1. Ch 7, Problem 106 and 108 First arrange the following groups of atoms in order of increasing size. Then arrange them in order of increasing order of first ionization energy. Explain your orders! Note: Simply stating the trend of "atomic radius increases down the periodic table" is not sufficient. Explain why. a. Rb, Na, Be b. Ве, С, О
1. Ch 7, Problem 106 and 108 First arrange the following groups of atoms in order of increasing size. Then arrange them in order of increasing order of first ionization energy. Explain your orders! Note: Simply stating the trend of "atomic radius increases down the periodic table" is not sufficient. Explain why. a. Rb, Na, Be b. Ве, С, О
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![1. Ch 7, Problem 106 and 108
First arrange the following groups of atoms in order of increasing size. Then arrange
them in order of increasing order of first ionization energy. Explain your orders! Note:
Simply stating the trend of "atomic radius increases down the periodic table" is not
sufficient. Explain why.
a. Rb, Na, Be
b. Ве, С, О
2. a. How does electronegativity change as you go across the periodic table? Down the
periodic table? Why?
b. Hydrogen's location on the periodic table doesn't accurately reflect its relative
electronegativity. Look at the Figure 8.3, which provides quantitative values for
electronegativity (bigger number, more electronegative). If you were to place H
between two elements on the 2nd row, where would it go? 3rd row? Etc. It is important
to know where H fits into the trend so that you can predict dipole moments for X-H
bonds.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d1b384e-c50f-4ff0-a124-3a5f7d0a3354%2F49d3f4fc-f345-4305-98b3-5e6890196bc9%2F58co8db_processed.png&w=3840&q=75)
Transcribed Image Text:1. Ch 7, Problem 106 and 108
First arrange the following groups of atoms in order of increasing size. Then arrange
them in order of increasing order of first ionization energy. Explain your orders! Note:
Simply stating the trend of "atomic radius increases down the periodic table" is not
sufficient. Explain why.
a. Rb, Na, Be
b. Ве, С, О
2. a. How does electronegativity change as you go across the periodic table? Down the
periodic table? Why?
b. Hydrogen's location on the periodic table doesn't accurately reflect its relative
electronegativity. Look at the Figure 8.3, which provides quantitative values for
electronegativity (bigger number, more electronegative). If you were to place H
between two elements on the 2nd row, where would it go? 3rd row? Etc. It is important
to know where H fits into the trend so that you can predict dipole moments for X-H
bonds.
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