Chemistry

Chemistry, 29.09.2019 22:30, luhhbitilia566

What are the exceptions to the trend in ionization energy

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Chemistry, 30.07.2019 15:10, lauretta

The trend for ionization energy is a general increase from left to right across a period. however, phosphorus (p) is found to have a higher first ionization energy value than sulfur (s). explain this exception to the general trend in terms of electron arrangements and attraction/repulsion.

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Chemistry, 16.09.2019 04:30, kotetravels10

1.) use the interactive periodic table to answer the following questions about ionization energy. what is the first ionization energy (ie1) of sulfur (atomic number 16)? write the expressions for the successive ionization energies of s (ie1 to ie7)? plot the successive ionization energies of s (ie1 to ie7). what trend is seen in this plot? how do you explain the change in slope associated with the ie7? 2.) use the interactive periodic table to answer the following questions about ionization energy. start by selecting the periodic table link on the upper right side of the page beneath the sf6 molecule. using the pull down menu at the bottom of the table, select ionization energy. plot the first ionization energies (ie1) of the group 1 elements. what is the trend in ie1? what trend do you think you will you see if you plot any other group? (check your prediction.) compare the trend in ie1 to the trend in atomic radii. is there a connection? 3.)what is electron affinity? give a definition and illustrate it by showing the process for a gas phase atom.

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Physics, 30.09.2019 22:30, gianna78

What are the exceptions to the general periodic trend in first ionization energy within a period?

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Chemistry, 18.10.2019 18:30, hannahkharel2

When atoms lose more than one electron, the ionization energy to remove the second electron is always more than the ionization energy to remove the first. similarly, the ionization energy to remove the third electron is more than the second and so on. however, the increases in ionization energy upon the removal of subsequent electrons is not necessarily uniform. for example, consider the first three ionization energies of magnesium: first ionization energy 738kj/mol second ionization energy 1450kj/mol third ionization energy 7730kj/mol the second ionization energy is roughly twice the first ionization energy, but then the third ionization energy is over five times the second. use the electronic configuration of magnesium to explain why this is so? would you expect the same behavior in sodium? why or why not?

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