Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?(1 point)
Responses
Metals have low electronegativity, so they are conductive because they pass charges easily.
Metals have low electronegativity, so they are conductive because they pass charges easily.
An attraction between a positive charge and a negative charge is created.
An attraction between a positive charge and a negative charge is created.
The bonds can shift because valence electrons are held loosely and move freely.
The bonds can shift because valence electrons are held loosely and move freely.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
The bonds can shift because valence electrons are held loosely and move freely.
Between which types of elements do ionic bonds occur, and how do electrons act within the bond?(1 point)
Responses
metals and nonmetals, electrons transferred
metals and nonmetals, electrons transferred
nonmetals and nonmetals, electrons shared
nonmetals and nonmetals, electrons shared
metals and metals, electrons freely moving
metals and metals, electrons freely moving
nonmetals and metals, electrons shared
metals and nonmetals, electrons transferred
Which kind of bond would occur between sodium (Na, Group IA) and chlorine (Cl, Group VIIA)?(1 point)
Responses
ionic
ionic
covalent
covalent
metallic
metallic
no bond
ionic
Which type of bond and how many bonds would occur as carbon dioxide (CO2) is formed from carbon in Group IVA and oxygen in Group VIA?(1 point)
Responses
four covalent bonds
four covalent bonds
one covalent bond
one covalent bond
two ionic bonds
two ionic bonds
three metallic bonds
four covalent bonds
How many covalent bonds is nitrogen (Group 5A) likely to form?(1 point)
Responses
two
two
three
three
four
four
five
three
The correct answer is: The bonds can shift because valence electrons are held loosely and move freely.
The reason metallic bonds are responsible for properties like conductivity in metals is due to the nature of these bonds. Metallic bonding occurs when metal atoms come together and their valence electrons become delocalized. Unlike in ionic or covalent bonds, where electrons are shared or transferred between individual atoms, metallic bonds involve a sea of freely moving electrons surrounding the metal ions.
Because the valence electrons in metallic bonds are held loosely and not confined to specific atoms, they are able to move freely throughout the structure of the metal. This mobility allows the valence electrons to easily carry electric charge or current, making metals excellent conductors of electricity. When a voltage is applied to a metal, the loosely held valence electrons are able to flow in response to the electric field, transferring charge from one point to another.
In contrast, in ionic or covalent bonds, the electrons are held more tightly to their respective atoms and are less mobile. This restricts their ability to move and carry charge, resulting in lower conductivity compared to metals.
Therefore, the ability of metallic bonds to hold valence electrons loosely and allow them to move freely is what makes metals conductive.