(a) Interpretation: The reason as to why ionization energy should increase as atomic number increases within a period is to be stated. Concept introduction: The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Question

Want to see the full answer?

Answer 1

Question

Chapter 11, Problem 109E

Interpretation Introduction

(a)

Interpretation:

The reason as to why ionization energy should increase as atomic number increases within a period is to be stated.

Concept introduction:

The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Interpretation Introduction

(b)

Interpretation:

The features of electron configurations with the locations of the breaks in Periods 2 and 3 shown in Figure 11-31 are to be correlated.

Concept introduction:

Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

(a) Write the electron configuration for Li and estimate theeffective nuclear charge experienced by the valence electron.(b) The energy of an electron in a one-electron atom or ion equals (-2.18 x 10-18 J) aZ2/n2 b, where Z is the nuclear chargeand n is the principal quantum number of the electron. Estimatethe first ionization energy of Li. (c) Compare the resultof your calculation with the value reported in Table 7.4 andexplain the difference. (d) What value of the effective nuclearcharge gives the proper value for the ionization energy? Doesthis agree with your explanation in part (c)?

Use electron configurations to explain the following observations:(a) The first ionization energy of phosphorus is greaterthan that of sulfur. (b) The electron affinity of nitrogen islower (less negative) than those of both carbon and oxygen.(c) The second ionization energy of oxygen is greater thanthe first ionization energy of fluorine. (d) The third ionizationenergy of manganese is greater than those of both chromiumand iron.

Answer 2

Question

Chapter 11, Problem 109E

Interpretation Introduction

(a)

Interpretation:

The reason as to why ionization energy should increase as atomic number increases within a period is to be stated.

Concept introduction:

The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Interpretation Introduction

(b)

Interpretation:

The features of electron configurations with the locations of the breaks in Periods 2 and 3 shown in Figure 11-31 are to be correlated.

Concept introduction:

Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 11, Problem 109E

Interpretation Introduction

(a)

Interpretation:

The reason as to why ionization energy should increase as atomic number increases within a period is to be stated.

Concept introduction:

The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Interpretation Introduction

(b)

Interpretation:

The features of electron configurations with the locations of the breaks in Periods 2 and 3 shown in Figure 11-31 are to be correlated.

Concept introduction:

Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 11, Problem 109E

Interpretation Introduction

(a)

Interpretation:

The reason as to why ionization energy should increase as atomic number increases within a period is to be stated.

Concept introduction:

The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Interpretation Introduction

(b)

Interpretation:

The features of electron configurations with the locations of the breaks in Periods 2 and 3 shown in Figure 11-31 are to be correlated.

Concept introduction:

Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 11, Problem 109E

Interpretation Introduction

(a)

Interpretation:

The reason as to why ionization energy should increase as atomic number increases within a period is to be stated.

Concept introduction:

The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Interpretation Introduction

(b)

Interpretation:

The features of electron configurations with the locations of the breaks in Periods 2 and 3 shown in Figure 11-31 are to be correlated.

Concept introduction:

Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.

Answer 6

Chapter 11, Problem 109E

Interpretation Introduction

(a)

Interpretation:

The reason as to why ionization energy should increase as atomic number increases within a period is to be stated.

Concept introduction:

The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Answer 7

Chapter 11, Problem 109E

Interpretation Introduction

(a)

Interpretation:

The reason as to why ionization energy should increase as atomic number increases within a period is to be stated.

Concept introduction:

The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.

Answer 8

Interpretation Introduction

(b)

Interpretation:

The features of electron configurations with the locations of the breaks in Periods 2 and 3 shown in Figure 11-31 are to be correlated.

Concept introduction:

Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The features of electron configurations with the locations of the breaks in Periods 2 and 3 shown in Figure 11-31 are to be correlated.

Concept introduction:

Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.

Answer 10

Expert Solution & Answer

Answer 11

Expert Solution & Answer

Answer 12

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 13

Ch. 11 - Prob. 1E Ch. 11 - Prob. 2E Ch. 11 - Identify measurable wave properties that are used...Ch. 11 - Prob. 4E Ch. 11 - Which among the following are not quantized? a...Ch. 11 - Which of the following are quantized? a canned...Ch. 11 - Prob. 7E Ch. 11 - In the Bohr model of the hydrogen atom, the...Ch. 11 - Prob. 9E Ch. 11 - Prob. 10E

Solution Summary: The author explains why ionization energy should increase as atomic number increases within a period. The highest occupied energy level indicates the period and the number of valence electrons indicate to the groups.

Want to see the full answer?

Chapter 11 Solutions