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

Periodic trends reveal patterns in element properties based on atomic numbers, 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, as metals are primarily 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 and bonding.

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 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 will 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 at the periodic table, we see sulfur here, and we see tellurium here. Remember, the trend is as we head towards the top right corner, our metallic character will decrease. As we move down a group, our metallic character will increase. So since Tellurium is further down, it should have more metallic character; it's closer to the metals. As we go up the group, we're becoming less metallic, and therefore sulfur would have a lower metallic character. 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 the periodic trend for metallic character?

The periodic trend for metallic character indicates how easily an element can lose an electron. Metallic character decreases as you move from left to right across a period and increases as you move down a group. This trend occurs because metals, which are more likely to lose electrons, are located on the left and bottom of the periodic table. As you move towards the top right corner, elements become less metallic and more nonmetallic, meaning they are more likely to gain electrons rather than lose them.

How does metallic character change across a period?

Metallic character decreases as you move from left to right across a period. This is because elements on the left side of the periodic table are metals, which easily lose electrons. As you move to the right, elements become less metallic and more nonmetallic, meaning they are more likely to gain electrons. This trend is due to the increasing nuclear charge, which makes it harder for atoms to lose electrons as you move across a period.

Why does metallic character increase down a group?

Metallic character increases as you move down a group because the atomic size increases, making it easier for atoms to lose electrons. As you go down a group, additional electron shells are added, which increases the distance between the nucleus and the outermost electrons. This reduces the effective nuclear charge experienced by the outer electrons, making it easier for the atom to lose an electron and thus increasing its metallic character.

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, such as metals, lose electrons easily. This is because metals have lower ionization energies, meaning less energy is required to remove an electron. Conversely, nonmetals have low metallic character and tend to gain electrons instead of losing them. Therefore, the easier it is for an element to lose an electron, the greater its metallic character.

How do metals, metalloids, and nonmetals differ in terms of metallic character?

Metals, metalloids, and nonmetals differ significantly in their metallic character. Metals, found on the left side and bottom of the periodic table, have high metallic character and easily lose electrons. Metalloids, located between metals and nonmetals, have intermediate properties and can either lose or gain electrons depending on the conditions. Nonmetals, found on the right side and top of the periodic table, have low metallic character and tend to gain electrons. Understanding these differences is crucial for predicting the behavior of these elements in chemical reactions and bonding.