Homework Answers
Because xenon is a noble gas , it has stable electronic configuration 5s2 5p6, so to disturb this stability, high energy is to be given to remove an electron,
Whereas in cesium, its has electronic configuration [Xe]6s1,
So, here electron can be easily removed with leass energy.
Therefore, first ionisation energy of cesium is lower than xenon.
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4. (5 points) Why is the first ionization energy for cesium lower than xenon? Explain your...
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.
45.5kJ/mol-1 Cesium has the lowest ionization energy of all the elements. 3-1 a) Explain why. (Don't...
45.5kJ/mol-1
Cesium has the lowest ionization energy of all the elements. 3-1 a) Explain why. (Don't just cite the periodic trends. Make sure you give a chemical explanation for this property.) b) What is the wavelength of a photon that could ionize a Cs atom? What region of the electromagnetic spectrum does this light belong to?
answer a b or c Why is the atomic radius of magnesium ion much smaller than...
answer a b or c
Why is the atomic radius of magnesium ion much smaller than that of a neutral charged magnesium atom? (See the atomic radius graph) The magnesium ion's electrons require less space. No electrons are lost, they move to unoccupied spaces about the nucleus. The magnesium ion has fewer principle quantum energy levels, this causes a decrease in atomic radius. The magnesium ion has a higher Z-effective nuclear charge. The magnesium ion has more principle quantum 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...
Why does boron have a lower ionization energy than beryllium? (explain in space provided below)
Why does boron have a lower ionization energy than beryllium? (explain in space provided below)
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...
Element Na First Ionization Energy (J/mol) 4.95 x 105 4.19 x 105 K 6. The first...
Element Na First Ionization Energy (J/mol) 4.95 x 105 4.19 x 105 K 6. The first ionization energies for Na and K are given in the table above. a. Write the complete electron configuration for Na. b. Based on principles of atomic structure, explain why the first ionization energy of K is lower than the first ionization energy of Na. c. Which ionic solid would have the greatest melting point, NaCl or KCI? Justify your answer in terms of lattice...
Please match the compound to its spectrum and explain why cpd 22 Spectrum A 100- 60...
Please match the compound to its spectrum and explain
why
cpd 22 Spectrum A 100- 60 40 20 100 125 50 75 m/z Spectrum B 100 80- 60 40 20- 10 20 30 40 50 60 70 0 90 100 110 120 m/z (6 points) Match EOT Spectrum C 100- 80- 60 40 75 100 125 50 m/z Spectrum D 100 80 60- 40 20- 25 50 75 100 125 m/z Spectrum E 100 80 60 20 10 20 30...
4. In a plot of elemental abundance in the solar system, the elements that fall after...
4. In a plot of elemental abundance in the solar system, the elements that fall after the iron group (Z >28) are much less abundant than most elements with Z< 28. Explain why. [5 points] Log abundance / 106 Si atoms 2000 & Xe YDPL 1 Tm Ta 0 10 20 30 70 80 90 100 40 50 60 Atomic number (2)
asap please 4. Consider the boxplot shown below of the points earned on the 124 points...
asap please
4. Consider the boxplot shown below of the points earned on the 124 points of problems on the Fall 2018 STA2220 final exam for the 108 students in the 3 Tuesday/Thursday sections: -++Points o 10 20 30 40 50 60 70 80 90 100 110 120 130 (2 a) Describe the distribution as symmetric, left-skewed, or right-skewed. (2) b) About what proportion of the students scored at least half of the points possible on these problems? CS) c)...
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.
45.5kJ/mol-1
Cesium has the lowest ionization energy of all the elements. 3-1 a) Explain why. (Don't just cite the periodic trends. Make sure you give a chemical explanation for this property.) b) What is the wavelength of a photon that could ionize a Cs atom? What region of the electromagnetic spectrum does this light belong to?
answer a b or c
Why is the atomic radius of magnesium ion much smaller than that of a neutral charged magnesium atom? (See the atomic radius graph) The magnesium ion's electrons require less space. No electrons are lost, they move to unoccupied spaces about the nucleus. The magnesium ion has fewer principle quantum energy levels, this causes a decrease in atomic radius. The magnesium ion has a higher Z-effective nuclear charge. The magnesium ion has more principle quantum energy...
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...
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...
Element Na First Ionization Energy (J/mol) 4.95 x 105 4.19 x 105 K 6. The first ionization energies for Na and K are given in the table above. a. Write the complete electron configuration for Na. b. Based on principles of atomic structure, explain why the first ionization energy of K is lower than the first ionization energy of Na. c. Which ionic solid would have the greatest melting point, NaCl or KCI? Justify your answer in terms of lattice...
Please match the compound to its spectrum and explain
why
cpd 22 Spectrum A 100- 60 40 20 100 125 50 75 m/z Spectrum B 100 80- 60 40 20- 10 20 30 40 50 60 70 0 90 100 110 120 m/z (6 points) Match EOT Spectrum C 100- 80- 60 40 75 100 125 50 m/z Spectrum D 100 80 60- 40 20- 25 50 75 100 125 m/z Spectrum E 100 80 60 20 10 20 30...
4. In a plot of elemental abundance in the solar system, the elements that fall after the iron group (Z >28) are much less abundant than most elements with Z< 28. Explain why. [5 points] Log abundance / 106 Si atoms 2000 & Xe YDPL 1 Tm Ta 0 10 20 30 70 80 90 100 40 50 60 Atomic number (2)
asap please
4. Consider the boxplot shown below of the points earned on the 124 points of problems on the Fall 2018 STA2220 final exam for the 108 students in the 3 Tuesday/Thursday sections: -++Points o 10 20 30 40 50 60 70 80 90 100 110 120 130 (2 a) Describe the distribution as symmetric, left-skewed, or right-skewed. (2) b) About what proportion of the students scored at least half of the points possible on these problems? CS) c)...
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