Unit 2 (Part 1) Bonding Review

Oxygen has a -2 charge when it forms an ion because it ________ electrons.

• gains

• loses

Answer explanation

Oxygen has a -2 charge when it forms an ion because it gains electrons. By gaining two electrons, it achieves a stable electron configuration, resulting in the negative charge.

In an ionic bond electrons are​ (a)   .

In a metallic bond electrons are​ (b)   .

In a covalent bond electrons are​ (c)   .

• not involved in the bonding process

• partially transferred

• fully transferred from one atom to another

• free to move and create a 'sea' of electrons

• equally shared between atoms

Answer explanation

In an ionic bond, electrons are fully transferred from one atom to another, creating charged ions. In a metallic bond, electrons are free to move, forming a 'sea' of electrons. In a covalent bond, electrons are equally shared between atoms.

The Electron Sea Model is used to describe which type of bonding?

• Ionic Bonding

• Covalent Bonding

• Metallic Bonding

• Trauma Bonding

Answer explanation

The Electron Sea Model describes metallic bonding, where electrons are delocalized and shared among a lattice of metal cations, allowing for conductivity and malleability. This model does not apply to ionic or covalent bonding.

According to the octet rule, elements forming covalent bonds do so to attain how many valence electrons?

• Seven (7)

• Four (4)

• Two (2)

• Eight (8)

Answer explanation

According to the octet rule, atoms form covalent bonds to achieve a stable configuration of eight valence electrons. This is crucial for chemical stability, making 'Eight (8)' the correct answer.

Tags

NGSS.HS-PS1-1

Match the terms to the correct definitions:

Malleable- (a)  

Ductile-​ (b)  

Covalent bond-​ (c)  

Ionic bond-​ (d)  

Metallic bond-​ (e)  

• A type of metal.

• A type of rock.

• Capable of being hammered into sheets/foil/leaf.

• Able to be drawn out into a thin wire.

• A type of duct tape.

• A type of fabric.

• A type of bond where electrons are shared.

• A type of bond where electrons are transferred.

• Able to conduct electricity.

• A type of bond where electrons are delocalized.

Answer explanation

Malleable means capable of being hammered into sheets, ductile refers to being drawn into wires, covalent bonds involve shared electrons, ionic bonds involve transferred electrons, and metallic bonds have delocalized electrons.

Select the option(s) that define conductivity.

• The measure of a material's ability to conduct heat

• The measure of a material's ability to conduct electricity

• The measure of a material's ability to conduct light

• The measure of a material's ability to conduct sound

Answer explanation

Conductivity refers to a material's ability to conduct heat and electricity. The other options, light and sound, do not define conductivity in the context of materials.

Tags

NGSS.HS-PS2-5

NGSS.HS-PS3-5

Match the pictograms to the corresponding hazard.

• Explosive

• 
• Acute Toxicity

• 
• Flammable

• 
• Corrosive

• 

Tags

NGSS.HS-ETS1-3

Why are metals malleable, ductile, and good conductors?

• Because metals have free electrons

• Because metals are hard and shiny

• Because metals are heavy

• Because metals are naturally occurring elements

Answer explanation

Metals are malleable and ductile due to the presence of free electrons, which allow atoms to slide past each other without breaking bonds. This also enables them to conduct electricity efficiently.

The term "delocalized electrons" applies to which type of bond?

• ionic bonds

• covalent bonds

• metallic bonds

• parental bonds

Answer explanation

Delocalized electrons are characteristic of metallic bonds, where electrons are not confined to individual atoms but are free to move throughout the metal lattice, contributing to conductivity and malleability.

Tags

NGSS.HS-PS1-1

Covalent bonds occur when 2 elements have a small difference in electronegativity. Most covalent bonds occur between what type(s) of elements?

• metals

• nonmetals

• metalloids

Answer explanation

Covalent bonds typically form between nonmetals, as they have similar electronegativities and can share electrons effectively. Metals usually form ionic bonds, while metalloids can exhibit both behaviors.