CPC Unit 5 True or False

Front

Metals are poor conductors.

Back

False. Metals are generally good conductors of heat and electricity due to the presence of free-moving electrons.

Front

Elements tend to react so that they acquire the electron structure of a halogen.

Back

False. Elements tend to react to achieve a stable electron configuration, often resembling that of noble gases, not halogens.

Front

The crystal lattice of ionic compounds affects their melting and boiling points.

Back

True. The strong electrostatic forces in the crystal lattice lead to high melting and boiling points.

Front

A sodium (Na) atom tends to lose one electron when it reacts.

Back

True. Sodium has one valence electron and readily loses it to form a Na+ ion.

Front

Elements in group 1 lose their one valence electron, forming an ion with a 1+ charge.

Back

True. Group 1 elements, like sodium and potassium, lose one electron to form cations with a +1 charge.

Front

Ionic compounds are formed by the transfer of electrons from one atom to another.

Back

True. Ionic bonds form when electrons are transferred, resulting in the attraction between positively and negatively charged ions.

Front

Covalent bonds involve the sharing of electrons between atoms.

Back

True. In covalent bonding, atoms share pairs of electrons to achieve stability.

Front

The octet rule states that atoms are most stable when they have eight electrons in their outer shell.

Back

True. Atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons.

Front

Metals typically form anions when they react.

Back

False. Metals usually lose electrons to form cations.

Front

Nonmetals tend to gain electrons during chemical reactions.

Back

True. Nonmetals often gain electrons to achieve a full outer shell, forming anions.