Questions about chemistry

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timer Asked: Oct 16th, 2018
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There are questions about chemistry in word file that I attached,

Please answer all the questions correctly in word file.

Homework #6 Name ________________ Student ID ______________ Date ______________ 6.10 Calculate the wavelengths, in meters, of radiation of the following frequencies. (a) 5.00  1015 s–1, (b) 2.11  1014 s–1, (c) 5.44  1012 s–1 6.28 According to the Bohr model of the atom, what happens when an atom absorbs energy? 6.32 A neon atom emits light at many wavelengths, two of which are at 616.4 nm and 638.3 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) If a transition between the two higher energy states could be observed, what would the frequency of the light be? 6.36 What are the mathematical origins of quantum numbers? 6.38 Which of the following represent valid sets of quantum numbers? For a set that is invalid, explain briefly why it is not correct. (a) n = 3,  = 3, m = 0, (b) n = 2,  = 1, m = 0, (c) n = 6,  = 5, m = –1, (d) n = 4,  = 3, m = –4 6.40 Why are there no 2d orbitals? 6.42 How many orbitals correspond to each of the following designations? (a) 3p, (b) 4p, (c) 4px, (d) 6d, (e) 5d, (f) 5f, (g) n = 5, (h) 7s 6.44 Define the term nodal plane (or node). 6.52 Depict two ways to place electrons in the 2p orbitals for a nitrogen atom. Which depiction is the correct one according to Hund’s rule? 6.54 Write the ground state electron configuration for (a) B, (b) Ba, (c) Be, (d) Cl, (e) Br. 6.56 From the list of atoms and ions given, identify any pairs that have the same electron configurations and write that configuration. Na+, S2–, Ne, Ca2+, Fe2+, Kr, I–. 6.58 Distinguish between the terms core electrons and valence electrons. 6.66 Use the electronic configuration of the alkali metals and your knowledge of orbitals and quantum numbers to explain the trend in atomic size of alkali metal atoms. 6.68 Define the term ionization energy. What is the difference between the definition of the first ionization energy and the second ionization energy? 6.70 Arrange the following atoms in order of increasing ionization energy: Li, K, C, and N. 6.74 Indicate which species in each pair has the more favorable (more negative) electron affinity. Explain your answers. (a) Cl or S, (b) S or P, (c) Br or As 6.86 Arrange the following sets of anions in order of increasing ionic radii: (a) Cl–, S2–, P3–, (b) O2–, S2–, Se2–, (c) N3–, S2–, Br–, P3–, (d) Cl–, Br–, I– 6.92 The red color seen in fireworks is the result of having strontium-containing salts in the fireworks bomb. Similarly the green/blue colors sometimes seen in fireworks arise from copper salts. Based on your understanding of atomic spectra and the colors seen in fireworks, describe which atom, copper or strontium, has more widely separated energy levels.

Tutor Answer

PerfectGrade
School: Cornell University

Attached.

Homework #6
Name ________________ Student ID ______________ Date ______________

6.10

Calculate the wavelengths, in meters, of radiation of the following frequencies.
(a) 5.00  1015 s–1, (b) 2.11  1014 s–1, (c) 5.44  1012 s–1

a) Frequency (ν) = Speed(c) * wavelength(λ)
ν=cλ
λ= c/ ν
λ= 2.998*108 /5.00  1015= 5.996*10-8m
b) λ= 2.998*108 / 2.11  1014=1.4209 *10-6m
c) 2.998*108 / 5.44  1012= 5.511*10-5m

6.28

According to the Bohr model of the atom, what happens when an atom
absorbs energy?

The electrons in the atom absorbs the energy and thus become exited and in turn jump to
the next energy level i.e. the exited state condition. When in this excited state condition,
the atom is unstable and for it to regain stability i.e. the lowest energy state the electron
loses the excess energy by emitting light energy.
6.32
A neon atom emits light at many wavelengths, two of which are at 616.4 nm and 638.3
nm. Both of these transitions are to the same final state. (a) What is the energy difference
between the two states for each transition? (b) If a transition between the two higher
energy states could be observed, what would the frequency of the light be?

E= hν =h c/ λ
Where h= 6.63*10-34J.S
C=2.998*108ms-1
E =E1-E2
E1= h c/ λ =(6.63*10-34 *2.998*108)(616.4*10-9)=3.225*10-19 J
E2= h c/ λ =(6.63*10-34 *2.998*108)(638.3*10-9)=3.114*10-19 J
E =E1-E2=3.225*10-19 J -3.114*10-19 J=1.11*10-20 J
E=1.11*10-20 J = hν
Frequency (ν)= E/h =1.11*10-20 J/ 6.63*10-34 = 1.674*1014 S-1

6.36

What are the mathematical origins of quantum numbers?

Quantum numbers are the values explaining state of an electron i.e. their distance from
the nucleus, orientation s...

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Anonymous
Outstanding Job!!!!

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