Consider the following information for sodium and chlorine: Atomic radius: Na (186 pm) and Cl (100pm)...
Consider the following information for sodium and
chlorine:
Atomic radius: Na (186 pm) and Cl (100pm)
Ionic radius: Na+(102pm) and Cl-(181pm)
Why does the atomic radius decrease while ionic radius
increase?
The outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do.
Monatomic ions are bigger than the atoms from which they are formed.
The outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do.
The inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion.
The inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do.
Homework Answers
The outermost electrons in chloride experience a smaller effective nuclear charge than those sodium cation do that's why in chloride there is less attraction between outermost electron and nucleus so greater radius
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Consider the following information for sodium and
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Atomic radius: Na (186 pm) and Cl (100pm)...
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Sodium (Na) atoms are larger than chlorine (Cl) atoms, but in NaCl sodium ions (Na+) are much smaller than chloride (Cl-) ions. Discuss why there is a change in size of each element (i.e., why is Na --> Na+ a decrease in size and Cl --> Cl- is an increase in size).
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Help with explanation if possible.
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answer a b or c
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- Parta Explain why atomic radius decreases as you move to the right across a period for main-group elements but not for transition elements Match the words in the left column to the appropriate blanks in the sentences on the right Reset Help proton larger As you move to the right across a row in the periodic table for the main-group elements, the effective nudear charge (Zl) experienced by the electrons in the outermost principal energy level resulting in a...
Help with explanation if possible.
Nae Section -Date Now let's look at chlorine A chlorine atom has how many protons Therefore, we know that a chlorine atom has how many electrons? How many electrons will go in the first shell? How many in the second shell? Nucleus How many in the third? Draw this in Figure 2.2 We know that a chlorine atom requires eight electrons in its valence shell to become stable. Will it be easier for chlorine to...
answer a b or c
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