Chem Ch 3
An electron in a 4p orbital can have a wave function with which of the following set of quantum numbers, (n, l, ml, ms)?
(4, 1, -1, -1/2)
Calculate the frequency of light associated with the transition from in the hydrogen atom.
4.57 × 1014 s-1
The ________ subshell contains only one orbital.
4s
What is the de Broglie wavelength of a 300. g object moving at a velocity of 25.0 m/s (about 100 mph)?
8.84 × 10-35 m
Which group in the periodic table contains only nonmetals?
8A
There are ________ orbitals in the third shell.
9
List all the elements that have a ground-state configuration with five unpaired electrons in the 3d subshell.
Cr and Mn
For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy? A) 7f → 5d B) 2p → 6d C) 2s → 3p D) 6p → 4s
D) 6p → 4s
Of the following, only ________ is not a metalloid. A) Si B) B C) As D) Po E) Ge
D) Po
Which of the following does not have their valence electrons in the same shell? A) As B) Br C) Ga D) S
D) S
Which one of the following orbitals can hold two electrons? A) 4dxy B) 3s C) 2px D) all of the above E) none of the above
D) all of the above
Identify the isoelectronic elements. A) Ne, Ar, Kr, Xe, He B) Zn2+, Co2+, Cu2+, Cr2+, Cd2+ C) Cl-, F-, Br-, I-, At- D) N3-, S2-, Br-, Cs+, Sr2+ E) P3-, S2-, C1-, K+, Ca2+
E) P3-, S2-, C1-, K+, Ca2+
No two electrons can have the same four quantum numbers is known as (the)
Pauli exclusion principle.
Which orbitals have two nodal planes passing through the nucleus?
d
The photoelectric effect is ________
the ejection of electrons by a metal when struck with light of sufficient energy
The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X?
transition metal
A sunburn is caused by overexposure to ________ radiation.
ultraviolet
Lithium is a ________ and magnesium is a ________.
metal and metal
Potassium is a ________ and chlorine is a ________.
metal, nonmetal
Arrange the following spectral regions in order of increasing energy:infrared, microwave, ultraviolet, visible.
microwave < infrared < visible < ultraviolet
According to the Balmer-Rydberg equation, electromagnetic radiation with the shortest wavelength will be emitted when an electron undergoes which of the following transitions?
n = 2 → m = 1
For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular momentum quantum number, l?
n = 4 and l = 1
Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a one-electron system (such as hydrogen)?
n only
When a bromine atom forms the bromide ion, it has the same charge as the ________ ion. A) nitrate B) ammonium C) sulfide D) sulfite E) phosphate
nitrate
Elements in Group 8A are known as the ________.
noble gases
What is the general valence-electron ground-state electron configuration for neutral alkaline earth metals?
ns2
Which of the following represent electron configurations that violate the Pauli exclusion principle? (A) [Ne]3s13p5 (B) [Kr]4d125s25p6 (C) [Ar]3d104s24p2
only (B)
Which of the above fourth-shell orbitals is a 4dx2-y2 orbital
orbital d
For a multielectron atom, a 3s orbital lies lower in energy than a 3p orbital because
other electrons more effectively shield electrons in the 3p orbital from the nucleus.
All of the orbitals in a given subshell have the same value as the ________ quantum number.
principal
What color of visible light has the longest wavelength?
red
Two electromagnetic waves are represented below.' If wave (a) represents green light, wave (b) might represent
red light.
The intensity of a beam of light is related to its
relative number of photons.
What are the possible orbitals for n = 3?
s, p, d
Elements in the same group of the periodic table typically have ________.
similar physical and chemical properties
The subshell designations follow the alphabet after f. What is the first shell in which an h orbital would be allowed?
sixth
A spectrum containing only ________ wavelengths is called a line spectrum.
specific
The spheres below represent atoms of Li, Be, B, and F (not necessarily in that order). Which one of these spheres represents an atom of F?
sphere (a)
All of the following are a result from the solution of the Schrodinger equation except ________.
spin
What are the possible values of l if n = 5?
0, 1, 2, 3, or 4
Fluorine forms an ion with a charge of ________.
1-
Calculate the wavelength of light associated with the transition from n=1 to n=3 in the hydrogen atom.
103 nm
How many h orbitals are allowed in a given shell?
11
Give the ground state electron configuration for F⁻.
1s2 2s2 2p6
Which is the correct electron configuration for an oxide ion?
1s2 2s2 2p6
Give the complete electronic configuration for nitrogen.
1s2 2s2 2px1 2py1 2pz1
How many valence electrons do the alkaline earth metals possess?
2
The first shell in the ground state of a krypton atom can contain a maximum of ________ electrons.
2
What is the first ionization energy for a hydrogen atom in the ground state? The Rydberg constant is .
2.18 × 10-18 J
What is the de Broglie wavelength of an electron (m = 9.11 × 10-31 kg) moving at a velocity of (10% of the speed of light)?
2.4 × 10-11 m
The principal quantum number of the first d subshell is ________.
3
What value of l is represented by a f orbital?
3
Electromagnetic radiation travels through vacuum at a speed of ________ m/s.
3.00 × 108
Which of the following statements is TRUE? A) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. B) All orbitals in a given atom are roughly the same size. C) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. D) We can sometimes know the exact location and speed of an electron at the same time. E) All of the above are true.
A) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.
Of the following, which atom has the largest atomic radius? A) K B) Cl C) Na D) Br
A) K
Which metal does not form cations of differing charges? A) Na B) Sn C) Co D) Cu E) Fe
A) Na
The element ________ is the most similar to helium in chemical and physical properties.
Ar
Place the following in order of increasing IE1.
As < N < F
Electrons filling up the orbitals from low to high is known as (the)
Aufbau principle.
Which of the following elements has a ground-state electron configuration different from the predicted one? A) Ca B) Cu C) Ti D) Cl E) Xe
B) Cu
Which of the following is not quantized? A) the charge on a monatomic ion B) the distance between two objects C) the static charge on a balloon rubbed with wool D) the population of the United States
B) the distance between two objects
Which has the highest Zeff for its valence electrons? A) Na B) Cl C) Mg D) Si
B) Cl
Which atom in each group (I and II) has the smallest atomic radius? (I)Rb, Zr, I(II)Sb, N, As A) Rb; Sb B) Te; Sb C) Rb; As D) Te; As
B) Te; Sb
Which have the largest number of unpaired electrons in p orbitals in their ground-state electron configurations? A) B, Ga, Tl B) F, At, Br C) N, As, Bi D) Ne, Ar, Xe
C) N, As, Bi
Which of the following statements is TRUE? A) The angular momentum quantum number (l) describes the the size and energy associated with an orbital. B) The principal quantum number (n) describes the shape of an orbital. C) The magnetic quantum number (ml) describes the orientation of the orbital. D) An orbital is the path that an electron follows during its movement in an atom. E) All of the above are true.
C) The magnetic quantum number (ml) describes the orientation of the orbital.
Which pair of elements is most apt to form a molecular compound with each other? A) magnesium, iodine B) aluminum, oxygen C) sulfur, fluorine D) barium, bromine E) potassium, lithium
C) sulfur, fluorine
Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? A) 2p B) 2s C) 2d
C) 2d
Which of the compounds, C5H12, CaF2, Pd(NO3)2, OCl2, are expected to exist as molecules?
C5H12 and OCl2
Which group 1A element is not a metal?
H
________ does not combine with any other element.
Helium
When filling degenerate orbitals, electrons fill them singly first, with parallel spins. This is known as (the)
Hund's rule.
According to the Bohr model, when a hydrogen electron makes a transition from n=4 to n=2, which of the following statements is true? I.Energy is emitted. II.Energy is absorbed. III.Electrons lose energy. IV.Electrons gain energy.
I and III
Magnesium reacts with a certain element to form a compound with the general formula MgX. What would the most likely formula be for the compound formed between potassium and element X?
K2X
Which of the following quantum numbers describes the shape of an orbital?
angular momentum quantum number
The ground-state electron configuration of the element ________ is [Kr]5s14d5.
Mo
In which set do all elements tend to form anions in binary ionic compounds?
N, O, Cl
Which of the following is the correct chemical formula for a molecule of nitrogen?
N2
The solid compound, Na2CO3, contains
Na+ ions and CO3 2-ions.
The solid compound, Na4SiO4, contains
Na+ ions and SiO44- ions.
Which two elements have the same ground-state electron configuration?
No two elements have the same ground-state electron configuration.
Which statement is false? A) The 4s orbital lies lower in energy than the 3d orbital for atoms K, Ca, Sc, and Ti. B) For any atom, the 4s orbital lies lower in energy than the 5s orbital. C) For a hydrogen atom, a 4s orbital, a 4p orbital, and a 4d orbital all have the same energy. D) The 4s orbital lies lower in energy than the 3d orbital for Cu and Fe2+.
The 4s orbital lies lower in energy than the 3d orbital for Cu and Fe2+. (THIS IS NOT TRUE)
The n = 2 to n = 6 transition in the Bohr hydrogen atom corresponds to the ________ of a photon with a wavelength of ________ nm
absorption, 410
Elements in Group 1A are known as the ________.
alkali metals
________, used to destroy molecules within unwanted cells such as cancer cells, are called ionizing radiation.
X-rays and gamma rays
What is the correct ground state electron configuration for chromium?
[Ar]4s13d5
What is the ground-state electron configuration of tellurium?
[Kr]4d105s25p4
Give the ground state electron configuration for Pb.
[Xe]6s2 4f14 5d10 6p2
Which of the following elements would you predict to have an anomalous electron configuration? A)W B)Mg C)Al D)Sb
a) W
Calcium is a ________ and silver is a ________.
metal and metal
An element that appears in the lower left corner of the periodic table is ________.
definitely a metal
The n = 5 to n = 3 transition in the Bohr hydrogen atom corresponds to the ________ of a photon with a wavelength of ________ nm.
emission, 1280
The angular momentum quantum number is 3 in ________ orbitals.
f
Which of the following is true? The probability density
for all s orbitals is independent of direction from the nucleus.
The vertical columns of the periodic table are called
groups.
If two electrons in the same atom have the same value of l, they are
in the same sublevel, but not necessarily in the same level.
The heat that is felt from a hot object is called ________ radiation.
infrared
The definitive distinction between ionic bonding and covalent bonding is that
ionic bonding involves a transfer of electrons and covalent bonding involves a sharing of electrons.
For an electron in a given atom, the larger n, the
larger the average distance from the nucleus and the higher the orbital energy.
Wave (b) has the
lower amplitude and weaker intensity than wave (a).
The wave characteristics of a large, moving object, such as an automobile, are difficult to observe because the
wavelength is very small.