Question

Consider the following electron configurations for neutral atoms: Atom I = 1s2 2s2 2p6 3s2 Atom II = 1s2 2s2 2p6 3s2 3p4 Atom III = 1s2 2s2 2p6 3s2 3p6 Which atom would be expected to have the largest third ionization energy?

Answer #1

Ionization energy is the energy required to remove the electron from an neutral atom to rise a positive charge on it.

And the Ionization energy increases across a period and decreases along a group

Here Ar has highest ionization energy because it is a noble gas. It has complete filled orbitals.

The increasing order of the ionization energy :

Mg < S < Ar

The element with largest third ionization energy is Mg

The following are represented them hypothetical neutral atoms X,
Y, Z and T and their respective electronic configurations:
X - 1s2
Y - 1s2 2s2
Z - 1s2 2s2 3s2 3p6 2P6
T - 1s2 2s2 3s2 3p6 4s2 2P6
What is more ionization energy is:
Explain your resposat.
a) Y
b) Z
c) T
d) X

Answer all the following multiple choices with the right
answer.
Question 1
Which object(s) would you use to describe the shape of the
2p orbital?
Question 1 options:
a)
a circle
b)
a sphere
c)
a dumb-bell
d)
two perpendicular dumb-bells
e)
a doughnut
Question 2
Which situation must be true for two electrons to occupy the
same orbital?
Question 2 options:
a)
The electrons must have low energy.
b)
The electrons must have identical sets of quantum numbers.
c)...

All parts of this question refer to neutral atoms in their
ground states.
a) What are the principal and orbital quantum numbers (n and l)
of all the electrons in aluminum (Z=13) atoms? Please use the
standard notation for specifying electron configurations in
atoms.
b) Estimate (and explain briefly) the ionization energy for the
least tightly bound electron in a lithium (Z=3) atom.
c) Estimate (and explain briefly) the energy that it would take
to remove all the electrons from...

Give the uncondensed ground state electron configurations for
the following atoms and ions.
a. Te2-
b. As
c. Cr
d. The smallest halogen atom
e. Al3+

How
do I calculate the electron numbers in neutral atoms? How do I
calculate the number of ion(actions and anions) are in an atom? How
do I calculate how many isotopes are in an atom?

Consider these 3 transitions for an electron in a hydrogen
atom.
I) n = 7 --> n = 1 II ) n = 7 --> n = 5
III ) n = 1 --> n = 7
IV) n = 7 --> n = 6.
Which of these has a negative ΔE?
I only
III and IV
II only
I and III
I and II
IV only
I, II and IV
I, II , III , and IV

(I) What is the full ground state electron configuration for a
neutral atom with ? = 22 protons?
(II) A hydrogen atom with a principal quantum number of ? =
4.
a. write all the possible values for the other quantum
numbers.
b. calculate the total number of possible quantum states that
can exist for this principal quantum state.
(III) An excited hydrogen atom is in the 6?1 state.
a. What is the principal quantum
number of the electron?
b....

Consider the following four transitions in a hydrogen atom.
(i) ni = 6, nf = 9 (ii) ni = 6, nf = 12 (iii) ni = 10, nf = 12
(iv) ni = 9, nf = 6
(a) Give the wavelength of the longest-wavelength photon that
can be emitted or absorbed by these transitions. m
(b) Give the wavelength of the shortest-wavelength photon that
can be emitted or absorbed by these transitions. m
(c) For which of these transitions does...

Arrange the following atoms in order of increasing electron
affinity: C, F, Ne, O
Which of the following has the largest first ionization energy?
Nitrogen, Phosporus, Arsenic, Antimony

Consider the Bohr model of the hydrogen atom for which an
electron in the ground state executes uniform circular motion about
a stationary proton at radius a0. (a) Find an expression
for the kinetic energy of the electron in the ground state. (b)
Find an expression for the potential energy of the electron in the
ground state. (c) Find an expression for the ionization energy of
an electron from the ground state of the hydrogen atom. The
ionization energy is...

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