Unit2Day6-LaBrake
Monday, October 07, 2013
3:35 PM
Vanden Bout/LaBrake/Crawford
CH301
ELECTRONS and BONDING WRAP
UNIT 2 Day 6
CH301 Vanden Bout/LaBrake Fall 2013
Important Information
EXAM WEDNESDAY 7PM – 9PM
CH301 Vanden Bout/LaBrake Spring 2013
Unit2Day6-LaBrake Page 1
QUIZ: CLICKER QUESTION 1
Which of the of following is the electronic
configuration for K and K+ , respectively?
a)1s22s22p63s23p64s1 ; 1s22s22p63s23p64s1
a)1s22s22p63s23p64s1 ; 1s12s22p63s23p64s1
a)1s22s22p63s23p64s1 ; 1s22s22p63s23p6
a)1s22s22p63s23p64s1 ; 1s22s22p63s23p64s2
CH301 Vanden Bout/LaBrake Fall 2013
Relate electron configuration to periodic table
QUIZ: CLICKER QUESTION 2
A laser pulse shines for 10 s delivering a total energy
of 4 mJ of 633 nm light. Another laser delivers the same amount of
energy with a wavelength of 408 nm.
Unit2Day6-LaBrake
Pageto
2 the sample?
Which laser is delivering
more photons
QUIZ: CLICKER QUESTION 2
A laser pulse shines for 10 s delivering a total energy
of 4 mJ of 633 nm light. Another laser delivers the same amount of
energy with a wavelength of 408 nm.
Which laser is delivering more photons to the sample?
A)
B)
C)
D)
RED Laser
BLUE Laser
BOTH ARE THE SAME
NOT ENOUGH INFORMATION
CH301 Vanden Bout/LaBrake Fall 2013
QUIZ: CLICKER QUESTION 3 and 4
Each of these lasers shines on calcium ( = 2.90 eV).
What will happen when a 10 s pulse of red laser
shines on calcium?
a) NOTHING
b) Electrons will be ejected
c) Electrons will be ejected, but fewer than for the
blue laser
What will happen when a 10 s pulse of the blue laser
shines on calcium?
a) NOTHING
b) Electrons will be ejected
c) Electrons will be ejected, but there will be fewer
than for the red laser
CH301 Vanden Bout/LaBrake Fall 2013
Unit2Day6-LaBrake Page 3
2. Please explain the change in effective nuclear charge, Zeff ,
as you move across a row in the periodic table from left to right.
Indicate how this change in Zeff affects the ionization energy and
the atomic radii of the atoms as you move across a row.
Use the elements calcium and selenium as
specific examples predicting
which would have the smaller atomic nucleus and why.
CH301 Vanden Bout/LaBrake Fall 2013
EXPLANATION SPACE
CH301 Vanden Bout/LaBrake Fall 2013
Unit2Day6-LaBrake Page 4
QUIZ: CLICKER QUESTION 5
Please write out the electron
configuration for Germanium,
Ge,
using the noble gas short hand
method
a) [Ar]3s23p64s23d104p2
b) [Ar] 4s24p2
c) [Ar] 4s23d104p2
d) [Kr] 4s23d104p2
e) [Kr] 4s24p4
CH301 Vanden Bout/LaBrake Fall 2013
QUIZ: CLICKER QUESTION 6
Given that the correct electron configuration for
Germanium, Ge is: [Ar] 4s23d104p2
Which of the following sets of quantum numbers will not be
an allowed set for an electron in the ground state of Ge?
a) 1,0,0,½
b) 4,1,0,½
c) 3,1,1,½
d) 4,2,-2,½
e) 4,1,-1,-½
CH301 Vanden Bout/LaBrake Fall 2013
Unit2Day6-LaBrake Page 5
QUIZ: CLICKER QUESTION 6
Please draw the Lewis structure for the molecule,
oxalate ion, C2O42-.
The formal charge for each atom in the structure is correct in
which diagram?
CH301 Vanden Bout/LaBrake Fall 2013
QUIZ: CLICKER QUESTION 7
The concept of electronegativity refers to:
a)The notion that metals tend to lose electrons to form cations.
b)The notion that nonmetals have a greater affinity for electrons,
so will tend to form anions to achieve a noble gas type electron
configuration.
c)The notion that within the context of a covalent bond, an atom
which has a stronger affinity for electrons will attract the shared
pair to a greater extent.
d)The notion that covalent compounds share their bonding pairs
electrons equally between atoms producing pure covalent or non
polar type bonds.
CH301 Vanden Bout/LaBrake Fall 2013
Unit2Day6-LaBrake Page 6
CH302 Vanden Bout/LaBrake Fall 2012
What have we learned?
Electromagnetic radiation interacts with matter.
Understanding EM radiation, helps to understand matter on
the micro-scale. The physical model of the behavior of teeny
tiny things is quite complicated and difficult to understand.
The number of protons and the number and arrangement of
electrons is important for predicting the chemical
properties of the elements. You can abbreviate complicated
electron configurations using a series of numbers and letters.
The periodic table is your friend.
You can name compounds. You can understand the
structure
of ionic compounds. You can predict basic bonding in
CH302 Vanden Bout/LaBrake Fall 2013
molecules using Lewis structures.1
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