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Chemistry
Chapter 5
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Chapter 5.1 - Light and Quantized Energy - p. 134
Positive charge and all mass in nucleus w/ electrons
1. What did Rutherford propose about the structure of
around
an atom?
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2. Draw a sketch of a wave as shown in Fig. 5.2 on p.
137. Be sure to label wavelength and amplitude.
wavelength
→|
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| ←-- amplitude
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3. What is the definition, Greek symbol, and unit of
measurement for:
a) wavelength =shortest dist between equivalent
points on wave. λ. m
b) frequency= number of waves that pass a given
point in a given amt of time. ν. Waves/sec
4. What is the symbol and value of the speed of light?
c. 3 x 108m/s
5. What is the relationship between frequency and
wavelength?
c = λν
6. What is the relationship between energy and the
frequency of electromagnetic radiation?
E = hν h= Planck’s constant
7. Look at Fig. 5.5 on p. 139. List the different
segments of the electromagnetic spectrum in order
from shortest wavelength to longest wavelength.
8. What could the wave model of light not explain?
(p.141)
9. What is a quantum?
10. What is an analogy for Planck's theory of
quantized energy? (p. 142)
11. What is a photon? What is the dual nature of
light?
12. Define atomic emission spectrum. What color do
strontium atoms emit in a burner flame?
gamma rays, x rays, ultraviolet, visible, infrared,
microwaves, radiowaves
why objects only emit certain frequencies of light at
a given temp
a small specific amount of energy. (min energy
gained or lost by an atom)
building a wall with bricks. Gets bigger or smaller in
the increment the size of the brick
bundle of light energy.(a quantum of energy in
massless package)
a series of lines produced by the light emitted when
electrons move from one energy level to another
Chapter 5.2 - Quantum Theory and the Atom .
1. How did Bohr suggest electrons move in a
hydrogen atom?
2. What is an atom's ground state?
3. What are two reasons given for why Bohr's model
was not correct?
electrons move only in specific circular orbits.
While there are many different orbits they can only
occupy one at a time. They will gain energy to jump
to higher orbit and lose energy to fall to lower
lowest energy for atom (all electrons in orbits closest
to nucleus)
couldnot explain other atom’s spectra
couldnot account for chemical behavior of atoms
that these particles can have wave properties
4. What was De Broglie's idea about the nature of
electrons?
5. What is the Heisenberg uncertainty principle? What
does this mean for the positions of electrons in atoms?
we can not know both the location and the speed of
an electron.
we cannot assign fixed paths to the movement of the
electrons
6. What is an atomic orbital?
a three dimensional region around nucleus
describing electron’s probable location.( solved
wave equation)
7. Explain the relationship between principal energy
levels and energy sublevels. (p. 153)
8. What are the shapes of s and p orbitals? How many
electrons can a single orbital hold?
principle = size and energy of orbital
sub = general shape of orbitals
s = spherical
p= dumbbell
Chap 5.3 - Electron Configuration - p. 156
1. What is an atom's electron configuration?
arrangement of electrons around nucleus. (placement
in levels and sublevels)
2. State the aufbau principle.
each electron will occupy the lowest energy level
(orbital) available. (electrons fill from low energy
levels to high)
3. What is the Pauli exclusion principle? How do we
represent an electron's spin?
Any orbital can hold 2 e- at the maximum, and if
there are 2 they must spin in opposite directions
Vector arrows are used to designate spin↑↓
4. What is Hund's rule?
When electrons fill degenerate(identical)
orbitals(p’s d’s or f’s) each orbital must have one
electron before any orbital has two
(electrons stay unpaired as long as possible)
5. Using sodium as an example, provide the electron
configuration and orbital diagram. (p. 159)
1s2 2s2
↑↓ ↑↓
6. What are valence electrons?
electrons in outer level
7. Who was the American chemist that devised
electron dot structures and when did he first use them?
Lewis. Used them while teaching college chemistry
8. What is the electron dot structure for Fluorine? for
Chlorine?
.
.
: F : : Cl :
..
..
2p6
3s1
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