Livingston Public Schools / LPS Homepage



NAME: ANSWER KEYPERIOD: __________CHAPTER 6PERIODIC TABLEHOMEWORK/PRACTICE PACKET4629151200153596640266065632460140335HW#1PERIODIC TABLE VOCABULARYMatch the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line.Column Aa 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 levelc 4. one half the distance between the nuclei of two atoms of the same element when the atoms are joinedk5. decreases for cations and anions from left to right across a periodb 6. measures the ability of an atom to attract electrons when the atom is in a compoundl7. an atom or group of atoms that has a positive or negative chargeg 8. elements in which the highest occupied s and p sublevels are filledo 9. nonmetals of Group 7Ai10. The highest occupied s sublevel and a nearby f sublevel contain electrons.e11. energy required to remove an electron from an atomf12. positively charged ionh 13. Group 1A elementsd 14. good conductors of heat and electric currentp15.negatively charged ionj 16. poor conductors of heat and electric currentColumn Ba. representative elementsb. electronegativityc. atomic radiusd. metalse. ionization energyf. cationg. noble gasesh. alkali metalsi. inner transition metalsj. nonmetalsk. ionic radiusl. ionm. Group 2An. transition metalo. halogensp. anionHW#2CLASSIFYING THE ELEMENTSPart 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.189765432The 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 7.1110The 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. names2.atoms3.alkali metals4.alkali earth metals5.representative elements6. halogens7. noble gases8. transition metals9. inner transition metals10. p11. not filledPart 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 Af16. alkali metalse17. inner transition metalg 18. representative elementd 19. transition metalb 20. noble gasc 21. alkaline earth metalsa 22. halogensColumn Ba. nonmetals of Group 7Ab. an element in which the highest occupied s and p sublevels are filledc. Group 2A elementsd. an element whose highest occupied s sublevel and a nearby d sublevel contain electronse. an element whose highest occupied s sublevel and a nearby f sublevel generally contain electronsf. Group 1A elementsg. an element whose highest occupied s or p sublevels are partially filledHW#3789940107950ANSWERSCFAHBDGEJIHW#4Periodic Table: Fill in the blanks.1. Where are the most active metals located? Group 1, Alkali metals2. Where are the most active nonmetals located? Group 17 Halogens3. 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 metals6. Elements of Group 2A are called alkali earth metals7. Group 7A elements are called halogens8. The most active element in group 7A is fluorine9. Group 8A elements are called noble gases10. Elements in the “B” groups are called transition metals11. 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? d13. Elements within a group have a similar number of valence electrons14. Elements in the same period have the same number of energy levels15. The majority of elements in the periodic table are (metals / nonmetals ).16. Elements in the periodic table are arranged according to their atomic number17. An element with both metallic and nometallic properties is called a metallioid18. 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 cation22. Another word for a negative ion is anion23. The most stable and unreactive elements are the noble gases24. Classify the following properties as metallic (m) or nonmetallic (nm):Luster mmalleable mConducts electricity mfound in all 3 states of matter nmDuctile mconducts heat mFound mostly as solids minsulators mHW#5Periodic TableFor each of the following, circle the correct element.LiSiSmetalKCaSclargest atomic massSClArmember of the halogen familyVNbTalargest atomic numberTeIXemember of noble gasesSiFrBemember of alkali metalsAsSeBr6 valence electronsHLiNanonmetalHgTlPbmember of transition metalsNaMgAlelectron distribution ending s2p1PbBiPometalloidBCNgas at room temperatureCaScTielectron distribution ending in s2d2KSBahas an electron dot like: X:UZnKrmember of inner transition metalsCaSBrforms a +2 ionFNaMgmember of the alkaline earth metalsAlCrP3 valence electronsRbIAlforms a -1 ionHHeOa gas that is not reactiveHW#8096253524256PERIODIC TRENDS1. 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 neonf. krypton (Kr) or neon (Ne)2. Arrange the elements below in order of increasing radius:Cesium (Cs), Potassium, Bromine, SeleniumBr<Se<K<Cs3. Circle the member of each pair that has the greatest ionization energy: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 neonf. krypton (Kr) or neon (Ne)4. Arrange the elements below in order of increasing ionization energy:Cesium (Cs), Potassium, Bromine, SeleniumCs<K<Se<Br5. Select the member of each pair that has a greater electronegativity: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 (noble gas so no electronegativity value)f. krypton (Kr) or neon (Ne)neither (noble gas so no electronegativity value)HW#7SECTION 6.1 ORGANIZING THE ELEMENTS1. Which element listed below should have chemical properties similar tofluorine (F)?a. Lib. Sic. Brd. Ne2. Identify each element as a metal, metalloid, or nonmetal.a. fluorine-NMb. germanium-Metalloidc. zinc-Md. phosphorus-NMe. lithium-M3. Which of the following is not a transition metal?a. magnesiumb. titaniumc. chromiumd. mercuryName two elements that have properties similar to those of the elementpotassium.: Li, Na,Rb, Cs, Fr5. 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 ELEMENTSUse 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.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.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 4s24p5brominec. the Group 6A element in period 4: selenium5. Identify the elements that have electron configurations that end as follows.a. 2s22p4oxygenb. 4s2calciumc. 3d104s2zinc6. 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: 1s22s22p6Ar: 1s22s22p63s23p67. 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 1s22s22p63s23p63d64s2HW#8SECTION 6.3 PERIODIC TRENDSExplain 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, NN< N-3b. Mg2+, Mg Mg2+< Mgc. Li, Li+1, Be+2Be+2< Li+1< Lid. F, F-1, O-2F < F-1< O-2HW#9 PRACTICE MOLE CONVERSIONS:List the diatomic elements: Br2 I2 N2 Cl2 H2 O2 F22. Find the mass of:3.0 moles of oxygen 96.00g 1.15 moles of chlorine 81.54g 0.35 moles of argon13.98g 1.14 x 1026 molecules of bromine30,262.64g 2.55 x 1022 atoms of barium2.91g3. Convert to moles:4.0g of hydrogen1.98 mol 7.68 x 1024 molecules of iodine12.76 mol4. Find the number of molecules in:16.0g of chlorine1.36 x 1023 molecules 2.5 moles of nitrogen1.51 x 1024 molecules***5. How many atoms are in 4.0g of fluorine?1.27 x 1023 atomsColored 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 & ActinidesMetalloids5. 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 Electronegativity7. Identify fluorine as the most reactive non-metal8. Identify francium as being in the spot for the most reactive metal9. 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. ................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download