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.

E M B I B E

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

MEDIUM

MYP:4-5

IMPORTANT

Earn 100

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.

Important Questions on Why do Electrons Matter?

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.

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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.

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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.

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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.

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