Electronic Configuration and Shell Model

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Electronic Configuration and Shell Model — Free MYP5 Chemistry Practice Questions

1QuestionElectron Configuration NotationConcept Practice

2 marks~3 minCriterion A

A sodium atom (

\text{Na}

) has 11 protons and therefore 11 electrons. The shell model places electrons in successive shells outward from the nucleus: the first shell holds a maximum of 2 electrons, the second shell holds a maximum of 8 electrons, and any remaining electrons occupy the third shell.

State the number of electrons in each shell of a sodium atom. [1]

Deduce the complete electron configuration of sodium in the notation used for the shell model, showing shells in order from innermost to outermost. [1]

Solutions

2QuestionRelating Configuration to ReactivityAssessment Practice

5 marks~8 minCriterion D

A water treatment plant disinfects drinking water using chlorine (Cl) gas. A chemist proposes switching to iodine (I) to reduce harmful by-products such as chlorinated hydrocarbons.

Electron configurations:
Cl: 2, 8, 7
I: 2, 8, 18, 18, 7

State the group and period of chlorine and iodine in the periodic table. [1]

Using their electron configurations, explain why iodine is less reactive than chlorine. [2]

Evaluate the proposal to replace chlorine with iodine for water disinfection, considering both the reduction in harmful by-products and the consequences of iodine's lower reactivity and excess iodine intake. [2]

Solutions

3QuestionElectronic Configuration of Ions IntroAssessment Practice

5 marks~8 minCriterion C

A student performs flame tests on four unknown metal compounds and records the following results:

Unknown X	Lilac, intensity 3
Unknown Y	Yellow-orange, intensity 8
Unknown Z	Brick red, intensity 4
Unknown W	Green, intensity 2

The student hypothesises: "Ions with a +2 charge always produce more intense flame colours than +1 ions."

Electron configurations of relevant metals:

\text{Na: } 1s^2 2s^2 2p^6 3s^1

(forms

\text{Na}^+

)

\text{K: } 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1

(forms

\text{K}^+

)

\text{Ca: } 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2

(forms

\text{Ca}^{2+}

)

Identify the metals most likely present in unknowns X, Y, and Z, and state the ion charge each metal forms. [2]

Using the electron configurations provided, explain why Na and K produce different flame colours despite both forming +1 ions. [1]

Evaluate whether the flame test data support or contradict the student's hypothesis, using specific intensity values in your answer. [2]

Solutions

4QuestionElectron Configuration NotationAssessment Practice

6 marks~9 minCriterion B

Emission spectra data for four elements are shown below.

Element	H	He	Li	Be
Number of visible spectral lines	4	15	1	10
Electron configuration	$1s^1$	$1s^2$	$1s^2 2s^1$	$1s^2 2s^2$

Analyse the data to identify the relationship between the number of visible spectral lines and the number of valence electrons for these four elements. [2]

The emission spectrum of boron (B) shows 5 visible spectral lines. Deduce the full electron configuration of boron, using the pattern you identified in (a). [2]

Explain, with reference to the shell model of the atom, why more valence electrons in the same principal energy level do not always produce more visible spectral lines than elements in a lower principal energy level. [2]

Solutions

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