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+
Use the periodic table to write electron configurations for each
of the following elements. Represent core electrons with the symbol
of the previous noble gas in brackets.
Part A
P
Express your answer in condensed form in order of increasing
orbital energy as a string without blank space between orbitals.
For example, [He]2s22p2 should be entered as
[He]2s^22p^2.
Part B
As
Part C
Sr
Part D
Sb
Write electron configurations for each of the following.
a) Ti, Ti2+, Ti4+
Ti:
Ti2+
Ti4+
b) Os, Os2+, Os3+
Os
Os2+
Os3+
c) Ir, Ir2+, Ir3+
Ir
Ir2+
Ir3+
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...
Chapter 8: Electron Configurations and Periodicity
Complete for a thumbs up!
a. Write the electronic configuration and draw the orbital
diagram of iron.
b. Create a table summarizing the group traits of elements.
c. Explain why Hund's rule is incredibly important. Use examples
or images to help back up your explanation
d. In the science field, chemists often use NMR for confirmation
of the structure of newly synthesized drugs. This is what MRIs do
to humans at hospitals. Please explain...
Identify the atoms that correspond to each of the following
electron configurations. Then, write the Lewis symbol for the
common ion formed from each atom: (a) 1s22s22p5 (b) 1s22s22p63s2
(c) 1s22s22p63s23p64s23d10 (d) 1s22s22p63s23p64s23d104p4 (e)
1s22s22p63s23p64s23d104p1
The following table gives the first ionization energies for the
second period elements. Using electron configurations, explain why
boron and oxygen have lower ionization energies than would be
expected based on the general trend.
Element
Li
Be
B
C
N
O
F
NE
IE (KJ/mol)
520
899
801
1086
1402
1314
1681
2081
Write the complete electron configurations Cobal(Co) atom for
its:
1-its ground state
2- an
excited
state
2- Draw the orbital diagram for the complete electron configuration
of Sulfur atom
3-Briefly explain how the following
concepts are used in developing electron configuration of atoms:
Hund’s rule and Pauli Exclusion principle.
21. a. Following is a list of electron configurations. Group the
configurations in pairs that would represent similar chemical
properties of the atoms. Give the chemical symbols for the elements
represented by each electron configuration.
1s2 2s2 2p6 3s2 1s2 2s2 2p3 1s2 2s2 2p6 3s2 3p6 4s2 3d104p6
1s2 2s2 3s2 3p3 1s2 2s2 1s2 2s2 2p6
b. A 2+ ion derived from a transition metal has 3 electrons in
the 3d subshell. What element made this ion?
c....