name: regents chemistry: mrs. mintz...

Name:

Regents Chemistry: Mrs. Mintz

Practice Packet

Chapter 6: Periodic Table

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WHY?

Substances that contain only atoms with the same number of protons are called elements. The Periodic Table lists all the known elements in order of their atomic number and in columns that depend on similarities in their chemical and physical properties. The Periodic Table is a useful tool for both students and professionals to identify the properties of the elements and understand the properties of molecules.

INFORMATION

Dmitri Mendeleev (1834 − 1907), a Russian scientist, constructed the first Periodic Table by listing the elements in horizontal rows in order of increasing atomic mass. He started new rows whenever necessary to place elements with similar properties in the same vertical column. Mendeleev found that the correlations in properties between some elements in the columns were not perfect. These observations led him to predict the existence of undiscovered elements and to wonder how the table might be better organized. Later H.G.J. Moseley used x-ray spectra to refine the ordering and show that atomic numbers rather than atomic masses should be used to order the elements.

In the Periodic Table, elements with similar properties occur in vertical columns called groups. Two numbering conventions are used to label the groups. The older convention numbers the groups using Roman numerals I through VIII followed by a letter A or B; the other convention numbers each column 1 through 18. The A groups are known as the main group elements. The B groups are called the transition elements. The group numbers IA through VIIIA in the older convention tells you how many valence electrons an element has. The valence electrons are the outer electrons that are most important in determining the chemical bonding and other properties of the element.

The horizontal rows of the table are called periods, and are numbered 1 through 7 starting with the row that only contains H and He.

INFORMATION

There are three categories of elements in the Periodic Table: metals, nonmetals, and metalloids. The metals are located in the left and center. They are good conductors of heat and electricity. The nonmetals are in the upper right-‐hand corner. They are poor conductors of heat and electricity. The metals and nonmetals are separated by the metalloids, which are six elements on a diagonal line. These elements are B, Si, Ge, As, Sb, and Te. The metalloids are also called semimetals or semiconductors because their conductivity is between that of metals and nonmetals. Metals readily lose electrons to form positive ions, called cations, and nonmetals readily gain electrons to form negative ions, called anions.

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KEY QUESTIONS

1. What information about an element is provided in each box for that element in the Periodic Table in the model?

2. What determines the sequence of the elements from the first to the last?

3. What determines where one row stops and another begins? Where are the metals, nonmetals, and metalloids located?

4. What is the difference between a group and a period?

5. How can you determine the total number of electrons that an atom has from the Periodic Table?

6. How can you determine the number of valence electrons that atoms in groups 1, 2 and 13 through 18 have?

www.middleschoolscience.com 2008

Lewis Structures Name:

• Lewis structures, or dot diagrams, are a simplified way to show how the valence electrons are arranged in the outer shell. This is where the chemical reactions take place. Atoms will either share or give away these electrons to form bonds.

• Using your periodic table, determine the number of valence electrons for each element. • Draw a dot to represent each valence electron around the element symbol. • Follow the pattern below starting with position number 1.

Xe

Li Be N C B

Mg P Si Al Na

K Ca

NeF O

S Cl Ar

H He1 5

3 7

6 2

8 4

Examples:

Ba In Se

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Using colored pencils & markers, color the following two periodic tables according to the following directions carefully. Before you begin:

PERIODIC TABLE #1 Draw your staircase à Use your Reference Table and a thick black marker to do this – it must be easily visible! Using pen or pencil, write the atomic symbols and #’s of the elements in the correct box. Now, using THREE DIFFERENT DARK MARKERS, draw a BORDER around the elements that are categorized below. Be sure to include a color key of Table #1. There should not be any empty squares when done.

Semi-‐Metals (Metalloids) à Elements that have characteristics of both metals and nonmetals Metals à These elements easily lose electrons and form positive ions. They have a metallic luster when polished. They also have a sea of valence electrons that aid to help bond themselves to one another. Found to the left of the staircase (be careful for the “1” exception). DON’T FORGET to include the two bottom-‐most rows on the Table! Nonmetals à Elements that are highly electronegative and therefore attract electrons in order to form negative ions. They are also typically covalently bonded to each other or form ionic bonds with metals. Found to the right of the staircase.

___________________________________________

Now, using THREE DIFFERENT COLORED PENCILS, SHADE IN the elements that are: Liquids (at STP) à Br and Hg are the only elements in this state Gases (at STP) à H, N, O, F, Cl, and all the noble gases (group 18) Solids (at STP) à All the rest of the elements (besides liquids and gases)

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Periodic Table #2 Using pen or pencil, write the atomic symbols and #’s of the elements in the correct box. Use a different color for each of the following. Include a KEY at the top or bottom of the periodic table so that others can read and identify the following on your table:

Diatomic Elements à Place a colored border (all the same color) around each of the 7 diatomic elements. Diatomic elements are elements that cannot exist in nature by themselves. They therefore bond to themselves and travel in pairs (ex: N2 instead of N). The seven diatomic elements are H, O, F, Br, I, N, and Cl. The last “7” listed elements form a numeral seven on the Periodic Table and the H is found “UP” to the upper left corner (atomic number 1). Hence, the memory device “7UP.”

Color the following elements by shading in their box with a different color (each group). For the diatomic elements, just simply color within the border that you have already created for them:

• Alkali Metals à All EXCEPT for Hydrogen (it is excluded from this group), these are the Group 1 elements. They are very reactive metals and always form +1 ions within ionic compounds.

• Alkaline Earth Metals à These are the Group 2 elements. They are

reactive, but not as much as the alkali metals. They always form +2 ions within ionic compounds.

• Transition metals à These metals are found in the D-‐block (groups 3-‐12) of

the Periodic Table (the mid-‐section). They can have more than one possible positive charge when part of an ionic compound. We use Roman numerals to denote the charge when naming them. They also usually form colored solutions when mixed with water. This is one of their unique characteristics!

• Halogens à Group 17 elements that are very reactive nonmetals. They usually

have a –1 charge when in ionic compounds.

• Noble Gases à Group 18 elements that are extremely stable & unreactive compounds that do not form bonds with other compounds in nature (AKA inert gases).

• Lanthanoid Series à Top row of the bottommost two rows on table.

Elements 58-‐71.

• Actinoid Series à Bottom row of the bottommost two rows on table. Elements 90-‐103.

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Periodic Table #2

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Questions

1. The periodic table is arranged by increasing ___________________.

2. The periodic table is essentially divided into two categories of elements. Those categories are __________________ and _______________.

3. What do we call the horizontal rows of the periodic table?

4. What do all the elements in a given row have in common?

5. What do we call the vertical columns of the periodic table?

6. What to all the elements in a given column have in common?

7. Are atoms of the elements in the family of noble gases reactive (do readily form bonds with other atoms)? Why is this?

8. The most metallic elements on the periodic table are found in the a. Upper right b. Lower right c. Upper left d. Lower left

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An Alien Periodic Table

Purpose: To correctly place given physical and chemical properties of unknown elements in a blank periodic table Materials: Blank periodic table, modified for this activity List of observations of the unknown elements Pencil Background Information: Earth’s scientists have announced that they have made radio contact with intelligent life on a distant planet. One of this alien planet’s languages has been translated, and scientific information has begun to be exchanged. The planet is composed of the same elements as Earth. However, the inhabitants of the planet have different names and symbols for them. Since the alien scientists do not know the names of our elements, they have radioed the following data on the known properties of the elements. Strangely, but luckily, there are no transition or rare earth elements on the alien planet. This means that their periodic table consists only of the “A” groups of elements. The data are as follows:

1. The inert gases are bombal (Bo), wobble (Wo), jeptum (J), and logon (L). Bombal (Bo) is a noble gas but does not have 8 valence electrons. The outside energy level of logon (L) is its second energy level. Of these noble gases, wobble (Wo) has the greatest atomic mass.

2. The alkali metals are xtalt (X), byyou (By), chow (Ch), and quackzil (Q). Of these alkali metals, chow (Ch) has the lowest atomic mass. Quackzil (Q) is in the same period as wobble (Wo).

3. The halogens are apstrom (A), vulcania (V), and kratt (Kt). Vulcania (V) is in the same period as quackzil (Q) and wobble (Wo).

4. The metalloids are Ernst (E), highho (Hi), terriblum (T), and sississ (Ss). Sississ (Ss) is the metalloid with the highest atomic mass. Ernst (E) is the metalloid with the lowest atomic mass. Highho (Hi) and terriblum (T) are in Group IV. T has more protons than Hi. The element called yazzar (Yz) is a metalloid by location but has properties that suggest it is a light metal.

5. The most metallic element on the planet is called xtalt (X). The most chemically active nonmetal on the planet is called apstrom (A). The lightest element on the planet is called pfsst (Pf). The heaviest element on the planet is elrado (El). It is highly radioactive.

6. The chemical makeup of the alien planet’s oceans seems to be about the same as Earth’s oceans. When seawater is distilled, the liquid that is boiled off and then condensed has been shown to have molecules consisting of two atoms of pfsst (Pf) and one atom of nuutye (Nu). The solid left behind after the distillation consists mainly of a crystal made up of the elements byyou (By) and kratt (Kt).

7. The element called doggone (D) has only 4 protons in its atom. 8. Floxxit (Fx) is a black crystal with 4 electrons in the outer shell. Both rhastrap (R) and

doadeer (Do) have atoms with four energy levels. But R is less metallic than Do.

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9. Magnificon (M), goldy (G), and sississ (Ss) are all members of Group V. G has fewer total electrons than M.

10. Urrp (Up), oz (Oz), and nuutye (Nu) all gain 2 electrons. Nu is diatomic. Oz has a lower atomic number than Up.

11. The element anatom (An) tends to lose 3 electrons. The elements zapper (Z) and pie (Pi) both lose 2 electrons. Pi loses them from its fifth energy level, while Z loses them from its third. Procedure: Fill in the blank periodic table with the correct alien planet symbol for each element. The symbol is given in parentheses after the element name in the data statements.

1. Most elements that occur in the same group (family) on the periodic table have

similar chemical characteristics. Explain why this is true? __________________________________________________________________________________________________________________________________________________________________________________________________

2. What happens to valence electrons as you move left to right in a row?

__________________________________________________________________________________________________________________________________________________________________________________________________

3. What are 4 common properties of metals? __________________________________________________________________________________________________________________________________________________________________________________________________

4. What are 4 common properties of non-‐metals? __________________________________________________________________________________________________________________________________________________________________________________________________

5. Hydrogen is obviously not an alkali metal. Why is it in column 1 of the table? __________________________________________________________________________________________________________________________________________________________________________________________________

Name: Element 118, Heaviest Ever, Reported for 1,000th of a Second

A team of Russian and American scientists said yesterday that it had created the heaviest element ever seen in a laboratory, a dab of matter that lasted for less than one-‐thousandth of a second but would add an entry at the farthest reaches of the periodic table and suggest that strange new elements may lie beyond.

By convention, the substance remains the Baby Doe of elements until its existence is confirmed at other laboratories. For now, the new substance will be principally known as element 118 for the number of protons in its nucleus, more than in any other element occurring naturally or produced in the laboratory.

Sabrina Fletcher and Thomas Tegge/Lawrence Livermore National Laboratory Calcium, with 20 protons, being accelerated into Californium, with 98 protons. Sabrina Fletcher and Thomas Tegge/Lawrence Livermore National Laboratory The new element traveling through the accelerator to the detector.

Hydrogen, the lightest element, has one proton in its nucleus, and uranium, the heaviest naturally occurring element, has 92. Element 118 would fit comfortably just below radon in a column of the periodic table containing what are called noble gases for their inert chemical properties.

The results were met with praise but also caution from other scientists in the field, particularly given the fraught history of element 118. Another California lab, the Lawrence Berkeley National Laboratory, announced that it discovered the element in 1999 but retracted the claim two years later after an investigation found that one of its researchers, Dr. Victor Ninov, had fabricated data. Dr. Ninov was later fired.

Dr. Ken Moody, the lead American researcher on the work, said everything had been done to guard against fabrication, with independent analyses being carried out in Russia and the United States. And the group’s paper on the putative find has been accepted at a prestigious journal, Physical Review C, after other scientists reviewed the work, said Dr. Jonathan Lenaghan, an editor at the journal.

But it was less the fear of fraud than ordinary scientific caution that caused some scientists to reserve judgment on the discovery. The Russian lab and its collaborators have now

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announced the discovery of five elements — 113, 114, 115, 116 and now 118 — none of which have been confirmed by other scientists.

“One has to be extremely careful with those enthusiastic announcements,” said Dr. Witold Nazarewicz, a nuclear theorist at the University of Tennessee and the Oak Ridge National Laboratory.

“This is not because one is doing something wrong,” Dr. Nazarewicz said. “It’s because these are very difficult measurements. They are playing on the edges of statistics.”

The team that created the element, made up of scientists at the Lawrence Livermore National Laboratory in California and the Joint Institute for Nuclear Research in Dubna, Russia, said they had produced three atoms of the new element in six months of smashing lighter elements together and trying to make them stick.

The scientists said their results also gave hope that they were approaching a long-‐predicted “island of stability” of even heavier elements, with longer lives and possibly strange new chemical properties.

“This considerably expands the borders of the existing material world,” Dr. Yuri Oganessian said in an e-‐mail message. He is the scientific director of the Flerov Laboratory of Nuclear Reactions at the Dubna institute, where the experiments were carried out in a cyclotron, the circular particle accelerator.

A Livermore scientist, Dr. Nancy J. Stoyer, said the team had calculated that there was less than one chance in 100,000 that the results were a statistical fluke.

“We’re very confident,” Dr. Stoyer said.

Other experimental scientists said nothing was obviously amiss with the work.

“I think the evidence they have is convincing,” said Dr. C. Konrad Gelbke, director of the National Superconducting Cyclotron Laboratory at Michigan State University. “It looks pretty good.”

The experiments were performed when scientists at the Russian laboratory used the cyclotron to bash atoms of calcium, with 20 protons, into a target of Californium, with 98 protons, like little clumps of putty that they hoped would stick together, said Dr. Dawn A. Shaughnessy, another Livermore scientist who worked on the experiment.

In extremely rare instances, they did stick. In 10 billion billion bombardments, detectors found that the two sets of protons glommed together to produce element 118.

An element’s weight is determined by the total number of protons, which have a positive electrical charge, and neutrons, which are neutral, in its nucleus.

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By that measure, too, the new element is the heaviest ever created.

Dr. Gelbke said that there was one good reason that the Russian laboratory might be ahead of its competitors elsewhere in the world. Scientists at that lab, he said, are skilled in handling Californium, which is very radioactive and dangerous to the uninitiated.

“I wouldn’t want to do that myself,” Dr. Gelbke said, chucking. “It’s a fairly nasty substance for most people to handle.”

If the results are confirmed, they would represent one more step toward the “island of stability” that theorists have predicted in even heavier regions of the periodic table. Nuclei have shell-‐like structures, and the most stable atoms contain so-‐called “magic numbers” of protons and neutrons that produce closed, or complete, shells.

The numbers 2, 8, 20, 28, 50 and 82 are magic for both protons and neutrons. The highest known magic number for neutrons alone is 126, meaning that common lead, with 82 protons and 126 neutrons, is the heaviest known “doubly magic,” or extremely stable, isotope in the periodic table.

But the theorists have predicted that there is another closed shell out beyond all elements discovered so far, including the latest one.

“It’s rather like Plum Island at the end of Long Island,” Dr. Martin Blume, the overall editor of Physical Review, said. “You go there, there’s a gap, and then there’s Plum Island.”

There is general agreement that the next neutron magic number is 184. But that is still out of reach of current experiments.

The next proton magic number is a matter of disagreement.

“That is, I think, the basis for looking in this region,” Dr. Blume said. “Have you reached the island of stability?”

http://www.nytimes.com/2006/10/17/science/17heavy.html?ref=chemistry&_r=0

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Chemistry Literacy -‐ Heavy Element 118 Chemistry -‐ Breed

Directions: Take a few minutes to read the article below either online (or on the back of this page.) Write responses to the statements or questions below. Cut/copy/paste is not allowed – use your own words and thoughts, based in research if needed.

Read more: http://www.nytimes.com/2006/10/17/science/17heavy.html?ref=chemistry Fact-‐finding: List three facts that you learned in this article.

1.

2.

3.

Vocabulary: List and define three unfamiliar words in the space below.

Implications: What are your feelings about this “discovery”? Express your feelings (tactfully) about whether this is an advancement of science or a bad idea.

Example: H = .37cm Example: H = 1.31 cm Example: Li = 0.76 cm Example: H = 1.10 cm

Part 1: ATOMIC

RADIUS

Draw a circle to depict

the size of an atom of

each element using the

measurements below.

Scale: 1cm =1/2 Å

atomic

radius

1 H 0.37

2 He 0.31

3 Li 1.52

4 Be 1.12

5 B 0.85

6 C 0.77

7 N 0.75

8 O 0.73

9 F 0.72

10 Ne 0.71

11 Na 1.86

12 Mg 1.60

13 Al 1.43

14 Si 1.18

15 P 1.10

16 S 1.03

17 Cl 1.00

18 Ar 0.98

19 K 2.27

20 Ca 1.97

31 Ga 1.35

32 Ge 1.22

33 As 1.20

34 Se 1.19

35 Br 1.14

36 Kr 1.12

Part 2: IONIZATION

ENERGY

Draw an “energy bar” to

depict the energy

needed to remove one

electron.

Scale: 1cm=1kJ/mol

ionization energy

1 H 1.31

2 He 2.40

3 Li 0.52

4 Be 0.90

5 B 0.80

6 C 1.09

7 N 1.40

8 O 1.31

9 F 1.68

10 Ne 2.08

11 Na 0.50

12 Mg 0.74

13 Al 0.59

14 Si 0.79

15 P 1.06

16 S 1.00

17 Cl 1.26

18 Ar 1.52

19 K 0.42

20 Ca 0.59

31 Ga 0.58

32 Ge 0.78

33 As 1.01

34 Se 0.94

35 Br 1.14

36 Kr 1.35

Part 3: IONIC

RADIUS

Draw a circle to depict

the size of an ion of

each element.

Scale: 1cm=1/2 Å

ionic

radius

1 H -

2 He -

3 Li 0.76

4 Be 0.31

5 B 0.20

6 C -

7 N 1.46

8 O 1.40

9 F 1.33

10 Ne -

11 Na 1.02

12 Mg 0.72

13 Al 0.54

14 Si 0.41

15 P 2.12

16 S 1.84

17 Cl 1.81

18 Ar -

19 K 1.38

20 Ca 1.00

31 Ga 0.62

32 Ge 0.53

33 As 2.22

34 Se 1.98

35 Br 1.95

36 Kr -

Part 4: ELECTRO-

NEGATIVITY

Draw a bar to depict the

ability of an element’s

atoms to attract

electrons in a chemical

bond.

scale: 1cm = 1 Pauling

electro-

negativity

1 H 2.1

2 He -

3 Li 1.0

4 Be 1.5

5 B 2.0

6 C 2.5

7 N 3.0

8 O 3.5

9 F 4.0

10 Ne -

11 Na 0.9

12 Mg 1.2

13 Al 1.5

14 Si 1.8

15 P 2.1

16 S 2.5

17 Cl 3.0

18 Ar -

19 K 0.8

20 Ca 1.0

31 Ga 1.6

32 Ge 1.8

33 As 2.0

34 Se 2.4

35 Br 2.8

36 Kr -

1 1 1 3

1

2 13 14 15 16 17

2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 31 32 33 34 35 36

Atomic Radius (Scale: 1 cm = ½Å)

1 18

1

2 13 14 15 16 17

2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 31 32 33 34 35 36

Ionization Energy (Scale: 1 cm = 1 kJ/mol)

1 18

1

2 13 14 15 16 17

2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 31 32 33 34 35 36

Ionic Radius (Scale: 1 cm = ½Å)

1 18

1

2 13 14 15 16 17

2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 31 32 33 34 35 36

Electronegativity (Scale: 1 cm = 1 Pauling)

1 18

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Periodic Trends Summary

Directions: Write “increases” or “decreases” on the line.

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Love Always, Francium by Becky Ratzlaff

Dear John,

I’m writing to tell you that I can’t marry you—I’m breaking our engagement. I guess you want to know why, so let me explain. I’ll start at the beginning. . .

It all started when I was born the daughter of Actinium-‐227 by alpha emission. I not only grew up unstable, but my psychiatrist recently diagnosed me as a paranoid schizophrenic and said she has trouble telling my 20 isotopes apart. The sad truth is that 223Fr (my longest lived isotope) has a half-‐life of only 21 minutes, after which I decay into that awful 223Ra! And my 221Fr has a half-‐life of only 4.8 minutes! So you see, there’s no use continuing our relationship when I won’t be around long.

I was a quiet child. When my existence was finally discovered in 1939 by Marguerite Perey at the Curie Institute in Paris, I was thrilled! They named me Francium after the country in which I was discovered. They introduced me to my sisters: Lithium, Sodium, Potassium, Rubidium, and Cesium. Soon I learned that, as members of the Alkali metal family, we had a lot in common. We all had a valence of one, tarnished in air, had low melting points, and reacted with water. Not only that, we generally had soft crystals and were commonly found as halides and as aluminosilicates and combined vigorously with other elements.

Father said that the strong similarity between my sisters and me was the arrangement of the electrons in our atoms. But then, Father always had an explanation for everything. I asked him once why he liked Lithium best. He said he loved us all equally and that I was only being my unstable self. But I kept bugging him, and finally he admitted that he liked Lithium best because she was used in the treatment of steel parts and was making something of her life. He said I had no meaningful purpose that he could see. Then he looked me up and down and grunted that I ought to do something about my atomic weight. I ran to my room in tears and looked in the mirror. My atomic weight was around 223, more than anyone else in my Alkali metal family. John, I just can’t bear it! You saw how futile my attempts to diet were.

Sitting in the Earth’s crust the way I do in tiny amounts (never more than one ounce), I have a lot of time to think. It isn’t so bad having a melting point of 27 °C, and my changes of phase add some excitement to my life. But something has been bothering me. Even though I was discovered more than 30 years ago, my sisters still leave me out of everything. The Alkali family has always been famous, but nobody knows the real me! Why, I remember that in “Inorganic Chemistry,” R. T. Sanderson said, “Relatively little is known of this element except that a close resemblance to Cesium has been recognized.”

Cesium! He compared me with Cesium—my sister who hangs out in a mineral called pollucite. No one would ever catch a weighable amount of me in that trash! I’m sorry-‐there I go being unstable again.

Hey, did you hear that people are actually cloning me? It’s true! What they do is bombard thorium with protons, and they’ve got instant artificially made Francium. Neat, isn’t it? Who knows? Maybe some day, good old atomic number 87 will find her niche in society, and I will be accepted for what I am! But until then, I know we could never be right for each other.

John, I am really sorry. Please try to understand. I will always love you and will never forget our half-‐lives together.

Love always Francium Alkali

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Questions

1. Write the nuclear reaction that produced Francium.

2. How many different isotopes of Francium exist? _________________

3. Write the nuclear reaction for Francium-‐223 the longest-‐lived isotope? What type of radiation particle is produced? _________________

4. Which country discovered Francium? ___________________________

5. Who are the “sisters” of Francium and what do they have in common?

6. To which group/family does Francium belong? _________________________________

7. What period does Francium belong to? _____________________

8. Is Francium classified as a metal, nonmetal or metalloid?

9. What is Francium’s: a. Electron configuration ____________________________________

b. Melting Point ____________________________________

c. Atomic Radius ____________________________________

d. Ionization energy ____________________________________

e. Electronegativity ____________________________________

f. Average atomic mass ____________________________________

10. Why is Francium Alkali ending her relationship with John?

Directions: Put a check in each box that applies to each term listed.

Conduct Electricity

Very Reactive

High Luster

Brittle All Solids at STP

All Gases at STP

Can be Solid, Liquid or Gas at STP

High Electro- negativity and Ionization energy

Large Atomic Radius

Form Cations

Form Anions

Metals

Nonmetals

Metalloids

Alkali Metals

Alkaline Earth Metals

Halogens

Noble Gases

Transition Metals

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Periodic Table Transfer Task

Background: Walter White has devised a plan to communicate the name of his secret project to his accomplices, which will tell them which person will be in charge of the project. He only left a strange set of clues to them about different elements in the Periodic Table which will help them figure out where his sinister plot will be carried out. As a member of the CIA, you have been tipped to some of the cipher (code) that Walter uses. Also, you have been told it will occur at a State Capitol building. Using the directions below, determined by your brave, devoted, fearless, genius, awesome chemistry teachers, FOIL WALTER’S PLOT!!!! Determine at which state’s capitol building the crime will be committed, and therefore, the accomplice who will be in charge of the crime!! Good luck!!

Accomplice Location Fred Vermont Agatha Virginia Arnold California Tony New York Billy-‐Bob-‐Ray Arkansas Sue-‐Ann Alabama Vivian Florida Blaine Minnesota

Directions: For each of the following unknown elements, use the clues to determine the element being described. Along the way, please circle any multiple choices (shown in bold) and fill in any blanks within the questions. When you determine the element, write its element symbol in the box provided. When finished, rearrange the element symbols to decode Heisenberg’s accomplice. Element #1: Answers: 1. The radius decreases when an atom of this element forms an ion. Metal/Non-‐metal 2. Unknown element has electrons in four energy levels. Period/Group: ____(number) 3. Not a colorful compound or ion 4. Has a higher ionization energy than potassium

Element #2: 5. Contains five valence electrons in the ground state Period/Group: ____(number) 6. Has properties of metals and non-‐metals Type of element: ___________ 7. Has a higher electronegativity value than zinc Element #3: 8. It is shiny and malleable. Metal/Non-‐metal

9. It forms an oxide with the formula X2O. Period/Group: ____(number)

10. At STP, it is the solid with the smallest nuclear charge in its group.

1

2

3

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Element #4: 11. Diatomic molecule at STP Possible elements: __________ 12. In the halogen family Period/Group: _____(number) 13. Solid at STP 14. Sublimes at room temperature Element #5: 15. Atoms of this element form anions. Metal/Non-‐metal 16. Is a diatomic molecule at STP Possible elements: __________ 17. Located in a group that contains elements that exist as all Group: ____ (number)

three phases at STP 18. Highest electronegativity in the group Top/Bottom of group

Element #6: 19. Nonconductor Metal/Non-‐metal 20. Monatomic gas Possible Elements: __________ 21. 8 valence electrons Period/Group: ____ (number)

22. Highest shielding in its group for naturally occurring elements Element #7: 23. Gains electrons when forming an ion Metal/Non-‐metal 24. Smaller atomic radius than carbon Possible elements: __________ 25. Least metallic in its group Top/Bottom of group

26. Diatomic gas at room temperature Possible elements: __________

27. Has two allotropes in our atmosphere

Combine the symbols of the unknown elements to solve the question:

_______ _______ _______ _______ _______ _______ _______

1 3 5 7 6 4 2

Who will commit the crime???? ___________________________________________________________

7

6

5

4

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