Alkali Metals - Group 1 Quiz

Study Notes

Alkali Metals - Group 1

Group 1 includes Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr).
They are univalent, forming ions by losing one electron: e.g., Na → Na⁺ + e⁻.
Strongly electropositive, they readily lose electrons to become positive ions.
Highly reactive, alkali metals are naturally found combined with other elements.
They tarnish quickly in air by reacting with oxygen and moisture, necessitating storage in inert liquids like paraffin oil.
Serve as powerful reducing agents, conducting heat and electricity effectively.
Characterized by malleability and ductility; they are soft with low melting points and densities.
React violently with cold water, releasing hydrogen gas.

Transition Metals

Transition metals are located between groups 2 and 3, spanning periods 4 to beyond.
First-row transition metals include Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), and Zinc (Zn), with atomic numbers 21 to 30.
They share comparable properties across the transition series, exhibiting high hardness and melting points.
Additional transition metals exist in subsequent periods.

Noble Gases and Sarps Series

Noble gases are chemically inert due to complete outer electron shells (2 or 8 electrons).
Argon provides an inert atmosphere for welding, while Helium is used for filling balloons and meteorological airships.

Characteristics of Transition Metals

Exhibit variable oxidation states.
Form colored hydrated salts or ions.
Commonly used as catalysts, with examples including Nickel, Iron, and Platinum.
Capable of forming complexes and displaying paramagnetic properties.

Other Elements

Hydrogen resides in both groups 1 and 7 due to its dual behavior: it loses one electron like alkali metals and gains one electron like halogens.
Period 1 of the periodic table includes only Hydrogen and Helium.

Metalloids

Positioned between metals and non-metals, metalloids exhibit a mix of properties characteristic of both.
Commonly referred to as semi-metals or semiconductors, they do not easily lose electrons.

Physical Properties of Metals

Metals are typically lustrous, malleable, ductile, and exhibit excellent conductivity for heat and electricity.
They are generally hard with high melting points.
Examples include Aluminum, Gold, Copper, and Silver.

Non-Metals

Non-metals possess four or more electrons in their outermost shells.
Except for noble gases, they achieve inert gas structure by gaining or sharing electrons.

Physical Properties of Non-Metals

Non-metals act as insulators, generally not conducting heat and electricity, though Graphite is an exception.
They tend to be brittle.
Examples include Phosphorus (P), Sulfur (S), Iodine (I), Oxygen (O), and Nitrogen (N).

Metallic Character

Metals can lose electrons from their outer shells, forming cations to attain stable inert gas configurations.
Metals with a tendency to lose electrons easily exhibit stronger metallic character, resulting in high reactivity.

Description

Test your knowledge on the alkali metals in Group 1, including their properties, reactivity, and individual elements. This quiz covers important concepts such as ion formation and electropositivity. Prepare to explore the fascinating world of these highly reactive metals.