Pharmaceutical Organic Chemistry I PC101 Quiz

In the ground state of an atom or ion, electrons fill subshells of the lowest available energy first, then higher energy subshells.

An atom that forms one chemical bond.

Carbon forms four covalent bonds.

A pair of valence electrons that are not shared with another atom.

The arrangement of atoms in a molecule, where lone pairs of electrons on the central atom are not considered.

A molecular geometry with 4 bonding groups, arranged around a central atom at angles of approximately 109.5 degrees.

A molecular geometry with 3 bonding groups, arranged around a central atom at angles of approximately 120 degrees.

A molecular geometry with 2 bonding groups, arranged in a straight line (180 degrees) around a central atom.

Different compounds with the same molecular formula but different structural arrangements.

A visual representation of the arrangement of atoms and bonds in a molecule.

A way to describe the delocalization of pi electrons in a molecule or ion, where bonding cannot be shown by a single structure.

A carbon atom bonded to only one other carbon atom.

A carbon atom bonded to two other carbon atoms.

Weak attractive forces between atoms and molecules.

Attractive forces between the positive and negative ends of polar molecules.

Strong dipole-dipole attraction between a hydrogen atom bonded to a highly electronegative atom (N, O, or F) and another electronegative atom.

Shows the change in a reaction, from reactants to products.

Represents a reversible reaction where products can revert to reactants and vice-versa.

Shows the movement of electrons within a molecule to form different resonance structures.

Short-lived species formed during a reaction, but not a final product.

Electron-deficient species attracted to electron-rich species.

Electron-rich species that donates electrons.

Mixing of atomic orbitals to form new hybrid orbitals.

Mixing of one s and three p atomic orbitals to form four equivalent sp3 hybrid orbitals.

CH4(methane) is an example of sp3 hybridization. Four sigma bonds are created.

A species with a positive charge or positive end of a polar bond that is attracted to electron-rich groups.

Compounds with strong covalent bonds are more stable than those with weaker bonds.

Electron distribution at reaction sites (functional groups) significantly impacts reactions.

A type of electronic effect related to electron shifting.

Another type of electronic effect that depends on resonance structures.

Atoms' spatial arrangement; crowding creates unfavourable 'steric hindrance'.

The difficulty of reactions due to the spatial arrangement of atoms.

The solvent can affect how reactions proceed.

A detailed description of bond changes during a reaction.

In reaction mechanisms, a full head arrow shows a complete electron pair movement.

In reaction mechanisms, a half-headed arrow shows a single electron movement.

When a bond breaks, and each fragment gets one electron.

When a bond breaks, and both electrons go to one fragment.

A species that has a high concentration of electrons

A process in which one or more substances are changed into different substances.

Ethylene's carbon atoms use three hybrid orbitals (sp2) to form bonds, while the remaining unhybridized p-orbital forms a pi bond.

Acetylene's carbon atoms form two sp hybrid orbitals for sigma bonds and two unhybridized p-orbitals for pi bonds.

Bond formed by electrostatic attraction between oppositely charged ions.

Bond formed by sharing electrons between atoms.

Fluorine (atomic no. 9) has 2 electrons in the first shell and 7 in the second shell.

Magnesium Oxide has an ionic bond

A species that accepts an electron pair.

An atom that can form three bonds.

A molecule with a hydrogen atom bonded to a highly electronegative atom (N, O, or F).

180° bond angle, linear. It forms triple bonds.

Carbon typically forms 4 covalent bonds.

Dipole-dipole interactions are the dominant intermolecular forces in dimethyl ether.

Hydrogen bonds form between molecules containing a hydrogen atom bonded to a highly electronegative atom (e.g., oxygen, nitrogen) and another electronegative atom in a separate molecule.

Organic compounds with polar groups (able to form hydrogen bonds) are more soluble in water; nonpolar compounds (no hydrogen bonding capability) are generally insoluble.

The polar, hydrogen-bonding part of a molecule, which interacts favorably with water.

The nonpolar, non-hydrogen-bonding part of a molecule, which tends to avoid interaction with water.

A process where reactants transform into different products.

The substance undergoing change in a chemical reaction.

The resulting substance after a chemical reaction.

Environmental factors affecting the rate and outcome of a chemical reaction (e.g., temperature, pressure, catalysts, solvent).

A substance that speeds up a chemical reaction without being consumed in the process.

A reaction where the number of sigma bonds increases, usually by the conversion of a pi bond to sigma bonds.

A reaction where the number of sigma bonds decreases, often creating a new pi bond.

A reaction where one atom or group is replaced by another.

A reaction that produces an isomer by rearranging atoms or groups within the molecule.

A reaction where a carbon atom loses hydrogen atoms or gains bonds to more electronegative atoms.

A reaction where a carbon atom gains hydrogen atoms or loses bonds to more electronegative atoms.