1 atomic structure notes / pts last name per atom work 2015.pdf• number of neutrons mass number...

4 ATOMIC STRUCTURE NOTES __ /__ pts Per__ First Last Name___

Anticipatory Response Cornell Question & Ans 1. Matter can be divided? Y N Directions:Make 5 questions2. Atoms are indivisible? Y N & answers that are different3. Dalton tests showed that than the Anticipatory Responseatoms were indivisible? Y N 1.Example: Why was 4. Atoms of the same element Daltons theory better are identical? Y N than Democritus’? 5. Chemical reactions involve Answer: Dalton had breaking & joining bonds? Y N experimentation to back his theory. 2. 3. 4. Anticipatory Response 1.Carbon always has 6 protons, 6 electrons & 6 neutrons? Y N 5. 2. Carb‐14 has 14 Neutron?Y N 3. Carbon‐13 has 6 e‐? Y N 4.The Nucleus was found to be Small, dense & positive? Y N 5. Sodium has 11 protons? Y N Summary Section:

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Chapter 4 Atomic Structure 83

Name ___________________________ Date ___________________ Class __________________

DEFINING THE ATOM4.1

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Name ___________________________ Date ___________________ Class __________________

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 CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.

Elements are composed of tiny particles called . 1. _______________________

Atoms of any one element are from those of any 2. _______________________

other element. Atoms of different elements can form 3. _______________________

by combining in whole-number ratios. Chemical reactions 4. _______________________

occur when atoms are .

Part B True-FalseClassify 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 duringchemical reactions.

________ 6. Atoms combine in one-to-one ratios to form compounds.

________ 7. Atoms of one element are different from atoms of other elements.

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Name ___________________________ Date ___________________ Class __________________

STRUCTURE OF THE NUCLEAR ATOM4.2

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Section Review

Objectives• Identify three types of subatomic particles

• Describe the structure of atoms according to the Rutherford model

Vocabulary


Dalton theorized that atoms are indivisible, but the discovery 1. _______________________

of particles changed this theory. Scientists now know that 2. _______________________

atoms are made up of electrons, which have a charge; 3. _______________________

,which have a positive charge; and , which are 4. _______________________

neutral. The latter two particles are found in the of the 5. _______________________

atom. It was who discovered the nucleus of the atom. The 6. _______________________

nucleus, which has a charge, occupies a very small volume 7. _______________________

of the atom. In contrast, the negatively charged occupy 8. _______________________

most of the volume of the atom.


______ 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.

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• electrons

• cathode ray

• protons

• neutrons

• nucleus

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86 Core Teaching Resources

Name ___________________________ Date ___________________ Class __________________©

Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.

Part C MatchingMatch each description in Column B to the correct term in Column A

Part D Questions and ProblemsAnswer 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?

20. Describe Rutherford’s model of the atom, including the location of protons,neutrons, and electrons with respect to the nucleus. How does this modelexplain the deflections of a beam of alpha particles aimed at a sheet of gold foil?

Column B

a. stream of electrons produced at the negative electrodeof a tube containing a gas at low pressure

b. the central core of an atom, which is composed ofprotons and neutrons

c. negatively charged subatomic particles

d. subatomic particles with no charge

e. positively charged subatomic particles

Column A

electrons

cathode ray

protons

neutrons

nucleus

________ 13.

________ 14.

________ 15.

________ 16.

________ 17.

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Name ___________________________ Date ___________________ Class __________________

DISTINGUISHING BETWEEN ATOMS4.3

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Section Review

Objectives• Explain how isotopes differ from one another

• Use the atomic number and mass number of an element to find the numbersof protons, electrons, and neutrons

• Calculate the atomic mass of an element from isotope data

Vocabulary

Key Equations• atomic number � number of protons � number of electrons

• number of neutrons � mass number � atomic number


The number of in the nucleus of an atom is the 1. _______________________

atomic of that element. Because atoms are electrically 2. _______________________

neutral, the number of protons and in an atom are equal. 3. _______________________

The total number of and neutrons in an atom is the mass 4. _______________________

number. Atoms of the same element are identical in most respects, 5. _______________________

but they can differ in the number of in the nucleus. Atoms 6. _______________________

that have the same number of protons but different mass numbers 7. _______________________

are called . 8. _______________________

The of an element is the weighted average of the 9. _______________________

masses of the isotopes of that element. Each of the three known 10. _______________________

isotopes of hydrogen has proton(s) in the nucleus. The

most common hydrogen isotope has neutrons. It has a

mass number of and is called hydrogen-1.10

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• atomic number

• mass number

• isotopes

• atomic mass unit (amu)

• atomic mass

• periodic table

• period

• group

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88 Core Teaching Resources

Name ___________________________ Date ___________________ Class __________________©

Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.


________ 11. The atomic number of an element is the sum of the protons andelectrons in an atom of that element.

________ 12. The atomic number of an atom is the total number of protons in anatom 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 bysubtracting the atomic number from the mass number.

Part C MatchingMatch each description in Column B to the correct term in Column A

Part D Questions and ProblemsSolve the following problem in the space provided.

24. Given the relative abundance of the following naturally occurring isotopes ofoxygen, calculate the average atomic mass of oxygen.

oxygen-16: 99.76%oxygen-17: 0.037%oxygen-18: 0.204%

Column B

a. atoms that have the same number of protons butdifferent numbers of neutrons

b. weighted average mass of the atoms in a naturallyoccurring sample of an element

c. equals the number of neutrons plus the number ofprotons in an atom

d. �112� the mass of a carbon-12 atom

e. the number of protons in the nucleus of an atom ofan element

f. an arrangement of elements according to similarities in their properties

g. a vertical column of elements in the periodic table

h. a horizontal row of the periodic table

Column A

atomic number

periodic table

mass number

group

isotopes

atomic mass unit (amu)

atomic mass

period

________ 16.

________ 17.

________ 18.

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________ 22.

________ 23.

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Identifying Elements &

& Their Sub-Atomic Particles

Complete the table

Isotope Symbol Atomic # At. Mass p+ n0 e- Hydrogen-1 H 1 1 1 0 1

4He

Xenon-132

20 40

18 22

Tungsten-184

6 6

32S

47 61

56Fe

Fluorine-19

41 52

79 197

85Rb

37Cl

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195 117

15 31

17O

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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 (99 + 100) x 0.5 ? 2 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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Name ___________________________ Date ___________________ Class __________________

ATOMIC STRUCTURE 4

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Practice ProblemsIn your notebook, solve the following problems.

SECTION 4.1 DEFINING THE ATOM1. 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? Expressyour answer in millimeters.

SECTION 4.2 STRUCTURE OF THE NUCLEAR ATOM1. 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 � 10�24 g. Approximately what number ofneutrons would equal a mass of one gram?

3. Which statement is consistent with the results of Rutherford’s gold foilexperiment?

a. All atoms have a positive charge.

b. Atoms are mostly empty space.

c. The nucleus of an atom contains protons and electrons.

d. Mass is spread uniformly throughout an atom.

SECTION 4.3 DISTINGUISHING BETWEEN ATOMS1. 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 Number of Number of Atomic MassProtons Electrons Neutrons Number Number

Manganese 25 30

Sodium 11 12

Bromine 35 45

Yttrium 39 89

Arsenic 33 75

Actinium 227

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GVUser

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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?

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COMPLETE THE FOLLOWING TABLE

Symbol Atomic Mass Number Number Number

Number Number of p+ of e

- n

o

Fe 64 158 64 30 131 55 38 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?”

58 26 96 42 201 80

Name Date Per ________

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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 Pr______ El_____ Ne______ Location Mass Charge

3. Fill out the chart for these elements. Name Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Symbol Atomic # Electrons Neutrons +Protons = Mass # of The isotope

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 Oxygen Flourine Neon Alumimum Iron Gold Symbol Atomic # Electrons Neutrons +Protons = Mass # of The isotope

Bonus-AvgAtomicMass 15.9994 _________ ________ ___________ ___________ ___________

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_________________ Cartoon Lab Safety Questions

1. List 3 unsafe activities shown in the picture and explain why each is unsafe. a. ________________________________________________________________ __________________________________________________________________ b.________________________________________________________________ __________________________________________________________________ c.________________________________________________________________ __________________________________________________________________ 2. List 3 correct lab procedures in the picture. a. ________________________________________________________________ __________________________________________________________________ b.________________________________________________________________ __________________________________________________________________ c.________________________________________________________________ __________________________________________________________________ 3. What should Bob do after the accident? 4. What should Sue have done to avoid an accident? 5. Compare Luke and Duke’s lab techniques. Who is following the rules and how? a. Luke -______________________________________________________ ____________________________________________________________ b. Duke -______________________________________________________ ____________________________________________________________ 6. What are 3 things shown in the lab that should not be there and why? a. ________________________________________________________________ __________________________________________________________________ b.________________________________________________________________ __________________________________________________________________ c.________________________________________________________________ __________________________________________________________________ 7. Compare Joe & Carl’s lab techniques. Explain who is doing it correctly and why? a. Joe -______________________________________________________ ____________________________________________________________

b. Carl -_______________________________________________________ ____________________________________________________________

8. 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? 13. How might you plan or prepare yourself so that you will do the above correctly? ________________________________________________________________________________________________________________________________________________ ________________________________________________________________________

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Questions:

Cartoon on Lab Safety http://www.biologycorner.com/worksheets/safety.html

2 of 3 8/16/2010 8:33 AM

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H

1.0079 Hydrogen

Name, Last Name PeriodThe 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? ___

Atomic Mass 10. What is the average of all of Hydrogen’s isotopes ?_______ 11. What is Hydrogen’s average Atomic Mass?____ 12. Which is probably the most abundant Isotope of Hydrogen? _________

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. What is Carbon‐12’s Mass Number?___ 8. What is Carbon‐13’s Mass Number?___ 9. What is Carbon‐14’s Mass Number? ___

Atomic 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 ________.

1 H 1

Hydrogen‐1

1 H 2

Hydrogen‐2 Deuterium

1H 3

Hydrogen‐3 Tritium

6 C 12

Carbon‐12

6 C 13

Carbon‐13

6C 14

Carbon‐14

6

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12.0107 Carbon

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___________________________ First Name, Last ________

Period

SCORE: ___/10 pts

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: Protons Neutrons Both 8. How many electrons does the lightest Flourine have? 8 9 18 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

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F 9

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F 9

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F 18.998

4 Different Flourine Isotopes

Combined Isotopes 17

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___________________________ First Name, Last ________

Period

SCORE: ___/10 pts

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? 8 15.999 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 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.

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O 8

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O 15.999

4 Different Oxygen Isotopes

Combined Isotopes 18

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___________________________ 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.

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___________________________ 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.

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1 atomic structure notes / pts last name per atom work 2015.pdf• number of neutrons mass number...

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