Group 2 Elements Quiz

Ionization energy decreases down group 2 due to added electron shells, increased shielding, and greater distance between outer electrons and the nucleus.

Atomic radius increases down group 2 because extra electron shells are added.

+2

<p>Hydroxides. General equation: M(s) + 2H₂O(l) → M(OH)₂(aq) + H₂(g). Ions: M²⁺ and OH⁻.</p> Signup and view all the answers

<p>Oxides. General equation: 2M(s) + O₂ → 2MO(s). Ions: M²⁺ and O²⁻.</p> Signup and view all the answers

<p>Chlorides. General equation: M(s) + Cl₂(g) → MCl₂(s). Ions: M²⁺ and Cl⁻.</p> Signup and view all the answers

<p>Magnesium oxide and hydrogen gas. Equation: Mg(s) + H₂O(g) → MgO(s) + H₂(g).</p> Signup and view all the answers

<p>Reactivity increases down the group because ionization energy decreases, making it easier for them to react.</p> Signup and view all the answers

<p>Beryllium oxide</p> Signup and view all the answers

<p>Hydroxides. General equation: MO(s) + H₂O(l) → M(OH)₂(aq)</p> Signup and view all the answers

<p>Metal chloride and hydrogen gas (MCl₂, and H₂). General equation: M + 2HCl → MCl₂ + H₂</p> Signup and view all the answers

<p>Metal sulfate and hydrogen gas (MSO₄, H₂). General equation: M + H₂SO₄ → MSO₄ + H₂</p> Signup and view all the answers

<p>Metal chloride and water (MCl₂, and H₂O). General equation: MO + 2HCl → MCl₂ + H₂O</p> Signup and view all the answers

<p>Metal sulfate and water (MSO₄, H₂O). General equation: MO + H₂SO₄ → MSO₄ + H₂O</p> Signup and view all the answers

<p>Neutralization reaction, producing salt and water.</p> Signup and view all the answers

<p>Metal chloride and water (MCl₂) and H₂O. General equation: M(OH)₂ + 2HCl → MCl₂ + 2H₂O</p> Signup and view all the answers

<p>Metal sulfate salt and water (MSO₄) and H₂O. General equation: M(OH)₂ + H₂SO₄ → MSO₄ + 2H₂O</p> Signup and view all the answers

<p>Solubility increases.</p> Signup and view all the answers

<p>As an antacid for indigestion, to neutralize HCl in the stomach.</p> Signup and view all the answers

<p>Decreases.</p> Signup and view all the answers

<p>Barium sulfate</p> Signup and view all the answers

<p>Barium meals (medical tracer for internal imaging). It doesn't enter the bloodstream because it's insoluble so its toxicity is not a danger to the patient</p> Signup and view all the answers

<p>Acidified barium chloride (BaCl₂). Reacts to form barium sulfate as a white precipitate when sulfate ions are present. Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)</p> Signup and view all the answers

<p>A measure of the extent to which a compound decomposes. A compound that doesn't decompose at all is VERY thermally stable.</p> Signup and view all the answers

<p>As the ionic radius of the cation gets larger, they cause less distortion of the anion, due to the lower charge density, thus making the carbonate/nitrate compound more stable.</p> Signup and view all the answers

<p>They have a higher charge (so greater charge density) thus they cause greater distortion to the anion, meaning the less stable the carbonate/nitrate compound becomes.</p> Signup and view all the answers

<p>They are thermally stable and do not decompose. Exception: Lithium carbonate (Li₂CO₃) decomposes to form Lithium oxide and carbon dioxide (Li₂O + CO₂).</p> Signup and view all the answers

<p>Metal nitrite and oxygen (MNO₂ + O₂), If brown fumes are observed (lithium nitrate) metal oxide, nitrogen dioxide and oxygen (MO + NO₂ + O₂).</p> Signup and view all the answers

<p>Greater decomposition.</p> Signup and view all the answers

<p>Decomposition occurs when the cation has a 2+ charge (group 2 elements), or the cation has a 1+ charge and is also the smallest group 1 cation (lithium). This is because there is an increased charge density meaning the negative ion can be polarised, the less heat is required to separate the 2 ions meaning the the larger cations form more stable carbonates and nitrates.</p> Signup and view all the answers

<p>Measure the time it takes for a certain amount of oxygen or brown NO₂ gas to be produced.</p> Signup and view all the answers

<p>Measure the time it takes for carbon dioxide to be produced. Carbon dioxide, when bubbled through limewater, turns it cloudy.</p> Signup and view all the answers

<p>Red</p> Signup and view all the answers

<p>Lilac</p> Signup and view all the answers

<p>Red/purple</p> Signup and view all the answers

<p>no colour</p> Signup and view all the answers

<p>no colour</p> Signup and view all the answers

<p>Crimson red</p> Signup and view all the answers

<ol> <li>Mix a small amount of the compound being tested with hydrochloric acid. 2. Heat a platinum or nichrome wire in the blue part of the Bunsen flame. 3. Dip the wire into the solution and hold it in the blue part of the flame. 4. Note color produced.</li> </ol> Signup and view all the answers

<p>The energy absorbed from the flame causes the electrons to move to higher energy levels. When the electrons fall back down to lower energy levels, releasing energy in the form of light. The difference between the higher and lower energy levels determines the wavelength of the light which determines the colour of the light.</p> Signup and view all the answers

<ul> <li>many compounds contain small amounts of sodium compounds as impurities, so the sodium colour can mask other colours.</li> <li>describing colours is subjective</li> </ul> Signup and view all the answers

<p>Add sodium hydroxide solution, warm mixture, ammonia gas is released which turns damp red litmus paper blue. Equation: NH₄⁺ + OH⁻ → NH₃ + H₂O</p> Signup and view all the answers

Ionisation energy decreases down group 2 due to added electron shells and shielding.

The atomic radius increases down group 2 due to the addition of extra electron shells.

Group 2 elements form +2 ions when they react.

Group 2 elements react with water to form hydroxides: M(OH)₂.

Group 2 elements burn in oxygen to form oxides: MO.

Group 2 elements react with chlorine to form chlorides: MCl₂.

Magnesium reacts with steam to form magnesium oxide (MgO) and hydrogen.

Reactivity increases down group 2 as ionisation energy decreases.

Beryllium oxide is the insoluble oxide in Group 2.

Group 2 oxides react with water to form hydroxides: M(OH)₂.

Group 2 metals react with dilute HCl to form MCl₂ and H₂.

Group 2 metals react with dilute sulfuric acid to form MSO₄ and H₂.

Group 2 metals react with dilute nitric acid to form M(NO₃)₂ and H₂.

Hydroxides react with dilute HCl to form MCl₂ and H₂O.

Solubility of hydroxides increases down group 2.

Barium sulfate is insoluble, used in medical imaging.

Add acidified barium chloride; a white ppt indicates sulfate ions.

Thermal stability measures a compound's decomposition extent.

Thermal stability increases down group 2 due to larger ionic radius.

Lithium produces a red flame when tested in a flame test.

Sodium gives an orange-yellow flame in a flame test.

Chlorine appears virtually colorless in water.

The reaction is a neutralization producing salt and water.

Reducing power increases down group 7 as ionic size increases.

More reactive halogens displace less reactive ones from compounds.