MC EXAMPLE. Which of the following is expected to have the largest size? a. O2+
ID: 1042965 • Letter: M
Question
MC EXAMPLE. Which of the following is expected to have the largest size? a. O2+ b. O ?. 02. d. S2+ e. S2 MC EXAMPLE. Which of the following has the largest ionic radius? a. O2 C. Na+ d. Mg2+ e. They all have about the same size FREE RESPONSE. Consider only all alkaline earth metals and all halogens. Determine which element has: a. the largest atomic size b. the highest electronegativity c. the largest ionization energy d. the highest metallic character e. the highest molecular weight (molar mass) FREE RESPONSE: Consider the elements lithium, beryllium, sodium, and magnesium Of these four elements: a. Which has the largest atomic mass? b. Which is the most electronegative? c. Which has the highest first ionization energy? d. Which has the most metallic character? e. Which is most likely to have five neutrons in an atom?Explanation / Answer
4.
(a) Magnesium has largest atomic mass.
As you go from left to right in the Periodic Table, you are adding more protons and neutrons to the nuclei. The atoms in the rows further down have even more protons and nucleons. Therefore, atomic mass increases from left to right and from top to bottom of the Periodic Table.
(b) Beryllium
From left to right across a period of elements, electronegativity increases. If the valence shell of an atom is less than half full, it requires less energy to lose an electron than to gain one. Conversely, if the valence shell is more than half full, it is easier to pull an electron into the valence shell than to donate one.
From top to bottom down a group, electronegativity decreases. This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius.
(c) Beryllium
Across a period, Zeff increases and n (principal quantum number) remains the same, so the ionization energy increases.
Down a group, n increases and Zeff increases slightly; the ionization energy decreases.
(d)
Move left across period and down the group: increase metallic character (heading towards alkali and alkaline metals)
Move right across period and up the group: decrease metallic character (heading towards nonmetals like noble gases).
(e) All the elements have five and more neutrons.
3.
(a) Radon
Atomic radius decreases from left to right within a period. This is caused by the increase in the number of protons and electrons across a period. One proton has a greater effect than one electron; thus, electrons are pulled towards the nucleus, resulting in a smaller radius.
Atomic radius increases from top to bottom within a group. This is caused by electron shielding.
(b) Fluorine
From left to right across a period of elements, electronegativity increases. If the valence shell of an atom is less than half full, it requires less energy to lose an electron than to gain one. Conversely, if the valence shell is more than half full, it is easier to pull an electron into the valence shell than to donate one.
From top to bottom down a group, electronegativity decreases. This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius.
(c) Fluorine
The ionization energy of the elements within a period generally increases from left to right. This is due to valence shell stability.
The ionization energy of the elements within a group generally decreases from top to bottom. This is due to electron shielding.
(d) Radon
Move left across period and down the group: increase metallic character (heading towards alkali and alkaline metals)
Move right across period and up the group: decrease metallic character (heading towards nonmetals like noble gases)
(e) Radon
?Atomic number 88.
2. O2-
Explained in above questions.
1. Answer is option (e) S2-.
Atomic size of S is greater than O. Since extra principal quantum number is added. Again extra two electrons are being added in S in S2-.
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