Metals Conducting Heat and Cutting Ability Quiz

Which property makes metals like mercury and potassium good conductors of heat?

Which metal is an exception as it has a very low melting point compared to other metals?

Why are nonmetals generally not good conductors of electricity?

Which type of substance exhibits a metallic luster in its solid state?

Which nonmetal is the exception by being a good conductor of electricity?

What property allows metals to conduct electricity both in liquid and solid states?

What property of diamonds makes them a poor conductor of electricity?

Which element is known for its high thermal conductivity?

Which substance is shiny, has a low melting point, and is not a good conductor of electricity?

What property of metals decreases with exposure to atmospheric oxygen?

Which type of substance has the property of brittleness?

What property of metals allows them to change shape without breaking?

What is the purpose of dipping the copper wire in ferrous sulphate solution?

How can one recognize that a reaction has taken place in this experiment?

What is the significance of using reactivity series of metals in this experiment?

Why are oxygen, water, and acids not useful in determining the relative reactivity of all metals?

What is the purpose of observing continually at fixed intervals during the experiment?

How does the displacement reaction of metals with solutions serve as a useful tool?

Metals like mercury and potassium are good conductors of heat due to their high thermal conductivity.
Mercury is an exception among metals, having a very low melting point compared to others.
Nonmetals are generally poor conductors of electricity because they do not have free electrons to carry electrical current.
Metals exhibit a metallic luster in their solid state.
Carbon (in the form of graphite) is an exception among nonmetals, being a good conductor of electricity.

Metals can conduct electricity in both liquid and solid states due to the mobility of their electrons.
The high thermal conductivity of metals, such as copper, makes them useful for conducting heat.
The property of metals that allows them to change shape without breaking is malleability.
Metals can react with atmospheric oxygen, leading to a decrease in their ductility.

Diamonds have a poor electrical conductivity due to the strong covalent bonds between their carbon atoms.
The property of diamonds that makes them poor conductors of electricity is their strong covalent bonds.

Dipping a copper wire in ferrous sulphate solution helps to observe the reaction and identify the reactivity of metals.
Recognizing a reaction has taken place can be done by observing changes such as color changes, gas formation, or precipitation.
The reactivity series of metals is useful in determining the relative reactivity of metals, as it helps to predict the outcome of displacement reactions.
Oxygen, water, and acids are not useful in determining the relative reactivity of all metals, as they may react with some metals but not others.
Observing the experiment at fixed intervals allows for the monitoring of reaction rates and the identification of patterns.
The displacement reaction of metals with solutions serves as a useful tool for determining the reactivity of metals and predicting their behavior in different situations.