1

Unit 10:

The Periodic Table

(Chapter 6)

Name ____________________________________________________ Period ___________________

2

THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155–160) This section describes the development of the periodic table and explains the periodic law. It also describes the classification of elements into metals, nonmetals, and metalloids. Searching For An Organizing Principle (page 155)

1. How many elements had been identified by the year 1700? ________________

2. What caused the rate of discovery to increase after 1700? _____________________________________

_________________________________________________________________________________________

3. What did chemists use to sort elements into groups? __________________________________________

_______________________________________________________________________________________

Mendeleev’s Periodic Table (page 156)

4. Who was Dmitri Mendeleev? _______________________________________________________________

5. What property did Mendeleev use to organize the elements into a periodic table?

_________________________________________________________________________________________

6. True/false? Mendeleev used his PT to predict the properties of undiscovered elements.__________

The Periodic Law (page 157)

7. How are the elements arranged in the modern periodic table? _________________________________

8. True or false? The periodic law states that when elements are arranged in order of increasing atomic

number, there is a periodic repetition of physical and chemical properties. ______________________

Metals, Nonmetals, and Metalloids (pages 158–160)

9. Explain the color coding of the squares in the periodic table in Figure 6.5. _______________________

________________________________________________________________________________________

10. Which property below is not a general property of metals.

a. ductile b. poor conductor of heat c. malleable d. high luster

11. True/False. The variation in properties among metals is greater than the variation in properties

among nonmetals. __________________

12. Under some conditions, a metalloid may behave like a _____________________ .

Under other conditions, a metalloid may behave like a _____________________ .

3

SECTION 6.2 CLASSIFYING THE ELEMENTS (pages 161–167)

This section explains why you can infer the properties of an element based on the properties of other

elements in the periodic table. It also describes the use of electron configurations to classify elements.

5. Classify each as a (an) alkali metal, alkaline earth metal, halogen, or noble gas.

a. sodium ______________________ e. xenon ______________________

b. chlorine ______________________ f. potassium ______________________

c. calcium ______________________ g. magnesium ______________________

d. fluorine ______________________

6. How many electrons are in the highest occupied energy level?

a. Group 3A __________ b. Group 1A __________ c. Group 8A __________ it

8. Circle the letter of the elements found in the p block.

a. Groups 1A and 2A and helium

b. Groups 3A, 4A, 5A, 6A, 7A, and 8A except for helium

c. transition metals

d. inner transition metals

Match the category of elements with an element from that category.

_______________ 9. Noble gases a. gallium

_______________ 10. Representative elements b. nobelium

_______________ 11. Transition metals c. argon

_______________ 12. Inner transition metals d. vanadium

13. Use Figure 6.12 on page 166. Write the electron configurations for the following elements.

a. magnesium ______________________________________

b. cobalt ______________________________________

c. sulfur ______________________________________

4

Historical Figures in Chemistry

The arrangement of elements in the

modern periodic table is clearly connected

to atomic structure. However, the concept

of the periodic table has been known for

more than 100 years, and it was developed

long before our more recent knowledge

of electron configurations. The history of

the ideas of chemical periodicity is filled

with interesting people, and one of the

most important was the Russian chemist

Dmitri Mendeleev (1834 - 1910).

In the 19th century many chemists tried

to find relationships between atomic

weights and the properties of the elements.

These efforts largely failed because atomic

weights were not known for all elements,

and many measured values were inaccurate.

However, at a conference in 1860 in Germany,

Stanislao Cannizzaro (1826 - 1910) described his

method for determining accurate and unambiguous

atomic weights, and this began to set things right.

Mendeleev was at the conference and doubtless

head Cannizzaro’s paper. It led him to become the

founder of the concept of chemical periodicity.

Mendeleev’s ideas on periodicity began in the late

1860’s with his work on a book on inorganic

chemistry. To help organize the material for his book,

he had a file of note cards, one for each element. On

each card he wrote the atomic weight of the

element, then known more accurately owing to

Cannizzaro’s work, and some properties of the

element. When he arranged these cards in order of

increasing atomic weight, he saw there was a

repetition of properties every eight or eighteen

elements. Thus was born Mendeleev’s periodic table.

More than 100 years later, we recognize Mendeleev’s

work as a milestone, because he had the genius to

realize that (a) there were many elements to be

discovered and (b) the characteristics of an element

could be predicted from its atomic weight and its

position on the table. Mendeleev’s table led directly

to the discovery of several elements within a few

years after he published the table.

In spite of Mendeleev’s great achievement,

problems arose when new elements were discovered

and more accurate atomic weights were determined.

Using the modern periodic table,

look at the following pairs of

elements: Ar and K, Te and I, and

Co and Ni. In each case, the first

element has the greater atomic

weight. Arranging them in order of

increasing atomic weight would

place a very reactive metal in the

column with the very inert elements.

The fault lies in Mendeleev’s

assumption that properties of

elements are periodic functions of

their weight.

H.G.J. Moseley, a young scientist

working with Ernest Rutherford,

found that the wavelengths of x-rays emitted by an

element are related in a precise way to the atomic

number of the element. He quickly realized that

other atomic properties may be related to atomic

number and not, as Mendeleev had proposed, to

atomic weight. Indeed, if the elements are arranged

by atomic number, the defects in Mendeleev’s table

are corrected. It was therefore Moseley who

discovered the law of chemical periodicity, which

states that the properties of elements are periodic

functions of their atomic numbers.

After Mendeleev published his work on chemical

periodicity, he did little else with the subject. Instead,

he went on to other interests. In 1876 he visited the

US to study the fledgling oil industry and was

impressed by the industry but not the country.

America, he thought, was not interested in science,

and even worse, carried on the worst features of

European civilization.

One final note: All pictures of Mendeleev show

him with long hair. He made it a rule to get his hair

cut only once a year, in the spring, whether he

needed it or not.

Dmitri Mendeleev and the Periodic Table

A young Dmitri Mendeleev

Dmitri Mendeleev in 1904

5

6

Properties of the groups on the periodic table

Circle the correct answer

1. Mendeleev noticed that properties of elements appeared at regular intervals when the elements

were arranged by

a. atomic mass. c. reactivity.

b. number of protons. d. atomic number.

2. Elements in the same group or column on the periodic table can be expected to have similar

a. atomic masses. c. atomic numbers.

b. number of neutrons. d. properties.

3. The radioactive elements with atomic numbers from 89-102 on the periodic table are referred to as

the

a. noble gases. c. lanthanides.

b. actinides. d. halogens.

4. Argon, krypton, and xenon are all

a. noble gases. c. alkaline earth metals.

b. actinides. d. transition elements.

5. Elements on the right side of the periodic table tend to exhibit properties of

a. nonmetals. c. metals.

b. metalloids. d. gases.

6. Elements in which the d sublevel is being filled exhibit properties of

a. nonmetals. c. metals.

b. metalloids. d. gases.

7. Since the column one elements are highly reactive, these alkali metals exist as ______ in nature.

a. elements. c. compounds.

b. solutions. d. gases.

8. Compared to the alkali metals, the alkaline earth metals

a. are less reactive. c. are less dense.

b. have lower melting points. d. combine more readily with nonmetals.

9. What group of elements reacts vigorously with water?

a. halogens c. noble gases

b. alkali metals d. transition metals

10. Tungsten and copper are elements that belong to the

a. halogens. c. noble gases.

b. alkali metals. d. transition metals.

11. The most reactive nonmetals are the

7

a. halogens. c. noble gases.

b. oxygen family of elements. d. 1s electron filling elements.

Fill in the blank with the correct word or phrase.

12. The Law _________________________________________________________________, also called the

Periodic Law, states that “the physical and chemical properties of elements are periodic functions of

their atomic numbers.”

13. The work of _________________________________ led to the periodic table based on atomic number.

14. Neutral atoms with an s2p

5 configuration are called _____________________________________.

15. Elements that border the “staircase” on the periodic table are called _____________________________.

true or false:

16. Elements in the same row have similar electron configurations. _________________

17. Elements in the same column exist in the same phase at room temperature. _________________

18. Elements in the same family must all be metals or nonmetals. _________________

19. Elements in the same period have their valence electrons in the same energy level. ________________

20. Elements in the same group have similar chemical properties. _________________

8

SECTION 6.3 PERIODIC TRENDS (pages 170–178) This section explains how to interpret group trends and periodic trends in atomic size, ionization energy, ionic size, and electronegativity. Trends in Atomic Size (pages 170–171) 1. True/false? The radius of an atom can be measured directly. ______________________

2. What are the atomic radii for the following molecules?

molecule Hydrogen Oxygen Nitrogen Chlorine

atomic radius _____________ _____________ _____________ _____________

3. What is the general trend in atomic size within a group? Within a period? _______________________

________________________________________________________________________________________

4. What are the two variables that affect atomic size within a group?

a. _____________________________________ b. _____________________________________

5. For each pair of elements, pick the element with the largest atom.

a. Helium & argon _____________________ b. Potassium & argon _____________________

6. What is an ion? _________________________________________________________________________

7. How are ions formed? ___________________________________________________________________

8. An ion with a (+) charge is called a(n) ___________; an ion with a (-) charge is called a(n) __________.

9. Complete the following table about anions and cations.

Anions Cations

Charge

Metal/Nonmetal

-/+

Trends in Ionization Energy (page 173 - 175)

10. ______________________ is the energy required to overcome the attraction of protons in the nucleus

and remove an electron from a gaseous atom.

11. Why does ionization energy tend to decrease from top to bottom within a group? ________________

_________________________________________________________________________________________

12. Why does ionization energy tend to increase as you move across a period? ______________________

_________________________________________________________________________________________

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Trends in Ionic Size (page 176)

14. Metallic elements tend to ______________________ electrons and form ______________________ ions.

Nonmetallic elements tend to ____________________ electrons and form ____________________ ions.

15. Circle the letter of the statement that is true about ion size.

a. Cations are always smaller than the neutral atoms from which they form.

b. Anions are always smaller than the neutral atoms from which they form.

c. Within a period, a cation with a greater charge has a larger ionic radius.

d. Within a group, a cation with a higher atomic number has a smaller ionic radius.

16. Which ion has the larger ionic radius: Ca+2 or Cl- ? ________

Trends in Electronegativity (page 177)

17. What property of an element represents its tendency to attract electrons when it chemically

combines with another element? _____________________________

18. Use Table 6.2 on page 177. What trend do you see in the relative electronegativity values of elements

within a group? Within a period? ___________________________________________________________

19. Circle the letter of each statement that is true about electronegativity values.

a. The electronegativity values of the transition elements are all zero.

b. The element with the highest electronegativity value is sodium.

c. Nonmetals have higher electronegativity values than metals.

d. Electronegativity values can help predict the types of bonds atoms form.

Summary of Trends (page 178)

20. Use Figure 6.22 on page 178. Circle the letter of each property for which aluminum has a higher

value than silicon.

a. first ionization energy b. electronegativity c. atomic radius d. ionic radius and the

group 1A

Reading Skill Practice

A graph can help you understand comparisons of data at a glance. Use the graph paper

(in landscape orientation) on the next page to make a graph of the data in Table 6.2 on

page 177. Plot electronegativity values on the vertical axis. Use a range from 0 to 4. Plot

atomic number on the horizontal axis. Label each period and the first element in each

period.

10

11

Significance and Use of the Periodic Table

DISCUSSION: When the Russian chemist, Dimitri Mendeleev, designed the first Periodic Table, he left blanks for elements he knew had not yet been discovered. His table was so accurate for the s and p electron columns that he was able to predict the properties of these elements. Since none of the atomic particles had been discovered by the 1860’s, he knew nothing about electron configurations, so he had to base his predictions solely on observable chemical and physical properties. We have looked at four trends in atomic properties — atomic and ionic radii, ionization energy, electronegativity, and electron affinity. In this “experiment,” you will play the role of a modern-day Mendeleev and predict some atomic and physical properties of four “unknown” elements from their location in the table.

PROCEDURE: Use the data contained in the periodic table on the next page to predict the properties of elements T, X, Y, and Z. 1. Base your predictions on the properties of

neighboring elements and the apparent trends which occur across a period and down a group of the table. The properties which you will predict are shown below.

Mendeleev Games

atomic # melting point

symbol

electronegativity I.E.

atomic radius

12

Name _________________________________________________________________ Period _____________

periodic table of the representative elements of periods 2-6

CONCLUSION: Use the data provided in the table and your predictions to answer the following

questions.

1. Write the definition for each of the following trends. Then write the general trend that occurs for the following properties across a period from left to right and down a group: a. electronegativity: _______________________________________________________________

______________________________________________________________________________________

______________________________________________________________________________________

b. atomic radius: _________________________________________________________________

______________________________________________________________________________________

______________________________________________________________________________________

c. ionization energy (I.E.): _________________________________________________________

______________________________________________________________________________________

______________________________________________________________________________________

2. Examine the melting point data. As one moves across a period, the melting point increases at first, and then decreases. Make a prediction as to why this occurs. _________________________________________________________________________________

________________________________________________________________________________________

13

According to the periodic table on the front of this page:

3. What element has the highest electronegativity? _______ Lowest electronegativity ________

4. Complete the following charts for element T, X, Y, and Z.

Element T

symbol

name

predicted EN

shorthand SN

common ion(s)

formula of oxide

compound

(ionic bond)

Element Y

symbol

name

predicted

atomic radius

shorthand SN

common ion(s)

formula of oxide compound

(ionic bond)

Element X

symbol

name

predicted EN

shorthand SN

common ion(s)

formula of oxide

compound (ionic bond)

Element Z

symbol

name

predicted

atomic radius

shorthand SN

common ion(s)

formula of hydrogen

compound (ionic bond)

14

15

Periodic Trends Online Tutorial DIRECTIONS: 1. Go to: http://www.wwnorton.com/web/chem1e/. Click on the picture 2. Near the top left hand corner of the page, click on “Choose a chapter.” Click on Chapter 8: Chemical bonding

and atmospheric molecules

3. Scroll down to where it says, “Chapter 8 ChemTours” & choose “Periodic Table.” Answer the following questions 1. Why is the periodic table useful? _____________________________________________________________________ __________________________________________________________________________________________________ 2. _______________________ developed the first periodic table. He used TWO criteria to organize the

elements. What were they? _______________________________________________________________

3. The atomic number is the number of ________________________ in an element.

4. In a neutral atom, the number of _________ equals the ____________________ ___________________ 5. The mass of a sample of an element is the weighted ____________ of the different mass values of its isotopes. 6. The periodic table is divided into several vertical columns called ______________________, in which the elements have similar ________________________ _______________________. 7. By moving your mouse over several of the red group numbers, name and describe 6 groups on the PT.

a. ______________________________________________________________________________________________

______________________________________________________________________________________________

b. ______________________________________________________________________________________________

______________________________________________________________________________________________

c. ______________________________________________________________________________________________

______________________________________________________________________________________________

d. ______________________________________________________________________________________________

______________________________________________________________________________________________

e. ______________________________________________________________________________________________

______________________________________________________________________________________________

f. ______________________________________________________________________________________________

______________________________________________________________________________________________

8. The horizontal rows on the periodic table are called _______________________. 9. The period number of each row corresponds to the _____________________ ______________________. 10. Name the two series or periods that appear at the bottom of the periodic table. The ______________________ ____________________, which is part of period _____________.

The ______________________ ____________________ , which is part of period ____________.

NAME _____________________________________________________ PERIOD _________

16

11. Describe a metalloid? ______________________________________________________________________________ __________________________________________________________________________________________________ 12. Define electronegativity. ___________________________________________________________________________

__________________________________________________________________________________________________ 13. What Nobel Prize winner developed the electronegativity scale? __________________ ________________ 14. What is the highest electronegativiy that an element can have? ______________ 15. What is the trend in electronegativity on the periodic table? ____________________________________________ __________________________________________________________________________________________________ 16. Define atomic radius. _______________________________________________________________________________

__________________________________________________________________________________________________ 17. What is the trend in atomic radius on the periodic table? ________________________________________________ __________________________________________________________________________________________________ 18. Arrange the following elements – Pr, Ag, Ra, F, Ge – in order of a.) increasing atomic radius ____________________________________

b.) increasing electronegativity ____________________________________

THE FOLLOWING QUESTIONS ARE #1-4 ON THE TUTORIAL 1. Which element has the following ground state electron configuration? a.) [Kr]4d

55s

2 ________ b.) [Ar]3d

104s

24p

4 ________ c.) [Xe]6s

1 ________ d.) 1s

22s

22p

3 ________

2. Answer the question and sketch your answer on the periodic tables below.

Increasing Increasing Electronegativity Atomic Radius Based on the trends of the periodic table, circle the element below that you would expect to have the greatest electronegativity.

3. a. Sb b. Br c. As 3. a. Ca b. Sr c. Ba Based on the trends of the periodic table, circle the element below that you would expect to have the greatest atomic radius. 4. a. Ag b. Cu c. Au

4. a. Rb b. Zr c. Sn

17

Periodic Trends Review

1. Finish the following sentences with, “increases,” or “decreases.”

a. As one moves from left to right across a period, the atomic size ___________________.

b. As one moves from top to bottom in a group, the atomic size ____________________.

c. As one moves from left to right across a period, the electronegativity ______________.

d. As one moves from top to bottom in a group, the electronegativity ________________.

e. As one moves from left to right across a period, the ionization energy ______________.

f. As one moves from top to bottom in a group, the ionization energy _______________.

2. In each of the following sets of elements, which element has the smallest atomic size?

a. Na, K, Rb ___________ e. Ba, Ca, Ra ___________

b. Na, Si, S ___________ f. P, Si, Al ___________

c. N, P, As ___________ g. Rb, Cs, K ___________

d. N, O, F ___________ h. Cu, Ge, Bi ___________

3. Arrange the following sets of elements in order of increasing atomic size.

a. Sn, Xe, Rb, Sr ____________________________________________

b. Rn, He, Xe, Kr ____________________________________________

c. Pb, Ba, Ca, At ____________________________________________

4. In each of the following sets of elements, which element has the largest electronegativity?

a. Na, K, Rb ___________ d. Ba, Ca, Ra ___________

b. Na, Si, S ___________ e. P, Si, Al ___________

c. F, Cl, Br ___________ f. Zn, Ag, Pt ___________

5. In each of the following sets of elements, which element has the smallest ionization energy?

a. N, P, As ___________ d. Rb, Cs, K ___________

b. N, O, F ___________ e. Cu, Ge, Br ___________

c. Fr, Sr, V ___________ f. Sn, As, S ___________

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Factors affecting periodic trends

Factor Definition Effect Result

Nuclear Charge

As the nuclear charge _______ across a period, the attraction between the protons & outermost electrons _______, thus causing……

Atomic size _____

Ionization E ____

Atomic Size

Down a group, as the outer electrons get further from the nucleus (more energy levels), the electrostatic attraction _______, thus causing……

Atomic size _____

Ionization E ____

Shielding Effect

As the number of inner shell electrons __________ down a group, the electrostatic attraction_______, thus causing…..

Atomic size _____

Ionization E ____

Electron Configuration

Filled and half-filled sublevels are more _________________, thus causing…..

Exceptions to some trends

19

Investigating the periodic trends among the elements

INTRODUCTION:

March Madness is upon us! Every sports fan around the nation completes a bracket and tries their best to predict the winners and losers for each round of the national basketball championship. Creating the brackets, however, has a so-called scientific foundation called "bracketology." The NCAA Selection Committee uses this method to seed the field by ranking all teams from first through sixty-eight. In this lab you will apply the principles of bracketology to the properties of the elements. The competition among the 64 elements is stiff, and there is a wealth of information to research. Good luck and enjoy this, “elementary" version of March Madness. REVIEW OF ELEMENT PROPERTIES: Use your book (pages 170 - 178) and/or prior knowledge to define each of the following properties of the elements and describe any periodic trend in the property across a period or down a group. 1. Electronegativity a. Definition - _________________________________________________________________________ ______________________________________________________________________________________ b. Periodic Trend - _____________________________________________________________________ ______________________________________________________________________________________ 2. Atomic Radius a. Definition - _________________________________________________________________________ ______________________________________________________________________________________ b. Periodic Trend - _____________________________________________________________________ ______________________________________________________________________________________ 3. Ionization Energy a. Definition - _________________________________________________________________________ ______________________________________________________________________________________ b. Periodic Trend - _____________________________________________________________________ ______________________________________________________________________________________

It’s Elementary – March Madness

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SUMMARY OF PERIODIC TRENDS: Fill in the lines with the appropriate periodic trend (electronegativity, atomic radius, or ionization energy) from page 1. NOTE: Pay close attention to the direction of the arrows. You are not filling in the periodic table with element symbols. DETERMINE WHICH TRENDS DECREASE & INCREASE AS ONE MOVES UP THE PERIODIC TABLE AND TO THE RIGHT.

______________________________________________________DECREASES

______________________________________________________INCREASES

______________________________________________________INCREASES

__________

__________

__________

__________

__________

DECREASES

__________

__________

__________

__________

__________I

NCREASES

__________

__________

__________

__________

__________I

NCREASES

21

It’s Elementary – March Madness

22

CONCLUSION: Answer the following questions. 1. Which element won "Elemental March Madness?" _______________________________ 2. Write its shorthand spectroscopic notation. _______________________________ 3. Draw its Lewis Structure. _______________________________ 4. Predict all stable ions that the atom can form. _______________________________ 5. Draw the Lewis Dot Structure for the ion(s). _______________________________ 6. Go to the website: http://www.chemicool.com/

Use the periodic table to research the champion and answer the following questions:

a. List five common uses

b. For each of the champion’s opponents compare the actual atomic radii, electronegativity (EN), and first ionization energy. Was your prediction correct?

Atomic Radii

Round

Champion

Opponent

Prediction Correct? (Y or N)

EN

Round

1st IE

ROUND

23

Periodicity Review

Ion Formation Review

Ions are formed by the _________________________ of electrons between atoms.

Metals _____________________ e- to form ________________________.

Nonmetals _________________________ e- to form ________________________.

24

Ionic Size

When metals ______________________ electrons they become _________________.

When nonmetals __________________ electrons they become _________________.

So…… cations are always ________________________ than the atom.

antion are always _______________________ than the atom.

Atom vs. Cation

Atom vs. Anion

25

Examples: 1. Circle the particle in each pair that has the larger radius.

a. K, K

+ c. O, O

-2

b. Br, Br

- d. Sb, Sb

+3

2. In each pair, circle the larger ion:

a. Sr

+2 , Be

+2 c. Te

-2 , I

-1

b. Fe

+2 , Fe

+3 d. Cs

+1 , Tl

+3

3. Which of the following atoms increase in size when they become ions?

Cs, I, Zn, O, Sr, Al

4. List the following ions in order of increasing ionic radius: Na

+ , Cl

- , S

-2 , F

-1 , Al

+3 , Se

-2

__________________________________________________________

26

Atomic Size Decreases

Electronegativity Increases

Ionization Energy Increases

Atom vs. Ion

*Positive ion is always SMALLER than the atom (ex: Ca+2 is smaller than Ca)*

*Negative ion is always BIGGER than the atom (ex: S-2 is larger than S)*

Ato

mic

Siz

e D

ecre

ase

s

Ele

ctr

on

eg

ati

vit

y In

cre

ase

s

Ion

iza

tio

n E

ne

rgy In

cre

ase

s

Size of cations decreases Size of anions decreases

27

Atomic Size

Definition: the approximate size of an atom’s electron cloud Trend Across a Period: As the pull of the nucleus on the outer electrons increases, the size of the

atom decreases. Trend Down a Group: As the number of energy levels increases, the size of the atom also

increases.

Positive Ion Size

Definition: the approximate size of an cation’s electron cloud

General Trend: When forming cations, electrons are removed but the nuclear charge remains the same. Therefore, positive ions are always smaller than their corresponding atoms.

Trend Across a Period: As the pull of the nucleus on the remaining outer electrons increases, the size of the ion decreases

Trend Down a Group: As the number of energy levels increases, the size of the cation also increases.

Negative Ion Size

Definition: the approximate size of an anion’s electron cloud

General Trend: When forming anions, electrons are gained but the nuclear charge remains the same. Therefore, because of the overabundance of electrons which repel one another, negative ions are always larger than their corresponding atoms.

Trend Across a Period: As the pull of the nucleus on the outer electrons decreases, the size of the ion decreases.

Trend Down a Group: As the number of energy levels increases, the size of the anions also increases.

Electronegativity

Definition: the measure of the ability of an atom to attract electrons to itself in a

covalent bond. EN is a rating system, not a measurement. Trend Across a Period: As the pull of the nucleus on the outer electrons increases, the

electronegativity increases. Trend Down a Group: As the number of energy levels increases, the electronegativity decreases.

Ionization Energy

Definition: the quantity of energy required to remove one electron from an atom;

high IE indicates that it is difficult to remove an electron Trend Across a Period: As the pull of the nucleus on the outer electrons increases, the ionization

energy of the atom increases (harder to remove) Trend Down a Group: As the number of energy levels increases, which increases the shielding

effect, the ionization energy of the atom decreases (easier to remove an electron).

28

Name ____________________________________________________ Period ___________________

THE PERIODIC TABLE - Vocabulary Review

Match the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line. Each answer can only be used once.

a. representative elements h. ionization energy o. ionic radius b. electronegativity i. transuranium elements p. ion c. atomic radius j. alkali metals q. anion d. metals k. inner transition metals r. halogens e. cation l. alkaline earth metals s. nonmetals f. nuclear charge m. shielding effect t. noble gases g. transition elements n. period u. group ___________ 1. Elements found in groups 1A – 8A. Most of their highest occupied s and p

sublevels are partially filled.

___________ 2. Group B metals in which the highest s sublevel and a nearby d sublevel

generally contain electrons.

___________ 3. Elements in group IIA that have only 2 e- in the highest occupied E level.

___________ 4. One half the distance between the nuclei of two atoms of the same

element when the atoms are joined.

___________ 5. The approximate size of a cation’s or anion’s electron cloud.

___________ 6. The measure of the ability of an atom to attract electrons to itself in a

covalent bond; a rating system, not a measurement.

___________ 7. An atom or group of atoms that has a positive or negative charge.

___________ 8. Elements in group 8A, in which the highest occupied s and p sublevels are

filled.

___________ 9. Nonmetals of group 7A.

__________10. Elements in which the highest s sublevel and a nearby f sublevel generally

contain electrons; an element in the lanthanide or actinide series; also called

rare earth elements

__________11. The quantity of energy required to remove one electron from an atom; high

values indicates that it is difficult to remove an electron.

__________12. A positively charged ion. Are always smaller than their atom.

__________13. Group 1A elements, which have only 1 e- in the highest occupied E level.

__________14. Good conductors of heat and electricity. They can be found on the left side

of the staircase, center, and bottom of the periodic table.

__________15. Poor conductors of heat and electricity. They can be found to the right side

of the staircase.

__________16. The number of p+ in the nucleus--it increases across a period.

__________17. The inner shell e- shield the outermost e- from the pull of the nucleus.

__________18. A negatively charged ion. Are always larger than their atom.

__________19. Elements found after uranium on the periodic table. They are not found in

nature, they are man-made.

__________20. Horizontal row on the periodic table. __________21. Vertical column on the periodic table.

29

Name ____________________________________________________________ Period ________________

Periodic Table Review

1. Why did Mendeleev leave spaces in his periodic table? ___________________________________________

___________________________________________________________________________________________

2. Identify each property below as more characteristic of a metal or a nonmetal.

a) a gas at room temperature ____________________________________________

b) malleable ____________________________________________

c) poor conductor of electric current ____________________________________________

d) shiny ____________________________________________

3. In which group are the following located in the periodic table:

a) alkali metals ______ b) halogens ______ c) alkaline earth metals ______ d) noble gases ______

4. Write the shorthand spectroscopic notation for the following elements:

a) boron ____________________________________________

b) arsenic ____________________________________________

c) fluorine ____________________________________________

d) zinc ____________________________________________

e) aluminum ____________________________________________

5. Circle the element in each pair that has atoms with a larger atomic radius.

a) sodium, lithium b) strontium, magnesium c) carbon, germanium d) selenium, oxygen

6. Circle the element in each pair that has a greater ionization energy.

a) lithium, boron b) magnesium, strontium c) cesium, aluminum d) fluorine, bromine

7. Circle the particle in each pair that has the larger radius.

a) Na atom, Na+ b) S, S-2 c) I atom, I-1 d) Al atom, Al+3

8. For which of these properties does lithium have a larger value than potassium?

a) ionization Energy b) atomic radius c) electronegativity d) ionic radius

9. Write the symbol of the element or elements that fit each description.

a) A nonmetal in Group 4A ____________________________

b) Inner transition metal with lowest atomic number ____________________________

c) A metal in group 5A ____________________________

d) All the nonmetals for which their atomic number is a multiple of 5 ____________________________

10. In each pair, circle the larger ion:

a.) Ca+2, Mg+2 b) Cl-1, P-3 c) Cu+1, Cu+2 d) Si, Si-4 e) Li+1, Rb+1

30

Standardized Test Prep

1) Which of the following properties increase as you move across a period from left to right? I. electronegativity II. ionization energy III. atomic radius

a) I and II only b) I and III only c) II and III only d) I, II, and III e) III only 2) Which group has the symbols for sodium, sulfur, and cesium in order of increasing atomic radii.

a) Na, S, Cs b) Cs, Na, S c) S, Na, Cs d) Cs, S, Na e) Na, Cs, S 3) The electron configuration for an element in the halogen group should always end with

a) ns2np6. b) ns2np5. c) ns2np4. d) ns2np2. e) ns2np1.

4) If the pictures above represent the potassium atom and ion.

a) Which sphere would most likely represent the atom? __________ The ion? __________

5) If the pictures above represent the sulfur atom and ion.

a) Which sphere would most likely represent the atom? __________ The ion? __________

Use the data table to answer question 6

6) Is the relationship between the following properties inverse (I) or direct (D)?

a) atomic radius and IE ______ b) atomic radius and EN ______ c) IE and EN ______

Each of the following questions are false. Explain why.

7) Electronegativity values are higher for metals than for nonmetals because atoms of nonmetals are

among the largest atoms. ______________________________________________________________________

____________________________________________________________________________________________

8) A calcium atom is larger than a calcium ion because ions are always smaller than the atoms from which

they are formed. ______________________________________________________________________________

_____________________________________________________________________________________________

9) The element hydrogen is a metal because it is on the left in the periodic table. _________________________

____________________________________________________________________________________________

10) Among all the elements in a period, the noble gas always has the smallest ionization energy because

within any period, atomic radii tend to decrease moving from right to left. __________________________

___________________________________________________________________________________________

Alkali Metal

Atomic Radius

Ionization Energy (IE)

Electronegativity Value (EN)

Li 152 pm 520 kJ/mol 1.0

Na 186 pm 495.8 kJ/mol 0.9

K 227 pm 418.8 kJ/mol 0.8

Rb 244 pm 250 kJ/mol 0.8

Cs 262 pm 210 kJ/mol 0.7

a. b.

31

The Periodic Law Pretest

Choose the letter of the correct answer AND explain the reason for your answer in the spaces provided. ____________ 1. According to the modern periodic law the properties of the elements are a

periodic function of their a. ionic size. c. atomic mass. b. ionization energy. d. atomic number. ___________________________________________________________________________________________ ____________ 2. Which of the following properties has a higher value for aluminum than silicon? a. Ionization energy c. Atomic size b. Electronegativity d. All of the above ____________________________________________________________________________________________ ____________ 3. The electron configuration of an element ends with 4s1. Which of the following

describes the element’s family? a. transition metal c. alkaline earth metal b. noble gas d. alkali metal ____________________________________________________________________________________________ ____________ 4. The more an atom wants to lose an electron, the ___________ its ionization energy

value is. a. higher c. none of the above. b. lower d. all of the above. ____________________________________________________________________________________________ ____________ 5. Neutral atoms with an s2p6 end notation would be classified as a a. noble gas. c. transition metal. b. halogen. d. alkali metal. ____________________________________________________________________________________________ ____________ 6. Elements in a group have similar chemical properties because of similar a. nuclear structure. c. principal quantum number. b. outer electron configuration. d. mass number. ____________________________________________________________________________________________ ____________ 7. The energy required to remove an electron from an atom is the atom’s a. electron affinity. c. electronegativity. b. electron energy. d. ionization energy. ____________________________________________________________________________________________

32

____________ 8. The electron configuration of a potassium ion, K+, matches that of an atom of a. argon. c. sodium. b. calcium. d. krypton. ____________________________________________________________________________________________ ____________ 9. The electronegativity value of Mg is ______ than Al’s. a. greater c. less b. the same as d. none of the above. ____________________________________________________________________________________________ ____________ 10. Which of the following has the largest electronegativity? a. cesium c. arsenic b. sodium d. chlorine ____________________________________________________________________________________________

33

The Periodic Law Practice Test Choose the best answer. 1. What two properties did Mendeleev use to organize his Periodic Table?

a. Chemical properties and atomic mass. c. Periodic trends and atomic number. b. Periodic trends and number of protons. d. Similar electron configurations and atomic mass.

2. Moseley developed the first Periodic Table based on atomic

a. mass. c. size. b. weight. d. number.

3. According to modern periodic law the properties of the elements are periodic functions of their

a. ionization energy. c. ionic size. b. atomic mass. d. atomic number.

4. The more an atom wants to lose an electron, the ___________ its ionization energy value is.

a. higher c. none of the above. b. lower d. all of the above.

5. Neutral atoms with an s2p6 end notation would be classified as a a. noble gas. c. transition metal. b. halogen. d. alkali metal.

6. Elements in a group have similar chemical properties because of similar

a. nuclear structure. c. principal quantum number. b. outer electron configuration. d. mass number

7. Which of the following statements is true?

a. The size of a cation is larger than the size of its neutral atom b. The size of a cation is smaller than the size of its neutral atom. c. The size of an anion is smaller than the size of its neutral atom. d. None of the above.

8. The electron configuration of a rubidium ion, Rb+, matches that of an atom of a. He c. Ar b. Ne d. Kr

9. Which of the following is listed in order of decreasing electronegativity?

a. chromium, carbon, cobalt c. carbon, cobalt, chromium b. chromium, cobalt, carbon d. None of the above.

10. Which of the following has the largest electronegativity?

a. potassium c. astatine b. sodium d. bromine

11. Which of the following properties decreases as you move across a period from left to right?

I. Electronegativity II. Ionization energy III. Atomic size a. I only. c. I and II only. b. III only. d. I, II, and III.

True or False.

34

12. Among all the elements in a period, the noble gas always has the largest ionization energy. _______ 13. It is more difficult to remove an electron from strontium than beryllium. _______ 14. Francium is the most electronegative element. _______ 15. The barium atom is smaller than the barium ion. _______ 16. The P-3 ion is smaller than the P atom. _______ 17. The noble gases are the most reactive nonmetals. _______ 18. Electronegativity values are lower for metals than for nonmetals. _______ 19. Atomic radius and electronegativity have similar trends. _______ 20. Atoms and moles are conserved in a chemical reaction. _______ 21. Aluminum is a metalloid. _______ 22. The alkali metals are the most reactive metals on the periodic table. _______

Cumulative Review 23. How many significant figures are in the measurement 0.000456 grams?

a. 2 c. 6 b. 7 d. 3

24. How many formula units are contained in one mole of calcium chloride?

a. 6 c. 6.02 x 1023 b. 111 d. 3.6 x 1024

25. Pick the best term to describe a banana split.

a. heterogeneous mixture c. element b. compound d. solution

26. The products of a complete combustion reaction are

a. carbon monoxide and water. c. oxygen and hydrogen. b. carbon dioxide and water. d. oxygen and water.

27. What are the most common ions formed by the lead atom?

a. -2, -4 c. +2, +3 b. +1, +2 d. +2, +4

28. The presence of hydroxide in a chemical formula indicates that the compound is a(n)

a. base. c. hydrate. b. acid. d. salt.

29. The formula for ammonia is ______.

a. NH4 c. NH3 b. NH2 d. NH4

+1 30. An element in the ‘f’ block of elements would best be described as(n)

a. transition metal. c. inner transition metal. b. noble gas. d. halogen.

31. An element that is a poor conductor of heat and electricity is

a. sulfur. c. gold. b. copper. d. titanium.

32. The most common type of ion formed by Group IIIA is a(n)

a. cation b. anion

35

Periodic Law Prelab

In this lab we are going to use water displacement to calculate the volume of a metal sample. To do this properly, we need to determine the best instruments to use by being aware of the error that can evolve from measurements. Determine the calibration and estimated column of the following graduated cylinders. Then read the instruments and place the answer in the space provided.

Cal ___________________ Cal ___________________ Est ___________________ Est ___________________

________________________ _______________________ The volume of the sample is _________________________________.

The mass of the sample of copper is 0.22 g.

The density of copper is __________________________.

How do you know that this answer cannot be correct? ___________________________________.

What changes to your technique would eliminate this error in your result?

____________________________________________________________________________________

Let’s use another student’s volume measurement.

Volume __________________________ Density ___________________________

Should the answers at least be close to each other? _______________ Are they? ______________

36

Let’s do the same thing, only this time we will use a larger sample that weighs one hundred times the first sample – 22 g and a different graduated cylinder.

_______________________ _______________________ The volume of the sample is _________________________________.

The density of copper is __________________________.

Does this seem more plausible than the first result? ___________________________________.

Compare your answer to another student who has a different volume. Are your results more

similar than the first trial? _____________________________________________________________

This exercise should show you the importance of using the appropriate size sample for the equipment you choose. Remember to read the

instruments properly and make sure your answers make sense!

37

Examination of some periodic properties of the elements

INTRODUCTION:

When the elements are arranged in order of increasing atomic number, there is a periodic

recurrence of properties that leads to the grouping of elements in the periodic table. Elements in vertical columns form groups or families that are characterized by marked similarities in physical and chemical properties. These similarities are due, in large part, to the fact that all the elements within a group have the same outer-shell electron configuration. H. G. J. Moseley formulated this trend into the Law of Chemical Periodicity. Within a group, periodic trends of certain properties can be observed. The properties of density and

solubility of compounds, for example, are known to vary regularly within groups of elements. In this experiment, you will investigate the periodic variation of density and solubility of compounds within groups. Specifically, you will determine the densities of certain elements in Group IVA and the solubilities of certain salts of Group IIA elements. You will then use your results to make predictions of the densities of other Group IVA elements and the general trend that exists among the solubilities of alkaline earth metal ions.

OBJECTIVES:

To examine the periodic variation of the density and solubility of compounds within groups of elements.

To make predictions of densities of untested Group IVA elements.

MATERIALS: lead shot, Pb 0.1 M barium nitrate

silicon, Si 0.1 M calcium nitrate tin, Sn 0.1 M magnesium nitrate test tube rack 0.1 M strontium nitrate distilled water 1 M sodium carbonate 4 small test tubes 1 M potassium chromate 0.25 M ammonium oxalate, (NH4)2C2O4 PROCEDURE:

Part A. Densities of Group IVA Elements 1. Obtain dry samples of tin (1 piece), lead (a

spoonful or two), and silicon (a few pieces). 2. Collect the data necessary to determine the

densities of the tin, lead, and silicon samples by

the water displacement method. The amount of sample and the equipment used is up to you, so be smart about it to obtain accurate results.

3. Place the wet samples in the properly labeled beakers on the center distribution table. DO NOT throw them away.

Part B. Solubilities of Salts of Group IIA Elements

1. Obtain four test tubes; clean them thoroughly with soap and water. Rinse with distilled water.

2. To the first tube, add 1 mL ( roughly 20 drops) of Mg(NO3)2 solution. To the second tube, add 1 mL of Ca(NO3)2 solution. To the third tube, add 1 mL of Sr(NO3)2 solution, and to the fourth, 1 mL of Ba(NO3)2 solution. Note that these volume measurements need only be approximate as this procedure is qualitative.

3. Add 1 mL of 1M potassium chromate solution to each test tube to provide the chromate ions for

reaction with the Group IIA metal ions. If the metal chromate salt (MgCrO4, CaCrO4, SrCrO4, or BaCrO4) is insoluble in water, the solution will become cloudy and a thick precipitate will be formed upon addition of K2CrO4. If the salt is slightly insoluble in water, the solution will produce a few specs of solid. If the metal chromate salt is soluble in water, the solution will remain clear upon addition of K2CrO4. Record the solubility of each metal chromate salt as S (soluble), SI (slightly insoluble) or I (insoluble).

4. Rinse the test tubes with distilled water; repeat step 2.

5. Add 1 mL of 0.25 M ammonium oxalate, (NH4)2C2O4, to each test tube. Record your solubility results.

6. Rinse the test tubes with distilled water; repeat step 2 again.

7. Add 1 mL of 1M sodium carbonate to each test tube. Record your solubility results.

8. Clean the test tubes; return them to their original location.

CONCLUSIONS:

1. Calculate the densities of the Si, Sn, and Pb samples. Record in Table 1. You do not need to show your work.

Answer questions 2-5 below the tables.

2. Using a complete sentence, state a general trend in density for elements in the same group on the periodic table.

3. Predict the numeric densities of carbon and germanium. Explain your reasoning.

4. Using a complete sentence, state a general trend in solubility for the alkaline earth metals.

5. Predict the solubilities of the beryllium and radium salts. Explain your reasoning.

The Periodic Law

38

Names ______________________________________________________________ Period _________

Table 1: Densities of Group IVA Elements

Si Sn Pb

mass of metal

volume of water

volume of water & metal

volume of metal

density of metal

Table 2: Solubilities of Salts of Group IIA Elements CrO4

-2 C2O4-2 CO3

-2

Mg+2

Ca+2

Sr+2

Ba+2

2. _________________________________________________________________________________

_________________________________________________________________________________

3. Density of C ______________________________

_________________________________________________________________________________

Density of Ge _____________________________

_________________________________________________________________________________

_________________________________________________________________________________

4. _________________________________________________________________________________

5. _________________________________________________________________________________

_________________________________________________________________________________

39

WHAT dO I need to know??

Unit 10: The Periodic Table

PART I: multiple choice

o Dmitri Mendeleev (how did he organize his table?

o Who was Moseley? How did he organize the PT? o State the modern periodic law o location of groups on the periodic table (i.e. alkali

metals, alkaline earth metals, halogens, noble gases, etc.)

o electron configurations o Definitions (ionization energy, electronegativity,

atomic radius, period, family/group, cation, anion) o Ion size vs. atom size o Periodic trends:

Atomic Radius Electronegativity Ionization Energy Ionic Radius

PART II: True & False

o periodic trends

o most electronegative element

o least electronegative element

o atom vs. ion size

40

part III: cumulative review

o definition of atomic mass

o significant figures

o Avogadro’s number and the mole

o homogeneous vs. heterogeneous

o solution vs. mixture

o most wanted list (ammonia, methane, baking soda, chalk, road salt, etc.)

o combustion reactions (incomplete vs. complete)

o ion formation

o formulas of acids vs. bases

PART Iv: periodic table puzzle

o you will be given a set of clues and your job is to arrange the elements in the proper periodic order