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Worksheets - Answers Grade 11 IBUnit 2 Atomic StructureNo Worksheet – Mass SpectrometerRead Pgs 42 – 47, Pg 65 Q# 1 – 5Worksheet 1 – Aufbau DiagramsRead Pgs 38 – 41Read Pgs 50 – 61 Pg 65 Q# 6 – 16Worksheet 2 – Blank Periodic TableWorksheet 3 – Energy Level Diagrams Worksheet 4 – Electron ConfigurationsWorksheet 5 – Orbital and Energy Level DiagramsWorksheet 6 – Quantum NumbersRead Pgs 291 – 299, Pg 300 Q# 1 - 4Worksheet 7 – Atomic Structure Review Unit 3 PeriodicityWorksheet 8 – Periodic TrendsRead Pgs 70 – 74, Pgs 75 – 90Pg 91 Q#1 – 13Worksheet 9 – Alkali Metals and HalogensWorksheet 10 - PolarityNo Worksheet – d -sublevelRead Pgs 301 – 313, 316 – 326Pg 327 Q#1 – 13 Worksheet 4 – Electron Configurations of AtomsWrite the full and shorthand (condensed) electron configurations for each of the following atoms.phosphorus1s22s22p63s23p3[Ne]3s23p3beryllium1s22s2[He]2s2fluorine1s22s22p5[He]2s22p5calcium1s22s22p63s23p64s2[Ar]4s2zinc1s22s22p63s23p64s23d10[Ar]4s23d10tellurium, 1s22s22p63s23p64s23d104p65s24d105p4[Kr] 5s24d105p4sodium1s22s22p63s1[Ne]3s1nickel1s22s22p63s23p64s23d8[Ar]4s23d8oxygen1s22s22p4[He]2s22p4iron1s22s22p63s23p64s23d6[Ar]4s23d6magnesium1s22s22p63s2[Ne]3s2aluminum1s22s22p63s23p1[Ne]3s23p1Write shorthand (condensed) electron configuration for each of the following atoms.holmium[Xe]6s24f11osmium[Xe]6s24f145d6lead[Xe]6s24f145d106p2radium[Rn]7s2bohrium[Rn]7s25f146d5Determine which elements have the following electron configurations:a) 1s22s22p63s23p4 Sb) 1s22s22p63s23p64s23d104p65s1 Rbc) [Kr] 5s24d105p3 Sb d) [Xe] 6s24f145d6 Ose) [Rn] 7s25f11 EsDetermine which electron configurations are not valid.a) 1s22s22p63s23p64s24d104p5 nob) 1s22s22p63s33d5 noc) [Ra] 7s25f8 nod) [Kr] 5s24d105p5 yese) [Xe] no – better to put [Kr]5s24d105p6 Which block of the periodic table are each of the following elements located in?a) einsteiniumfb) poloniumpc) rutherfordiumdd) franciumsWithout looking at the periodic table, identify the group number, period number, and block of an atom that has each of the following electron configurations.a) [Ne]3s1group 1, period 3, s blockb) [He]2s2group 2, period 2, s blockc) [Kr]5s24d105p5group 17, period 5, p blockWhat is the number of orbitals in each of the following subshells?a) 2s 1b) 4p3c) 3d5d) 1p 0e) 4f7f) 2p3g) 2d5h) 6g9What is the maximum number of electrons in each of the following subshells?a) 2s2b) 4p6c) 3d10d) 1p0e) 4f14f) 2p6g) 2d10h) 6g18Worksheet 5 – Orbital and Energy Level DiagramsIdentify and correct the errors in each of the following valence shell orbital diagrams: Element s orbital p orbitalsa) carbonCorrect:b) sulfurCorrect:c) aluminumCorrect:Consider the valence level electron configurations of the following five elements:Elements orbitalp orbitals12345a) Which of the above elements are metals? 2, 3, 4 could be metalsb) Which of the above elements would form an ion with a +2 charge? 3, possibly 4c) Which of the above elements is a noble gas? 1, possibly 3 a halogen? 5d) Which of the above elements has the same configuration as S2- ? 1Write the orbital occupied by the last electron of each of the following elements:AsWLiUORnV4p5d2s5f2p6p3dDraw an orbital diagram for each of the following. a) a cobalt atom (Co)1s2s2p3s3p4s3db) a sulfide ion S2–1s2s2p3s3p4sc) a cadmium ion (Cd2+) 1s2s2p3s3p4s3d4p5s4dDraw a complete energy level diagram (vertical) for an atom of iron, Fe.Worksheet 6 – Quantum NumbersState the four quantum numbers and the possible values they may have.n = 1,2,3,4,5,6,7,8 , l = 0,1,2,3 , ml = -l...+l , ms = +? , -?2. Name the orbitals described by the following quantum numbers??? a. n = 3, L = 0 , 3s??? b. n = 3, L = 1, 3p??? c. n = 3, L = 2, 3d??? d. n = 5, L = 0, 5s3. Give the n and L values for the following orbitals??? a. 1s, n = 1 l = 0 ??? b. 3s, n = 3 l = 0??? c. 2p, n = 2 l = 1??? d. 4d, n = 4 l = 2??? e. 5f, n = 5 l = 34. Place the following orbitals in order of increasing energy:??? 1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p , 1s, 3s, 3p, 4s, 3d, 5p, 6s, 5d, 7s5. What are the possible mL values for the following types of orbitals???? a. s, 0??? b. p, -1, 0, +1??? c. d, -2, -1, 0, +1, +2??? d. f, -3, -2, -1, 0, +1, +2, +36. How many possible orbitals are there for n =??? a. 4, 16??? b. 10, 1007. How many electrons can inhabit all of the n=4 orbitals?328. Tabulate all of the possible orbitals (by name, i.e. 4s) for n=4 and give the three quantum numbers which define each orbital.4s n = 4, l = 0, ml = 0 4p n = 4, l = 1, ml = -1, 0, +1 4d n = 4, l = 2, ml = -2, -1, 0, +1, +2 4f n = 4, l = 3, ml = -3, -2, -1, 0, +1, +2, +39. Write electron configurations for the following atoms:??? a. H 1s1d. F1s22s22p5??? b. Li1s22s1e. Br1s22s22p63s23p64s23d104p5??? c. N1s22s22p3??? Worksheet 7 - Atomic Structure Test Review1) Which one of the following statements regarding Rutherford’s gold foil experiment is TRUE?Rutherford predicted that most of the alpha particles would pass straight through the foil because atoms are mainly empty space.Rutherford predicted that the alpha particles that hit negative particles would bounce back towards the radioactive source.The actual experimental results led Rutherford to conclude that atoms have a central positive core because most of the alpha particles were deflected at large angles.Since most of the alpha particles passed straight through the foil without deflection, Rutherford concluded that atoms are mainly empty space.The most surprising thing about the experimental results was that only some of the alpha particles were deflected at large angles.2) In Thomson’s model of the atom:negative particles are embedded within a sphere of positive chargeatoms are tiny, indivisible spherespositive particles are embedded within a sphere of negative chargethere is a positive nucleus surrounded by empty space3518535323215X020000X34804352908303) Which one of the following could be the electron configuration for an element with the following Lewis diagram?a) 1s22s1b) 1s22s22p3c) 1s22s22p1d) [Ar]4s23d3e) more than one are correct4330700269875004) The species with the following energy level diagram is:a) Neb) Nac) Na+d) Ke) Cl– 5) In the emission spectrum of hydrogen, which electronic transition would produce a line in the visible region of the electromagnetic spectrum?a) n = 2 n = 1b) n = 3 n = 2c) n = 2 n = 3d) n = n = 16) How many unpaired electrons are in the ground state energy level diagram for an atom of sulfur?a) 1b) 2c) 3d) 4e) 57) Which of the following particles has the same electron configuration as krypton?a) Ga3+b) Ga3–c) Sn4+d) Sn2+e) As3–8) Complete the following table:Name of ElementSymbol of Atom or IonAtomic NumberMass NumberNumber of ProtonsNumber of NeutronsNumber of ElectronsOverall ChargeaberylliumBr494540bfluorineF-919910101-cironFe3+26562630233+dseleniumSe2-34793445362- 9) Write the full electron configuration for each of the following atoms:a) strontium1s22s22p63s23p64s23d104p65s2b) germanium1s22s22p63s23p64s23d104p210) Write the shorthand electron configuration for each of the following atoms:a) silicon[Ne]3s23p2b) molybdenum[Kr]5s24d4c) terbium[Xe]6s24f9d) gold[Xe]6s24f145d9e) seaborgium[Rn]7s25f146d411) Draw orbital diagrams for each of the following ions (shorthand), indicate which electrons have been gained/lost:a) Cu+ 4s↑ 3d↑↓↑↓↑↓↑↓↑↓b) Pb2+ 6s↑↓ 5d↑↓↑↓↑↓↑↓↑↓ 6p↑↑c) Br– 4s↑↓ 3d↑↓↑↓↑↓↑↓↑↓ 4p↑↓↑↓↑↓d) Sb3– 5s↑↓ 4d↑↓↑↓↑↓↑↓↑↓ 5p↑↓↑↓↑↓e) Ba2+ 6s↑↓f) Sn4+ 5s↑↓ 4d↑↓↑↓↑↓↑↓↑↓ 5p↑↑12) What is the maximum number of electrons in:a) n = 3 , 18b) 3d , 10c) 6p , 6d) 4f, 14e) 2s , 2f) n = 5 , 50g) all d orbitals of curium, Cm , 3013) State the four quantum numbers for each of the following:a) the 31st electron of Ga , 4, 1, -1, +?b) the 12th electron of magnesium, 3, 0, 0, -?c) the 80th electron of mercury, 4, 2, +2, -?d) the 54th electron of xenon, 5, 1, +1, -?e) the 68th electron of holmium, 4, 3, 0, +?Worksheet 8 - Periodic Trends1) Which of the following elements has the largest atomic radius?a) berylliumb) carbonc) nitrogen d) oxygen2) Which of the following elements has the smallest atomic radius?a) sulfurb) seleniumc) oxygend) tellurium3) Which of the following elements has the smallest first ionization energy?a) strontiumb) calciumc) bariumd) magnesium4) Which of the following elements has the largest first ionization energy?a) bromine b) potassiumc) arsenicd) calcium5) Which of the following elements has the highest electron affinity?a) chlorineb) siliconc) sodiumd) phosphorus6) Which element in the following sets should have the largest atomic radius, and why?a) boron, lithium, or fluorineb) potassium, lithium, or sodium7) Which element in the following pairs has the higher first ionization energy?a) cesium or goldb) sulfur or phosphorusc) magnesium or aluminumd) neon or kryptone) oxygen or seleniumf) barium or calcium8) Which element in the following sets loses an electron most readily, and why?a) boron, lithium, or fluorineb) potassium, lithium, or sodium9) List each of the following sets in order of increasing radius:a) Ne, Na+, O2–b) Mg2+, Na+, Al3+c) N3–, O2–, F1–10) The ion Na+ and the atom Ne have the same electron configuration. To remove an electron from gaseous neon atoms requires 2081 kJ/mol. To remove an electron from a gaseous Na+ ion requires 4562 kJ/mol. Why are these values not the same?11) The second ionization energy of magnesium is only about twice as great as the first ionization energy. However, the third ionization energy is about ten times as great as the first. Why does it take so much more energy to remove the third electron from magnesium?12) The following graph shows the melting points (and boiling points) of the period 3 elements.a) Why is there a general increase in melting point for Na, Mg, and Al?b) Why does Si have the highest melting point?c) Why is there a general decrease in melting point for P4, S8, and Cl2?d) Why do the noble gases have the lowest melting point?13) Although the first ionization energy of K is smaller than that of Ca, the second ionization energy of K is much higher than that of Ca. Why is this so?14) ElementI1I 2I 3I 1 = 1st ionization energy (kJ/mol) AA 53110876270I 2 = 2nd ionization energy (kJ/mol) BB209031354180I 3 = 3rd ionization energy (kJ/mol) CC523836011704Which of the above elements would most likely be an alkali metal?Which of the above elements would most likely be a noble gas?Worksheet 9 - Alkali Metals and HalogensState whether each of the following properties increase or decrease going down the alkali metal group.a) atomic radiusb) ionic radiusc) ionization energyd) electronegativitye) reactivityState whether each of the following properties increase or decrease going down the halogen group.a) atomic radiusb) ionic radiusc) ionization energyd) electronegativitye) reactivityWhat is the state of matter at room temperature for each of the following?a) F2b) Cl2c) Br2d) I2For each of the following, circle the correct element. Li Si S metal N P As smallest ionization energy K Ca Sc largest atomic mass S Cl Ar member of the halogen family Al Si P greatest electron affinity Ga Al Si largest atomic radius V Nb Ta largest atomic number Te I Xe member of noble gases Si Ge Sn 4 energy levels Li Be 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 in s2 p1 Pb Bi Po metalloid B C N gas at room temperature Ca Sc Ti electron distribution ending in s2 d2Worksheet 10 – PolarityIn each of the following problems, rank the molecules from lowest to highest polarity:1)PF3, LiOH, SF2, NF32)Ni(OH)3, N2H2, CH3OH, C2H5OH3)NO2, SeCl2, PbCl2, SO 4)PH3, PF3, NH3, NF35)H2O, H2S, HF, H2 ................
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