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(a) Rank these elements in order of increasing atomic radius: O, S, F. Briefly explain your reasoning.

(b) Which element has the largest first ionization energy: P, Si, S, Se? Briefly explain your reasoning.

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Patrick Suarez
Patrick SuarezLv10
25 Nov 2020

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Related questions

Answer each of the following:

(a) Place the following elements in order of increasing ionization energy: F, O, and S

(b) Which has the largest ionization energy: O, S, or Se?

(c) Which has the most negative electron attachment enthalpy: Se, Cl, or Br?

(d) Which has the largest radius: O2-, F-, or F?

1.Arrange the following elements in order of decreasing ionization energy. Rank from highest to lowest ionization energy. To rank items as equivalent, overlap them. Lowest ionization energyHighest ionization energy

sulfur calcium iron zinc carbon The correct ranking cannot be determined.;

part 2. Arrange the following elements in order of decreasing metallic character. Rank from most to least metallic character. To rank items as equivalent, overlap them. P Cr F Ca S Co Zn Rb Least metallic characterMost metallic character

part 3.Rank the following elements by atomic radius.

Rank from largest to smallest atomic radius. To rank items as equivalent, overlap them.

Ar

Mg

Si

S

Al

Smallest

Largest

part 4.

Rank the following atoms by number of valence electrons.

Rank from most to fewest valence electrons. To rank items as equivalent, overlap them.

Br

Ga

Xe

As

K

Arrange the elements Na, Si, and S in the order of

(a) decreasing atomic radius.

(b) increasing first ionization energy.

(c) decreasing electronegativity.

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