6 p erio dic t table - golden valley high school · 2012. 8. 14. · chapter 6 the periodic table...

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Anticipatory Response Cornell Question & Ans 1. Elements in the same row & Directions:Make 5 questionscolumn behave similarly? Y N & answers that are different2. Alkalis are in column 1? Y N than the Anticipatory Response3. Metalloids are on the stair 1. Steps of the table? Y N 4. Metals are on the right? Y N 5. A family, group, or column Are the same thing? Y N 2. 3. 4. Anticipatory Response 1.Elements are bigger toward The right side of a row? Y N 2. Elements get bigger as you 5. Move down a column? Y N 3. It’s harder to remove an electron from metals? Y N 4. Metals have higher ionization Energies than non‐metals? Y N 5. Shielding remains constant In a row or energy level? Y N Summary Section:

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PERIODIC TRENDS

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Chapter 6 The Periodic Table 131

Section Review

Objectives• Explain how elements are organized in a periodic table

• Compare early and modern periodic tables

• Identify three broad classes of elements

Vocabulary• periodic law

• metals

• nonmetals

• metalloids

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.

Chemists used the of elements to sort them into groups. 1. _______________________

The periodic table organizes the elements into vertical 2. _______________________

and horizontal in order of increasing . The table is 3. _______________________

constructed so that elements that have similar chemical properties 4. _______________________

are in the same . have a high luster, or sheen, 5. _______________________

when cut. Most nonmetals are at room temperature. 6. _______________________

Elements with properties that are similar to those of metals 7. _______________________

and nonmetals are called . Across the periodic table, 8. _______________________

the properties of elements become metallic and 9. _______________________

nonmetallic. 10. _______________________10

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Name ___________________________ Date ___________________ Class __________________

ORGANIZING THE ELEMENTS6.1

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132 Core Teaching Resources

Part B True-FalseClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

________ 10. In his periodic table, Mendeleev arranged the elements in order ofatomic number.

________ 11. There are six periods in a periodic table.

________ 12. Most of the elements in the periodic table are metals.

________ 13. The elements within a period have similar properties.

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.

19. List the elements of Group 5A. Tell whether each is a metal, nonmetal, ormetalloid.

20. List three properties of metals.

21. Name two elements that have similar properties to those of chlorine.

Column B

a. a vertical column of elements in the periodic table

b. good conductors of heat and electric current

c. poor conductors of heat and electric current

d. have properties that are similar to those of metals andnonmetals

e. the horizontal rows of the periodic table

Column A

metals

periods

group

nonmetals

metalloids

________ 14.

________ 15.

________ 16.

________ 17.

________ 18.

Name ___________________________ Date ___________________ Class __________________©

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

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Section Review

Objectives• Describe the information in a periodic table

• Classify elements based on electron configuration

• Distinguish representative elements and transition metals

Vocabulary


The periodic table displays the symbols and of 1.

the elements along with information about the structures of their 2.

. The Group 1A elements are called , and the 3.

Group 2A elements are called . The elements in Groups 1A 4.

through 7A are called the . The nonmetals of Group 7A 5.

are , and the make up Group 8A. Between Groups 6.

2A and 3A, there are in periods 4 through 7 and 7.

in periods 6 and 7. 8.

The atoms of the noble gas elements have their highest occupied 9.

s and sublevels filled. The highest occupied s and p 10.

sublevels of the representative elements are . 11.


________ 12. Group A elements are representative elements.

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• alkali metals

• alkaline earth metals

• halogens

• noble gases

• representative elements

• transition metals

• inner transition metals

Name ___________________________ Date ___________________ Class __________________

CLASSIFYING THE ELEMENTS6.2

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________ 13. Chlorine has the electron configuration 1s22s22p63s23p7.

________ 14. The element in Group 4A, period 3, is gallium.

________ 15. There is a relationship between the electron configurations of elementsand their chemical and physical properties.

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

Part D Questions and ProblemsAnswer the following in the space provided.

23. List the electron configurations for the highest occupied energy level of theelements in period 3 from left to right.

24. List the elements of Group 6A. Tell whether each is a solid, liquid, or gas at roomtemperature and whether it is a metal, nonmetal, or metalloid.

Column B

a. nonmetals of Group 7A

b. an element in which the highest occupied s and psublevels are filled

c. Group 2A elements

d. an element whose highest occupied s sublevel and anearby d sublevel contain electrons

e. an element whose highest occupied s sublevel and anearby f sublevel generally contain electrons

f. Group 1A elements

g. an element whose highest occupied s or p sublevelsare partially filled

Column A

________ 16. alkali metals

________ 17. inner transition metal

________ 18. representative element

________ 19. transition metal

________ 20. noble gas

________ 21. alkaline earth metals

________ 22. halogens

Name ___________________________ Date ___________________ Class __________________©


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Section Review

Objectives• Describe trends among elements for atomic size

• Explain how ions form

• Describe and explain periodic trends for first ionization energy, ionic size, andelectronegativity

Vocabulary


Atomic radii generally as you move from left to right 1.

in a period. Atomic size with atomic number within a 2.

group because there are more occupied and an 3.

increased shielding effect, despite an increase in nuclear . 4.

The energy required to remove an electron from an atom is 5.

known as energy. This quantity generally as you 6.

move left to right across a period. Ions form when are 7.

transferred between atoms. Cations are always than the 7.

atoms from which they form. The ability of an atom to attract 8.

electrons when it is in a compound is called , and this 9.

value as you move from left to right across a period. 10.


________ 11. Compounds are composed of particles called ions.

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• atomic radius

• ion

• cation

• anion

• ionization energy

• electronegativity

Name ___________________________ Date ___________________ Class __________________

PERIODIC TRENDS6.3

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________ 12. Removing one electron from an atom results in the formation of apositive ion with a 1� charge.

________ 13. An anion has more electrons than protons.

________ 14. Elements with a high electronegativity value tend to form positive ions.

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

Part D Questions and ProblemsAnswer the following in the space provided.

21. For the following pairs of atoms, tell which one of each pair has the largest ionic radius.

a. Al, B

b. S, O

c. Br, Cl

d. Na, Al

e. O, F

22. Indicate which element of the following pairs is the most electronegative.

a. calcium, gallium

b. lithium, oxygen

c. chlorine, sulfur

d. bromine, arsenic

Column B

a. half the distance between the nuclei of two atoms of thesame element when the atoms are joined

b. a negatively charged ion

c. the energy required to remove an electron from an atomin its gaseous state

d. an atom or group of atoms that has a positive or negativecharge

e. a positively charged ion

f. the ability of an atom of an element to attract electronswhen the atom is in a compound

Column A

________ 15. ion

________ 16. ionization energy

________ 17. electronegativity

________ 18. atomic radius

________ 19. cation

________ 20. anion

Name ___________________________ Date ___________________ Class __________________©


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Chapter QuizFill in the word(s) that will make each statement true.

1. In the modern periodic table, when elements are arranged 1.according to their atomic , there is a periodic repetition of properties.

2. There are periods in the periodic table. 2.

3. The elements in any in the periodic table have 3.similar physical and chemical properties.

4. Oxygen and sulfur, Group 6A elements, have 4.electrons in their highest occupied energy level.

5. For the inner transition elements, electrons are added to an 5.f sublevel with a principal energy level that is than the period number.

Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

________ 6. The atomic radius of an element in period 3 is larger that the 6.3atomic radius of an element in period 2.

________ 7. For Group 3A elements, there is a relatively small increase in 6.3ionization energy between the second and third ionization energies.

________ 8. Anions are smaller than the neutral atoms from which they are 6.3formed.

________ 9. Atoms with low electronegativity values tend to form positive ions. 6.3

________ 10. As a group, alkali metals have the highest electronegativities. 6.3

56.2

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Name ___________________________ Date ___________________ Class __________________©


THE PERIODIC TABLE6

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Questions About The Periodic Table

1. Which of the following is a NOBLE GAS? a. Oxygen b. Nitrogen c. Hydrogen d. Helium e. all of the above are noble gasses 2. Sodium and Magnesium are both… a. alkali metals b. alkaline earth metals c. metals d. non-metals e. semi-metals 3. The family (column) at the far right side of the periodic table are called… a. the metallic gasses b. the alkaline earth gasses c. the noble gasses d. the smelly gasses e. all of the above 4. A row in the periodic table (across from left to right) is called a… a. period b. family c. group d. semi-family e. none of the above 5. A semi-metal is the same thing as a ….. a. metal b. non-metal c. metalloid d. semi-non-metal e. both a and b above 6. MALLEABLE means… a. breaks easily b. is made of non-metals c. a mixture of metals d. can be bent or pounded into shapes e. can be found in a MALL 7. DUCTILE means … a. that a substance is brittle b. that a substance easily breaks c. that a substance bends

d. that a substance can be pulled into wires e. all of the above

Name

Date Period

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8. Cesium is …. a. an alkaline earth metal b. an alkali metal c. a non-metal d. a semi-metal e. both a and b above 9. Barium is … a. an alkaline earth metal b. an alkali metal c. a non-metal d. a semi-metal e. both c and d above 10. Two or more metals mixed together are called an… a. alloy b. metal soup c. non-metal d. metalloid e. semi-non-metalloid

CIRCLE True or False on the problems below

11. T F An atomic number tells us the number of neutrons in an atom. 12. T F Protons are located in the nucleus of an atom 13. T F Uranium is a metal 14. T F Most elements are non-metals 15. T F Metals do not conduct electricity 16. T F metalloids are found along the “zig-zag” on the periodic table 17. T F metals tend to have very low melting points 18. T F There are no metals that are a liquid at room temperature 19. T F Calcium is a white powder non-metal found in bones. 20. T F All metals conduct electricity. MATCH THE FOLLOWING ON THE LEFT WITH THE CHOICES ON THE RIGHT

21. Argon a. metal 22. Silicon b. non-metal 23. Uranium c. semi-metal 24. Antimony 25. Oxygen 26. Potassium 27. Iron 28. Chlorine 29. Boron 30. Mercury

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Practice ProblemsIn your notebook, solve the following problems.

SECTION 6.1 ORGANIZING THE ELEMENTS1. Which element listed below should have chemical properties similar to

fluorine (F)?

a. Li

b. Si

c. Br

d. Ne

2. Identify each element as a metal, metalloid, or nonmetal.

a. fluorine

b. germanium

c. zinc

d. phosphorus

e. lithium

3. Which of the following is not a transition metal?

a. magnesium

b. titanium

c. chromium

d. mercury

4. Name two elements that have properties similar to those of the elementpotassium.

5. Elements in the periodic table can be divided into three broad classes basedon their general characteristics. What are these classes and how do theydiffer?

Name ___________________________ Date ___________________ Class __________________

THE PERIODIC TABLE6

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SECTION 6.2 CLASSIFYING THE ELEMENTS1. Use the periodic table to write the electron configuration for silicon. Explain

your thinking.

2. Use the periodic table to write the electron configuration for iodine. Explainyour thinking.

3. Which group of elements is characterized by an s2p3 configuration?

4. Name the element that matches the following description.

a. one that has 5 electrons in the third energy level

b. one with an electron configuration that ends in 4s24p5

c. the Group 6A element in period 4

5. Identify the elements that have electron configurations that end as follows.

a. 2s22p4

b. 4s2

c. 3d104s2

6. What is the common characteristic of the electron configurations of theelements Ne and Ar? In which group would you find them?

7. Why would you expect lithium (Li) and sulfur (S) to have different chemical andphysical properties?

8. What characterizes the electron configurations of transition metals such assilver (Ag) and iron (Fe)?

SECTION 6.3 PERIODIC TRENDS1. Explain why a magnesium atom is smaller than atoms of both sodium and

calcium.

2. Predict the size of the astatine (At) atom compared to that of tellurium (Te).Explain your prediction.

3. Would you expect a Cl� ion to be larger or smaller than an Mg2� ion? Explain.

4. Which effect on atomic size is more significant, an increase in nuclear chargeacross a period or an increase in occupied energy levels within a group?Explain.

5. Explain why the sulfide ion (S2�) is larger than the chloride ion (Cl�).

6. Compare the first ionization energy of sodium to that of potassium.

7. Compare the first ionization energy lithium to that of beryllium.

8. Is the electronegativity of barium larger or smaller than that of strontium?Explain.

9. What is the most likely ion for magnesium to form? Explain.

10. Arrange oxygen, fluorine, and sulfur in order of increasing electronegativity.

Name ___________________________ Date ___________________ Class __________________©


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35 Br 79 90

Jeopardy 5 & 6 Study Guide 1‐100 Noble gases have their S & P orbitals filled but alkali metals have their S & P orbital only half filled. 1‐200 1s2 2s2 2p6 3s2 3p4 a. magnesium b. Cobalt c. Sulfur d. Selenium 1‐300 Scandium, Titanium and other elements in the middle of the PeriodicTable are known as ________________

metals or the T____________ elements. 1‐400 The numbers 35, 79.904, & 45 represent 1‐500 Which groups on the Periodic table are the Easiest to predict the Ionic charge or # of valence electrons 2‐100 The atomic radii of which groups is arranged from smallest to greatest distance and Why?

Na, K, Rb, Cs Na, Mg, Al, Si He, Ne, Ar, Kr 2‐200 The ionization energy of the following groups are arranged from smallest to greatest a. Na, Si, Cl b. Na, K, Cs c. Si, P, S 2‐300 Which group decrease in ionic radius Explain why they get small: Na, P, Cl F, Ne, Na 2‐400 Which group increases in shielding.Explain why. Na, P, Cl O, S, Se 2‐500 Which group increases in electronegativities & Why? a. H, Li, Na, b. K, Se, Kr c. N, O, F 3‐100 The below Lewis dot structures are all correct? 3‐200 The Blue, red & brown on this P.T. are: A. alkalis, Alkali earth, halogens B. alkalis, Alkali earth, nobles C. alkalis, Alkali earth, transitions D. none of the above 3‐300 The lewis dot structure for O and S are the same. Explain 3‐400 What is the maximum number of orbitals that the P block has 3‐500 What are the number of electrons that Flourine and Oxygen gain 4‐100 P stands for the: Shape of the orbital The energy level of the orbital The electrons None above 4‐200 In AlCl3 each Al probably lost _____ electrons & each Cl gain _____ electron 4‐300 Oxygen has how many electrons in its outermost energy level? What’s its Lewis Dot? 4‐400 Bohr said that electrons had fixed____________ 4‐500 Which one is Magnesium? Why? 1s2 2s2 2p5 1s2 2s2 2p6 3s2 none correct 5‐100 What is the max # of orbitals in the P‐sublevel? __What the max # electrons?_____ 1 or 2 or 3 or 4 or 5 or 6 5‐200 What is the maximum number of electrons in the 1st 2nd & 3rd energy levels? Hint: 1s2 2s2 2p6 3s2 3p63d10 5‐300 What is true about the spins of the 2 electrons in the 1s2 orbital? both counter clockwise symmetrical NONE 5‐400 What’s the flame test for potassium?_________ Copper? _________ 5‐500 What is the lowest energy level that an electron usually occupies? 6‐100 What color has the shortest wavelength yet the most energy? 6‐200 Which two atoms can have the most violent reactions A. Na, F B. Na, Cl C. Cs, F D. Cs, Cl 6‐300 Mendeleevs Per.Ttable was in order of inceasing atomic _______ Modern tables‐ in order of increasing atomic _. 6‐400 What’s the electron configuration for Chlorine ion Cl‐ which gained an electron [ ] 3s2 __________________. 6‐500 What are the representitive elements A group 1A thru 7A B group B C group C D The alkalis 7‐100 The periodic Table is arranged in increasing ____________________ 7‐200 Which has the same outer configuration as Nitrogen? Oxygen Phosphorus Sulfur Cesium 7‐300 A Metal which becomes a cation usually becomes ______ but _________ musually become bigger 7‐400 Which 6 elements are the metalloids? What is another name for metalloids? 7‐500 Why does the ionization energy increase as you move to the right on the periodic table? 8‐100 Why does atomic size increase toward the left of the Periodic T.? 8‐200 Which in the 2nd period is biggest and why? Lithium Carbon Potassium Cesium 8‐300 S sublevels hold ______ electrons D holds ___ P holds ___ F holds ___ 8‐400 _What is the electron configuration and Lewis dot for Silicon 8‐500 Which element has the correct P & E. A. Zn 30 & 60 B. In 49 & 49 C. Cs 55 & 132.9 D.none above

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Image 1 ___________________________ First Name, Last ________

Period

SCORE: ___/10 pt

6 Periodicity Formative Assessment 3

Write True or False in the blank. 1. Image 1, shows Electronegativity an increase from the left to the right. This is due to

more electrons in the nucleus which can pull on electrons harder.

2. Image 1, shows Ionic Sizes and Shielding to increase from top to bottom of the Periodic Table. This is because there are more energy levels. 3. Below in Graph 1, one can observe that atomic radii decreases as we move from LEFT to RIGHT with in a period or row because of greater proton pull. 4. In Graph 1, one can observe that atomic radii increase as we move down a column Or family because there are more energy levels. 5. In Graph 2, one can observe that ionization energy increases as we move from Left to right with in a period or row because of more protons pulling electrons. 6. In Graph 2, one can observe that ionization energy decreases as we move down a Column or family because of a great atomic radius.

7. Image 1 Which metal is smallest because of the least amount of energy levels & more relative protons or nuclear charge?

A. Li B. Be C. Na D. Ca 8. Which metal has the lowest ionization energy because of relatively few protons for

its’ energy level and yet the most energy levels? A. Rb B. Cs C. Sr D. Ba 9. Which nonmetal has the highest electro-negativity because of the smallest atomic

radius more protons or nuclear charge? A. O B. N C. S D. P 10. Which nonmetal has the smallest radii because of the most protons (nuclear charge)? A. O B. N C. S D. P Graph 1 Graph 2

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___________________________ First Name, Last ________

Period

SCORE: ___/10 pts

s d p

5 Electrons Configuration Formative Assessment 2 Directions: Use the Periodic Table above. Circle the best answer. 1. In what row & period is calcium? 2 3 4 2. In what group or column is calcium? 2 3 4 3. What is Calciums’ outermost electron configuration?

3s2 4s2 4p2 4. In what row & period is Magnesium? 2 3 4 5. In what group or column is Magnesium? 2 3 4 6. What is Magnesiums’ outermost electron configuration?

3s2 4s2 4p2 Directions: Use this true statement to determine if the below questions are True or False.

Bromines’ noble gas shorthand electron configuration is [Ar] 4s2 3d104p5 7. The 4’s in Bromines configuration tell the row, period & energy level. 8. The “ 2 ” & “ 5 ” tells how many “s” & “p” valence electrons are present. 9. The [Ar] represents the inside 16 electrons that Argon has. 10. Bromines Lewis Dot would be: .

: Br : .

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___________________________ First Name, Last ________

Period

SCORE: ___/10 pts

s1 d1 p1

Periodic Table Formative Assessment 1

1. Which does not fit in because 2 elements do not behave similarly? a. groups b. family c. period d. column

2. Which element is in group 2 and period 4? a. Be b. Ca c. Ti d. none correct

3. Which does not fit in? a. family b. period c. row d. energy level

4. Which is an alkali earth metal? a. K b. Mg c. Sc d. Ge e. Br

5. Which is a transition metal? a. K b. Mg c. Sc d. Ge e. Br

6. Which is a metalloid? a. K b. Mg c. Sc d. Ge e. Br

7. Which in a nonmetal? a. K b. Mg c. Sc d. Ge e. Br

8. Where are the metals compared to the stair steps? a. right b. left c. on the steps d. none correct

9. Where are the inner transition metals? a. between the metals & nonmetals b. right of the stair step b. between alkali earth & transitions d. none correct

10. Which electron configuration is a noble gas? a. 1s22s22p6 3s23p6

b. 1s22s22p6 3s23p5

c. 1s2 2s22p6

d. 1s1

e. more than 1 correct

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First Last Name Per Score ___/20

4 & 25 & 5 Cumulative Reteaching 4 Atomic Structure Problem Number

Symbol

Isotope Name

Avg Atomic Mass

Mass Number

Atomic Number =

Neutrons

Electrons

Protons

1. 35 Cl 17

Chlorine‐35 35.5 35 =

2.

17 = 20

3.

Oxygen ‐16

4.

= 9 8

Directions: Look at the above tables & highlight all appropriate answers (all, some or none are correct). 5. Isotopes always share the same: atomic #, protons, electrons, neutrons, mass number 6. Elements are always identified by the same: atomic #, protons, neutrons, atomic mass 7. If the avg. atomic mass of Oxygen is 15.99 a.m.u., which is more abundant? Oxygen – 16 or Oxygen – 15

25 Nuclear Chemistry 8. Proton 9. Electron 10. Beta 11. Alpha 12. Neutron Mass 1 amu Letter P Charge +1 Directions: Look at the above tables & highlight all appropriate answers (all, some or none are correct). 13. Which two have the same mass? (protons, electrons, neutrons) 14. Which two have the same charge? (protons, electrons, beta) 15. Which three have no mass? (electrons, neutrons, gamma, beta) 16. Which has the biggest mass & charge so penetrates the least? (alpha, gamma, beta) Fill in all missing numbers

Reaction type Radioisotope Reactants Reacts To

Produce

Products Fission Or

Fusion 17. Alpha decay Uranium‐ 238 238U

2He

+

18. Which results in a decrease in the atomic number and atomic mass? (Alpha decay, beta decay, Alpha Capture)

5 Electron Configuration Element Electron Configuration Noble Gas Shorthand Highest Energy Level

with Electrons # electrons in highest level Lewis Dot

19. Oxygen 20. 1s2 2s2 2p6 3s2 3p6 4s1 21. In “6s1 “, the 6 represents which 3 (column, group, family, period, row or energy level). 22. In “6s1 “, the s1 represents which one? (alkalis, alkali earth, halogens, noble gas). 23. In “6s1 “, the s1 represents 3 (column, group, family, period, row or energy level). 24. In “6s1 “, the s1 represents how many valence electrons that can lose (1, 2, 3, 6).

Corrected by:_________________

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6 p erio dic t table - golden valley high school · 2012. 8. 14. · chapter 6 the periodic table...

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