Question 1

The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of these colors, ______ has the shortest wavelength.

Accepted Answer

The answer of The colors of the visible spectrum are...

Question 2

A ground-state atom of manganese has ___ unpaired electrons and is _____.

Accepted Answer

A) 0, diamagnetic 
B) 2, diamagnetic 
C) 3, paramagnetic 
D) 5, paramagnetic 
E) 7, paramagnetic 
A) 0, diamagnetic 
B) 2, diamagnetic 
C) 3, paramagnetic 
D) 5, paramagnetic 
E) 7, paramagnetic

Question 3

The electron configuration of a ground-state vanadium atom is

Accepted Answer

A) [Ar]4s24d3. 
B) [Ar]4s24p3. 
C) [Ar]4s23d3. 
D) [Ar]3d5. 
A) [Ar]4s24d3. 
B) [Ar]4s24p3. 
C) [Ar]4s23d3. 
D) [Ar]3d5.

Question 4

What is the difference in the electron configuration between carbon-14 and carbon-12?

Accepted Answer

There is n

Question 5

Which element has the following ground-state electron configuration? 1s22s22p63s2

Accepted Answer

A) Na 
B) Mg 
C) Al 
D) Si 
E) Ne 
A) Na 
B) Mg 
C) Al 
D) Si 
E) Ne

Question 6

How many electrons are there in the 2nd principal energy level (n = 2)of a phosphorus atom?

Accepted Answer

A) 3 
B) 5 
C) 6 
D) 8 
E) 10 
A) 3 
B) 5 
C) 6 
D) 8 
E) 10

Question 7

Calculate the energy of a photon of light with a wavelength of 360 nm.

Accepted Answer

5.5 * 10<s

Question 8

Which of the following atoms is paramagnetic both in its ground state and in all of its excited states?

Accepted Answer

A) C 
B) N 
C) O 
D) Ti 
E) Cr 
A) C 
B) N 
C) O 
D) Ti 
E) Cr

Question 9

With regard to electron behavior, what happens when light is absorbed or emitted by an atom?

Accepted Answer

The electr

Question 10

What is the wavelength of radiation that has a frequency of 5.39 * 1014 s-1? (c = 2.9979 * 108 m/s)

Accepted Answer

A) 1.80 * 10-3 nm 
B) 556 nm 
C) 618 nm 
D) 6180 nm 
E) 1.61 * 1023 nm 
A) 1.80 * 10-3 nm 
B) 556 nm 
C) 618 nm 
D) 6180 nm 
E) 1.61 * 1023 nm

Question 11

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

Accepted Answer

A) 2.07 * 10-29 J 
B) 2.19 * 105 J 
C) 2.04 * 10-18 J 
D) 3.27 * 10-17 J 
E) 2.25 * 10-18 J 
A) 2.07 * 10-29 J 
B) 2.19 * 105 J 
C) 2.04 * 10-18 J 
D) 3.27 * 10-17 J 
E) 2.25 * 10-18 J

Question 12

In the following diagram of a wave

Accepted Answer

A) (a)is amplitude and (b)is wavelength 
B) (a)is frequency and (b)is amplitude 
C) (a)is wavelength and (b)is frequency 
D) (a)is amplitude and (b)is frequency 
E) (a)is wavelength and (b)is amplitude 
A) (a)is amplitude and (b)is wavelength 
B) (a)is frequency and (b)is amplitude 
C) (a)is wavelength and (b)is frequency 
D) (a)is amplitude and (b)is frequency 
E) (a)is wavelength and (b)is amplitude

Question 13

What is the wavelength, in meters, of an alpha particle with a kinetic energy of 8.0 * 10-13 J? [mass of an alpha particle = 4.00150 amu; 1 amu = 1.67  * 10-27 kg]

Accepted Answer

6.4 * 10<s

Question 14

As the frequency of an electromagnetic wave increases

Accepted Answer

A) its speed must increase. 
B) its wavelength must increase. 
C) its amplitude must increase. 
D) its energy must increase. 
A) its speed must increase. 
B) its wavelength must increase. 
C) its amplitude must increase. 
D) its energy must increase.

Question 15

The bonds of oxygen molecules are broken by sunlight. The minimum energy required to break the oxygen-oxygen bond is 495 kJ/mol. What is the wavelength of sunlight that can cause this bond breakage?

Accepted Answer

The answer of The bonds of oxygen molecules are broken...

Question 16

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 *105 m/s. Calculate the binding energy of electrons to the magnesium surface.

Accepted Answer

A) 386 kJ/mol 
B) 419 kJ/mol 
C) 32.7 kJ/mol 
D) 321 kJ/mol 
E) 353 kJ/mol 
A) 386 kJ/mol 
B) 419 kJ/mol 
C) 32.7 kJ/mol 
D) 321 kJ/mol 
E) 353 kJ/mol

Question 17

A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If $\Delta$H for the reaction Cl2(g)$\rarr$ 2Cl(g)is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine atoms in solution?

Accepted Answer

A) 246.3 nm 
B) 465.2 nm 
C) 349.3 nm 
D) 698.6 nm 
E) 492.6 nm 
A) 246.3 nm 
B) 465.2 nm 
C) 349.3 nm 
D) 698.6 nm 
E) 492.6 nm

Question 18

Calculate the frequency of visible light having a wavelength of 686 nm.

Accepted Answer

A) 4.37 * 1014 /s 
B) 4.37 * 105 /s 
C) 6.17 * 1014 /s 
D) 2.29 * 10-15 /s 
E) 2.29 * 10-6 /s 
A) 4.37 * 1014 /s 
B) 4.37 * 105 /s 
C) 6.17 * 1014 /s 
D) 2.29 * 10-15 /s 
E) 2.29 * 10-6 /s

Question 19

If one electron is added to the outer shell of chlorine, it would have the same electron configuration as what element?

Accepted Answer

The answer of If one electron is added to the...

Question 20

Write the ground state electron configuration for a lead atom.

Accepted Answer

The answer of Write the ground state electron configuration for...

Exam 7: The Electronic Structure of Atoms

The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of these colors, ______ has the shortest wavelength.

A ground-state atom of manganese has ___ unpaired electrons and is _____.

The electron configuration of a ground-state vanadium atom is

What is the difference in the electron configuration between carbon-14 and carbon-12?

Which element has the following ground-state electron configuration? 1s22s22p63s2

How many electrons are there in the 2nd principal energy level (n = 2)of a phosphorus atom?

Calculate the energy of a photon of light with a wavelength of 360 nm.

Which of the following atoms is paramagnetic both in its ground state and in all of its excited states?

With regard to electron behavior, what happens when light is absorbed or emitted by an atom?

What is the wavelength of radiation that has a frequency of 5.39 * 1014 s-1? (c = 2.9979 * 108 m/s)

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

In the following diagram of a wave

What is the wavelength, in meters, of an alpha particle with a kinetic energy of 8.0 * 10-13 J? [mass of an alpha particle = 4.00150 amu; 1 amu = 1.67 * 10-27 kg]

As the frequency of an electromagnetic wave increases

The bonds of oxygen molecules are broken by sunlight. The minimum energy required to break the oxygen-oxygen bond is 495 kJ/mol. What is the wavelength of sunlight that can cause this bond breakage?

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 *105 m/s. Calculate the binding energy of electrons to the magnesium surface.

A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If Δ\DeltaΔ H for the reaction Cl2(g) →\rarr→ 2Cl(g)is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine atoms in solution?

Calculate the frequency of visible light having a wavelength of 686 nm.

If one electron is added to the outer shell of chlorine, it would have the same electron configuration as what element?

Write the ground state electron configuration for a lead atom.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

A ground-state atom of manganese has _ unpaired electrons and is ___.

Which element has the following ground-state electron configuration? 1s²2s²2p⁶3s²

What is the wavelength of radiation that has a frequency of 5.39 * 10¹⁴ s^-1? (c = 2.9979 * 10⁸ m/s)

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E_n = -2.18 * 10^-18 J(1/n²)

What is the wavelength, in meters, of an alpha particle with a kinetic energy of 8.0 * 10^-13 J? [mass of an alpha particle = 4.00150 amu; 1 amu = 1.67 * 10^-27 kg]

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 *10⁵ m/s. Calculate the binding energy of electrons to the magnesium surface.

A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If $\Delta$ H for the reaction Cl₂(g) $\rarr$ 2Cl(g)is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine atoms in solution?