Consider the following statements about first ionization energies: I. Because the effective nuclear charge for Mg is greater than that for Be, the first ionization energy of Mg is greater than that of Be. II. The first ionization energy of O is less than that of N because in O we must pair electrons in the 2p orbitals. III. The first ionization energy of Ar is less than that of Ne because a 3p electron in Ar is farther from the nucleus than a 2p electron in Ne. Which of the statements I, II, and III is or are true? O Only one of the statements is true O Statements I and Il are true O Statements I and II are true Statements Il and IIlI are true O All three statements are true

Consider the following statements about first ionization energies: I. Because the effective nuclear charge for Mg is greater than that for Be, the first ionization energy of Mg is greater than that of Be. II. The first ionization energy of O is less than that of N because in O we must pair electrons in the 2p orbitals. III. The first ionization energy of Ar is less than that of Ne because a 3p electron in Ar is farther from the nucleus than a 2p electron in Ne. Which of the statements I, II, and III is or are true? O Only one of the statements is true O Statements I and Il are true O Statements I and II are true Statements Il and IIlI are true O All three statements are true

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The effective nuclear charge experienced by the outer most electron of NA is different than the…

A: From given The atomic number----> Na is 11 Ne is 10. So Sodium (Na) has a total number of 11…

Q: Which statements completed with a to e will be true and whichwill be false?In Group 4A (14), an atom…

A: The answer is option b. , which is ionization energy. Because, Ionization energy(I.E.) is the energy…

Q: Use noble gas notation to depict electron configurations for the following metals of the third…

Q: 1. Which of the following represent impossible combinations of n and l? (a) 1p, (b) 4s, (c) 5f,…

A: Since you asked for multiple question and no one specified that which is solve. So only solve first…

Q: The energy required to completely remove the outermost electron from the excited xenon atom is 369…

A: The energy required to remove an electron from an atom is known as ionization energy. In this case,…

Q: a. Which type of ions – cations or anions – have smaller radii than the corresponding neutral atoms?…

A: Cations have smaller radii than their corresponding neutral atoms. During the formation of cations,…

Q: State the exclusion principle. What does it imply about the number and spin of electrons in an…

Q: Write equations corresponding to the following. (Use the lowest possible coefficients. Be sure to…

A: Ionization energy is defined as amount of energy required to remove the most loosely bound electron…

Q: A. A main group element with the valence electron configuration 5s²5p4 is in periodic group It forms…

A: The given elements can donate or accept electrons to complete the octet. The number of electrons…

Q: 1 I X I I 1 This sketch is about 1800 pm wide. The coordinate (x, y, and z) axes are also shown. You…

A: Answer:Orbital is a space around the nucleus where probability of finding an electron is maximum.

Q: Po b. Write the symbol of the element with the largest atomic radius in period 5. Fr c. Write the…

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Q: > 8. Detailed calculations show that the value of Zeff for the outermost electrons in Si and Cl…

A: Effective nuclear charge () is the actual or the net amount of positive charge gained by an electron…

Q: . The abbreviated electron configuration [Ar] 4s23d104p1 corresponds to the element: 2. The number…

Q: The ionization energy of magnesium is 737.75 kJ/mol while the ionization energy of aluminum is 577.6…

A: We have to tell which option is correct

Q: Why is Calcium, Ca (IE1 = 6.1132 eV) has a higher first ionization energy than Gallium, Ga (IR1 =…

A: Given: Calcium, Ca (IE1 = 6.1132 eV) has a higher first ionization energy than Gallium, Ga (IE1 =…

Q: 1. Given the elements below, rank them by the following categories and fully explain your reasoning!…

Q: Ive read the honor code and it says that their a question can have up to 3 subparts (i.e. part a, b,…

Q: Part C State whether this observed trend in ionization energies is supported by Slater's rules. O…

A: Higher the value of effective nuclear charge felt by an electron higher will be its ionisation…

Q: Which atom is more likely to lose an electron (has a lower ionization energy): Mg or S? Ca or F?…

A: (1) among Mg and S S will release the electron because the configuration is 1s2 2s2 2p6 3s2 3p4 to…

Q: Which of the following statements is true? A. The first ionization energy for potassium is greater…

A: Ionization energy (I.E.) is the minimum amount of energy needed to remove the most loosely bound…

Q: Give an example of a transition metal element with an irregular electron configuration (i.e. one…

Q: What are the condensed electron configuration of a. Li^+ b. Ca c. F^- d. Mg^2+ e. Al^3+ f. Which…

A: The electron configuration of an atom represented in form of its nearest noble-gas element of lower…

Q: How many unpaired electrons does phosphorous have in its highest energy subshell? (note: this is…

A: According to Pauli's Exclusion Principle, no two electrons in the same atom can have identical…

Q: A Chlorine atom has a first ionization energy of 1251.2 kJ/mol. Light of what frequency is required…

Q: Write equations corresponding to the first through fourth ionization energies for Mg. Between which…

A: Ionization energy, also called ionization potential, in chemistry and physics the amount of energy…

Q: a. Write the electron configuration for Ba²+. (Express your answer as a series of orbitals, in order…

A: Electronic configuration refers to the arrangement of electrons within an atom or an ion. It…

Question

Part A - Periodic Trends in lonization Energy
Consider the following statements about first ionization energies:
I. Because the effective nuclear charge for Mg is greater than that for Be, the first ionization energy of Mg is greater than that of Be.
II. The first ionization energy of O is less than that of N because in O we must pair electrons in the 2p orbitals.
III. The first ionization energy of Ar is less than that of Ne because a 3p electron in Ar is farther from the nucleus than a 2p electron in Ne.
Which of the statements , II, and III is or are true?
O Only one of the statements is true
O Statements I and Il are true
Statements I and III are true
Statements Il and III are true
O All three statements are true
Submit
Request Answer
Provide Feedback
O #Cn I
B.
Word
amazon
3000
P Type here to search
B-1080

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A. If an element with the valence configuration 4s'3d10 loses 2 electron(s), these electron(s) would be removed from the |subshell(s). B. An element with the valence electron configuration 4s²4p* would form a monatomic ion with a charge of In order to form this ion, the element will| |electron(s) from/into the| | subshell(s).
Peovide electron configurations of the both subparts of the question in clear handwritten on paper!
8
use the photon energies (Li E = 178.428 KJ/mol) to determine the valence orbital energies for both Li and Na. For lithium, the transition is from the 2p- to the 2s-orbital, and the 2s-orbital energy is –520.3 kJ/mol. Use this to find the energy of the 2p-orbitals in Li. For sodium, the higher-energy photon is emitted when the electron drops from one of the 3p-orbitals to the 3s-orbital, while the lower energy photon is emitted when the electron drops from one of the 3d-orbitals to one of the 3p-orbitals. Use these facts, along with the known energy of the 3s-orbital (–495.8 kJ/mol), to find the energies of the 3p- and 3d-orbitals.
Use noble gas notation to depict electron configurations for the following metals of the third transition series. (Express your answer using the noble gas notation. For example, the electron configuration of Li would be entered as [He]2s¹.) a. Tungsten, W. Tungsten is mainly used in the production of hard materials based on tungsten carbide. b. Gold, Au. Gold and its alloys are used in monetary exchange, jewelry, and investment.
14. The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. How do you explain the great jump in ionization energy after the first electron is removed?
6. Using Slater's rules, calculate the Zeff on one of the 3d electrons compared to that on one of the 4s electrons for Mn. 7. Using Slater's rules, calculate the Zef on a 3p electron in Al and in Cl. Explain how your results relate to a. the relative atomic radii of the two atoms. b. the relative first ionization energies of the two atoms.
A. An element with the valence electron configuration 5s' would form a monatomic ion with a charge of In order to form this ion, the element will| v electron(s) from/into the| subshell(s). B. An element with the valence electron configuration 4s²4p would form a monatomic ion with a charge of In order to form this ion, the element will v electron(s) from/into the v subshell(s).
Use what you know about the valence electron configuration of silver, Ag, to explain why it is a transition metal with a fixed charge (it always forms a +1 cation)
Imagine a universe where there are three spin states for the electron instead of two (for example, spin up, spin down, and spin cray-cray). The number of subshells per shell and number of orbitals per subshell stay the same, but an orbital now holds three electrons instead of two. The names of the elements stay the same. Draw the top three rows of what this new periodic table would look like, indicating which elements are in which groups in our new universe, and show the electron configurations of each of the elements of these three rows.