Chemistry I Unit 2B Pretest Review Ray Tedder NBC Chemistry Teacher

Unit 2A Test Preview 1. On an outline of the periodic table and draw in and label the s, p, d, and f sublevel regions.

Unit 2A Test Preview s sublevel region p sublevel region d sublevel region f sublevel region He

Unit 2A Test Preview 2. On another outline of the periodic table and illustrate the pattern of electronegativity found among the elements on the periodic table.

Unit 2A Test Preview Lower electronegativity Higher electronegativity Noble gases are NOT included

Unit 2A Test Preview 3. Explain what electronegativity is (define it). Electronegativity is a measure of the ability of an atom to attract electrons from another atom when the 2 atoms are bonded together.

Unit 2A Test Preview 4. On another outline of the periodic table illustrate the pattern of first ionization energy found among the elements on the periodic table.

Unit 2A Test Preview Lower 1 st ionization energy Higher 1 st ionization energy

Unit 2A Test Preview 5. Explain what first ionization energy is (define it). First ionization energy is the energy required to remove an electron from an atom.

Unit 2A Test Preview 6. Write the orbital notation for phosphorous (P). 1 IA Periodic Table of the Elements 18 VIIIA 1 H Hydrogen IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA He 2 Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB10 11 IB 12 IIB 13 Al Aluminum Si Silicon P Phosphorous S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenu m Tc Technetium ( ) 44 Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium La Lanthanum Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mecury Tl Thallium Pb Lead Bi Bismuth Polonium ( ) 85 At Astatine ( ) 86 Rn Radon ( ) 87 Fr Francium (223) 88 Ra Radium (226) 89 Ac Actinium (227) 104 Rf Rutherfordium (261) 105 Db Dubnium (262) 106 Sg Seaborgium (266) 107 Bh Bohrium (264) 108 Hs Hassium (277) 109 Mt Meitnerium (268) 110 Ds Darmstadtium (271) 111 Rg Roentgeniu m (272) 112 Uub Ununbium (277) 114 Uuq Ununquadium (289) (287) 116 Uuh Ununhexium (289) 118 (293) P: 1s 2s 2p 3s 3p He 2 Helium

Unit 2A Test Preview 7. Write the complete electron configuration for phosphorous (P). 1 IA Periodic Table of the Elements 18 VIIIA 1 H Hydrogen He Helium IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 He Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB10 11 IB 12 IIB 13 Al Aluminum Si Silicon P Phosphorous S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenu m Tc Technetium ( ) 44 Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium La Lanthanum Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mecury Tl Thallium Pb Lead Bi Bismuth Polonium ( ) 85 At Astatine ( ) 86 Rn Radon ( ) 87 Fr Francium (223) 88 Ra Radium (226) 89 Ac Actinium (227) 104 Rf Rutherfordium (261) 105 Db Dubnium (262) 106 Sg Seaborgium (266) 107 Bh Bohrium (264) 108 Hs Hassium (277) 109 Mt Meitnerium (268) 110 Ds Darmstadtium (271) 111 Rg Roentgeniu m (272) 112 Uub Ununbium (277) 114 Uuq Ununquadium (289) (287) 116 Uuh Ununhexium (289) 118 (293) P: 1s 2 2s 2 2p 6 3s 2 3p 3 P: 1s 2s 2p 3s 3p

1 IA Periodic Table of the Elements 18 VIIIA 1 H Hydrogen He Helium IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 He Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB10 11 IB 12 IIB 13 Al Aluminum Si Silicon P Phosphorous S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenu m Tc Technetium ( ) 44 Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium La Lanthanum Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mecury Tl Thallium Pb Lead Bi Bismuth Polonium ( ) 85 At Astatine ( ) 86 Rn Radon ( ) 87 Fr Francium (223) 88 Ra Radium (226) 89 Ac Actinium (227) 104 Rf Rutherfordium (261) 105 Db Dubnium (262) 106 Sg Seaborgium (266) 107 Bh Bohrium (264) 108 Hs Hassium (277) 109 Mt Meitnerium (268) 110 Ds Darmstadtium (271) 111 Rg Roentgeniu m (272) 112 Uub Ununbium (277) 114 Uuq Ununquadium (289) (287) 116 Uuh Ununhexium (289) 118 (293) Unit 2A Test Preview 8. Write the noble gas shorthand electron configuration for phosphorous (P). P: 1s 2 2s 2 2p 6 3s 2 3p 3 P: 1s 2s 2p 3s 3p P: [Ne] 3s 2 3p 3

1 IA Periodic Table of the Elements 18 VIIIA 1 H Hydrogen He Helium IIIA 14 IVA 15 VA 16 VIA 17 VIIA 2 He Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB10 11 IB 12 IIB 13 Al Aluminum Si Silicon P Phosphorous S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenu m Tc Technetium ( ) 44 Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium La Lanthanum Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mecury Tl Thallium Pb Lead Bi Bismuth Polonium ( ) 85 At Astatine ( ) 86 Rn Radon ( ) 87 Fr Francium (223) 88 Ra Radium (226) 89 Ac Actinium (227) 104 Rf Rutherfordium (261) 105 Db Dubnium (262) 106 Sg Seaborgium (266) 107 Bh Bohrium (264) 108 Hs Hassium (277) 109 Mt Meitnerium (268) 110 Ds Darmstadtium (271) 111 Rg Roentgeniu m (272) 112 Uub Ununbium (277) 114 Uuq Ununquadium (289) (287) 116 Uuh Ununhexium (289) 118 (293) Unit 2A Test Preview 9. Write the electron dot notation for phosphorous (P). P: 1s 2 2s 2 2p 6 3s 2 3p 2 P: 1s 2s 2p 3s 3p P: [Ne] 3s 2 3p 2 P

Unit 2A Test Preview 10. Define nuclear fission. Fission is the splitting of a large nucleus into 2 smaller nuclei. 11. Define nuclear fusion. Fusing is the combining of 2 smaller nuclei into 1 larger nuclei.

Unit 2A Test Preview 12. Describe the structure of an alpha particle. An alpha particle is made up of protons and neutrons. a) Explain what kind of subatomic particles are in an alpha particle. There are 2 protons and 2 neutrons in an alpha particle. b) Explain how many of each of those subatomic particles there are in an alpha particle. The nucleus looses 2 protons and 2 neutrons. So, the atomic mass is reduced by 4 and the atomic number is reduced by 2. c) How does the emission of an alpha particle change the nucleus of an atom?

Unit 2A Test Preview 13. Describe the structure of a beta particle. A beta particle is a high speed electron that comes from a neutron. a) Explain what kind of subatomic particle makes up a beta particle. One. b) How many of those subatomic particles there are in a beta particle? A neutron is turned into a proton. So, the atomic mass is not changed but the atomic number is increased by 1. c) How does the emission of a beta particle change the nucleus of an atom?

Unit 2A Test Preview 14. Describe the structure of a gamma radiation. Gamma radiation is very high energy radiation. a) How does the emission of a gamma radiation change the structure of a nucleus? There is essentially no change in the structure of the nucleus.

Unit 2A Test Preview 15. What kind of nuclear emission is very highly penetrating, is mostly stopped by a thick layer of steel or concrete, but even a few cm of dense lead doesn't stop all of it? Gamma radiation – symbol . 16. What kind of nuclear emission has low penetrating power and is stopped by smoke or a sheet of paper? Beta radiation – symbol . 17. What kind of nuclear emission has moderate penetrating power in which most of it is stopped by a few mm of metal? Alpha radiation – symbol .

Unit 2A Test Preview 18. Complete this nuclear equation.

Unit 2A Test Preview 19. Finish the incomplete nuclear reaction illustration below. n Transition Form

Unit 2A Test Preview 19. Write a complete nuclear equation from the illustration above. n Transition Form

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