Download Unit 2 Review KEY

CP Chem
Ms. Lummis
Unit 2 Exam Review 1 Worksheet KEY
Electromagnetic Radiation – form of energy that exhibits wavelength behavior as it travels
through space.
Wavelength (λ) – the distance between corresponding points on adjacent waves.
Frequency (v) – number of waves that pass a given point in a specific time (1 sec)
Photoelectric Effect – an emission of electrons from a metal when light shines on a metal.
Quantum – minimum quantity of energy that can be lost or gained by an atom.
Photon – particle of electromagnetic radiation having zero mass and carrying a quantum of
energy.
Heisenberg uncertainty principle – it is impossible to determine at the same time both the
position and the velocity of an electron or any other very small particle.
Quantum theory – describes mathematically the wave properties of electrons and other very
small particles.
Orbital – the region of space where it is most likely to find an electron (90%)
Principal Quantum number(n) - the main energy level.
Angular Momentum Quantum Number (l) - the energy sublevel. It indicates the shape of
the orbital, s, p, d, f.
Magnetic Quantum Number (m) - indicates the orientation of the orbital.
Magnetic Spin Quantum Number(s) - fundamental spin state of an electron in an orbital.
Aufbau Principle – the electron occupies the lowest-energy orbital that can receive it.
Pauli Exclusion Principle – no 2 electrons in the same atom can have the same set of
quantum numbers.
Hund’s Rule – orbitals of equal energy are each occupied by one electron before any orbital is
occupied by a second electron. All electrons in singly occupied orbitals must have the same
spin state.
Directions: use the diagram below of the Bohr model to help answer the following
questions:
1.
Which letters correspond to energy levels? A, B, D
2.
What type of particles are allowed to exist in these energy levels? electrons
3. Which letter represents an orbit with the lowest energy state? A
4. Which letter represents a point where electrons could not reside, according to the
Bohr model. C
5. Explain what these orbitals represent, according to quantum theory. Principal
quantum number.
Fill in the following table:
Sublevel
# of Orbitals
Max # of Electrons
s (0)
Description
of shape
sphere
1
2
p (1)
dumbbell
3
6
d (2)
cloverleaf
5
10
f (3)
complex
7
14
Directions: Answer the following questions regarding an atom with the electron
configuration 1s22s22p6. (Note: this is an example)
How many electrons are present in this atom? 10
What element is this atom? Neon
How many of this atom’s p orbitals are completely filled? 3
How many unpaired electrons are there in this atom? 0
How many inner-shell electrons does this atom have? 2
Write the electron configurations and Noble gas notation of the following elements:
Li
1s22s1
[He] 2s1
Mg 1s22s22p63s2
[Ne] 3s2
As 1s22s22p63s23p64s23d104p3
[Ar] 4s23d104p3
Mo 1s22s22p63s23p64s23d104p65s24d4
Ba
1s22s22p63s23p64s23d104p65s24d105p66s2
S
1s22s22p63s23p4
K
1s22s22p63s23p64s1
[Kr] 5s24d4
[Xe] 6s2
[Ne] 3s23p4
[Ar] 4s1
Write the orbital notations for Li, S, K and As: DO NOT DO THIS ONE
_____+1/2 ___ -1/2__________ The spin quantum numbers are what 2 numbers?
_____2_______ If you are in the second energy level, what orbitals are there?
___4:____s__p__d___f__ On the 4th energy level, how many sublevels are there?
___________6____________ How many electrons can be found in the p-orbitals?
_________14____________ How many electrons are found in the f-orbitals?
_____s___p___d____f_____ If you are in the fifth energy level, what orbitals are there?
_____spherical___________ What is the shape of the s-orbital?
_________s_________Which orbital can be found at every energy level?
_______dumbbell_________ What shape are the p-orbitals?
Draw the arrow diagram: See your notes