You're viewing free preview questions. Upgrade to access more MYP4 questions.Upgrade
Atomic Structure and the Periodic Table

Atomic Structure and the Periodic Table — Free MYP4 Chemistry Practice Questions

1QuestionMetals Non-Metals and MetalloidsConcept Practice
2 marks~3 minCriterion B
Outline the steps of an experiment to test whether a given sample is a metal, non-metal, or metalloid. The apparatus diagram shows a circuit with a battery, a bulb, and two wires ending in clips to hold the sample, plus a hammer and a tile.
Question diagram

Solutions

2QuestionStructure of the Nucleus and Electron ShellsConcept Practice
2 marks~3 minCriterion B
The electron configurations of the first four elements are:

Hydrogen: 1s11s^1
Helium: 1s21s^2
Lithium: 1s22s11s^2 2s^1
Beryllium: 1s22s21s^2 2s^2
a
Identify the pattern in how electrons fill subshells as atomic number increases from hydrogen to beryllium. [1]
b
Deduce the electron configuration of boron (Z=5Z = 5), justifying your answer using the pattern identified in part (a). [1]

Solutions

3QuestionDevelopment of Atomic Models Dalton to BohrConcept Practice
4 marks~6 minCriterion A
The diagrams below show two historical models of the atom.

Diagram A: Dalton's model — a solid, featureless sphere.
Diagram B: Thomson's model — a sphere of uniform positive charge with electrons embedded within it.
a
State what Dalton's model proposes about the internal structure of the atom. [1]
b
Describe the internal structure proposed by Thomson's model. [1]
c
Analyse how Thomson's model challenged a fundamental assumption of Dalton's model, and explain what this change implied about the divisibility of the atom. [2]
Question diagram

Solutions

4QuestionDefinition and Examples of IsotopesConcept Practice
2 marks~3 minCriterion A
Iodine-123 (123^{123}I) is a radioactive isotope used in hospitals to image a patient's thyroid gland. A small quantity is administered to the patient, and its gamma emissions are detected to produce a diagnostic image.
a
Outline what makes 123^{123}I an isotope of iodine. [1]
b
A patient undergoing this procedure expresses concern about radiation exposure. Discuss one limitation of using 123^{123}I for thyroid imaging that is directly related to this concern. [1]
Question diagram

Solutions

5QuestionElectron Configuration NotationConcept Practice
3 marks~5 minCriterion A
Sodium (Na) has the electron configuration 2,8,12, 8, 1 and chlorine (Cl) has the electron configuration 2,8,72, 8, 7.
a
State the electron transfer each atom must undergo to achieve a stable noble gas configuration. [1]
b
Using the octet rule and the electron configurations of Na and Cl, explain why each atom achieves greater stability by the transfer you described in (a) rather than the alternative. [2]
Question diagram

Solutions

6QuestionIdentifying Groups Periods and Atomic NumberAssessment Practice
8 marks~12 minCriterion D
Neodymium (Nd\text{Nd}, Z=60Z = 60), dysprosium (Dy\text{Dy}, Z=66Z = 66), and lanthanum (La\text{La}, Z=57Z = 57) are rare-earth elements used in high-strength permanent magnets for electric vehicle (EV) motors. All three are in Period 6, Group 3 of the periodic table. They are mined predominantly at Bayan Obo, Inner Mongolia, China. Extraction releases thorium (Th\text{Th}, Z=90Z = 90, Period 7, Group 3) as a mildly radioactive byproduct and requires removal of large amounts of overburden, causing habitat destruction.
a
Explain why Nd\text{Nd}, Dy\text{Dy}, and La\text{La} are chemically similar and tend to occur together in the same ore deposits, using their positions in the periodic table. [2]
b
Identify and explain one societal benefit of extracting these rare-earth elements for EV magnets. [2]
c
Analyse one environmental trade-off associated with the extraction of these elements, using evidence from the context above. [2]
d
Discuss why recycling rare-earth elements from end-of-life EV magnets cannot, on its own, resolve the trade-offs identified in part (c). [2]
Question diagram

Solutions

7QuestionIdentifying Groups Periods and Atomic NumberAssessment Practice
8 marks~12 minCriterion A
When Group 1 metals react with water at room temperature, the following observations are recorded:

Lithium: fizzes gently, moves slowly on the water surface.
Sodium: fizzes vigorously, moves rapidly, melts into a ball.
Potassium: reacts violently, ignites with a lilac flame, moves extremely fast.
a
Identify the trend in reactivity down Group 1 and use the observations above to support your answer. [2]
b
Rubidium (Rb) is a Group 1 element below potassium. Deduce the products of its reaction with water and write a balanced chemical equation, including state symbols. [2]
c
Justify the predicted reactivity of rubidium relative to potassium by explaining how atomic radius, electron shielding, and ionisation energy change down Group 1, and linking these changes to the ease of losing the valence electron. [4]
Question diagram

Solutions

8QuestionGroup 17 Halogens and Group 18 Noble GasesAssessment Practice
4 marks~6 minCriterion C
Three test tubes each contain a colourless solution. Chlorine water (Cl2Cl_2) is added to each.

Test tube 1: potassium chloride (KClKCl)no colour change
Test tube 2: potassium bromide (KBrKBr)yellow-orange colour appears
Test tube 3: potassium iodide (KIKI)brown colour appears
a
State the reactivity trend of the halogens down Group 17. [1]
b
Explain why chlorine displaces bromine from KBrKBr and iodine from KIKI, but produces no change in KClKCl. [2]
c
The displacement of iodine from KIKI produces a more intense colour than the displacement of bromine from KBrKBr. A student claims this means iodine is more reactive than bromine. Evaluate this claim. [1]
Question diagram

Solutions

9QuestionTrends in Atomic Radius Ionization EnergyAssessment Practice
6 marks~9 minCriterion D
Dichlorodifluoromethane (CCl2F2CCl_2F_2), known as CFC-12, was widely used in refrigerators and aerosol sprays. When released into the atmosphere, it rises to the stratosphere where ultraviolet (UV) radiation breaks chemical bonds, releasing halogen atoms that can destroy ozone (O3O_3) molecules.

First ionization energies of the halogens in CFC-12:

F: 1681 kJ mol−11681 \ \text{kJ mol}^{-1}
Cl: 1251 kJ mol−11251 \ \text{kJ mol}^{-1}
a
Using the ionization energy data, explain why the C–F bond in CFC-12 is more resistant to UV breakdown than the C–Cl bond. [2]
b
Explain how the difference in bond stability between C–F and C–Cl bonds affects the ability of CFC-12 to deplete the ozone layer. [2]
c
Evaluate the reliability of using ionization energy alone to predict which halogen-containing compounds pose the greatest risk to the ozone layer. [2]
Question diagram

Solutions

10QuestionTrends in Atomic Radius Ionization EnergyAssessment Practice
6 marks~9 minCriterion A
The table below shows atomic radius and first ionisation energy for three consecutive Period 3 elements.

Atomic radius (pm): Na\text{Na}: 186, Mg\text{Mg}: 160, Al\text{Al}: 143

First ionisation energy (kJ mol−1^{-1}): Na\text{Na}: 496, Mg\text{Mg}: 738, Al\text{Al}: 578
a
Describe the trend in atomic radius from Na\text{Na} to Al\text{Al}, quoting the data. [2]
b
Explain, using nuclear charge and electron shielding, why atomic radius decreases across this period. [2]
c
Analyse the first ionisation energy data, accounting for both the general trend from Na\text{Na} to Al\text{Al} and the anomaly at Al\text{Al}. [2]
Question diagram

Solutions

11QuestionPredicting Properties of Unknown ElementsAssessment Practice
5 marks~8 minCriterion B
The table below shows atomic radius and first ionisation energy for Group 14 elements.

ElementCSiGeSnPbFl
Atomic radius (pm)77111125145175?
First ionisation energy (kJ/mol)1086787762709715?


Flerovium (Fl, element 114) is a synthetic Group 14 element positioned below lead.
a
Explain the trend in atomic radius from C to Pb, and deduce the atomic radius of Fl. [2]
b
Explain the trend in first ionisation energy from C to Pb, and deduce the first ionisation energy of Fl. [2]
c
Construct a balanced chemical equation, with state symbols, for the reaction of Fl with oxygen. Justify the oxidation state you have assigned to Fl, referring to trends in Group 14. [1]
Question diagram

Solutions

12QuestionPredicting Properties of Unknown ElementsAssessment Practice
3 marks~5 minCriterion C
The melting points of the Group 17 halogens are given below.

F2\text{F}_2: −220 °C-220\ °\text{C}
Cl2\text{Cl}_2: −101 °C-101\ °\text{C}
Br2\text{Br}_2: −7 °C-7\ °\text{C}
I2\text{I}_2: 114 °C114\ °\text{C}
a
Describe the trend in melting points down Group 17 from F2\text{F}_2 to I2\text{I}_2. [1]
b
Explain why this trend occurs, referring to intermolecular forces and molecular properties. [1]
c
Astatine (At2\text{At}_2) lies below iodine in Group 17. Evaluate whether the trend established in (a) and (b) is sufficient to predict a reliable melting point for At2\text{At}_2, and state your predicted value with justification. [1]
Question diagram

Solutions

13QuestionSubatomic Particles Protons Neutrons ElectronsAssessment Practice
6 marks~9 minCriterion D
Technetium-99m (99m^{99m}Tc) is a radioactive isotope widely used in medical imaging. It is produced from molybdenum-99 (99^{99}Mo), which is generated by uranium-235 fission in nuclear reactors. Technetium-99m decays by gamma emission with a half-life of 6 hours. Global supply depends on fewer than ten aging reactors, raising concerns about radioactive waste, reactor safety, and nuclear security.
a
Explain how the nuclear properties of technetium-99m make it suitable for medical imaging. [2]
b
Analyse the environmental and supply-chain risks created by the current method of producing molybdenum-99. [2]
c
Evaluate the overall societal trade-offs of continuing to use technetium-99m in healthcare, and justify whether investment in alternative production technologies is warranted. [2]
Question diagram

Solutions

14QuestionAtomic Number Mass Number and Nuclear SymbolAssessment Practice
5 marks~8 minCriterion C
A student investigates the hypothesis: "Atomic number, not mass number, determines the chemical identity of an element." A mass spectrometer analyses two chlorine isotopes and an unknown ion X, giving the following data:

Cl-35\text{Cl-35}: m/z=35.0m/z = 35.0, abundance =75.8%= 75.8\%, first ionization energy =1251 kJ mol−1= 1251 \ \text{kJ mol}^{-1}

Cl-37\text{Cl-37}: m/z=37.0m/z = 37.0, abundance =24.2%= 24.2\%, first ionization energy =1251 kJ mol−1= 1251 \ \text{kJ mol}^{-1}

Ion X\text{Ion X}: m/z=36.0m/z = 36.0, abundance =0.01%= 0.01\%, first ionization energy =1252 kJ mol−1= 1252 \ \text{kJ mol}^{-1}
a
State the number of protons, neutrons, and electrons in Cl-35\text{Cl-35} (assume singly charged cation). [1]
b
Explain why Cl-35\text{Cl-35} and Cl-37\text{Cl-37} are classified as the same element despite having different mass numbers. [2]
c
Evaluate which piece of experimental evidence — m/zm/z ratio, relative abundance, or first ionization energy — provides the strongest support for the hypothesis. Use data from all three species in your answer. [2]
Question diagram

Solutions

15QuestionStability of Isotopes and Radioactivity IntroAssessment Practice
4 marks~6 minCriterion B
The stability of an isotope depends on its neutron-to-proton ratio (n/pn/p). Data for five isotopes are given below.

IsotopeH-1H-2He-4C-14U-238
Protons112692
Neutrons0128146
n/pn/p ratio0.001.001.001.331.59
Stabilitystablestablestableradioactiveradioactive
a
Describe the relationship between the n/pn/p ratio and isotope stability, referring to specific values in the data above. [2]
b
Deduce whether oxygen-16 (8 protons, 8 neutrons) and oxygen-18 (8 protons, 10 neutrons) are stable or radioactive. Justify each prediction using the pattern from part (a). [2]

Solutions

16QuestionCalculating Relative Atomic Mass RAMAssessment Practice
6 marks~9 minCriterion D
A nuclear accident releases iodine-131 into a local water supply. Natural iodine consists entirely of iodine-127 (mass = 126.9045 u). A contaminated water sample contains 80% iodine-127 and 20% iodine-131 (mass = 130.9061 u) by number of atoms.
a
Calculate the relative atomic mass (RAM) of iodine in the contaminated sample. [2]
b
Deduce whether the altered RAM alone is sufficient to confirm the presence of iodine-131 contamination. Justify your reasoning with reference to the standard RAM of iodine. [2]
c
Evaluate the limitations of using RAM as a monitoring tool for iodine-131 contamination, with reference to the health risks posed by iodine-131 accumulation in the thyroid gland. [2]
Question diagram

Solutions

17QuestionDefinition and Examples of IsotopesAssessment Practice
5 marks~8 minCriterion C
Mass spectrometry of a chlorine sample produces two peaks:

m/z=35m/z = 35, relative abundance =75.8%= 75.8\%
m/z=37m/z = 37, relative abundance =24.2%= 24.2\%

A separate experiment determines the average atomic mass of chlorine to be 35.45 amu35.45 \text{ amu}.

The weighted-average formula for atomic mass is:

average atomic mass=(m1×a1)+(m2×a2)100\text{average atomic mass} = \frac{(m_1 \times a_1) + (m_2 \times a_2)}{100}

where m1m_1, m2m_2 are isotope masses and a1a_1, a2a_2 are their percentage abundances.
a
Calculate the average atomic mass of chlorine predicted by the two-isotope data. [2]
b
Deduce whether the experimentally determined value of 35.45 amu35.45 \text{ amu} is consistent with chlorine existing as only two stable isotopes. Justify your reasoning using your answer to part (a) and the concept of experimental error. [3]
Question diagram

Solutions

18QuestionRelating Configuration to ReactivityAssessment Practice
8 marks~12 minCriterion D
Sodium (Na) is used as a liquid coolant in some nuclear reactors; lithium (Li) powers rechargeable batteries in electric vehicles and portable electronics. Both metals are extracted through mining and chemical processing. Lithium-ion batteries can be recycled, but the process remains inefficient and uncommon. Sodium coolant leaks pose fire and explosion hazards, while damaged lithium batteries can overheat and ignite.
a
State the electronic configurations of Na and Li, and explain why both metals are highly reactive. [2]
b
Compare the societal benefits of sodium-cooled nuclear reactors with those of lithium-ion batteries. [2]
c
Discuss the environmental and safety limitations of both technologies, referring to mining impacts, recycling challenges, and fire hazards. [3]
d
Evaluate which technology presents a better overall balance of benefits and limitations, justifying your conclusion. [1]
Question diagram

Solutions

19QuestionUnderstanding Electron ShellsAssessment Practice
5 marks~8 minCriterion C
The successive ionisation energies for a magnesium atom are given below.

Electron removed1st2nd3rd4th5th6th7th8th9th10th
Ionisation energy (kJ/mol)7381450773010500136001800021700256003160035400
a
Calculate the difference in ionisation energy between the 2nd and 3rd electrons removed. [1]
b
Magnesium has the electron configuration 2, 8, 2. Using this configuration, explain why the ionisation energy increases more sharply between the 2nd and 3rd electrons than between any two consecutive electrons in the outermost shell. [2]
c
A student claims: "The steady increases seen from the 3rd to the 10th ionisation energies also support the electron shell model." Evaluate this claim, identifying what additional shell boundary is revealed in the data and justifying your reasoning. [2]
Question diagram

Solutions

20QuestionElectron Configuration NotationAssessment Practice
5 marks~8 minCriterion B
The table below shows first ionisation energies (kJ/mol) for elements Z=1Z = 1 to Z=20Z = 20.

H: 1312 — He: 2372 — Li: 520 — Be: 899 — B: 801 — C: 1086 — N: 1402 — O: 1314 — F: 1681 — Ne: 2081 — Na: 496 — Mg: 738 — Al: 578 — Si: 787 — P: 1012 — S: 1000 — Cl: 1251 — Ar: 1521 — K: 419 — Ca: 590

A two-shell hypothesis proposes that the first shell holds 2 electrons and the second shell holds all remaining electrons.
a
State what the two-shell hypothesis predicts about the trend in first ionisation energy from Z=3Z = 3 (Li) to Z=20Z = 20 (Ca). [1]
b
Identify two pairs of adjacent elements where the data contradict the two-shell hypothesis, and explain why each drop in ionisation energy indicates the start of a new electron shell. [2]
c
Evaluate whether the ionisation energy data support the modern shell-subshell model (filling pattern 2, 8, 8, 2), using the smaller drops at Be–B, N–O, Mg–Al, and P–S as evidence. [2]
Question diagram

Solutions