Deck 4: Atoms and Light

Question 1

Understand some of the fundamental aspects of atoms.

Answer 1

Atoms have mass, contain positive nuclei, contain electrons, and occupy volume.

Question 2

Understand some of the fundamental aspects of light.

Answer 2

Light has wave-like and particle-like characteristics.

Question 3

Explain the origins of atomic spectra and relate electron energies in the hydrogen atom to its emission spectrum.

Answer 3

The energies of electrons in atoms are quantized.

Question 4

Describe properties of free electrons and those in atoms or molecules.

Question 5

Write valid sets of quantum numbers for a given set of orbitals.

Question 6

Recognize shapes of s, p, d, and f orbitals.

Question 7

Describe the major chemical reactions in the troposphere and stratosphere and explain the chemistry of the greenhouse effect.

Question 8

One of the characteristics of atoms is that they attract one another. What characteristic of gases supports this notion?

A) Equal numbers of molecules occupy equal volumes.
B) Gas molecules have a small, but definite volume.
C) The volume of a gas increases with increasing temperature.
D) Non-ideal behaviour is observed at low temperatures.
E) Volume decreases with increasing pressure.

Question 9

The volume of an atom is determined by

A) the number of protons in the nucleus.
B) the number of protons and neutrons in the nucleus.
C) the number of electrons in the nucleus.
D) the electron cloud surrounding the nucleus.
E) the period it occupies in the periodic table.

Question 10

The mass of an atom is determined by

A) the number of protons in the nucleus.
B) the number of protons and neutrons in the nucleus.
C) the number of electrons in the electron cloud surrounding the nucleus.
D) the number of neutrons and electrons.
E) the period it occupies in the periodic table.

Question 11

Most of the volume of an atom is made up of

A) electrons.
B) protons.
C) neutrons.
D) protons and neutrons.
E) empty space.

Question 12

When a gas such as argon condenses

A) atoms combine with one another to form chemical bonds.
B) atoms are attracted to one another due to electrical forces acting between electrons on one atom and protons of the other.
C) electrons of one atom repel those on another causing the gas to condense and form a liquid.
D) atoms are attracted to one another due to electrical forces acting between electrons on one atom and neutrons of the other.
E) atoms are attracted to one another due to electrical forces acting between neutrons on each of the atoms.

Question 13

Use the following equations for Questions
c = 3.0 x10⁸m/s = $\lambda$$\nu$ ;E = h $\nu$ ; h = 6.626 x 10^-34 J.s
E = h $\nu$ - h $\nu$ ₀; E = ½ mv² (KE of an electron) mass_e = 9.11 x 10^-31 kg

-Which of the following provides the greatest energy?

A) 5.00 x 10¹⁰ photons of frequency 1.00 x10⁹ 1/s
B) 7.00 x 10⁶ photons of wavelength 550 nm
C) 5.00 x 10⁵ photons of frequency 1.05 x 10¹⁴ 1/s
D) 7.20 x10⁸ photons of wavelength 200 nm
E) 5.00 x 10¹⁵ photons of wavelength 15 m

Question 14

Use the following equations for Questions
c = 3.0 x10⁸m/s = $\lambda$$\nu$ ;E = h $\nu$ ; h = 6.626 x 10^-34 J.s
E = h $\nu$ - h $\nu$ ₀; E = ½ mv² (KE of an electron) mass_e = 9.11 x 10^-31 kg

-Which of the following radiation is the most energetic?

A) radiation of wavelength 500 nm
B) radiation of frequency 5.76 x10¹⁴ Hz
C) radiation of frequency 8.25 x10¹⁴ Hz
D) radiation of wavelength 250 nm
E) cannot be determined based on the information given

Question 15

Use the following equations for Questions
c = 3.0 x10⁸m/s = $\lambda$$\nu$ ;E = h $\nu$ ; h = 6.626 x 10^-34 J.s
E = h $\nu$ - h $\nu$ ₀; E = ½ mv² (KE of an electron) mass_e = 9.11 x 10^-31 kg

-Sodium emits yellow light of wavelength 690nm when heated in a flame. What is the frequency of this light?

A) 2.07 x 10¹¹ s^-1
B) 4.35 x 10⁵ s^-1
C) 4.35 x10¹⁴ s^-1
D) 207 nm
E) 1.04 x 10¹⁴ s^-1

Question 16

Use the following equations for Questions
c = 3.0 x10⁸m/s = $\lambda$$\nu$ ;E = h $\nu$ ; h = 6.626 x 10^-34 J.s
E = h $\nu$ - h $\nu$ ₀; E = ½ mv² (KE of an electron) mass_e = 9.11 x 10^-31 kg

-Chromium metal has a binding energy of 7.21 x 10^-19J for certain electrons. What is the photon frequency needed to eject electrons with 2.2 x 10^-19J of energy?

A) 1.4 x 10¹⁵ s^-1
B) 2.4 x 10¹⁵ s^-1
C) 5.5 x 10¹⁵ s^-1
D) 1.2 x 10¹⁴ s^-1
E) 1.3 x 10¹⁶ s^-1

Question 17

Use the following equations for Questions
c = 3.0 x10⁸m/s = $\lambda$$\nu$ ;E = h $\nu$ ; h = 6.626 x 10^-34 J.s
E = h $\nu$ - h $\nu$ ₀; E = ½ mv² (KE of an electron) mass_e = 9.11 x 10^-31 kg

-Chromium metal, binding energy of 7.21 x 10^-19J for certain electrons, is subjected to a photon source of frequency 1.4 x 10¹⁵ s^-1. If the intensity of the photon source in increased, one would expect

A) the energy of the ejected electrons to increase.
B) the energy of the ejected electrons to decrease.
C) the number of ejected electrons to increase.
D) the number of ejected electrons to decrease.
E) no change.

Question 18

Use the following equations for Questions
;
E =
_n



-If a hydrogen atom is excited into the n = 4 state, how many transitions are possible by emitting electromagnetic radiation?

A) 1
B) 2
C) 3
D) 4
E) 5

Question 19

Use the following equations for Questions
;
E =
_n



-An electron in an H atom is excited to an energy level of -8.72 x 10^-20 J. What energy level does this correspond with?

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

Question 20

Use the following equations for Questions
;
E =
_n



-An excited electron on a hydrogen atom releases a photon as it falls from energy level 6 to level 3. What is the wavelength of the photon released?

A) 2.74 x10¹⁶ s^-1
B) 2.18 x10^-16 J
C) 1090 nm
D) 109 nm
E) 3 m

Question 21

Use the following equations for Questions
;
E =
_n



-An excited electron on a hydrogen atom releases a photon as it falls from energy level 6 to level 3. What is the change in energy of the atom and the energy of the photon released?

A) 1.1 x10⁵ J, 1.1x10⁵ J
B) -1.1x10⁵ J, 1.1x10⁵ J
C) 1.8x10^-19 J, 1.8x10^-19 J
D) -1.8x10^-19 J, -1.8x10^-19 J
E) -1.8x10^-19 J, 1.8x10^-19 J

Question 22

Use the following equations for Questions
;
E =
_n



-A hydrogen atom absorbs a photon resulting in an electron transitioning from the n = 2 to n = 5 energy level. What is the wavelength of the absorbed photon and what is the change in energy of the atom?

A) 434 $\mu$ m, 4.6x10^-19 J
B) 434 $\mu$ m, -4.6x10^-19 J
C) 434 nm, -4.6x10^-19 J
D) 434 nm, 4.6x10^-19 J
E) 6.9x10¹⁴ s^-1, 4.6x10^-19 J

Question 23

Use the following equations for Questions
E_kinetic = ½ mv²; mass_e = 9.11 x 10^-31kg;


-What is the wavelength of a proton (m = 1.67 x 10^-27 kg) moving at 1.2 x 10⁵ m/s?

A) 0.033 nm
B) 3.3 x 10^-2 nm
C) 3.3 x 10^-9 m
D) 3.3 x 10^-12 m
E) 3.3 nm

Question 24

Use the following equations for Questions
E_kinetic = ½ mv²; mass_e = 9.11 x 10^-31kg;


-The Heisenberg uncertainty principle

A) places limits on the accuracy of measuring both position and motion.
B) is most important for microscopic objects.
C) makes the idea of "orbits" for electrons meaningless.
D) a, b
E) a, b and c

Question 25

Use the following equations for Questions
E_kinetic = ½ mv²; mass_e = 9.11 x 10^-31kg;


-Which of the following objects would we expect NOT to have any meaningful wave properties?

A) electrons
B) protons
C) neutrons
D) a mole of carbon atoms
E) photons

Question 26

Use the following equations for Questions
E_n =


-Which of the following set of quantum numbers is NOT possible?

A) n =2, l = 1, m_l = 0, m_s =1/2
B) n =3, l = 2, m_l = 2, m_s =1/2
C) n =4, l = 2, m_l = 2, m_s = -1/2
D) n =3, l = 3, m_l = 2, m_s = -1/2
E) n = 2, l = 1, m_l = 1, m_s = -1/2

Question 27

Use the following equations for Questions
E_n =


-Which of the following set of quantum numbers is possible?

A) n =2, l = 0, m_l = 1, m_s =1/2
B) n =3, l = 3, m_l = 2, m_s =1/2
C) n =4, l = 3, m_l = 3, m_s = -1/2
D) n =3, l = 3, m_l = 2, m_s = -1/2
E) n = 2, l = 1, m_l = 2, m_s = -1/2

Question 28

Use the following equations for Questions
E_n =


-Which of the following sets of quantum numbers is valid for an electron in a 4d orbital?

A) n =4, l=1, m_l=1, m_s =1/2
B) n =4, l=2, m_l=3, m_s = -1/2
C) n =4, l=3, m_l=2, m_s =1/2
D) n =4, l=2, m_l=1, m_s = -1/2
E) n =4, l=0, m_l=0, m_s = -1/2

Question 29

Use the following equations for Questions
E_n =


-Which of the following sets of quantum numbers is valid for an electron in a 4f orbital?

A) n =4, l=1, m_l=1, m_s =1/2
B) n =4, l=3, m_l=4, m_s = -1/2
C) n =4, l=3, m_l=2, m_s =1/2
D) n =4, l=2, m_l=1, m_s = -1/2
E) n =4, l=4, m_l=1, m_s = 1/2

Question 30

Use the following equations for Questions
E_n =


-An electron in an H atom is excited to an energy of -8.72 x 10^-20 J which corresponds to a primary level 5. What is the largest value of m_l possible for this energy level?

A) 3
B) 4
C) 5
D) 6
E) 9

Question 31

Use the following equations for Questions
E_n =


-An electron in an H atom is excited to an energy of -8.72 x 10^-20 J which corresponds to a primary level 5. How many possible m_l values are there for this energy level?

A) 4
B) 18
C) 5
D) 11
E) 9

Question 32

Use the following equations for Questions
E_n =


-An electron in an H atom is excited to an energy of -2.42 x 10^-19 J. What is the largest value of m_l possible for this energy level?

A) 1
B) 2
C) 3
D) 0
E) 7

Question 33

Use the following equations for Questions
E_n =


-The magnetic quantum number

A) is always less than the value of l.
B) is always less than n.
C) is always greater than m_s.
D) correlates strongly with the energy of the electron.
E) must be a positive number.

Question 34

Use the following equations for Questions
E_n =


-The principle quantum number for the outermost 2 electrons in Sr would be

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

Question 35

Use the following equations for Questions
E_n =


-The principle quantum number for the 3 outermost electrons in Sc are

A) 3, 3 and 3.
B) 4, 4 and 3.
C) 4, 4 and 4.
D) 3, 3, and 4.
E) 4, 4, and 5.

Question 36

Use the following equations for Questions
E_n =


-The azimuthal quantum number for the outermost electron on K is

A) 0.
B) 1.
C) 2.
D) 3.
E) 4.

Question 37

How many nodes are there in a 3p orbital?

A) 0
B) 1
C) 2
D) 3
E) 4

Question 38

An electron in which subshell will, on average, be closer to the nucleus of an atom?

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

Question 39

Which atom has a smaller 3s orbital?

A) an atom with more protons
B) an atom with fewer protons
C) an atom with more neutrons
D) an atom with fewer neutrons
E) the size of the 3s orbital is the same for all atoms.

Question 40

How many orbitals are there in the d sublevel?

A) 1
B) 3
C) 5
D) 6
E) 7

Question 41

The quantum numbers that correspond to size and orientation of orbitals are

A) principal and azimuthal.
B) principal and magnetic.
C) azimuthal and magnetic.
D) n and l.
E) azimuthal and spin.

Question 42

What wavelength photons are required to "split" molecular O₂ into O atoms?

A) microwave region of wavelengths
B) infrared region of wavelengths
C) 280-320 nm
D) 240-280 nm
E) 180-220 nm

Question 43

What is the main reason for CO₂'s significant participation in global warming?

A) its high concentration
B) its rapid destruction in the atmosphere
C) its efficiency in absorbing visible light
D) its slow uptake into the biosphere
E) its efficiency in absorbing infrared light

Question 44

Which of the following reactions is NOT predominant in the thermosphere?

A) N₂ +h $\upsilon$ $\rarr$ N₂⁺
B) O₂ + h $\upsilon$ $\rarr$ 2 O
C) CO + 1/2 O (\rarr\) CO₂
D) 2 O $\rarr$ O₂ + heat
E) N₂⁺ $\rarr$ N₂ + heat

Question 45

The temperature at the last ice age was how much different than today's average temperature?

A) It was the same on average.
B) 3° to 8° C warmer
C) 3° to 8° C colder
D) 10° to 20°C colder
E) 20° to 30°C colder

Question 46

There are a number of layers in the atmosphere where oxygen molecules are broken into atoms that can combine with other O₂ molecules to make ozone (O₃). Why is it that there is only a specific region/layer where ozone is made in any significant amount?

A) The reaction is faster at higher altitudes.
B) The concentration of O₂ is not large enough at higher altitudes.
C) The energy from the sun is not strong enough at higher altitudes.
D) The molecules cannot breathe at higher altitudes.
E) The reaction is slow at higher altitudes.

Question 47

How would you explain to a friend the size of the nucleus of an atom versus the size of the entire atom?

Question 48

How many electrons are present in 8.0 grams of He?

Question 49

How many protons are in 3.5 moles of carbon atoms?

Question 50

The density of lead is 11.34 g/cm³; if the lead nucleus is 1/100 000 times that of the atom, determine the density of the nucleus.

Question 51

The density of gold is 19.3 g cm^-3. Determine the radius of a single gold atom.

Question 52

Magnesium has a binding energy of 258.6 kJ/mole. If filtered light from a mercury lamp with wavelength 383 nm is absorbed by magnesium metal, what is the maximum kinetic energy of electrons observed?

Question 53

Platinum is a quite inert metal used in many ways, recently popular in jewelry. It has a binding energy of 513 kJ/mole. What is the longest wavelength of electromagnetic radiation possible that will have enough energy to eject photoelectrons from a platinum atom?

Question 54

Lasers are commonly used to mark and cut metals with high precision. One industrial laser is the neodymium-YAG laser that produces laser light of wavelength 1065 nm. If you want to vaporize 50 mg of Pt, which requires about 250 J of energy, how many photons of YAG laser light are needed?

Question 55

The ruby laser contains chromium (III) ions in Al2O3. It is the Cr(III) ion that emits light of 627 nm under the laser emission conditions. If a ruby contains 0.0010% Cr by mass, what is the minimum mass of a ruby (in g) required to produce a single pulse with energy 1.5 J?

Question 56

A glass filled with water absorbs 2.5 x 10²⁰ photons of wavelength 1500 nm. How much energy is transferred to the water?

Question 57

An electron on a hydrogen atom in the outer atmosphere of a star can be excited to very high quantum numbers. What is the wavelength of light emitted when a hydrogen atom undergoes a transition from n = 1000 to n = 999?

Question 58

Hydrogen atoms are present for fleeting amounts of time in combustion processes. They can be observed by monitoring the amount of light absorbed at the wavelength corresponding to the n = 2 to n = 3 transition. What is the wavelength of this electromagnetic radiation and in what region of the spectrum does it lie?

Question 59

The energy levels of the dication of lithium, Li²⁺, are described by a modified Bohr equation; all energy levels are nine times those of the H atom. What is the wavelength (in nm) emitted by n Li²⁺ ion going from the n = 5 to n = 4 energy level?

Question 60

A number of scientists, when they saw the hydrogen gas emission lines, thought that the electrons in the hydrogen atom could have any energy and that they were only seeing a few of those energies. How did Bohr interpret these emission lines and why was this a new or unique interpretation?

Question 61

Show the path of an electron on an atom as it absorbs energy going from energy level 1 to level 6 and then releasing energy (as a photon) to fall to energy level 3. Be sure to show the relative differences in energy of the levels.

Question 62

The photoelectric effect experiment is performed on strontium metal. When light with ? = 389 nm shines on the metal, electrons are ejected at a velocity of 3.97 x 10⁵ m/s. What is the threshold frequency, $\nu$ _o, for strontium metal?

Question 63

What is the wavelength of electrons moving at 1.5 x10⁶ m/s (about 0.5% the speed of light)?

Question 64

What is the kinetic energy in kJ/mole of electrons with a wavelength of 0.22 nm (the distance between some atoms)?

Question 65

What is the wavelength of electrons with kinetic energy 95 kJ/mole?

Question 66

At what velocity would an electron need to travel at to have a wavelength of 0.1 nm?

Question 67

An electron has velocity of 3 x 10² m s^-1; determine the wavelength and frequency of this electron.

Question 68

One wavelength of infrared radiation absorbed by water is 3150 nm. At what velocity will electrons have this wavelength?

Question 69

List the possible values of m_l for an electron in a 3p subshell.

Question 70

List the possible values for l for an electron in the 4^th principle quantum level.

Question 71

List all possible quantum sets for an electron in the 4p quantum level.

Question 72

Atomic orbitals on different atoms can interact with each other, with different results. For now, consider two atoms, A and X. Draw contour pictures of the interaction of the 2s orbital on A with the 2p orbital on X, with the preferred axis of the p orbital (one of the lobes) pointing at the s orbital.

Question 73

Atomic orbitals on different atoms can interact with each other, with different results. For now, consider two atoms, A and X. Draw contour pictures of the 2p orbital on A and the 2p orbital on X where the preferred axes are parallel (a side-by-side interaction).

Question 74

Which of the following pictures shows the appropriate number of nodes for a 3d orbital?

Question 75

Which of the following is a view of the d_xy orbital from the z axis?

Question 76

Please define what a node is and how many would be found in a 4p orbital.

Question 77

The energy required to convert O₂ molecules to O atoms is 496 kJ/mole. If electromagnetic radiation of 180 nm is absorbed by 1 mole of O₂ molecules, how much kinetic energy will be present in the O atoms?

Question 78

Draw a molecular picture illustrating the decomposition of O₃ to O₂ + O in the stratosphere.

Question 79

The bond energy for molecular oxygen, O₂, is 495 kJ/mol; the maximum wavelength of light capable of fragmenting the ozone molecule is 340 nm. What is the difference between the bond energies of O₂ and O_3?

Question 80

The bond energy for molecular oxygen, O₂, is 495 kJ/mol and differs from that of O₃ by 145 kJ mol^-1; what is the maximum wavelength of light capable of fragmenting the ozone molecule?