Course Calendar : Course Calendar SAT II PREP
Course Calendar : Course Calendar SAT II PREP
Course Calendar : Course Calendar SAT II PREP
Topics Covered : Topics Covered SAT II PREP Structure of Matter 25%
Atomic structure ?
Molecular structure ?
Bonding ?
States of matter 16%
Gases ?
Liquids & solids ?
Solutions ?
Reaction types 14%
Acids & bases ?
Oxidation-reduction ?
Precipitation ?
Stoichiometry 14%
Molec concept ?
Chemical equations ? Equilibrium & Reaction rates 5%
Equilibrium systems ?
Rates of reactions ?
Thermochemistry ? 6%
Descriptive chemistry ? 12%
Laboratory ? 8%
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Key terms
Subatomic particles
Neutron
Proton
Electron
Mass #
Atomic #
Line emission spectra
Isotope
Ions
Electronic configuration
Bohr model of atom
Quantum mechanical model
Principal quantum number
Angular momentum quantum number
Azimuthal quantum number
Magnetic quantum number
Spin quantum number Ground state
Excited state
s-orbital
p-orbital
d-orbital
Nucleus
Subshell
Heisenberg uncertainty principle
Pauli exclusion principle
Atomic mass unit
Atomic weight
Quantization
Rutherford
Thomson
Cathode ray tube
Gold foil experiment
Energy level
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Key concepts and skills
Be able to compare the mass, charge and location of the 3 subatomic particles.
Know the difference between mass number and atomic number.
Be able to calculate the atomic weight of an element when given information about the element’s isotopes.
Be able to determine the number of subatomic particles in atom from incomplete information about the element.
Be able to describe Bohr’s model of the atom.
Be able to describe Thomson, Dalton and Rutherford’s contribution to the development of the atomic model.
Know the 5 statements of Dalton’s atomic theory and be able to describe any shortcomings. Be able to explain how a line emission spectrum is created.
Be able to write electronic configurations for elements.
Be able to describe the 4 quantum numbers.
Be able to identify electron configurations for elements in the excited state.
Be able to write electron configurations for ions.
Be able to give the values of the quantum numbers for a given orbital.
Be able to list the types of light in the electromagnetic spectrum based on energy, frequency or wavelength.
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Subatomic particles
Electron mass = 0amu charge = -1 location: in orbitals
Proton mass = 1amu charge = +1 location: in nucleus
Neutron mass = 1amu charge = 0 location: in nucleus
Atomic number = protons in atom (and electrons in a neutral atom)
Mass number = protons + neutrons
2 notations to know:
C-12 (means the element Carbon with mass number 12)
Or
(where 6 is the atomic number and 12 is the mass number)
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Subatomic particles – sample questions
Determine the number of protons, neutrons and electrons in:
a. Nickel-58.
b. Nickel-602+
c.
d. Ca2+
Determine the numbers of each of the subatomic particles in:
a. An element with atomic number 5 and mass number 13
b. An element with mass number 37, with 17 electrons
3. How many neutrons are present in an atom of tin that has the atomic number 50 and a mass number of 119?
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Isotopes and atomic weight
Isotopes are atoms of an element that have the same number of protons but a different number of neutrons (and therefore different mass numbers)
To calculate the atomic weight of an element:
Atomic weight = (mass of isotope 1)(abundance of isotope 1) + (mass of isotope 2)(abundance of isotope 2)
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Isotopes and atomic weight- Sample questions
Element Q consists of 3 different isotopes, A, B and C. Isotope A has an atomic mass of 40amu and accounts for 60% of naturally occurring Q. The atomic mass of isotope B is 44amu and accounts for 25% of Q. Finally, isotope C has an atomic mass of 41amu and a natural abundance of 15%. What is the atomic weight of element Q?
The mass of a copper-63 atom is 62.94amu and that of a copper-65 atom is 65.93amu. Using this data and the abundance of these two isotopes, determine the average atomic mass of native copper. The abundance of copper-63 is 69.17%. The abundance of copper-65 is 30.83%.
Which of the following could represent a pair of isotopes?
a. b.
c. d.
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Bohr’s model of the atom
Bohr thought that in atoms electrons rotated around the nucleus in precise orbits.
Electrons could move from low energy orbits (close to the nucleus) to high energy orbits (further away) by absorbing energy.
When electrons moved back down to the low energy orbit they give off energy in the form of light.
The many electrons in a substance moving from high energy orbits to low energy orbits, giving off light energy creates lines of color in what is called a line emission spectrum.
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP The Quantum mechanical model of the atom
Electrons are found in 3D regions of space, called orbitals (not rings or orbits).
Orbitals are the region of space where the electron is likely to be found 90% of the time.
Orbitals in atoms have different shapes(s, p, d, and f), sizes and energies.
Electrons are described with 4 quantum numbers:
Principal quantum number (n), angular momentum quantum number(l), magnetic quantum number (ml)and the spin quantum number(ms)
There are rules that specify what values the quantum numbers can have:
n = 0, 1, 2, 3, 4…
l = 0, 1, 2, 3…(n-1)
ml = -l…0…1
ms = ±1/2
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP The Quantum mechanical model of the atom – sample questions
Calculate the maximum number of electrons that can occupy the 4th principal energy level.
Write the orbital diagram for Aluminum.
Explain what law the following configuration violates.
1s22s32p63s1
The maximum number of electrons with quantum numbers n = 2 and l = 1 in one atom is ____.
How many subshells are found in the 3rd principal quantum level?
How many orbitals are there in the 5d subshell?
The location of an electron is identified by the atomic orbital it is in. Which properties of an atomic orbital are specified by the first three quantum numbers?
a. Length, width, and height d. Size, exact location and velocity
b. Mass, speed and direction e. Color, frequency and wavelength
c. Size, shape and orientation
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Electron configurations
The order of the orbitals is: 1s 2s 2p 3s 3p 4s 3d 4p 5s
Each s-sublevel can hold 2 electrons
Each p-sublevel can hold 6 electrons
Each d-sublevel can hold 10 electrons
Electronic configurations can be written by filling in the electrons in the orbitals starting with the lowest energy.
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP Electron configurations – Sample problems
What is the lowest energy orbital in an atom?
Write the electron configuration for Boron.
Write the electron configuration for Ca2+
Write the electron configuration for copper.
Write the electron configuration for Cl-
6. Which of the following electron configurations corresponds to an excited state?
1s22s23p1
1s22s22p6
1s22s22p43s1
[Ar] 4s23d54p1
Which of the following is the ground-state electron configuration of an oxide ion?
a. 1s22s22p4
b. 1s22s22p5
c. 1s22s22p6
d. 1s22s22p63s1
e. 1s22s22p63s2
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP MORE PROBLEMS
Lesson 1 Atomic structure : Lesson 1 Atomic structure SAT II PREP MORE PROBLEMS
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Key terms
Halogens
Noble gases
Alkali metals
Alkaline earth metals
Metals
Nonmetals
metalloids
Period
Group/family
Valence electrons
Modern periodic law
Mendelev
S block
P block
D block
F block Octet rule
Atomic radius
Ionization energy
Electronegativity
First ionization energy
Electron affinity
Malleability
Ductility
Transition elements
Ionic radius
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Key concepts and skills
Know the periodic trends for: atomic radii, ionization energy, electronegativity, electron affinity, reactivity, boiling point, density.
Know the modern periodic law.
Know why elements in the same group have similar chemical properties.
Be able to determine the number of valence electrons an element has based on its position in the periodic table.
Know the location of metals, nonmetals and metalloids in the periodic table.
Know basic properties/characteristics of groups. Know the location or the s,p , d and f blocks in the periodic table.
Be able to determine an element’s valence electrons and ions formed from its position in the periodic table.
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Periodic trends
Electronegativity: increases from left to right and down to up.
Atomic radius: increases from right to left and up to down.
Ionization energy: increases from left to right and down to up.
Electron affinity: increases from left to right and from down to up.
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Periodic trends-sample questions
In which of the following pairs is the first element expected to have a higher electronegativity than the second?
a. O, P
b. Cs, Rb
c. I, Br
d. Al, P
e. Sb, As
In which pair of elements is the larger atom listed first?
a. K, Ca
b. Na, K
c. Cl, S
d. Mg, Na
e. O, N
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table
Elements in periodic table are ordered by increasing atomic number.
Elements in the same groups have the same number of valence e’s which explains why they have similar chemical properties.
The blocks of the table are s, d, p (from left to right).
S-block elements are Groups 1 and 2
D-block elements are in Groups 3-12
P-block elements are in Groups 13-18
To determine an element’s valence electrons:
For Group 1 and 2 group number = # valence electrons
For Group 13-18 group number -10 = # valence electrons
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table – sample questions
A solid element has 2 valence electrons. That element must be:
a. A halogen
b. A noble gas
c. A radioactive element
d. An alkali metal
e. An alkaline earth metal
The differentiating electrons for transition elements are:
a. D electrons
b. S electrons
c. P electrons
d. F electrons
e. Valence electrons
3. How many protons, neutrons and electrons are in an atom of Bromine?
Chemical properties of elements are defined by the____________.
a. Electrons
b. Ionization energy
c. Protons
d. Neutrons
e. electronegativity
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Structure of the table – sample questions
Which pair of elements is expected to have the most similar properties?
a. Potassium and lithium
b. Sulfur and phosphorus
c. Silicon and carbon
d. Strontium and barium
e. Fluorine and iodine
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP MORE PROBLEMS
Lesson 1 Nuclear chemistry : Lesson 1 Nuclear chemistry SAT II PREP Key terms
Nucleus
nuclide
Nucleon
Atomic number
Mass number
Isotope
Atomic mass unit
Nuclear binding energy
Mass defect
Radioactivity
Radioactive decay
Fusion
Fission
Daughter isotope
Parent isotope
Alpha particle
Alpha decay
Beta particle
Beta decay Gamma ray
Gamma decay
Positron emission
Electron capture
Half life
Exponential decay
Carbon dating
Decay constant
Transmutation
Nuclear chain reaction
Lesson 1 Nuclear chemistry : Lesson 1 Nuclear chemistry SAT II PREP Key concepts and skills
Be able to identify isotopes.
Be able to solve half-life and radioactive decay problems.
Be able to balance nuclear equations.
Know the key characteristics of the subatomic particles: positron, beta particle, alpha particle, gamma ray, etc.
Be able to classify nuclear reactions by looking at their equations.
Be able to explain mass defect and binding energy.
Be able to describe how the nucleus changes in different types of radioactive decay processes.
Be able to distinguish between fission, fusion, radioactive decay and transmutation.
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Subatomic particles
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Types of nuclear reactions
Beta decay Fission of uranium
Electron capture Fusion reaction
Positron emission
Alpha decay C 14 6 N 14 7 + e 0 -1 Cr 51 24 V 51 23 + e 0 -1 + ? Cr 49 24 V 49 23 e 0 +1 + U 238 92 Th 234 90 He 4 2 + U 92 n 1 0 + Ba 87 35 + La 146 57 + 3 n 1 0 235 H 2 1 He 4 2 + H 3 1 + n 1 0
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Types of nuclear reactions- sample questions
The radiation given off by iodine-131 in the form of beta particles is used to treat cancer of the thyroid gland. Write the nuclear equation to show what happens when an iodine-131 nucleus decays.
The decay of uranium-238 results in the spontaneous ejection of an alpha particle. Write the nuclear equation that describes this process.
When a radon-222 nucleus decays, an alpha particle is emitted. Write the nuclear equation to show what happens when a radon-222 nucleus decays. What is the other product that forms?
A fusion reaction that takes place in the sun is the combination of two helium-3 nuclei to form 2 hydrogen atoms and one other atom. Write the balanced nuclear equation for this fusion reaction. Be sure to include both products that are formed.
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Balancing nuclear equations
The total of the superscripts on the left side of the equation must equal the total of the superscripts on the right side of the equation.
The total of the subscripts on the left side of the equation must equal the total of the subscripts on the right side of the equation.
Summary of effect of different nuclear changes
Emission of a beta particle: increases atomic number by one but does not change the mass number.
Emission of a positron: decreases the atomic number by one but does not change the mass number
Electron capture: decreases the atomic number by one but does not change the mass number
Alpha decay: decreases atomic number by 2 and the mass number by four.
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Balancing nuclear equations – sample questions
Write balanced equations for the following nuclear reactions:
a. Uranium-233 undergoes alpha decay.
b. Copper-66 undergoes beta decay.
c. Beryllium-9 and an alpha particle combine to form carbon-13. The carbon-13 nucleus then emits a neutron.
d. Uranium-238 absorbs a neutron. The product then undergoes successive beta emissions to become plutonium-239
2. Write in the missing particle in the following nuclear reactions. Mn 55 25 n 1 0 + He 4 2 + Np 239 93 Pu 239 94 + C 11 6 B 11 5 + Li 6 3 n 1 0 + He 4 2 + U 235 92 n 1 0 + Ba 139 56 + Fr 94 36 + 3
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Half-life and radiactive decay calculations
Half life is the time required for one half of a radioactive sample to completely decay.
Two equations to know:
N/No = e-kt N is the amount of the radioactive sample at some later time, t. No is the original amount of the radioactive sample.
k is the rate constant
t is the time that the sample decays for
t1/2 = 0.693/k k is the rate constant
Lesson 1 Nuclear Chemistry : Lesson 1 Nuclear Chemistry SAT II PREP
Lesson 1 Periodic table : Lesson 1 Periodic table SAT II PREP Half-life and radiactive decay calculations- Sample questions
Part A Simple ½ life problems
A radioactive substance has a half-life of 20 minutes. If we begin with a 500 g sample, how much of the original sample remains after two hours?
How much of a 100.0g sample of Au-198 is left after 8.10 days if gold’s half-life is 2.70days?
After a 50.0g sample of N-16 decays for 14.4 seconds 12.5g of the original sample remains. What is N-16’s half-life?
Part B ½ life problems that require equations & calculation
The half-life of Ag-104 is 16.3 min. What is the rate constant in units of reciprocal seconds (s-1)?
Bromine-82 has a half-life of 35.7 hours. How many milligrams of Br-82 will remain if 2.30g of Br-82 decays for exactly one week?
After 3.24 hrs 75% of a radioactive substance is left. What is the rate constant in units of reciprocal hours?
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Key terms
Molecule
Chemical bond
Valence electrons
Intermolecular forces
Intramolecular forces
Octet rule
Ionic bonds
Covalent bonds
Polar covalent bonds
Cations
Anions
Polyatomic ions
Double bond
Single bond
Triple bond
Bond length
Bond energy
Lewis structures Formal charge
Resonance structures
Partial charge
Nonpolar covalent bonds
Coordinate covalent bonds
VSEPR
Linear
Trigonal planar
Tetrahedral
Trigonal bipyramidal
Octahedral
Dipole moment
Hybridization
sp hybridization
sp2 hybridization
sp3 hybridization
Sigma bond
Pi-bond W
o
r
d
s
2
k
n
o
w
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Molecule Chemical bond Valence
electrons Intermolecular forces Intramolecular forces Octet rule Ionic bonds Covalent bonds Polar
covalent
bonds Cations Anions Polyatomic ions Double bond Single bond Triple bond Bond length Bond
energy Lewis structures Formal
charge Resonance
structures Partial
charge Nonpolar
covalent
bonds Coordinate
covalent
bonds VSEPR Linear Trigonal
planar Tetrahedral Trigonal
bipyramidal Octahedral Dipole
moment Hybridization sp
hybridization sp2
hybridization sp3
hybridization Sigma bond Pi-bond Concept Map
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Key concepts and skills
Be able to draw lewis structures (and resonance structures when necessary).
Be able to explain why some covalent bonds are more or less polar than others.
Be able to determine formal charges on atoms in a molecule.
Know the octet rule.
Be able to draw lewis dot diagrams for ions.
Know the most likely ions formed by main group elements.
Know what kinds of bonds (pi/sigma) make up single, double and triple bonds.
Be able to predict whether a molecule will be polar or not. Be able to predict the shapes of molecules.
Be able to explain the differences between nonpolar and polar covalent bonds.
Know the relative bond energies and length for single, double and triple bonds.
Know the naming system for ionic and molecular compounds (know names of common polyatomic ions). Be able to do
these things.
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Bond Polarity
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Bond Polarity
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Polyatomic Ions PO43- CO32- PO33- NO3- SO42- HCO3- ClO4- ClO3- phosphate chlorate sulfate perchlorate carbonate nitrate phosphite hydrogen carbonate
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dots P O2- F- N S H Cl C
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dot structures for molecules
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dot structures for molecules O2 CO NH3 CO2 BCl3
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Lewis dot structures & resonance CO32-
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP VSEPR theory predicts shapes of molecules
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP 4 sp3 hybrid orbitals
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP 3 sp2 hybrid orbitals
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals Bonding in Ethene C2H4
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals 2 sp hybrid orbital
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals Bonding in Ethyne C2H2
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals
Lesson 5 Chemical Bonding : Lesson 5 Chemical Bonding SAT II PREP Hybridization- mixing of orbitals
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Sample Problems
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Sample Problems
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Sample Problems
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Solutions
to problems
Lesson 5 Chemical bonding : Lesson 5 Chemical bonding SAT II PREP Solutions
to problems