Homework Answers
Fully filled and half filled configurations are exceptionally more stable and higher ionization energies will be required to remove an electron from a half filled or fully filled configurations.
Configuration of Oxygen = 1s2 , 2s2 , 2p4
Configuration of nitrogen = 1s2 , 2s2 , 2p3
Nitrogen has half filled configuration which is more stable, hence more energy will be required to remove an electron from extra stable half filled configuration.
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(2 pts) Why is the first ionization energy of oxygen smaller than the first ionization energy...
8-7 Why is the first ionization energy for phosphorous higher than the first ionization energy for...
8-7 Why is the first ionization energy for phosphorous higher than the first ionization energy for sulfur even though the general trend in the periodic table is to have the ionization energy increase as you go from left to right on the table. 8-8 The three most common oxidation states for Fe are +2, +3 and +6 what are the most likely electronic configurations for these three ions? 8-9 Why do transition metals have magnetic properties? 8-10 Just looking at...
3. Explain each of the following observations. (a) Sodium has a lower first-ionization energy than lithium....
3. Explain each of the following observations. (a) Sodium has a lower first-ionization energy than lithium. (b) Oxygen has a lower first-ionization energy than nitrogen.
Would you expect hydrogen gas (H2) to have a smaller or larger first ionization energy than...
Would you expect hydrogen gas (H2) to have a smaller or larger first ionization energy than atomic hydrogen? Explain.
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers...
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
40. (4 pts) Use the bond energies provide bond energies provided to estimate for the reaction...
40. (4 pts) Use the bond energies provide bond energies provided to estimate for the reaction below. 2 Brz() + CH3(g) → CH.Br.) AH...? Br-Br C.C CC C-Br CH Bond Energy (kJ/mol 193 837 347 276 414 41. (3 pts) Which would have a more exothermic lattice energy, and why? MgO or MgCl2 42 (2 pts) Why is the first ionization energy of oxygen smaller than the first ionization energy of nitrogen? 43. (2 pts) Give the ground state electron...
What is the general trend in ionization energy across a row on the periodic table? Using...
What is the general trend in ionization energy across a row on the periodic table? Using a ground state electron configuration as your basis of comparison, explain Why the ionization energy of boron is less than that of beryllium Why the ionization energy of oxygen is less than that of nitrogen
4. (5 points) Why is the first ionization energy for cesium lower than xenon? Explain your...
4. (5 points) Why is the first ionization energy for cesium lower than xenon? Explain your reasoning. 25 He first ionization energy (eV) Rn Rb Cs 0 10 20 30 40 50 60 70 80 90 atomic number
7) Decide whether the statement concerning ionization energy is true or false. If the statement is...
7) Decide whether the statement concerning ionization energy is true or false. If the statement is false, correct the statement (4 points). True or False Correction if false Statement An oxygen (0) atom has larger first ionization energy than a fluorine (F) atom. A cesium (Cs) atom has smaller first ionization energy than lithium (Li) atom.
Which would have a low first ionization energy and a high second ionization energy? Potassium Calcium...
Which would have a low first ionization energy and a high second ionization energy? Potassium Calcium Neon 2. which is an oxidizer carbon flourine nitrogen
Rb : [kr] Rb++[Ar]4323d104p) b Why is the second ionization energy much greater than the first?...
Rb : [kr] Rb++[Ar]4323d104p) b Why is the second ionization energy much greater than the first? Second ionization energy is always 4 times greater than the first. After removal of the second electron, rubidium has a configuration of noble gas. The second electron is removed from 4p, which is much closer to the nucleus than 58, Rb has a configuration of noble gas, which is stable. Submit What experiments could be done to provide some evidence that the correct formulation...
8-7 Why is the first ionization energy for phosphorous higher than the first ionization energy for sulfur even though the general trend in the periodic table is to have the ionization energy increase as you go from left to right on the table. 8-8 The three most common oxidation states for Fe are +2, +3 and +6 what are the most likely electronic configurations for these three ions? 8-9 Why do transition metals have magnetic properties? 8-10 Just looking at...
3. Explain each of the following observations. (a) Sodium has a lower first-ionization energy than lithium. (b) Oxygen has a lower first-ionization energy than nitrogen.
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
40. (4 pts) Use the bond energies provide bond energies provided to estimate for the reaction below. 2 Brz() + CH3(g) → CH.Br.) AH...? Br-Br C.C CC C-Br CH Bond Energy (kJ/mol 193 837 347 276 414 41. (3 pts) Which would have a more exothermic lattice energy, and why? MgO or MgCl2 42 (2 pts) Why is the first ionization energy of oxygen smaller than the first ionization energy of nitrogen? 43. (2 pts) Give the ground state electron...
What is the general trend in ionization energy across a row on the periodic table? Using a ground state electron configuration as your basis of comparison, explain Why the ionization energy of boron is less than that of beryllium Why the ionization energy of oxygen is less than that of nitrogen
4. (5 points) Why is the first ionization energy for cesium lower than xenon? Explain your reasoning. 25 He first ionization energy (eV) Rn Rb Cs 0 10 20 30 40 50 60 70 80 90 atomic number
7) Decide whether the statement concerning ionization energy is true or false. If the statement is false, correct the statement (4 points). True or False Correction if false Statement An oxygen (0) atom has larger first ionization energy than a fluorine (F) atom. A cesium (Cs) atom has smaller first ionization energy than lithium (Li) atom.
Rb : [kr] Rb++[Ar]4323d104p) b Why is the second ionization energy much greater than the first? Second ionization energy is always 4 times greater than the first. After removal of the second electron, rubidium has a configuration of noble gas. The second electron is removed from 4p, which is much closer to the nucleus than 58, Rb has a configuration of noble gas, which is stable. Submit What experiments could be done to provide some evidence that the correct formulation...
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