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

Periodic trends reveal patterns in element properties based on atomic number, particularly metallic character, which indicates how easily an element can lose an electron. Metallic character decreases from left to right across a period and increases down a group, with metals located on the left and bottom of the periodic table. Understanding these trends is crucial for grasping the behavior of metals, metalloids, and nonmetals in chemical reactions, particularly in oxidation-reduction processes where electron transfer is key.

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. So keep that in mind as we investigate each and every one.

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 periodic table classifications, we have our metals, our metalloids, and our nonmetals. And we're going to say the periodic trend here is that 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. 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 sulfur versus tellurium. Looking on the periodic table, we see sulfur here, we see tellurium 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, our metallic character will 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 get to the metals, the greater our metallic character will be. The further we get from the metals, the lower our metallic character will be.

Between which two elements is the difference in metallic character the greatest?

• A. Rb and O
• B. O and I
• C. Rb and I
• D. Li and O
• E. Li and Rb

Here’s what students ask on this topic:

What is metallic character in the periodic table?

Metallic character refers to how easily an element can lose an electron. Elements with high metallic character tend to lose electrons easily, making them good conductors of electricity and heat. Metals, which are located on the left and bottom of the periodic table, exhibit high metallic character. This property decreases as you move from left to right across a period and increases as you move down a group. Understanding metallic character is crucial for predicting the behavior of elements in chemical reactions, especially in oxidation-reduction processes where electron transfer is key.

How does metallic character change across a period?

Metallic character decreases as you move from left to right across a period in the periodic table. This is because elements on the left side of a period have fewer valence electrons and can lose them more easily, exhibiting higher metallic character. As you move to the right, elements have more valence electrons and hold onto them more tightly, making it harder to lose electrons and thus decreasing their metallic character. This trend is due to increasing nuclear charge, which attracts electrons more strongly.

Why does metallic character increase down a group?

Metallic character increases as you move down a group in the periodic table. This is because elements lower in a group have more electron shells, which means the outermost electrons are farther from the nucleus and are less tightly held. This makes it easier for these elements to lose electrons, thereby increasing their metallic character. Additionally, the increased shielding effect from inner electron shells reduces the effective nuclear charge felt by the outermost electrons, further facilitating electron loss.

What is the relationship between metallic character and electron loss?

Metallic character is directly related to how easily an element can lose an electron. Elements with high metallic character lose electrons easily, which is a characteristic feature of metals. This ease of electron loss is due to the lower ionization energy of metals, which allows them to participate readily in oxidation-reduction reactions. Conversely, nonmetals, which have low metallic character, tend to gain electrons rather than lose them. Understanding this relationship helps in predicting the reactivity and chemical behavior of elements.

Where are metals located on the periodic table?

Metals are primarily located on the left side and towards the bottom of the periodic table. This includes groups 1 (alkali metals), 2 (alkaline earth metals), and the transition metals in the center. These elements exhibit high metallic character, meaning they lose electrons easily and are good conductors of heat and electricity. As you move from left to right across a period or up a group, the metallic character decreases, and you encounter metalloids and nonmetals, which do not lose electrons as easily.