Chem 1410 Ch 1-4

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Which element has a partially filled atomic orbital? A.Be B. Zn C. Ag D. Ne E. Yb

Which element has a partially filled atomic orbital? A.Be B. Zn C. Ag D. Ne E. Yb

Which of the following is not isoelectronic with the others? A. Cl^{-} B. S^{2-} C. Ar D. Ti^{4+} E. Rb^{+}

Which of the following is not isoelectronic with the others? A. Cl^{-} B. S^{2-} C. Ar D. Ti^{4+} E. Rb^{+}

*What kind of orbital (s, p, d, or f) is this? * 2 lobes on one axis with node in middle

p

What is the effective nuclear charge for the valence electrons in Cl?

7.0

What is the effective nuclear charge for the valence electrons in P?

5.0

Which of the following correctly uses the rational of Z_eff in explaining that atomic radius of Cl is smaller than that of P? A. The stronger the attractive force from the larger effective nuclear charge, the larger the atom. B. The weaker the attractive force from the larger effective nuclear charge, the larger the atom. C. The stronger the attractive force from the larger effective nuclear charge, the smaller the atom. D. The weaker the attractive force from the larger effective nuclear charge, the smaller the atom.

Which of the following correctly uses the rational of Z_eff in explaining that atomic radius of Cl is smaller than that of P? A. The stronger the attractive force from the larger effective nuclear charge, the larger the atom. B. The weaker the attractive force from the larger effective nuclear charge, the larger the atom. C. The stronger the attractive force from the larger effective nuclear charge, the smaller the atom. D. The weaker the attractive force from the larger effective nuclear charge, the smaller the atom.

Rank in order from largest (at the top) to smallest (at the bottom), the atomic radii of the following atoms: A. Rb B. K C. Cs D. Na E. Li

Rank in order from largest (at the top) to smallest (at the bottom), the atomic radii of the following atoms: C. Cs A. Rb B. K D. Na E. Li

Which is the correct order for atomic size? A. Rb > Na > K B. O > N > F C. Mg > Al > Si D. Cl > S > P E. He > Ne > Ar

Which is the correct order for atomic size? A. Rb > Na > K B. O > N > F C. Mg > Al > Si D. Cl > S > P E. He > Ne > Ar

Consider the isoelectronic series N^{3-}, O^{2-}, F^{-}, Na^{+}, Mg^{2+}, and Al^{3+} (all with 1s^{2} 2s^{2} 2p^{6}). Rank from smallest to largest (top to bottom). A. N^3- B. F^- C. Mg^2+ D. O^2- E. Al^3+ F. Na^+

Consider the isoelectronic series N^{3-}, O^{2-}, F^{-}, Na^{+}, Mg^{2+}, and Al^{3+} (all with 1s^{2} 2s^{2} 2p^{6}). Rank from smallest to largest (top to bottom). E. Al^3+ C. Mg^2+ F. Na^+ B. F^- D. O^2- A. N^3-

Note: The greater the nuclear charge, the stronger the attractive force.

https://youtu.be/ZblwivlX4L4

Rank the following atoms from largest IE_1 (at top) to smallest IE_1 (at bottom). A. F B. I C. Br D. Cl

Rank the following atoms from largest IE_1 (at top) to smallest IE_1 (at bottom). A. F D. Cl C. Br B. I

From the following data, identify the period 3 element. Enter only the chemical symbol as your answer. (kJ/mol) IE_1 = 786 IE_2 = 1577 IE_3 = 3232 IE_4 = 4356 IE_5 = 16091 IE_6 = 19805

Si

Which element has the largest electron affinity (most negative value)? A. Lithium B. Barium C. Oxygen D. Silicon E. Xenon

Which element has the largest electron affinity (most negative value)? A. Lithium (1+) B. Barium (2+) C. Oxygen (2-) D. Silicon (4+) E. Xenon (---)

Note: Double check reasoning here

Arrange the following pairs of elements in order of increasing electronegativity difference. Smallest difference at the top and largest difference at the bottom. D. C-O C. B-C B. Na-Cl A. Ca-Se

Arrange the following pairs of elements in order of increasing electronegativity difference. Smallest difference at the top and largest difference at the bottom. C. B-C D. C-O A. Ca-Se B. Na-Cl

Based on the differences in electronegativity which bond is most likely to be an ionic bond? A. Ca-Se B. C-O C. B-C D. Na-Cl

Based on the differences in electronegativity which bond is most likely to be an ionic bond? A. Ca-Se B. C-O C. B-C D. Na-Cl

Which element has the greater effective nuclear charge? A. Be B. N

Which element has the greater effective nuclear charge? A. Be B. N

Rank the elements in order of increasing atomic radius with the smallest at the top of the list and the largest at the bottom. A. Cs B. Na C. H D. Li

Rank the elements in order of increasing atomic radius with the smallest at the top of the list and the largest at the bottom. C. H D. Li B. Na A. Cs

Does the radius of magnesium increase or decrease as it loses electrons? A. Increase B. Decrease

Does the radius of magnesium increase or decrease as it loses electrons? A. Increase B. Decrease

Less attraction between nucleus and electrons if there are less electrons.

Match elements with the most similar ionization energies. 1. Br 2. C 3. Mg A. I B. Ge C. Xe

Match elements with the most similar ionization energies. 1. C 2. A 3. B

From its position in the periodic table, rank the elements in order of electronegativity (highest value at the top to lowest value at the bottom). A. F B. B C. O D. Ca E. Cl F. Al

From its position in the periodic table, rank the elements in order of electronegativity (highest value at the top to lowest value at the bottom). A. F C. O E. Cl B. B F. Al D. Ca

What is the atomic radius of Xe (in pm)?

108.0

What is the first ionization energy of Xe (in kJ/mol)?

1170.4

What is the electron affinity of Xe (in kJ/mol)?

0.0

In p-block of Period 2 of the Periodic Table, which atom does not follow the trend (an outlier)? Use the chemical symbol in the answer.

O

Which of the following best describes the driving forces for the trends in ionization energy periodicity of atoms? A. The effective nuclear charge for the valence electrons increases across the period, and, therefore, it takes more energy to remove the electron. Moving down a group, the valence electrons are further from the nuclease as the effective nuclear charge increases; therefore, it takes less energy to remove the electron. However, there are exceptions. B. The atomic radius for the valence electrons increases across the period, and, therefore, it takes more energy to remove the electron. Moving down a group, the valence electrons are further from the nuclease as n increases; therefore, it takes less energy to remove the electron. However, there are exceptions. C. The effective nuclear charge for the valence electrons increases across the period, and, therefore, it takes more energy to remove the electron. Moving down a group, the valence electrons are further from the nuclease as n increases; therefore, it takes less energy to remove the electron. There are no exceptions to this trend. D. The effective nuclear charge for the valence electrons increases across the period, and, therefore, it takes more energy to remove the electron. Moving down a group, the valence electrons are further from the nuclease as n increases; therefore, it takes less energy to remove the electron. However, there are outliers.

D.

Key: "there are outliers"

What is the name of the point where the sign of the wavefunction changes?

node

What kind of orbital (s, p, d, or f) is this? Round, circular

s

What kind of orbital (s, p, d, or f) is this? Dumbell on xy axis

p

Which element has a partially filled atomic orbital? A. Be B. Zn C. Ag D. Ne E. Yb

Which element has a partially filled atomic orbital? A. Be B. Zn C. Ag D. Ne E. Yb

How many valence electrons does the ground-state configuration of nitrogen have? A. None B. 2 C. 3 D. 5 E. 7

How many valence electrons does the ground-state configuration of nitrogen have? A. None B. 2 C. 3 D. 5 E. 7

Which of the following describes the 1s bonding orbital compared to the 1s antibonding orbital? A. There is less electron probability located between the two nuclei in a bonding orbital than an antibonding orbital. B. There is more electron probability located above the two nuclei in a bonding orbital than an antibonding orbital. C. There is more electron probability located between the two nuclei in a bonding orbital than an antibonding orbital. D. There is more electron probability located below the two nuclei in a bonding orbital than an antibonding orbital.

Which of the following describes the 1s bonding orbital compared to the 1s antibonding orbital? A. There is less electron probability located between the two nuclei in a bonding orbital than an antibonding orbital. B. There is more electron probability located above the two nuclei in a bonding orbital than an antibonding orbital. C. There is more electron probability located between the two nuclei in a bonding orbital than an antibonding orbital. D. There is more electron probability located below the two nuclei in a bonding orbital than an antibonding orbital.

Will the following pairs of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (-) . (+) o---o (+) . (-) A. Constructively B. Destructively C. No net overlap

Will the following pairs of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (-) . (+) o---o (+) . (-) A. Constructively B. Destructively C. No net overlap

Like-like for constructive

Will the following pairs of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (-) . . (-) o--(+)o(+) (+) . . (-) A. Constructively B. Destructively C. No net overlap

Will the following pairs of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (-) . . (-) o--(+)o(+) (+) . . (-) A. Constructively B. Destructively C. No net overlap

Decide if the following molecular orbitals are bonding or antibonding. 2 regions separated with each region surrounding one nuclei . . . | (Red) | (Blue) . . . | A. Bonding B. Antibonding

Decide if the following molecular orbitals are bonding or antibonding. 2 regions separated with each region surrounding one nuclei . . . | (Red) | (Blue) . . . | A. Bonding B. Antibonding

Decide if the following molecular orbitals are bonding or antibonding. One region surrounding both nuclei A. Bonding B. Antibonding

Decide if the following molecular orbitals are bonding or antibonding. One region surrounding both nuclei A. Bonding B. Antibonding

What is the HOMO for B_2? A. σ_1 B. σ_2 C. σ_3 D. σ_4 E. π F. π*

What is the HOMO for B_2? A. σ_1 B. σ_2 C. σ_3 D. σ_4 E. π F. π*

Note: B,C,N (ΔE > 13 eV) and O,F (ΔE > 13 eV)

What is the LUMO for O_2? A. σ_2s B. σ*_2s C. σ_2pz D. σ*_2pz E. π F. π*

What is the LUMO for O_2? A. σ_2s B. σ*_2s C. σ_2pz D. σ*_2pz E. π F. π*

What is the bond order for a molecule of N_2?

3.0

Bond order: (1/2)*(#el. in bonding MOs - #el. in antibonding MOs)

Note: Use MO Diagram to determine # of electrons in bonding and antibonding orbitals

https://youtu.be/HEW3aJ_RsW4

What is the bond order for a molecule of F_2?

1.0

Bond order: (1/2)*(#el. in bonding MOs - #el. in antibonding MOs)

Note: Use MO Diagram to determine # of electrons in bonding and antibonding orbitals

Below is shown the atomic orbitals that may be used to construct molecular orbitals for carbon monoxide (CO). Click on the orbitals that can combine with carbon's 2p_z orbital to form σ molecular orbitals. Look on TopHat

C's 2s and O's 2pz

Below is shown the molecular orbital diagram for carbon monoxide (CO). Click on the pair of electrons that is most consistent with a lone pair of electrons localized on the carbon atom. Look on TopHat

σ_3

What are the factors that govern the degree of overlap of atomic orbitals on different atoms?

A. symmetry of the atomic orbitals B. distance between the overlapping atomic orbitals C. size of the atomic orbitals D. energy levels of the overlapping orbitals E. all of the above F. none of the overlap

What are the factors that govern the degree of overlap of atomic orbitals on different atoms?

A. symmetry of the atomic orbitals B. distance between the overlapping atomic orbitals C. size of the atomic orbitals D. energy levels of the overlapping orbitals E. all of the above F. none of the overlap

Will the following pair of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (+)o(-)-----(+) A. Constructively B. Destructively C. No net overlap

Will the following pair of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (+)o(-)-----(+) A. Constructively B. Destructively C. No net overlap

Will the following pair of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (+) (-) . (-) (+) o------- o (-) (+) . (+) (-)

A. Constructively B. Destructively C. No net overlap

Will the following pair of atomic orbitals interact constructively, destructively, or with no net overlap if they approach along the indicated axis? (+) (-) . (-) (+) o------- o (-) (+) . (+) (-)

A. Constructively B. Destructively C. No net overlap

What is the HOMO for C_2? Look on TopHat

1st diagram π_2px and π_2py

What is the LUMO for C_2? Look on TopHat

1st diagram σ_3

Calculate the bond order for C_2 using the molecular orbital energy level diagram.

2.0

How many unpaired electrons are present in C_2?

0.0

What is the HOMO for F_2? Look on TopHat

2nd Diagram π*_2px π*_2py

What is the LUMO for F_2? Look on TopHat

2nd Diagram σ*_2pz

Calculate the bond order for F_2 using the molecular orbital energy level diagram?

1.0

The single bond present in F_2 is derived from the overlap of two ____-orbitals contributed by each of the F atoms.

The single bond present in F_2 is derived from the overlap of two p-orbitals contributed by each of the F atoms.

The single bond present in HF is derived from the overlap of one ____-orbitals contributed by the H atom and one ____ contributed by the F atom. Hint use Figure 4.11; you don't need to build the MO diagram.

The single bond present in HF is derived from the overlap of one s-orbitals contributed by the H atom and one p contributed by the F atom. Hint use Figure 4.11; you don't need to build the MO diagram.

How many unpaired electrons are present in F_2?

0.0

Choose the best description for the molecular orbital below. ( - )o( . . + . . )o( - ) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Choose the best description for the molecular orbital below. ( - )o( . . + . . )o( - ) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Choose the best description for the molecular orbital below. ( . . - . . )o( + ) | ( - )o( . . + . . ) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Choose the best description for the molecular orbital below. ( . . - . . )o( + ) | ( - )o( . . + . . ) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Choose the best description for the molecular orbital below. ( o . o ) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Choose the best description for the molecular orbital below. ( o . o ) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Choose the best description for the molecular orbital below. (+) . . . . (-) o-- | --o (-) . . . . (+) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Choose the best description for the molecular orbital below. (+) . . . . (-) o-- | --o (-) . . . . (+) A. σ¸ bonding B. σ¸ antibonding C. π¸ bonding D. π¸ antibonding

Populate the molecular orbital energy level diagram for the hydroxide ion (HO^-) below and then click on the LUMO. Look on TopHat

σ*_3

Is N_2 stable? A. Yes B. No

Is N_2 stable? A. Yes B. No

What information allowed you to answer the above question? A. There are more electrons in the antibonding orbitals than the bonding orbitals. Thus, the bond order is greater than zero and the molecule is stable. B. There are more electrons in the bonding orbitals than the antibonding orbitals. Thus, the bond order is greater than zero and the molecule is stable. C. The energy of the lowest occupied orbital is below zero. Thus, the bond order represents a stable molecule. D. The energy difference between the 2s mixed orbitals is lower than the 2p orbitals. Thus, the molecule is stable.

What information allowed you to answer the above question? A. There are more electrons in the antibonding orbitals than the bonding orbitals. Thus, the bond order is greater than zero and the molecule is stable. B. There are more electrons in the bonding orbitals than the antibonding orbitals. Thus, the bond order is greater than zero and the molecule is stable. C. The energy of the lowest occupied orbital is below zero. Thus, the bond order represents a stable molecule. D. The energy difference between the 2s mixed orbitals is lower than the 2p orbitals. Thus, the molecule is stable.

Is N_2 paramagnetic or diamagnetic? A. diamagnetic B. paramagnetic

Is N_2 paramagnetic or diamagnetic? A. diamagnetic B. paramagnetic

What feature of the molecular orbital diagram allowed you to answer the previous question? A. All electrons are paired in the molecular orbitals. B. There are electrons in the antibonding orbitals that are formed for the mixing of the atomic p-orbitals. C. There are unpaired electrons. D. The orbitals formed for the mixing of the 2s atomic orbitals are occupied.

What feature of the molecular orbital diagram allowed you to answer the previous question? A. All electrons are paired in the molecular orbitals. B. There are electrons in the antibonding orbitals that are formed for the mixing of the atomic p-orbitals. C. There are unpaired electrons. D. The orbitals formed for the mixing of the 2s atomic orbitals are occupied.

What is the bond order of N_2? A. 3 B. 2 C. 1 D. 0

What is the bond order of N_2? A. 3 B. 2 C. 1 D. 0

Based on the bond order what type of bond does N_2 have? A. no bond, it is unstable B. single C. double D. triple

Based on the bond order what type of bond does N_2 have? A. no bond, it is unstable B. single C. double D. triple

What is the charge of N_2? A. -1 B. -2 C. neutral D. +1 E. +2

What is the charge of N_2? A. -1 B. -2 C. neutral D. +1 E. +2

How many unparied electrons does N_2 have? A. none B. 1 C. 2 D. 3

How many unparied electrons does N_2 have? A. none B. 1 C. 2 D. 3

Which of the following highlights a major difference between your molecular orbital diagram and the one calculated with Spartan (check all that apply)? A. there are two columns labeled a and b B. the 2s bonding orbital is not shown C. there are actual energy values assigned to the orbitals D. the bonding orbital that arises from the two pz atomic orbitals doesn't look like how we or the book draws it

Which of the following highlights a major difference between your molecular orbital diagram and the one calculated with Spartan (check all that apply)? A. there are two columns labeled a and b B. the 2s bonding orbital is not shown C. there are actual energy values assigned to the orbitals D. the bonding orbital that arises from the two pz atomic orbitals doesn't look like how we or the book draws it

What additional information do you obtain with Spartan that you could not have in your sketched diagrams (select all that are correct)? A. energy values B. more accurate estimates of the mixing of the atomic orbitals to form the molecular orbitals C. more accurate representation of the shape of the molecular orbitals D. Spartan provides the exactly right representation of the molecular orbitals and their energies

What additional information do you obtain with Spartan that you could not have in your sketched diagrams (select all that are correct)? A. energy values B. more accurate estimates of the mixing of the atomic orbitals to form the molecular orbitals C. more accurate representation of the shape of the molecular orbitals D. Spartan provides the exactly right representation of the molecular orbitals and their energies

What is the bond order for O_2? A. 0 B. 1 C. 2 D. 3

What is the bond order for O_2? A. 0 B. 1 C. 2 D. 3

Which of the following statements describe the arrangement and properties of the particles in an atom? A. Neutrons and protons form the nucleus at the center of the atom. B. Electrons are arranged around the nucleus C. Electrons rotate around the nucleus. D. There is an attractive force between the negatively charged electrons and the positively charged nucleus.

Which of the following statements describe the arrangement and properties of the particles in an atom? A. Neutrons and protons form the nucleus at the center of the atom. B. Electrons are arranged around the nucleus C. Electrons rotate around the nucleus. D. There is an attractive force between the negatively charged electrons and the positively charged nucleus.

Rank the subatomic particles in order of increasing relative charge, with the smallest at the top and the largest at the bottom.

Electron, proton, neutron

1. electron

2. neutron

3. proton

Compared to the rest of an atom, which of the following describes the nucleus? A. Smaller and contains most of the atom's mass B. Smaller and contains hardly of an atom's mass C. Larger and contains most of the atom's mass D. Larger and contains hardly of an atom's mass

Compared to the rest of an atom, which of the following describes the nucleus? A. Smaller and contains most of the atom's mass B. Smaller and contains hardly of an atom's mass C. Larger and contains most of the atom's mass D. Larger and contains hardly of an atom's mass

As n increases, the Bohr radius increases/decreases.

As n increases, the Bohr radius increases/decreases.

What is the relationship between the energy of an orbital and its average radius? A. As the radius increases, the orbital energy decreases. B. As the radius increases, the orbital energy increases.

What is the relationship between the energy of an orbital and its average radius? A. As the radius increases, the orbital energy decreases. B. As the radius increases, the orbital energy increases.

What happens to the energy of an electron as it gets farther from the nucleus? A. As an electron gets farther from the nucleus the principal quantum number goes up and the energy increases and the electron is less stable. B. As an electron gets farther from the nucleus the principal quantum number goes down and the energy increases and the electron is less stable. C. As an electron gets farther from the nucleus the principal quantum number goes up and the energy decreases and the electron is less stable. D. As an electron gets farther from the nucleus the principal quantum number goes up and the energy decreases and the electron is more stable.

What happens to the energy of an electron as it gets farther from the nucleus? A. As an electron gets farther from the nucleus the principal quantum number goes up and the energy increases and the electron is less stable. B. As an electron gets farther from the nucleus the principal quantum number goes down and the energy increases and the electron is less stable. C. As an electron gets farther from the nucleus the principal quantum number goes up and the energy decreases and the electron is less stable. D. As an electron gets farther from the nucleus the principal quantum number goes up and the energy decreases and the electron is more stable.

Calculate the energy, in joules (J), required to remove hydrogen's one electron from the ground state. This is known as hydrogen's ionization energy.

2.18e-18 J https://youtu.be/UwRfe2GiB0g

Click on the value of the radius on the x-axis you think the electron with an R_{2s} wave-function is most likely to be found.

The x-axis point (radius) where wave-function has highest peak

Which of the following combinations of n and ℓ are not allowed? A. n = 1 and ℓ= 0 B. n = 3 and ℓ = 1 C. n = 4 and ℓ = 0 D. n = 2 and ℓ = 2 E. n = 5 and ℓ = 3

Which of the following combinations of n and ℓ are not allowed? A. n = 1 and ℓ= 0 B. n = 3 and ℓ = 1 C. n = 4 and ℓ = 0 D. n = 2 and ℓ = 2 E. n = 5 and ℓ = 3

https://youtu.be/9Oqb3P3FN0w

What type of orbital does an electron with n = 3 and ℓ = 2 occupy?

3d or d

How many different f orbitals are there?

(2ℓ+1) = ? f-orbital => ℓ = 3 (2(3)+1) = 7.0

How many angular nodes does a d_{yz} orbital have?

ang. nodes = ℓ

d-orbital => ℓ = 2

ang. nodes = 2.0

State # of Radial and Angular nodes for each orbital:

1. 1s

2. 3p_z

3. 4d_xy

4. 6p_x

1. 0 radial, 0 angular total nodes: n - 1 n = 1 total = 0 2. 1 radial, 1 angular total nodes: n - 1 n = 3 total = 3 - 1 = 2

ang. nodes = ℓ

p-orbital => ℓ = 1

ang. nodes = 1

rad. nodes = (n-1) - ℓ = 1

3. 1 radial, 2 angular total nodes: n - 1 n = 4 total = 4 - 1 = 3

ang. nodes = ℓ

d-orbital => ℓ = 2

ang. nodes = 2

rad. nodes = (n-1) - ℓ = 1

4. 4 radial, 1 angular total nodes: n - 1 n = 6 total = 6 - 1 = 5

ang. nodes = ℓ

p-orbital => ℓ = 1

ang. nodes = 1

rad. nodes = (n-1) - ℓ = 4

https://youtu.be/wW27P3OCKNw

Match the quantum number with what the number represents.

1. the overall shape of an orbital

2. the orientation of an electron with respect to a magnetic field

3. the orientation of an orbital in space

4. the distance of an electron from the nucleus

1. ℓ

2. m_s

3. m_ℓ

4. n

Why does it become difficult to mathematically describe the Coulombic interactions in a multi-electron atom? A. The negatively charged electrons will attract each other. B. The negatively charged electrons will cancel out the charge of the protons in the nucleus. C. Heisenberg's uncertainty principle makes it impossible to determine the exact location of the electrons. D. There are no equations to describe the Coulombic interactions between moving charges.

Why does it become difficult to mathematically describe the Coulombic interactions in a multi-electron atom? A. The negatively charged electrons will attract each other. B. The negatively charged electrons will cancel out the charge of the protons in the nucleus. C. Heisenberg's uncertainty principle makes it impossible to determine the exact location of the electrons. D. There are no equations to describe the Coulombic interactions between moving charges.

Nitrogen has a 1s^{2} 2s^{2} 2p^{3} electron configuration. How many of nitrogen's electrons have ℓ = 1?

3.0

How many electrons are needed to fill a complete set of d orbitals?

10.0

Which orbital is the HOMO of a ground-state carbon atom?

2p

Which orbital is the LUMO of a ground-state carbon atom?

2p (has only 2 electrons in p orbital leaving the last p orbital empty)

How many unpaired electron(s) does a carbon atom have in its ground state?

2.0

Determine which electron configuration is the excited state. A. Oxygen - 1s^{2} 2s^{2} 2p^{4} B. Sodium - 1s^{2} 2s^{2} 2p^{6} 3s^{1} C. Chlorine- 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{5} D. Aluminum - 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{1} E. Magnesium - 1s^{2} 2s^{2} 2p^{6} 3s^{1} 3p^{1}

E. Magnesium - 1s^{2} 2s^{2} 2p^{6} 3s^{1} 3p^{1}

Match the elements with the correct valence electron configurations.

1. He

2. Be

3. C

4. P

5. V

1. 1s^2

2. [He]2s^2

3. [He]2s^2 2p^2

4. [Ne]3s^2 3p^3

5. [Ar]4s^2 3d^3

Which ion is not isoelectronic with the others? A. N^3- B. O^2− C. Ne^+ D. Al^3+ E. Mg^2+

Which ion is not isoelectronic with the others? A. N^3- B. O^2− C. Ne^+ D. Al^3+ E. Mg^2+

*What is the ground-state electron configuration of Cu^+ ? * A. [Ar]4s^2 3d^8 B. [Ar]4s^2 3d^10 C. [Ar]4s^1 3d^9 D. [Ar]3d^9 E. [Ar]3d^10

*What is the ground-state electron configuration of Cu^+ ? * A. [Ar]4s^2 3d^8 B. [Ar]4s^2 3d^10 C. [Ar]4s^1 3d^9 D. [Ar]3d^9 E. [Ar]3d^10

What orbital type has the radial probability distribution in the above graph (Q02)?

Graph has 2 "humps" (peaks)

A. 3d B. 2p C. 2s D. 4f

What orbital type has the radial probability distribution in the above graph (Q02)?

Graph has 2 "humps" (peaks)

A. 3d B. 2p C. 2s D. 4f

The first maximum in the above graph of the radial probability distribution refers to what phenomenon.

1st hump is smaller

A. electrostatic repulsion B. electron penetration C. additional energy levels D. Pauli's principal E. orbital mixing

The first maximum in the above graph of the radial probability distribution refers to what phenomenon.

1st hump is smaller

A. electrostatic repulsion B. electron penetration C. additional energy levels D. Pauli's principal E. orbital mixing

Which of the following orbitals can be represented by the set of quantum numbers (n = 4), (l = 1), (m_l = −1), (m_s = 1/2)?

A. 4d B. 4p C. 4s D. 1s

Which of the following orbitals can be represented by the set of quantum numbers (n = 4), (l = 1), (m_l = −1), (m_s = 1/2)?

A. 4d B. 4p C. 4s D. 1s

Match the quantum numbers to the description.

1. n

2. l

3. m_l

A. Size and Energy of orbital B. Orientation of orbital C. Shape of the subshell D. Number of combined orbitals

1. A. Size and energy of orbital

2. C. Shape of the subshell

3. B. Orientation of the orbital

Match the quantum numbers and the subshell (orbitals) in which electrons are found

1. n=3 and l=2

2. n=2 and l=0

3. n=5 and l=1

A. 2s B. 3d C. 5p

1. B. 3d

2. A. 2s

3. C. 5p

Which subshell is higher in energy? A. 5p B. 6s

Which subshell is higher in energy? A. 5p B. 6s

What would be the gravitational force (in Newtons) between a proton and an electron in a hydrogen atom? Use "E" for scientific notation. For example, the number 2.1 x 10^66 would be written as 2.1E6. Use 2 significant figures.

3.6e-47

Use equation F=((m_1*m_2)*G)/(r^2)