Chemistry

Chemistry, 18.10.2019 20:40, skeeziks2005

How does ionization energy change on the periodic table?

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Chemistry, 17.07.2019 17:40, ednalovegod

1. how are atomic radii and ionization energy related (i.e. as atomic radius increases, what happens to the ionization energy)? 2. generally, as you go from left to right across a period on the periodic table, what happens to atomic radius? what about ie? 3. generally, as you go down a group in the periodic table, what happens to atomic radius and ie? 4. why does radius increase as you go down a group (hint: think of b-r diagrams)? why would an increase in radius make it easier to lose an outer electron (i.e. give a lower ionization energy)?

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Chemistry, 02.08.2019 00:00, anyaimartinez1901

Ionization energy is a measure of how strongly an atom holds onto its electrons. a higher ionization energy indicates that more energy would be needed to remove an electron. atoms that have a smaller atomic radius tend to have higher ionization energies because their electrons are closer to the nucleus. based on the periodic table, which element would be expected to have the lowest ionization energy? a) calcium (ca) b) cesium (cs) c) sodium (na) d) strontium (sr) wrong answers will be reported.

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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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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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