Lesson Worksheet: Metallic Bonding Chemistry • 7th Grade
In this worksheet, we will practice describing metallic bonding and the effect it has on the physical and chemical properties of metals.
Q1:
Which of the following is the best description of delocalized electrons in metallic bonding?
- ACore electrons bound to metal ions
- BCore and valence electrons that can move freely between metal ions
- CValence electrons that can move freely between metal ions
- DValence electrons bound to metal ions
- ECore electrons that can move freely between metal ions
Q2:
In a sample of calcium metal, how many electrons does an atom of calcium contribute to the sea of delocalized electrons?
Q3:
In a sample of potassium metal, how many electrons does an atom of potassium contribute to the sea of delocalized electrons?
Q4:
Metals are typically shiny and electrically conductive, while ionic solids are dull and electrically insulating. Which feature of metals is responsible for this difference?
- AThe delocalized electrons
- BThe number of neutrons in the nuclei
- CThe charges of the positive ions
- DThe atomic mass of the nuclei
- EThe crystal lattice of positive ions
Q5:
In metallic bonding, what is the dominant form of attraction between the lattice of positive ions and the sea of delocalized electrons?
- AGravitational
- BNuclear
- CMagnetic
- DElectrostatic
- ECovalent
Q6:
Shown in the diagram are the electronic structures of lithium and calcium atoms.
The melting temperature of lithium is , while that of calcium is . Based on the electronic structures of the atoms and the strength of their metallic bonds, explain this difference in melting temperature.
- AMetallic bonds are stronger in lithium as the valence electrons are closer to the nucleus, so more thermal energy is needed to break up the metal lattice.
- BMetallic bonds are stronger in lithium as there are fewer valence electrons, so more thermal energy is needed to break up the metal lattice.
- CMetallic bonds are weaker in lithium as there are fewer valence electrons, so less thermal energy is needed to break up the metal lattice.
- DMetallic bonds are stronger in lithium as there are more valence electrons, so more thermal energy is needed to break up the metal lattice.
- EMetallic bonds are weaker in lithium as the valence electrons are closer to the nucleus, so less thermal energy is needed to break up the metal lattice.
Q7:
Which of the following atoms would form a solid metal with the highest melting point?
- A
- B
- C
- D
- E
Q8:
Which of the following atoms would form a solid metal with the highest electrical conductivity?
- A
- B
- C
- D
- E
Q9:
Which of the following atoms would form a solid metal with the lowest thermal conductivity?
- A
- B
- C
- D
- E
Q10:
Which of the following is the best description of electrical conduction in a solid metal?
- APositive ions flow through a lattice of negative ions.
- BNegatively charged particles flow through a lattice of positive ions.
- CPositively charged particles flow through a lattice of positive ions.
- DPositively charged particles flow through a lattice of negative ions.
- ENegative ions flow through a lattice of positive ions.
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