Question

Compare the physical and chemical properties of metals and nonmetals.

Short answer

Metals are shiny, conductive, and malleable; they lose electrons chemically. Nonmetals are dull, insulating, and brittle; they gain electrons chemically.

Step-by-step solution

Identify Physical Properties of Metals

Metals generally have a shiny appearance, are good conductors of heat and electricity, are malleable (can be hammered into thin sheets), ductile (can be drawn into wires), and most metals are solid at room temperature (except for mercury).

Identify Physical Properties of Nonmetals

Nonmetals can be found in solid, liquid, or gaseous states at room temperature. They usually have a dull appearance, are poor conductors of heat and electricity, and are not ductile or malleable. Many nonmetals are brittle when in solid form.

Explore Chemical Properties of Metals

Metals tend to lose electrons during chemical reactions, forming positive ions. They often react with acids to produce hydrogen gas and usually form ionic compounds with nonmetals.

Explore Chemical Properties of Nonmetals

Nonmetals generally gain electrons during chemical reactions, forming negative ions. They can react with metals to form ionic compounds, and with other nonmetals to form covalent compounds. Nonmetals can also form acidic oxides.

Key concepts

Physical Properties

Metals and nonmetals can be distinguished by their distinct physical properties.

• **Metals**: Typically have a shiny, lustrous appearance due to their ability to reflect light. They are usually solid at room temperature, with mercury being a notable liquid exception. Metals are also known for being good conductors of heat and electricity, making them valuable in wiring and other applications. Their most impressive features are malleability and ductility, allowing them to be hammered into thin sheets or drawn into wires, respectively.
• **Nonmetals**: Often lack the shine of metals and appear dull. These elements can exist in solid, liquid, or gaseous states at room temperature. Solid nonmetals tend to be brittle, making them challenging to shape without breaking. Moreover, nonmetals are poor conductors, meaning they do not allow heat or electricity to pass through easily.

Understanding these properties helps determine how both metals and nonmetals are used in everyday applications.

Chemical Properties

The chemical properties of metals and nonmetals reveal how they behave in reactions with other substances.

• **Metals**: Metals are prone to losing electrons during chemical reactions, which transforms them into positive ions. This electron donation allows them to easily form ionic bonds, particularly when reacting with nonmetals. Metals frequently react with acids, often resulting in the formation of hydrogen gas. This electron loss allows metals to form various compounds.
• **Nonmetals**: In contrast, nonmetals usually gain electrons in reactions, turning them into negative ions. This electron gain makes nonmetals adept at forming ionic compounds when mixed with metals. Nonmetals can also bond with each other through covalent bonds, where they share electrons rather than exchange them. Many nonmetals are known for forming acidic oxides when they react with oxygen.

These chemical properties are crucial for predicting the types of compounds metals and nonmetals can make.

Conductivity

Conductivity refers to a material's ability to allow heat or electricity to pass through it.
**Metals** are renowned for their high conductivity. Their atomic structure allows electrons to move freely, making metals excellent conductors of electricity and heat. This property is why metals are widely used in electrical wiring and as cooking utensils, as they efficiently transfer energy.
On the other hand, **Nonmetals** generally exhibit low conductivity. The lack of free-moving electrons in nonmetals makes them poor conductors of electricity and heat. This property makes nonmetals suitable for insulation purposes, as they do not conduct heat or electricity well, ensuring safety and energy conservation.
Understanding whether a material is a good conductor influences how it is used in technology and everyday applications.

Malleability

Malleability is a material's ability to deform under compressive stress, such as hammering or rolling.
**Metals** are highly malleable, a characteristic that allows them to be shaped into thin sheets without breaking. This property is due to the metallic bonds in metals, where atoms are arranged in layers that can slide over one another without disrupting the overall structure. Malleability is why metals are frequently used in construction and manufacturing. **Nonmetals**, conversely, lack malleability. Instead, they tend to be brittle, especially when solid. This brittleness means nonmetals can easily crack or shatter when force is applied. The lack of malleability in nonmetals limits their use in applications where structural integrity is essential.
Recognizing a material's malleability is vital for determining its role in industrial and practical uses.

Electron Transfer

Electron transfer describes how electrons move between atoms during chemical reactions.
In **Metals**, electrons are typically lost. This loss results in the formation of positive ions, which can form ionic bonds with negatively charged ions from nonmetals. The tendency to lose electrons makes metals reactive with a variety of substances and allows them to participate actively in reactions. For **Nonmetals**, electron transfer usually involves gaining electrons. This gain typically occurs during reactions with metals, resulting in the formation of negative ions. Nonmetals tend to either share or gain electrons, leading to the formation of covalent or ionic bonds, respectively. Understanding electron transfer is crucial in predicting how elements will react and the kinds of compounds they can form. This knowledge is essential in chemistry for designing new materials and understanding natural processes.