Group 1 Alkali Metals Quiz

Group 1 elements in the periodic table, including Lithium, Sodium, Potassium, Rubidium, Caesium, and Francium.

Alkali metals are very reactive because they readily lose one electron to become stable.

Alkali metals are soft, low-density, low-melting metals.

The reaction of an alkali metal with water produces metal hydroxide and hydrogen gas.

Alkali metals all have one electron in their outermost shell, causing similar properties.

As you move down Group 1, the reactivity of alkali metals increases.

Alkali metals are soft, have low melting points, and are less dense than water.

The melting point of Group 1 elements decreases as you move down the group.

Elements lower in Group 1 are more reactive than elements higher in the group.

Rubidium, being below potassium in Group 1, would react even more vigorously with air and water.

Based on its position, rubidium would be a soft, shiny, grey solid, denser than potassium, and have a lower melting point than potassium.

A trend is a recurring pattern of behavior in chemical properties as you move down a group or across a period in the periodic table.

Alkali metals have only one electron in their outermost shell, which they readily lose to achieve a stable electron configuration, making them highly reactive.

A positively charged ion (1+) is formed, and the next inner shell becomes the outermost, achieving a stable noble gas configuration.

The distance between the outermost electron and the nucleus increases down Group 1, making the electron easier to remove.

The reactivity of alkali metals is directly related to their electronic configuration, specifically the ease with which they lose their outermost electron.

When an alkali metal reacts with water, it produces a metal hydroxide and hydrogen gas, which is flammable. The reaction becomes more vigorous as you move down the group.

The general formula for hydroxides formed by alkali metals is MOH, where 'M' represents the alkali metal.

Alkali metals react with oxygen in the air, forming metal oxides which cover the surface of the metal with a dull coating. This is called tarnishing. The rate of tarnishing increases as you move down the group.

As you move down the group, the alkali metals become more reactive due to increasing atomic size and decreasing ionization energy. This makes it easier for the metal to lose its outer electron, leading to a more vigorous reaction with water.

The reactivity of alkali metals with oxygen increases as you go down the group. This means they react more easily and form metal oxides more quickly.

The reactivity of alkali metals with water increases as you go down the group. This means that the reaction becomes more vigorous and produces more heat.

Lithium forms lithium oxide (Li2O), while potassium forms potassium peroxide (K2O2). The other alkali metals form peroxides or superoxides when reacting with oxygen.

Alkali metals react with water to produce metal hydroxides. These hydroxides are strong bases, which means they release hydroxide ions (OH-) in solution, making the solution alkaline.

Common observations include: a fizzing sound due to the release of hydrogen gas; the alkali metal moving on the surface of the water due to the heat generated in the reaction; a visible flame from the burning hydrogen gas, especially for the heavier alkali metals.