Properties of Metals, Nonmetals, and Metalloids

Elements are generally grouped into three broad classifications: metals, nonmetals, and metalloids (or semimetals, as those elements are commonly called). Each class has different characteristics.

Metals are typically good thermal and electrical conductors. In addition, metals are malleable (they can be hammered or rolled into thin sheets) and ductile (they can be stretched into wires without breaking).

If you think of a piece of metal, it is most likely a solid piece of material that, when polished, will appear silvery. The main exception is mercury, which is a liquid at room temperature, unlike most metal.

Nonmetals, however, exhibit low thermal and electrical conductivity and do not exhibit mechanical properties of metals like bending or stretching. They also can be in three distinctly different physical states at room temperature: gas, liquid, or solid.

The third class of elements are the metalloids, which exhibit properties similar to metals and nonmetals. Generally, they appear more similar to nonmetals, but they may also be able to conduct electricity under certain conditions.

Because of this conductivity, metalloids (or semiconductors, as they are often referred to in this context) are extremely important in modern technology (especially in computer hardware and other electronics).

If you refer to a periodic table, you may notice a zigzag (stair-step) line dividing the metals from the nonmetals along the right side. Metals lie to the left of this dividing line (with the exception of hydrogen, which is a nonmetal), nonmetals lie to the right, and the elements that are in close proximity to the zigzag line are the metalloids.

When elements react with one another to form compounds, they undergo either one of two principal types of chemical bonds. The first is an ionic bond, which arises when one or more electrons are transferred from one atom to another.

This transfer creates ions with one positive and one negative charge that are pulled to one another due to their opposite charges. The second is called a covalent bond. In the case of a covalent bond, the atoms share electrons, leading to the formation of neutral molecules.

Generally speaking, when a metal reacts with a nonmetal, they form ionic compounds. Whereas, when two nonmetals react with one another, they form covalent compounds (molecules).

Metals in the periodic table

If you had access to the periodic table, you would see that most elements are metals, which are not spread out randomly but group together from the center of the table to the left side.

When we say metals, we mean any of the five groups: alkaline metals, alkaline earth metals, transition metals, and even lanthanides and actinides, which may get a special row all their own.

We are grouping properties from each group, but there are some properties that are common to most metals that are different from nonmetals and metalloids.

More Resources: What is Metal and Their Types?

Alkali Metals

Alkali metals are found in the first column farthest left of the Periodic Table. Alkali metals are memorable as they are relatively soft and exceptionally reactive metals. The reason they are so reactive is because each alkali metal has a single electron in its outermost s sub-shell.

The alkali metals are a very small group of six elements: lithium, sodium, potassium, rubidium (usually derived from the mineral lepidolite), cesium, and francium. These alkali metals have sufficiently consistent chemical behaviors to allow us to easily identify them as a group.

Alkaline Earth Metals

Referred to as the alkaline earth metals, the Group 2 elements on the periodic table are located just to the left of the alkali metals and are the hardest and heaviest looking of the alkali metals.

The alkaline earth metals are not distinguished by having two s electrons on their outer s sub-shell alone, as many of their chemical properties relate back to this feature.

While quite interestingly each of these metals produces a unique flame color, when heated, which is a useful way of identifying the metal in the laboratory.

The alkaline earth metals include six elements: beryllium, magnesium, calcium, strontium, barium, and radium.

Transition Metals

The transition metals are located in a central region of the Periodic Table of Elements (shown below) and are often included in the environmentally and toxicologically regulated group of “heavy metals” because they have a greater density compared to the less dense alkali or alkaline earth metals.

There are 38 examples of elements classified as transition metals, including some examples, but not limited to, cobalt, copper (including native copper like that found in Arizona), gold, iron, silver, platinum, mercury, titanium, tungsten, and zinc.

Rare Earth Metals

Rare earth metals are usually given their own special place below the main Periodic Table – almost like a footnote. In fact, they should be located at the center of the Periodic Table. Rare earth metals can be separated into two groups: lanthanides and actinides.

Lanthanide Metals

On the Periodic Table there are a total of fifteen lanthanides and determining differences between lanthanides can sometimes feel impossibly difficult.

Lanthanides are classified together because of their remarkable similarities in both chemical and physical properties that make differences between them hard to understand.

For example, cerium, promethium, gadolinium, dysprosium and lutetium are all examples of elements that belong to this classification; but rather than being ten separate and unique elements, they are considered to belong to a set that is all unique but still closely related subset of the lanthanide series.

Actinide Metals

There are presently 15 actinides recognized in the Periodic Table. Most of these elements do not occur in nature from the perspective of their instability. Thus, for the most part these elements can be produced by scientist in a contained manner, such as in reactors or via particle accelerators.

Some examples of actinides are thorium, uranium, plutonium, californium and mendelevium.

Other Metals

The category referred to as “other metals” is located in the right-hand portion of the main body of the Periodic Table. This group of metals may also be referred to as semimetals or post-transition metals – at times, terminology can be inconsistent.

They differ from other metals as they are softer and have lower melting points than most other metals.

None of this is to say that there is a uniform understanding among either chemists in the field or laypeople. Depending on your rendition of the Periodic Table, there are between 8 and 14 other metals.

Some familiar examples are aluminum, bismuth, indium, lead, and tin. Specifically bismuth crystals are noted, largely based on unique appearances and traits.

Properties of Metals

Metals are a particular class of elements that are distinguished by their ability to lose electrons, and to form positive ions with the exception of hydrogen, and so they are considered to be electropositive and this characteristic is related to their relatively low ionization energies.

When you think of metals, you probably envision something shiny, heavy, and difficult to melt, which is true for most metals.

Metals are also generally lustrous, can be drawn into wires (ductility) or hammered into sheets (malleability), and are also characterized by their high conductivity of electricity and heat.

With the one exception of mercury, which is in the liquid phase at room temperature, every metal that you will find in your environment is a solid at room temperature.

In chemical bonding, metals typically bond with nonmetals to form ionic bonds with the exception of a few anecdotes. Most metals make at least one basic oxide, while some are amphoteric and have more chemical flexibility.

The reactivity of metals spans quite a range—many metals react quickly, while others do not react at all. There are some metals that are categorized by their unique properties: the noble metals—ruthenium, rhodium, palladium, platinum, gold, osmium, iridium, and silver are resistant to corrosion and oxidation.

There are the refractory metals—niobium, molybdenum, tantalum, tungsten, and rhenium are refractory because they have extremely high melting points and will not melt.

Physical Properties of Metals:

When you look at metals and what makes them stand out, a few key physical properties are worth knowing about:

• Malleability: Most metals are malleable, meaning that they can be hammered into thin sheets without cracking. A good specific example is gold, which is, in fact, the most malleable metal available. Gold can be stretched and shaped without cracking or breaking.
• Ductility: Metals are also ductile, allowing them to be drawn out into wires. If you think about how flat, fine wires are made out of silver, it is notable because silver is one of the most ductile metals.
• Conductivity: What metals are great at is conducting, so they conduct electricity and heat. Found in pans or powerlines, metals are used all the time!
• Luster: Metals often have a natural shine or “luster” that are aesthetically pleasing. Patina can form as metals oxidize, removing their original shine.
• Tensile Strength: I bet you are thinking why we use metals to build bridges or skyscrapers; the answer is their tensile strength! Zinc metals give us great strength to weight ratios—they can withstand their weight!
• Sonorous Quality: Have you ever noticed that a metal or metal object rings when struck? This is because metals are sonorous and produce a sharp distinct sound.
• Hardness: Metals aren’t easy to cut. Their hardness allows them to be durable. Hence, their uses in tools, construction, etc.
• Forming Cations: Chemically, metals tend to oxidize and lose electrons in aqueous solutions to form cations. You can see this play out with reactions and electrochemistry.
• Melting Points and Boiling Point: While many metals have a high melting point and boiling point, a few elements have low melting points: cesium, gallium, mercury, rubidium, and tin. These metals are more of the exception than the norm! When it comes to boiling points, most metals can withstand relatively high temperatures before changing phase to vapor.
• Density: Most metals are heavier, or denser, than nonmetals. For example, when you handle metals such as tungsten and platinum, they are heavy! The densities of of metals such as osmium and platinum, and gold and iridium also would shock you!
• Color: Most metals are just silvery, grey metals; but some metals stand out! Gold is yellow; copper is reddish; cesium is an example with a golden tint!

Chemical Properties of Metals

Metals are electropositive elements that generally form basic or amphoteric oxides with oxygen. Other chemical properties include:

• Electropositive Character: Metals tend to have low ionization energies, and typically lose electrons (i.e. are oxidized) when they undergo chemical reactions They normally do not accept electrons. For example:
  • Alkali metals are always 1+ (lose the electron in s subshell)
  • Alkaline earth metals are always 2+ (lose both electrons in s subshell)
  • Transition metal ions do not follow an obvious pattern, 2+ is common (lose both electrons in s subshell), and 1+ and 3+ are also observed

Na0→Na⁺+e⁻

Mg0→Mg₂++2e⁻

Al0→Al₃⁺+3e⁻

Compounds of metals with non-metals tend to be ionic in nature. Most metal oxides are basic oxides and dissolve in water to form metal hydroxides:

Na₂O(s)+H₂O(l)→2NaOH(aq)

CaO(s)+H₂O(l)→Ca(OH)₂(aq)

Metal oxides exhibit their basic chemical nature by reacting with acids to form metal salts and water:

MgO(s)+HCl(aq)→MgCl₂(aq)+H₂O(l)

NiO(s)+H₂SO₄(aq)→NiSO₄(aq)+H₂O(l)

Location of Metals on the Periodic Table

If you were to take a moment to review the periodic table, you’d notice that metals are the most commonly occurring elements. In fact, more than three-quarters of all the elements on the table are metals, so it’s no wonder they fill the majority of the table.

In general, you’ll find metals on the left side of the periodic table; however, don’t forget about those two additional rows under the table (called lanthanides and actinides). Those are commonly referred to as metals as well.

Notice there is a sort of stair-step line that begins at boron (B, atomic number 5) and winds its way down to polonium (Po, atomic number 84). This line is useful little boundary: besides germanium or antimony (two exceptions), any element to the left is a metal.

So when you’re looking for metals on the table, the stair-step line is a quick way to identify them.

Uses of Metals

Metals find use in every aspect of life. Here is a list of some of their uses:

• Structural components
• Containers
• Wires and electrical appliances
• Heat sinks
• Mirrors
• Coins
• Jewelry
• Weapons
• Nutrition (iron, copper, cobalt, nickel, zinc, molybdenum)

Nonmetals In Periodic Table

If you take a look at the periodic table, you will see that the nonmetals are typically grouped together in the upper right-hand corner of the table. This group includes not only the traditional nonmetals, but also the halogens and noble gases.

What distinguishes the nonmetals in the periodic table is that they share some common chemical characteristics with one another that differentiate them, as a group, chemically from metals.

Therefore, any nonmetal, whether it is oxygen, chlorine, or even helium, has much more in common with the other nonmetals in the group than they do with metals other places on the periodic table.

Groups of Nonmetals

The periodic table has a well-defined subgroup of nonmetals known as the nonmetal elements. It contains hydrogen, carbon, nitrogen, oxygen, phosphorus, sulfur, and selenium, most of which are familiar to us.

While it may seem out-of-place at times, hydrogen is widely classified as a nonmetal since it generally acts and can be described as a nonmetal at standard temperature and pressure, so it is included as a nonmetal element.

A further subgroup of nonmetals is a group of seven nonmetals collectively called the halogens; they are located in group 7 of the periodic table. In halogen normally each atom has an oxidation state of -1.

There is a thin-yet-clear pattern of the physical state when going down the group of halogens. For example, the two elements that are at the top, fluorine and chlorine are gases, next is bromine, which is a liquid, and iodine and astatine are solids.

There is also another halogen member, called tennessine, whose behavior is still a bit of a mystery, and is not as clear in relation to this group compared to a group of metalloids.

Finally, the noble gases group is the last column of the periodic table (group 8). The noble gas elements, helium, neon, argon, krypton, xenon, radon, oganesson, are all known for being very unreactive, and the large majority are gases at room temperature. Oganesson is likely the exception to this, as it is likely not a gas at standard temperature and pressure.

More Resources: What are the Nonmetals?

Properties of Nonmetals

Non-metals are elements that tend to gain electrons in a chemical reaction, resulting in the formation of typically anions.

Non-metals are quite different from metals when compared to their ability to attract electrons. In terms of electronegativity and ionization energy, non-metals are generally quite strong at making it difficult to remove their electrons by having very high ionization energies.

In regard to their physical properties, non-metals are non-lustrous, brittle, tend to have poor to moderate thermal and electric conductivity, with graphite being a common exception in that regard.

Moreover, non-metals can exist in any one of the three-state forms, respectively: gases, liquids, and solids.

Physical Properties of Nonmetals

• State: Nonmetals are in gas and solid phase, at room temperature (r.t.). For example, oxygen is a gas, while carbon is solid. Bromine is unique in this group, because at r.t. it is a liquid, the only nonmetal in that state of matter.
• Malleable and Ductile: Nonmetals are fragile and brittle, they cannot be hammered into sheets or drawn into wires. The absence of malleability and ductility are another characteristics distinguishing it from metals.
• Conduction/ Electrical and Thermal Conductivity: Nonmetals are usually not conductors of heat or electricity. They are bad conductors in every respect because metal conducts the transfer of energy well.
• Lustre: Nonmetals are not shiny, so lack a surface to reflect. Nonmetals do not have metallic lustre as they do not reflect light.
• Melting and boiling: Melting and boiling are both physical changes in a substance in which energy is required to overcome the forces holding the particles (i.e., atoms) together. Metals have metallic bonding and there are electrostatic attractive forces between the metal ion(s) and the delocalized electrons. These are the forces in metals that give them high melting and boiling points and are comparable to ionic compounds and not covalent compounds.
• Diatomic Molecules: Under standard or laboratory conditions, seven nonmetals are naturally occurring diatomic molecules. These elements are hydrogen (H₂), nitrogen (N₂), oxygen (O₂), fluorine (F₂), chlorine (Cl₂), bromine (Br₂), and the black solid, iodine (I₂). Each element can be either gas, liquid or solid states of matter, depending of course.

Chemical Properties of Nonmetals

Non-metals usually gain or share electrons with other atoms which indicates they are electronegative. When non-metals react with metals, they typically gain electrons to reach a stable electron configuration with a noble gas (electron configuration), and produces anions . In the following reaction we will examine the rection of bromine to aluminum:

3Br₂​(l)+2Al(s)→2AlBr₃​(s)

Here, bromine atoms gain electrons from aluminum, producing aluminum bromide.

Compounds comprised entirely of non-metals are called covalent substances. They generally react with oxygen and yield either neutral or acidic oxides. These oxides will dissolve in water to give acids, such as how carbon dioxide dissolves in water to yield carbonic acid:

CO₂​(g)+H₂​O(l)→H₂​CO_3​(aq)

This is also why carbonated waters can be slightly acidic (carbonic acid is in carbonated water).

In addition, non-metal oxides can react with bases to form salts. For example, carbon dioxide reacts with sodium hydroxide to give sodium carbonate and water:

CO_2​(g)+2NaOH(aq)→Na₂​CO₃​(aq)+H₂​O(l)

Location of Nonmetals on the Periodic Table

Nonmetals principally occupy the far right of the periodic table, with the exception of hydrogen, which is placed in the upper left portion of the table.

In total, there are 17 nonmetals. Including hydrogen, the 17 nonmetals are as follows: Helium, carbon, nitrogen, oxygen, fluorine, neon, phosphorus, sulfur, chlorine, argon, selenium, bromine, krypton, iodine, xenon, and radon.

While there are distinctions in the chemical properties of each of these elements, they are all classified as nonmetals. Nonmetals will have distinct properties that are different from metals and metalloids.

Uses of Nonmetals

In contrast to metals, nonmetals may not have diverse applications universally, but they do serve specific functions in areas where they are frequently utilized collectively.

Several of these nonmetals are essential for life; nonmetals such as carbon, hydrogen, nitrogen, oxygen, sulfur, chlorine, and phosphorus play key roles in biological processes.

In agriculture, hydrogen, nitrogen, phosphorus, sulfur, chlorine, and selenium are applied in fertilizers as nonmetals to make plants grow in the production of food.

Some nonmetals are included in refrigeration and cryogenics, such as hydrogen, helium, nitrogen, oxygen, fluorine, and neon, that are applied according to their unique physical properties as refrigerants and in technology for cooling and freezing.

Many nonmetals are elemental components of various important industrial acids, including carbon, nitrogen, fluorine, phosphorus, sulfur, and chlorine.

Nonmetals have further applications in technology, such as those associated with lasers and lamps, but including their function in medicine and pharmaceuticals, and in other areas in which they provide important material in medical and technical applications and devices.

Nonmetals also serve an important function in many forms of technology and industrial production as they are central to the production of many thousands of compounds.

Actually, most of what the nonchemistry-nonscientific community interacts with every day, such as water, food, fabrics, plastics, and much more, likely contains one or more nonmetal elements in their compositions.

Properties of Metals and Non-Metals- What’s the Difference?

Properties	Metal	Non-Metal
Appearance	Shiny	Dull
State at room temperature	Solid (except mercury, which is a liquid)	About half are solids, about half are gases, and one (bromine) is a liquid
Density	High (they feel heavy for their size)	Low (they feel light for their size)
Strength	Strong	Weak
Malleable or brittle	Malleable (they bend without breaking)	Brittle (they break or shatter when hammered)
Conduction of heat	Good	Poor (they are insulators)
Conduction of electricity	Good	Poor (they are insulators, apart from graphite)
Magnetic material	Only iron, cobalt, and nickel	None
Sound when hit	They make a ringing sound (they are sonorous)	They make a dull sound
Type of oxide	Basic or alkaline	Acidic

Metalloid On The Periodic Table

Metalloids, also known as semimetals, have a distinct status in the periodic table because they show properties that are somewhere between metals and nonmetals.

Although the exact list of metalloids varies somewhat, there are usually between 6 and 9 elements classified as metalloids, lying on the diagonal line that separates metals from nonmetals.

There is considerable agreement that six boron, silicon, germanium, arsenic, antimony, and tellurium are definitely metalloids.

Some definitions even include bismuth, polonium, and astatine as metalloids but there is less certainty in their inclusion in the metalloid group. The difficulty in establishing an exact list of metalloids is to a degree, the idea of a single definitive property that all metalloids have in common is a elusive one.

Metalloids are better thought of in terms of the mix of metal and nonmetal properties they exhibit. For example, metalloids usually have atomic structures that forms covalent crystals, which are typically nonmetal rather than metal bonding structures. This geometric shape plays an important part in their behavior and uses.

One of the best known practical applications of metalloids was in electronics. Many metalloids serve as semiconductor materials for many household electronics.

This calls attention to the importance of the elements as they represent a practical valued classification between metals and nonmetals chemcially and functional.

Properties of Metalloids

The term “metalloid” is used to describe substances that exhibit properties between metals and nonmetals, but there is greater variation in characteristics between metalloids than there are for metals or nonmetals.

Metalloids are used extensively in the electronics industry to create semiconductors because they can conduct electricity in certain conditions.

All metalloids are solids at room temperature, and they are also able to create alloys with metals.

Silicon and germanium, are both metalloids and semiconductors. They can conduct electricity, but under limited conditions.

Silicon is shiny and lustrous, but it is not ductile or malleable; it is brittle which is more characteristic of a nonmetal. Metalloids generally conduct heat and electricity much less efficiently than metals.

Metalloids resemble metals physically, but chemically they behave more like nonmetals. They exhibit a range of oxidation states from +5 to -2 depending on which position in the periodic table the metalloid occupies.

Metals	Non-metals	Metalloids
Gold	Oxygen	Silicon
Silver	Carbon	Boron
Copper	Hydrogen	Arsenic
Iron	Nitrogen	Antimony
Mercury	Sulfur	Germanium
Zinc	Phosphorus

Common Properties of Metalloids

Broadly speaking, we can consider metalloids as very interesting because they are in some way in-between metals and nonmetals and this “in-betweenness” plays a role in their properties. There are traditional properties of metalloids that are similar.

For example, electronegativities of metalloids are between metals and nonmetals, so neither will stimulate a strong attraction for electrons due to metal characteristics, nor have strong electron losses due to nonmetal properties. Likewise, their ionization energies- the energy needed to remove an electron- are also between metals and nonmetals.

The unique part of metalloids is their “double identity.” Metalloids display some behaviors as one element type and others as the other element type, making their reactivity dependent on the element type they are reacting with. They can be metallic-like, and nonmetal-like at other moments.

Another notable aspect of metalloids is their type as semiconductors, which make them significant elements utilized in electronics, to where they can conduct electricity in some conditions and behave as an insulator in other conditions.

Metalloids often exhibit metallic luster; however,while that is a property demonstrated by many metalloids, they can and often do present in ways that are specifically identifiable and distinguishable from metals, such as a nonmetal or dull metallic appearance.

Physically, they are generally brittle solids, meaning they break as opposed to bend, and they have slightly more unique physical properties in forming liquids and gases in extreme conditions.

Chemically, metalloids exhibit more non-metal character, but metalloids have bonding ability with metals to form alloys such as bronze and brass.

Ultimately, metalloids do not belong in any category, and that is why they are fun to work with because they literally straddle between metals and nonmetals both chemically and structurally.

Chemical properties of Metalloids

Chemical properties describe how a substance behaves when it interacts or reacts with other substances; it essentially describes how one substance changes into a different substance as a result of chemical interactions.

Chemical properties can only be determined through or after the establishment of a chemical reaction (rusting, combustion, tarnishing, and maybe even detonation). You can only calculate and define an element’s chemical properties based on that chemical reaction.

Chemical properties demonstrate some interesting behavior for metalloids:

• They easily oxidize to produce gases.
• Metalloids are able to reactive with metals to form a variety of alliances.
• In addition and they also contain allotropes that have both a metallic and non-metallic character.
• Ironically some metalloids contract when they melt instead of expands.
• Finally metalloids react their greatest ease with halogens to produce compounds.

Together, these traits highlight how metalloids occupy a unique space between metals and non-metals, exhibiting a mix of behaviors depending on the context.

Location of Metalloids on the Periodic Table

Metalloids form a curious “bridge” between metals and nonmetals on the periodic table, usually in a zigzag shape that describes a diagonal stretch from boron (B) in Group 13 down toward Group 16 (and possibly into Groups 17 or 18 if you want to draw the line that way).

Iron, copper, and aluminum sit on the metal side of the diagonal line, while oxygen, fluorine, and neon are insulators and gases on the nonmetal side. The exception is hydrogen; it acts like a nonmetal, but has its seat at the far left of the periodic table.

Although the “classic” metalloid family contains six elements (boron, silicon, germanium, arsenic, antimony, and tellurium), some chemists include bismuth (Bi), polonium (Po), and astatine (At) in period 6 as metalloids due to their mixed characteristics.

The only thing they all share is a middle-of-the-road behavior: they are partially conductors, have variable oxidation states, and have semiconducting properties, which may be why they are essential materials in electronics.

In practical terms, this slanted line is not simply a neat graphic; it signifies a continuum of chemical personalities. Metalloids are neither metallic nor nonmetallic; they present a mix of both metalloid and nonmetallic characters, offering materials that conduct electricity most of the time but also can insulate under certain conditions.

This combination of characteristics is why they are so useful and interesting, whether you are making microchips or just appreciate the orderliness in the periodic table.

More Resources: Where are Metalloids on the Periodic Table?

Trends in Metallic and Nonmetallic Character

When considering the periodic table, we can conclude that the elements on the left side of the table will have the most metallic character (i.e., alkali metals). These metallic characteristics decrease as you move to the right along the period and begin to introduce non-metallic character.

This is also noted by the fact that electronegativity and ionization energy increase as we move to the right, meaning that the elements become more charged to their electrons, less likely to remove electrons, which is essentially how we define metals and non-metals.

Now, if you consider the columns (groups), you will see that the metallic character increases with each column down the group. This happens because electronegativity and ionization energy usually decrease, meaning the element will more easily lose electrons and behave more like metals.

While this trend holds reasonably well, the transition metals (d block) in the middle of the periodic table tend to regard it less, establishing rules of their own.

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