Chemistry

Chemistry, 03.07.2019 22:00, 10027126

Among the elements listed, which would show the largest increase between the second and third ionization energies? a. p b. zn c. b d. ca

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Chemistry, 17.07.2019 03:20, kcain1020

The ionization energies of rubidium and silver are 4.18 and 7.57 ev, respectively. calculate the ionization energies of an h atom with its electron in the same outermost orbitals as in these two atoms and account for the differences in values in these different elements.

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Chemistry, 26.07.2019 12:30, s103394

Why are the trends and exceptions to the trends in ionization energy observed? check all that apply. ionization energy tends to increase down a group because the electrons get farther away from the nucleus. ionization energy tends to increase across a period because the nuclear charge increases. ionization energy tends to increase across a period because electrons are added to the same main energy level. the ionization energies of the elements in group 16 tend to be slightly smaller than the elements in group 15 because the fourth electron is added to an unfilled p orbital. the ionization energies of elements in group 13 tend to be lower than the elements in group 2 because the full s orbital shields the electron in the p orbital from the nucleus.

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Chemistry, 16.10.2019 13:30, osmanysalvador9

Which of the following statements about ionization energy is true? a. in a period, elements farther to the right generally have lower ionization energies than elements on the left. b. elements toward the bottom of a group periodic table generally have higher ionization energies than elements at the top of the group. c. ionization energy is the amount of energy used to add an electron to an atom. d. potassium has a lower ionization energy than sodium.

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Chemistry, 30.10.2019 18:31, door9817

Why are the trends and exceptions to the trends in ionization energy observed? check all that apply. lonization energy tends to increase down a group because the electrons get farther away from the nucleus. b lonization energy tends to increase across a period because the nuclear charge increases. lonization energy tends to increase across a period because electrons are added to the same main energy level. the ionization energies of the elements in group 16 tend to be slightly smaller than the elements in group 15 because the fourth electron is added to an unfilled p orbital. the ionization energies of elements in group 13 tend to be lower than the elements in group 2 because the full s orbital shields the electron in the p orbital from the nucleus.

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