Group 2 Elements: Trends and Properties

The atomic radius increases down the group because the atoms have more shells of electrons, making the atom bigger.

The metallic bonding weakens as the atomic size increases, resulting in a decrease in melting points.

The outermost electrons become more shielded from the attraction of the nucleus due to the repulsive force of inner shell electrons.

<p>The reactivity of group 2 metals increases down the group due to the decrease in ionization energy.</p> Signup and view all the answers

<p>It is necessary to remove the magnesium oxide layer because it would react with acid at a different rate than the magnesium, giving a false result.</p> Signup and view all the answers

<p>2 Mg + O2 → 2 MgO</p> Signup and view all the answers

<p>MgO appears as a white powder, and its high melting point is due to ionic bonding.</p> Signup and view all the answers

<p>Mg(s) + H2O(g) → MgO(s) + H2(g), and the products are magnesium oxide and hydrogen.</p> Signup and view all the answers

<p>The reactivity of group 2 metals with cold water increases down the group, and the hydroxides produced make the water alkaline.</p> Signup and view all the answers

<p>The reaction with steam produces MgO and hydrogen, with a bright white flame, whereas the reaction with warm water produces Mg(OH)2 and hydrogen, with no flame.</p> Signup and view all the answers

<p>Titanium is abundant, has a low density, and is corrosion resistant.</p> Signup and view all the answers

<p>The reason is not specified in the text, but it is likely due to the high reactivity of titanium and the difficulty of reducing its oxide with carbon.</p> Signup and view all the answers