Question

Write the electron configurations for N2, O2, CO, NO, CN- and calculate the bond order for each. (b) Which are paramagnetic ? (c) Which have the shortest bond lengths ?

Answer #1

The bond length of N2 increases upon removing an electron while
that of O2 decreases upon removing an electron. The experimental
values of bond lengths of N2 and N2 + are 1.094 Å and 1.116 Å,
respectively. The experimental values of bond lengths of O2 and O2
+ are 1.207 Å and 1.123 Å, respectively. Account for this trend
using MO theory and bond order.

Consider the nitrogen molecule and the N2+ molecular ion:
(a) Give the bond order of each species. If a fraction is
needed, use a decimal number. Bond order N2 = Bond order N2+ =
(b) Predict which species should be paramagnetic. Is N2
paramagnetic? Is N2+ paramagnetic?
(c) Predict which species has the greater bond dissociation
energy. The species with the largest bond dissociation energy is:
a. N2 b. N2+

Write the electron configurations for the following atoms. Enter
full electron configuration in order electrons fill the
subshells.
As
Cl
Ni
Si

Write ground-state electron configurations for the ions
Mg+, Na+,
F-and Zn2+.
Which do you expect will be paramagnetic due to the presence of
unpaired electrons?
(Express your answer as a series of orbitals. For example, the
electron configuration of Li would be entered in complete form as
1s2 2s1 or in condensed
form as [He]2s1.)
ion
electron configuration
paramagnetic
Mg+
_____yes no
Na+
_____yes no
F-
_____yes no
Zn2+
_____yes no

For the following atoms, write the ground-state orbital
diagrams, the electron configurations, and the
condensed electron configurations. Finally, state the number of
unpaired electrons.
(a) Nitrogen
(b) Sodium
(c) Argon
(d) Titanium
(e) Zinc

A) Write the condensed electron configurations
for the Ga atom. B)
Indicate how many unpaired electrons the
Ga atom has. C) Write
the condensed electron configurations for the
Ca atom. D) Indicate how
many unpaired electrons the Ca atom has.
E) Write the condensed electron configurations for
the V atom. F) Indicate
how many unpaired electrons the V atom
has. G) Write the condensed electron
configurations for the I atom.
H) Indicate how many unpaired electrons the
I atom has....

Write the electron configurations for the following atoms or
ions:
(a) B3+
(b) O–
(c) Cl3+

Write the electron configurations for the following atoms. Enter
full electron configuration in order electrons fill the subshells.
Enter subshells in parentheses followed by numbers of electrons in
the exponent. For example you should enter
"(1s)2(2s)2(2p)5" for atom of
fluorine. The answer is case sensitive.
As, Cl, Ni, Si
Calculate the energy in joules of a photon of green light having
a wavelength of 537 nm. Report your result to three significant
figures.
What is the letter code for a...

Write electron configurations for the following atoms
or ions and indicate the number of valence electrons:
a) Cl- (atomic number 17)
b) Cr (atomic number 24)
c) Ba2+ (atomic number 56)
d) Pb (atomic number 82)

Describe the electronic structure using molecular orbital
theory, calculate the bond order of each and decide whether it
should be stable. For each state whether the substance is
diamagnetic or paramagnetic. (Enter the bond order to 1 decimal
place.)
(a) B2
KK(σ2s)2(σ2s*)2(π2p)2
KK(σ2s)2(σ2s*)1(π2p)2
KK(σ2s)2(σ2s*)2(π2p)1
KK(σ2s)2(π2s*)2(π2p)2
bond order------------
-----------stability
stable or unstable
magnetic character
paramagnetic diamagnetic
(b) B2+
KK(π2s)2(σ2s*)2(π2p)1
KK(σ2s)2(σ2s*)2(π2p)1
KK(σ2s)2(σ2s*)1(π2p)1
KK(σ2s)2(σ2s*)2(π2p)2
bond order---------
------------stability
stable unstable
magnetic character
paramagnetic diamagnetic
(c) O2−
KK(σ2s)2(σ2s*)2(π2p)4(σ2p)2(σ2p*)3
KK(σ2s)2(σ2s*)2(π2p)4(σ2p)2(π2p*)3
KK(σ2s)2(σ2s*)2(π2p)4(σ2p)2(π2p*)1
KK(σ2s)2(σ2s*)2(π2p)4(σ2p)2(π2p*)2
bond order---------
----------stability
stable...

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