Download Honors Chemistry Ms. K Pages 66

Name______________________ #_____
Period___
Honors Chemistry
Ms. K
Pages 66-95
Task Checklist:
Look at Online Textbook Materials
Look at Section 1 Visual Concepts
Look at Section 2 Visual Concepts
Look at Section 3 Visual Concepts
Take Section 1 Self-Check Quiz
Take Section 2 Self-Check Quiz
Take Section 3 Self-Check Quiz
Do the Composition of the Atom Concept Map
Look at the Sample Problems for Section 3
Other Tasks
Read Section 1
Read Section 2
Read Section 3
Review Chapter Packet
Examine Class Website
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
THOMSON’S EXPERIMENT REVISITED
While Fred was babysitting his younger brother, Phil, he noticed that Phil was trying to stick a magnet
on the screen of their black-and-white television. The magnet did not stick to the glass, but the picture
seemed to be distorted. The closer he held the magnet to the screen, the more the images bent. Fred
asked Phil if he could try an experiment with the magnet. When Fred touched the magnet to the
screen, the image curved away from the magnet in one direction. When he turned the magnet around
and tried again, the image curved away in the other direction. When he waved the magnet back and
forth across a part of the screen, the distortion in the images followed the magnet. (CAUTION: Do not
try this activity on your own television screen at home.)
1. The image on the television screen is produced when electrons hit the phosphorus coating and cause
it to glow. Why did Fred?s magnet affect the image on the screen?
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2. Why did the image curve away from the magnet in a different direction when the magnet was
reversed?
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3. If Fred had two bar magnets, could he have placed them near the screen without causing any
distortion in the image? Explain.
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4. Describe the effects a stronger magnet would have had on the television image.
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5. Speculate about how the television controls the electron beam that is continually scanned across and
down the screen.
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Name_____________________________ #_____
Date______________________ Period_________
Einstein?s Big Idea
Science is a human endeavor undertaken by many different individuals of various social and ethnic
backgrounds who carry out their science in the society in which they live. Choose one of the following
scientists or pair of scientists: (Circle your choice.)
o
o
o
o
o
o
o
Michael Faraday
Antoine-Laurent and Marie Anne Lavoisier
James Clerk Maxwell
Emilie du Châtelet
Albert Einstein
Otto Hahn and Fritz Strassman
Lise Meitner and Otto Robert Frisch
Answer the following questions:
1. What is the nationality of this scientist (or nationalities)? _____________________________
2. Describe the society and times in which each scientist lived.
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3. How was science viewed by the society in which each scientist lived? What tools and techniques were
available to the different scientists? How did scientists collaborate and share information in each time
period?
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4. Albert Einstein died in 1955. If he were alive today, what do students think would surprise, delight, or
horrify him about the technologies and modern developments that stem from his
equation?_______________________________________________________________________________
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Ms. K
Honors Chemistry
Name_____________________________________ #________
Date________________________ Period________
Subatomic Particles Table
Symbol
1
Name
Mass #
Atomic #
48
22
e-
Charge
U
iodine-127
3
4
0
20
39
K+
21
18
34
29
potassium 39 ion
6
7
no
238
2
5
p+
29
27
Al+3
8
56
26
0
9
82
35
0
10
sulfide-32 ion
Ms. K
Chemistry
Name_____________________________________ #________
Date________________________ Period________
Subatomic Particles Table #2 (Try again)
Symbol
Name
Mass #
Atomic #
e-
Charge
H
2
fluorine-19
3
36
4
48
235
6
6
0
92
5
chloride-35 ion
7
6
17
1
H+1
8
lithium-7 ion
9
argon-40
10
no
2
1
7
p+
87
38
38
0
Ms. K
Chemistry
Name__________________________ #___
Date_______________________ Period___
Atomic Mass Worksheet Introduction: Atoms are very small. If we reported the mass of these atoms in grams, it would be a
very small number. Scientists use a relative scale to report the masses of these atoms. The standard
for this relative scale has been chosen as the carbon-12 isotope. Carbon-12 has been arbitrarily
assigned a mass of exactly 12 atomic mass units or amu.
atomic mass unit (amu) ? 1/12 the mass of a carbon-12 atom
The atomic mass of any atom is determined by comparing the mass of that atom to the mass of carbon12.
isotope
hydrogen-1
oxygen-16
magnesium-24
atomic mass
1.007825 amu
15.994915 amu
23.985042 amu
There are often many isotopes of the same element. For example, hydrogen has two isotopes
that occur naturally, H-1 and H-2. However, they do not exist in the same abundance?it isn?t 50% of
one and 50% of the other. H-1 occur 99.9885% of the time and H-2 occurs 0.0115% of the time. To
find the average mass of these isotopes, you wouldn’t add up their individual masses and divide by two
(it is not 50/50). You have to take into account their % abundance.
average atomic mass ? the weighted average of the atomic masses of the naturally occurring isotopes
of an element
average atomic mass =
∑ (atomic mass of each isotope x percentage natural abundance as a decimal)
This is the number seen on the periodic table. It is a weighted average. Looking at the table, the most
common isotope can often be determined from the atomic mass. For example, oxygen?s atomic mass
is 15.9994 amu. This is so close to 16 that one would believe that the oxygen-16 isotope is in greatest
abundance, and it is.
Example: Calculate the atomic mass of Li using the following data:
isotope
Li-6
Li-7
atomic mass
6.0151 amu
7.0160 amu
percent abundance
7.42
92.58
Answer:
atomic mass = (6.0151amu x 0.0742) + (7.0160amu x 0.9258)
=
0.446amu
+
6.495amu
= 6.941amu
(Use significant figures!)
Problems: Using the data in your book on page 82, calculate the atomic masses for both oxygen and
carbon. Check your answers with the periodic table ☺
Ms. K
Chemistry
? + 42 He →
17
8
Name__________________________ #______
Date______________________ Period_______
O + 11 H
Help for problem 4
Particle
alpha
Symbol
4
He or 4α
2
0
-1
0
0
beta
2
β or -10 e
γ
gamma
1. The reaction of an α particle with magnesium-25 produces a proton ( 1 H ) and a nuclide of another element.
1
Identify the new nuclide produced.
25
12
Mg + He → H + ?
4
2
1
1
2. The first radioactive element that was found, naturally occurring polonium, was discovered by the Polish
scientist Marie Curie and her husband, Pierre, in 1898. It decays by alpha emission. If polonium-212 was used,
what would be produced? (Write the nuclear equation for this process.)
3. Technetium, a radioactive element that does not occur naturally on the earth and was first prepared in 1937,
decays by beta emission. In beta emission, a neutron in the nucleus changes into a proton (that remains in the
nucleus) and an electron (beta particle) is ejected. If 98 Te decays by beta emission, what would be produced?
43
(Write the nuclear equation for this process.)
4. The first element prepared by artificial means was prepared in 1919 by bombarding a sample of atoms with
alpha particles. If the nuclear equation shows that oxygen-17 and 1 H was produced, what is the sample of
1
atoms that was bombarded? (If this is too hard for you, peek at the top to get some help.)
5. When a plant dies, it stops photosynthesis and its carbon-14 isotopes begin to decay by beta emission.
Carbon-14 decays with a half-life of 5730 years. How many years have passed if a 100.g sample of carbon-14
has decayed to 12.5g of carbon-14?
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
Molar Mass Practice
1. Calculate the molar mass of the following:
Ex: CO2
______44.01 g/mol____
FeSO4
____________________
Ca(C2H3O2)2 ____________________
N2
____________________
Au
____________________
(NH4)3PO4
____________________
NaNO3
____________________
2. If you had 88.02 g of CO2, how many moles of CO2 would you have? __________
3. Why can you call 12.01 g/mol the atomic mass or the molar mass of carbon, but you CAN?T call
44.01 g/mol the atomic mass of carbon dioxide, just the molar mass of carbon dioxide?
What is the difference between the words atomic mass and molar mass?
Ms. K
Chemistry
Name__________________________ #______
Date______________________ Period_______
Conversions Using the Mole
1. How many moles of atoms are in 45.0g of gold?
2. How many grams are in 1.53 mole of carbon?
3. In photosynthesis, plants use energy from the sun to combine carbon dioxide and water, forming glucose and oxygen.
How many moles of glucose are 90.0g of glucose?
4. Milk of magnesia, Mg(OH)2, is used to neutralize stomach acid. How many moles are in 26.89g of magnesium
hydroxide, Mg(OH)2?
5. How many carbon atoms are in 1.53 mol of carbon?
6. Liquid hydrogen is the fuel used in the space shuttle?s main engines. 1st: How many molecules of hydrogen are in 7.75
moles of hydrogen gas molecules (H2)? 2nd: How many total atoms would that be?
7. How many grams would 8.76 x 1024 molecules of O2 weigh?
8. Sodium fluoride is used in some toothpastes to help prevent cavities. How many grams of NaF are in
1.25 x 1025 formula units of NaF?
9. Ibuprofen, the active ingredient in many nonprescription pain relievers, has the molecular formula C13H18O2. The
molar mass of ibuprofen is 206.2860 g/mol. If a bottle contains a total of 33g of ibuprofen, how many molecules of
ibuprofen are in the bottle?
10. Strychnine, C21H22N2O2, is a powerful poison and has been used to eradicate rats. If a can of rat poison contains
0.75g of strychnine, how many nitrogen atoms are present?
11. What is the mass of one iron atom, in grams?
12. One of the events of a track and field meet is the shot put. If the shot is made of iron and it contains 7.83 x 1025 atoms
of Fe, could you lift it easily? (1 lb = 454g)
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
Chapter 3 Review Terms and Concepts
Democritus
atom
Aristotle
Law of Conservation of Mass
Lavoisier
Law of Definite Proportions
Proust
Law of Multiple Proportions
Dalton
Dalton?s Atomic Theory
Dalton?s model of the atom
flaws of Dalton?s atomic theory
nucleus
electron cloud
proton
neutron
electron
subatomic particles
amu ? atomic mass unit
Franklin
electricity
Faraday
positive and negative charges
attraction and repulsion
cathode
anode
CRT ? how does it work?
Crookes
cathode rays
J.J. Thomson
How did Thomson run his experiment?
Plum pudding model of the atom
Millikan
oil drop experiment
charge
coulomb, C
ampere, A
Roentgen
X-rays
Becquerel
Curie and Curie
Rutherford
α, β, γ radiation ? charges and relative masses
gold foil experiment
nucleus ? dense, small, positive
Chadwick
Bohr?s model
nuclear forces
atomic number
neutral atoms
ions
cation
anion
charge determination from periodic table
isoelectronic
mass number
isotope
nuclide
daughter
parent
atomic mass
calculation of atomic mass
percent natural abundance
nuclear reaction
All nuclei with atomic numbers greater than 83
are radioactive.
radioactive decay
alpha decay
beta decay
half-life
the mole
Avogadro?s number
molar mass
conversions
• grams ? moles
• atoms ? moles
• grams ? atoms
Know the people.
Know the dates.
Know the experiments.
Know the atomic models.
Be sure to look at all the
visual concepts for this
chapter.
Ms. K
Honors Chemistry
Name_____________________________________ #________
Date________________________ Period________
Chapter 3 Review Sheet
1. When reacting 10.g of reactants, the products will also weigh 10.g. What law does this concept
reflect? _______________________________________________
2. Sodium chloride always contains 39.34% Na and 60.66% Cl by mass. What law does this concept
reflect? _______________________________________________
3. Carbon and oxygen can combine to form carbon monoxide, CO, or carbon dioxide, CO2. What law
does this concept reflect? _______________________________________________
4. The following are the 5 concepts in Dalton’s Atomic Theory. Which one(s) are incorrect and why?
1.
2.
3.
4.
5.
All matter is composed of extremely small particles called atoms.
Atoms of a given element are identical in size, mass, and other properties.
Atoms cannot be subdivided, created, or destroyed.
Atoms of different elements combine in simple whole-number ratios to form chemical compounds.
In chemical reactions, atoms are combined, separated, or rearranged.
5. Name 5 subatomic particles. ________________________________________________________
6. For what does CRT stand? _________________________________________________________
7. Why did the cathode rays bend in Thomson?s experiment?
8. What made the cathode rays glow in Thomson?s experiment?
9. In 1897 the English physicist Joseph John Thomson was able to measure the ratio of what to what?
10.
What model of the atom is this? __________________________
11. Who determined that the charge of the electron to be 1.602 X 10-19 C? _____________________
12. What did Henri Becquerel discover?
13. Draw and explain the gold foil experiment. What did this experiment contribute to the atomic
theory?
14. Write the nuclear equation for alpha decay of plutonium-239.
15. Write the nuclear equation for the beta decay of potassium-34.
16. Know the following people and their contribution to ideas about the atom: Democritus, Aristotle,
Lavoisier, Dalton, Franklin, Crookes, Thomson, Curie, Curie, Becquerel, Millikan, Rutherford, Bohr,
and Chadwick.
17. The following concepts should be reviewed:
atom
3 basic laws of matter
Dalton?s atomic theory
nucleus, density
electron cloud
subatomic particles
CRT experiments
oil drop experiment
radiation – three types
gold foil experiment
discovery of neutron
nuclear forces
atomic number
ions
mass number
isotopes
nuclide
parent
daughter
percent natural abundance
atomic mass
atomic mass calculation
nuclear stability
radioactive decay
alpha decay
beta decay
half-life
mole
mole calculations
Avogadro?s number
molar mass