ELECTRON ARRANGEMENT AND THE PERIODIC TABLE



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|UNIT 2: Atomic Theory and Structure |

|Part D: The Periodic Table of the Elements |

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|Big Picture Idea: An element’s electronic structure determines its chemical and physical properties and therefore its placement on the |

|periodic table. |

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|Big Picture Question: How does the periodic table use physical and chemical properties to arrange the elements? |

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|Suggested Resources… |

|Homework Assignments |

|Classwork Assignments |

|Laboratory Activities |

|Formative Assessments |

|Textbook pages: Chapter 6 |

|Websites: |

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|Key Terms: |

|Mendeleev |

|Moseley |

|Periodic Law |

|period |

|group/family |

|Alkali Metals |

|Alkaline Earth Metals |

|Halogen |

|Nobel Gases |

|metals |

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|nonmetals |

|semimetals/metalloid |

|valence electrons |

|s,p,d,f blocks |

|atomic radius |

|ionic radius |

|ionization energy (+ ion) |

|electronegativity |

|transition metals |

|24. Lanthanide series |

|25. Actinide series |

|26. diatomic elements |

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|Directions: Use this information as a general reference tool to guide you through this unit. Don’t hesitate to ask your teacher for |

|help! |

|By the conclusion of this unit, you should know the following: |By the conclusion of this unit, you should be able to do the |

|Contributions of Moseley and Mendeleev in the development of the |following: |

|current periodic table. |Given a group of atoms, arrange them based on periodic trends. |

|Arrangement of periodic table based on electron configuration and |State the periodic law |

|names of groups/periods. |Know scientists and their contributions to the development of the |

|Group/Period trends for atomic radius, ionization energy, |Periodic Table |

|electronegativity, and metallic character based on atomic |Explain why elements in a group have similar properties |

|structure. |Identify the four blocks on the periodic table |

|Molar mass can be used to covert between grams, moles and molecules|Identify four important periodic trends and explain how each reflects |

|of a diatomic element. |the electron configurations of the elements |

| |Use dimensional analysis to convert between molecules, moles and grams|

| |of a diatomic element. |

Practice Problems:

1. What did Mendeleev contribute and how does this relate to Moseley?

2. What does the Periodic Law state?

3. Look at a periodic table- identify periods, groups, families, s block, p block, d block, f block, alkali metals, alkaline earth metals, halogens, noble gases, metals, semimetals, nonmetals, metalloids .

Draw arrows for ionization energy, atomic radius and electronegativity. Which element is highest for each?

4. Looking at electron configurations, what stays the same and what changes in a family (do it again for a period)?

5. What happens to ion size when ions gain electrons/ when they lose electrons?

6. Rank in order of increasing electronegativity a) Sr, K, Ca b) S, Se, Cl c) B, C, N d) Na, Li, K

7. Rank in order of atomic radius and explain why these trends happen a) Li, Be, B b) S, P, Cl c) Rb, K, Cs d) Na, K, Ca

8. Rank the ions in order of ionic radius, why do these trends happen a) Mg2+, Na+, Al3+ b) Ba2+, Ca2+, Sr2+ c) Se2-, O2-, S2- d) Mg2+, Mg, Ca e) S, S2-, O

9.Rank the atoms from lowest to highest ionization energy a) Cl, Br, Ar b) K, Rb, Na c) C, N, O d) Rb, Ba, Sr

10. Write the short hand electron configuration for element 19, element 53, element 88. Which families do they belong to and give electron dot structure.

11. Specify properties of m, nm, sm. Given an unknown element with some general properties can you identify it as a metal, non-metal, or semimetal?

12. List the diatomic elements.

13. a. Find the mass of 2.5 moles of nitrogen gas. B. How many molecules are in 50.0g of chlorine?

PERIODIC TABLE ELECTRON CONFIGURATION ACTIVITY

1. Complete the chart below.

2. Find the square corresponding to each element on the blank periodic table. Copy the last part of the electron configuration into the periodic table square.

3. Look for patterns, and fill in as many of the squares as you can.

|Element |Electron Configuration |Dot Diagram |

|Hydrogen | | |

|Helium | | |

|Lithium | | |

|Potassium | | |

|Francium | | |

|Beryllium | | |

|Magnesium | | |

|Barium | | |

|Vanadium | | |

|Chromium | | |

|Manganese | | |

|Zinc | | |

|Boron | | |

|Aluminum | | |

|Carbon | | |

|Germanium | | |

|Nitrogen | | |

|Flourine | | |

|Neon | | |

|Xenon | | |

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Reading Electron Configuration Directly from the Periodic Table

|Element |Electron Configuration |

|Cesium |[Xe] 6s1 |

|Strontium |[Kr]5s2 |

|Silicon |[Ne] 3s23p2 |

|Argon |[Ne] 3s23p6 |

|Chromium |[Ar] 4s23d4 |

|Chlorine |[Ne] 3s23p5 |

|Tin |[Kr] 5s24d105p2 |

|Radium |[Rn] 7s2 |

|Nickel |[Ar] 4s23d8 |

|Palladium (Pd) |[Kr] 5s24d8 |

|Antimony (Sb) |[Kr] 5s24d105p3 |

|Francium (Fr) |[Rn] 7s1 |

|Electron Configuration Ending |Element |

|[Ne] 3s2 |Mg |

|[Ar] 4s23d104p5 |Br |

|[Kr] 5s24d3 |Nb |

|[Rn] 7s25f146d107p4 |116 (Uuh) |

|1s22s22p6 |Ne |

|[Kr] 5s1 |Rb |

|[Ar] 4s23d10 |Zn |

|[Kr] 5s2 |Sr |

|[Kr] 5s24d105p3 |Sb |

|[Xe] 6s24f145d4 |W |

History:

Mendeleev 1st periodic table (arranged elements by mass)

Moseley revised periodic table (arranged by atomic number)

Periodic Law the elements physical and chemical properties follow periodic (repeating) trends (based on their location of the periodic table) ***Patters repeat***

Parts of the Periodic Table:

Group/Family column – same valence electrons or outer configuration

Period row, same energy level

Metals good conductor, solid @ room temp., shiny, ductile, malleable, form + ions

Non-Metals poor conductor, solid/liquid/gas @ room temp., brittle, form - ions

Metalloids elements that touch the staircase (except Al), have intermediate properties

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Families

| |Reactivity |Ion Formation |Misc. |

|Alkali Metals |violently |+1 |Not found free in nature, e- |

| | | |configuration ends in s1 |

|Alkaline Earth Metals |very |+2 |e- configuration ends in s2 |

|Transition Metals |More stable |Form ions with more than one charge |Form colored solutions, d block |

|Inner Transition Metals |Many are radioactive |Varying charges |F block |

|Halogens |Most reactive nonmetals |-1 |Diatomic as elements, e- |

| | | |configuration ends in p5 |

|Noble Gases |stable |Do not form ions |Full valence electron shell, e- |

| | | |configuration ends in p6 |

Blocks

s block – 1st 2 columns on left side of the table

p block – last 6 columns on right side of the table

d block – middle 10 columns of the table

f block – lower (removed) 2 rows of the table

CLASSIFYING THE ELEMENTS

Part A Completion

Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number.

The periodic table displays the symbols and _______ the elements along with information about the structures of their _______. The Group 1A elements are called _______, and the Group 2A elements are called _______. The elements in Groups 1A through 7A are called the _______. The nonmetals of Group 7A are _______, and the _______ make up Group 8A. Between Groups 2A and 3A, there are _______in periods 4 through 7 and _______ in periods 6 and 7.

The atoms of the noble gas elements have their highest occupied s and _______ sublevels filled. The highest occupied s and p sublevels of the representative elements are _______.

1. names

2. atoms

3. alkali metals

4. alkaline earth metals

5. representative elements

6. halogens

7. noble gases

8. transition metals

9. inner transition metals

10. p

11. not filled

Part B True-False

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

ST_____ 12. Group A elements are representative elements.

NT 13. Chlorine has the electron configuration 1s22s22p63s23p7.

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

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

Part C Matching

Column A

f 16. alkali metals

e 17. inner transition metal

g 18. representative element

d 19. transition metal

b 20. noble gas

c 21. alkaline earth metals

a 22. halogens

Column B

a. nonmetals of Group 7A

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

c. Group 2A elements

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

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

f. Group 1A elements

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

Worksheet: Periodic Table

For each of the following, circle the correct element.

Li Si S metal

K Ca Sc largest atomic mass

S Cl Ar member of the halogen family

V Nb Ta largest atomic number

Te I Xe member of noble gases

Si Cs B member of alkali metals

As Se Br 6 valence electrons

H Li Na nonmetal

Hg Tl Pb member of transition metals

Na Mg Al electron distribution ending s2p1

Pb Bi Po metalloid

B C N gas at room temperature

Ca Sc Ti electron distribution ending in s2d2

K S Ba has an electron dot like: X:

U Zn Kr member of inner transition metals

Ca S Br forms a +2 ion

F Na Mg member of the alkaline earth metals

Al Cr P 3 valence electrons

Rb I Al forms a -1 ion

H He O a gas that is not reactive

NOTES – PERIODIC TRENDS

Li F

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K

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|Definition |Down a Group |Across a Period |

|Atomic Radius – size of an atom (1/2 the distance |increases down a group because of more energy levels |elements gets smaller (stronger nuclear pull) |

|between 2 nuclei of different atoms) |and more shielding | |

|Ionization Energy - energy needed to remove an electron|Decreases down a group because the electron is far from|increases because nucleus is stronger, better protects |

|from an atom |the nucleus and shielding |electron |

|Electronegativity - ability of an atom to remove and |Decreases down a group because the electron is far from|increases because nucleus is stronger, better able to |

|electron from another atom |the nucleus and shielding from nucleus |take electrons (EXCEPT noble gases) |

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PROBLEMS:

1. Circle the member of each pair that has the greatest radius:

a. oxygen (O) or carbon (C) b. calcium (Ca) or barium (Ba)

c. magnesium (Mg) or phosphorus (P) d. strontium (Sr) or silver (Ag)

2. Arrange the elements below in order of increasing radius:

sodium (Na), potassium (K), nickel (Ni), bromine (Br)

Na ................
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