Electrons in Atoms --Unit Test 8

Electrons In Atoms

True/False

Bohr's model of the atom explained the spectra of the hydrogen atom.
In the Bohr model of the atom, an electron gives off energy as it changes from the 2nd to the 4th energy level.
The Heisenberg uncertainty principle states that it is impossible to know both the position and path of an electron.
The 3s orbital is spherical.
There are nine different sub-orbitals in the 3rd energy level.
It is impossible to have a p-type orbital in the second energy level.
When writing electron configurations, the 4s orbitals fill before the 3d orbitals.
Noble gases are stable because their outer-level s, p, and d levels are completely filled.
An Al atom has a larger radius than an Al³⁺ ion.
Sodium has a low first ionization energy compared to other elements in its period.
A Ne atom has a larger atomic radius and a larger ionization energy than an Ar atom.
The reaction that representates the ionization energy of an F atom is: F (g) + e^- Energy + F^- (g).

Multiple Choice (Choose the best answer.)

When an electron in an atom of hydrogen moves from the second to the first principal energy level, the result is the emission of
alpha particles

nuclear mass

quantized energy

neutrons

beta particles
The lowest sub-level in each principal energy level is represented by the symbol:
f

p

s

d

g
What is the maximum number of electrons in the "nth" principle energy level?
n

2n

n²

2n²

2n³ - 3
Which electron transition is accompanied by the emission of energy?
1s to 2s

2s to 2p

3s to 3p

4p to 3p

More than one of these are correct.
Which atom has an electron configuration for its valence shell that is most similar to that of a phosphorus atom?
N

Se

S

Ar

F
Which electron configuration corresponds to a nitrogen atom at ground state?
1s² 2s²p⁶ 3s²

1s² 2s²p⁶ 3s¹

1s² 2s²p⁶

1s² 2s²p⁵

1s² 2s²p³
Which of the electron configurations would likely form a -1 ion?
1s² 2s²p⁶ 3s²

1s² 2s²p⁶ 3s¹

1s² 2s²p⁶

1s² 2s²p⁵

1s² 2s²p³
Which of the electron configurations would you expect to have the lowest first ionization energy?
1s² 2s²p⁶ 3s²

1s² 2s²p⁶ 3s¹

1s² 2s²p⁶

1s² 2s²p⁵

1s² 2s²p³
Identify the FALSE statement about orbitals.
There is one s orbital for each energy level.

The symbol 4p⁵ means there are 4 electrons in the 5 p orbitals.

They are regions of space likely to be occupied by electrons around a nucleus.

There are four orbitals in the second energy level.

In each energy level greater than one, there are three p orbitals.
Identify the FALSE statement about this electron configuration:
[Kr] 5s2 4d10 5p4

There are four valence electrons.

It has a similar electron configuration to oxygen.

It represents Te.

It likely forms a 2- ion.

It has 52 electrons.
Which of the following correctly ranks atoms by increasing atomic radius?
V, Ca, Sr

Sr, Ca, V

Ca, V, Sr

Ca, Sr, V

None of the above are correct.
Which of the following correctly ranks atoms by increasing ionization energy?
V, Ca, Sr

Sr, Ca, V

Ca, V, Sr

Ca, Sr, V

None of these are correct.
Which pair or pair(s) shown below correctly compairs atomic and ionic radii?
Li < Li ⁺

N > N ^3-

Cl > Cl ^-

More than one of these are correct.

None of these are correct.

Problem Solving (Show All Work. Use significant figures.)

1. Determine the wavelength, in meters, of the radio signal, KCHM at a frequency of 1510 kilohertz (cycles per second). The velocity of light is 3.00 x 10⁸ m/s.

2. About 100 Kcal are needed to break a mole of typical chemical bonds. Would absorption of light having a frequency of 5.2 x 10 ¹⁴ Hertz be sufficient to break a mole of typical chemical bonds? Planck's constant, h, = 9.52 x 10 ^-14(Kcal*sec)/mol.

3. For the atoms shown below:

a) draw an energy diagram

b) write the electron configuration (1s² 2s² and so on)

c) state the number of valence electrons

d) pick one of the atoms and sketch a picture showing all its orbitals

Na:

Na⁺:

S:

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