Podcast
Questions and Answers
What is the group number of alkali metals in the periodic table?
What is the group number of alkali metals in the periodic table?
Group IA
How many valence electrons do alkali metals have?
How many valence electrons do alkali metals have?
One
Why do alkali metals have low ionization energies?
Why do alkali metals have low ionization energies?
Weak attraction between the nucleus and the valence electron
What is the appearance of alkali metals?
What is the appearance of alkali metals?
Signup and view all the answers
Why are alkali metals known as electropositive metals?
Why are alkali metals known as electropositive metals?
Signup and view all the answers
What type of ions do alkali metals readily form?
What type of ions do alkali metals readily form?
Signup and view all the answers
Which alkali metals are liquid at room temperature?
Which alkali metals are liquid at room temperature?
Signup and view all the answers
Why are alkali metals good conductors of heat and electricity?
Why are alkali metals good conductors of heat and electricity?
Signup and view all the answers
What determines the reactive nature of alkali metals?
What determines the reactive nature of alkali metals?
Signup and view all the answers
With which elements do alkali metals easily combine?
With which elements do alkali metals easily combine?
Signup and view all the answers
Study Notes
S Block Elements: Alkali Metals
The alkali metals, also known as Group IA elements or group 1 elements, are located in the first column of the periodic table's s-block. They consist of lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). These elements have one valence electron and tend to lose one electron to achieve a stable, inert gas configuration. Some characteristics of alkali metals are:
- Low ionization energy: They have low ionization energies due to the weak attraction between the nucleus and the valence electron.
- Electropositive: They are highly electropositive and readily form positive ions (cations), which is why they are also known as electropositive metals.
- Silvery-white appearance: They are typically found as silvery-white metals due to their high reflectivity.
- Reactive: They are highly reactive, a property determined by their ionization energy and the ease with which they form positive ions.
- Active nature: They are highly active and easily combine with the halogens, sulfur, nitrogen, phosphorus, and oxygen.
- Good conductors of heat and electricity: They have excellent thermal conductivity and electrical conductivity due to their metallic nature.
- Liquid at room temperature: Only potassium and caesium are liquid at standard temperature and pressure (25°C/0°C), while the others are solid.
Alkali metals form compounds with most other elements and are commonly found as metal oxides, hydroxides, carbonates, and fluorides. The alkali metals have diverse applications, including the production of sodium hydroxide used in soaps and detergents, potassium chlorate in explosives, and lithium batteries for portable electronics.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Description
Explore the characteristics and properties of alkali metals located in the first column of the periodic table's s-block. Learn about their low ionization energy, electropositive nature, silvery-white appearance, reactivity, and applications in various industries.
