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Unit 1 - Periodic Motion and Wave Mechanics

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Interactive Testing and Evaluation: Lesson 1 – Chemical Bonding and Types of Compounds

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1.
Which of the following compounds exhibits polar covalent bonding due to a significant difference in electronegativity between 0.4 and 1.7?
Water (H2O)
Chlorine gas (Cl2)
Sodium chloride (NaCl)
Methane (CH4)
2.
The nitrogen molecule (N2) contains a:
Triple covalent bond (one sigma bond and two pi bonds) sharing 3 electron pairs
Coordinate dative bond
Double covalent bond
Single ionic bond
3.
Solid ionic compounds such as crystal NaCl do NOT conduct electricity in the solid state because:
They contain no electrical charges
They decompose in the presence of air
Electrons are moving too rapidly
Their ions are tightly locked in fixed positions within the rigid crystal lattice and cannot move freely
4.
A metallic bond is physically described as the electrostatic attraction between:
Protons and neutrons in the nucleus
Positive metal cations in the crystal lattice and the mobile sea of delocalized valence electrons
Dipole molecules in a polar liquid
Positive ions and negative non-metal anions
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