Chemical Bonding Quiz

A hydrogen bond between an H atom of one molecule and O, N, or F of another molecule.

A hydrogen bond between an H atom and O, N, or F within the same molecule.

Include high melting and boiling points, high solubility of some compounds, and formation of 3D crystal lattice.

Some covalent compounds dissolve in water due to hydrogen bonding with water molecules.

A stable structure formed by hydrogen bonds, as seen in water (H2O).

Complementary strands of DNA are held together by hydrogen bonds between nucleotides (A&T, C&G).

N-H---O hydrogen bonds help maintain the structure of proteins.

Hydrogen bonding stabilizes structures in DNA and proteins, essential for life functions.

Electrostatic attraction between H bonded to electronegative atom X and lone pair on X in another molecule.

Atoms with high electronegativity capable of forming hydrogen bonds, specifically O, N, and F.

Hydrogen bonds are weaker than covalent bonds, with energy less than 10 kcal/mole vs. 120 kcal/mole.

Requires high electronegativity and small size of the atom bonded to hydrogen for effective bonding.

Hydrogen bonds favor a straight-line bonding direction due to lone pair electron distribution.

N forms stronger hydrogen bonds than Cl, despite equal electronegativity, due to smaller atomic size.

Common hydrogen bonding molecules include HF, H2O, and NH3, due to their high electronegativity.

Hydrogen bonds lead to clustering or chains of associated molecules, like many tiny magnets together.

An attraction force between non-metal atoms formed by sharing an electron pair.

Compounds that contain covalent bonds between atoms.

Electrons in the outer shell that determine an atom's bonding behavior.

A configuration where an atom has eight electrons in its outer shell, achieving stability.

A condition where two atoms attract electrons equally, necessary for covalent bonding.

A bond formed by equal sharing of electrons due to similar electron affinities.

Covalent compounds can exist as gases, liquids, or soft solids at room temperature.

Covalent compounds typically have low melting and boiling points due to weak intermolecular forces.

A force between atoms that holds them in a stable molecule.

Ionic, covalent, and coordinate covalent bonds are the main types.

The capacity of an element to bond with others, indicated by the number of bonds formed.

Bonding electrons participate in bond formation; non-bonding electrons do not.

Atoms tend to achieve a stable arrangement of eight electrons in their outer shell.

For Helium and certain light elements, a stable configuration is achieved with two electrons.

Atoms achieve stability by transferring or sharing electrons to mimic noble gas configuration.

A molecule composed of three oxygen atoms, often found in the Earth's stratosphere.

A colorless, odorless gas consisting of one carbon atom bonded to one oxygen atom, poisonous in high concentrations.

A type of bond where electrons are shared unequally, creating partial charges on atoms.

A measure of the separation of positive and negative charges in a molecule, indicating polarity.

The tendency of an atom to attract shared electrons towards itself in a bond.

Forces of attraction that require little energy to break, such as hydrogen bonds and van der Waals interactions.

Chemical interactions that do not involve electron sharing, crucial for biological stability.

Interactions between water and nonpolar molecules, leading to non-polar molecules maximizing interaction with each other.

The tendency of nonpolar molecules to cluster together in a polar solvent to minimize undesirable interactions.

Hydrophobic interactions contribute to protein folding and stability, aiding biological activity.

Forces that mediate interactions between molecules, including attraction or repulsion between them.

Forces that hold atoms together within a single molecule, such as covalent bonds.

Intermolecular forces act between molecules, while intramolecular forces act within a molecule; intermolecular forces are weaker.

Categories of intermolecular forces include hydrogen bonding, ionic bonding, dipole-dipole interactions, and van der Waals forces.

Covalent bonds and hydrogen bonding within a molecule represent examples of intramolecular forces.