Patterns in the Periodic Table: Practice Questions

A solution containing both potassium chloride and potassium iodide is tested. Which of the following observations correctly identifies the outcome when aqueous chlorine is added to this mixture, followed by the addition of acidified silver nitrate?

Four metals \(\text{W}\), \(\text{X}\), \(\text{Y}\), and \(\text{Z}\) undergo the following reactions:
1. Metal \(\text{W}\) displaces metal \(\text{X}\) from an aqueous solution of its nitrate.
2. Heating the oxide of \(\text{Z}\) with carbon produces \(\text{Z}\), but heating the oxide of \(\text{W}\) with carbon causes no reaction.
3. Metal \(\text{Y}\) does not react with cold water or steam, whereas metal \(\text{X}\) reacts with steam.

What is the order of reactivity of these four metals, from most reactive to least reactive?

An atom of element \(\text{M}\) has a nuclide notation of \(^{31}_{15}\text{M}\). Which of the following correctly gives the position of element \(\text{M}\) in the Periodic Table, the formula of its stable hydride, and the nature of its oxide?

Which of the following sets of trends correctly describes the changes observed in Group 1 (alkali metals) and Group 17 (halogens) as the atomic number increases down each group?

Three elements \(X\), \(Y\), and \(Z\) are located in Period 3 of the Periodic Table. \(X\) is a Group 1 alkali metal, \(Y\) is in a group with intermediate properties, and \(Z\) is a Group 17 halogen. Which of the following correctly describes the trend in properties as one moves across the period from \(X\) to \(Z\)?

A) Electrical conductivity increases and metallic character increases.
B) Electrical conductivity decreases and metallic character decreases.
C) Atomic radius increases and electronegativity decreases.
D) Number of valence electrons decreases and oxide character changes from acidic to basic.

Three halogen elements, \(P\), \(Q\), and \(R\), belong to Group 17 of the Periodic Table. Aqueous solutions of their sodium salts were tested against each other. Element \(P\) can displace element \(Q\) from its aqueous salt solution, but cannot displace element \(R\). Furthermore, the silver nitrate test on the aqueous salt of \(Q\) yields a yellow precipitate. Which of the following correctly identifies \(P\), \(Q\), and \(R\), and describes the trend in first ionisation energy among them?

A) \(P\) is bromine, \(Q\) is iodine, \(R\) is chlorine; first ionisation energy decreases from \(R\) to \(Q\).
B) \(P\) is bromine, \(Q\) is chlorine, \(R\) is fluorine; first ionisation energy increases from \(R\) to \(Q\).
C) \(P\) is chlorine, \(Q\) is iodine, \(R\) is bromine; first ionisation energy decreases from \(R\) to \(Q\).
D) \(P\) is iodine, \(Q\) is bromine, \(R\) is chlorine; first ionisation energy increases down the group.

An element \(X\) is located in Period 4 and Group 1 of the Periodic Table, while another element \(Y\) is located in Period 3 and Group 17 of the Periodic Table. When element \(X\) reacts with element \(Y\), a stable ionic compound is formed.

Which of the following statements concerning elements \(X\) and \(Y\) and their compound is correct?

A) Element \(X\) has a higher melting point than lithium and is harder than transition metals.

B) Element \(Y\) is a liquid at room temperature and its aqueous solution yields a white precipitate with acidified silver nitrate.

C) Element \(X\) reacts more vigorously with cold water than sodium does, producing hydrogen gas and an alkaline solution.

D) The compound formed between \(X\) and \(Y\) has a low melting point and conducts electricity in the solid state.