Periodic Table and Reactivity Series Practice

A complete set of vocabulary and concept flashcards based on lecture notes covering the Periodic Table structure, Group properties, Transition metals, and the Reactivity Series.

Periodic Table

An arrangement of elements in periods and groups and in order of increasing proton number/atomic number.

Periods

The horizontal rows in the periodic table; going along a period, elements change from metallic to non-metallic character.

Groups

The vertical columns in the periodic table; elements in the same group share similar chemical properties due to their electronic configuration.

Valence electrons

Electrons located in the most outer most shell of an atom.

Valency

The number of electrons an atom tends to lose, gain, or share to be stable like one of the noble gases.

Group I Alkali Metals

A group of soft, silvery grey, reactive metals including lithium, sodium, and potassium that are stored under oil to prevent reaction with oxygen and water.

Group I Trends

Down the group, melting points decrease, while density and reactivity increase.

Group VII Halogens

A group of diatomic non-metals including chlorine, bromine, and iodine; reactivity decreases down the group while density increases.

Chlorine ($Cl_2$)

A Group VII halogen that appears as a pale yellow-green gas at r.t.p.

Bromine ($Br_2$)

A Group VII halogen that appears as a red-brown liquid at r.t.p.

Iodine ($I_2$)

A Group VII halogen that appears as a grey-black solid at r.t.p.

Transition Elements

Metals in the middle block of the periodic table characterized by high densities, high melting points, the formation of colored compounds, and variable oxidation numbers (e.g., iron(II) and iron(III)).

Catalyst

A chemical substance that speeds up the rate of a chemical reaction without being consumed, often transition elements or their compounds.

Group VIII Noble Gases

Unreactive, monatomic gases with full outer shells of electrons, such as helium, neon, and argon.

Molar Gas Volume

The volume of one mole of any gas is $24\,dm^3$ at room temperature and pressure (r.t.p.).

Physical Change

A change where matter changes form but not its chemical identity, such as melting ice or shredding paper.

Chemical Change

A change where a chemical reaction occurs and new products are formed, such as burning wood or rotting bananas.

Amphoteric Oxide

An oxide that can behave as both acidic and basic; aluminum oxide ($Al_2O_3$) is a specific example from Period 3.

Displacement Reaction

A reaction where a more reactive halogen or metal displaces a less reactive one from its salt or compound.

Test for Chlorine gas ($Cl_2$)

Using damp blue litmus paper, which turns red and then becomes colorless (bleached).

Halide Test

Using silver nitrate in the presence of nitric acid; $Cl^-$ gives white precipitate, $Br^-$ gives creamy precipitate, and $I^-$ gives yellow precipitate.

Reactivity Series

A list of elements arranged according to reactivity: potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold, platinum.

Aluminium unreactivity

The apparent lack of reactivity in aluminium due to a protective oxide layer ($Al_2O_3$) that must be removed before the metal can react with acids.

Oxidation

The process of gaining oxygen or losing hydrogen during a chemical reaction.

Reduction

The process of losing oxygen or gaining hydrogen during a chemical reaction.

Thermite Reaction

A highly energetic reaction used in welding: $2Al (s) + Fe_2O_3 (s) \rightarrow Al_2O_3 (s) + 2Fe(s)$, where aluminium reduces iron(III) oxide.

Thermal Decomposition

The process of splitting a substance into simpler substances using heat, such as metal carbonates splitting into metal oxides and carbon dioxide.