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Would you expect it to be harder to remove an electron from Na or O?
Wiki User
∙ 13y ago
oxygen
Wiki User
∙ 13y ago
It would be easier to remove an electron from Na compared to O. Sodium (Na) has a smaller effective nuclear charge and a larger atomic radius compared to oxygen (O), making its valence electron easier to remove. Oxygen has a higher electronegativity and a stronger pull on its electrons, making it harder to remove an electron from O.
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How many electrons does magnesium have in its outermost electron as a result you would expect magnesium to form ions charge of?
Magnesium has 2 electrons in its outermost electron shell. As a result, you would expect magnesium to form ions with a charge of +2 by losing these two outer electrons to achieve a stable electron configuration.
What electron would require the least amount of energy to remove from the atom of sulfur?
This is an electron situated on the outermost level.
In an electron dot diagram of potassium There is one dot. In an electron dot diagram of silicon there are four dots. Which element would you expect to be more reactive?
silicon
What type of bond would you expect 39k19 to form?
39K19 refers to the element potassium. Potassium is an alkali metal that tends to form ionic bonds due to its tendency to lose an electron and achieve a stable octet configuration. Therefore, you would expect 39K19 to form ionic bonds with other elements by donating its one valence electron.
Would you expect nonmetals to have larger electron affinities than metals?
Yes. Non metals have larger electron affinity than metals as non metals accept electrons more easily than metals.
What would be harder to remove an electron from sodium or chlorine?
It would be harder to remove an electron from chlorine because it has a higher electronegativity compared to sodium. This means that chlorine has a stronger pull on its electrons, making it more difficult to remove an electron.
Would it be most difficult to remove an electron from sodium aluminum sulfur or chlorine?
It would be most difficult to remove an electron from chlorine because it has the highest electron affinity among the elements mentioned. Sodium has the lowest ionization energy, meaning it's easiest to remove an electron from it.
Would it be more difficult to remove an electron from sodium or bromine?
It would be more difficult to remove an electron from bromine than from sodium because bromine's valence electron is farther from the nucleus, experiencing weaker attraction compared to sodium's valence electron, which is closer to the nucleus.
What electron would require the least amount of energy to remove from the atom of sulfur?
This is an electron situated on the outermost level.
In an electron dot diagram of potassium there is one dot. in an electron dot diagram of silicone there are four dots. which element would you expect to be more reactive?
silicon
In an electron dot diagram of potassium There is one dot. In an electron dot diagram of silicon there are four dots. Which element would you expect to be more reactive?
silicon
If enough energy was added to remove an electron for calcium which energy level would the electron be removed?
The electron would be removed from the outermost energy level, which is the fourth energy level, for calcium.
What type of bond would you expect potassium to form?
Potassium would typically form an ionic bond, because it readily donates its outer electron to achieve a more stable electron configuration. This electron transfer allows potassium to bond with other elements that can accept its electron.
It would take more or less energy to remove an electron from sodium than from chlorine?
It would take less energy to remove an electron from sodium than from chlorine because sodium has a lower ionization energy than chlorine. This means that sodium's outer electron is held less tightly compared to chlorine's outer electron.
Would you expect a chlorine ion to be smaller than a magnesium ion?
No, I would expect a chlorine ion to be slightly larger than a magnesium ion. Chlorine gains an electron to form a chloride ion, which increases its electron cloud size, while magnesium loses electrons to form a magnesium ion, making it slightly smaller due to the loss of electron shielding.
Why would you never expect to find Na2Cl as a stable compound?
Na2Cl would not be a stable compound because sodium typically loses one electron to achieve a stable electron configuration, while chlorine gains one electron for stability. In this case, sodium would need to lose two electrons to chlorine, which is energetically unfavorable. Thus, NaCl is the stable compound where sodium donates one electron to chlorine.
If you were to remove an electron from this sodium(Na)atomwhat would be the electrical charge of the ion?
+ (positive)
