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%
Unit 1 Atomic structure : Unit 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
Unit 1 Atomic structure : Unit 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 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. 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.
Unit 1 Atomic structure : Unit 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)
Unit 1 Atomic structure : Unit 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
Unit 1 Atomic structure : Unit 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)
Unit 1 Atomic structure : Unit 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?
2. 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%.
Unit 1 Atomic structure : Unit 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.
Unit 1 Atomic structure : Unit 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
Unit 1 Atomic structure : Unit 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?
Unit 1 Atomic structure : Unit 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.
Unit 1 Atomic structure : Unit 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-
Which of the following electron configurations corresponds to an excited state?
1s22s23p1
1s22s22p6
1s22s22p43s1
[Ar] 4s23d54p1
Unit 1 Atomic structure : Unit 1 Atomic structure SAT II PREP
Unit 1 Atomic structure : Unit 1 Atomic structure SAT II PREP