Name: _________________________________________

Chapter 9 Worksheet Packet

Section 1 Reading Guide (313-323)1. The Greek philosopher Democritus thought that matter is made of ___________, solid objects

that ____________ be divided, created, or destroyed.

2. True or false: Aristotle agreed with Democritus’s ideas. __________________

3. What is an atom?

4. Which scientist came up with the atomic theory? ________________

5. What are the four main ideas of the atomic theory?a.

b.

c.

d.

6. Would Dalton’s model look much different than Democritus’s? _______

7. In 1897, a British scientist named J.J. Thomson showed that there are small __________ inside the atom; this means that atoms can be divided into even smaller parts.

8. Looking at Figure 4 on page 316, add in the missing information to the diagram

9. What subatomic particle did Thomson discover? ___________

10. What is an electron?

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WORKSHEET 1

11. Sketch below what Thomson’s idea of an atom may have looked like

12. What results did Rutherford see in his experiment? a. Most particles went through the gold foilb. Some of the particles were deflected (turned to one side)c. Some bounced straight backd. All of the above

13. Rutherford proposed that in the center of the atom is a tiny, extremely dense, positively charged part called the __________. It has a positive charge because of particles called _______________.

14. Sketch below what Rutherford’s idea of an atom may have looked like based on his results

15. Who discovered the neutron? _____________________

16. What charge does a neutron have? _____________

17. Niels Bohr’s work focused on which subatomic particle? _______________

18. Bohr’s model said that electrons move around the nucleus in certain paths, or __________________________.

19. Sketch below what Bohr’s idea of an atom may have looked like

20. Was Bohr’s idea of electrons traveling around in paths correct? _____

21. According to the current atomic theory, there are regions inside the atom where electrons are like to be found. These regions are called _______________________.

22. Using Figure 10 on page 322 as a guide, label the

diagram to the right. Use the words proton, neutron, nucleus, and electron cloud

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Atomic Models Worksheet

Directions: Fill in the blanks on the right with the information in the chart below.

Word Listatom neutronBohr nucleusDalton protonDemocritus Rutherforddestroyed subatomic particleelectron substanceselectron cloud Thomson

More than 2000 years ago, the Greek philosopher __(1)__ proposed the existence of very small, indivisible particles, each of which was called a(n) __(2)__. The theory that such particles existed was supported, much later, by several different scientists. In 1803, a scientist by the name of __(3)__ came up with the atomic theory, which had three points to it:

I. All substances are made of atoms. Atoms are small particles that cannot be created, divided, or __(4)__.

II. Atoms of the same element are exactly alike, and atoms of different elements are different

III. Atoms join with other atoms to make new __(5)__.

It was later proposed that the atom was not indivisible, but is made up of smaller particles, each of which is called a(n) __(6)__. These particles include the negatively-charged __(7)__, the positively-charged __(8)__; and the uncharged __(9)__. The small electrons were discovered by a scientists named __10)__, who created a model called the Plum Pudding model. The larger two particles are present in the __(11)__, or center, of the atom, which was discovered by __(12)__ in his gold foil experiment.

The Danish physicist __(13)__ proposed a model of the atom in which the electrons orbit the nucleus without losing energy. He called each possible orbit an electron level. Today, the modern atomic theory suggests that an electron’s position cannot be predicted, but the area where one is likely to be is a(n) __(14)__.

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WORKSHEET 3

1. ____________________

2. ____________________

3. ____________________

4. ____________________

5. ____________________

6. ____________________

7. ____________________

8. ____________________

9. ____________________

10. ____________________

11. ____________________

12. ____________________

13. ____________________

14. ____________________

WORKSHEET 2

1. Elements join in a ____________ ratio according to their masses to form a compound.

2. What type of charge do protons have? _____________________

3. The SI unit used to express the masses of particles in atoms is the __________________ ____________.

4. What type of charge do neutrons have? ________________________

5. Which subatomic particle(s)are found in the nucleus (circle any that are true)a. Protonb. Neutronc. Electron

6. Both the proton and the neutron have a mass of about ___ amu, which the mass of an electron is usually thought of as ____ amu.

7. To have a neutral charge, an atom has to have the same number of protons and ________________.

8. Does an atom need to have equal number of protons and neutrons? _____

9. What is the atomic number?

10. The atomic number is always equal to the number of _______ in an atom; it can be thought of as the identity of an atom.

11. What is an isotope?

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12. Look at Table 3 on page 328. What is different between the three isotopes?

13. Look at how the isotopes are named in Table 3. If I have a sample of Boron with 5 protons, 5 neutrons, and 5 electrons, how would I name this isotope? ___________________________

14. What is the mass number?

15. How is the mass number useful tor telling isotopes apart?

16. What is average atomic mass?

17. How is atomic mass different than atomic number?

18. _______________ atoms (isotopes) spontaneously fall apart after a certain amount of time. The process that occurs when they change into other atoms is called _______________________________________.

19. To have a neutral charge, an atom has to have the same number of protons and ________________.

20. What is an ion?

21. True or false: Positive ions are formed by gaining electrons : _______________

22. Calcium losing two electrons to become Ca2+ would make it a _____________ ion.

23. Complete the graphic organizer below

a.

Building Atoms worksheet

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How is each produced?

Different elements:

Different isotopes:

Different ions:

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Directions: Below you will find the ten most common elements found in Earth’s crust. The element symbol has been given to you on your left. Using the periodic table, complete the chart below.

ELEMENT NAME

ATOMIC #

Atomic Weight/ma

ssPROTON

#Electron

#NEUTRO

N #

Isotope…or New Element?

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H

He

Li

C

O

Ne

Na

Cl

K

Au

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For each problem you are given a pair of elements. Based on the information about each elements, please determine if they are different elements or isotopes of the same element.

1. Element D has 6 protons and 7 neutronsElement F has 7 protons and 7 neutrons

2. Element J has 27 protons and 32 neutronsElement L has 27 protons and 33 neutrons

3. Element x has 17 protons and 18 neutronsElement Y has 18 protons and 17 neutrons

4. Element Q has 56 protons and 18 neutronsElement R has 56 protons and 82 neutrons

5. Element T has an atomic number of 20 and an atomic mass of 40Element Z has an atomic number of 21 and an atomic mass of 41

6. Element W has 8 protons and 8 neutronsElement V has 7 protons and 8 neutrons

7. Element P has an atomic number of 92 and an atomic mass of 238Element S has 92 protons and 143 neutrons

Now, you need to identify each elemnt and give it the proper isotope name.

Example: Element D has 6 protons, which makes it Carbon. Its mass number is 13 (6 protons and 7 neutrons), so the proper name is Carbon-13

Element F: ________________________________

Element J: ________________________________

Element L: ________________________________

Element X: _______________________________

Element Y: _______________________________

Element Q: _______________________________

Element R: ________________________________

Element T: ________________________________

Element Z: ________________________________

Element W: _______________________________

Element V: _______________________________

Element P: _______________________________

Element S: _______________________________

Atomic Mass Worksheet

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} Element OR Isotope

} Element OR Isotope

} Element OR Isotope

} Element OR Isotope

} Element OR Isotope

} Element OR Isotope

} Element OR Isotope

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1. Rubidium is a soft, silvery-white metal that has two common isotopes, Rb-85 and Rb-87. If the abundance of Rb-85 is 72.2% and the abundance of Rb-87 is 27.8%, what is the average atomic mass of rubidium?

2. Uranium is used in nuclear reactors and is a rare element on earth. Uranium has three common isotopes. If the abundance of U-234 is 0.01%, the abundance of U-235 is 0.71%, and the abundance of U-238 is 99.28%, what is the average atomic mass of uranium?

3. Titanium has five common isotopes: Ti-46 (8.0%), Ti-47 (7.8%), Ti-48 (73.4%), Ti-49 (5.5%), Ti-50 (5.3%). What is the average atomic mass of titanium?

4. Calculate the average atomic mass of sulfur if 95.00% of all sulfur atoms have a mass of 32 amu, 0.76% has a mass of 33 amu and 4.22% have a mass of 34amu.

5. Calculate the average atomic mass of bromine. One isotope of bromine has an atomic mass of 79amu and a relative abundance of 50.69%. The other major isotope of bromine has an atomic mass of 81amu and a relative abundance of 49.31%.

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Atomic Drawings Worksheet)

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Draw the model for each of the atoms in the box.

Include the correct number of:

1. Protons2. Electrons3. Neutrons4. Energy levels5. Correctly place electrons

Aluminum

Fluorine

Sodium Magnesium

Lithium Neon

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Atomic # _____

Mass # _____

Protons ____

Electrons ____

Neutrons ____

Atomic # _____

Mass # _____

Protons ____

Electrons ____

Neutrons ____

Atomic # _____

Mass # _____

Protons ____

Electrons ____

Neutrons ____

Atomic # _____

Mass # _____

Protons ____

Electrons ____

Neutrons ____

Atomic # _____

Mass # _____

Protons ____

Electrons ____

Neutrons ____

Atomic # _____

Mass # _____

Protons ____

Electrons ____

Neutrons ____

WORKSHEET 8

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