Pes

Which element has the electron configuration 1s²2s²2p⁶3s²3p⁵?

• chlorine

• fluorine

• sulfur

• phosphorus

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

How many peaks would you see for the PES graph for the element with an electron configuration of 1s²2s²2p⁶3s¹

• 2

• 3

• 4

• 5

Tags

NGSS.HS-PS1-1

What is the electron configuration for this PES graph?

• 1s²2s²2p⁶3s²3p²

• 1s²2s²2p⁶3s²3p¹

• 1s²2s²2p⁶3s²3p³

• 1s²2s²2p⁶3s²

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which element is represented by this PES graph?

• aluminum

• phosphorus

• sulfur

• silicon

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which element is represented by this PES graph?

• argon

• potassium

• calcium

• scandium

Tags

NGSS.HS-PS1-1

Which element is represented by this PES graph?

• calcium

• potassium

• titanium

• scandium

Tags

NGSS.HS-PS1-1

The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the right of the peak in the lower spectrum?

• Nitrogen atoms have a half-filled p subshell.

• There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms.

• Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p sub shell of nitrogen atoms.

• Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

Answer explanation

"Nuclear charge" = charge of the nucleus. A greater nuclear charge will result in a greater attraction to the 1s electrons, and therefore more energy will be required to remove those electrons.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

A sample containing atoms of C and F was analyze using x-ray photoelectron spectroscopy. The portion of the spectrum showing the 1s peaks for atoms of two elements is shown above. Which of the following correctly identifies the 1s peak for the fluorine atoms and provides an appropriate explanation?

• Peak X, because F has a smaller first ionization energy than C has.

• Peak X, because F has a greater nuclear charge than C has.

• Peak Y, because F is more electronegative than C is.

• Peak Y, because F has a smaller atomic radius than C has.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

The complete photoelectron spectrum for an element is shown above. Which of the following observations would provide evidence that the spectrum is consistent with the atomic model of the element?

• A neutral atom of the element contains exactly two electrons.

• The element does not react with other elements to form compounds.

• In its compounds, the element tends to form ions with a charge of +1.

• In its compounds, the element tends to form ions with a charge of +3.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

How many peaks would you expect to see on the PES graph for potassium? (*Hint: write out the electron configuration first.)

• 5

• 6

• 7

• 8

Answer explanation

1s²2s²2p⁶3s²3p⁶4s¹ -- 6 peaks

Tags

NGSS.HS-PS1-1