Question

What is the term for the elements on the left side of the periodic table?

Short answer

The elements on the left side of the periodic table are metals, specifically alkali metals and alkaline earth metals.

Step-by-step solution

Understanding the Periodic Table Layout

The periodic table is organized into groups (vertical columns) and periods (horizontal rows). The elements on the left side are in groups 1 and 2 of the table.

Identify the Types of Elements in These Groups

Elements found in Groups 1 and 2 of the periodic table are primarily metals. Group 1 is known as the alkali metals, while Group 2 is known as the alkaline earth metals.

General Term for Left-Side Elements

Elements on the far left side of the periodic table, including those in the alkali metals and alkaline earth metals groups, are generally referred to as 'metals.'

Key concepts

Groups and Periods

To understand the organization of the periodic table, first, we need to learn about groups and periods, which are fundamental to its structure. The periodic table is akin to a map where each element has a specific location.

**Groups** are vertical columns. They're numbered from 1 to 18 and contain elements with similar chemical properties due to having the same number of valence electrons. This similarity in valence electrons means that elements in the same group often react in similar ways, making group number crucial for predicting element behavior.

• For instance, all elements in Group 1 have one valence electron, leading to highly reactive and similar interaction patterns.
• Meanwhile, Group 18 contains noble gases, which are generally unreactive due to having a full set of valence electrons.

**Periods** are horizontal rows. They indicate elements with the same number of atomic orbitals. As you move from left to right across a period, the atomic number increases by one, meaning each subsequent element has one more proton and, typically, one more electron than the preceding element. Each period on the table corresponds to the filling of a different quantum shell. This sequential ordering leads to predictable changes in elemental properties, like atomic size and ionization energy.

Understanding groups and periods is key to navigating the periodic table and predicting element behavior. They help scientists and students alike identify which elements might share similar properties and how they're likely to interact.

Alkali Metals

The alkali metals belong to Group 1 of the periodic table. These elements are lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). Characterized by their distinct properties, alkali metals are intriguing and highly reactive.

These metals have just one valence electron in their outermost shell. This single electron is easily lost, making alkali metals highly reactive, especially with water.

• They need to be stored under oil to prevent them from reacting with moisture from the air.
• This reactivity increases as you move down the group, with lithium being the least reactive and francium the most.

Due to their high reactivity, alkali metals are never found free in nature but are instead isolated in compounds. They share common characteristics such as being soft (they can often be cut with a knife) and having low densities compared to other metals. Sodium and lithium, for example, are less dense than water and will float on it.

In terms of usage, alkali metals have various applications in everyday life. Lithium is used in batteries, especially in rechargeable lithium-ion batteries, and sodium is a key component of table salt when combined with chlorine. Potassium has important roles in biological systems, such as nerve function in animals.

Understanding alkali metals helps you grasp why these elements are considered highly significant both industrially and biologically.

Alkaline Earth Metals

Moving over to Group 2 on the periodic table, we find the alkaline earth metals. This group consists of beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). These elements also play a crucial role in various chemical processes and have distinct properties.

Alkaline earth metals are known for having two valence electrons. This makes them less reactive than alkali metals; however, they can still lose their outer electrons to form ionic compounds readily.

• They typically react by donating two electrons to achieve a stable electron configuration.
• Calcium and magnesium are especially significant in biological processes.

In nature, alkaline earth metals are not found freely because of their reactivity. They occur in stable mineral compounds, often used in various industrial applications.

Some key characteristics include being harder and having higher melting points compared to the alkali metals. They are typically shiny and good conductors of electricity. Magnesium, for instance, is utilized in lightweight metal alloys, essential in manufacturing, while calcium is vital in building materials like cement and also plays a role in bone structure.

The importance of alkaline earth metals is easily seen in both geological and biological contexts. These elements help illustrate how subtle changes in electron configuration can significantly impact chemical behavior.