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Molecular Orbital Theory

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Wize University Chemistry Textbook > Molecular Orbital Theory

Molecular Orbital Theory

7 Activities

Wize University Chemistry Textbook > Periodic Table Trends

Ionization Energy

5 Activities

Choose the correct option:
More Molecular Orbital Theory Questions:
MO Theory, Bond Order, Magnetic Properties
Rank the following species in terms of increasing bond length and comment on their magnetic properties:
O22+, O2+, O2, O2―, and O22―.
Choose the correct option (D stands for diamagnetic, P stands for paramagnetic):
MO theory
Which MO does this picture represent if the molecule is Be2 and x is the bonding axis?
Molecular Orbital Theory
All of the following statements concerning molecular orbital (MO) theory are correct EXCEPT
A. The Pauli exclusion principle must be obeyed.
B. Hund's rule must be obeyed.
Molecular Orbital Theory
Molecular orbital theory focuses on the overlap of:
Molecular orbital theory
Which of the following orbitals has the lowest energy
Which of the following statements is true
MO theory
Which MO does this picture represent if the molecule is Be2 and x is the bonding axis?
More Ionization Energy Questions:
Periodic Trends: Ionization Energy
Choosing from the following elements answer the following questions. K, Ca, N, Ar, F
Which as the greatest second ionization energy?
Periodic Trends: Ionization Energy
Choosing from the following elements answer the following questions. K, Ca, N, Ar, F
Which has the largest first ionization energy
Periodic Trends: Ionization Energy
Choosing from the following elements answer the following questions. K, Ca, N, Ar, F
Which has the smallest 1st ionization energy?
Ionization Energy, Electronic Configuration
Compare the 3rd IE of Ca, Sr and Y.
To which third period (row) element do these ionization values belong?
IE1= 578 kJ/mol IE2= 1820 kJ/mol IE3= 2750 kJ/mol IE4= 11600 kJ/mol
Periodic Trends: Ionization energy
Ionization Energy refers to the amount of energy require to do what?
IE
Identify the elements with highest and lowest IE: B, Al, C, or Si
IE
Rank the following according to increasing first ionization energy: Ne, Na, P, Ar, K.
Ionization Energy
a. Arrange the following elements in order of increasing IE1: Si, In, F, N.
b. Arrange the following elements in order of decreasing IE1: Br, Sb, Sn, N.
Ionization Energy
Consider the set of successive ionization energies:
IE1 = 540 kJ / mol; IE2 = 1430 kJ / mol; IE3 = 2628 kJ / mol; IE4 = 4200 kJ / mol; IE5 = 15700 kJ / mol;
Which element can these values correspond to if the element is in a. period 3, b. period 4?
Electronic Transition
What is the 4th ionization energy of Be?
MO Theory
Choose the correct statement.
MO Theory
Rank the following species in decreasing order of IE1:
He, O, He2+, O22+.
Ionization Energy
Which of the following statements are true regarding the second ionization energy (IE2) of calcium (Mg) vs potassium (Na).
Ionization Energy
Rank the following atoms in terms of increasing ionization energy (1 = smallest, 5 = largest).
Ionization Energy
Which of the following statements are true regarding the second ionization energy (IE2) of calcium (Ca) vs potassium (K).
Ionization Energy
A student has an exam question asking which has the higher first ionization energy, beryllium or boron. They answer boron, because based on Periodic Trends, boron is further to the right and hence will have the higher ionization energy; however, the answer is beryllium. Why?
Ionization Energy
Rank the following atoms in terms of increasing ionization energy (1 = smallest, 5 = largest).
Periodic trends: Second Ionization Energy
Which of the following correctly represents the second ionization energy of beryllium?
Periodic Trends: Comparing Ionization Energies
Which one of the following statements are true for the first ionization energy (IE1) of aluminum (Al) vs the IE1 of silicon (Si).
Periodic Trends: Ionization Energy
Rank the following atoms in order of increasing first ionization energy (1 = smallest; 6 = largest): Fe, O, Ba, Si, V, Zr
Periodic Trends: Ionization Energy
Which element from the ones shown below has the highest first ionization energy?
Periodic Trends: Ionization Energy
Choosing from the following elements answer the following questions. K, Ca, N, Ar, F
Which as the greatest second ionization energy?
Periodic Trends: Ionization Energy
Choosing from the following elements answer the following questions. K, Ca, N, Ar, F
Which has the largest first ionization energy
Periodic Trends: Ionization Energy
Choosing from the following elements answer the following questions. K, Ca, N, Ar, F
Which has the smallest 1st ionization energy?
Which element from the ones shown has the highest 2nd ionization energy? (IE2)
Periodic Trends: Ionization Energy
To which third period (row) element do these ionization values belong?
IE1= 578 kJ/mol IE2= 1820 kJ/mol IE3= 2750 kJ/mol IE4= 11600 kJ/mol
Periodic Trends: Ionization Energy
Which of the following has the largest second ionization energy for each of the following sets?
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY.
Periodic Trends: Ionization Energy
Which of the following has the highest second ionization energy?
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY.
Rank the following elements by increasing first ionization Energy:
O, Ge, Sc, Ba
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY.
Rank the following species from lowest to highest 2nd Ionization energies :
F, C, Ga, Fe, Mg, K
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY.
Periodic Trends:: Ionization Energy
Which of the following has the lowest ionization energy?
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY.
Rank the following atoms/ions in order of increasing ionization energy: Ca, O, Te, Ne, O-.
Periodic Trends: Ionization Energy
Which of the following atoms is the following successive ionization energy data for?
Third ionization energy (IE3) = 2912 kJ/mol
Fourth ionization energy (IE4) = 4956 kJ/mol
If A > B means that the ionization energy of A is greater than the ionization energy of B then which of the following is INCORRECT?
Periodic Trends: Ionization Energy Exception
Contrary to what we would predict based on Zeff the Ionization Energy of aluminum is actually less than magnesium.This is because,
If A > B means the first ionization energy (I1) of A is greater than the first ionization energy of B, then which of the following comparisons is INCORRECT?
Periodic Trends: Lowest Ionization Energy
Select the element with the lowest 3rd ionization energy.
Periodic Trends
Which species should have the highest ionization energy?
Periodic Trends
Which group of the periodic table can most easily donate an electron in a chemical reaction?
Choose the answer below which correctly ranks the following elements in order of decreasing ionization energy: Cr, As, N, Sr, F
Periodic Trends: Ionization Energy
Which of these elements has the highest third ionization energy?
Periodic trends: Ionization Energy
Rank the following elements by increasing first ionization Energy: Si, Mn, O, K, F
Periodic Trends: Ionization Energy
Rank the following elements from smallest to greatest ionization energy: O, Al, Ca, Cs,
Ni.
Periodic Trends: Ionization Energy
Rank the following elements in increasing order of ionization energy: Al, F, Pd, Rb, Zr
Rb
<
Zr
<
Pd
<
Al
<
F
Atom: Atomic Properties
Students in a previous year were asked a certain set of questions. For each of the questions and the given responses, in the corresponding boxes, identify whether the student response is correct or incorrect and the corrections that need to be made.
a) Question: IE for O = 1310 kJ/mol and IE for Cl = 1250 kJ/mol. Explain why this difference exists.
Student’s response: Because Cl has a higher n-value the electrons are further from the nucleus, giving the atom more room and the ability to add additional electron(s).
like Winter 2015 MT1
Which equation describes the first ionization energy of Bromine?