6) Write the electron configurations for the following using
noble gas core notation: a) Na b) S c) I
7)Given: N2 (g) + 3H2(g) ⇒ 2NH3 (g) ΔH = -92 kJ 92 kJ is the
quantity of heat which is: a. gained from the surroundings when 1
mol of ammonia is formed. b. gained from the surroundings when 2
mol of ammonia are formed. c. lost to the surroundings when 1 mol
of ammonia is formed. d. lost to the...
Write the electron configurations for the following ions, and
determine which have noble-gas configurations.
A) Ru 3+ B) As3-
C) Y3+ D) Pd2+ E)
Pb2+ F) Au3+
Write the ground state electron configurations for the
following. Use the noble gas shorthand notation. List orbitals in
filling order
Element number 14:
Electron configuration of neutral:
Electron configuration of doubly positive ion:
Element number 34:
Electron configuration of neutral:
Electron configuration of doubly positive ion:
Element number 92:
Electron configuration of neutral:
Electron configuration of doubly positive ion:
What is the Henry's law constant for CO2 at 20∘C?
Express your answer to three significant figures and include the
appropriate units.
What pressure is required to achieve a CO2 concentration of
9.40×10−2 M at 20∘C?
Express your answer to three significant figures and include the
appropriate units.
At 1 atm, how many moles of CO2 are released by raising the
temperature of 1 liter of water from 20∘C to 25∘C?
Express your answer to four decimal places and include...
Part B
Indicate the number of unpaired electrons for following: [noble
gas]ns2np5
Express your answer as an integer.
Part C
Identify the group of elements that corresponds to the following
generalized electron configuration: [noble
gas]ns2(n?1)d2
Incorrect; Try Again; 5 attempts remaining
Part D
Indicate the number of unpaired electrons for following: [noble
gas]ns2(n?1)d2
Express your answer as an integer.
Part E
Identify the group of elements that corresponds to the following
generalized electron configuration: [noble
gas]ns2(n?1)d10np1
Incorrect; Try Again; 5...
Part A
Write the full electron configuration for the nitrogen atom.
Express your answer as a series of subshells. For example, the
full electron configuration for carbon should be entered as
1s^22s^22p^2.
Part B
Write the full electron configuration for the aluminum atom.
Express your answer as a series of subshells. For example, the
full electron configuration for carbon should be entered as
1s^22s^22p^2.
Part C
Part complete
Write the full electron configuration for the neon atom.
Express your answer...
Part A
Zn(s)+Al3+(aq)?Zn2+(aq)+Al(s)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Part B
Cd(s)+Cu+(aq)?Cd2+(aq)+Cu(s)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
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Part C
I?(aq)+SO42?(aq)?H2SO3(aq)+I2(s)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
What is the only possible value of mℓ for an electron in an s
orbital?Express your answer numerically.
2.
Which of the following set of quantum numbers (ordered
n, ℓ, mℓ, ms) are possible for an
electron in an atom?
Check all that apply.
-1, 0, 0, -1/2
3, 2, 2, -1/2
3, 1, 0, -1/2
4, 3, -4, -1/2
3, 2, 0, -1/2
2, 1, 3, 1/2
2, 1, 0, -1
3, 3, 1, -1/2
Predict the common charge of the silver ion. Explain your
reasoning in terms of electron configurations.
Construct a quantum number tree for the principal quantum number
n = 4 similar to that depicted for n = 3
Use diagrams similar to Figure 1.12 to determine the number of
unpaired electrons in atoms of (a) nitrogen; (b) silicon; (c)
iron.
Write the electron confi guration expected for element 113 and
the confi gurations for the two cations that it is most...