Chemistry Chapter 4 Flashcards

Chemical Bonding and Structure

• Polarity of bonds is determined by the difference in electronegativity between the two atoms involved.
• A correct Lewis structure for Bromine Chloride (BrCl) illustrates the sharing of electrons between the two elements.

Chemical Naming and Formulas

• Ammonium sulfate is represented by the formula (NH4)2SO4, indicating two ammonium ions and one sulfate ion.
• The covalent compound N2O4 is named dinitrogen tetroxide, reflecting its molecular structure.

Molecular Geometry

• Ammonia (NH3) has a pyramidal molecular structure with a triangular base due to its lone pair of electrons.

Interparticle Forces

• Dispersion forces, also known as London dispersion forces, are the weakest type of intermolecular forces and typically lead to compounds with the lowest melting points.

Molecular Polarity

• Hydrogen sulfide (H2S) is expected to be the most polar molecule among the options due to the significant difference in electronegativity between hydrogen and sulfur.

Electron Configuration and Noble Gas Configuration

• A calcium atom can achieve a noble gas configuration by losing two electrons, transitioning to a more stable electron arrangement.
• Group VA (15) elements, such as phosphorus, attain noble gas configuration through the gain of three electrons.

Isoelectronic Species

• Sodium ion (Na+) and fluoride ion (F−) are isoelectronic, meaning they have the same electron configuration, despite being different elements.

Electronegativity Trends

• Oxygen (O) has the highest electronegativity among common elements, indicating its strong tendency to attract electrons in chemical bonds.