Here
is how we play the homework game in AP Chemistry. I am more than willing to take care of your
grade if you are willing to do the work I ask.
Homework needs to be completed and turned in ON TIME. If you do not turn it in on time, it will go
in as a ZERO, if turned in late it will be lowered 10% each day!! This would be bad since most assignments are
worth around 100 points easy. REMEMBER
TO NOT WRITE IN THE BOOK!!! I suggest:
1. Read the chapter over the span of a few days
and make a general outline for the chapter.
2. Try to answer the summary questions based on
that outline, looking up answers in the book when necessary. Even though the outline and the chapter
summary questions may overlap, they both need to be done and both will be
scored.
3. Answer the exercises assigned from the book
as you are reading the chapter. These
should be done in order on a separate piece of paper and be neat
so that I can follow them and score them easily. You don’t want me grading angry, yo.
CIRCLE
any ones you have questions on - when we go over it later you want to be able
to remember which ones were weird.
4. At the end of the chapter, answer the
multiple choice questions, GRADE THEM,
and circle ones that you have
questions on so I may address any that you still do not understand when I see
you in class. Do the same with the free
response. These will be for points. Show work and actually try them please –
don’t just copy them and write down the answers – this is not helping you at
all. I am not the homework police – you
need to take responsibility for your education when working the assignments. I can tell if you are just copying stuff down
- I am not a moron.
5. Use a calculator and the formula sheet that
is given in the book. You need to become
familiar with the equations they will give you because it helps us tell what
questions that could choose. You can use
a calculator on the free response, but not on the multiple choice section -
they removed that option last year.
Thanks a lot!
JUNE HOMEWORK SET #1 Name:
CHAPTER 1 - structure of the atom
Chapter
1 Book Assignments: your score: /95
pts
ASSIGNMENT 1: _____ /27 points
|
Due Date
|
Your pts/total
|
Read pages 79-89
|
||
Create “smart guys list” – from summary
sheet
|
/17
|
|
Outline Ch 1: structure of the atom for part I
|
/10
|
|
Read Part II pages 89-97
|
||
ASSIGNMENT 2: _____ /68 points
|
||
Outline Ch 1: structure of the atom for part II
|
/10
|
|
Answer Block’s summary sheet
|
/22
|
|
AP Practice Quiz pgs 100-103 – GRADE
IT!!!
|
/26
|
|
Free response page 104
|
/10
|
Chapter
1 Homework Assignments: your score: /110 pts
Assignment:
|
Your pts/total
|
Quantum Numbers worksheet
|
/35
|
Para/Diamagnetic worksheet
|
/20
|
Ch 1 crib notes review
|
/10
|
Diagnostic
Test #1: take it and grade it!! (Completion)
|
/45
|
Chapter 1 TOTAL PTS: your score: /205 pts
Block’s Summary Sheet: Chapter 1:
Structure of the atom – 22 pts
This is different than your outline. Both must be completed for points!!
1. List
and describe the 4 laws about the atom.
(4 pts)
2.
Make a separate list of the 17 smart guys, their discoveries in order
with years,
and their significance
on your smart guys sheet. (smart guys list)
3.
Compare the three subatomic particles’ masses and charges. (3 pts)
4.
List the 3 equations regarding ENERGY and electromagnetic radiation,
noting
what each
variable stands for, the units, and rearrange the equations. (3 pts)
5.
List the constants for these 2 equations. (2 pts)
6.
Note and write the equation for the energy of an orbit that is given on
the AP
Test.
What does “n” stand for in that
equation? (2)
7.
Discuss the difference between the Bohr model versus the wave model. (1)
8.
List the four quantum numbers, how to assign them, and give examples of
each. (4 pts)
9.
Write the Aufbau Principle. (1 pt)
10. List the five common elements that
are exceptions to the Aufbau
Principle and
write their configurations. (2 pts)
CH 1. Para Vs. Diamagnetic/Quantum Numbers Name:
20 points
Short-hand notation: use [noble gas before it], then:
s-block:
ns1 or ns2
p-block:
ns2np 1-6
d-block:
ns2(n-1)d1-10
1. Write the symbol and electron configuration
notation for:
potassium
carbon
manganese
tantalum
2. Write the symbol and the shorthand notation
for:
francium
platinum
lead
osmium
n = levels or periods = 1 thru 7
l = sublevels or blocks = s = 0, p = 1, d = 2,
f = 3
m = rooms in the sublevel s = 0, p = -1,0,+1, d = -2,-1,0,+1,+2, f =
-3,-2,-1,0,+1,+2,+3
s = spin, either up +1/2 or down -1/2
3. Draw the symbol and the last orbital box for
these elements. Then write the four
quantum numbers for the last electron in that element:
beryllium
lithium
nitrogen
molybdenum – it is a
jumper!!!!
In a DIAMAGNETIC ELEMENT: all of the electrons are spin-paired so their
sub-shells are completely filled, causing them to be unaffected by magnetic
fields
In a PARAMAGNETIC
ELEMENT: they are strongly affected by
magnetic fields because their sub-shells are NOT completely filled with
electrons.
4. Which of the elements is diamagnetic?
5. Which of the elements is paramagnetic?
Quantum Number Activity Name:
35 points
Here are the
quantum numbers for He thru Ca. Draw the
orbital boxes for each to show where the last electron of that element is.
Designate
each of the following sets of quantum numbers as possible or impossible
according to the above. If the set of
quantum numbers is NOT possible, circle the one that makes it so. If the set of quantum numbers IS possible,
draw the orbital box for the last electron of that element. Do your work here:
Chapter 1 Crib Notes – THE ATOM Name:
10 points
Dalton: Atomic Theory and the Law of Multiple
Proportions
Bohr: “solar
system of orbits” atomic model
N = principal quantum number, orbits, periods, levels (1
thru 7)
L = AKA “azimuthal” quantum number, blocks, shape of the orbitals,
sublevels (s=0, p=1, d=2, f=3)
|
Ml
= magnetic quantum number, orientation of the orbitals, the boxes have
assigned numbers:
Ms=spin quantum number of the electron in that
orbital (+1/2 or -1/2)
Diamagnetic = all
subshells are filled/paired with electrons, elements are NOT affected by a
magnet (all electrons are paired)
Paramagnetic =
all subshells are NOT completely filled/paired with electrons, elements will be
affected by a magnet (some electrons are unpaired)
Rutherford: discovered the nucleus using his gold foil
experiment which led to his discovery of the proton, and he also separated
radiation into alpha, beta, gamma rays using a magnet.
Thomson
discovered the electron using his cathode ray tube experiment and Millikan found the charge and mass of
that electron suing his oil drop experiment.
Chadwick
discovered the neutron when bombarding a beryllium atom with alpha particles –
what fun!
deBroglie –
wave/particle nature of light
Rydberg equation: related energy with the level the electron is
on: En = -2.178 X 10 -18
J
n 2
The jumpers are: Ag, Au, Cr, Cu, Mo
Short-hand notation: use [noble gas before it], then:
s-block:
ns1 or ns2
p-block:
ns2np 1-6
d-block:
ns2(n-1)d1-10
Anytime you see the word “ENERGY” you need to bring out these equations:
c = lѵ c = speed of light = 3 X 108
m/s l= wavelength ѵ = frequency
E = hѵ so: E
= hc/ ѵ
h = Planck’s constant = 6.626 X 10 -34 Js
1 m = 1 X 109 nm – need to convert anything
meters to nm to find the color of the visible light
Blue = low wavelength, high frequency, high energy, 350 –
450 nm
Red = big wavelength, low frequency, low energy, 650 - 750
nm
Free response
question: write on a separate sheet of
paper and attach to this sheet: 10 pts
1. Write the complete
and shorthand electron configuration notation for copper and give the set of 4
quantum numbers for its last electron. (HINT: pour it all out there)
2. Be sure to write
it as a jumper cuz it is.
