TBR Chem 2 Example 2.23

[MedPR]

---

Members do not see this ad.

The trend in electronegativity increases with which of the following?
A. Ionization Energy
B. Atomic Radius
C. Atomic Number
D. Number of Valence Electrons


Based on the question, none of the answers is true. Oxygen has less valence electrons than Chlorine, but is more electronegative. To get the correct (according to TBR) answer, you would have to assume that the question is referring only to the same row. Under the same assumption, and excluding the noble gases, answer C is true since Fluorine has the highest atomic number among row 2 elements. However, you can make answer A true if you consider Fluorine compared to Iodine (Fluorine is more electronegative and has a higher ionization energy).

Am I missing something?

 

[MT Headed]

Without any context, all of the answers are correct except B.

 

[chiddler]

Without any context, all of the answers are correct except B.

A isn't true either. Ti to V for example decreases in ionization energy while electronegativity increases.

I think you're right, medpr, about it being a flawed question.

 

[MrNeuro]

The trend in electronegativity increases with which of the following?
A. Ionization Energy
B. Atomic Radius
C. Atomic Number
D. Number of Valence Electrons


Based on the question, none of the answers is true. Oxygen has less valence electrons than Chlorine, but is more electronegative. To get the correct (according to TBR) answer, you would have to assume that the question is referring only to the same row. Under the same assumption, and excluding the noble gases, answer C is true since Fluorine has the highest atomic number among row 2 elements. However, you can make answer A true if you consider Fluorine compared to Iodine (Fluorine is more electronegative and has a higher ionization energy).

Am I missing something?

this question tripped me up as well the only "justification" i could make was that comparing diagonally is not possible? but if you were to just compare within a elements period and group you'd find that valence fits.

Correct me if I'm wrong.

 

[MedPR]

this question tripped me up as well the only "justification" i could make was that comparing diagonally is not possible? but if you were to just compare within a elements period and group you'd find that valence fits.

Correct me if I'm wrong.

Elements in the same group have the same number of valence electrons, but as you move up a group the electronegativity increases.

Valence only fits in the same period.

 

[MrNeuro]

Elements in the same group have the same number of valence electrons, but as you move up a group the electronegativity increases.

Valence only fits in the same period.

What i meant to say is valence is the "best" choice

across a period we can cancel out A and B
down a group
Atomic # increases
valence shel doesn't change
electronegativity decreases

They're both wrong but one is a better choice....personally i think TBR its frustrating as hell sometimes with some of these questions...

 

[MedPR]

What i meant to say is valence is the "best" choice

across a period we can cancel out A and B
down a group
Atomic # increases
valence shel doesn't change
electronegativity decreases

They're both wrong but one is a better choice....personally i think TBR its frustrating as hell sometimes with some of these questions...

Doesn't ionization energy increase across a period?

Yea valence is the best choice under certain conditions, but anytime I can easily prove an answer wrong I throw it out. Valence is only true if you stay within the period.

 

[MrNeuro]

Doesn't ionization energy increase across a period?

Yea valence is the best choice under certain conditions, but anytime I can easily prove an answer wrong I throw it out. Valence is only true if you stay within the period.

ionization energy does increase across a period however it varies due to s2 and half filled shell stability