Question 1

What information do boundary-surface representations of orbitals provide?

Accepted Answer

A) They enclose a region in which the probability of finding the electron is about 90%. 
B) They show the radial nodes in an orbital. 
C) They depict the path the electron takes over time. 
D) They are graphical solutions to the Schrödinger equation. 
E) They plot Ψ2 versus distance from the nucleus. 
A) They enclose a region in which the probability of finding the electron is about 90%. 
B) They show the radial nodes in an orbital. 
C) They depict the path the electron takes over time. 
D) They are graphical solutions to the Schrödinger equation. 
E) They plot Ψ2 versus distance from the nucleus.

Question 2

According to de Broglie's explanation of matter waves, if the circumference of the electron's orbit in the hydrogen atom is twice the electron's wavelength, the orbit will _______.

Accepted Answer

A) decay until the electron falls into the nucleus. 
B) diverge, allowing the electron to escape. 
C) be stable. 
D) cause the electron to emit a photon. 
E) not be circular. 
A) decay until the electron falls into the nucleus. 
B) diverge, allowing the electron to escape. 
C) be stable. 
D) cause the electron to emit a photon. 
E) not be circular.

Question 3

Calculate the de Broglie wavelength of an electron (9.11 * 10-31 kg) that is traveling at 0.100% of the speed of light.

Accepted Answer

A) 218 m 
B) 1.38 m 
C) 2.42 pm 
D) 2.42 nm 
E) 0.727 mm 
A) 218 m 
B) 1.38 m 
C) 2.42 pm 
D) 2.42 nm 
E) 0.727 mm

Question 4

A hydrogen atom is excited to ninitial = 8.A 955 nm photon is emitted as the electron falls to nfinal = _______.

Accepted Answer

A) 6 
B) 5 
C) 4 
D) 3 
E) 2 
A) 6 
B) 5 
C) 4 
D) 3 
E) 2

Question 5

Which statement regarding atomic emission spectra and the hydrogen atom is incorrect?

Accepted Answer

A) Electronic transitions in the atom are quantized. 
B) Discrete wavelengths of light can be absorbed or emitted by atoms. 
C) Atoms can absorb all wavelengths of light but only emit photons of discrete energies. 
D) Balmer proved that the hydrogen atom had a wavelike nature. 
E) Balmer and Rydberg developed empirical equations to fit experimental data. 
A) Electronic transitions in the atom are quantized. 
B) Discrete wavelengths of light can be absorbed or emitted by atoms. 
C) Atoms can absorb all wavelengths of light but only emit photons of discrete energies. 
D) Balmer proved that the hydrogen atom had a wavelike nature. 
E) Balmer and Rydberg developed empirical equations to fit experimental data.

Question 6

What is the orbital designation for an electron with the quantum numbers n = 3, $ l $ = 2?

Accepted Answer

A) 3s 
B) 3d 
C) 2p 
D) 2$ f $ 
E) 3e 
A) 3s 
B) 3d 
C) 2p 
D) 2$ f $ 
E) 3e

Question 7

In which orbital would an electron feel the highest effective nuclear charge?

Accepted Answer

A) 3s 
B) 4s 
C) 3p 
D) 4p 
E) 3d 
A) 3s 
B) 4s 
C) 3p 
D) 4p 
E) 3d

Question 8

Which arrangement is in the correct order of increasing radii?

Accepted Answer

A) Cs  Mn2+  Mn 
B) Ra   Li  Li+ 
C) P  P3-  AS3- 
D) Cr  Cr3+ Ca 
E) H  He+ 
A) Cs  Mn2+  Mn 
B) Ra   Li  Li+ 
C) P  P3-  AS3- 
D) Cr  Cr3+ Ca 
E) H  He+

Question 9

Calculate the de Broglie wavelength of an electron (9.11* 10-31 kg) moving at 99% of the speed of light.This is closest in size to which of the following (approximate dimensions are given): a proton (2 fm); a helium atom (60 pm); a bacterium (10 µm); a mosquito (1 mm); a baseball bat 1 m); a football field (100 m)?

Accepted Answer

2.45 *10<s

Question 10

What is the de Broglie wavelength of an electron (9.11 *10-31 kg) traveling at 95% of the speed of light?

Accepted Answer

A) 2.6 fm 
B) 2.6 pm 
C) 240 pm 
D) 24 fm 
E) 2.4 pm 
A) 2.6 fm 
B) 2.6 pm 
C) 240 pm 
D) 24 fm 
E) 2.4 pm

Question 11

Which of the following statements about the angular momentum quantum number, $ l $, is true?

Accepted Answer

A) It reflects the size of an orbital. 
B) It determines the energy of an orbital. 
C) Its value must be a positive integer. 
D) There are 2$ l $ + 1 orbitals in a subshell. 
E) Each value specifies the location of at most two electrons. 
A) It reflects the size of an orbital. 
B) It determines the energy of an orbital. 
C) Its value must be a positive integer. 
D) There are 2$ l $ + 1 orbitals in a subshell. 
E) Each value specifies the location of at most two electrons.

Question 12

Which statement about Rutherford's model of the atom is NOT correct?

Accepted Answer

A) It detailed the arrangement of electrons in the atom. 
B) It hypothesized that most of the mass of the atom is located in a very small region at the center of the atom called the nucleus. 
C) It did not explain some experimental findings, such as the photoelectric effect and the colors of light emitted by heated objects. 
D) It suggested that most of the atom is empty space. 
E) It suggested that the positive charge is not spread out over the atom's entire volume but rather is concentrated in the nucleus. 
A) It detailed the arrangement of electrons in the atom. 
B) It hypothesized that most of the mass of the atom is located in a very small region at the center of the atom called the nucleus. 
C) It did not explain some experimental findings, such as the photoelectric effect and the colors of light emitted by heated objects. 
D) It suggested that most of the atom is empty space. 
E) It suggested that the positive charge is not spread out over the atom's entire volume but rather is concentrated in the nucleus.

Question 13

What is the energy (E, in joules) of a 6.00 * 1010 Hz photon from a microwave oven?

Accepted Answer

A) 3.98 * 10-30 J 
B) 3.98 * 10-39 J 
C) 3.98 *10-23 J 
D) 3.98 * 10-17 J 
E) 3.98 * 10-13 J 
A) 3.98 * 10-30 J 
B) 3.98 * 10-39 J 
C) 3.98 *10-23 J 
D) 3.98 * 10-17 J 
E) 3.98 * 10-13 J

Question 14

Why is the electron not likely to be found at the nucleus?

Accepted Answer

A) The atom cannot emit enough energy to allow the electron to fall to such a low-energy state. 
B) As electrons approach the nucleus, they radiate energy and annihilate themselves. 
C) The electron is traveling too fast to approach the nucleus. 
D) The electron is repelled by the strong nuclear force. 
E) The volumes of the spherical shells very close to the nucleus are exceedingly small. 
A) The atom cannot emit enough energy to allow the electron to fall to such a low-energy state. 
B) As electrons approach the nucleus, they radiate energy and annihilate themselves. 
C) The electron is traveling too fast to approach the nucleus. 
D) The electron is repelled by the strong nuclear force. 
E) The volumes of the spherical shells very close to the nucleus are exceedingly small.

Question 15

The absorption and emission spectra of an atom and its ions) are different.This is evidence that the spectra observed are due to energy changes associated with the _______.

Accepted Answer

A) electrons. 
B) protons. 
C) neutrons. 
D) nuclei. 
E) electromagnetic interactions. 
A) electrons. 
B) protons. 
C) neutrons. 
D) nuclei. 
E) electromagnetic interactions.

Question 16

Which of the following species is NOT isoelectronic to the others?

Accepted Answer

A) Cl- 
B) Ar 
C) Mg2+ 
D) P3- 
E) SC3+ 
A) Cl- 
B) Ar 
C) Mg2+ 
D) P3- 
E) SC3+

Question 17

The first ionization energies of phosphorus and of sulfur are 1012 and 1000 kJ/mol.Why is IE1 for S lower than that of P when the usual trend is for IE to increase across a row?

Accepted Answer

A) Zeff decreases from left to right on the periodic table. 
B) Sulfur is smaller than phosphorus. 
C) More electrons in a subshell decrease orbital energy. 
D) An electron from phosphorus must be removed from a lower-energy subshell. 
E) Removing an electron from sulfur produces a half-filled subshell and reduces electron-electron repulsions. 
A) Zeff decreases from left to right on the periodic table. 
B) Sulfur is smaller than phosphorus. 
C) More electrons in a subshell decrease orbital energy. 
D) An electron from phosphorus must be removed from a lower-energy subshell. 
E) Removing an electron from sulfur produces a half-filled subshell and reduces electron-electron repulsions.

Question 18

How many unpaired electrons does CO3+ have?

Accepted Answer

A) 0 
B) 1 
C) 3 
D) 4 
E) 6 
A) 0 
B) 1 
C) 3 
D) 4 
E) 6

Question 19

Which of the following photons has the highest energy?

Accepted Answer

A) a photon with $\lambda$ = 1.064 µm 
B) a photon with $\nu$ = 5.83 * 1014 Hz 
C) a photon with $\lambda$ = 647 nm 
D) a photon with $\nu$ = 1.55 *1015 Hz 
E) a photon with $\lambda$= 633 pm 
A) a photon with $\lambda$ = 1.064 µm 
B) a photon with $\nu$ = 5.83 * 1014 Hz 
C) a photon with $\lambda$ = 647 nm 
D) a photon with $\nu$ = 1.55 *1015 Hz 
E) a photon with $\lambda$= 633 pm

Question 20

What is meant when two or more orbitals are said to be degenerate?

Accepted Answer

They have

Exam 3: Atomic Structure Explaining the Properties of Elements

What information do boundary-surface representations of orbitals provide?

According to de Broglie's explanation of matter waves, if the circumference of the electron's orbit in the hydrogen atom is twice the electron's wavelength, the orbit will _______.

Calculate the de Broglie wavelength of an electron (9.11 * 10-31 kg) that is traveling at 0.100% of the speed of light.

A hydrogen atom is excited to ninitial = 8.A 955 nm photon is emitted as the electron falls to nfinal = _______.

Which statement regarding atomic emission spectra and the hydrogen atom is incorrect?

What is the orbital designation for an electron with the quantum numbers n = 3, l l l = 2?

In which orbital would an electron feel the highest effective nuclear charge?

Which arrangement is in the correct order of increasing radii?

What is the de Broglie wavelength of an electron (9.11 *10-31 kg) traveling at 95% of the speed of light?

Which of the following statements about the angular momentum quantum number, l l l , is true?

Which statement about Rutherford's model of the atom is NOT correct?

What is the energy (E, in joules) of a 6.00 * 1010 Hz photon from a microwave oven?

Why is the electron not likely to be found at the nucleus?

The absorption and emission spectra of an atom and its ions) are different.This is evidence that the spectra observed are due to energy changes associated with the _______.

Which of the following species is NOT isoelectronic to the others?

The first ionization energies of phosphorus and of sulfur are 1012 and 1000 kJ/mol.Why is IE1 for S lower than that of P when the usual trend is for IE to increase across a row?

How many unpaired electrons does CO3+ have?

Which of the following photons has the highest energy?

What is meant when two or more orbitals are said to be degenerate?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

Calculate the de Broglie wavelength of an electron (9.11 * 10^-31 kg) that is traveling at 0.100% of the speed of light.

A hydrogen atom is excited to n_initial = 8.A 955 nm photon is emitted as the electron falls to n_final = _______.

What is the orbital designation for an electron with the quantum numbers n = 3, $l$ = 2?

What is the de Broglie wavelength of an electron (9.11 *10^-31kg) traveling at 95% of the speed of light?

Which of the following statements about the angular momentum quantum number, $l$ , is true?

What is the energy (E, in joules) of a 6.00 * 10¹⁰ Hz photon from a microwave oven?

The first ionization energies of phosphorus and of sulfur are 1012 and 1000 kJ/mol.Why is IE₁ for S lower than that of P when the usual trend is for IE to increase across a row?

How many unpaired electrons does CO³⁺ have?