Nonmetals and Metalloids Practice Quiz

Oxygen is a nonmetal with typical nonmetal properties such as high electronegativity and poor conductivity. The other options are metals with distinctly different characteristics.

Nonmetals are known for their insulating properties due to the absence of free electrons. They are neither malleable nor shiny like metals.

Metalloids exhibit properties that are intermediate between metals and nonmetals. They often display characteristics such as semiconductivity and brittleness.

Noble gases are nonmetals known for their inert behavior and are located in Group 18. The other groups are primarily made up of metals.

Solid nonmetals usually appear dull and are brittle due to directional bonding forces. This contrasts with metals, which are shiny and malleable.

Silicon is a metalloid widely used in electronics because of its semiconducting capabilities. Its intermediate conductivity distinguishes it from typical metals and insulators.

Electronegativity increases across a period because of the increasing effective nuclear charge. This trend is particularly noticeable for nonmetals.

Nonmetals usually exhibit high ionization energies because their valence electrons are held tightly by the nucleus. This contrasts with metals, which have lower ionization energies due to a looser electron hold.

Metalloids can conduct electricity when conditions such as temperature or doping are favorable, a hallmark of semiconductors. They do not behave like metals that conduct continuously.

Nitrogen, a nonmetal, constitutes roughly 78% of Earth's atmosphere. The other elements are metals and are not present in significant amounts in the air.

Metalloids show a mix of metallic and nonmetallic characteristics, including brittleness and variable electrical conductivity. These traits are unlike the consistent malleability and high conductivity of true metals.

Many nonmetals, including oxygen and nitrogen, exist as gases at room temperature. This is in contrast to metals, which are usually solid under standard conditions.

As the effective nuclear charge increases across a period, nonmetals have a smaller atomic radius because electrons are pulled closer to the nucleus. This is a well-established periodic trend.

Carbon is the cornerstone of organic chemistry because of its ability to form diverse compounds essential for life. Its unique bonding properties set it apart from other elements.

The directional nature of covalent bonds in nonmetals leads to rigid and brittle structures. This is in contrast to the non-directional metallic bonds that allow flexibility in metals.

As you move across a period, the effective nuclear charge increases, pulling electrons closer and thus increasing electronegativity. This is the primary factor behind the observed trend in nonmetals.

Nonmetals typically share electrons to form covalent bonds, whereas metalloids have intermediate properties that allow for both polar covalent and limited metallic bonding. This mixed bonding behavior is a key characteristic of metalloids.

Nonmetals have low conductivity because they lack free electrons that facilitate heat and charge transfer. This absence of delocalized electrons is the main reason for their insulating properties.

Nonmetals possess a smaller atomic radius because of a higher effective nuclear charge, which holds electrons more tightly and requires more energy to remove an electron. This directly results in higher ionization energies compared to metalloids.

Antimony is a metalloid that exhibits variable oxidation states, which makes it valuable in electronics and flame retardant applications. Its versatility in bonding is not found in the other elements listed.