Practice Questions for Year 11 Chemistry Module 1: Properties and Structure of Matter

Question 11

A student has found that sample A emitted blue/purple light while sample B emitted red light. Based on their observations, deduce what elements sample A or B might be and provide explanations for your choice (4 marks).

(L2.4: investigate energy levels in atoms and ions through collecting primary data from a flame test using different ionic solutions of metals)

Question 12

Assess the advantages and limitations of the Bohr model and the Schrödinger model as an account for spectral analysis. (6 marks) 

(L2.4: investigate energy levels in atoms and ions through examining spectral evidence for the Bohr model and introducing the Schrödinger model)

Question 13

A scientist has found a new element, X and has derived the following to describe the new element: 

Predict whether this new element is stable or unstable. Provide explanations (3 marks).

(L2.5: investigate the properties of unstable isotopes using natural and human-made radioisotopes as examples, including but not limited to types of radiation and types of balanced nuclear reactions)

Question 14

Write the nuclear decay equation that results in the following isotopes with their respective decay. (5 marks)

a) Th-234 (alpha decay)

b) U-234 (beta decay)

c) Ra-226 (alpha decay) 

d) Xe-131 (beta decay) 

(L2.5: investigate the properties of unstable isotopes using natural and human-made radioisotopes as examples, including but not limited to types of radiation and types of balanced nuclear reactions)

Periodicity:

Inquiry Question: Are there patterns in properties of elements? 

Question 15

With reference to the periodic table, explain how trends in its periods and groups can be used to predict an element’s reactivity, electronegativity and state of matter at room temperature. (4 marks)

(L3.1: demonstrate, explain and predict the relationships in the observable trends in the physical and chemical properties of elements in periods and groups in the periodic table, including but not limited to the state of matter at room temperature, electronic configurations and atomic radii, first ionisation energy and electronegativity and reactivity with water)

Question 16

A scientist has found an element with a large atomic radii.

What implications does this have on its electronic configuration, reactivity with water and most probable state of matter at room temperature? Provide explanations. (6 marks) 

(L3.1: demonstrate, explain and predict the relationships in the observable trends in the physical and chemical properties of elements in periods and groups in the periodic table, including but not limited to the state of matter at room temperature, electronic configurations and atomic radii, first ionisation energy and electronegativity and reactivity with water)

Question 17

Explain why the second ionization energy is lower than the first ionization energy with reference to the structure and composition of the element. (3 marks) 

(L3.1: demonstrate, explain and predict the relationships in the observable trends in the physical and chemical properties of elements in periods and groups in the periodic table, including but not limited to the state of matter at room temperature, electronic configurations and atomic radii, first ionisation energy and electronegativity and reactivity with water)

Bonding

What binds atoms together in elements and compounds? 

Question 18

Using their electronegativities, determine whether the following elements will form an ionic or covalent bond. Include calculations. (10 marks) 

a) Sodium and fluoride 

b) Magnesium and oxygen 

c) Lead and chloride 

d) Potassium and sulfur 

e) Beryllium and Selenium 

(L4.1: investigate the role of electronegativity in determining the ionic or covalent nature of bonds between atoms)

Question 19

Using Lewis dot diagrams, explain the differences between the ionic bond between NaCl and the covalent bond of H2O. (4 marks) 

(L4.2: investigate the differences between ionic and covalent compounds through using nomenclature, valency and chemical formulae (including Lewis dot diagrams)

Question 20

Using named examples, explain how the electronegativity of atoms can be used to determine whether it will produce a polar compound. (3 marks) 

(L4.2: investigate the differences between ionic and covalent compounds through examining the spectrum of bonds between atoms with varying degrees of polarity with respect to their constituent elements’ positions on the periodic table

Question 21

Illustrate why the shape of a water molecule is bent and not linear. Include diagrams. (3 marks)

(L4.2: investigate the differences between ionic and covalent compounds through modelling the shapes of molecular substances)

Question 22

Carbon has many allotropes. Discuss how the structure of 3 carbon allotropes contribute to their uses. (7 marks) 

(L4.3: investigate elements that possess the physical property of allotropy)

Question 23

Account for the physical and chemical properties that result from the following chemical structures: (12 marks)

a) Ionic networks

b) Covalent networks

c) Covalent molecular

d) Metallic structure 

(L4.4: investigate the different chemical structures of atoms and elements, including but not limited to ionic networks, covalent networks (including diamond and silicon dioxide), covalent molecular and metallic structure)

Question 24

Explain how intramolecular and intermolecular bonds differ, with reference to its effect on the strength of a named compound (4 marks). 

Question 25

Between HCl, H2O and H2, which substance would have the highest intermolecular strength? Include diagrams in your explanation. (6 marks)

(L4.5: explore the similarities and differences between the nature of intermolecular and intramolecular bonds and the strength of the forces associated with each, in order to explain the physical properties of elements and physical properties of compounds)