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chem 111-exam 2

Terms in this set (110)

Predict the charge that an aluminum ion would have.
1-
5-
2+
3+
1+
3+
Which reaction below represents the second ionization of Sr?
Sr2+(g) + e- → Sr+(g)
Sr(g) → Sr+(g) + e-
Sr+(g) → Sr2+(g) + e-
Sr-(g) + e- → Sr2-(g)
Sr+(g) + e- → Sr(g)
Sr+(g) → Sr2+(g) + e-
Place the following in order of decreasing IE1.

Cs Mg Ar

Ar > Mg > Cs
Cs > Ar > Mg
Mg > Cs > Ar
Cs > Mg > Ar
Mg > Ar > Cs
Ar > Mg > Cs
For a given atom, identify the species that has the smallest radius.
cation
neutral
anion
They are all the same size.
cation
Choose the valence orbital diagram that represents the ground state of Sr2+.
orbital diagram where the 5s orbital contains 1 pair of electrons. 4d orbitals contain 2 unpaired electrons.

orbital diagram where the 4s orbital contains 1 pair of electrons. 4p orbitals contain 3 pairs of electrons.

orbital diagram where 4p orbitals contain 3 pairs of electrons.

orbital diagram where the 5s orbital contains 1 pair of electrons.

orbital diagram where the 5s orbital contains 1 pair of electrons. 5p orbitals contain 2 unpaired electrons.
orbital diagram where the 4s orbital contains 1 pair of electrons. 4p orbitals contain 3 pairs of electrons.
Give the complete electronic configuration for Ca2+.
1s22s23p64s25p6
1s22s2p63s2p6
1s22s22p63s24p6
1s22s22p63s23p5
1s22s22p63s23p6
1s22s22p63s23p6
How many electrons are in the ion, S2-?
34
14
18
30
18
Which of the following elements is not a solid at room temperature?
Al
Ag
Br
Fe
Br
Give the number of core electrons for Cd.
44
38
36
46
48
36
Choose the orbital diagram that represents the ground state of N.

orbital diagram where 1s and 2s orbitals contain 1 pair of electrons each. 2p orbitals are empty.

orbital diagram where 1 s and 2 s orbitals contain 1 pair of electrons each. 2 p orbitals contain 3 pairs of electrons.

orbital diagram where 1s and 2s orbitals contain 1 pair of electrons each. 2p orbitals contain 1 pair of electrons and an unpaired electron.

orbital diagram where 1s and 2s orbitals contain 1 pair of electrons each. 2p orbitals contain 3 unpaired electrons.

orbital diagram where 1s and 2s orbitals contain 1 unpaired electron each. 2p orbitals contain 2 pairs of electrons and 1 unpaired electron.
orbital diagram where 1s and 2s orbitals contain 1 pair of electrons each. 2p orbitals contain 3 unpaired electrons.
Part complete
The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is ________
vanadium
chromium
manganese
iron
titanium
chromium
Give the ground state electron configuration for Cd.
[Kr]5s24d8
[Kr]5s24d105p2
[Kr]5s25d10
[Kr]5s24d10
[Kr]4d10
[Kr]5s24d10
Choose the statement that is TRUE.
a.) Core electrons effectively shield outer electrons from nuclear charge.

b.)Valence electrons are most difficult of all electrons to remove.

c.)Core electrons are the easiest of all electrons to remove.

d.)Outer electrons efficiently shield one another from nuclear charge.

e.)All of the above are true.
Core electrons effectively shield outer electrons from nuclear charge
Why does an electron found in a 2s orbital have a lower energy than an electron found in a 2p orbital in multielectron systems?

Electrons in the 2s orbital are shielded by electrons in the 2p.

The larger number of electrons found in the 2p orbital leads to greater repulsion.

The shape of the orbital ultimately determines the energy of the electrons.

Electrons in the 2s orbital can penetrate the 1s orbital and be closer to the nucleus .

There are more nodes found in the 2s orbital.
Electrons in the 2s orbital can penetrate the 1s orbital and be closer to the nucleus .
Which of the following elements is NOT a metal?
Ba
Xe
Mg
Pb
Ga
Xe
How many orbitals are present when l=3?
1
3
5
7
9
7
Which of the following quantum numbers describes the shape of an orbital?
angular momentum quantum number
principal quantum number
magnetic quantum number
spin quantum number
Schrödinger quantum number
angular momentum quantum number
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is the transition from n = 1 to n = ∞.
3.62 × 103 kJ
5.33 × 103 kJ
7.62 × 103 kJ
1.31 × 103 kJ
2.76 × 103 kJ
1.31 × 103 kJ
What is the energy of light associated with a transition from n=3 to n=8 in a hydrogen atom? Does this represent absorption or emission of a photon?
4.54 × 10-19 J, absorption
2.08 × 10-19 J, absorption
6.81 × 10-20 J, absorption
4.54 × 10-19 J, emission
2.08 × 10-19 J, emission
2.08 × 10-19 J, absorption
Choose the transition (in a hydrogen atom) below that represents the absorption of the shortest wavelength photon.
n = 3 to n = 1
n = 2 to n = 3
n = 4 to n = 6
n = 1 to n = 2
n = 6 to n = 5
n = 1 to n = 2
Identify the correct values for a 1s sublevel.
n = 4, l = -1, ml = -2
n = 2, l = 0, ml = 1
n = 2, l = 1, ml = -2
n = 3, l = 1, ml = 0
n = 1, l = 0, ml = 0
n = 1, l = 0, ml = 0
What are the possible values of l if n = 2?
-5, -4, -3, -2, -1, 0, +1, +2, +3, +4, or +5
0 or 1
2
-4, -3, -2, -1, 0, +1, +2, +3, or +4
0 or 1
Determine the lowest frequency of light capable to remove an electron from a sample of Ti metal, if the binding energy of titanium is 3.14 × 103 kJ/mol.
2.11 x 1015 Hz
7.87 x 1015 Hz
1.27 x 1015 Hz
6.19 x 1015 Hz
4.74 x 1015 Hz
7.87 x 1015 Hz
Which statement about electromagnetic radiation is correct?
As the wavelength decreases the energy decreases.

The amplitude of a wave depends on the frequency.

Radio waves have a smaller wavelength than visible light.

As the energy decreases the frequency decreases.

The wavelength and frequency are independent of each other.
As the energy decreases the frequency decreases
Electromagnetic radiation with a wavelength of 575 nm appears as yellow light to the human eye. The energy of one photon of this light is ________ J.
1.14 × 10-22
3.46 × 10-19
2.89 × 1018
3.46 × 10-28
1.14 × 10-31
3.46 × 10-19
The distance from the sun to Earth is 1.496*10^8 km. How long does it take light to travel from the sun to the Earth?
499 seconds
List these types of electromagnetic radiation in order of (i) increasing wavelength (ii) increasing energy per photon
a.) radio waves
b.) microwaves
c.) infrared radiation
d.)ultraviolet radiation
i) d, c, b, a
ii) a, b, c, d
Calculate the frequency of each wavelength of electromagnetic radiation:
a.) 632.8 nm
b.) 503 nm
c.) 0.052 nm
a.) 4.74 * 10^14 Hz
b.) 5.96 * 10^14 Hz
c.) 5.8 * 10^18 Hz
Calculate the energy of a photon of electromagnetic radiation of each of the wavelengths:
a.) 632.8 nm
b.) 503 nm
c.) 0.052 nm
a.) 3.14 * 10 ^-19 J
b.) 3.95*10^-19 J
c.) 3.8 * 10^-15 J
A laser pulse with a wavelength 532 nm contains 3.85 mJ of energy. How many photons are in the laser pulse?
a.)
b.)
c.)
Determine the energy of 1 mol of photons for each kind of light. (assume three significant figures)
a.) infrared radiation (1500 nm)
b.) visible light (500 nm)
c.) ultraviolet radiation (150 nm)
a.)
b.)
c.)
Put the types of electromagnetic radiation in order of decreasing frequency.

ultraviolet > infrared > radio > microwave
radio > microwave > infrared > ultraviolet
ultraviolet > infrared > microwave > radio
microwave > radio > infrared > ultraviolet
ultraviolet > infrared > microwave > radio
A radio station's channel, such as 100.7 FM or 92.3 FM, is actually its frequency in megahertz (MHz), where 1MHz=106Hz and 1Hz=1s−1.
λ =
3.291 m
Green light has a frequency of about 6.00×1014s−1. What is the energy of a photon of green light?
Ephoton =
3.98×10−19 J
Hospital X-ray generators emit X-rays with wavelength of about 15.0 nanometers (nm), where 1nm=10−9m. What is the energy of a photon of the X-rays?
Ephoton =
1.32×10−17 J
Arrange the colors of visible light, green, red, and blue, in order of increasing wavelength.
blue < green < red
red < green < blue
green < blue < red
blue < green < red
Arrange the colors of visible light, green, red, and blue, in order of increasing frequency.
red < green < blue
red < blue < green
blue < green < red
red < green < blue
Arrange these three colors of visible light, green, red, and blue, in order of increasing energy per photon
blue < green < red
red < blue < green
red < green < blue
red < green < blue
A 100-watt light bulb radiates energy at a rate of 100 J/s. (The watt, a unit of power or energy over time, is defined as 1 J/s.) If all of the light emitted has a wavelength of 525 nm , how many photons are emitted per second?
radiation =
2.64×1020
photons per second
The energy required to dislodge electrons from sodium metal via the photoelectric effect is 275 kJ/mol . What wavelength of light, in nanometers, has sufficient energy per photon to dislodge an electron from the surface of sodium?
wavelength of light =
435 nm
A microwave oven operates at 3.00 GHz . What is the wavelength of the radiation produced by this appliance?
λ = 1.00×108nm
How much time (in seconds) does it take light to travel 1.70 billion km?
5.67×103s
5.10×1017s
5.67 s
5.10×1020s
5.67×10^3s
Which wavelength of light has the highest frequency?
6 nm
18 mm
18 nm
6 mm
6 nm
How much energy (in J) is contained in 1.00 mole of 555 nm photons?
2.16×105 J
5.95×10−43 J
3.58×10−28 J
3.58×10−19 J
2.16×10^5 J
A laser produces 16.0 mW of light. In 2.00 hr , the laser emits 3.02×1020 photons. What is the wavelength of the laser?
λ = 521 nm
A carbon-carbon bond requires 348 kJ/mol to break.What is the longest wavelength of radiation with enough energy to break carbon-carbon bonds?
λmax = 344 nm
What is a photon?
charge transporting particle
the way of any interaction
the smallest particle
a packet of light
a packet of force
a packet of light
How is the energy of a photon related to its wavelength?
E=h⋅λ/ν
E=h⋅λ/c
E=h⋅c/λ
E=h⋅c⋅λ
E=h⋅ν/λ
E=h⋅c/λ
How is the energy of a photon related to its frequency?
E=h⋅ν/λ
E=h⋅λ/ν
E=h⋅c/ν
E=h⋅ν
E=c⋅h⋅ν
E=h⋅ν
Determine the wavelength of the light absorbed when an electron in a hydrogen atom makes a transition from an orbital in which n=2 to an orbital in which n=7.
λ = 397 nm
An electron in the n=6 level of the hydrogen atom relaxes to a lower energy level, emitting light of λ=93.8nm. Find the principal level to which the electron relaxed.
n=1
n=4→n=3
Express the frequency in inverse seconds.
ν1 =
1.60×10^14s−1
n=5→n=1
Express the frequency in inverse seconds.
ν2 =
3.16×10^15s−1
n=5→n=4
Express the frequency in inverse seconds.
ν3 =
7.40×10^13s−1
n=6→n=5
Express the frequency in inverse seconds.
ν4 =
4.02×10^13 s−1
Which statement related to particle and wave properties of matter is correct?
a.)Particles exhibit diffraction while waves do not.

b.)A wave travels straight through a slit.

c.)Interference patterns are observed when a wave passes through a barrier with two slits.

d.)Particles interfere constructively and destructively whereas waves do not.
c.) Interference patterns are observed when a wave passes through a barrier with two slits.
The two-slit diffraction experiment shows how light can be treated as particles and how light waves carry the statistical information for the experiment. If we were to use a beam of electrons instead of light in the experiment, how would the results differ?

a.)There would be a diffraction pattern similar to, but different from, that using light.

b.)There would be no change.

c.)There would only be a single spot from the electron beam.

d.)There would be no diffraction pattern.
a.)There would be a diffraction pattern similar to, but different from, that using light.
If electrons were used in the two-slit experiment instead of light, what change would need to be made to the slit spacing in order to see a diffraction pattern?
a.)Electrons cannot diffract.
b.)The slit spacing has to decrease.
c.)The slit spacing has to increase.
d.)No change
The slit spacing has to decrease.
What is the energy uncertainty ΔE associated with a short pulse of laser light that lasts for only 3.2 femtoseconds (fs)?
ΔE =
1.6×10−20 J
Suppose the low-energy end of the pulse had a wavelength of 701 nm . What is the wavelength of the high-energy end of the pulse that is limited only by the uncertainty principle?
λmax =
660 nm
Which electron transition produces light of the highest frequency in the hydrogen atom?
5s→1s
4s→1s
3s→1s
6s→1s
6s→1s
Calculate the wavelength of light emitted when an electron in the hydrogen atom makes a transition from an orbital with n=6 to an orbital with n=2.
4.84×10−19m
4.10×10−7m
3.28×10−6m
3.28×10−7m
4.10×10−7m
Which of the following statements about nodes and probability density are accurate?
The 2s orbital does not have any nodes.

The probability of finding an electron at the center of a d orbital is greater than zero.

The probability of finding an electron at the center of a p orbital is zero.

The 4f orbitals have three nodes.

The 3p orbitals have two nodes.
The probability of finding an electron at the center of a p orbital is zero.
The 4f orbitals have three nodes.
The 3p orbitals have two nodes.
Calculate the wavelength of light produced if an electron moves from n=2 state to n=1 state of an electron in a hydrogen atom.
1.22×10−7 m
Predict if this wavelength higher or lower than those produced if an electron moves from n=5 state to n=1 state.
higher
lower
higher
Calculate the energies of the n=1,n=2, and n=3 levels for an electron in a box with a length of 390 pm .
E1, E2, E3 =
3.96×10−19,1.58×10−18,3.56×10−18
J
Calculate the wavelength of light required to make a transition from n=1→n=2 and from n=2→n=3.
λ1→2, λ2→3 =
167, 100nm
For λ = 1875 nm.
n=4→n=3
n=5→n=3
n=6→n=3
n=7→n=3
n=4→n=3
For λ = 1282 nm.

n=4→n=3
n=5→n=3
n=6→n=3
n=7→n=3
n=5→n=3
For λ = 1093 nm.
n=4→n=3
n=5→n=3
n=6→n=3
n=7→n=3
n=6→n=3
What minimum frequency of light is required to ionize boron?
νmin =
2.01×10^15s−1
Which set of quantum numbers cannot specify an orbital?
n=4,l=3,ml=3
n=3,l=1,ml=−1
n=3,l=−3,ml=0
n=2,l=1,ml=−1
n=3,l=−3,ml=0
What are the possible values of l for each of the following values of n? n=3
l = 0,1,2
What are the possible values of l for each of the following values of n? n=4
l = 0,1,2,3
What are the possible values of l for each of the following values of n? n=2
l = 0,1
What are the possible values of l for each of the following values of n? n=1
l = 0
Which electron is, on average, further from the nucleus: an electron in a 3p orbital or an electron in a 4p orbital?
4p
Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital?
an electron in a 2s orbital
an electron in a 3s orbital
an electron in a 2s orbital
What are the possible values of the magnetic quantum number ml?

all the positive integers: 1,2,3, etc.

represented by the formula: m = 2l + 1, where l is an angular momentum quantum number

all the integer: -3,-2,-1,0,1,2,3, etc
.
all the non-negative integers: 0,1,2,3, etc.

all the integers in range from -l to +l, where l is an angular momentum quantum number

represented by the formula: m = 2k + 1, where k is a positive integer
all the integers in range from -l to +l, where l is an angular momentum quantum number
What does the magnetic quantum number determine?
the overall size of an atom

the possible number of electorns on particular orbital

the orientation of the orbital

the energy of the electron on the outer shell
the orientation of the orbital
Which of the following is the term used to describe a set of elements whose properties tend to be largely predictable based on their position on the periodic table?
Transition
Inner transition
Main-group
Period
main-group
What is the electron configuration of aluminum?
1s 22s 22p 1
1s 22s 22p 63s 23p 3
1s 22s 22p 63s 23p 34s 24p 1
1s 22s 22p 63s 23p 1
1s 22s 22p 63s 23p 1
Which of the following factors are involved in explaining why the energy of orbitals within a principle quantum level in multielectron atoms are not degenerate?
Coulomb's law
shielding
penetration

B and C only
A and C only
A, B, and C
A and B only
A, B, and C
What is the electron configuration of the element located in the fourth row of the periodic table in group 5A?
[Ar] 4s 23d 3
[Ar] 4s 24p 3
[Ne] 3s 23p 3
[Ar] 4s 23d 104p 3
[Ar] 4s 23d 104p 3
Which of the following sets contains elements that will form ions with a charge of 2−?
Te, S, and O
Sr, Ca, and Be
As, P, and N
Si, P, and S
Te, S, and O
Which of the following arranges the given atoms in order of increasing atomic radius (shortest to longest)?
K, Ca, Se, and Kr
I, Br, Cl, and F
Cl, Ar, K, and Ca
Kr, Se, Ca, and K
Kr, Se, Ca, and K
Which of the following statements is correct?
The valence electrons of P experience a larger effective nuclear charge than those of Cl.

The size of Br atoms is larger than that of As atoms.

The atoms of K are smaller than those of Ca.

The valence electrons of Ba experience larger effective nuclear charge than those of Cs.
The valence electrons of Ba experience larger effective nuclear charge than those of Cs
Which of the following arranges the atoms in order of increasing ionization energy (smallest to largest)?
K, Ca, Cl, and Ar
Mg, Ca, Sr, and Ba
Xe, I, Sb, and Rb
Ne, Se, Sb, and Pb
K, Ca, Cl, and Ar
Which of the following species is diamagnetic?
Cl
Fe2+
S2−
Al
S2−
What is the electron configuration of calcium, which has 20 electrons?
[Ne] 3s23p63d2
[Ne] 3s23p8
[Ar] 3d2
[Ar] 4s2
[Ar] 4s2
List a possible set of four quantum numbers (n, ℓ, mℓ, ms) in order, for the highest energy electron in gallium, Ga. Refer to the periodic table as necessary.
4,1,-1,+1/2
Which set of four quantum numbers corresponds to an electron in a 4p orbital?
n=4,l=2,ml=0,ms=12
n=4,l=4,ml=3,ms=−12
n=4,l=1,ml=0,ms=12
n=4,l=3,ml=3,ms=−12
n=4,l=1,ml=0,ms=12
Choose the correct electron configuration for S
1s22s22p63s23p4
1s22s22p4
1s22s22p63p4
3s23p4
1s22s22p63s23p4
Determine the number of unpaired electrons for argon.
0
How many orbitals are there in the third shell (n=3)?
9
What element is represented by the electron configuration [Ar]4s23d8?
Ca
Pd
Ni
Co
Ni
Which statement is true?

An orbital that does not penetrate into the region occupied by core electrons is less shielded from nuclear charge than an orbital that penetrates and will therefore have a lower energy.

An orbital that does not penetrate into the region occupied by core electrons is less shielded from nuclear charge than an orbital that penetrates and will therefore have a higher energy.

An orbital that does not penetrate into the region occupied by core electrons is more shielded from nuclear charge than an orbital that penetrates and will therefore have a lower energy.

An orbital that does not penetrate into the region occupied by core electrons is more shielded from nuclear charge than an orbital that penetrates and will therefore have a higher energy.
An orbital that does not penetrate into the region occupied by core electrons is more shielded from nuclear charge than an orbital that penetrates and will therefore have a higher energy.
Elements 35 and 53 have similar chemical properties.Based on their electronic configurations predict the atomic number of a heavier element that also should have these chemical properties.
85
A certain element forms an ion with 54 electrons and a charge of +2. Identify the element.
Ba
number of valence electrons in each of the following elements. Ba
2
number of valence electrons in each of the following elements. Cs
1
number of valence electrons in each of the following elements. Ni
10
number of valence electrons in each of the following elements. P
5
What is the charge of the ion most commonly formed by Br?

+
−
2+
2−
-
Based on periodic properties, what two elements would you expect to be most like carbon?
Si Ge
Ca
Express your answer as an ion.
Ca2+
Cl
Express your answer as an ion.
Cl-
Br
Express your answer as an ion.
Br-
Na
Express your answer as an ion.
Na+
specifying an orbital
n≥1.
0≤l<n.
−l≤ml≤l.
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