Chem FInal
How many of the following elements have 1 unpaired electron in the ground state? B Al O Cl 2 1 4 3
3
How many of the following molecules have sp3d2 hybridization on the central atom? SeCl6, XeF4, IF5, AsBr5 1 4 0 2 3
3
How many unpaired electrons are present in the ground state As atom? 4 2 1 0 3
3
How many valence electrons does an atom of Al possess? 2 1 8 3 5
3
Identify the number of electron groups around a molecule with sp2 hybridization. 5 1 2 3 4
3
What is the maximum number of p orbitals that are possible? 9 7 1 3 5
3
Calculate the frequency of the red light emitted by a neon sign with a wavelength of 690 nm. 2.30 × 1014 s-1 5.05 × 1014 s-1 4.35 × 1014 s-1 3.45 × 1014 s-1 3.90 × 1014 s-1
4.35 × 1014 s-1
Part complete What are the electron and molecular geometries, respectively, for hydrogen sulfide, H2S? View Available Hint(s) Electron geometry is tetrahedral. Molecular geometry is linear. Electron geometry is bent. Molecular geometry is tetrahedral. Electron geometry is linear. Molecular geometry is bent. Electron geometry is tetrahedral. Molecular geometry is bent.
Electron geometry is tetrahedral. Molecular geometry is bent.
Which element has the ground-state electron configuration [Xe]6s 2 4f 7? Eu Gd Re Ir
Eu
Draw the best Lewis structure for Cl3-. What is the formal charge on the central Cl atom? 0 -1 +1 +2 -2
-1
How many unpaired electrons are present in the ground state Kr atom? 0 2 1 5 3
0
In the best Lewis structure for NO +, what is the formal charge on the N atom? +1 +2 -1 0
0
For n = 3, what are the possible sublevels? 0, 1 0, 1, 2 0 0, 1, 2, 3
0, 1, 2
What are the possible values of l if n = 6? 6 0, 1, 2, 3, 4, or 5 -4, -3, -2, -1, 0, +1, +2, +3, or +4 -5, -4, -3, -2, -1, 0, +1, +2, +3, +4, or +5
0, 1, 2, 3, 4, or 5
What values of l are possible for n = 3? 0 (or s ) 0 and 1 (or s and p ) 0, 1, and 2 (or s, p, and d ) 0, 1, 2, and 3 (or s, p, d, and f )
0, 1, and 2 (or s, p, and d )
How many lone pairs of electrons are on the S atom in SF4 ? 3 1 0 2
1
How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3 3 2 1 0 4
1
How many of the following species are paramagnetic? Sc3+ Cl- Ba2+ Se 2 0 3 1 4
1
How many unpaired electrons are there in the ground state of Cl? 2 4 1 3 5
1
How many valence electrons do the alkali metals possess? 1 2 7 6 8
1
How many valence electrons does an atom of Ag possess? 3 1 11 2 5
1
What is the maximum number of orbitals that are possible in the s sublevel? 3 5 9 1 7
1
A single covalent bond contains ________ of electrons. 2 pairs 4 pairs 3 pairs 0 pairs 1 pair
1 pair
Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m/s. 7.60 × 10-36 m 3.57 × 10-32 m 2.15 × 10-32 m 2.68 × 10-34 m 1.32 × 10-34 m
1.32 × 10-34 m
Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s. 5.52 × 10-9 m 1.99 × 10-10 m 2.76 × 10-9 m 5.03 × 10-10 m 1.81 × 10-10 m
1.99 × 10-10 m
The bond angle in H2O is 120° 109.5° 104.5° 95° 107°
104.5°
The bond angle in NH3 is 107° 95° 120° 109.5° 104.5°
107°
Give the approximate bond angle for a molecule with a tetrahedral shape. 180° 109.5° 90° 105° 120°
109.5°
What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75 × 1014 Hz? 110 kJ 219 kJ 457 kJ 182 kJ 326 kJ
110 kJ
Give the number of pairs of valence electrons for BF3. 12 14 10 16 8
12
Give the approximate bond angle for a molecule with a trigonal planar shape. 105° 180° 45° 109.5° 120°
120°
How many orbitals are there in the fourth shell? 4 3 16 6
16
Give the approximate bond angle for a molecule with a linear shape. 90° 180° 109.5° 120° 105°
180°
Give the electron configuration for O. 1s22s22p4 1s22p4 1s22s12p1 1s22s22p5 1s22s22p3
1s22s22p4
Give the ground state electron configuration for Mg2+. 1s22s22p63s2 1s22s22p63s1 1s22s22p63s23p2 1s22s22p6 1s22s22p63s23p6
1s22s22p6
Give the complete electronic configuration for Ca2+. 1s22s22p63s23p5 1s22s22p63s23p6 1s22s2p63s2p6 1s22s22p63s24p6 1s22s23p64s25p6
1s22s22p63s23p6
Give the complete electronic configuration for S2-. 1s22s23p64s25p6 1s22s22p63s23p6 1s22s2p63s2p6 1s22s22p63s24p6 1s22s22p63s23p5
1s22s22p63s23p6
The complete electron configuration of argon, element 18, is ________. 1s22s22p103s23p2 1s42s42p63s4 1s62s62p23s4 1s22s22p63s23p6 1s42s42p10
1s22s22p63s23p6
The complete electron configuration of gallium, element 31, is ________. 1s42s42p103s43p9 1s42s42p83s43p84s3 1s42s42p63s43p64s43d3 1s22s22p63s23p63d104s24p1 1s22s22p103s23p104s23d3
1s22s22p63s23p63d104s24p1
Place the following in order of increasing metallic character. Rb Cs K Na Cs < Rb < K < Na Na < Rb < Cs < K Na < K < Rb < Cs K < Cs < Na < Rb K < Cs < Rb < Na
Na < K < Rb < Cs
Place the following in order of increasing radius. Br- Na+ Rb+ Na+ < Rb+ < Br- Rb+ < Br- < Na+ Br- < Na+ < Rb+ Br- < Rb+ < Na+ Rb+ < Na+ < Br-
Na+ < Rb+ < Br-
Choose the paramagnetic species from below. Cd O2- Ca Zn2+ Nb3+
Nb3+
Which element has the highest first electron affinity? Mg Ne Na O
O
Which of the following elements can form compounds with an expanded octet? Li Se F C All of the above elements can form compounds with an expanded octet.
Se
The condensed electron configuration of krypton, element 36, is ________. [Ar]4s4 [Kr]4s43d8 [Ar]4s43d4 [Kr]4s23d8 [Ar]3d104s24p6
[Ar]3d104s24p6
Choose the ground state electron configuration for Ti 2 +. [Ar]4s2 3d4 [Ar]4s2 3d2 [Ar] 4d2 [Ar]4s2 [Ar]3d2
[Ar]3d2
Give the ground state electron configuration for Se. [Ar]4s23d104p6 [Ar]4s24d104p4 [Ar]4s23d104p4 [Ar]3d104p4 [Ar]4s23d10
[Ar]4s23d104p4
Give the ground state electron configuration for Br-. [Ar]4s24p6 [Ar]4s24d104p6 [Ar]4s23d104p4 [Ar]4s23d104p5 [Ar]4s23d104p6
[Ar]4s23d104p6
Give the ground state electron configuration for Rb+. [Kr]5s2 [Ar]4s24p6 [Kr]5s1 [Kr]5s24d2 [Ar]4s23d104p6
[Ar]4s23d104p6
Give the ground state electron configuration for Sr. [Kr]5s24d2 [Kr]5s25d105p2 [Kr]5s24d105p2 [Kr]5s24d10 [Kr]5s2
[Kr]5s2
Give the ground state electron configuration for Cd. [Kr]5s24d105p2 [Kr]4d10 [Kr]5s25d10 [Kr]5s24d8 [Kr]5s24d10
[Kr]5s24d10
Give the ground state electron configuration for I. [Kr]5s25d105p6 [Kr]5s25p6 [Kr]5s24d105p6 [Kr]4d105p6 [Kr]5s24d105p5
[Kr]5s24d105p5
The condensed electron configuration of silicon, element 14, is ________. [Ne]2p10 [He]2s62p2 [Ne]3s23p2 [He]2s42p6 [He]2s4
[Ne]3s23p2
Give the ground state electron configuration for Pb. [Xe]6s25d106p2 [Xe]6s24f145d106p2 [Xe]6s26p2 [Xe]6s24f145d106s26p2 [Xe]6s25f146d106p2
[Xe]6s24f145d106p2
Give the complete electronic configuration for Br-. 1s22s22p63s23p64s24d104p6 1s22s22p63s23p64s23d104p5 1s22s22p63s23p64s23d104p6 1s22s22p63s23p64s24p6 1s22s2p63s2p64s23d104p6
1s22s22p63s23p64s23d104p6
Give the complete electronic configuration for Mn. 1s22s22p63s23p64s24d5 1s22s22p63s23p64s23d5 1s22s22p63s23p64s13d6 1s22s22p63s23p64s24p5
1s22s22p63s23p64s23d5
Give the number of valence electrons for Cd. 6 12 10 8 2
2
How many of the following molecules are polar? XeO2, SiCl2F2, C2Br2, SeF6 4 0 1 3 2
2
How many of the following species are diamagnetic? Fr Zr2+ Al3+ Hg2 0 2 4 1 3
2
How many sublevels are contained in the second shell (n = 2) of a given atom? 9 4 3 2 1
2
How many subshells are there in the shell with n = 2? 2 3 4 1
2
How many unpaired electrons are present in the ground state C atom? 1 4 2 3 5
2
How many valence electrons do the alkaline earth metals possess? 1 7 2 6 8
2
How many valence electrons does an atom of Mg possess? 5 8 2 1 3
2
How many valence electrons does an atom of Ti possess? 6 8 0 4 2
2
Identify the number of electron groups around a molecule with sp hybridization. 5 1 2 3 4
2
What value of l is represented by a d orbital? 1 2 0 3
2
Identify the number of bonding pairs and lone pairs of electrons in water. 2 bonding pairs and 1 lone pair 3 bonding pairs and 2 lone pairs 1 bonding pair and 1 lone pair 1 bonding pair and 2 lone pairs 2 bonding pairs and 2 lone pairs
2 bonding pairs and 2 lone pairs
A double covalent bond contains ________ of electrons. 1 pair 0 pairs 4 pairs 3 pairs 2 pairs
2 pairs
Give the number of valence electrons for CH2Cl2. 12 22 16 20 18
20
Determine the mass of a ball with a velocity of 35.0 m/s and a wavelength of 8.92 x 10-34 m. 594 g 26.0 g 2.07 g 47.1 g 21.2 g
21.2 g
Determine the velocity of a marble (m = 8.66 g) with a wavelength of 3.46 × 10-33 m. 38.8 m/s 52.9 m/s 22.1 m/s 2.21 m/s 45.2 m/s
22.1 m/s
Give the number of core electrons for Se. 26 32 34 30 28
28
How many different values of l are possible in the third principal level? 4 2 0 1 3
3
How many lone pairs are on the Br atom in BrCl2-? 0 1 2 3
3
How many of the following elements can form compounds with an expanded octet? I O Br Xe 1 3 2 0 4
3
How many of the following elements can form compounds with an expanded octet? P Kr Xe B 1 4 3 2 0
3
What value of l is represented by a f orbital? 1 2 3 0
3
Identify the number of bonding pairs and lone pairs of electrons in N2. 2 bonding pairs and 3 lone pairs 6 bonding pair and 1 lone pair 4 bonding pair and 2 lone pairs 2 bonding pairs and 1 lone pair 3 bonding pairs and 2 lone pairs
3 bonding pairs and 2 lone pairs
A triple covalent bond contains ________ of electrons. 4 pairs 0 pairs 1 pair 2 pairs 3 pairs
3 pairs
How many valence electrons do the noble gases possess? 8 6 1 2 7
8
How many orbitals are contained in the third principal level (n = 3) of a given atom? 9 18 3 7 5
9
Give the approximate bond angle for a molecule with an octahedral shape. 180° 105° 120° 109.5° 90°
90°
Which of the following contains an atom that does not obey the octet rule? ClF CsI ClF5 SnO2
ClF5
Identify the most reactive alkali metal with water. Na Rb Cs Li K
Cs
Of the following, which atom has the largest atomic radius? At I Rb Cs
Cs
Give the number of valence electrons for Br. 8 7 4 6 5
7
How many valence electrons do the halogens possess? 6 2 7 1 5
7
What is the maximum number of f orbitals that are possible? 3 1 5 9 7
7
Identify the compound with the smallest percent ionic character. LiF HCl HF IBr
IBr
Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The energy of one photon of this light is ________ J. 3.79 × 10-19 1.04 × 10-22 2.64 × 1018 1.04 × 10-31 3.79 × 10-28
3.79 × 10-19
Give the number of valence electrons for SO42-. 36 30 28 32 34
32
Give the number of valence electrons for SBr4. 28 32 30 34
34
Give the number of valence electrons for Si. 2 28 12 4 26
4
How many of the following elements have 2 unpaired electrons in the ground state? C Te Hf Si 2 1 3 4
4
Identify the number of electron groups around a molecule with a tetrahedral shape. 2 1 3 4 5
4
Identify the number of valence electrons for Ti. 8 4 7 2
4
Which wavelength of light has the highest frequency? 10 nm 10 mm 4 mm 4 nm
4 nm
What is the frequency of light for which the wavelength is 710 nm? View Available Hint(s) 4.2 × 1014 s −1 4.2 × 105 s −1 2.4 × 10 −6 s −1 210 s −1
4.2 × 1014 s −1
Give the number of core electrons for Cd. 46 48 44 45 47
46
How many valence electrons does an atom of As have? 4 8 3 5 6
5
Identify the number of electron groups around a molecule with a trigonal bipyramidal shape. 5 2 4 3 1
5
What is the maximum number of d orbitals that are possible? 5 7 3 1 9
5
Draw the Lewis structure for SO42-. How many equivalent resonance structures can be drawn? 8 4 3 2 6
6
Give the number of valence electrons for Se. 8 6 4 0 2
6
Identify the number of electron groups around a molecule with an octahedral shape. 4 5 3 6 2
6
If the angular momentum quantum number, l, for a given electron is two (l = 2), in what type of orbital will the electron be found? View Available Hint(s) A d-orbital An s-orbital A p-orbital You cannot determine the type of orbital from the angular momentum quantum number.
A d-orbital
Use Lewis theory to determine the chemical formula for the compound formed between Al and O. AlO2 Al3O2 AlO Al2O Al2O3
Al2O3
Which electron in sulfur is most shielded from nuclear charge? An electron in the 1s orbital An electron in the 2s orbital An electron in a 3p orbital none of the above (All of these electrons are equally shielded from nuclear charge.)
An electron in a 3p orbital
Which of the following statements is TRUE? An ionic bond is formed through the sharing of electrons. An ionic bond is much stronger than most covalent bonds. Once dissolved in water, ionic compounds rarely conduct electricity. Ionic compounds at room temperature typically conduct electricity. None of the above are true.
An ionic bond is much stronger than most covalent bonds.
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
Of the following, which atom has the smallest atomic radius? Rb As Sb K
As
Which of the following statements is TRUE? Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. We can sometimes know the exact location and speed of an electron at the same time. All orbitals in a given atom are roughly the same size. All of the above are true.
Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.
Identify the compound with atoms that have an incomplete octet. CO2 Cl2 BF3 CO ICl5
BF3
Which compound is likely to have an incomplete octet? N2O CH4 BH3 SF6
BH3
Of the following elements, which has the lowest electronegativity? At Sr Ba I
Ba
Place the following elements in order of increasing electronegativity. Ba Se Li Se < Ba < Li Ba < Li < Se Se < Li < Ba Li < Se < Ba Ba < Se < Li
Ba < Li < Se
Which of the molecules below will be polar? CS2, BF3, SO2, CH3Br View Available Hint(s) CH3Br only CS2 only Both BF3 and CH3Br Both SO2 and CH3Br
Both SO2 and CH3Br
Which property or properties of an electromagnetic wave are directly proportional to the energy of the wave? View Available Hint(s) Frequency only Amplitude only Wavelength only Both amplitude and frequency
Both amplitude and frequency
Identify the element that has a ground state electronic configuration of [Ar]4s23d104p 5 . Cl Br F I
Br
Which of the following elements can form compounds with an expanded octet? Br Li F C None of the above can form compounds with an expanded octet.
Br
Which molecule or compound below contains a pure covalent bond? Br2 SCl6 NaCl Li2CO3 PCl3
Br2
Place the following in order of decreasing metallic character. C O N F C > N > O > F F > O > N > C O > N > F > C F > N > O > C N > C > O > F
C > N > O > F
Choose the bond below that is most polar. N-O C-F Cl-Cl C-N C-C
C-F
Choose the bond below that is least polar. C-Br C-F C-I P-F C-Cl
C-I
Which of the molecules below will exhibit resonance? CO2, CO3 2−, NO3 −, O3 O3 only CO3 2− and NO3 − only CO2 only CO3 2−, NO3 −, and O3
CO3 2−, NO3 −, and O3
Of the following, which element has the highest first ionization energy? P Na Cl Al
Cl
Place the following elements in order of increasing atomic radius. P Ba Cl Cl < Ba < P Ba < Cl < P Ba < P < Cl Cl < P < Ba P < Cl < Ba
Cl < P < Ba
When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as Hund's rule Aufbau principle Pauli exclusion principle Heisenberg uncertainty principle
Hund's rule
What are the electron and molecular geometries, respectively, for iodine trifluoride, IF3? View Available Hint(s) Electron geometry is trigonal bipyramidal. Molecular geometry is T-shaped. Electron geometry is trigonal planar. Molecular geometry is trigonal bipyramidal. Electron geometry is octahedral. Molecular geometry is T-shaped. Electron geometry is trigonal bipyramidal. Molecular geometry is trigonal planar.
Electron geometry is trigonal bipyramidal. Molecular geometry is T-shaped.
Place the following elements in order of decreasing electronegativity. S F Se Se > F > S F > S > Se F > Se > S Se > S > F S > F > Se
F > S > Se
Which ionization process requires the most energy? F(g) → F+(g) + e- F2+(g) → F3+(g) + e- O2+(g) → O3+(g) + e- O(g) → O+(g) + e-
F2+(g) → F3+(g) + e-
How many dots are there in the Lewis symbol for a nitrogen atom, N? View Available Hint(s) Five Seven Three Two
Five
Choose the bond below that is most polar. C-H H-Cl H-Br H-I H-F
H-F
Which molecule could have an expanded octet? HNO2 H2CO3 H3PO4
H3PO4
Place the following in order of decreasing metallic character. P As K As > K > P K > P > As P > As > K As > P > K K > As > P
K > As > P
List the following compounds in decreasing electronegativity difference. F2 HF KF KF > F2 > HF F2 > HF > KF HF > KF > F2 KF > HF > F2
KF > HF > F2
Which reaction below represents the electron affinity of Li? Li(g) + e- → Li+(g) Li+(g) → Li(g) + e- Li+(g) + e- → Li(g) Li(g) + e- → Li-(g) Li(g) → Li+(g) + e-
Li(g) + e- → Li-(g)
Identify the compound with the highest percent ionic character. HCl HF IBr LiF
LiF
Which of the following have the same number of valence electrons? N, As, Bi B, Si, As He,Ne,F Li, N, F
N, As, Bi
Which molecule or compound below contains a nonpolar covalent bond? AgF NCl3 C2H4 K I ZnS
NCl3
Which molecule or compound below contains an ionic bond? OCl2 C2Br4 CO2 NH4NO3 SCl2
NH4NO3
Which molecule would you expect to be a free radical? NO2 N2O CO2 CO
NO2
Which of the following resonance structures for OCN- will contribute most to the correct structure of OCN-? O(1 lone pair)=C(2 lp)=N(1 lone pair) O(2 lone pairs)=C=N (2 lone pairs) O(3 lone pairs)-C≡N(with 1 lone pair) O(1 lone pair)≡C-N(3 lone pairs) They all contribute equally to the correct structure of OCN-.
O(3 lone pairs)-C≡N(with 1 lone pair)
Using Lewis structures and formal charge, which of the following ions is most stable? OCN- ONC- NOC- OCN- NOC- ONC- None of these ions are stable according to Lewis theory. All of these compounds are equally stable according to Lewis theory.
OCN-
Of the following elements, which has the highest electronegativity? P Ti Ge Si
P
No two electrons can have the same four quantum numbers is known as the Heisenberg uncertainty principle Aufbau principle Hund's rule Pauli exclusion principle
Pauli exclusion principle
Only two electrons, with opposing spins, are allowed in each orbital is known as the Pauli exclusion principle Aufbau principle Heisenberg uncertainty principle Hund's rule
Pauli exclusion principle
1s 22s 22p 63s 23p 3 is the ground state electron configuration for what element? View Available Hint(s) Arsenic, As Phosphorus, P Nitrogen, N Argon, Ar
Phosphorus, P
Place the following in order of increasing IE1. K Ca Rb Rb < K < Ca Rb < Ca < K Ca < K < Rb Ca < Rb < K K < Ca < Rb
Rb < K < Ca
Place the following elements in order of increasing electronegativity. Li Rb P P < Li < Rb P < Rb < Li Li < P < Rb Rb < Li < P Rb < P < Li
Rb < Li < P
Place the following elements in order of decreasing atomic radius. Xe Rb Ar Xe > Rb > Ar Rb > Ar > Xe Ar > Xe > Rb Rb > Xe > Ar Ar > Rb > Xe
Rb > Xe > Ar
Which reaction below represents the second electron affinity of S? S(g) → S+(g) + e- S-(g) → S(g) + e- S-(g) + e- → S2-(g) S2-(g) → S-(g) + e- S(g) + e- → S-(g)
S-(g) + e- → S2-(g)
Which molecule is polar? SF6 CO2 BF3 SF4
SF4
Using periodic trends, place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S Si-P < Si-S < Si-Cl Si-Cl < Si-S < Si-P Si-Cl < Si-P < Si-S Si-S < Si-Cl < Si-P Si-P < Si-Cl < Si-S
Si-P < Si-S < Si-Cl
Choose the diamagnetic species from below. Sn2+ I Cr N None of the above are diamagnetic.
Sn2+
Identify the element that has a ground state electronic configuration of [Kr]5s24d5. Ru Mn Tc Nb
Tc
Place the following in order of decreasing radius. Te2- F- O2- F- > O2- > Te2 O2- > F- > Te2 Te2- > O2- > F Te2- > F- > O2 F- > Te2- > O2
Te2- > O2- > F
According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, a molecule that has four electron groups around the central atom will exhibit what electron geometry? Tetrahedral Square planar Trigonal bipyramidal Determination of electron geometry requires information on whether the electron groups are lone pairs or bonding groups.
Tetrahedral
Which of the following statements is TRUE? The angular momentum quantum number (l) describes the the size and energy associated with an orbital. The principal quantum number (n) describes the shape of an orbital. The magnetic quantum number (ml) describes the orientation of the orbital. An orbital is the path that an electron follows during its movement in an atom. All of the above are true.
The magnetic quantum number (ml) describes the orientation of the orbital.
Which statement is always true according to VSEPR theory? The shape of a molecule is determined only by repulsions among nonbonding electron groups. The shape of a molecule is determined by the polarity of its bonds. The shape of a molecule is determined only by repulsions among bonding electron groups. The shape of a molecule is determined by repulsions among all electron groups on the central atom (or interior atoms, if there is more than one).
The shape of a molecule is determined by repulsions among all electron groups on the central atom (or interior atoms, if there is more than one).
According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, a molecule that has five electron groups around the central atom will have what basic geometry? View Available Hint(s) Pentagonal planar Octahedral Tetrahedral Trigonal bipyramidal
Trigonal bipyramidal
Which ionization process requires the most energy? W2+(g) → W3+(g) + e- W(g) → W+(g) + e- W+(g) → W2+(g) + e- W3+(g) → W4+(g) + e-
W3+(g) → W4+(g) + e-
________ are used to image bones and internal organs. X-rays Microwaves Radio waves Ultraviolet light Gamma rays
X-rays
The vertical height of a wave is called wavelength amplitude area median frequency
amplitude
Which of the following quantum numbers describes the shape of an orbital? angular momentum quantum number magnetic quantum number Schrödinger quantum number principal quantum number spin quantum number
angular momentum quantum number
Which of the following visible colors of light has the highest frequency? green yellow orange red blue
blue
Identify a characteristic of halogens. forms water in reactions absorbs water in reactions inert powerful reducing agents powerful oxidizing agents
powerful oxidizing agents
Of the following, which element has the highest first ionization energy? lithium boron beryllium carbon
carbon
The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is ________. vanadium titanium iron chromium manganese
chromium
When waves of equal amplitude from two sources are in phase when they interact, it is called ________. amplitude effusion diffraction constructive interference destructive interference
constructive interference
In an atom, which electrons tend to do the most shielding (core electrons or valence electrons)? core electrons valence electrons both make equal contribution into shielding
core electrons
When waves of equal amplitude from two sources are out of phase when they interact, it is called ________. effusion amplitude constructive interference diffraction destructive interference
destructive interference
When a wave encounters an obstacle or a slit that is comparable in size to its wavelength, it bends around it. This characteristic is called ________. constructive interference effusion diffraction amplitude destructive interference
diffraction
Describe the shape of a p orbital. dumbbell shaped spherical three balls four balls eight balls
dumbbell shaped
Determine the electron geometry (eg) and molecular geometry (mg) of CO2. eg=linear, mg=trigonal planar eg=tetrahedral, mg=tetrahedral eg=trigonal planar, mg=bent eg=linear, mg=linear eg=trigonal planar, mg=trigonal planar
eg=linear, mg=linear
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4. eg=trigonal bipyramidal, mg=tetrahedral eg=tetrahedral, mg=tetrahedral eg=octahedral, mg=square planar eg=linear, eg=linear eg=tetrahedral, mg=bent
eg=octahedral, mg=square planar
Give the electron geometry (eg), molecular geometry (mg), and hybridization for XeF4. eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 eg=octahedral, mg=octahedral, sp3d2 eg=octahedral, mg=square planar, sp3d2 eg=tetrahedral, mg=tetrahedral, sp3 eg=trigonal bipyramidal, mg=seesaw, sp3d
eg=octahedral, mg=square planar, sp3d2
Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O. eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 eg=tetrahedral, mg=trigonal pyramidal, sp3 eg=trigonal planar, mg=trigonal planar, sp2 eg=bent, mg=bent, sp2 eg=tetrahedral, mg=bent, sp3
eg=tetrahedral, mg=bent, sp3
Determine the electron geometry (eg) and molecular geometry (mg) of SiF4. eg=octahedral, mg=square planar eg=tetrahedral, mg=bent eg=trigonal bipyramidal, mg=trigonal pyramidal eg=tetrahedral, mg=tetrahedral eg=tetrahedral, mg=trigonal pyramidal
eg=tetrahedral, mg=tetrahedral
Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3. eg=trigonal planar, mg=trigonal planar, sp2 eg=tetrahedral, mg=trigonal pyramidal, sp3 eg=trigonal pyramidal, mg=tetrahedral, sp3 eg=tetrahedral, mg=trigonal planar, sp2 eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
eg=tetrahedral, mg=trigonal pyramidal, sp3
Determine the electron geometry (eg) and molecular geometry (mg) of XeF2. eg=trigonal bipyramidal, mg=bent eg=trigonal bipyramidal, mg=linear eg=linear, mg=linear eg=tetrahedral, mg=linear eg=tetrahedral, mg=bent
eg=trigonal bipyramidal, mg=linear
Determine the electron geometry (eg) and molecular geometry (mg) of PF5. eg=trigonal bipyramidal, mg=trigonal bipyramidal eg=trigonal bipyramidal, mg=tetrahedral eg=tetrahedral, mg=trigonal pyramidal eg=trigonal planar, mg=octahedral eg=octahedral, mg=octahedral
eg=trigonal bipyramidal, mg=trigonal bipyramidal
Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1. eg=tetrahedral, mg=trigonal pyramidal eg=tetrahedral, mg=trigonal planar eg=tetrahedral, mg=tetrahedral eg=trigonal planar, mg=bent eg=trigonal planar, mg=trigonal planar
eg=trigonal planar, mg=trigonal planar
Determine the electron geometry (eg) and molecular geometry (mg) of CO32-. eg=tetrahedral, mg=trigonal planar eg=tetrahedral, mg=trigonal pyramidal eg=trigonal planar, mg=trigonal planar eg=tetrahedral, mg=tetrahedral eg=trigonal planar, mg=bent
eg=trigonal planar, mg=trigonal planar
Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. eg=trigonal planar, mg=trigonal planar eg=trigonal bipyramidal, mg= trigonal bipyramidal eg=tetrahedral, mg=trigonal pyramidal eg=trigonal planar, mg=bent eg=tetrahedral, mg=trigonal planar
eg=trigonal planar, mg=trigonal planar
An implication of Hund's rule is that _____. View Available Hint(s) electrons fill degenerate orbitals singly first, with parallel spins, before the electrons will pair up in multielectron atoms the 4s orbital is lower in energy than the 3d orbital. electrons will fill the lowest energy orbitals first before occupying higher energy orbitals if two electrons occupy the same orbital they must have opposite spin quantum numbers (m s).
electrons fill degenerate orbitals singly first, with parallel spins, before the electrons will pair up
The bright lines of an emission spectrum are the result of _____. View Available Hint(s) electrons losing energy as they spiral into the nucleus of an atom electrons transitioning from a higher energy level to a lower energy level electrons transitioning from a lower energy level to a higher energy level electrons being ejected from atoms
electrons transitioning from a higher energy level to a lower energy level
An implication of the Pauli exclusion principle is that _____. View Available Hint(s) electrons fill degenerate orbitals singly first, with parallel spins, before the electrons pair up in multielectron atoms, the 4s orbital is lower in energy than the 3d orbital if two electrons occupy the same orbital, they must have opposite spin quantum numbers (m s) electrons will fill the lowest energy orbitals first before occupying higher energy orbitals
if two electrons occupy the same orbital, they must have opposite spin quantum numbers (m s)
If two electrons in the same atom have the same value of "l", they are in the same orbital. in the same sublevel, but not necessarily in the same level. in different levels and in different shaped orbitals. in the same level, but different sublevel. none of the above.
in the same sublevel, but not necessarily in the same level.
Describe the reaction of the noble gases with metals. vigorous inert mild reaction forms water dissolves
inert
On the electromagnetic spectrum, visible light is immediately between two other wavelengths. Name them. infrared and x-ray radio and microwave microwave and x-ray gamma ray and ultraviolet infrared and ultraviolet
infrared and ultraviolet
Using the VSEPR model, the molecular geometry of the central atom in XeF2 is ________. trigonal planar linear tetrahedral trigonal pyramidal bent
linear
Which of the following quantum numbers describes the orientation of an orbital? Schrödinger quantum number spin quantum number angular momentum quantum number magnetic quantum number principal quantum number
magnetic quantum number
Food can be cooked by ________ radiation. radio microwave ultraviolet gamma x-ray
microwave
The element that corresponds to the electron configuration 1s22s22p6 is ________. lithium sodium beryllium neon magnesium
neon
Do resonance structures always contribute equally to the overall structure of a molecule? yes no
no
CH4 nonpolar polar
non polar
F3 nonpolar polar
nonpolar
A molecule containing a central atom with sp3d2 hybridization has a(n) ________ electron geometry. trigonal planar trigonal bipyramidal octahedral bent tetrahedral
octahedral
Which of the following types of electromagnetic radiation has the lowest frequency? purple blue yellow green orange
orange
H2O polar nonpolar
polar
SBr2 nonpolar polar
polar
Which of the following quantum numbers describes the size and energy of an orbital? Schrödinger quantum number magnetic quantum number principal quantum number angular momentum quantum number spin quantum number
principal quantum number
Which of the following visible colors of light has the longest wavelength? green yellow blue violet red
red
What are the possible orbitals for n = 3? s, p, d s, p s, p, d, f s
s, p, d
What is the molecular geometry of Se Br 4? square pyramidal seesaw square planar tetrahedral
seesaw
Identify the weakest bond. single covalent bond triple covalent bond double covalent bond all of the above bonds are the same strength
single covalent bond
Give the hybridization for the S in SO3. sp3d2 sp sp2 sp3d sp3
sp2
Give the hybridization for the Br in BrCl3. sp3 sp sp2 sp3d sp3d2
sp3d
Give the hybridization for the Br in BrF5. sp2 sp3 sp3d2 sp sp3d
sp3d2
Give the hybridization for the S in SF6. sp3d sp sp3 sp2 sp3d2
sp3d2
Describe the shape of a s orbital. three balls four balls dumbbell shaped eight balls spherical
spherical
Using the VSEPR model, the molecular geometry of the central atom in XeF4 is ________. square planar square pyramidal seesaw trigonal bipyramidal tetrahedral
square planar
What is the molecular geometry of ClF4 -? tetrahedral square planar seesaw square pyramidal
square planar
What is the molecular geometry of SF5-? trigonal bipyramidal seesaw octahedral square pyramidal
square pyramidal
Using the VSEPR model, the electron-domain geometry of the central atom in SF2 is ________. trigonal planar trigonal bipyramidal linear tetrahedral octahedral
tetrahedral
Using the VSEPR model, the molecular geometry of the central atom in CF4 is ________. tetrahedral bent trigonal planar linear trigonal pyramidal
tetrahedral
What geometric arrangement of charge clouds is expected for an atom that has four charge clouds? square planar tetrahedral trigonal bipyramidal octahedral
tetrahedral
What is effective nuclear charge? the average or net charge from the nucleus experienced by the inner electrons the net charge of nucleus and all electrons the average or net charge from the nucleus experienced by the electrons in the outermost levels the net charge of the electrons in the outermost levels
the average or net charge from the nucleus experienced by the electrons in the outermost levels
Heisenberg's uncertainty principle tells us that _____. View Available Hint(s) the more accurately we know the position of a particle, the less accurately we can know the velocity of that particle complementary properties are those properties that can be measured simultaneously the de Broglie wavelength of an electron is related to its velocity an electron is actually something intermediate between a particle and a wave
the more accurately we know the position of a particle, the less accurately we can know the velocity of that particle
Using the VSEPR model, the electron-domain geometry of the central atom in SF4 is ________. trigonal bipyramidal octahedral linear tetrahedral trigonal planar
trigonal bipyramidal
Using the VSEPR model, the molecular geometry of the central atom in BF3 is ________. trigonal planar bent tetrahedral linear trigonal pyramidal
trigonal planar
Identify the shortest bond. double covalent bond single covalent bond triple covalent bond all of the above bonds are the same length
triple covalent bond
Identify the strongest bond. single covalent bond double covalent bond triple covalent bond all of the above bonds are the same strength
triple covalent bond
A sunburn is caused by overexposure to ________ radiation. x-ray microwave radio gamma ultraviolet
ultraviolet
The element that corresponds to the electron configuration 1s22s22p63s23p64s23d3 is ________. cobalt vanadium iron manganese scandium
vanadium
Describe the reaction of the alkali metals with non-metals. forms water mild reaction inert dissolves vigorous
vigorous
Which of the following colors of electromagnetic radiation has the shortest wavelength? violet orange green yellow blue
violet
The distance between adjacent crests is called amplitude frequency wavelength median area
wavelength