Honors Unit 4 Bonding and Molecular Geometry

What type of bond involves the transfer of electrons from a metal to a nonmetal?

• Covalent bond
• Metallic bond
• Hydrogen bond
• Ionic bond
• Coordinate bond

Answer explanation

Ionic bonds involve electron transfer from metals to nonmetals.

Which of the following is NOT a property of ionic compounds?

• High melting points
• Conductivity in molten form
• Form discrete molecules
• Brittleness
• Crystal lattice formation

Answer explanation

Ionic compounds form lattices, not discrete molecules.

What is the primary type of bonding in a sample of copper metal?

• Ionic bonding
• Covalent bonding
• Hydrogen bonding
• Metallic bonding
• Coordinate bonding

Answer explanation

Metallic bonding occurs in pure metals like copper.

What explains why metals are malleable and conduct electricity well?

• Strong ionic attractions
• Shared electron pairs
• Delocalized electrons
• Low electronegativity
• Covalent crystal structures

Answer explanation

Delocalized electrons in metals allow conductivity and malleability.

In covalent bonding, electrons are:

• Transferred from one atom to another
• Shared between nonmetals
• Delocalized among ions
• Trapped in crystal lattices
• Moved into d-orbitals

Answer explanation

Covalent bonding involves sharing electrons between nonmetals.

Select all that are properties of metallic substances.

• Ductile
• Shiny
• Poor conductor
• High melting point
• Form discrete molecules

Answer explanation

Metals are ductile, shiny, and have high melting points.

Which bond type is characterized by a 'sea of electrons'?

• Ionic
• Metallic
• Covalent
• Hydrogen
• Polar

Answer explanation

Metallic bonds involve a 'sea of electrons' shared among atoms.

Which element combination is most likely to form an ionic bond?

• Oxygen and chlorine
• Sodium and fluorine
• Carbon and hydrogen
• Nitrogen and oxygen
• Chlorine and bromine

Answer explanation

Sodium and fluorine (metal + nonmetal) form an ionic bond.

Covalent compounds tend to have:

• High melting points and high conductivity
• Crystal lattices and ionic bonds
• Low melting points and no conductivity
• Free-flowing electrons
• Strong ion-dipole forces

Answer explanation

Covalent compounds are typically poor conductors with low melting points.

In metallic bonding, the strength of the bond increases with:

• Atomic radius
• Number of protons
• Electron affinity
• Number of valence electrons
• Atomic mass

Answer explanation

More valence electrons lead to stronger metallic bonding.