ionization energy Q

[cloak25]

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For an element with a first ionization energy of 589 kJ/mole, a second ionization energy of 1146 kJ/mole, and a third ionization energy of 4892 kJ/mole, what is true of its oxide?

A. It's oxide will be acidic
B. It will be a solid at room temperature
C. It will have a boiling point less than water
D. It will have a 2:1 ratio between the element and the oxygen in it's fully oxidized state.

Answer: B

Can someone explain how they found the identity of the element based off of the ionization energy values given? Thanks

 

[GeorgiadisMD]

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[hiaips]

For an element with a first ionization energy of 589 kJ/mole, a second ionization energy of 1146 kJ/mole, and a third ionization energy of 4892 kJ/mole, what is true of its oxide?

A. It's oxide will be acidic
B. It will be a solid at room temperature
C. It will have a boiling point less than water
D. It will have a 2:1 ratio between the element and the oxygen in it's fully oxidized state.

Answer: B

Can someone explain how they found the identity of the element based off of the ionization energy values given? Thanks

Note the large jump between IE2 and IE3 values and recall that a great deal of energy is required to remove electrons from a filled valence shell. Together, these facts suggest that the element in question has two electrons in its outer shell, which is consistent with elements from group 2 (i.e., alkaline earth metals). From there you should be able to eliminate choices A, C, and D.

 

[Class1P]

A is what I chose.

I assumed since it was oxidized and had high energies, it would be more likely to pick up electrons making it a lewis acid.

 

[cloak25]

A is what I chose.

I assumed since it was oxidized and had high energies, it would be more likely to pick up electrons making it a lewis acid.

If you figure that the element is an alkali earth metal, i.e. Mg2+, then A should be eliminated immediately because metal oxides are basic. Nonmetal oxides are acidic.