Organic Chemistry Basics Quiz

Compounds primarily composed of carbon, hydrogen, and oxygen.

Compounds typically made of atoms other than carbon. They often have strong bonds between atoms.

The type of bond found in organic compounds, usually formed between carbon and hydrogen.

The type of bond often found in inorganic compounds, with atoms losing or gaining electrons.

Organic compounds tend to have weaker bonds and easily break apart, leading to low melting and boiling points.

Organic compounds typically don't dissolve well in water.

Most inorganic compounds are good at conducting electricity due to the presence of metal atoms.

A theory that stated organic compounds could only be produced by living organisms due to a mysterious vital force.

A German chemist who disproved the Vital Force Theory by synthesizing urea from an inorganic compound.

The ability of carbon atoms to bond together in chains or rings of various sizes, leading to a wide variety of organic molecules.

A compound with the chemical formula NaCl, commonly known as table salt.

A compound with the chemical formula CH4, the simplest alkane and the main component of natural gas.

A compound with the chemical formula C6H6, a colorless liquid that is a key ingredient in plastics and paints.

A compound with the chemical formula CH3OH, commonly known as wood alcohol.

A bond formed between an ion (charged atom) and a polar molecule (with uneven electron distribution, creating a positive and negative end).

An interaction between an ion and a non-polar molecule (with even electron distribution). The ion induces temporary polarity in the non-polar molecule.

A weak bond between two non-polar molecules, arising from temporary fluctuations in electron distribution, creating temporary dipoles.

A weak bond between a polar molecule and a non-polar molecule. The permanent dipole in the polar molecule induces a temporary dipole in the non-polar molecule.

A weak bond between two polar molecules. The permanent dipoles of the molecules attract each other.

The collective term for weak interactions between molecules, including London Dispersion, Debye Induction, and Keesom Orientation Forces.

A molecule with an uneven distribution of electrons, leading to a positive and a negative end.

A molecule with an even distribution of electrons, lacking any distinct positive or negative ends.

An atom with an imbalance of protons and electrons, resulting in a net positive or negative charge.

The attraction between molecules, weaker than the bonds that hold atoms together within a molecule.

Valence electrons are the outermost electrons in an atom, which participate in chemical bonding.

A theory explaining how chemical bonds form between atoms by sharing electrons through overlapping atomic orbitals.

The Lewis Structure is a diagram that shows the arrangement of electrons around atoms in a molecule, using dots or lines to represent electrons.

Regions in an atom where electrons are most likely to be found.

Hybridization is the process where atomic orbitals mix to form new hybrid orbitals, which are more stable and suitable for bonding.

A new orbital formed when atomic orbitals overlap during bond formation, containing two electrons.

The degree of overlap between atomic orbitals, with greater overlap resulting in stronger bonds.

A sigma bond is a single covalent bond formed by the direct overlap of atomic orbitals along the internuclear axis.

A pi bond is a covalent bond formed by the lateral overlap of atomic orbitals above and below the internuclear axis.

A type of covalent bond formed by the head-on overlap of atomic orbitals, resulting in a strong and longer bond.

A type of covalent bond formed by the sideways overlap of atomic orbitals, resulting in a weaker and shorter bond.

The process of combining atomic orbitals to form new hybrid orbitals, leading to stronger bonds.

The first bond to form between atoms, often a sigma bond.

A type of bond formed when two atoms share two pairs of electrons, resulting in a stronger bond than a single bond.

A type of bond formed when two atoms share three pairs of electrons, resulting in a stronger bond than a single or double bond.