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