Download Safety First I can… o Follow safe laboratory practices o Identify lab

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…
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Find the mass of any atom (in amu’s) on a periodic table.
Write symbols and names for the elements.
Give examples of atoms, molecules, elements, and compounds.
State the # and kind of atoms in formulas using parentheses [ex., Ca(NO3)2  CaN2O6]
List the seven diatomic elements.
How Are Measurements Different from Regular Numbers?
I can…
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Recognize the difference between accuracy (how close measurements are to a “true” value) and precision (how
close measurements are to each other).
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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 using  notation or 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…
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Write equalities as conversions factors. [ex.,
1 mile
]
5280 feet
Use “dimensional analysis” (train tracks) to set up problems that convert one unit to another.
Calculate answers from a dimensional analysis set up.
List the three metric prefixes (centi-, milli-, and kilo-) as conversion factors for Liters (volume), meters (length), and
grams (mass).
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Enter numbers written in scientific notation into a scientific calculator.
What is Matter?
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Define matter
Classify a substance as a solid, liquid, and gas
Identify a phase change and classify as endothermic or exothermic
Use a triple point curve to identify the state of matter based on temperature and pressure
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 a pure substance and a mixture
Why Is Density A Useful Property of Matter?
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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.
What Happens When Chemicals Are Put Together?
What Happens When Fuels Burn?
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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…
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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…
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state four types of chemical reactions (besides combustion) and show their patterns:
double replacement
(XY + AB  XB + AY)
single replacement
(XY + A  AY + X)
synthesis
(X + Y  XY)
decomposition
(XY  X + Y)
match actual chemical equations to these four types and combustion
make, collect, and identify three gases, H2, O2, and CO2. Additionally, I can classify the chemical reactions used to
make and test these gases according to the four types studied in class.
state that active metals and acids form H2 gas
define “precipitate” as a solid product in a double replacement reaction
What Are Ionic Compounds Made Of?
I can…
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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 40 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…
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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.
recognize acids as ionic compounds where the positive ion is H+
name acids according to the ending of the negative ion
ending
acid name
ide
hydro____ic acid
ate
____ic acid
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example
HCl
hydrochloric acid
HClO3
chloric acid
add “ur” or “or” when sulfur or phosphorus are part of the ion
What Do Atoms Look Like?
Parts of an Atom
I can…
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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
Where the Electrons Live
I can…
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define the 4 quantum numbers (n, l, ml, ms)
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.
Electrons behave like waves and light
I can…
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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…
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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.
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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…
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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
Radioactivity—What is the Nucleus Like?
I can…
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list and describe three kinds of Becquerel rays that fly out of the nucleus
alpha, 
2 p+ 2 n
4
2
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He
beta, 
high NRG e-
gamma, 
high NRG light
0
1 e
0
0
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 (2 p+’s and 2 n’s are emitted)
o beta (beta negative) (n  p+ + -)
o positron (beta positive) (p+  n + +)
o gamma (nucleus changes from high energy to lower energy state and emits a photon of high energy light)
Is Radioactivity Dangerous?
I can…
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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?
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explain that radioactive nuclei decay randomly, but follow simple mathematical rules when considered collectively
Can 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
How Do Atoms Stick Together? (Bonding)
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name the three kinds of bonds: ionic, covalent, and metallic
describe each kind of bonding:
covalent—they share e-‘s between two atoms
ionic—they trade e-‘s (+ ion loses e-‘s while – ion gains e-‘s) and then they attract each other.
metallic—they share e-‘s among multiple atoms
state the kind of bond that will form between any two atoms
metal/nonmetal
metal/metal
nonmetal/nonmetal
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use electronegativity difference to predict the bond type
What Substances Use These Bonds?
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give examples of the three kinds of substances:
CH4, CO2, H2O, C2H5OH
Au, Ag, Ni, Zn, Cu, brass, bronze
NaCl, K2SO4, Al2S3, NaOH
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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.
metallic bond
metals
+ ions in a
“sea of e-‘s”
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covalent bond
molecules or
network solids
nonmetal atoms
ionic bond
ionic solids
(salts)
alternating + and 
ions
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?
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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