Periodic Trend: Metallic Character - Online Tutor, Practice Problems & Exam Prep

Understanding the metallic character of elements is essential in grasping periodic trends, which are patterns based on atomic numbers as we move across the periodic table. Metallic character refers to the ease with which an element can lose an electron, a trait more common in metals than nonmetals. As we traverse from left to right across a period and ascend a group towards the top right corner of the periodic table, the metallic character decreases. This aligns with the positioning of metals, which are predominantly found on the left and lower sections of the table. Therefore, proximity to metals indicates higher metallic character, while distance suggests a reduction in this property.

Periodic Trend: Metallic Character

Now before we can talk about metallic characteristics of the elements in the periodic table, it's first important to talk about the periodic trends themselves. Now, the periodic trends are specific patterns in the property of elements based on their changing atomic numbers.

We're going to say as we examine these periodic trends, we will examine these patterns while moving to the top right corner of the periodic table. So we're generally going to be moving this way to the top right corner of the periodic table when discussing the different types of periodic trends that exist.

O keep that in mind as we investigate each and everyone.

Periodic Trend: Metallic Character

Now, metallic character has to do with how easily an element can lose an electron. The easier it is for an element to lose an electron, the greater its metallic character. Now remember, metals tend to lose electrons, Nonmetals tend to gain electrons.

When it comes to the major table, major periodic table classifications, we have our metals, our metalloids and our nonmetals. And we're going to say the periodic trend here is metallic character is going to decrease as we move from left to right across a period. So as we're going this way and as we go up a group, this makes sense because where are the metals on the periodic table? They're all clustered more to the left and the bottom.

As we're heading towards the top right corner, we're moving away from the metals. So our metallic character is supposed to decrease. So just remember this is one of the simplest periodic trends to understand metallic character. The closer you are to the metals, the more metallic character you have. The further away you are from the metals, the less metallic character you're going to have.

Periodic Trend: Metallic Character Example 1

So here it says based on the periodic trend, which element would have the greater metallic character. So here let's compare sulphur versus tellerium. So looking on the periodic table, we see sulfur here, we see tellerium here.

Remember the trend is as we head towards the top right corner, our metallic character will decrease, and as we move up a Group A metallic character, we'll also decrease. So since Tellurium is further down, it should have more metallic character. It's closer to the metals.

As we're going up the group, we're becoming less metallic and therefore sulfur would have a lower metallic character. So just remember, the closer we the closer we get to the metals, the greater a metallic character will be. The further away we get from the metals, the lower our metallic character will be.

Here’s what students ask on this topic:

What is a periodic trend?

A periodic trend refers to the predictable patterns observed in the properties of elements across different periods (rows) and groups (columns) in the periodic table. These trends arise due to the regular variations in the atomic structure of elements as one moves through the table. For instance, atomic radius decreases from left to right across a period due to the increasing positive charge in the nucleus, which pulls electrons closer. Conversely, atomic radius generally increases as you move down a group because each successive element has an additional electron shell.

Other notable periodic trends include ionization energy (the energy required to remove an electron), which typically increases across a period and decreases down a group, and electronegativity (the tendency of an atom to attract electrons), which often shows a similar pattern to ionization energy. Understanding these trends is crucial for predicting the chemical behavior of elements and their compounds, making them fundamental concepts in chemistry.

What is metallic character?

Metallic character refers to the set of chemical properties associated with elements that are metals. These properties are typically exhibited by elements that readily lose electrons to form positive ions (cations). Elements with a high metallic character are found on the left and towards the bottom of the periodic table, as these positions indicate a greater tendency to donate electrons during chemical reactions.

The key properties of metals that define their metallic character include high electrical and thermal conductivity, luster (they are shiny when polished), malleability (they can be hammered into thin sheets), ductility (they can be drawn into wires), and often a high density. Metals also tend to have lower electronegativity values, meaning they have a weaker attraction for electrons compared to nonmetals. The metallic character of an element increases as you move from right to left across a period and from top to bottom down a group in the periodic table. This is because the atomic size generally increases in these directions, making it easier for the outermost electrons to be lost and metallic bonds to be formed.

Which group has the greatest metallic character?

The metallic character of an element refers to its ability to lose electrons and form positive ions (cations). In the periodic table, metallic character increases as you move from right to left across a period and from top to bottom down a group. This is because atoms become larger and have more electron shells as you go down a group, making it easier for them to lose the outermost electrons, and they have fewer protons across a period, making the effective nuclear charge (the pull on the electrons) weaker.

Considering these trends, the group with the greatest metallic character is the alkali metals group, which is Group 1 of the periodic table. This group includes elements like lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). Among these, francium is theoretically the most metallic; however, it is extremely rare and radioactive, so cesium is often considered the most metallic of the stable elements.

How does metallic character change across a period?

Metallic character refers to the level at which an element exhibits the physical and chemical properties of metals, such as malleability, ductility, and conductivity. As you move across a period in the periodic table from left to right, the metallic character of elements decreases. This happens because elements across a period have an increasing number of protons in their nuclei, leading to a stronger attraction between the positively charged nucleus and the negatively charged electrons. This stronger pull makes it harder for atoms to lose electrons and form positive ions, which is a characteristic property of metals.

As a result, elements on the left side of a period are typically metals, and they gradually change to metalloids and then to nonmetals as you move to the right. For example, in the third period, sodium (Na) on the left is a highly reactive metal, while chlorine (Cl) on the right is a nonmetal. This transition reflects a shift from elements that easily give up electrons to form cations to those that tend to gain electrons to form anions.