Light
Periodic
Trends
Electronic
Electron
Mixed Bag
Structure Configuration
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Mixed Bag
Which element
has the electron
configuration
2
2
6
2
3
1s 2s 2p 3s 3p ?
If you add up the
exponents, there
are 15 electrons
which corresponds
to phosphorous.
Home
What is the difference
between the ground
state and the excited
state for an electron?
The ground state is the
lowest energy level for an
electron; the excited state is
when an electron is at an
energy level above its
normal state (the excited
state is temporary).
Home
How many valence
electrons does carbon
have in it’s outer
shell?
C=
2
2
2
1s 2s 2p
The second energy level is
the outside shell in this
case. There are
4 electrons in the second
energy level (valence shell)
for carbon.
Home
What is wrong with the following
orbital diagrams? Which
rules/principles do they violate?
1)
2)
***Violates Hund’s Rule – electrons won’t
pair up within a sublevel until they have to!
**Violates Hund’s Rule & Aufbau Principle:
electrons must completely fill lower energy
sublevels before filling higher energy
sublevels
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How many unpaired electrons
are in a bromine atom?
How does this relate to the
charge on a bromide ion?
Bromine has 1 unpaired
electron in it’s orbital
diagram which makes sense
since bromide ions have a
charge of -1 (they have
gained 1 e to complete their
valence shell).
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Periodic
Trends
Which atom would
have the largest
ionization energy –
Mg or Cl?
Chlorine would have
the largest I.E. because
it is farther right on the
periodic table
(e- are held closer so it
will be harder to rip the
e- off)
Home
Define the term
“electron
affinity”
The energy involved
when an atom gains an
electron.
(The opposite of
ionization energy)
Home
Rank the following
elements in order
of increasing
atomic radius:
In, Al, B, Ga
B < Al < Ga < In
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Rank the elements
in order of
increasing metallic
character:
N, Zr, Cs, Co
N < Co < Zr < Cs
Home
Describe the
comparative size of
a cation compared
to the atom from
which it forms.
Cations are smaller than
the atoms from which
they form due to the
increasing
proton/electron
attraction due to the loss
of electrons. Home
Electron
Configuration
What is the
electron
configuration for
cobalt?
Co =
2
2
6
2
6
2
7
1s 2s 2p 3s 3p 4s 3d
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What is the noble
gas configuration
for zirconium?
Zr =
2
2
[Kr]5s 4d
Home
What is the orbital
configuration for
sulfur?
(i.e. Draw an orbital diagram)
1s
2s
3s
2p
3p
Home
What is the electron
configuration for
iridium?
Ir =
2
2
6
2
6
2
10
1s 2s 2p 3s 3p 4s 3d
6
2
10
6
2
14
7
4p 5s 4d 5p 6s 4f 5d
or
2
14
7
[Xe]6s 4f 5d
Home
What do the
coefficient, letter, and
exponent signify
when writing electron
configurations?
(Not just the relation to the periodic table!)
Coefficient = principal
energy level
Letter = sublevel
Exponent = # of
electrons in sublevel
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Electronic
Structure
What are the 3-D shapes
of the atomic orbitals
comprising the s, p, d,
and f sublevels?
(Think about what the letters stand for)
s = sphere
p = peanut
d = dumbell (clover)
f = flower
Home
Which sublevels (s, p,
d, or f) are located in
the fifth principal
energy level?
The fifth energy level
has s, p, d, and f
sublevels present.
Home
How many total electrons
can fit into the third
principal energy level?
(Taking into account all
sublevels present)
The third energy
level contains s, p,
and d sublevels so
2 + 6 + 10 =
18 total electrons!
Home
How do you draw
arrows in an orbital
diagram and why are
they drawn that way?
Arrows are drawn with the
first pointing up and the
second pointing down due
to the Pauli Exclusion
Principal (electrons must
have opposite spins in the
same orbital).
Home
Define the Aufbau
Principle and how it
relates to the electrons
in an atom.
The Aufbau Principle
says that electrons
completely fill from the
lowest energy level to
the highest energy level.
Home
Light
What is meant by
the statement:
“Light has a dual
nature”
Light behaves as
both a particle and a
wave.
Home
What is the
wavelength of a
portion of light
having a frequency
12
of 4.73 x 10 Hz?
Use c = λν…
λ = 6.34 x
-5
10
m
Home
Calculate the
energy of a photon
of light having a
frequency of
13
3.11 x 10 kHz.
Use E = hv…
E = 2.06 x
-17
10 J
Home
What is the wavelength (in
nanometers!) of a portion
of light having an energy of
-12
1.44 x 10 J?
Use both light equations or
E = hc/λ!
First calculate the frequency…
21
v = 2.17 x 10 Hz
Then use v to find λ…
λ = 1.38 x
m=
-4
1.38 x 10 nm
-13
10
Home
Describe why you saw
colors in the flame
during the flame test lab
(think about what is
going on with the
electrons)
As the element samples are
placed in the flame, the electrons
are given energy so they jump
from the ground state to the
excited state. When the electrons
go back down to the ground state,
they emit this extra energy which
we see as light (the color depends
on the λ and v).
Home
Final Jeopardy
What is the electron
configuration for a
chloride ion?
Final Jeopardy
Chloride would be isoelectronic with
argon after gaining one electron to
form the Cl ion (they have the same
number of electrons although they
have different numbers of protons).
-1
Cl
=
2
2
6
2
6
1s 2s 2p 3s 3p