Download 4 ATOMIC STRUCTURE NOTES __ /__ pts

1
4 ATOMIC STRUCTURE NOTES __ /__ pts 6 electrons & 6 neutrons? Y N 2. Carb‐14 has 14 Neutron?Y N Anticipatory Response
1. Matter can be divided? Y N 2. Atoms are indivisible? Y N 3. Dalton tests showed that atoms were indivisible? Y N 4. Atoms of the same element are identical? Y N 5. Chemical reactions involve breaking & joining bonds? Y N Anticipatory Response 1.Carbon always has 6 protons, 3. Carbon‐13 has 6 e‐? Y N Small, dense & positive? Y N 5. Sodium has 11 protons? Y N Summary Section: 4.The Nucleus was found to be 1
First Last Name___Per__ Cornell Question & Ans
Directions: Make 5 questions
& answers that are different
than the Anticipatory Response
1.Example: Why was Daltons theory better than Democritus’? Answer: Dalton had experimentation to back his theory. 2. 3. 4. 5. What is the same about the two? 1__________________________
___________________________
___________________________
___________________________
___________________________ What is the same about the two? 1__________________________
___________________________
___________________________
___________________________
___________________________ What is different about the two? COMPARE
What is different about the two? CONTRAST
Double Bubble Compare & Contrast
2__________________________
___________________________
___________________________
___________________________
___________________________ What is the same about the two? 3__________________________
___________________________
___________________________
___________________________
___________________________ What is different about the two? 3__________________________
___________________________
___________________________
___________________________
___________________________ 2
2__________________________
___________________________
___________________________
___________________________
___________________________ 3__________________________
___________________________
___________________________
___________________________
___________________________ What is different about the two? 2__________________________
___________________________
___________________________
___________________________
___________________________ What is different about the two? 1__________________________
___________________________
___________________________
___________________________
___________________________ What is different about the two? CONTRAST
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05_CTR_ch04 7/9/04 3:26 PM Page 83
Name ___________________________
4.1
3
Date ___________________
Class __________________
DEFINING THE ATOM
Section Review
Objectives
• Describe Democritus’s ideas about atoms
• Explain Dalton’s atomic theory
• Describe the size of an atom
Vocabulary
• atom
• Dalton’s atomic theory
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
Elements are composed of tiny particles called
2
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
Atoms of any one element are
1
.
1. _______________________
from those of any
2. _______________________
3
3. _______________________
by combining in whole-number ratios. Chemical reactions
4. _______________________
other element. Atoms of different elements can form
occur when atoms are
4
.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 5. Atoms of one element change into atoms of another element during
chemical reactions.
________ 6. Atoms combine in one-to-one ratios to form compounds.
________ 7. Atoms of one element are different from atoms of other elements.
3
↑
Chapter 4 Atomic Structure
83
05_CTR_ch04 7/9/04 3:26 PM Page 85
Name ___________________________
4
Date ___________________
Class __________________
STRUCTURE OF THE NUCLEAR ATOM
4.2
Section Review
Objectives
• Identify three types of subatomic particles
• Describe the structure of atoms according to the Rutherford model
Vocabulary
• electrons
• cathode ray
• protons
• neutrons
• nucleus
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
Dalton theorized that atoms are indivisible, but the discovery
1
of
particles changed this theory. Scientists now know that
2
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
atoms are made up of electrons, which have a
3
4
,which have a positive charge; and
6
nucleus, which has a
3. _______________________
, which are
4. _______________________
5
5. _______________________
of the
who discovered the nucleus of the atom. The
7
charge, occupies a very small volume
of the atom. In contrast, the negatively charged
2. _______________________
charge;
neutral. The latter two particles are found in the
atom. It was
1. _______________________
8
occupy
6. _______________________
7. _______________________
8. _______________________
most of the volume of the atom.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
______
9. According to Dalton’s atomic theory, atoms are composed of protons,
electrons, and neutrons.
______
10. Atoms of elements are electrically neutral.
______
11. The mass of an electron is equal to the mass of a neutron.
______
12. The charge on all protons is the same.
4
↑
Chapter 4 Atomic Structure
85
05_CTR_ch04 7/9/04 3:26 PM Page 86
Name ___________________________
5
Date ___________________
Class __________________
Part C Matching
Match each description in Column B to the correct term in Column A
Column A
Column B
________ 13. electrons
a. stream of electrons produced at the negative electrode
of a tube containing a gas at low pressure
________ 14. cathode ray
b. the central core of an atom, which is composed of
protons and neutrons
________ 15. protons
c. negatively charged subatomic particles
________ 16. neutrons
d. subatomic particles with no charge
________ 17. nucleus
e. positively charged subatomic particles
Part D Questions and Problems
Answer the following questions in the space provided.
18. Which subatomic particles are found in the nucleus of an atom?
19. Which subatomic particles are charged?
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20. Describe Rutherford’s model of the atom, including the location of protons,
neutrons, and electrons with respect to the nucleus. How does this model
explain the deflections of a beam of alpha particles aimed at a sheet of gold foil?
86
Core Teaching Resources
5
↑
05_CTR_ch04 7/9/04 3:26 PM Page 87
Name ___________________________
6
Date ___________________
Class __________________
DISTINGUISHING BETWEEN ATOMS
4.3
Section Review
Objectives
• Explain how isotopes differ from one another
• Use the atomic number and mass number of an element to find the numbers
of protons, electrons, and neutrons
• Calculate the atomic mass of an element from isotope data
Vocabulary
• atomic number
• mass number
• isotopes
• atomic mass unit (amu)
• atomic mass
• periodic table
• period
• group
Key Equations
• atomic number number of protons number of electrons
• number of neutrons mass number atomic number
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
The number of
atomic
2
in the nucleus of an atom is the
1. _______________________
of that element. Because atoms are electrically
2. _______________________
3
in an atom are equal.
3. _______________________
and neutrons in an atom is the mass
4. _______________________
neutral, the number of protons and
The total number of
4
number. Atoms of the same element are identical in most respects,
but they can differ in the number of
5
5. _______________________
in the nucleus. Atoms
6. _______________________
that have the same number of protons but different mass numbers
7. _______________________
are called
The
6
7
.
8. _______________________
of an element is the weighted average of the
9. _______________________
masses of the isotopes of that element. Each of the three known
isotopes of hydrogen has
8
proton(s) in the nucleus. The
most common hydrogen isotope has
mass number of
10
10. _______________________
9
neutrons. It has a
and is called hydrogen-1.
6
↑
Chapter 4 Atomic Structure
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05_CTR_ch04 7/9/04 3:26 PM Page 88
Name ___________________________
7
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. The atomic number of an element is the sum of the protons and
electrons in an atom of that element.
________ 12. The atomic number of an atom is the total number of protons in an
atom of that element.
________ 13. An atom of nitrogen has 7 protons and 7 neutrons.
________ 14. Relative atomic masses are expressed in amus.
________ 15. The number of neutrons in the nucleus can be calculated by
subtracting the atomic number from the mass number.
Part C Matching
Match each description in Column B to the correct term in Column A
Column A
Column B
a. atoms that have the same number of protons but
different numbers of neutrons
________ 17. periodic table
b. weighted average mass of the atoms in a naturally
occurring sample of an element
________ 18. mass number
c. equals the number of neutrons plus the number of
protons in an atom
________ 19. group
d.
________ 20. isotopes
e. the number of protons in the nucleus of an atom of
an element
________ 21. atomic mass unit (amu)
f. an arrangement of elements according to similarities
in their properties
________ 22. atomic mass
g. a vertical column of elements in the periodic table
________ 23. period
h. a horizontal row of the periodic table
1
12
the mass of a carbon-12 atom
Part D Questions and Problems
Solve the following problem in the space provided.
24. Given the relative abundance of the following naturally occurring isotopes of
oxygen, calculate the average atomic mass of oxygen.
oxygen-16:
oxygen-17:
oxygen-18:
88
99.76%
0.037%
0.204%
Core Teaching Resources
7
↑
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
________ 16. atomic number
8
Identifying Elements
&
& Their Sub-Atomic Particles
Complete the table
Isotope
Symbol
Hydrogen-1
H
Atomic #
At. Mass
1
1
20
40
p+
n0
e
1
0
1
18
22
6
6
-
4
He
Xenon-132
Tungsten-184
32
S
47
61
56
Fe
Fluorine-19
41
79
52
197
85
Rb
37
Cl
35
195
15
30
117
31
17
O
14
7
8
9
Subatomic Particles & A.M.U.’s
1.
What are the 3 sub-atomic particles?
_____________ ______________ _______________
2.
Which of the 3 sub-atomic particles determines which element is present?
3.
Which of the 3 sub-atomic particles when different, makes the atom an
isotope?
What is an isotope?
4.
Which of the 3 sub-atomic particles when gained or lost, makes the atom
become an ion with a charge?
5.
Why is the Bohr model a FALSE picture of the atom?
It describes the atoms similar to the pl_________ mo_________ rather
a cl_______ or sph________ model.
6.
Where is most of the mass of an atom found?
7
Why is there almost no mass found anywhere except in the nucleus?
8.
What is the difference between Atomic Mass and Atomic Number?
9.
What is an “a.m.u.?”
10.
What is the average atomic mass of an element that is found to be 50%,
In nature, 99.0 a.m.u.’s & 50% 100.0 a.m.u.’s.
Method 1 (50/50)
Transition
Method 2 (all %’s)
(99.0 + 100.0) = _____
?
(99+100) X 1
2
(99 + 100) x 0.5
11.
What is Chlorine’s avg atomic mass which is 75% 35.0 amu. & 25% 37.0
12.
What is Hydrogen’s average atomic mass if H-1 is 99.985%, H-2 is 0.015% &
there is 0% Hydrogen -3?
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05_CTR_ch04 7/9/04 3:26 PM Page 89
10
Name ___________________________
4
Date ___________________
Class __________________
ATOMIC STRUCTURE
Practice Problems
In your notebook, solve the following problems.
SECTION 4.1 DEFINING THE ATOM
1. According to Figure 5.2, 100,000,000 copper atoms would form a line 1 cm
long. How long would a line formed by 1 107 copper atoms be? Express
your answer in millimeters.
SECTION 4.2 STRUCTURE OF THE NUCLEAR ATOM
1. A sulfur-32 atom contains 16 protons, 16 neutrons, and 16 electrons. What is
the mass (in grams) of a sulfur-32 atom?
2. The mass of a neutron is 1.67 1024 g. Approximately what number of
neutrons would equal a mass of one gram?
3. Which statement is consistent with the results of Rutherford’s gold foil
experiment?
a. All atoms have a positive charge.
b. Atoms are mostly empty space.
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
c. The nucleus of an atom contains protons and electrons.
d. Mass is spread uniformly throughout an atom.
SECTION 4.3 DISTINGUISHING BETWEEN ATOMS
1. How many protons are found in an atom of each of the following?
a. boron
c. neon
b. sulfur
d. lithium
2. Complete the table for the following elements.
Element
Number of
Protons
Manganese
25
Sodium
Bromine
Number of
Electrons
Atomic
Number
Mass
Number
39
89
30
11
35
12
45
Yttrium
Arsenic
Number of
Neutrons
33
Actinium
75
227
10
↑
Chapter 4 Atomic Structure
89
11
Isotopes Quiz B
1. What is Carbon’s symbol
2. Write Carbon’s’ 2 smallest isotopes – ex: Li – 6 or Li - 7
3. List the 2 isotopes number of Protons, Electrons & Neutrons.
Protons =
Electrons =
Neutrons =
4. Which isotope is more common?
5. How do you know # 4 above?
6. About what % of the Isotopes weigh 12.
7. Where is most of an atoms wt
8. What occupies most of the volume of an atom.
Scientists Discoveries
1. What was Democritus known for?
2.
What was John Dalton famous for?
3.
What did JJ Thompson discover?
4.
What ratio did Millikan find with his oil drop experiment?
5.
What did Goldstein find?
6. With his gold foil experiment what did Rutherford conclude about the
center of the atom?
7.
What did Rutherford conclude about the rest of the atom?
8.
What did Chadwick find?
9.
What did Mendeleev find?
10. Which scientist in the room only wishes he would discover something
important?
11
12Name
Per ________
Date
COMPLETE THE FOLLOWING TABLE
Symbol
58
26
Atomic
Number
Mass
Number
64
158
Number
+
of p
30
131
55
38
201
80
Number
o
n
Fe
64
96
42
Number
of e
52
Mo
Hg
2. What sub-atomic particle determines which element is present?
3. In a neutral atom, which sub-atomic particles will always have equal numbers?
4. Where are electrons found?
5. Most of the mass of an atom is found in the ….
6. What is the difference between atomic mass and atomic number?
7. What is an “amu?”
12
13
How Many Protons, Neutrons and Electrons are in Common Elements
Classzone.com activity
http://www.classzone.com/books/earth_science/terc/content/investigations/es0501/es0501page01.cfm?chapter_no=05
Go to classzone.com. Then go to the earth science book for California and the investigations for
Chapter 5 or search ES0501. Answer the questions below.
1. What elements are in these common items? Diamonds –Carbon ________________
________________ _________________ _______________ ________________
2. . Give the mass,charge and location (nucleus or orbit) of each particle in the atom.
Name
Location
Mass
Charge
Pr______ El_____
Ne______
3. Fill out the chart for these elements.
Name
Hydrogen Helium Lithium Beryllium
Symbol
Atomic #
Electrons
Neutrons
+Protons
= Mass # of
The isotope
Boron Carbon Nitrogen
Directions: Forward through the “Next” and “Skip” prompts. Then experiment with the program
to answer the questions below:
4. Which particle controls what element an atom is (hint: See which particle when added changes
the element name in the info box)?_________
5. What do you get when you change the number of neutrons in the nucleus?
6. What 2 particles control the mass of an atom(hint: Look at which particle doesn’t change the
mass)?_____________________________________________________________________
7. What happens when you cluster the electrons or move them into another level? They r______.
Why do they behave the way they do?____________________________________________
8. What do you get if the # of protons and electrons in your model differ? An un_________ _____.
9. Fill out the chart for these elements,
Name
Symbol
Atomic #
Electrons
Neutrons
+Protons
Oxygen
Flourine
Neon
Alumimum
Iron
Gold
= Mass # of
The isotope
Bonus
-AvgAtomicMass 15.9994
_________
________
___________
13
___________ ___________
14
_________________
Cartoon Lab Safety Questions
1.
3.
List 3 unsafe activities shown in the picture and explain why each is unsafe.
a. ________________________________________________________________
__________________________________________________________________
b.________________________________________________________________
__________________________________________________________________
c.________________________________________________________________
__________________________________________________________________
List 3 correct lab procedures in the picture.
a. ________________________________________________________________
__________________________________________________________________
b.________________________________________________________________
__________________________________________________________________
c.________________________________________________________________
__________________________________________________________________
What should Bob do after the accident?
4.
What should Sue have done to avoid an accident?
5.
8.
Compare Luke and Duke’s lab techniques. Who is following the rules and how?
a.
Luke -______________________________________________________
____________________________________________________________
b.
Duke -______________________________________________________
____________________________________________________________
What are 3 things shown in the lab that should not be there and why?
a. ________________________________________________________________
__________________________________________________________________
b.________________________________________________________________
__________________________________________________________________
c.________________________________________________________________
__________________________________________________________________
Compare Joe & Carl’s lab techniques. Explain who is doing it correctly and why?
a.
Joe -______________________________________________________
____________________________________________________________
b.
Carl -_______________________________________________________
____________________________________________________________
What will happen to Ray and Tim when the teacher catches them?
9.
List 3 items in the picture that are there for the safety of the students in the lab.
10.
What is Betty doing wrong?
11.
Which one of the good actions in the picture will be easy for you to do correctly?
12.
Honestly, which one do you think you may not follow correctly?
2.
6.
7.
13.
How might you plan or prepare yourself so that you will do the above correctly?
________________________________________________________________________
________________________________________________________________________
________________________________________________________________________
14
Cartoon on Lab Safety
2 of 3
15
http://www.biologycorner.com/worksheets/safety.html
Questions:
15
8/16/2010 8:33 AM
16
Name, Last Name Period
1
H
1 H 1 1 H 2 1
H 3 Hydrogen‐1 Hydrogen‐2 Deuterium Hydrogen‐3 Tritium The Difference Between Atomic & Mass Number Atomic Number 1. What is Hydrogen‐1’s atomic number?___ 2. What is Hydrogen‐2’s atomic number?___ 3. Do Isotopes of the same element have the same Atomic number? ______ Mass Number 4. What is Hydrogen‐2’s mass number? _____ 5. What is Hydrogen‐3’s mass number?_____ 6. Do isotopes of the same element have the same mass number? _______ The Difference Between Atomic Mass
& Mass Number Mass Number 7. What is Hydrogen‐1’s Mass Number?___ 8. What is Deuterium’s Mass Number?___ 9. What is Tritium’s Mass Number? ___ 1.0079
ÅAtomic Mass
10. What is the average of all of Hydrogen’s isotopes ?_______
Hydrogen
11. What is Hydrogen’s average Atomic Mass?____ 12. Which is probably the most abundant Isotope of Hydrogen? _________ 6
C
6 C 12 6 C 13 6
C 14 Carbon‐12 Carbon‐13 Carbon‐14 The Difference Between Atomic & Mass Number Atomic Number 10. What is Carbon‐12’s atomic number?___ 11. What is Carbon‐13’s atomic number?___ 12. Do Isotopes of the same element have the same Atomic number? ______ Mass Number 4. What is Carbon‐12’s mass number? _____ 5. What is Carbon‐13’s mass number?_____ 6. Do isotopes of the same element have the same mass number? _______ The Difference Between Atomic Mass
& Mass Number Mass Number 7. 8. 9. 12.0107
Carbon
What is Carbon‐12’s Mass Number?___ What is Carbon‐13’s Mass Number?___ What is Carbon‐14’s Mass Number? ___ ÅAtomic Mass 10. What is the average of all of Carbon’s isotopes ?_______ 11. What is Carbon’s average Atomic Mass?____ 12. Which is probably the most abundant Isotope of Carbon? _________ Conclusion: Average Atomic Mass is an _______ of several whole numbers so it has decimals. Mass number is a counting integer or a ________ so it has no ________. 16
17
18
F
9
20
19
F
F
9
Combined Isotopes
21
9
F
9
9
F
4 Different Flourine Isotopes
___________________________
First Name, Last ________
Period
SCORE: ___/10 pts
18.998
4 Atomic Structure Formal Assessment 3
Directions:
Circle the best answer for each question.
1.
How many protons does Flourine – 18 have?
9
18
19
2.
How many protons does Flourine – 19 have?
9
X
X
3.
What is the atomic number of Flourine -19?
9
18
19
4.
What is the average Atomic Mass of Flourine?
18
19
neither
5.
How many positive charges does Oxygen have in its’ nucleus?
8
18 it varies
6.
How many Atomic Mass Units (a.m.u.) is the heaviest Flourine Isotope?
18 19 20 21
7.
Atomic Mass Units are made up of:
8.
How many electrons does the lightest Flourine have?
Protons
Neutrons
Both
8
18
9
True or False
9.
The name of the heaviest shown Flourine Isotope is Flourine 18.998.
10.
In Flourine – 18, the 18 stands for how many particles (protons and neutrons) are
in the nucleus), while the 9 stands for how many protons it has in the nucleus.
Bonus (circle the best answer).
11.
What is the difference between atomic mass and atomic number?
a.
Atomic Number is a whole number.
b.
Atomic Mass is an average of the masses of all the isotopes.
c.
Atomic Mass is a decimal because it is an average
d.
All above answers are correct
17
18
15
O
8
17
16
O
O
8
18
8
Combined Isotopes
O
8
8
O
4 Different Oxygen Isotopes
___________________________
First Name, Last ________
Period
SCORE: ___/10 pts
15.999
4 Atomic Structure Formative Assessment 2
Directions:
Circle the best answer for each question.
1.
What is the average Atomic Mass of Oxygen?
8
15.999
Neither
2.
How many protons does Oxygen have?
8
15.999
It varies
3.
How many positive charges does Oxygen have in its’ nucleus?
8
15.999
It varies
4.
What is the Atomic Number of Oxygen?
It varies
5.
How many Atomic Mass Units (a.m.u.) is the heaviest Oxygen Isotope?
8
16
18
6.
How many neutrons does the lightest Oxygen Isotope have?
7
8
9
7.
How many electrons does the heaviest Oxygen have?
7
8
16
8.
How many electrons does the lightest Oxygen have?
7
8
16
8
15.999
True or False
9.
The name of the heaviest shown Oxygen Isotope is Oxygen -18.
10.
The name of the lightest Oxygen Isotope shown is Oxygen -8.
*Bonus
11.__Atomic Mass is the average mass of the 3 isotope, resulting in a decimal but
Mass Number is the mass of one of the isotopes, resulting in a whole number.
18
19
___________________________
First Name, Last ________
Period
SCORE: ___/10 pts
Atomic Structure Formal Assessment 1
Circle the correct answers
1.
How many protons does Carbon – 12 have?
3
6
12
13
14
2.
How may protons does Carbon – 13 have?
3
6
12
13
14
3.
What is the atomic number of Carbon -12?
3
6
12
13
14
4.
What is the atomic number of Carbon-13?
3
6
12
13
14
5.
How many neutrons does Carbon – 12 have? 6
7
8
13
14
6.
How many neutrons does Carbon – 13 have? 6
7
8
13
14
Write True or False in the blank
7.
Carbon has 3 isotopes which differ in their number of neutrons. The
Carbon – 12 has 12 – 6 = 6 neutrons. Carbon – 13 has 13 – 6 = 7 neutrons.
8.
Most of the mass of all the isotopes are in the center or nucleus because
the electrons almost weigh zero.
9.
Protons and Electrons have the same positive charge while neutrons have a
neutral charge.
10.
The nucleus is filled with negative charges which hold together because of
The stronger nuclear forces between all the nuclear particles.
19
20
___________________________
Name
________
Period
SCORE: ___/10 pts
Science Rules Formal Assessment 1
Multiple Choice – Circle one or more as directed
1. Circle 3 things that shouldn’t be out/visible in class and will be taken away.
a. gum b. food/drink c. water d. phones e. ipod/mp3… f. calculator
2. Circle 3 things that will cause loss of points.
a.
Being out of seat when bell rings.
b.
Not covering answers during a test.
c.
Using a calculator on a test
d.
Turning in homework a few minutes late or forgetting to write name.
e.
Raising ones’ hand before speaking or answering a question.
3. What times can one make up tests & quizzes? (pick 1)
a.
anytime
b.
Tuesday intervention
c.
Wednesday and Friday Lunch
d.
ASAP (in the following days) during the above b & c answers
e.
2-5 weeks after the assignment was due during Tues/Wed./Friday lunches
Write True or False
4.
Extra point quizzes are only given on the day of correcting homework.
5.
Mr. Abouaf will drop the lowest “Zero” earned. If none he will drop the lowest other grade.
6.
Absent students are responsible for finding out missing work, quizzes, tests from others.
7.
Students can talk to Mr. Abouaf or be out of their seat during roll call, as long as
they are in the class room.
8.
Intervention will be Tuesdays after school from 3:05 to 4:05 for 1 point extra credit.
9.
Students are allowed to complain about food or drink being thrown in the trash because
They forgot, didn’t know or were never told.
10.
Test help sheets can be used on make up tests.
20