A student obtains a 10.0g sample of a white powder labeled as BaCl 2 . After completely dissolving the powder in 50.0mL of distilled water, the student adds excess Na 2 SO 4 (s), which causes a precipitate of BaSO 4 (s) to form, as represented by the equation above. The student filters the BaSO 4 (s), rinses it, and dries it until its mass is constant. Which of the following scientific questions could best be answered based on the results of the experiment?

Is the BaCl 2 (s) used in the experiment pure?

Is the Na 2 SO 4 (s) used in the experiment pure?

What is the molar solubility of BaCl 2 in water?

What is the molar solubility of BaSO 4 in water?

A student measures the mass of a sample of a metallic element, M. Then the student heats the sample in air, where it completely reacts to form the compound MO. The student measures the mass of the compound that was formed. Which of the following questions can be answered from the results of the experiment?

What is the melting point of M?

What is the melting point of MO?

A 42.0g sample of compound containing only C and H was analyzed. The results showed that the sample contained 36.0g of C and 6.0g of H. Which of the following questions about the compound can be answered using the results of the analysis?

What is the empirical formula of the compound?

What was the volume of the sample?

What is the molar mass of the compound?

What is the chemical stability of the compound?

A student obtains a mixture of the chlorides of two unknown metals, X and Z. The percent by mass of X and the percent by mass of Z in the mixture is known. Which of the following additional information is most helpful in calculating the mole percent of XCl(s) and of ZCl(s) in the mixture?

The density of either XCl(s) or ZCl(s)

The percent by mass of Cl in the mixture

A vessel contains a mixture of gases. The mass of each gas used to make the mixture is known. Which of the following information is needed to determine the mole fraction of each gas in the mixture?

The density of the gases in the vessel

The total pressure of the gases in the vessel

The number of atoms per molecule for each gas

The complete photoelectron spectrum of an element is given above. Which labeled peak corresponds to the 1s electrons and why?

Peak X, because 1s electrons have the strongest attractions to the nucleus.

Peak X, because 1s electrons are the easiest to remove from the atom.

Peak Y, because electrons in the 1s sublevel are the farthest from the nucleus.

Peak Y, because there are fewer electrons in an s sublevel than in a p sublevel.

The photoelectron spectrum for the element boron is represented above. Which of the following best explains how the spectrum is consistent with the electron shell model of the atom?

The spectrum shows a single electron in the 2p subshell.

The spectrum shows an odd number electrons.

The spectrum shows equal numbers of electrons in the first and second electron shells.

The spectrum shows three electrons with the same binding energy in the second electron shell.

The complete photoelectron spectrum of the element carbon is represented above. Which of the following best explains how the spectrum is consistent with the electron shell model of the atom?

The spectrum shows equal numbers of electrons in the three occupied electron subshells.

The spectrum shows four electrons in the inner electron shell.

The spectrum shows that all the electrons in the valence shell have the same binding energy.

The spectrum shows more electrons in the inner electron shell than in the outer electron shell.

The atomic radii of the elements in the nitrogen group in the periodic table are given in the table above. Which of the following best helps explain the trend of increasing atomic radius from N to Bi?

The attractive force between the valence electrons and the nuclei of the atoms decreases.

The number of particles in the nucleus of the atom increases.

The number of electrons in the outermost shell of the atom increases.

The repulsive force between the valence electrons and the electrons in the inner shells decreases.

Which of the following best helps to explain why the atomic radius of K is greater than that of Br?

The effective nuclear charge experienced by valence electrons is smaller for K than for Br.

The first ionization energy of K is higher than that of Br.

The valence electrons in K are in a higher principal energy level than those of Br.

In the ground state, an atom of K has fewer unpaired electrons than an atom of Br has.

Which of the following best helps explain why the first ionization energy of K is less than that of Ca?

The valence electron of K experiences a lower effective nuclear charge than the valence electrons of Ca.

The electronegativity of K is greater than that of Ca.

The atomic radius of the K atom is less than that of the Ca atom.

The nucleus of the K atom has fewer neutrons, on average, than the nucleus of the Ca atom has.

Which of the following best helps explain why an atom of Rb gas more easily loses an electron in a chemical reaction than an atom of Li gas?

In the Rb atom the valence electron is farther from its nucleus than the valence electron of Li is from its nucleus.

Rb has a higher electronegativity than Li has.

The Rb atom has a greater number of valence electrons than the Li atom has.

The nucleus of the Rb atom has a greater number of protons and neutrons than the nucleus of the Li atom has.

Rb reacts with O in a mole ratio of 2 to 1, forming the ionic compound Rb 2 O. Which of the following elements will react with O in a mole ratio of 2 to 1, forming an ionic compound, and why?

Cs, because it is in the same group as Rb.

S, because it is in the same group as O.

Sr, because it is in the same period as Rb.

Br, because the atomic mass of Br is similar to that of Rb.

What charge does Al typically have in ionic compounds, and why?

+3, because it has three valence electrons.

+1, because in the ground state it has one unpaired electron.

+2, because it has two electrons in the 2s subshell.

+4, because it is in the fourth row of the periodic table.

A student obtains a sample of a pure solid compound. In addition to Avogadro's number, which of the following must the student know in order to determine how many molecules are in the sample.

molar mass of the compound and mass of the sample

molar mass of the compound and density of the sample

mass of the sample and the volume of the sample

mass of the sample and density of the sample

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

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

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

Which of the following is NOT directly determined by the principal quantum number, n, of the electron in an atom?

the shape of the corresponding atomic orbital(s)

the size of the corresponding atomic orbital(s)

the distance of the electron from the nucleus

Which of the following statements is FALSE?

The 3s orbital is held more tightly by the nucleus than the 2s orbital.

The spin quantum number of an electron must be either +½ or –½ .

In the usual order of filling, the 7s orbital is filled before the 5f orbital

An orbital can accommodate at most two electrons.

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. The difference best accounts for which of the following?

Na has a lower first ionization energy than Ne

Na has a greater density at standard condition than Ne

Na has a higher neutron to proton ratio than Ne

Na has a higher melting point that Ne

Strontium’s ionization energy is less than beryllium’s. This is accounted for because

strontium has more energy levels that beryllium

beryllium has a greater nuclear charge than strontium

strontium has a stronger Coulombic attraction than beryllium

strontium has more protons than beryllium

Examine the following isoelectronic series. K 1+ , P 3- , S 2- , Cl 1- You would expect

P 3- to be the largest because it has the least protons

P 3- to be the largest because it has the least electrons

P 3- to be the largest because it has the most electrons

P 3 - to be the smallest because it has the most protons

AP Chemistry Unit 1

Quiz

•

Chemistry

•

9th - 12th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-1, HS-PS1-7, HS-PS4-1

+6

Standards-aligned

Parker Drew

Used 6+ times

FREE Resource

80 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following numerical expressions gives the number of moles in 5.0g of CaO?

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

In a lab, a student is given a 21g sample of pure Cu metal. Which of the following pieces of information is most useful for determining the number of Cu atoms in the sample? Assume that the pressure and temperature in the lab are 1.0⁢atm and 25°C.

The molar mass of Cu

The density of Cu at 25°C

The volume of the Cu sample

The ratio of the two main isotopes found in pure Cu

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A 1.0⁢mol sample of which of the following compounds has the greatest mass?

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The mass spectrum for an unknown element is shown above. According to the information in the spectrum, the atomic mass of the unknown element is closest to

90 amu

91 amu

93 amu

94 amu

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The mass spectrum represented above is most consistent with which of the following elements?

Eu

Gd

Tb

Dy

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Based on the mass spectrum of a pure element represented above, the average atomic mass of the element is closest to which of the following?

185.7 amu

186.0 amu

186.3 amu

186.9 amu

A student obtains a 10.0g sample of a white powder labeled as BaCl₂. After completely dissolving the powder in 50.0mL of distilled water, the student adds excess Na₂SO₄(s), which causes a precipitate of BaSO₄(s) to form, as represented by the equation above. The student filters the BaSO₄(s), rinses it, and dries it until its mass is constant. Which of the following scientific questions could best be answered based on the results of the experiment?

Is the Na₂SO₄(s) used in the experiment pure?

Is the BaCl₂(s) used in the experiment pure?

What is the molar solubility of BaCl₂ in water?

What is the molar solubility of BaSO₄ in water?

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AP Chemistry Unit 1

80 questions

Which of the following numerical expressions gives the number of moles in 5.0g of CaO?

In a lab, a student is given a 21g sample of pure Cu metal. Which of the following pieces of information is most useful for determining the number of Cu atoms in the sample? Assume that the pressure and temperature in the lab are 1.0⁢atm and 25°C.

A 1.0⁢mol sample of which of the following compounds has the greatest mass?

The mass spectrum for an unknown element is shown above. According to the information in the spectrum, the atomic mass of the unknown element is closest to

The mass spectrum represented above is most consistent with which of the following elements?

Based on the mass spectrum of a pure element represented above, the average atomic mass of the element is closest to which of the following?

A 42.0g sample of compound containing only C and H was analyzed. The results showed that the sample contained 36.0g of C and 6.0g of H. Which of the following questions about the compound can be answered using the results of the analysis?

A jar labeled NaCl contains a powder. The table above contains information determined by analyzing a sample of the powder in the laboratory. What information in the table is the most helpful in determining whether the powder is pure NaCl?

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