1 of 51 of 5 Items
Question
Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?(1 point)
Responses
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
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.
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.
Skip to navigation
9 answers
The correct response to the question about why metallic bonds allow metals to be conductive is:
The bonds can shift because valence electrons are held loosely and move freely.
This explanation highlights the nature of metallic bonding, where the valence electrons are delocalized and can move freely throughout the metal lattice, allowing for electrical conductivity.
The correct response regarding between which types of elements ionic bonds occur and how electrons act within the bond is:
metals and nonmetals, electrons transferred.
In ionic bonding, electrons are transferred from the metal to the nonmetal, resulting in the formation of ions that are held together by electrostatic forces.
The correct response regarding the kind of bond that would occur between sodium (Na, Group IA) and chlorine (Cl, Group VIIA) is:
ionic.
Sodium donates an electron to chlorine, resulting in the formation of Na⁺ and Cl⁻ ions, which are held together by ionic bonds.
The correct response regarding the type of bond and how many bonds would occur as carbon dioxide (CO₂) is formed from carbon (Group IVA) and oxygen (Group VIA) is:
two ionic bonds.
However, please note that the formation of CO₂ actually involves two covalent bonds, where carbon shares two pairs of electrons with each oxygen atom (one double bond with each oxygen). If the intent is to capture the covalent nature of the bonds in CO₂, the most accurate response would be two covalent bonds.
If that option is not available or mistakenly provided, please let me know for clarification.
The correct response regarding how many covalent bonds nitrogen (Group 5A) is likely to form is:
three.
Nitrogen typically forms three covalent bonds to achieve a stable octet configuration by sharing three of its five valence electrons.
