Predict the physical state of Francium (Fr) at room temperature (25 °C). Justify your answer using the trend in the Group 1 metals.

Predict how the melting point of Rubidium (Rb) compares to that of Potassium (K). Explain your reasoning.

The densities of Group 1 metals generally increase going down the group. Predict whether Caesium (Cs) is denser or less dense than Sodium (Na). State one anomaly to this trend.

Predict the appearance and hardness of Francium metal compared to Lithium. Give a reason for the difference in hardness.

The atomic radii of Group 1 metals are: Li = 152 pm, Na = 186 pm, K = 227 pm, Rb = 248 pm. (a) Describe the trend. (b) Predict the atomic radius of Caesium. (c) Explain why atomic radius increases down the group.

Describe the expected reaction of Caesium with cold water. Compare it to the reaction of Sodium with cold water in terms of: (i) vigour, (ii) ignition of hydrogen gas, (iii) speed.

Predict what you would observe if a small piece of Rubidium is placed into a Universal Indicator solution. Give two observations.

Explain, in terms of electronic structure, why Caesium reacts more vigorously with water than Lithium does.

Francium has not been observed reacting with water in a laboratory setting. (a) Predict what would happen if it did react. (b) Give one reason why this reaction cannot be easily studied. (c) State the name of the product formed in solution.

Predict whether Rubidium would react with oxygen in the air. If yes, describe what you would observe and name the product.

Write the word equation for the reaction of Rubidium with water.

Write the balanced symbol equation for the reaction of Caesium with water. Include state symbols.

Write the balanced symbol equation for the reaction of Potassium with oxygen to form Potassium oxide.

Lithium reacts with water to produce a solution with a pH of 14. (a) Write the ionic equation for this reaction. (b) Identify the spectator ion. (c) Identify the ion responsible for the high pH.

A student adds an unknown Group 1 metal X to water. The reaction is more violent than Sodium but less violent than Caesium. The solution formed turns red litmus blue. (a) Identify the metal. (b) Write the full balanced equation with state symbols. (c) Calculate the volume of hydrogen gas produced at RTP when 8.5 g of X reacts completely with excess water. (Molar volume at RTP = 24 dm³/mol, Ar of X = 85)