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Chemistry
Q:
The Cr2+ion would be expected to have ____ unpaired electrons.
A) 4
B) 2
C) 3
D) 0
E) 1
Q:
What is the electron configuration for ?
A) B) C) D) E)
Q:
What is the ground-state electron configuration of the sulfide ion?
A) B) C) D) E)
Q:
What is the ground-state electron configuration of the ion?
A) B) C) D) E)
Q:
The formation of which monatomic ion of sulfur is the most energetically favorable?
A) B) C) D) E)
Q:
All of the following have ground-state noble-gas electron configurations exceptA) ArB) N3-C) P3+D) Mg2+E) Cl-
Q:
An unknown element, X, reacts with oxygen to form two oxides with the general formula X2O3 and X2O5. The pure element is strongly paramagnetic, and the oxides are amphoteric. Which of the following elements could be represented by X?
A) Sc
B) Na
C) Bi
D) S
E) Sb
Q:
The element selenium is in the same group as sulfur. Which of the following is the formula of selenous acid?
A) B) C) D) E)
Q:
The element antimony is in the same group as phosphorus. Which of the following is the formula of antimonous acid?
A) B) C) D) E)
Q:
A few atoms of the new element 113 were created in 2004 by a team of Russian and American scientists. It has been given the temporary name "ununtrium" and the temporary symbol "Uut." Based on ununtrium's position on the periodic table, what type of oxide(s) should it form?
A) Ununtrium should form a basic oxide with the formula Uut2O3.
B) Ununtrium should form an amphoteric oxide with the formula UutO.
C) Ununtrium should form an acidic oxide with the formula Uut2O3.
D) Ununtrium should form two acidic oxides having the formulas Uut2O and Uut2O3.
E) Ununtrium should form two basic oxides having the formulas Uut2O and Uut2O3.
Q:
Which element forms the most acidic oxide?
A) B
B) Tl
C) Al
D) In
E) Ga
Q:
Sodium and potassium have similar chemical and physical properties. This is best explained by the fact that both elements
A) have the same ground-state valence-electron configuration.
B) have low relative atomic masses.
C) are in Period 1 of the periodic table.
D) have relatively low first ionization energies.
E) are active metals.
Q:
Which of the following are incorrectly paired?
A) Group IIA, alkaline earth metals
B) Group IA, alkali metals
C) Group VIIIA, noble gases
D) Group IVA, halogens
E) Group VIA, chalcogens
Q:
Which of the following statements is true concerning a concentrated solution of lithium oxide in water?
A) The resulting solution is strongly basic.
B) The resulting solution is weakly acidic.
C) The resulting solution is neither acidic nor basic.
D) The resulting solution is weakly basic.
E) The resulting solution is strongly acidic.
Q:
Which of the following ground-state electron configurations corresponds to an atom that has the most negative value of the electron affinity?
A) 1s22s22p63s1
B) 1s22s22p63s23p5
C) 1s22s22p63s23p2
D) 1s22s22p63s23p63d54s2
E) 1s22s22p6
Q:
Which of the following forms the most stable anion in the gas phase?
A) Br (electron affinity = -325 kJ/mol)
B) I (electron affinity = -295 kJ/mol)
C) Te (electron affinity = -190 kJ/mol)
D) C (electron affinity = -122 kJ/mol)
E) As (electron affinity = -77 kJ/mol)
Q:
According to the general trend in electron affinities, which group (or family) of elements tend to form the most stable anions in the gas phase?
A) noble gases
B) halogens
C) transition metals
D) alkaline earth metals
E) alkali metals
Q:
An atom of which of the following elements has the most negative electron affinity?
A) Rb
B) As
C) Cl
D) Br
E) Se
Q:
Which of the following statements is true about the ionization energy of Mg+?
A) It will be equal to and opposite in sign to the electron affinity of Mg+.
B) It will be equal to and opposite in sign to the electron affinity of Mg.
C) It will be equal to and opposite in sign to the electron affinity of Mg2+.
D) It will be equal to the ionization energy of Li.
E) none of the above
Q:
The change in energy for which of the following processes corresponds to the electron affinity of iodine?
A) B) C) D) E)
Q:
The electron affinity value expected for the process would be
A) a small negative number.
B) a large positive number.
C) a small positive number.
D) a large negative number.
E) zero.
Q:
Rank the following ions in order of increasing first ionization energy: O2-, Mg2+,F-, Na+.A) Mg2+ < Na+ < F- < O2-B) Mg2+ < O2- < Na+ < F-C) O2- < F- < Mg2+ < Na+D) O2- < F- < Na+ < Mg2+E) O2- < Mg2+ < F- < Na+
Q:
Which of the following ground-state electron configurations corresponds to an atom having the largest ionization energy?
A) [Ar]3d104s24p3
B) [Ne]3s23p3
C) [Ne]3s23p2
D) [Kr]4d105s25p3
E) [Xe]4f145d106s26p3
Q:
An atom of which of the following elements has the largest second ionization energy?
A) Na
B) Cl
C) S
D) Si
E) Mg
Q:
An atom of which of the following elements has the largest first ionization energy?
A) Ca
B) Rb
C) Ge
D) Cl
E) P
Q:
An atom of which of the following elements has the smallest first ionization energy?
A) Rb
B) Si
C) F
D) As
E) Ca
Q:
An atom of which of the following elements has the largest first ionization energy?
A) N
B) Sb
C) As
D) P
E) Bi
Q:
An atom of which of the following elements has the smallest first ionization energy?
A) Sn
B) Pb
C) Ge
D) C
E) Si
Q:
An atom of which of the following elements has the largest ionization energy?
A) Te
B) Sn
C) Sb
D) I
E) Rb
Q:
An atom of which of the following elements has the smallest ionization energy?
A) I
B) Sb
C) Sn
D) Rb
E) Te
Q:
An atom of which of the following elements has the highest fourth ionization energy?
A) Al
B) Se
C) Si
D) Ga
E) As
Q:
The change in energy for which of the following processes corresponds to the second ionization energy of barium?
A) B) C) D) E)
Q:
The change in energy for which of the following processes represents the first ionization energy of bromine?
A) B) C) D) E)
Q:
The change in energy for which of the following processes corresponds to the first ionization energy of calcium?
A) B) C) D) E)
Q:
The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is
A) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that oxygen has one doubly occupied 2p orbital and nitrogen does not.
B) consistent with the general trend relating changes in ionization energy across a period from left to right because it is harder to take an electron from an oxygen atom than from a nitrogen atom.
C) consistent with the general trend relating changes in ionization energy across a period from left to right because it is easier to take an electron from an oxygen atom than from a nitrogen atom.
D) incorrect.
E) inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that the oxygen atom has two doubly occupied 2p orbitals and nitrogen has only one.
Q:
Which of the following properties, in general, increases from left to right across a period in the periodic table?
A) ionic charge
B) atomic radius
C) density
D) ionization energy
E) metallic character
Q:
Below are data on the first four ionization energies for a fictitious element X.
First ionization energy = 500 kJ/mol
Second ionization energy = 2000 kJ/mol
Third ionization energy = 3500 kJ/mol
Fourth ionization energy = 25000 kJ/mol
From the data, which of the following statements is incorrect?
A) The third ionization energy is greater than the second ionization energy because X2+ has a bigger charge than X+.
B) X could belong to Group IIIA.
C) X could belong to Group IIIB.
D) X could belong to group VA.
E) The fourth ionization energy is much greater than the third ionization energy because X3+ consists of a noble-gas core or a pseudo-noble-gas core.
Q:
Rank the following atoms in order of the largest to smallest atomic radius: Al, P, Cl, K.
A) K > Al > P > Cl
B) Al > K > P > Cl
C) P > Al > K > Cl
D) Al > P > Cl > K
E) K > P > Al > Cl
Q:
In which of the series of elements listed below would the elements have most nearly the same atomic radius?
A) Na, K, Rb, Cs
B) F, Cl, Br, I
C) Na, Mg, Al, Si
D) Sc, Ti, V, Cr
E) B, Si, As, Te
Q:
An atom of which of the following elements has the largest atomic radius?
A) Ge
B) K
C) Cl
D) Ca
E) As
Q:
An atom of which of the following elements has the smallest atomic radius?
A) Cl
B) Rb
C) Ca
D) Si
E) As
Q:
An atom of which of the following elements has the largest atomic radius?
A) As
B) Sb
C) P
D) Bi
E) N
Q:
An atom of which of the following elements has the smallest atomic radius?
A) At
B) F
C) I
D) Br
E) Cl
Q:
An atom of which of the following elements has the largest atomic radius?
A) Cl
B) P
C) Na
D) S
E) Si
Q:
An atom of which of the following elements has the smallest atomic radius?
A) Sb
B) I
C) Te
D) Rb
E) Sn
Q:
A section of the periodic table with all identification features removed is shown below.V W X Y ZWhich element has the smallest atomic radius?A) WB) YC) XD) ZE) V
Q:
Which of the following statements is true?
A) The krypton 1s orbital is smaller than the helium 1s orbital because krypton's nuclear charge draws the electrons closer.
B) The krypton 1s orbital is smaller than the helium 1s orbital because krypton's p and d orbitals crowd the s orbitals.
C) The krypton 1s orbital and the helium 1s orbital are the same size because both s orbitals can have only two electrons.
D) The krypton 1s orbital is larger than the helium 1s orbital because krypton contains more electrons.
E) The krypton 1s orbital is larger than the helium 1s orbital because krypton's ionization energy is lower so it's easier to remove electrons.
Q:
In general, atomic radii
A) decrease from left to right in a period and increase down a group.
B) increase from left to right in a period and decrease down a group.
C) do not change across a period or a group.
D) decrease from left to right and decrease down a group.
E) increase from left to right in a period and increase down a group.
Q:
When arranged in order of increasing atomic number, the elements exhibit periodicity for all the following properties except
A) electron affinity.
B) color.
C) ionization energy.
D) electron configuration.
E) atomic radius.
Q:
Which of the following elements would be expected to have chemical and physical properties most similar to those of the bromine (Br)?
A) chlorine (Cl)
B) neon (Ne)
C) gallium (Ga)
D) calcium (Ca)
E) lead (Pb)
Q:
Which of the following species would be expected to have chemical properties most similar to those of the nitrogen atom?
A) nitride ion
B) nitrite ion
C) phosphate ion
D) phosphide ion
E) phosphorus atom
Q:
Which of the following statements concerning the periodic table is incorrect?
A) The elements in a given group or family have similar chemical properties.
B) The chemical characteristics of the elements are periodic functions of their atomic numbers.
C) All the elements are arranged in order of increasing atomic weight.
D) Mendeleev left spaces in his periodic table for undiscovered elements.
E) Mendeleev received most of the credit for the early development of the periodic table.
Q:
Who was the first chemist to recognize patterns in chemical properties of the elements?
A) Bohr
B) Dobereiner
C) Meyer
D) Mendeleev
E) Newlands
Q:
Which of the following atoms is paramagnetic in its ground state?
A) tin (Sn)
B) barium (ba)
C) cadmium (Cd)
D) ytterbium (Yb)
E) argon (Ar)
Q:
Which of the following orbital diagrams represents a paramagnetic atom?
1s 2s 2p
A) B) C) D) E)
Q:
The ground-state electron configuration of a . Therefore, is
A) paramagnetic with four unpaired electrons.
B) diamagnetic.
C) paramagnetic with one unpaired electron.
D) paramagnetic with five unpaired electrons.
E) paramagnetic with three unpaired electrons.
Q:
Which of the following orbital diagrams represents a diamagnetic atom?
1s 2s 2p
A) B) C) D) E)
Q:
Which of the following orbital diagrams represent(s) a paramagnetic atom?
1s 2s 3s
1) 2) 3) A) 3 only
B) 2 and 3
C) 1 only
D) 1 and 2
E) 2 only
Q:
An atom of which of the following elements is not diamagnetic in the ground state?
A) Ca
B) Rn
C) All are diamagnetic.
D) Cd
E) Pt
Q:
Fe has ____ that is(are) unpaired in its d orbitals.
A) 2 electrons
B) 3 electrons
C) 1 electron
D) 4 electrons
E) none of these
Q:
How many unpaired electrons are found in the ground state electron configuration of selenium (Se)?
A) 2
B) 3
C) 5
D) 0
E) 1
Q:
The element whose atoms in the ground state have two half-filled orbitals is
A) Na.
B) Be.
C) Tl.
D) Po.
E) Sb.
Q:
Which principle or rule is violated by the following orbital diagram of an atom in its ground state?
1s 2s 2p A) Heisenberg uncertainty principle
B) No rules or principles are violated by this orbital diagram.
C) aufbau principle
D) Hund's rule
E) Pauli exclusion principle
Q:
The statement that "the lowest-energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals" is known as
A) the aufbau principle.
B) Hund's rule.
C) the Pauli exclusion principle.
D) Heisenberg uncertainty principle.
E) the quantum model.
Q:
What is the valence-shell electron configuration for the fourth-period element in Group VA?
A) B) C) D) E)
Q:
An element that has the same ground state valence-shell electron configuration as indium is
A) boron.
B) silicon.
C) krypton.
D) lithium.
E) barium.
Q:
Which of the following sets of four quantum numbers (n,l, ml, ms) correctly describes an electron occupying a d orbital of an element in the third row of the transition metals?A) 4 2 2 +B) 5 2 1 -C) 5 3 -1 D) 4 1 0 -E) 5 0 0 -
Q:
The angular momentum quantum number of the two highest-energy valence electrons in an atom of germanium is
A) 4.
B) 0.
C) 1.
D) 2.
E) 3.
Q:
The quantum numbers of an atom's highest-energy valence electrons are n = 5 and l = 1. The element to which this atom belongs could be a
A) inner transition metal.
B) alkali metal.
C) s-block main-group element.
D) transition metal.
E) p-block main-group element.
Q:
The elements that are filling the 5f subshell are called
A) alkali metals.
B) transition elements.
C) lanthanides.
D) actinides.
E) main-group elements.
Q:
If the electron could have a third spin state (that is, , -, and 0), what would be the ground-state electron configuration of carbon?A) 1s22s4B) 1s22s32p1C) 1s32s3D) 1s22s22p2E) 1s32s22p1
Q:
What noble gas core would be used when writing the ground state electron configuration for tungsten (W)?
A) [Xe]
B) [Rn]
C) [Kr]
D) [Ar]
E) [Ne]
Q:
What is the ground-state electron configuration of sulfur (S)?
A) B) C) D) E)
Q:
What is the ground-state electron configuration of terbium (Tb)?
A) 1s22s22p63s23p63d104s24p64d105s25p65d96s2
B) 1s22s22p63s23p63d104s24p64d104f145s25p3
C) 1s22s22p63s23p63d104s24p64d105s25p65d106s1
D) 1s22s22p63s23p63d104s24p64d94f105s25p66s2
E) 1s22s22p63s23p63d104s24p64d104f95s25p66s2
Q:
What is the ground-state electron configuration of tantalum (Ta)?
A) 1s22s22p63s23p64s24p64d104f145s25p3
B) 1s22s22p63s23p63d104s24p64d105s25p3
C) 1s22s22p63s23p63d104s24p64d104f145s25p65d36s2
D) 1s22s22p63s23p63d104s24p64d105s25p65d3
E) 1s22s22p63s23p63d104s24p64d104f3
Q:
Which of the following sets of four quantum numbers (n,l, ml, ms) correctly describes one of the valence electrons in a ground-state radium atom?
A) 7 1 0 B) 6 1 1 C) 7 2 0 D) 7 2 0 E) 7 0 0 +
Q:
How many valence electrons does an arsenic atom have?
A) 5
B) 8
C) 7
D) 2
E) 33
Q:
Which ground-state electron configuration is incorrect?
A) B) C) D) E)
Q:
What is the total number of electrons in p orbitals in a ground-state vanadium atom?
A) 6
B) 18
C) 12
D) 24
E) 30
Q:
All of the following ground-state electron configurations are correct except
A) .
B) .
C) .
D) .
E) .