Bonds Quick Check

Question

Bonds Quick Check

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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.
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9 answers
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Answer 1

Bot GPT 4-o mini answered
1 month ago

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.

Answer 2

cocopuff answered
1 month ago

Between which types of elements do ionic bonds occur, and how do electrons act within the bond?(1 point)

Responses

metals and metals, electrons freely moving
metals and metals, electrons freely moving

nonmetals and nonmetals, electrons shared
nonmetals and nonmetals, electrons shared

metals and nonmetals, electrons transferred
metals and nonmetals, electrons transferred

nonmetals and metals, electrons shared

Answer 3

Bot GPT 4-o mini answered
1 month ago

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.

Answer 4

cocopuff answered
1 month ago

Which kind of bond would occur between sodium (Na, Group IA) and chlorine (Cl, Group VIIA)?(1 point)

Responses

metallic
metallic

covalent
covalent

no bond
no bond

ionic

Answer 5

Bot GPT 4-o mini answered
1 month ago

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.

Answer 6

cocopuff answered
1 month ago

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

one covalent bond
one covalent bond

two ionic bonds
two ionic bonds

three metallic bonds
three metallic bonds

four covalent bonds

Answer 7

Bot GPT 4-o mini answered
1 month ago

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.

Answer 8

cocopuff answered
1 month ago

How many covalent bonds is nitrogen (Group 5A) likely to form?(1 point)

Responses

four
four

three
three

five
five

two

Answer 9

Bot GPT 4-o mini answered
1 month ago

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.