Which of the following best helps to account for the fact that the Fion is smaller than the O2- ion?

F - has a larger nuclear charge than O 2- has.

F - has a larger nuclear mass than O 2- has.

F - has more electrons than O 2- has.

F - is more electronegative than O 2- is.

Two different ionic compounds each contain only copper and chlorine. Both compounds are powders, one white and one brown. An elemental analysis is performed on each powder. Which of the following questions about the compounds is most likely to be answered by the results of the analysis?

What is the formula unit of each compound?

What is the density of each pure compound?

What is the chemical reactivity of each compound?

Which of the two compounds is more soluble in water?

A student conducts an experiment to determine the percentage of silver in an alloy by first reacting the alloy with nitric acid. The student then precipitates the Ag + (aq) by adding excess NaCl (aq) to form AgCl (s) according to the equation. Ag + (aq) + Cl - (aq) --> AgCl (s) The precipitate is filtered, dried, and weighed. Which of the following indicates the effect on the calculated percentage of silver if the precipitate was not dried completely before weighing it, and explains why?

The calculated percentage is too high because the additional water adds mass to the AgCl (s), and the student will calculate a higher mass of Ag in the sample.

The calculated percentage is too low because the additional water will cause a significant quantity of the AgCl (s) to dissolve and wash through the filter paper.

The calculated percentage is too low because water has a significantly lower molar mass than AgCl (s), which reduces the average mass of the precipitate.

The calculated percentage is the same because the additional water does not affect the mass of the alloy, and the student will react the same mass of Ag regardless.

To gravimetrically analyze the silver content of a piece of jewelry made from an alloy of Ag and Cu, a student dissolves a small preweighed sample in HNO 3 (aq). Ag + (aq) and Cu 2+ (aq) ions form in the solution. Which of the following should be the next step in the analytical process?

Adding a solution containing an anion that forms an insoluble salt with only one of the metal ions

Centrifuging the solution to isolate the heavier ions

Evaporating the solution to recover the dissolved nitrates

Adding enough base solution to bring the pH up to 7.0

For element X represented above, which of the following is the most likely explanation for the large difference between the second and third ionization energies?

The electron removed during the third ionization is, on average, much closer to the nucleus than the first two electrons removed were.

The effective nuclear charge decreases with successive ionizations.

The shielding of outer electrons increases with successive ionizations.

The ionic radius increases with successive ionizations.

. In his atomic theory, Dalton proposed that all atoms of a given element are identical. Which of the following observations provides the best evidence that the proposal is incorrect?

The mass spectrum of Cu has a peak at 63 amu and another peak at 65 amu.

The ionic radius of Cl - is 0.181 nm, and the atomic radius of Cl is 0.079 nm.

The dipole moment of O 3 is 0.53 debye, and the dipole moment of O 2 is 0.00 debye.

Elemental P can exist in both white and red forms.

Which of the following correctly compares periodic properties of two elements and provides an accurate explanation for that difference?

The atomic radius of Cl is smaller than that of S because Cl has a larger nuclear charge than S does.

The first ionization energy of Al is greater than that of B because Al has a larger nuclear charge than B does.

The first ionization energy of F is greater than that of O because O has a higher electronegativity than F has.

The atomic radius of Ca is larger than that of Mg because the valence electrons in Mg experience more shielding than the valence electrons in Ca do.

A group of students was asked to recover Cu(s) from a blue-green aqueous solution containing an unknown concentration of Cu 2+ (aq) . The students took a 100.0 mL sample of the solution and added an excess of 1.0 M Na 3 PO 4 (aq), causing the Cu 2+ (aq) to precipitate as Cu 3 (PO 4 ) 2 (s), as shown in step 1 below. The mass of the Cu(s) produced in step 3 was slightly more than the mass predicted from the 4.6 g of Cu 3 (PO 4 ) 2 (s) recovered from step 1. Which of the following could account for the discrepancy in the yield of Cu(s) from step 3 ?

Some unreacted Zn(s) was mixed in with the Cu(s).

All of the Cu 3 (PO 4 ) 2 (s) dissolved in the HCl(aq).

Some of the Cu(s) adhered to the side of the funnel used to filter the solution.

Too much Na 3 PO 4 (aq) was added to the original Cu 2+ (aq) solution.

A group of students was asked to recover Cu(s) from a blue-green aqueous solution containing an unknown concentration of Cu 2+ (aq) . The students took a 100.0 mL sample of the solution and added an excess of 1.0 M Na 3 PO 4 (aq), causing the Cu 2+ (aq) to precipitate as Cu 3 (PO 4 ) 2 (s), as shown in step 1 below. Finally, the Cu(s) was filtered, dried, and weighed. The mass of the Cu(s) produced in step 3 was slightly more than the mass predicted from the 3.8 g of Cu 3 (PO 4 ) 2 (s) recovered from step 1. Which of the following could account for the discrepancy in the yield of Cu(s) from step 3 ?

Some unreacted Zn(s) was mixed in with the Cu(s).

All of the Cu 3 (PO 4 ) 2 (s) dissolved in the HCl(aq).

Some of the Cu(s) adhered to the side of the funnel used to filter the solution.

Too much Na 3 PO 4 (aq) was added to the original Cu 2+ (aq) solution.

Which of the following best helps to explain why the electron affinity of Br has a greater magnitude than that of I?

There is a greater attraction between an added electron and the nucleus in Br than in I.

Br has a lower electronegativity than I does.

Br has a lower ionization energy than I does.

An added electron would go into a new shell in Br but not in I.

31. Which of the following best helps explain why the electronegativity of Cl is less than that of F?

When Cl and F forms bonds with other atoms, the Cl bonding electrons are more shielded from the positive Cl nucleus than the F bonding electrons are shielded from the positive F nucleus.

The mass of the Cl atom is greater than the mass of the F atom.

The Cl nucleus contains more protons than the F nucleus contains.

Because Cl is larger than F, the repulsions among electrons in the valence shell of Cl are less than the repulsions among electrons in the valence shell of F.

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 smaller nuclear charge than oxygen atoms.

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 subshell of nitrogen atoms.

The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following?

Na has a lower first ionization energy than Ne.

Na has a greater density at standard conditions than Ne.

Na has a higher melting point than Ne.

Na has a higher neutron-to-proton ratio than Ne.

Which of the following best represents the ground-state electron configuration for an atom of selenium?

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 4

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5

After completing an experiment to determine gravimetrically the percentage of water in a hydrate, a student reported a value of 38 percent. The correct value for the percentage of water in the hydrate is 51 percent. Which of the following is the most likely explanation for this difference?

The dehydrated sample absorbed moisture after heating.

Strong initial heating caused some of the hydrate sample to spatter out of the crucible.

The crucible was not heated to constant mass before use.

Excess heating caused the dehydrated sample to decompose

Silicon crystals are semiconductors. Which of the following is a correct reason for the increase in the conductivity of Si crystals when a small fraction of Si atoms are replaced with those of a different element?

P atoms introduce additional mobile negative charges.

P atoms introduce additional mobile positive charges.

Ge atoms have more electrons than Si atoms have.

Ge atoms are much smaller than Si atoms

AP Chemistry Unit 1 MCQ 1.5 minutes

Authored by Mohammad Saleh

Chemistry

12th Grade

NGSS covered

Used 1+ times

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MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following represents a pair of isotopes?

Tags

NGSS.HS-PS1-8

MULTIPLE CHOICE QUESTION

1 min • 1 pt

The elements I and Te have similar average atomic masses. A sample that was believed to be a mixture of I and Te was run through a mass spectrometer, resulting in the data above. All of the following statements are true. Which one would be the best basis for concluding that the sample was pure Te?

Te forms ions with a −2 charge, whereas I forms ions with a −1 charge.

Te is more abundant than I in the universe.

I consists of only one naturally occurring isotope with 74 neutrons, whereas Te has more than one isotope.

I has a higher first ionization energy than Te does

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following has the lowest first-ionization energy?

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following has the highest electronegativity?

Tags

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following has the largest atomic radius?

Tags

NGSS.HS-PS1-1

MULTIPLE CHOICE QUESTION

1 min • 1 pt

According to the information in the table above, a 1.00 g sample of which of the following contains the greatest mass of oxygen?

Na₂O

MgO

K₂O

CaO

Tags

NGSS.HS-PS1-7

MULTIPLE CHOICE QUESTION

1 min • 1 pt

The table above shows the first ionization energy and atomic radius of several elements. Which of the following best helps to explain the deviation of the first ionization energy of oxygen from the overall trend?

The atomic radius of oxygen is greater than the atomic radius of fluorine.

The atomic radius of oxygen is less than the atomic radius of nitrogen.

There is repulsion between paired electrons in oxygen’s 2p orbitals.

There is attraction between paired electrons in oxygen’s 2p orbitals.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

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