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NAME: ANSWER KEY PERIOD: __________

CHAPTER 6PERIODIC TABLE

HOMEWORK/PRACTICE PACKET

Ch 6 Periodic Table HW pkt

HW#1 PERIODIC TABLE VOCABULARY

Match the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line.

Column A

a 1. The highest occupied s and p sublevels are partially filled.

n 2. The highest occupied s sublevel and a nearby d sublevel contain electrons.

m 3. metals having only 2 electrons in the highest occupied energy level

c 4. one half the distance between the nuclei of two atoms of the same element when the atoms are joined

k5. decreases for cations and anions from left to right across a period

b 6. measures the ability of an atom to attract electrons when the atom is in a compound

l7. an atom or group of atoms that has a positive or negative charge

g 8. elements in which the highest occupied s and p sublevels are filled

o 9. nonmetals of Group 7A

i10. The highest occupied s sublevel and a nearby f sublevel contain electrons.

e11. energy required to remove an electron from an atom

f12. positively charged ion

h 13. Group 1A elements

d 14. good conductors of heat and electric current

p15.negatively charged ion

j 16. poor conductors of heat and electric current

Column B

a. representative elements

b. electronegativity

c. atomic radius

d. metals

e. ionization energy

f. cation

g. noble gases

h. alkali metals

i. inner transition metals

j. nonmetals

k. ionic radius

l. ion

m. Group 2A

n. transition metal

o. halogens

p. anion


HW#2 CLASSIFYING THE ELEMENTS

Part A CompletionUse 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.alkali 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-FalseClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

ST12. Group A elements are representative elements.

NT13. Chlorine has the electron configuration 1s22s22p63s23p7.

NT14. The element in Group 4A, period 3, is gallium.

AT15. There is a relationship between the electron configurations of elements and their chemical and physical properties.

Part C MatchingColumn A

f16. alkali metals

e17. 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


1

2 3

4

5

6 78

9

10

11

HW#3

ANSWERS

1. C2. F3. A4. H5. B6. D7. G8. E9. J10.I


HW#4 Periodic Table: Fill in the blanks.

1. Where are the most active metals located? Group 1, Alkali metals

2. Where are the most active nonmetals located? Group 17 Halogens

3. A negative ion is ( larger / smaller ) than its parent atom.

4. A positive ion is ( larger / smaller ) than its parent atom.

5. Elements of Group 1A are called alkali metals

6. Elements of Group 2A are called alkali earth metals

7. Group 7A elements are called halogens

8. The most active element in group 7A is fluorine

9. Group 8A elements are called noble gases

10. Elements in the “B” groups are called transition metals

11. As you go from left to right across the periodic table, the elements go from ( metals /

nonmetals ) to ( metals / nonmetals ).

12. What sublevels are filling across the transition elements? d

13. Elements within a group have a similar number of valence electrons

14. Elements in the same period have the same number of energy levels

15. The majority of elements in the periodic table are (metals / nonmetals ).

16. Elements in the periodic table are arranged according to their atomic number

17. An element with both metallic and nometallic properties is called a metallioid

18. Metals form ( positive / negative ) ions.

19. Nonmetals form ( positive / negative ) ions.

20. An atom or ion is most stable when it has 8valence electrons.

21. Another word for a positive ion is cation

22. Another word for a negative ion is anion

23. The most stable and unreactive elements are the noble gases

24. Classify the following properties as metallic (m) or nonmetallic (nm):

Luster m malleable m

Conducts electricity m found in all 3 states of matter nm

Ductile m conducts heat m

Found mostly as solids m insulators m


HW#5 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 Fr Be 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


HW#6 PERIODIC TRENDS

1. Circle the member of each pair that has the greatest radius:a. nitrogen or arsenic (As) b. calcium (Ca) or zinc (Zn)

c. manganese (Mn) or technetium (Tc) d. iodine (I) or rubidium (Rb)

e. boron (B) or neon f. krypton (Kr) or neon (Ne)

2. Arrange the elements below in order of increasing radius:Cesium (Cs), Potassium, Bromine, SeleniumBr<Se<K<Cs

3. Circle the member of each pair that has the greatest ionization energy:a. nitrogen or arsenic (As) b. calcium (Ca) or zinc (Zn)


e. boron (B) or neon f. krypton (Kr) or neon (Ne)

4. Arrange the elements below in order of increasing ionization energy:Cesium (Cs), Potassium, Bromine, SeleniumCs<K<Se<Br

5. Select the member of each pair that has a greater electronegativity:a. nitrogen or arsenic (As) b. calcium (Ca) or zinc (Zn)


e. boron (B) or neon (noble gas so no electronegativity value)

f. krypton (Kr) or neon (Ne)neither (noble gas so no electronegativity value)


HW#7 SECTION 6.1 ORGANIZING THE ELEMENTS1. Which element listed below should have chemical properties similar tofluorine (F)?

a. Li b. Sic. Br d. Ne

2. Identify each element as a metal, metalloid, or nonmetal.a. fluorine-NM b. germanium-Metalloid c. zinc-Md. phosphorus-NM e. lithium-M

3. Which of the following is not a transition metal?a. magnesium b. titanium c. chromium d. mercury

1. Name two elements that have properties similar to those of the elementpotassium.: Li, Na,Rb, Cs, Fr

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?

The metals: good conductors of heat and electric current; high luster when clean; malleable; ductile.The nonmetals: poor conductors of heat and electric current; nonlustrous. The metalloids: elements that have properties similar to those of metals and nonmetals depending on the conditions.

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

Silicon is in the third period. Its first and second energy levels are full (1s22s22p6). It is the fourth element in the period; so its electron configuration must end in 3s23p2. The complete configuration is 1s22s22p63s23p2.

2. Use the periodic table to write the electron configuration for iodine. Explain your thinking.Iodine is located in period 5. Its first four energy levels are full. It is Group 4A; so its electron configuration must end in 5s25p5. The complete configuration is 1s22s22p63s23p63d104s24p64d105s25p5.

3. Which group of elements is characterized by an s2p3 configuration?The configuration s2p3 indicates 5 electrons in the highest occupied energy level, which is a feature of Group 5A.

4. Name the element that matches the following description.

a. one that has 5 electrons in the third energy level: phosphorusb. one with an electron configuration that ends in 4s24p5 brominec. the Group 6A element in period 4: selenium

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

a. 2s22p4 oxygenb. 4s2 calciumc. 3d104s2 zinc

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

Both Ne and Ar have a completely filled highest occupied energy level. They are in Group 8A or 18, which is also known as the noble gases. Ne: 1s22s22p6 Ar: 1s22s22p63s23p6

7. Why would you expect lithium (Li) and sulfur (S) to have different chemical and physical properties?The chemical and physical properties are largely determined by their electron configurations. Lithium in Group 1A has only 1 electron in its highest occupied energy level. Sulfur in Group 6A has 6 electrons in its highest occupied energy level.

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


Transition metals are elements whose highest occupied s sublevel and a nearby d sublevel contain electrons. The electron configurations for Ag and Fe are: Ag 1s22s22p63s23p64s24p64d105s1 Fe 1s22s22p63s23p63d64s2

HW#8 SECTION 6.3 PERIODIC TRENDS

1. Explain why a magnesium atom is smaller than atoms of both sodium and calcium.A magnesium atom is smaller than a sodium atom because the shielding effect is constant for elements in the same period, but the nuclear charge is greater in magnesium. So the electrons are drawn closer to the nucleus.Magnesium and calcium have the same number of electrons in their highest occupied energy level. A magnesium atom is smaller than a calcium atom because there are fewer occupied energy levels.

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

Astatine is in period 6. Tellurium is in period 5. Astatine is in Group 7A; tellurium is in Group 6A. Although atomic size decreases across a period, the additional occupied energy level in astatine significantly increases the size ofthe astatine atom as compared to the tellurium atom. The prediction is that atoms of astatine are larger than atoms of tellurium.

3. Would you expect a Cl– ion to be larger or smaller than an Mg2+ ion? Explain.A chlorine atom is smaller than a magnesium atom because atomic size decreases from left to right across a period. When a magnesium atom reacts, it loses electrons from its highest occupied energy level. A magnesium ion hasfilled first and second levels. When chlorine reacts, it gains an electron in its highest occupied energy level. An ion with three occupied energy levels is larger than an ion with two occupied energy levels.

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

Across a period from left to right the principal energy level remains the same, but the nuclear charge increases. The increasing nuclear charge pulls the electrons closer to the nucleus, resulting in a smaller atomic radius. The trend is less pronounced as the number of electrons increases because the inner electrons shield the electrons in the highest occupied energy level. Atomic size increases as you move down a period because the electrons are added to higher principal energy levels. This enlarging effect is greater than the shrinking effect caused by increasing nuclear charge.

5. Explain why the sulfide ion (S2–) is larger than the chloride ion (Cl–).When a sulfur atom reacts to form an ion it adds two electrons while chlorine adds one electron. Sulfide and chloride ions have the same number of electrons. Because the chloride ion has the greater nuclear charge, it will be smaller than the sulfide ion.6. Compare the first ionization energy of sodium to that of potassium.Sodium’s first ionization energy is higher than that of potassium because ionization energy tends to decrease from top to bottom within a group.

7. Compare the first ionization energy lithium to that of beryllium. Beryllium’s first ionization energy is greater because first ionization energy tends to increase from left to right across a period.8. Is the electronegativity of barium larger or smaller than that of strontium? Explain.

Barium is less electronegative than strontium because electronegativity values tend to decrease from top to bottom within a group.

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


Because magnesium has a relatively low first and second ionization energy, the removal of two electrons from magnesium is likely. The relatively high third ionization energy indicates the difficulty of removing a third electron from the filled second energy level. Magnesium normally forms an ion with a 2_charge.

10. Arrange oxygen, fluorine, and sulfur in order of increasing electro negativity.Because electronegativity decreases from top to bottom within a group, sulfur is less electronegative than oxygen. Because electronegativity increases from left to right across a period, fluorine is more electronegative than oxygen. The correct order for increasing electronegativity is then sulfur <oxygen <fluorine.

Arrange the following from smallest to largest in size (atomic and ionic radius).

a. N-3, N N< N-3

b. Mg2+, Mg Mg2+< Mgc. Li, Li+1, Be+2Be+2< Li+1< Lid. F, F-1, O-2 F < F-1< O-2


HW#9 PRACTICE MOLE CONVERSIONS:

1. List the diatomic elements: Br2 I2 N2 Cl2 H2 O2 F2

2. Find the mass of:a. 3.0 moles of oxygen 96.00g

b. 1.15 moles of chlorine 81.54g

c. 0.35 moles of argon 13.98g

d. 1.14 x 1026 molecules of bromine 30,262.64g

e. 2.55 x 1022 atoms of barium 2.91g

3. Convert to moles:a. 4.0g of hydrogen 1.98 mol

b. 7.68 x 1024 molecules of iodine 12.76 mol

4. Find the number of molecules in:a. 16.0g of chlorine 1.36 x 1023 molecules

b. 2.5 moles of nitrogen 1.51 x 1024 molecules

***5. How many atoms are in 4.0g of fluorine? 1.27 x 1023 atoms


Colored PeriodicTable Instructions:

1. Number each group from left to right (1-18).

2. Number each period from top to bottom (1-7) .

3. Draw in the stepladder separating metals and nonmetals. Label metals vs. nonmetals on the table. Describe the properties of each group.

4. Create a color coded key for each of the following families or series of elements, or include the information within the colored block: Include a description of the properties of each group or block of elements.

Alkali Metal Family (***don’t include hydrogen) +1Alkaline Earth Metal Family +2Halogens -1Nobel GasesTransition MetalsInner Transition Metals-Lanthanides & ActinidesMetalloids

5. Write the ionic charge of the family (shown above) at the top of the column.

6. Indicate the trends down and across for each of the following properties using arrows: Atomic Radii Ionization Energy Electronegativity

7. Identify fluorine as the most reactive non-metal

8. Identify francium as being in the spot for the most reactive metal

9. Make the symbols of Br, I, N, Cl, H, O, F bolded. (they are elements: H2, N2, O2, F2, Cl2, Br2, I2)

10. Write the charges of Al3+, Zn2+, Ag+1next to their symbol.


web viewgroup a elements are representative elements. nt. ... the most stable and unreactive...

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