Chemistry Chapter 7.2

The second line of the Balmer series occurs at a wavelength of 486.1 nm. What is the energy difference between the initial and final levels of the hydrogen atom in this emission process? A) 2.44 × 1018 J D) 4.09 × 10-28 J B) 4.09 × 10-19 J E) 1.07 × 10-48 J C) 4.09 × 10-22 J

B) 4.09 × 10^-19 J e=HC/A (6.63 x 10^-34j)(3.00 x10^8)/486.1 x 10^-9m = 4.09 x 10^-19j http://www.bama.ua.edu/~blacksto/CH101/exams_quizzes/quiz6_key.pdf

What is the maximum number of electrons in an atom that can have the following quantum numbers? n = 3 l = 1 A) 18 B) 6 C) 3 D) 2 E) 1

B) 6

section 7.9 A possible set of quantum numbers for the last electron added to complete an atom of gallium (Ga) in its ground state is A) A B) B C) C D) D E) E

C) C

Which element has the following ground-state electron configuration? [Xe]6s24f145d10 A) Lu B) Cd C) Hg D) Lr E) Au

C) Hg

List the following sets of quantum numbers in order of increasing energy: I. n = 4, l = 0, ml = 0, ms = -1/2 II. n = 4, l = 2, ml = -1, ms = -1/2 III. n = 5, l = 0, ml = 0, ms = +1/2 A) I < II < III B) II < III < I C) III < II < I D) I < III < II E) III < I < II

D) I < III < II

Which of the following is the electron configuration of an excited state of an iron atom? A) [Ar]4s23d7 B) [Ar]4s23d6 C) [Ar]4s23d8 D) [Ar]4s13d7 E) [Ar]4s13d5

D) [Ar]4s13d7

Lanthanide (or rare earth elements) have atoms or ions with partially filled A) s subshells. D) f subshells. B) p subshells. E) g subshells. C) d subshells

D) f subshells

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = -2.18 × 10 -18 J(1/n2) A) 1.35 × 10-51 /s D) 8.22 × 1014 /s B) 1.03 × 108 /s E) 3.08 × 10^15 /s C) 2.06 × 1014 /s

E) 3.08 × 10^15 /s -2.18 x 10^-18 (1/4^2-1/1^2) =2.04^-18/6.63^-34 =3.08^15 ^=E/H

A ground-state chromium atom has how many unpaired electrons? A) 1 B) 2 C) 4 D) 5 E) 6

E) 6

Which ground-state atom has an electron configuration described by the following orbital diagram? A) antimony B) germanium C) indium D) lead E) tin

E) tin

The orbital diagram for a ground-state nitrogen atom is A) A B) B C) C D) D see chart

A

Calculate the frequency of visible light having a wavelength of 686 nm. A) 4.37 × 10^14 /s D) 2.29 × 10^-15 /s B) 4.37 × 105 /s E) 2.29 × 10^-6 /s C) 6.17 × 10^14 /s

A) 4.37 × 10^14 /s 3x10 ^8/686 x 10^-9)

When the electron in a hydrogen atom falls from the n = 3 excited energy level to the ground state energy level, a photon with wavelength l is emitted. An electron having this same wavelength would have a velocity of A) 7.10 × 10^3 m/s D) 7.10 m/s B) 2.93 × 106 m/s E) 3.00 × 108 m/s C) 2.93 × 103 m/s

A) 7.10 × 10^3 m/s

Which of the following atoms is diamagnetic in its ground-state? A) Ca B) As C) Cu D) Fe E) none of these

A) Ca

Which of the following electronic transitions is consistent with an increase in energy? A) From a 4s subshell to a 3d subshell D) From a 4f subshell to a 6s subshell B) From a 5p subshell to a 4d subshell E) From a 5d subshell to a 6s subshell C) From a 4d subshell to a 5s subshell

A) From a 4s subshell to a 3d subshell

Which element has the following ground-state electron configuration? [Xe]6s24f145d4 A) W B) Pm C) Mo D) Np E) Re

A) W

The electron configuration of a ground-state Co atom is A) [Ar]4s23d7 D) [Ar]4s13d5 B) 1s22s22p63s23d9 E) [Ar]4s24d7 C) [Ne]3s23d7

A) [Ar]4s23d7

Which of the following is the electron configuration of an excited state of a copper atom? A) [Ar]4s23d9 D) [Ar]4s23d8 B) [Ar]4s13d10 E) [Ar]4s03d10 C) [Ar]4s13d8

A) [Ar]4s23d9

The ground-state electron configuration of Cr, Mo, and Ag are exceptions to the Aufbau principle. Which of the following is the electron configuration for Mo? A) [Kr]5s14d5 B) [Kr]5s24d4 C) [Xe]6s25d4 D) [Ar]4s24d4 E) [Kr]5s24d6

A) [Kr]5s14d5

Which ground-state atom has an electron configuration described by the following orbital diagram? A) phosphorus B) nitrogen C) arsenic D) vanadium E) none of these

A) phosphorus

"No two electrons in an atom can have the same four quantum numbers" is a statement of A) the Pauli exclusion principle. D) de Broglie's relation. B) Bohr's equation. E) Dalton's atomic theory. C) Hund's rule

A) the Pauli exclusion principle.

If a hydrogen atom and a helium atom are traveling at the same speed, A) the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom. B) the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium. C) the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom. D) the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom. E) the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

A) the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.

7.1 1. In the following diagram of a wave A) (a) is amplitude and (b) is wavelength D) (a) is amplitude and (b) is frequency B) (a) is frequency and (b) is amplitude E) (a) is wavelength and (b) is amplitude C) (a) is wavelength and (b) is frequency Ans: E Category: Easy Section: 7.1

Ans: E Category: Easy Section: E) (a) is wavelength and (b) is amplitude

Which one of the following sets of quantum numbers is not possible? A) A B) B C) C D) D E) E

B

section 7.5 Which one of the following sets of quantum numbers is not possible? A) A B) B C) C D) D E) E

B

A possible set of quantum numbers to describe an electron in a 4s subshell is A) n = 4, l = 0, ml = 1 , ms = +1/2 D) n = 3, l = 1, ml = 1, ms = - 1/2 B) n = 4, l = 0, ml = 0, ms = - 1/2 E) n = 3, l = 0, ml = 0, ms = +1/2 C) n = 4, l = 1, ml = 1, ms = +1/2

B) n = 4, l = 0, ml = 0, ms = - 1/2

In an electron microscope, electrons are accelerated to great velocities. Calculate the wavelength of an electron traveling with a velocity of 7.0 × 103 kilometers per second. The mass of an electron is 9.1 × 10-28 g. A) 1.0 × 10-13 m B) 1.0 × 10-10 m C) 1.0 × 10-7 m D) 1.0 m 1 gram=0.001 kg 1kilometer=1000 meter

B) 1.0 × 10^-10 m A= h/mu 6.63 x 10^-34kg/(9.1 10^-31kg)(7.0x10^6m/s)

What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 × 10^2 nm? A) 4.72 × 10-43 J B) 1.71 × 105 J C) 12.4 kJ D) 256 kJ E) 2.12 × 1042 J

B) 1.71 × 10^5 J Energy = Planck constant*frequency*Avogadro constant frequency = 3*10^8 (m/s)/ 7*10^-7 m = 0,42857*10^15 Hz E = = 6,626*10^-34 Js * 0,42857*10^15 Hz * 6,022*10^23 E = 17,1*10^4 J

section 7.8 What is the maximum number of electrons in an atom that can have the following quantum numbers? n = 3 l = 2 A) 18 B) 10 C) 5 D) 2 E) 1

B) 10

What is the wavelength of radiation that has a frequency of 5.39 × 10^14 s-1? (c = 2.9979 ×10^8 m/s) A) 1.80 × 10-3 nm B) 556 nm C) 618 nm D) 6180 nm E) 1.61 × 1023 nm

B) 556 nm Wave equation: wavelength (greek letter lambda) x frequency = speed of light So wavelength = speed of light / frequency wavelength = 3.00 x 10^8 / 5.39 x 10^5 = 556 nm

What is the wavelength of radiation that has a frequency of 3.4 x 10^11 s -1? A) 8.8 x 10-4 nm D) 1.0 x 1011 nm B) 8.8 x 10^5 nm E) 1.0 x 10-9 nm C) 8.8 x 10-13 nm

B) 8.8 x 10^5 nm 3.00 x 10^8 /3.4 x 10^2=8.8x10^5 when your converting meters to nanometers your adding the exponents 11 minus - 9=2 wavelength = speed of light / frequency

Which choice lists two elements with ground-state electron configurations that are well known exceptions to the Aufbau principle? A) Cu and C B) Cr and Cu C) Cs and Cl D) Rb and Co E) Fe and C

B) Cr and Cu

Which of the following electronic transitions is consistent with a decrease in energy? A) From a 5s subshell to a 4d subshell D) From a 5s subshell to a 5p subshell B) From a 4f subshell to a 5p subshell E) From a 4f subshell to a 6p subshell C) From a 6s subshell to a 5d subshell

B) From a 4f subshell to a 5p subshell

Which element has the following ground-state electron configuration? 1s22s22p63s2 A) Na B) Mg C) Al D) Si E) Ne

B) Mg

Which element has the following ground-state electron configuration? [Kr]5s14d5 A) Mn B) Mo C) Nb D) Re E) Tc

B) Mo

Which of the following atoms is paramagnetic both in its ground state and in all of its excited states? A) C B) N C) O D) Ti E) Cr

B) N

Which element has the following ground-state electron configuration? [Kr]5s24d105p3 A) Sn B) Sb C) Pb D) Bi E) Te

B) Sb

Using the figure below, categorize electromagnetic radiation with an energy of 6.6 x 10-16 J/photon. A) Gamma rays B) X rays C) Ultraviolet D) Infrared E) Microwave

B) X rays

Which element has the following ground-state electron configuration? [Ar]4s23d104p5 A) aresnic B) bromine C) iodine D) selenium E) tellerium

B) bromine

53. Electrons in an orbital with l = 3 are in a/an A) d orbital. B) f orbital. C) g orbital. D) p orbital. E) s orbital.

B) f orbital Basically, when l = 0 the is one orbital and it is called an s-orbital. It can hold 2 electrons total. When l = 1, the orbitals are called p-orbitals and there are 3 of them. Each of the individual p-orbitals can hold 2 electrons each. This gives us a total of 6 electrons that can go into the 3 p-orbitals. When l = 2, the orbitals are called d-orbitals and there are 5 of them. Each of the individual d-orbitals can hold 2 electrons each. This gives a total of 10 electrons that can go into the 5 d-orbitals. When l = 3, the orbitals are called f-orbitals and there are 7 of them. Each of the individual f-orbitals can hold 2 electrons each. This gives a total of 14 electrons that can go into the 7 f-orbitals.

If a hydrogen atom and a helium atom have the same kinetic energy, A) the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom. B) the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium. C) the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom. D) the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom. E) the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

B) the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.

A possible set of quantum numbers to describe an electron in a 3d subshell is A) n = 3, l = 0, ml = 0 , ms = +1/2 D) n = 3, l = 3, ml = 1, ms = - 1/2 B) n = 3, l = 1, ml = 0, ms = - 1/2 E) n = 2, l = 0, ml = 0, ms = +1/2 C) n = 3, l = 2, ml = 1, ms = +1/2

C) n = 3, l = 2, ml = 1, ms = +1/2

What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m? (c = 2.9979 × 10^8 m/s; h = 6.626 × 10-34 J×s) A) 2.70 × 10-43 J D) 4.07 × 10-10 J B) 5.43 × 10-33 J E) 2.46 × 109 J C) 1.63 × 10-24 J

C) 1.63 × 10^-24 J E=H*C/wavelength (6.626 x10^-34)(3.00x10^8)(1000)/ 0.122 planks constant =h =6.63 x 10^-34 Speed of light=c=3 x 10^8 ^=wavelength E=H(C)/^

Which of the following is the electron configuration of an excited state of an oxygen atom?

C) 1s22s22p33s1

How many unpaired electrons does an atom of carbon have in its ground state? A) 0 B) 1 C) 2 D) 3 E) 4

C) 2 C has two unpaired electrons in its ground state. The ground-state electron configuration of P is [Ne]3s23p3. The 3s subshell contains one orbital (ml=0), which holds two spin-paired electrons; this subshell is full. The 4p subshell contains three orbitals (ml=-1, 0, 1). https://www.google.com/?gws_rd=ssl#q=How+many+unpaired+electrons+does+an+atom+of+carbon+have+in+its+ground+state%3F

How many unpaired electrons does an atom of sulfur have in its ground state? A) 0 B) 1 C) 2 D) 3 E) 4

C) 2 It has 2 unpaired electrons 3s2 3p4 , which means it has 3 orbitals in the the p subshell, each orbital can hold two electrons, Hunds rule tells us to put one electron in each orbital first and then we can fill up the orbitals. So if there are 4 electrons in the p subshell, the three orbitals will get one electron in each first, then the fourth electron will be paired with a lone electron in one of the orbitals, leaving 2 electrons unpaired/alone.

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

C) 2.04 × 10-18 J Energy needed = 2.18 . 10^-18 . (1/4^2 1/1^2 - ) = 2.04 . 10^-18 J E=-2.18 × 10^-18J x(final-inital) see que 7.31 in notes

A ground-state atom of vanadium has ___ unpaired electrons and is _____. A) 0, diamagnetic D) 5, paramagnetic B) 2, diamagnetic E) 4, diamagnetic C) 3, paramagnetic

C) 3, paramagnetic

7.2 Which of the following wavelengths of electromagnetic radiation has the highest energy? A) 450. nm D) 8.40 x 10-7 m B) 225 nm E) 2.50 x 10-5 m C) 3.50 x 10-9 m

C) 3.50 x 10-9 m

How many orbitals are allowed in a subshell if l = 2? A) 1 B) 3 C) 5 D) 7 E) 9

C) 5

Calculate the frequency of visible light having a wavelength of 486 nm. A) 2.06 × 1014 /s D) 1.20 × 10-15 /s B) 2.06 × 106 /s E) 4.86 × 10-7 /s C) 6.17 × 10^14 /s 1 nanometer = 1.0 × 10-9 meters

C) 6.17 × 10^14 /s frequency = velocity /wave length (3.0 x 10^8 m/s) / (486 x 10^-9 m) = 6.17 × 10^14 sec^-1 = 6.17 × 10^14 Hz

A possible set of quantum numbers for the last electron added to complete an atom of germanium (Ge) in its ground state is A) A B) B C) C D) D E) E

C) C

List the following sets of quantum numbers in order of increasing energy: I. n = 4, l = 1, ml = 1, ms = +1/2 II. n = 3, l = 2, ml = -1, ms = +1/2 III. n = 4, l = 0, ml = 0, ms = +1/2 A) I < II < III B) II < III < I C) III < II < I D) I < III < II E) III < I < II

C) III < II < I

Using the figure below, categorize electromagnetic radiation with an energy of 6.7 x 10-18 J/photon. A) Gamma rays B) X rays C) Ultraviolet D) Infrared E) Microwave

C) Ultraviolet

72. The electron configuration of a ground-state vanadium atom is A) [Ar]4s24d3 B) [Ar]4s24p3 C) [Ar]4s23d3 D) [Ar]3d5

C) [Ar]4s23d3

Which of the following is the ground-state electron configuration of Ir? A) [Xe]6s25d7 D) [Xe]6s25f146d7 B) [Xe]6s26d7 E) [Xe]4s25f146d7 C) [Xe]6s24f145d7

C) [Xe]6s24f145d7

Transition metal elements have atoms or ions with partially filled A) s subshells. D) f subshells. B) p subshells. E) g subshells. C) d subshells

C) d subshells

Which ground-state atom has an electron configuration described by the following orbital diagram? A) phosphorus B) germanium C) selenium D) tellurium E) none of these

C) selenium

The orbital diagram for a ground state carbon atom is A) A B) B C) C D) D

D

The orbital diagram for a ground-state oxygen atom is A) A B) B C) C D) D E) E

D

Calculate the wavelength associated with a 20^Ne+ ion moving at a velocity of 2.0 × 10^5 m/s. The atomic mass of 20Ne is 19.992 amu. A) 1.7 x 10-40 m D) 1.0 × 10-13 m B) 1.0 × 10-18 m E) 9.7 × 1012 m C) 1.0 × 10-16 m

D) 1.0 × 10^-13 m

Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 × 10-24 g) A) 1.6 pm B) 0.016 nm C) 0.16 nm D) 160 nm E) 1.6 × 10-4 m 250 cm= 2.5

D) 160 nm Using the de Broglie analogy λ =h/mv (particles with mass m, moving with velocity v .. behave in some ways like waves) • λ = (6.63 × 10-34) /{(1.675*10^-24)(0.25m/s)} ... ► = 1.58*10^-9 m

What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 3 l = 1 ml = -1 A) 18 B) 6 C) 3 D) 2 E) 1

D) 2

What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 3 l = 2 ml = -2 A) 18 B) 10 C) 5 D) 2 E) 1

D) 2

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 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/n En = -2.18 × 10-18 J(1/n2) A) 9.18 × 10-20 nm D) 2.16 × 103 nm B) 4.45 × 10-20 nm E) 1.38 × 1014 nm C) 2.16 × 10-6 nm Chttp://www.profpaz.com/id1.html

D) 2.16 × 10^3 nm -(2.18x10^-18)(1/4^2-1/7^2) =-9.17x10^-20 (6.63x10^34)(3.00x10^8)/(-9.17x10^-20) =-2.16x10^-6/10^-9=2.16x10^3 wavelength = hc/E =2.16x10^3nm

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = -2.18 × 10-18 J(1/n2). A) 1.82 × 10-19 /s D) 3.65 × 1014 /s B) 9.13 × 1013 /s E) 1.64 × 1015 /s C) 2.74 × 1014/s

D) 3.65 × 1014 /s -2.18x10^-18(1/6^2-1/3^2) =1.8166^-19 6.63x10^-34/1.816x10^-20= 3.65x10^14

A ground-state atom of manganese has ___ unpaired electrons and is _____. A) 0, diamagnetic D) 5, paramagnetic B) 2, diamagnetic E) 7, paramagnetic C) 3, paramagnetic

D) 5, paramagnetic

How many orbitals are allowed in a subshell if l = 3? A) 1 B) 3 C) 5 D) 7 E) 9

D) 7

Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = -2.18 × 10-18 J(1/n2) A) 6.8 × 10-18 nm B) 0.612 nm C) 82.6 nm D) 97.2 nm E) 365 nm

D) 97.2 nm 2.18x10^-18(1/4^2-1/1^2) =2.04x10^-18 E=2.04x10^-18 (6.63x10^-34)(3x10^8/(2.04x10^-18) =9.74x10^-8m 9.74x10^-8m/10^-9=97.4 http://facstaff.gpc.edu/~gnomura/1211/1211200708Exam3.pdf

What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 × 10^14 /s? A) 2.75 × 10-43 J/mol D) 99.7 kJ/mol B) 1.66 × 10-19 J/mol E) 7.22 × 1017 kJ/mol C) 1.20 × 10-6 J/mol

D) 99.7 kJ/mol The photon energy necessary to eject electrons from the metal is called the theshold energy - at the threshold frequency. The energy is given by (Planck's constant)×(frequency): E = hν = (6.63 × 10^-34 J•s)( 2.50 × 10^14 /s) = 1.6565 × 10^-19 J => (1.6565 × 10^-19 J)(6.022 × 10^23 /mol)(10^-3 kJ/J) = 99.756 kJ/mol

Which one of the following sets of quantum numbers represents an electron with the highest energy? A) n = 2, l = 1, ml = 0, ms = +1/2 D) n = 3, l = 2, ml = 1, ms = -1/2 B) n = 3, l = 0, ml = 0, ms = -1/2 E) n = 3, l = 1, ml = 1, ms = +1/2 C) n = 2, l = 0, ml = 0, ms = +1/2

D) n = 3, l = 2, ml = 1, ms = -1/2

A photon is roughly 1800 times more massive than an electron. If a proton and an electron have the same kinetic energy, A) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. B) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. C) the wavelength of the photon will be roughly equal to the wavelength of the electron. D) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon. E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon

D) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon.

A possible set of quantum numbers to describe an electron in a 5p subshell is A) n = 5, l = 2, ml = 2 , ms = +1/2 B) n = 4, l = 0, ml = 0, ms = - 1/2 C) n = 5, l = 0, ml = 0, ms = +1/2 D) n = 3, l = 1, ml = 1, ms = - 1/2 E) n = 5, l = 1, ml = 0, ms = +1/2

E) n = 5, l = 1, ml = 0, ms = +1/2

Which of the following frequencies of light has the highest energy? A) 2.5 x 1010 s-1 D) 5.0 x 1014 s-1 B) 7.0 x 1013 s-1 E) 1.4 x 1015 s-1 C) 2.3 x 1014 s-1

E) 1.4 x 10^15 s-1

What is the energy in joules of one photon of x-ray radiation with a wavelength of 0.120 nm? A) 2.50 x 109 J D) 2.50 x 1018J B) 1.66 x 10-24 J E) 1.66 x 10-15J C) 1.66 x 10-33 J

E) 1.66 x 10^-15J 3x10^8 *6.63x10^-34*1000/0.120*10^-9= 1.66 x 10^-15J

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? A) 6.46 × 10-25 J D) 12.4 kJ B) 6.46 × 10-16 J E) 246 kJ C) 2.46 × 10-4 J 1 nm=1.0 × 10-9 meters mole= 6.02x10^23

E) 246 kJ h=6.626x10−34J.s c=3x10^8ms−1 λ=486x10−9m 1 mol photons = 6.023x10^23 photon Energy of one mole photon (E) = (6.023x10^23 x6.63x10−34J.s x 3x10^8ms)/(486x10−9m) Energy of one mole photon (E) =2.46x10^5 http://www.bama.ua.edu/~blacksto/CH101/exams_quizzes/quiz6_key.pdf

A ground-state atom of iron has ___ unpaired electrons and is _____. A) 0, diamagnetic D) 5, paramagnetic B) 6, diamagnetic E) 4, paramagnetic C) 3, paramagnetic

E) 4, paramagnetic

Breaking the oxygen-oxygen bond in hydrogen peroxide requires 210 kJ/mol. What is the longest wavelength of light that can cause this bond to be broken? A) 5.7 × 10-4 m D) 9.5 × 10-28 m B) 9.5 × 10-31 m E) 5.7 × 10-7 m C) 2.8 × 10-7

E) 5.7 × 10-7 m

4. Using the figure below, categorize electromagnetic radiation with a wavelength of 1.0 x 10-3 m. A) Gamma rays B) X rays C) Ultraviolet D) Infrared E) Microwave

E) Microwave

The ground-state electron configuration for an atom of indium is A) [Kr]5s24p64d5 D) [Kr]5s25p64d5 B) [Ar]4s23d104p1 E) [Kr]5s24d105p1 C) [Ar]4s24p63d

E) [Kr]5s24d105p1

Which of the following is the ground-state electron configuration of Pb? A) [Xe]6s25d106p2 D) [Xe]6s25f146d106p2 B) [Xe]6s26d106p2 E) [Xe]6s24f145d106p2 C) [Xe]6s24f146p2

E) [Xe]6s24f145d106p2

section 7.7 Which one of the following sets of quantum numbers represents an electron with the highest energy? A) n = 3, l = 2, ml = -2, ms = +1/2 D) n = 5, l = 0, ml = 0, ms = +1/2 B) n = 4, l = 1, ml = 0, ms = -1/2 E) n = 4, l = 2, ml = -1, ms = -1/2 C) n = 4, l = 0, ml = 0, ms = +1/2

E) n = 4, l = 2, ml = -1, ms = -1/2

Which of the following is diamagnetic both in its ground state and in all of its excited states? A) Mg B) Ne C) Cu D) Zn E) none of these

E) none of these

7.4 A proton is roughly 1800 times more massive than an electron. If a proton and an electron are traveling at the same speed, A) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. B) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. C) the wavelength of the photon will be roughly equal to the wavelength of the electron. D) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon. E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photo

E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photo

The electron configuration of a ground-state copper atom is A) [Ar]4s24d4 B) [Ar]4s24p63d3 C) [Ar]4s23d9 D) [Ar]3d9 E)[Ar]4s13d

E)[Ar]4s13d