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Ions and the Octet Rule 1) Ca 2) Ca+2 3) S-2 4) S 5) I 6) I-1 7) Se-2 8) Se 9) Al+3 10) Al 11*) Xe 12*) Si ------------------------------------------------------------------------------------------------------------------------------------------------------------------ 13) B 14) B? 15) P? 16) P 17) ? ) ) 3) 18) ?? ) ) ) 19) ?? ) ) ) 20) ? ) ) ) 21) ? ) 1) 22) ?? ) ) 23) ?-? ) ) ) 24) ?+? ) ) ) 25) ? ) ) ) 26) ?-? ) ) ) 27) ?+3 ) ) ) 28) ? ) ) ) ) ) 4) 5) ) ) 29) Identify the following elements based on their electron configuration or orbital notation and their overall charge. a) 1s2 2s2 2p3 (neutral) _____ b) 1s2 2s2 2p6 3s2 3p6 (+2) _____ c) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 30) 31) (-3) _____ d) O | O OOO | O OOO OOOOO | O OOO OOOOO OOOOOOO | O (neutral) 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s _____ e) O | O OOO | O OOO OOOOO | O OOO OOOOO OOOOOOO | O OOO 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p _____ (+1) Write the electron configuration for each of the following ions and tell which noble gas each is isoelectronic with. a) Al+3 _____ b) Te-2 _____ c) Sr+2 _____ d) Ga+3 _____ e) I-1 _____ Write the electron configuration for each of the following ions. a) F-1 b) Na+1 c) Be+2 d) P-3 e) K+1 f) S-2 g) Ba+2 32) Write the electron configuration for each of the following ions. Tell which noble gas each ion is isoelectronic with. a) Se-2 _____ b) O-2 _____ c) Sb-3 _____ d) Mg+2 _____ e) Pb+4 _____ 33) Write the electron configuration for O and O-2. How many electrons are in each valence energy level? 34) Identify the following elements given their electron configuration and their charge. a) 1s2 2s2 2p6 (-2) _____ b) 1s2 2s2 2p6 (+3) _____ c) 1s2 2s2 2p6 3s2 3p6 (-1) _____ d) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 (+2) e) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 6s2 6p6 _____ (+1) _____ 35) Write the electron configuration for Br and its ion. How many electrons are in each of the valence energy levels? 36) Write the electron configuration for Ca and its ion. How many electrons are in each of the valence energy levels? 37) Write the electron configuration for Cl and its ion. How many electrons are in each of the valence energy levels? 38) Write the electron configuration for Na and its ion. How many electrons are in each of the valence energy levels? 39) Write the electron configuration for Sb and its ion. How many electrons are in each of the valence energy levels? 40) Identify the following elements given their electron configuration and their charge. a) 1s2 2s2 2p6 (-4) _____ b) 1s2 2s2 2p6 (+1) _____ c) 1s2 2s2 2p6 3s2 3p6 (-3) _____ d) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 (neutral) _____ e) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 6s2 6p6 41) (-1) _____ Identify the following elements based on their electron configuration or orbital notation and their overall charge: a) 1s2 2s2 2p6 3s2 3p5 (neutral) _____ b) 1s2 2s2 2p6 3s2 3p6 (-3) _____ c) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 d) O | O OOO 1s 2s 2p (+1) _____ (+3) _____ e) O | O OOO | O OOO OOOOO | O OOO OOOOO OOOOOOO | O 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 42) _____ Select the member of each pair that is larger. a) Ca or P 43) (neutral) b) Cl or Cl- Arrange in order of increasing radius: c) Na or Na+ Ca+2, Cl-, K+, S-2 d) I- or Te _____ : _____ : _____ : _____ Periodic Trends 44) On the Periodic Table, a horizontal row is called a __________ and a vertical column is called a __________. 45) Which would behave more similarly: elements in any one group or elements in any one period. __________________________________________________________________________________________ 46) What similarity is there among the outermost energy levels of elements within the same group? __________________________________________________________________________________________ 47) Arrange in order of increasing ionization potential: Ca, Cl, Rb, S, Sr ___ : ___ : ___ : ___ : ___ 48) Arrange in order of increasing atomic radius: As, I, P, Sb ___ : ___ : ___ : ___ 49) AR _____ as you move from the top to the bottom of a group on the PTE. 50) Explain why atomic radius changes as it does as we move from left to right in the Periodic Table. decreases increases __________________________________________________________________________________________ 51) Arrange in order of increasing atomic radius: F, H, In, S, Hg ___ : ___ : ___ : ___ : ___ 52) Where on the PTE do we find elements with the lowest ionization potential? _________________________ 53) Where on the PTE do we find the most un-reactive elements? _________________________ 54) _________________________ is the amount of energy needed to pull an electron away from an isolated atom. 55) Elements sodium and chlorine are both in period 3. Why is the ionization potential of chlorine so much greater? __________________________________________________________________________________________ 56) Arrange in order of increasing ionization potential: As, I, P, Sb ___ : ___ : ___ : ___ 57) Why it is more difficult to remove an electron from an atom that is located at the top of a group than the bottom. __________________________________________________________________________________________ 58) Arrange in order of increasing atomic radius: Ca, Cl, Rb, S, Sr ___ : ___ : ___ : ___ : ___ 59) Arrange in order of increasing ionization potential: Br, Cs, F, Ge, Se ___ : ___ : ___ : ___ : ___ 60) A positive ion is an atom that has _____. a) gained an electron 61) b) gained a proton c) lost an electron d) lost a proton b) gained 2 protons c) lost 2 electrons d) lost 2 protons Metallic elements tend to _____ electrons and form _____ ions. a) gain 64) d) lost a proton A Mg+2 ion is a Mg atom that has _____. a) gained 2 electrons 63) c) lost an electron A Cl- ion is a Cl atom that has _____. a) gained an electron 62) b) gained a proton b) lose c) positive Based on their actual electronegativity the following are arranged as follows: Based on the electronegativity trend the following are arranged as follows: Why the difference? d) negative Zn : Fe : Cu : Se Fe : Cu : Zn : Se __________________________________________________________________________________________ 65) Why should fluorine have the highest electronegativity? __________________________________________________________________________________________ 66) The ionization potential _____ as one moves down a group of elements. decreases increases 67) The ionization potential _____ as one moves from left to right across a period. decreases increases 68) The atomic radius _____ as one moves from left to right across a period. decreases increases 69) Arrange in order of increasing electronegativity: ___ : ___ : ___ : ___ : ___ 70) Within the same period, cations are larger than anions. True 71) Arrange in order of increasing atomic radius: ___ : ___ : ___ : ___ : ___ : ___ 72) Which of the transition metals should have the smallest ionization energy? _____ 73) Which of the noble gases should be the most likely to react with another atom? _____ 74) Which of the noble gases should be the least likely to react with another atom? _____ 75) Which family should have the highest electronegativity? a) alkali metals 76) F, O, S, P, Na K, Ca, Se, Br, Ba, I b) alkaline earth metals c) halogens False d) noble gases Explain above answer: _______________________________________________________________________________ Other Periodic Trends 77) Explain the size difference between a sodium ion and chlorine ion. 78) Explain the size difference between a fluorine atom, neon atom and a sodium ion. 79) Explain the size difference between an atom and its ion. 80) Explain the size difference between a series of isoelectronic atoms / ions. 81) Research the pattern for density. 82) Research the pattern for melting and boiling point.