Safety First
I can…
 Follow safe laboratory practices
 Identify lab equipment
What Can We Measure About Chemicals?
How Do We Communicate About Chemicals?
I can…
 Find the mass of any atom (in grams) on a periodic table.
 Determine the molar mass/gram formula mass for compounds and molecules.
 Give examples of atoms, molecules, elements, and compounds.
 State the # and kind of atoms in formulas using parentheses [ex., Ca(NO ) ≈ CaN O ]
 List the seven diatomic elements.
3 2
2
6
How Are Measurements Different from Regular Numbers?
I can…
 Recognize the difference between accuracy (how close measurements are to a “true” value) and precision (how
close measurements are to each other).
 Measure length, mass, and volume with the correct precision.
 Round off long numbers to a specified decimal place.
 Write very large or very small numbers in scientific notation.
 Analyze class data to indicate precision significant figures.
 Define significant figures as all those of which you are certain plus one more that involves judgment of the observer.
How Can I Show That My Calculations Are Correct?
I can…
 Write equalities as conversions factors. [ex., ]

problems that convert one unit to another.
 Use “dimensional analysis” (train tracks) to set up
 Calculate answers from a dimensional analysis set up.
 List the six metric prefixes (nano-, micro-, centi-, milli-, and kilo-) as conversion factors for Liters (volume), meters
(length), and grams (mass).
 Enter numbers written in scientific notation into a scientific calculator.
What is Matter?
I can…
 Define matter
 Classify a substance as a solid, liquid, and gas
 Identify a phase change and classify as endothermic or exothermic
 Identify properties of matter as physical or chemical
 Distinguish between physical and chemical changes
 Determine whether a property is extensive or intensive
 Distinguish between a homogenous and heterogeneous mixture
 Distinguish between elements and compounds
 Distinguish between elements as monoatomic and diatomic
 Distinguish between a pure substance and a mixture
Why Is Density A Useful Property of Matter?
I can…
 Define density.
 Calculate density from measurement data.
 Show calculations with enough detail so errors can be recognized.
 Make a simple data table with labels, units, and straight lines.
 Explain that since density does not depend on the size of the sample, it is more useful for identifying substances
than mass or volume.
How Do We Symbolize A Chemical Reaction?
I can…
 define and give examples of “reactants,” “products,” and “coefficients”
 explain that chemical equations are balanced because the number and kind of atoms do not change during a
chemical reaction, they are merely rearranged. Mass is conserved.
What Is Stoichiometry?
I can…
 use the coefficients in a balanced as a conversion factor for calculations
 calculate the mass, or number of particles of any substance in a chemical reaction given the mass or number of
particles of any other substance in the chemical reaction
What Do Atoms Look Like?
Parts of an Atom
I can…
 describe the progression of the atom through time and the contribution of the “dead dudes” to atomic theory
 describe the nuclear model of the atom
 list the three parts of the atom, their masses, their charges, their locations, and whether they contribute to the
mass or the volume of the atom
 describe the relative sizes of the electron, proton, neutron, atom, and nucleus (the 6-mile atom)
 identify an element’s atomic mass, atomic number, and probable mass number of the most abundant isotope from
the periodic table
 calculate an atoms atomic mass given masses and percent abundances of the stable isotopes
 identify pairs of isotopes given atomic numbers and mass numbers
Where the Electrons Live
I can…
 define the 4 quantum numbers (n, l, m , m )
 assign the 4 quantum number to the last electron placed
 identify the atom based on the 4 quantum numbers
 draw the atomic orbital diagram/notation (up to level 7)
 place electrons correctly into the orbital diagram
 state the electron configuration for any atom.
 state the number of electrons an atom has available for bonding. (valence electrons)
 explain the difference between the energy and location of an electron.
l
s
Electrons behave like waves and light
I can…
 define electromagnetic radiation (ER)
 define a quantum and photon of energy
 state how fast a photon of energy or a wave is traveling
 calculate the energy of a wave
 calculate the frequency or wavelength of a wave
 predict the type of ER based on energy, frequency, or wavelength
The Periodic Table—Families
I can…
 identify metals, non-metals, and semi-metals on the periodic table and state properties of each group including
conductivity (of heat and electricity), malleability, and ductility
 identify groups or families of the periodic table including hydrogen, alkali metals, alkaline earth metals, halogens,
noble gases, and transition metals
 give examples of how elements gain or lose electrons to have the same number of electrons as a noble gas.
 give examples of how members of a family act similarly chemically including ions formed, compounds formed, and
tendency to lose, gain, or maintain electrons
The Periodic Table—Trends
I can…
 use Zeff , shielding, and electron-electron repulsion to explain the trends
 discuss the size of an atom in terms of the size of the electron cloud. Discuss the role played by electron-electron
repulsions and electron-proton attractions on the size of the electron cloud.
 define and give an example of ionization energy. Relate atomic size to ionization energy
 define electronegativity and realize that it is a calculated value based on ionization energy
 state horizontal and vertical trends in atomic size and give a rationale for each trend
 describe and explain the change in size of an atom as it becomes a negative or positive ion (ionic radius)
 Discuss the reactivity of metals and non metals based on EN and IE
What Happens When Chemicals Are Put Together?
What Happens When Fuels Burn?
I can…
 state that burning is called combustion
 write the reactants and products for a complete combustion reaction of a hydrocarbon fuel
 balance combustion equations
 include “heat” as a product of combustion
How Do We Symbolize A Chemical Reaction?
I can…
 define and give examples of “reactants,” “products,” and “coefficients”
 explain the difference between a chemical reaction and a chemical equation
 write a chemical equation given a word equation for a chemical reaction
 balance chemical equations making certain that each side of the equation has the same number and kind of atoms
 explain that chemical equations are balanced because the number and kind of atoms do not change during a
chemical reaction, they are merely rearranged. Mass is conserved.
Can We Classify Reactions?
I can…
 state four types of chemical reactions (besides combustion) and show their patterns:
XY + AB → XB + AY
XY + A → AY + X
X + Y → XY
XY → X + Y
 match actual chemical equations to these four types and combustion
 state that active metals and acids form H gas
 define “precipitate” as a solid product in a double replacement reaction
2
What Are Ionic Compounds Made Of?
I can…
 define an ion as an atom or group of atoms with a charge
 state that a positive ion results when an atom loses electrons while a negative ion results when an atom gains
electrons
 memorize the common ions so I can give the symbol and charge when given the name and vice versa
 state the charges of some ions because of their position on the periodic table
 write an ionic compound from any positive and negative ion
 use parentheses appropriately when writing compound that involve polyatomic ions
 use the terms “anion” for a negative ion and “cation” for a positive ion
Are All Compounds Ionic?
I can…
categorize a substance as ionic or covalent.
recognize molecular compounds formed between two non-metals
 name molecular compounds using the prefixes mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, and deca-,
etc.
name an ionic compound and write the formula (don’t forget to balance the charges)
recognize acids as ionic compounds where the

ending
acid name
example
ion is H+
positive ide

ion
 add
name acids according to the ending of the negative
ite
“ur” or “or” when sulfur or phosphorus are part of
the ion
ate
How Do Atoms Stick Together? (Bonding)
I can…
 name the three kinds of bonds:
 describe each kind of bonding:



 state the kind of bond that will form between any two atoms
metal/nonmetal
metal/metal
nonmetal/nonmetal
 use electronegativity difference to predict the bond type
What Substances Use These Bonds?
I can…
 give examples of the three kinds of substances:
Ionic
Covalent
Metallic
 state that all solids have a “crystal lattice” and can state what makes up the points of the crystal lattice for each
type of substance.
 state the properties of a metal (malleable, ductile, shiny, good conductor of heat & electricity) and explain them in
terms of metallic bonding.
 state the properties of an ionic solid [brittle, cubic, good conductor of electricity as (l) or (aq)] and explain them in
terms of ionic bonding.
How Do We Symbolize These Bonds?
I can…
 write the Lewis symbol for any element or ion.
 show a covalent bond as a pair of electrons being shared between two atoms. (H:H)
 draw the Lewis structure for a simple molecule with a single, double, or triple bond.
 recognize a Lewis structure that has the correct number of valence electrons and follows the “octet rule”.
 Recognize a Lewis structure that has the correct number of valence electrons and does not follow the “octet rule”
has an expanded valence
 Identify the areas of electron density on the central atom
 Transform a Lewis structure into the correct VSEPR shape
 State the electronic structure and molecular shape
 Recognize whether a bond is polar or non polar
 Label a structure polar or non polar based on the polarity of the bond and the structure of the molecule
 Identify whether or not the substance is polar or non polar based on the molecular structure
o Label dipoles
What Can be Done With a Formula
I can …
 Calculate the mass of a molecule given its formula.
 State the # and kind of atoms in formulas using parentheses [ex., Ca(NO )  CaN O ]
 List the seven diatomic elements.
 Calculate the % composition (by mass) given the percent composition
 Calculate the empirical formula from percent composition data.
 Calculate the molecular formula given the empirical formula and molar mass of the molecular.
3 2
2
6
 Distinguish between empirical and molecular formula
What Is Stoichiometry?
I can…
 identify the limiting reactant (the reactant that runs out first) when amounts of two reactants are mixed
 solve limiting reactant problems in which two given values are supplied
 determine the percent yield of a substance after determining the theoretical yield.
How Hot can it Get (Thermo Review)
I can…
 distinguish the difference between heat (q) and temperature (T).
 describe the law of conservation of energy

Identify different forms of heat transfers
 define energy with appropriate units.

Identify different forms of energy
 define the universe in terms of the system and the surroundings
 describe and label the direction of heat flow in relation to the system using correct terminology and signage.

define exothermic and endothermic and assign correct signs.
 define specific heat (c) with appropriate units.
 calculate the amount of heat within a system when a temperature change is present (q=mcΔT).
 calculate the amount of heat required to change the phase of a substance.
 calculate the amount of heat transferred from one system to another and other related problems (ex. Calculate the
final temperature).
 define enthalpy (ΔH) and the units of enthalpy.
 define enthalpy of formation.
 calculate the enthalpy of reaction using enthalpy of formations.
 identify on a heating curve or cooling curve where a phase change is occurring.
 calculate the amount of energy required to heat a substance from T to T (don’t forget the phase changes).
 describe how the heat of a reaction changes as the reaction is manipulated (if the reaction is doubled the heat
1
2,
doubles)
 describe Hess’s Law
 calculate the heat of a reaction using Hess’s law and a reaction mechanism.


Identify a catalyst
Identify an intermediate
Unit 5 Gases: How Do Hot Air Balloons Float?
I can…



convert between pressure units (atm, mmHg, kPa)
convert K to C and C to K
explain that Kelvin temperature is always used in gas law calculations because 0 K actually means zero molecular
motion whereas 0 C is simply the freezing point of pure water










state the postulates of kinetic molecular theory and how they relate to Boyle’s, Charles’, and Gay-Lussac’s Laws.
identify a graph of two variables as directly proportional or inversely proportional
identify a problem as P·V,
P V PV
,
,
, or PV=nRT
T T T
explain what temperature and pressure look like in terms of the Kinetic Molecular Theory
 temperature = motion of particles (KE)
 pressure = collisions with the walls of the container
convert grams into moles, n, to use in PV=nRT
recognize which value of R to use in a PV=nRT problem
substitute and evaluate the PV=nRT equation correctly so I can solve the equation for various variables.
calculate for the moles or volume of a gas used or produced in a reaction using stoichiometry at:
 standard temperature and pressure
 at non-standard conditions
define limiting reactant
using stoichiometry:
 Identify the limiting reactant
 Calculate how much product can be produced using the limiting reactant
 Calculate how much of the excess reactant will have been used or remain.
Solutions & Molarity
I can…
 define Intermolecular Forces (IMFs).
 compare the relative strengths of the IMFs.
 based on polarity of the molecule predict the IMF present.
 predict the boiling point and freezing point of multiple substances based on the IMF.
 identify the solute and solvent in a solution.
 quantify the concentration of a solution using the definition of molarity.
 state the definition of molarity,
 make a solution correctly.
 use a solubility curve to predict whether a solution is unsaturated, saturated, or super saturated.
 describe how to create a unsaturated, saturated, or super saturated solution using a solubility curve.
 dilute a concentrated solution to make a specified quantity of a dilute solution, V M = V M
 distinguish between an electrolyte and non electrolyte.
 Write a net ionic equation
 Identify the spectator ions
Acids & Bases
i
I can…
 state the operation definitions of acids, bases, and neutral chemicals.
 state the theoretical definitions of acids, bases, and neutral chemicals. [Formulas]
i
f
f
 explain why the H ion is referred to as a proton.
 explain that when an acid donates a proton, another molecule (H O) must accept the proton to form hydronium ion
+
2
(H3O+).
 define acids & bases according to the Arrhenius definition.
 define acids & bases according to the Brønsted-Lowry definition.
 identify Brønsted-Lowry conjugate acid/base pairs
 neutralize an acid with a base.
 write formulas of common acids and bases and state whether they are weak or strong.
 write equations showing the neutralization of acid with base to form water and a salt.
 explain that water is a VERY weak electrolyte, making its formation a driving force for the double replacement
reaction that is acid-base neutralization.
 perform a titration using an acid-base indicator such as phenolphthalein solution.
 calculate the concentration of an unknown acid or base given titration data.
How Can An Acid Be “Weak”?
I can…
 explain how an acid can be weak in terms of “dissociation.”
 list the strong acids and strong bases.
What is pH?
I can…
 write the equilibrium equation associated with pure water.
 write the K expression for water and state that the value of
 explain that every aqueous solution contains some H and OH and that [H ][OH ] = 1 x 10
 calculate the [H ] and [OH ] for any aqueous acidic or basic solution.
 state the definition of pH as the “power” of the [H ].
 state the pH given simple data such as
[H ] = 1 x 10 M or [OH ] = 1 x 10 M.
 state that pH + pOH = 14 and explain:
w
+
+
-
+
-
-14
.
-
+
+
-5
-
[H+]
[OH-]
pH
pOH
-11
Titrations
I can…





identify the equivalence point on a titration curve.
label the titration as weak/strong or strong/strong based on the equivalence point.
determine the substance in the beaker prior to titrating based on the pH.
describe what is occurring at the equivalence point.
calculate the number of moles of titrant (substance added from the burette) added based on the equivalence
point given molarity and volume.
 calculate the amount or concentration of an acid or base needed to titrate a known acid or base.
 calculate the percent concentration of a substance using titration (mustard lab)
Radioactivity—What is the Nucleus Like?
I can…
 list and describe three kinds of radiation that fly out of the nucleus

describe radioactive elements as elements with unbalanced numbers of protons and neutrons (the band of
stability)
 state the changes that occur in a nucleus when each type of radioactivity is observed
o alpha
o beta
o positron (beta positive)
o gamma
Is Radioactivity Dangerous?
I can…
 state that nuclear radiation can be dangerous because “fast moving photons (gamma rays), electrons (beta rays)
and helium nuclei (alpha particles) can crash into other molecules and change their structure. If this happens to a DNA
molecule, it can damage the genetic information, and sometimes turn a cell cancerous. Radiation also causes burns,
much like sunburn, in large doses over short amounts of time.”*
 state that since alpha particles are the most easily stopped, they are the least dangerous. Gamma radiation is more
penetrating, but interacts with matter less frequently. Explain that even though radioactivity can damage tissue, it also
has great benefits
Does Radioactivity Go Away?
I can…
 explain that radioactive nuclei decay randomly, but follow simple mathematical rules when considered collectively.
 write the equation for half life and identify all of the variables.
 use the half life to calculate how much of a sample remain after a given period of time.
What Can Radioactivity Be Used For?
I can…
 list at least 5 uses for radioactivity [http://www.darvill.clara.net/nucrad/uses.htm]
 describe nuclear fission, fusion, and energy