Isotopes
c = (lamda)(nu)
Electron Config
Ionization Energy
Atomic/Ionic Radius
100
63Cu and 65Cu both have the same number of __, but a different number of ___.
63Cu and 65Cu both have the same number of PROTONS, but a different number of NEUTRONS.
100
An atom of hydrogen and He1+ are isoelectronic, yet their emission spectra are different. Explain why.
Although they both have 1 electron, it requires more energy to promote an electron in He1+ due to the greater effective nuclear charge. Because the amount of energy required to excite the electron would be different, the energy of light given off when the excited electrons return to ground state will be different, and if the photons of light have a different amount of energy, the bands of light you see will be a different color.
100
Write electron configuration notation for phosphorus and phosphide
P = 1s22s22p63s23p3
P3-=1s22s22p63s23p6
100
Ionization energy _____ as you go across a period _____ as you go down a family
Ionization energy INCREASES as you go across a period and DECREASES as you go down a family
100
Iodine has a larger atomic radius than chlorine. Explain why.
Although both atoms have 7 valence electrons, an atom of iodine has 5 energy levels, whereas an atom of chlorine has only 3 energy levels. The additional energy levels of iodine make the atomic radius of iodine larger than the atomic radius of chlorine.
200
List the number of protons, electrons and neutrons in an atom of Tungsten-180.
Protons = 74
Electrons = 74
Neutrons = 106
200
What is the frequency of a wave with a wavelength of 560 nm?
560 nm x 1m/1x109nm = 5.6 x 10-7m

c = λν
3.0 x 108m s-1 = (5.6 x 10-7m)(ν)
c = 5.4 x 1014s-1
200
1s22s22p66s2 would be an example of a/an
excited atom (doesn't follow Aufbau ordering) because you would expect the valence electrons for this element to be in the 3rd energy level (have a principle quantum number, n, of 3), but instead they have a principle quantum number of 6 (in other words, the valence electrons have been promoted to the 6th energy level.
200
The second ionization energy for sodium would be ___ than the first ionization for sodium because
The second ionization energy for sodium would be HIGHER than the first ionization for sodium because the first valence electron removed would be on the 3rd energy level, and the second valence electron removed would be down on the second energy level, and it takes more energy to remove an electron that is closer to the nucleus
200
Sulfur has a smaller radius than silicon. Explain why.
Although both atoms have 3 energy levels, sulfur has 16 protons pulling (greater effective nuclear charge) compared to silicon, which only has 14 protons pulling.
300
Antimony-121 and Antimony-123 both occur naturally. Which isotope is more abundant? Justify your answer.
121Sb is more common in nature. This can be determined by comparing the mass numbers of the nuclides to the average atomic mass of antimony on the periodic table. Because the average atomic mass, 121.75 is closer to 121 than it is to 123, 121Sb must be more abundant.
300
How much energy is given off by a wave with a frequency of 4.2 x 1014s-1?
E = hν
300
An orbital that has two up arrows disobeys...
the Pauli principle which states that two electrons in the same orbital should have opposite spin
300
Which element in the third period would have the following ionization energies?
I1 578 kJ/mol
I2 1817 kJ/mol
I3 2745 kJ/mol
I4 11,577 kJ/mol
I5 14842 kJ/mol
I6 18,379 kJ/mol
Aluminum (It takes substantially more energy to remove the 4th electron, which means the element has 3 electrons in its outermost shell, therefore, the element is Al)
300
The ionic radius of bromine is larger than the ionic radius of strontium. Explain why.
Although both ions are isoelectronic (same number of electrons), Sr2+ has more protons pulling on the valence shell, making the ionic radius of Sr2+ smaller than the ionic radius of Br1-
400
There are two naturally occurring isotopes of Gallium. The nuclide that has an atomic mass of 68.9257 amu makes up 60.40% found in nature. What is the mass of the other isotope of gallium?
69.72 = [(.6040)(68.9257)] + [(.3960)(x)]

69.72 = 41.6311228 + .3960x

28.09 = .3960x

x = 70.93 amu

400
How much energy is absorbed when an electron is promoted from the 2nd energy level to the 5th energy level?
E= -2.178 x 10-18 J - -2.178 x 10-18 J
n2       n2

E= -2.178 x 10-18 J - -2.178 x 10-18 J
52       22

E = 4.574 x 10-19 J
400
Noble gas configuration for mercury would be
[Xe]6s24f145d10
400
Write the BCE for the first three ionizations of sulfur.
S --> S1+ + 1 e-
S1+ --> S2+ + 1 e-
S2+ --> S3+ + 1 e-
400
The most metallic element on the periodic table is Fr because
it has the lowest ionization energy due to its large atomic radius.
500
There are two naturally occurring isotopes of Chlorine. One isotope has a mass of 34.968853 amu, the other isotope has a mass of 36.965903 amu. Calculate their abundances.
35.45 = [(x)(34.968853)] + [(1 - x)(36.965903)]

35.45 =   34.968853x + 36.965903 - 36.965903x

-1.52 = -1.99705x

x = .761

35Cl makes up 76.1% of the naturally occurring Cl, 37Cl makes up the rest, 23.9%
500
What is the longest wavelength of light (in nm) that has enough energy to overcome the 364 kJ mol-1 bond energy for ozone?
364 kJ/mol x 1000 J/1 kJ x 1 mol/6.022 x 1023 = 6.04 x 10-19 J

E = hν

6.04 x 10-19 J = (6.63 x 10-34J s-1)(&#957)

&#957 = 9.11 x 1014s-1


c = λν

3.0 x 108m s-1 = (λ)(9.11 x 1014s-1)

λ = 3.3 x 10-7m

3.3 x 10-7m x 1x109nm/1 m = 330 nm
500
Aluminum would be _______ (paramagnetic/diamagnetic) because it has __________________ .
Aluminum would be PARAMAGNETIC because it has at least one UNPAIRED ELECTRON.

↑  __ __ in 3p.

Being paramagnetic means the element would be attracted to a magnetic field.
500
Chloride would have a lower first ionization energy than chlorine because
Chloride has a larger atomic radius than chlorine (same number of energy levels, same number of protons pulling, added ve- in Cl1- makes valence shell bigger), and because it takes less energy to remove an electron from a larger atom, I1 is lower for Cl1- than it is for Cl
500
The ionic radius for iodide is larger than the atomic radius of iodine. Explain why.
Both iodine and iodide have 5 energy levels, both iodine and iodide have 53 protons pulling on the valence shell, iodide has one additional electron in the valence shell. The additional repulsion of the added valence electron makes the valence shell of I1-slightly larger than the valence shell of I, therefore the radius of iodide is slightly larger than the radius of iodine.
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