valence electrons in an element based on its location on the periodic table (3.1.4)
find the electron arrangement for an element based on its location on the periodic table- up to element #20 (3.1.3)
A define the terms atomic number (A), mass number (Z) and isotope (2.1.3)
t
o state the relative masses and charges of protons, neutrons, and electrons (2.1.2)
m
calculate the number of protons, neutrons, and electrons in an isotope and/or ion (2.1.1/5)
i
c
write isotope symbols for elements given mass number (2.1.4)
S
calculate average atomic masses and isotope abundance from given data (2.2.3)
t
r
Define the term radioisotope and name several uses for radioisotopes (2.1.7)
u
c
describe the electromagnetic spectrum- spectrum is in data booklet (2.3.1)
t
u
distinguish between continuous and line spectra (2.3.2)
r
e explain how the emission lines are related to electron energy levels (2.3.3)
describe and explain the operation of a mass spectrometer (2.2.1)
12
Describe how a mass spec can be used to determine relative atomic mass using C (2.2.2)
define ionization energy, electronegativity (3.2.1)
P
e T
describe and explain trends in atomic radii, ionic radii, first ionization energy, electronegativity and melting point (3.2.2/3)
r r
i e
rank electronegativity values of 2 or more elements based on their location on the periodic table (3.2.4)
o n
d d discuss similarities and differences in chemical properties of elements in the same group- alkali reaction with water, alkali
i s with halogens, halogens with halogen ions (3.3.1)
c discuss the changes in oxide reactions with water across the periodic table- specifically the reactions of Na 2O, MgO, P4O10,
SO3 with water (3.3.2)
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Bonding IB objective numbers)
(# in parentheses reference
describe ionic bonding using the terms electron transfer, attractive forces, and lattice structure (4.1.1/8)
determine which ions elements in groups 1-3 and 5-7 will form (4.1.2/3/4)
Deduce the formula and name for ionic compounds with and without polyatomic ions
memorize some common polyatomic ions (4.1.7)
identify ionic and covalent compounds by their formulas and electronegativity values (4.1.6/4.2.5)
describe covalent bonding in terms of electron sharing + electrostatic attraction between shared electrons and positive nucleus
(4.2.1/2)
draw Lewis structures for covalent compounds and ions with up to 4 electron pairs (4.2.3)
Name covalent compounds with two elements
Write formulas for ionic and covalent compounds when given the name
use the VSEPR theory to predict molecular shape and bond angle for covalent compounds with up to 4 electron pairs (4.2.7)
predict the polarity of a covalent compound based on the electronegativity differences and/or molecular shape (4.2.6/8)
state and explain the relationship between bond strength+ length and the number of bonds (4.2.4)
describe the types of intermolecular forces (dipoles and hydrogen bonding) and explain how they occur (4.3.1)
explain how intermolecular forces affect boiling point of a substance (4.3.2)
describe and compare the structure and bonding in the 3 allotropes of carbon- diamond, graphite, and C60 (4.2.9)
describe the structure and bonding of silicon and silicon dioxide (4.2.10)
determine the empirical formula from experimental data (1.2.5)
Calculate the empirical and molecular formulas of a substance given its percent composition (and molar mass) (1.2.4/5/6)
determine the empirical formula from experimental data (1.2.5)
describe metallic bonding in terms of a lattice of positive ions and delocalized electrons (4.4.1)
explain why metals have high malleability and conductivity metals ( 4.4.1)
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Redox
(# in parentheses reference IB objective numbers)
Textbook Chapter 4 (section 4 only) and Chapter 20 (sections 1-3, 7, and 9)
state names of compounds using oxidation #s of transition metals (9.1.3)
define reduction, reducing agent, oxidation, and oxidizing agent (9.1.1/9.2.3)
determine oxidation # of an element in a compound (9.1.2)
identify the elements being reduced and oxidized (and the oxidizing and reducing agents) in a redox
equation (9.1.4/9.2.4)
write half-equations given the species involved in a redox reaction (9.2.1)
balance half-equations in neutral and acidic conditions (9.2.2)
use the reactivity series to determine whether a redox reaction will occur (9.3.2)
deduce a reactivity series based upon the chemical behavior of a group of ox and red agents (9.3.1)
describe a voltaic cell by drawing a diagram and showing movement of electrons (9.4.1)
label anode=oxidation=negative electrode, cathode=reduction=positive electrode for a voltaic cell (9.4.2)
diagram an describe an electrolytic cell, including the essential components and electron movement
(9.5.1/3)
label anode=oxidation=positive electrode, cathode=reduction=negative electrode for an electrolytic cell
(9.5.2)
deduce the products of the electrolysis of a molten salt (9.5.4)
distinguish between the spontaneity of reactions involved in a voltaic and electrolytic cell
Kinetics
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Thermo + in parentheses reference IB objective numbers)
(#
write thermochemical equations using ΔH
draw an enthalpy level diagram for a reaction when given ΔH
Use an enthalpy level diagram to determine the relative stabilities of reactants and products, and the sign of the energy change (5.1.4)
define the terms exothermic, endothermic, enthalpy, and standard enthalpy change (5.1.1)
Identify exothermic and endothermic processes using temperature change and/or enthalpy change (5.1.3)
state the combustion and neutralization are exothermic processes (5.1.2)
use bond enthalpies to explain and/or calculate ΔH in a reaction (5.4.2)
define the term average bond enthalpy (5.4.1)
use Hess's law to calculate heat changes (5.3.1)
determine a procedure for measuring DH using calorimetry (5.2.2)
use q=mcΔT to solve for any missing variable using experimental data (5.2.1)
use q=mcΔT to find C for a metal using lab data from a calorimeter (5.2.3)
evaluate the results of calorimetry experiment (5.2.4)
define "rate of reaction" and "activation energy" (6.1.1/6.2.2)
State the 3 main tenets of Collision Theory (6.2.3)
describe experimental procedures for determining the rate of a reaction (6.1.2)
analyze data from rate experiments including graphs of concentration, volume, and mass against time (6.1.3)
sketch and interpret the Maxwell-Boltzmann energy diagram with and without a catalyst (6.2.5/7)
predict and explain the qualitative effects particle size, temperature, concentration, and a catalyst has on the rate of a reaction (6.2.4/6.2.6)
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Equilibrium, &(#Acid+Base
in parentheses reference IB objective numbers)
E Define and give examples of equilibrium systems- chemical (ex= NO2 N2O4 tubes) and physical (ex= water cycle) (7.1.1)
q
u
i Apply Le Chatelier's Principle to predict the qualitative effects of changes in temperature, pressure, concentration, and a catalyst on equilibrium (7.2.3/4)
l
i Write K expressions for equilibrium reactions (7.2.1)
b
r
Deduce the extent of a reaction from the magnitude of K (7.2.2)
i
u
m apply the concepts of kinetics and equilibrium to industrial processes (ex: Haber process, Contact process) (7.2.5)
distinguish between strong and weak acids and bases based on pH, dissociation (strong = full dissociation), conductivity (strong = higher), and reaction
(strong= fast) (8.3.1)
A
c memorize some major strong and weak acids and bases (8.3.2)
i
d
determine relative strengths of acids and bases using experimental data (8.3.3)
s
a state that the change of 1 unit in pH is equivalent to a 10-fold change in [H] (8.4.3)
n
d deduce changes in [H] when the pH of a solution changes by more than 1 pH unit (8.4.4)
B
list the characteristic properties of acids and bases, including reactions with carbonates and metals (8.2.1)
a
s
e define acids and bases using Bronsted-Lowry and Lewis theories (8.1.1/2)
s
deduce the formula for a conjugate acid/base of any Bronsted-Lowry acid/base (8.1.3)
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Organic (# in parentheses reference IB objective numbers)
define homologous series (10.1.1)
Organic Basics
distinguish between empirical, molecular, condensed structural formulas and full structural formulas (also in Bonding section) (10.1.3)
define and give examples of structural isomers (10.1.4)
Name/Form.
deduce structural formulas for non-cyclic alkane and alkene chains up to C6 (10.1.5/7)
Apply IUPAC rules for naming non-cylic alkanes and alkenes up to C6 (10.1.6/8)
write equations for complete and incomplete combustion of alkanes and alcohols (10.2.2 + 10.4.1)
write equations for reactions of alkenes with hydrogen, halogens, hydrogen halides, and water (10.3.1/2))
use bromine water to distinguish between alkanes and alkenes (10.3.3)
write reactions of methane and ethane with chlorine and bromine (10.2.3)
Reactions
explain the reactions of alkanes with chlorine and bromine in terms of a free-radical mechanism (10.2.4)
outline polymerization of alkenes, including identification of the repeating unit (10.3.4)
discuss the economic importance of alkene reactions: hydrogenation of vegetable oils, manufacture of ethanol, polymerization in plastics (10.3.5)
write equations for substitution reactions of haloalkanes with sodium hydroxide (10.5.1)
explain the halogen/NaOH substitution reactions in terms of Sn1 and Sn2 mechanisms (10.5.2)
determine structures for compounds up to C6 with one of the functional groups: alcohol, aldehyde, ketone, acid, and halide (10.1.9)
Name/Formula
apply IUPAC rules for naming compounds up to C6 with one of the functional groups: alcohol, aldehyde, ketone, acid, and halide (10.1.10)
identify amino, benzene ring, and ester functional groups (10.1.11) (note: don't need to name)
identify primary, secondary, and tertiary carbon atoms in alcohols and haloalkanes (10.1.12)
discuss melting point, volatility, and solubility in water for compounds with the functional groups: alcohol, aldehyde, ketone, acid, and halide (10.1.13)
Properties
predict and explain trends in boiling points in a homologous series (10.1.2)
explain low reactivity of alkanes in terms of bond enthalpy and bond polarity (10.2.1)
deduce reaction pathways given the starting materials and product (10.6.1)
Reactions
write equations for the complete combustion of alcohols (10.4.1)
write equations for the oxidation of primary and secondary alcohols (10.4.2, 10.4.3)
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Food Chem (# in parentheses reference IB objective numbers)
Distinguish between a food and a nutrient (F.1.1)
Basics
Describe chemical composition of lipids, carbohydrates, and proteins (F.1.2)
describe the difference in structure between saturated and unsaturated fatty acids (F.2.1)
Predict the degree of crystallization and melting point of fats and oils from their structure, and explain the relevance of this property at home and in
industry (F.2.2)
Fats
Deduce the stability of fats and oils from their structure (F.2.3)
Describe the process of hydrogenation of unsaturated fats (F.2.4)
Discuss the advantages and disadvantages of hydrogenating fats and oils (F.2.5)
Explain the meaning of the term shelf life (F.3.1)
Discuss the factors which affect the shelf life and quality of food (F.3.2)
Discuss the rancidity of fats (F.3.3)
Shelf Life
Compare the process of hydrolytic and oxidative rancidity in lipids (F.3.4)
Describe ways to minimize the rancidity rate and prolong shelf life of food (F.3.5)
Describe traditional methods used by different cultures to extend the shelf life of foods (F.3.6)
Define the term antioxidant (F.3.7)
List examples of common naturally ocurring antioxidants and their sources (F.3.8)
Antioxidants
Compare structural features of the major synthetic antioxidants in food (F.3.9)
Discuss the advantages and disadvantages associated with natural and synthetic antioxidants (F.3.10)
List some antioxidants found in traditional foods of different cultures that may have health benefits (F.3.11)
Distinguish between a dye and a pigment (F.4.1)
Explain the occurrence of color in naturally occurring pigments (F.4.2)
Describe the range of colors and sources of the naturally occurring pigments anthocyanins, cartenoids, chlorophyll, and heme (F.4.3)
Color
Describe the factors that affect the color stability of anthocyanins, cartenoids, chlorophyll, and heme (F.4.4)
Discuss the safety issues associated with the use of artificial colorants in foods (F.4.5)
Compare the processes of non-enzymatic (Maillard) and carmelization that cause browning in food (F.4.6)
Define genetically modified (GM) food (F.5.1)
GM
Discuss the benefits and concerns of using GM foods (F.5.2)
Solidifying
Distinguish between the following types of dispersed systems: suspensions, emulsions, and foams (F.6.1/2)
Describe the action of emulsifiers (F.6.3)
Chem
2e2e1596-4d3a-4e0e-a5c5-1e757002592d.xlsx-- Environmental (# in parentheses reference IB objective numbers)
Discuss methods for reduction of primary air pollution: catalytic converters, scrubbing, recirculation of exhaust gases, sulfur removal from coal and oil…
(E.1.2)
Describe sources of primary air pollution (E.1.1)
state what is meant by the term acid deposition (acid rain and acid particles) and outline its origins, including equations (E.2.1)
discuss the environmental effects of acid deposition and possible methods to counteract them (E.2.2)
A
i Describe the Greenhouse Effect, the influence of particulates on the Earth's temperature, and the effects of global warming on the earth (E.3.1/3)
r
List the main greenhouse gases, their sources, and relative effects (E.3.2)
Describe the natural formation and depletion of ozone in the stratosphere, including equations (E.4.1)
List some ozone-depleting products and their sources (E.4.2)
Discuss alternatives to CFCs and their properties (E.4.3)
Outline the importance of dissolved oxygen in water (E.5.1)
Distinguish between aerobic and anaerobic decomposition of organic material in water (E.5.2)
W Describe the process of eutrification and its effects (E.5.3)
a
t Describe the sources and effects of thermal pollution in water (E.5.4)
e
r
List the primary pollutants found in waste water and identify their sources (E.6.1)
Outline the stages of sewage treatment including the materials removed at each stage (E.6.2)
Evaluate the process to obtain fresh water from sea water using multi-stage distillation and reverse osmosis (E.6.3)
Discuss salinization, nutrient depletion, and soil pollution as causes of soil degradation (E.7.1)
Describe the relevance of the soil organic matter in preventing soil degradation and outline its physical and biological functions (E.7.2)
L
List common sources of organic soil pollutants (E.7.3)
a
n
d Outline and compare various methods of waste disposal- landfill, incineration… (E.8.1)
Describe the recycling of metal, glass, plastic, and paper and outline its benefits (E.8.2)
Describe the characteristics and sources of different types of radioactive waste and compare storage methods (E.8.3/4)