The Periodic Table: Classification of Elements (SL IB Chemistry)

The periodic table displays the chemical elements, arranged in order of increasing atomic number. It is made up of groups and periods of elements.

State and explain the general trend in first ionisation energy across a period of the periodic table.

The general trend in first ionisation energies stated in part (a) is seen across period 2 of the periodic table. However, boron and one other period 2 element deviate from this trend.

Identify this element and explain why it deviates from the general trend.

State why nitrogen is classed as a p block element and give its full electron configuration.

Identify the period 3 element that has the lowest melting point.

Explain your answer with reference to bonding and structure.

The first ionisation energy for all the elements is found in Section 9 of the IB data booklet.

The graph below in Figure 1 shows some information on the elements of period 3 of the periodic table.

Figure 1

State and explain the trend that this graph shows, including why there are values that deviate from the trend.

This question is about the structure of the periodic table.

Throughout the early history of the periodic table, scientists have attempted to order the elements according to different properties.

This question is about the element phosphorus.

Outline why the atomic radius is seen to decrease across period 2 (from lithium to fluorine).

Gallium forms an ion smaller than its element, whereas arsenic forms an ion larger than its element.

Explain these differences in ionic radius.

Bromine and selenium are both found in period 4 of the periodic table.

State and explain which of the two has a higher electronegativity.

Sketch on the axes shown below in Figure 1, a graph of the first ionisation energy against atomic number for the elements of Group 1.

Figure 1

Explain the trend in ionisation energy down group 1.

Discuss the similarities and differences between the trends in atomic radius and ionic radius down Group 1 and Group 17.

State how the first ionisation energy of potassium differs from that of:

Group 17 elements are known as highly electronegative non-metal elements.

Define the term electron affinity and write an equation to show the first electron affinity of bromine.

State, with reasons, whether the first electron affinity of iodine is more or less exothermic than bromine.

Suggest why the second electron affinity of oxygen is endothermic.

The hydrogen halides do not show perfect periodicity. A bar chart of boiling points, as seen in Figure 1, shows that the boiling point of hydrogen fluoride, HF, is much higher than periodic trends would indicate.

Figure 1

Explain why the boiling point of HF is much higher than the boiling point of the other hydrogen halides.

There is an increase in boiling point moving from HCl to HI.

Explain this trend in boiling points of the hydrogen halides.

A student dissolves the oxides of potassium and selenium in water and tests the resulting solutions with litmus paper.

Explain what the student would expect to observe.

Magnesium and silicon(V) oxides melt at high temperatures, unlike phosphorus(V) oxide and sulfur trioxide, which do so at lower temperatures.

State whether each of the four oxides would conduct electricity in their molten state.

For the solutions formed by dissolving the oxides in water in part (b), identify each as acidic, alkaline, or neutral.

Write equations for each of the reactions when the oxides of magnesium, phosphorus, and sulfur in part b) are dissolved in water.

Sodium oxide and silicon dioxide are two compounds of period 3 elements that react with water. Write equations for their separate reactions with water.

Suggest the pH of the resulting solutions when both sodium oxide and phosphorus(V) oxide react with water.

Aluminium oxide can react as both an acid and as a base.

Outline the acid-base nature of the oxides of the elements in period 3 from sodium to chlorine

Potassium is an element found in group 1 of the periodic table.

State how potassium reacts with water and write a balanced equation for the reaction including state symbols.

A student has a sample of lithium and sodium which he drops into a beaker of distilled water.

Compare the reactivity of lithium and sodium with water and state what the student would see in each reaction.

The student continues to react various group 1 metals with water and observes a change in reactivity as they move down the group.

Explain the trend in reactivity that would be observed.

From only the first three elements in each of Group 1 and Group 17, state which Group 1 element and Group 17 element would show the most vigorous reaction when they react together.

Write a balanced equation for the reaction.

Chlorine is a greenish-yellow gas, bromine is a dark red liquid, and iodine is a dark grey solid.

State and explain the property which most directly causes these differences in volatility.

Explain why Cl₂ rather than Br₂ would react more vigorously with a solution of I^-.

Describe what happens when aqueous bromine solution is added to separate solutions of sodium chloride and sodium iodide.

Include balanced equations for any reactions that occur.

Astatine, At, is the rarest naturally occurring element in the Earth’s crust. Before it was discovered in 1940 scientists could only predict its existence and properties.

Suggest the basis for these predictions.

When excess ammonia is added to copper(II) chloride solution, the dark blue complex ion, [Cu(NH₃)₄(H₂O)₂]²⁺, forms. 

State the molecular geometry of this complex ion and the bond angles within it.

This question refers to the elements in the first three periods of the Periodic Table.

Select an element from the first three periods that fits each of the following descriptions.

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This question is about the elements which have atomic numbers 33 to 37.

The first ionisation energies of these elements are shown in the table below.

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The first 3 elements of Period 3 show a general increase in melting point.

Explain this trend in melting point across these Period 3 elements.

This question is about hydrogen, the element with the atomic number Z = 1.

Hydrogen can be placed in several different positions in periodic tables. One is immediately above lithium in Group 1 as shown in section 6 of the data booklet. Another is in the centre of the first row.

Evaluate the position of hydrogen when it is placed immediately above lithium and state one reason in favour and two against. 

This question is about Period 4 of the Periodic Table. 

State and explain which of K⁺ and Ca²⁺ is the smaller ion.

Write the electron configuration for a Ca⁺ ion.

The first ionisation energies of the elements H to K are shown below.

State and explain the trend in first ionisation energies shown by the elements with the atomic numbers 2, 10 and 18.

Electrons in atoms occupy orbitals.

The figure below shows the first ionisation energies for six consecutive elements labelled A–F. 

Complete the graph of the first ionisation energies for the next five elements.

Explain why the value of the first ionisation energy for D is greater than for C.

The sequence of the first three elements in the Periodic Table is hydrogen, helium and then lithium.

Explain why the first ionisation energy of hydrogen is less than that of helium but greater than that of lithium.

First ionisation energies decrease down groups in the Periodic Table.

Explain this trend and the effect on the reactivity of groups containing metals.

The ionisation energy values show a general increase across period 4 from gallium to krypton.

State and explain how selenium deviates from this trend. 

Give one other element from period 2 or 3 which also deviates from this general trend, similar to selenium.

State and explain the trends in electronegativity down group 2 and across period 3.

Describe the trends in first ionisation energy and atomic radius as you move up Group 1. 

Potassium reacts with water to form hydrogen gas. Using sections 1 and 2 of the data booklet, determine the volume, in cm³, of hydrogen gas that could theoretically be produced at 273 K and 1.01105 Pa when 0.0587 g of potassium reacts with excess water.

Write equations for the separate reactions of lithium oxide and carbon dioxide with excess water and differentiate between the solutions formed. 

Lithium oxide................

Carbon dioxide.............

Differentiation..............

Suggest why it is surprising that dinitrogen monoxide dissolves in water to give a neutral solution.

Calcium carbide reacts with water to form ethyne, C₂H₂, and one other product_.

Estimate the pH of the resultant solution.

Impurities cause phosphine to ignite spontaneously in the air to form an oxide of phosphorus and water.

The oxide formed in the reaction with air contains 56.3 % phosphorus by mass. Determine the empirical formula of the oxide, showing your method.

The molar mass of the oxide is approximately 220 g mol⁻¹. Determine the molecular formula of the oxide.

State the equation for the reaction of this oxide of phosphorus with water.

Predict how dissolving an oxide of phosphorus would affect the electrical conductivity of water.

Iron is a transition element that forms several ions with iron in different oxidation states.

Deduce the condensed electron configuration of the iron cation that can form the complex ion [Fe(CN)₆]⁴⁻.

1,2-diaminoethane is a bidentate ligand which can form a complex with [Co(NH₃)₄(H₂O)₂]²⁺. In this reaction, only the ammonia molecules are replaced.                                              

i)    Write an equation for this reaction.

ii)          State the molecular geometry of the complex formed.

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