(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.

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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.

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Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?

5. The atoms and ions Ne, N³-, F, Mg2+, and Si4+ are part of an isoelectronic series. (a) Which of these will have the smallest effective nuclear charge acting on the outermost electron? (b) Which one possess the greatest effective nuclear charge? (c) Which ion will be the largest in size? Explain why.

Consider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?

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.

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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.

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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.

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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

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Answer 12

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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.

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