The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons. The table below shows the first electron affinity for selected atoms. The first electron affinity of oxygen is - 141 kJ · mol - 1 . The equation for the first electron affinity of oxygen is O ( g ) + e - → O - ( g ) . Formulate an equation (with state symbols) for the second electron affinity of oxygen.

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons, resulting in a mole of gaseous anions (negative ions). It is expressed in units of kJ · mol - 1 . So the meaning of ‘the first electron affinity of oxygen is - 141 kJ · mol - 1 ' means that 141 kJ · mol - 1 of energy is released when one mole of gaseous oxygen atoms gains a mole of electrons, resulting in a mole of gaseous anions ( O - ion). O ( g ) + e − → O − ( g ) First electron affinity = - 141 kJ · mol - 1 The second electron affinity of oxygen is the energy required to add a mole of electrons to one mole of gaseous O - ions to produce one mole of gaseous O 2 - ions. An equation (with state symbols) for the second electron affinity of oxygen is: O − ( g ) + e − → O 2 - ( g )

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons. The table below shows the first electron affinity for selected atoms. The first electron affinity of oxygen is - 141 kJ · mol - 1 . Explain why, in terms of electrostatics, oxygen has a lower first electron affinity than chlorine.

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons, resulting in a mole of gaseous anions (negative ions). It is expressed in units of kJ · mol - 1 . So the more negative the electron affinity the more favourable the electron addition process is. Not all elements form stable negative ions in which case the electron affinity is zero or even positive. Less energy is required to add an electron from atoms of elements on the left-hand side of the periodic table, which have larger radii and small numbers of valence electrons, compared to adding electrons to elements on the right-hand side. For similar reasons, radii increase down each group of the periodic table and less energy is required to add electrons to atoms of elements with increasing numbers of electron shells. Hence, the electron affinity value increases along a period from left to right. In group 18 , the valence shell is full, meaning that added electrons are unstable, tending to be ejected very quickly. Going down a group in the modern periodic table, the electron affinity decreases since the electron is being added increasingly further away from the atom. Among the given elements, the halogen chlorine will have the most negative electron affinity value and hence it will have the most favourable electron addition process. Going down group 17 , the other halogen after chlorine will have lesser negative values gradually, such as bromine and then the iodine. Oxygen belongs to group 16 and period 2 of the periodic table and hence will have a lesser negative electron affinity value as compared to the halogens given. Hence, oxygen has a lower first electron affinity than chlorine.

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons. The table below shows the first electron affinity for selected atoms. The first electron affinity of oxygen is - 141 kJ · mol - 1 . In terms of electrostatics, oxygen has a lower first electron affinity than chlorine. Explain why neon has a positive value of electron affinity.

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons, resulting in a mole of gaseous anions (negative ions). It is expressed in units of kJ · mol - 1 . So the more negative the electron affinity the more favourable the electron addition process is. Not all elements form stable negative ions in which case the electron affinity is zero or even positive. Less energy is required to add an electron from atoms of elements on the left-hand side of the periodic table, which have larger radii and small numbers of valence electrons, compared to adding electrons to elements on the right-hand side. For similar reasons, radii increase down each group of the periodic table and less energy is required to add electrons to atoms of elements with increasing numbers of electron shells. Hence, the electron affinity value increases along a period from left to right. In group 18 , the valence shell is full, meaning that added electrons are unstable, tending to be ejected very quickly. Going down a group in the modern periodic table, the electron affinity decreases since the electron is being added increasingly further away from the atom. Thus, noble gases like neon have a positive electron affinity value indicating the unstable anion formation. Hence, explained why neon has a positive value of electron affinity.

A hydrogen atom has the main energy levels (shells) shown in the diagram below. n refers to the shell number. This is the Bohr model of the atom. Describe the electron transition (movement) within the hydrogen atom using the shell numbers indicated above, that will release the most energy.

According to Bohr’s model of atomic structure, when an electron absorbs a specific, fixed amount of energy (called a quantum) it is promoted to a different orbit. The same amount of energy is re-emitted as electromagnetic radiation when the electron drops back to its lower energy level. Thus, the most energy will be released when the electron in the hydrogen atom given, jumps from shell numbers indicated by n = 4 to n = 1 .

A hydrogen atom has the main energy levels (shells) shown in the diagram below. n refers to the shell number. This is the Bohr model of the atom. Describe the electron transition (movement) within the hydrogen atom using the shell numbers indicated above, that will absorb the least energy.

Niels Bohr ( 1885 — 1962 ) suggested electrons occupied orbits around the nucleus, and that the volume of the space occupied by electrons around the nucleus depended on the energy of the electrons. These possible locations for electrons at different distances from the nucleus are also called shells or main energy levels. When an electron absorbs a specific, fixed amount of energy (called a quantum) it is promoted to a different orbit. The same amount of energy is re-emitted as electromagnetic radiation when the electron drops back to its lower energy level. Bohr’s model of atomic structure used a hydrogen atom, but his theories apply generally to the arrangement of electrons of atoms of all elements. Thus, the least energy will be absorbed when the electron in the hydrogen atom given, jumps from shell numbers indicated by n = 3 to n = 4 .

A hydrogen atom has the main energy levels (shells) shown in the diagram below. n refers to the shell number. This is the Bohr model of the atom. List these electron transitions in order of increasing wavelength of light absorbed or emitted: n = 1 to n = 2 n = 3 to n = 2 n = 2 to n = 4 n = 3 to n = 1

Niels Bohr ( 1885 — 1962 ) suggested electrons occupied orbits around the nucleus, and that the volume of the space occupied by electrons around the nucleus depended on the energy of the electrons. These possible locations for electrons at different distances from the nucleus are also called shells or main energy levels. When an electron absorbs a specific, fixed amount of energy (called a quantum) it is promoted to a different orbit. The same amount of energy is re-emitted as electromagnetic radiation when the electron drops back to its lower energy level. The electron transitions in order of an increasing wavelength of light absorbed or emitted are as follows: n = 3 to n = 2 < n = 2 to n = 4 < n = 1 to n = 2 < n = 3 to n = 1

A hydrogen atom has the main energy levels (shells) shown in the diagram below. n refers to the shell number. This is the Bohr model of the atom. Explain why a ladder is a good analogy or model for visualising the energy levels of atoms (and molecules), and what are the limitations of the analogy.

According to Bohr's model of an atom, the electrons encircle the nucleus of the atom in specific allowable paths called orbits. When the electron is in one of these orbits, its energy is fixed. The ground state of the hydrogen atom, where its energy is lowest, is when the electron is in the orbit that is closest to the nucleus. The orbits that are farther from the nucleus are of the successively greater energy. The electron is not allowed to occupy any of the spaces in between the orbits. An everyday analogy to the Bohr model is the rungs of a ladder. As we move up or down a ladder, we can only occupy specific rungs and cannot be in the spaces in between rungs. Moving up the ladder increases our potential energy while moving down the ladder decreases our energy. The limitations are, unlike a ladder, which has a limited length, the energy levels of an atom extend infinitely out from the nucleus and the energy levels are not evenly spaced. In Bohr's model of an atom, as the distance from the nucleus increases, the levels get closer together and contain more-energetic electrons. The energy of an electron in one of the levels at a considerable distance from the nucleus is greater than that of an electron at a closer level.

Annie Termaat and Christopher Talbot Solutions for Chapter: Why do Electrons Matter?, Exercise 19: SOME SUMMATIVE PROBLEMS TO TRY

Author:Annie Termaat & Christopher Talbot

Annie Termaat Chemistry Solutions for Exercise - Annie Termaat and Christopher Talbot Solutions for Chapter: Why do Electrons Matter?, Exercise 19: SOME SUMMATIVE PROBLEMS TO TRY

Attempt the free practice questions on Chapter 8: Why do Electrons Matter?, Exercise 19: SOME SUMMATIVE PROBLEMS TO TRY with hints and solutions to strengthen your understanding. MYP By Concept 4&5 Chemistry solutions are prepared by Experienced Embibe Experts.

Questions from Annie Termaat and Christopher Talbot Solutions for Chapter: Why do Electrons Matter?, Exercise 19: SOME SUMMATIVE PROBLEMS TO TRY with Hints & Solutions

MEDIUM

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 11

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons. The table below shows the first electron affinity for selected atoms.

Question Image

The first electron affinity of oxygen is

- 141 kJ \cdot {mol}^{- 1}

The equation for the first electron affinity of oxygen is $O (g) + e^{-} \to O^{-} (g)$ .

Formulate an equation (with state symbols) for the second electron affinity of oxygen.

HARD

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 11

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons. The table below shows the first electron affinity for selected atoms.

Question Image

The first electron affinity of oxygen is

- 141 kJ \cdot {mol}^{- 1}

Explain why, in terms of electrostatics, oxygen has a lower first electron affinity than chlorine.

MEDIUM

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 11

The first electron affinity is the energy change when one mole of gaseous atoms gains a mole of electrons. The table below shows the first electron affinity for selected atoms.

Question Image

The first electron affinity of oxygen is

- 141 kJ \cdot {mol}^{- 1}

In terms of electrostatics, oxygen has a lower first electron affinity than chlorine.

Explain why neon has a positive value of electron affinity.

MEDIUM

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 12

A hydrogen atom has the main energy levels (shells) shown in the diagram below. $n$ refers to the shell number. This is the Bohr model of the atom.

Question Image

Describe the electron transition (movement) within the hydrogen atom using the shell numbers indicated above, that will release the most energy.

MEDIUM

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 12

A hydrogen atom has the main energy levels (shells) shown in the diagram below. $n$ refers to the shell number. This is the Bohr model of the atom.

Question Image

Describe the electron transition (movement) within the hydrogen atom using the shell numbers indicated above, that will absorb the least energy.

HARD

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 12

A hydrogen atom has the main energy levels (shells) shown in the diagram below. $n$ refers to the shell number. This is the Bohr model of the atom.

Question Image

List these electron transitions in order of increasing wavelength of light absorbed or emitted:

$n = 1$ to $n = 2$
$n = 3$ to $n = 2$
$n = 2$ to $n = 4$
$n = 3$ to $n = 1$

HARD

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 12

A hydrogen atom has the main energy levels (shells) shown in the diagram below. $n$ refers to the shell number. This is the Bohr model of the atom.

Question Image

Explain why a ladder is a good analogy or model for visualising the energy levels of atoms (and molecules), and what are the limitations of the analogy.

HARD

MYP:4-5

IMPORTANT

MYP By Concept 4&5 Chemistry>Chapter 8 - Why do Electrons Matter?>SOME SUMMATIVE PROBLEMS TO TRY>Q 13

Analyse and evaluate the data about ionic compounds that are listed in the table below.

Identify and make scientifically supported judgments to explain any relationships between the size (radius) of ions present, and the predicted properties of their compounds. Your explanation should refer to your knowledge of ions, ionic bonding and the behaviour of electric charges. State any assumptions in your explanation.

Question Image

Annie Termaat and Christopher Talbot Solutions for Chapter: Why do Electrons Matter?, Exercise 19: SOME SUMMATIVE PROBLEMS TO TRY

Annie Termaat Chemistry Solutions for Exercise - Annie Termaat and Christopher Talbot Solutions for Chapter: Why do Electrons Matter?, Exercise 19: SOME SUMMATIVE PROBLEMS TO TRY

Questions from Annie Termaat and Christopher Talbot Solutions for Chapter: Why do Electrons Matter?, Exercise 19: SOME SUMMATIVE PROBLEMS TO TRY with Hints & Solutions

Learn and Prepare for any exam you want !