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Periodic Table

Physical Science Chapter 10

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Organizing the Elements

1. Define the following terms:

a. periodic table=

a. group=

b. periodic law=

c. period=

2. What properties of a deck of cards help Mendeleev?

3. In a periodic table, a set of properties repeat from

a. element to element.

b. column to column.

c. group to group.

d. row to row.

4. Describe how Mendeleev arranged the elements in his periodic table.

5. Circle the letter of each type of information Mendeleev know about each element.

a. Name

b. Number of protons

c. Relative mass

d. Properties

6. Why did Mendeleev leave spaces in his table?

7. What did the discovery of new elements do to Mendeleev’s periodic table?

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8. The usefulness of Mendeleev’s periodic table was confirmed by

a. the discovery of subatomic particles.

b. its immediate acceptance by other scientists.

c. the discovery of elements with predicted properties.

d. the discovery of the nucleus.

9. Scientists before Mendeleev had proposed ways to organize the elements. Why were Mendeleev’s

efforts more successful?

10. Why didn’t Mendeleev arrange is periodic table using protons?

11. How are the elements in the modern periodic table arranged?

12. What is similar in each group?

13. Circle the letters of two elements that have similar properties.

a. Zinc (Zn)

b. Nitrogen (N)

c. Chlorine (Cl)

d. Bromine (Br)

14. How do the properties change across a period?

15. Mendeleev’s table and the modern periodic table organize the elements based on different information,

yet most elements are in the same order in both tables. Explain why.

16. Explain how a calendar is similar to a periodic table and how it is different.

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Periodic Table Overview

17. Define the following terms:

a. atomic mass=

b. atomic mass unit=

c. metals=

d. nonmetals=

e. metalloids=

f. valence electrons=

18. What information is shown in a box on the periodic table?

19. Label the four types of information supplied in the diagram (put the name next to the symbol)

a.

b.

c.

d.

20. What does the atomic mass of an element depend on?

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21. Why is the atomic mass not a whole number?

22. How are elements classified on the periodic table?

23. Which classification are gases?

24. Which classification varies greatly in physical and chemical properties?

25. What two things does the number of valence electrons determine?

26. Why do properties vary across a period?

27. Why do elements in a group have similar properties?

28. Are properties identical for different elements?

29. An element that is shiny and conducts electric current is likely to be what?

30. Are the following sentences true or false?

a. Most elements exist as a mixture of two or more isotopes.

b. All metals react with oxygen in some way.

c. Nonmetals are poor conductors of heat and electric current.

d. Many metals are gases at room temperature.

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Periodic Table Groups

31. Define the following terms:

a. energy levels=

b. electron cloud=

c. orbital=

d. electron configuration=

e. ground state=

f. excited state=

32. What is used to organize the groups?

33. Complete the Table:

Group # of Valence Electrons Elements in the Group

Alkali Metals

Alkaline Earth Metals

Boron Family

Carbon Family

Nitrogen Family

Oxygen Family

Halogens

Noble Gases

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34. Why is hydrogen, a nonmetal, placed in the same group as the alkali metals?

35. How many metalloids are in the boron group?

36. What properties does the carbon group share?

37. How does the nitrogen group vary in its properties?

38. When oxygen reacts with metals, what can it form?

39. Which group does the halogens react readily with?

40. How is the outer shell in the noble gases?

41. Assume you have a sample of an unknown element. At room temperature, it is a soft solid. You cut a

small piece from the sample with a knife and drop the piece into a container of water. It bursts into

flames. Which group of the periodic table does the unknown element belong in?

42. Both hydrogen (H) and helium (He) are gaseous nonmetals. Why are they placed on opposite sides of

the periodic table?

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PPeerriiooddiicc SSqquuaarree You will be choosing an element from the Periodic Table, except for Boron. Using the internet, books, and magazines, you will gather information about your element.

A Lewis Structure is the electron dot diagram.

Bohr Diagram

Protons= Neutrons= Electrons=

Lewis Structure/Electron Dot Diagram

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43. Describe your element (physical description).

44. Who discovered your element?

45. When was it discovered?

46. How is it used?

47. List all the isotopes:

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Using Clues to Identify Elements

Pearson Education, Inc., publishing as Pearson Prentice Hall.

Background Information

Chemical elements can be classified according to their properties as metals, nonmetals, and metalloids. Metals are good conductors of heat and electricity. Many metals are malleable and ductile. Nonmetals are poor conductors of heat and electricity, and solid nonmetals tend to be brittle. Metalloids have properties between those of metals and nonmetals.

Elements in the same group on the periodic table have the same number of valence electrons, which are electrons in the highest occupied energy level of an atom. The number of an A group matches the number of valence electrons in atoms of each element in the group. For example, the Group 14 elements each have four valence electrons per atom. The exception to this pattern is the element helium, which is in Group 18 but has only two valence electrons.

Because elements in a group have the same number of valence electrons, they tend to have similar properties. The most reactive metals are the alkali metals in Group 1 on the far left side of the periodic table. The Group 2 elements are the alkaline earth metals, which are somewhat less reactive than the alkali metals. Groups of elements become less metallic in their properties from left to right across the periodic table. The most reactive nonmetals are the halogens in Group 17. Group 18 contains the noble gases, which are colorless and odorless, and rarely react with other elements.

In this investigation, you will use a list of clues to identify 34 elements and place them in their correct locations in the periodic table.

Problem

Where do the elements described in the clues fit in the periodic table?

Pre-Lab Discussion

Read the entire investigation. Then, work with a partner to answer the following questions.

1. How will the index cards be useful when you are reading the clues to the elements?

2. Do you have to know a specific, identifying property for each element in order to place all 34 elements in the

partial periodic table? Explain your answer.

3. Are elements with similar properties in the same row or the same column of the periodic table?

4. Explain how information about an element’s physical state at room temperature will help you fill in the

partial periodic table.

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5. How would information about number of valence electrons be useful for placing elements in the

periodic table?

6. Why is it important to review the clues after you have read all of the clues once?

Materials 25 cards with numbers on it (last page) plus a copy of the periodic table Procedure

1. Examine the partial periodic table that follows the list of clues. Note that it contains spaces for the 34 elements in Periods 1 through 5 and Groups 1 through 18, skipping the transition metals. The locations of the metalloids are shaded.

2. For this investigation, these 34 elements have been randomly assigned a number from 1 to 34. (Hint: This number has no relation to the atomic number or mass of the element.) By using the list of clues, you will identify where each element belongs in the partial periodic table.

3. Read the clues in order. You will probably find it useful to summarize the information in each clue by using index cards, to which you can refer later as needed. Fill in the partial periodic table by placing each element’s assigned number in the appropriate box. Use a pencil so that you can correct any mistakes.

4. Sometimes a single clue will enable you to identify an element and place its number in the correct box. In most cases, however, you will need to combine information from different clues in order to identify the element.

5. Reread the clues as many times as necessary. When you are certain that you have correctly identified all the elements referred to in a clue, set that index card aside.

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List of Clues

1. Elements 2, 5, 18, 29, and 33 are colorless, odorless, unreactive gases. Of these gases, element 29 has the

largest atomic mass.

2. Elements 13, 19, 23, and 34 have six valence electrons, and element 13 is a metalloid.

3. Elements 9, 14, 16, and 21 are highly reactive metals in the same group. Of these metals, element 16 is the

least reactive.

4. Elements 1, 8, 11, 13, 14, 17, 24, and 29 are in the same period.

5. Elements 11, 26, 27, and 28 have three valence electrons.

6. Elements 1, 4, 6, and 30 are found in the same group. Element 6 is in chlorophyll molecules.

7. Elements 10, 22, 24, and 32 are in the same group. Element 22 is a liquid at room temperature.

8. Elements 2, 10, 15, and 34 are nonmetals in the same period.

9. Elements 7, 15, 17, and 25 are in the same group. Of these, only element 7 is a gas at room temperature.

10. Elements 12, 20, and 26 are metalloids. Elements 20 and 12 are in the same group.

11. Element 30 is important to maintain strong bones and teeth.

12. An atom of element 21 has one more proton than an atom of element 2.

13. Elements 3 is a nonmetal with one valence electron.

14. Element 27 is the most abundant metal in Earth’s crust.

15. Element 31 is a solid at room temperature. Most of the compounds in your body contain this element.

16. Element 18 has two electrons.

17. Element 33 has a smaller atomic mass than element 5.

18. Element 32 is the most reactive nonmetal.

19. Element 20 and element 19 are combined in a compound found in glass.

20. Glass that contains element 26 does not shatter easily.

21. Element 19 is the most abundant element in Earth’s crust.

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Observations

Partial Periodic Table

Analysis and Conclusions

1. Identify each element in the list of clues by matching its assigned number to the correct name of the element.

2. Were you able to place some elements in the partial periodic table with just a single clue? Use examples to explain.

3. Provide at least two examples of when you needed to use more than one clue to identify an element.

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4. Why were you able to use clues about atomic mass to place elements, even though the periodic table is organized by atomic number?

5. Which elements are not included in the partial periodic table? Compare the number of elements in the partial periodic table to the number of known elements.

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