Classify Metals and Nonmetals: Practice Quiz

Metals are typically shiny and malleable, allowing them to be shaped without breaking. These properties contrast with nonmetals, which are often dull and brittle.

Nonmetals are generally poor conductors of electricity, contrasting with metals which are excellent conductors. They tend to be brittle and lack the shine seen in metals.

Brittleness is a characteristic commonly associated with nonmetals rather than metals. Metals are known for their ductility and malleability due to the nature of metallic bonding.

Metals are excellent conductors of electricity due to their free-moving electrons, making them ideal for wiring. In contrast, nonmetals do not conduct electricity well.

Nonmetals generally do not conduct heat well because they lack free-moving electrons. Metals, on the other hand, are typically good conductors of both heat and electricity.

The described properties are classic traits of metals. Nonmetals and metalloids generally do not exhibit malleability, ductility, and a shiny appearance all together.

Nonmetals generally do not conduct electricity when in a solid state due to the absence of free electrons. This differentiates them from metals, which exhibit strong conductive properties.

Metals are characterized by high electrical and thermal conductivity because of their delocalized electrons. Nonmetals lack these free electrons, which results in poor conductivity.

Metals tend to have higher densities due to their closely packed atomic structures. In contrast, nonmetals often have more open and less dense atomic arrangements.

Ductility refers to the ability of a material, typically a metal, to be stretched into wires. This property is due to the nature of metallic bonding which allows atoms to slide past each other.

Mercury stands out among metals as it is liquid at room temperature. This property is due to its unique electron configuration and bonding, which differs from that of most other metals.

While properties like electrical conductivity, malleability, and luster provide clear distinctions, color is not a reliable factor. Both metals and nonmetals can exhibit a range of colors that do not correlate with their classification.

The combination of properties such as electrical conductivity, malleability, and lustrous appearance are hallmarks of metals. Nonmetals or other compounds generally do not exhibit all these features simultaneously.

At room temperature, almost all metals exist in the solid state due to their strong metallic bonds and high melting points. Mercury is an exception, but it is not representative of most metals.

Nonmetals typically do not conduct electricity in the solid state because they lack free-moving electrons. Metals have delocalized electrons, which allow them to conduct electricity efficiently.

Metals are malleable because their atoms are held together by a 'sea of electrons' that can shift without breaking bonds. In contrast, nonmetals have more directional and fixed bonding, leading to brittleness.

Graphite has a layered structure in which electrons can move freely along the layers, imparting metallic conductivity. This unique structural arrangement gives graphite properties that differ from typical nonmetals.

Metals have electrons in their outer shells that are not tightly bound, resulting in a 'sea' of delocalized electrons. This electron mobility is key to the high electrical conductivity observed in metals.

The insulating nature of nonmetals is largely due to the absence of free-moving electrons, which are essential for electrical conduction in metals. Their electrons are localized, inhibiting electron flow.

The combination of lustrous appearance, malleability, and good heat conduction strongly indicates that the element is a metal. The slow reaction with acids suggests the presence of a passivating oxide layer, a phenomenon seen in some reactive metals.