Chemistry Chapter 2 Quiz

A chart displaying all known chemical elements, organized by their atomic number, electron configuration, and recurring chemical properties.

The number of protons in an atom's nucleus, which determines the element's identity.

The outermost shell of an atom containing electrons involved in chemical bonding.

Groups refer to columns in the periodic table. Elements within a group share similar chemical properties.

Elements that generally lack metallic characteristics, such as conductivity and malleability. They are often found as gases or brittle solids.

Forces that exist between molecules, responsible for holding them together.

A type of intermolecular force that occurs between polar molecules due to their permanent dipoles.

Temporary forces that occur between all molecules, even nonpolar ones, due to temporary dipoles.

The temperature at which a substance transitions from a solid to a liquid.

The temperature at which a substance transitions from a liquid to a gas.

A tiny particle found within atoms, carrying a negative electrical charge. It's constantly moving around the atom's nucleus.

Experiments using cathode ray tubes showed the deflection of these particles by magnets. This led to the discovery of electrons, as they are attracted to positive charges and repelled by negative ones.

Rutherford's experiment involved firing alpha particles at a thin gold foil. Most particles passed through, but some were deflected, indicating a small, dense, positively charged core within the atom. This core is the nucleus.

A subatomic particle found in the nucleus of an atom, carrying a positive electrical charge. It's approximately the same mass as a proton.

A subatomic particle found in the nucleus of an atom, carrying no electrical charge (neutral). Its mass is similar to that of a proton.

The number of protons in an atom's nucleus, defining the element's identity.

Different forms of the same element with the same number of protons but varying numbers of neutrons.

The total number of protons and neutrons in an atom's nucleus.

A symbolic representation of a molecule, showing the types and numbers of atoms that compose it.

A chemical formula representing the ionic bond between potassium (K) and oxygen (O), resulting in a stable compound.

Electron transitions between energy levels within an atom, releasing energy as light, resulting in a unique pattern of colored lines.

A model that describes electrons orbiting the nucleus in fixed energy levels. It explains the discrete lines in atomic spectra for hydrogen, but fails to explain the spectra of other elements.

A visual representation of the arrangement of electrons around an atom, where dots represent the valence electrons.

A type of chemical bond formed when atoms share electrons, forming stable molecules.

A type of chemical bond formed by the electrostatic attraction between oppositely charged ions.

A type of covalent bond forming a continuous, three-dimensional network of atoms without individual molecules, found in materials like diamond.

A chemical bond where electrons are delocalized, free to move throughout a lattice of positively charged metal ions, creating good electrical conductivity.

A substance that does not conduct electricity in its solid state but can conduct electricity when dissolved in a liquid or melted.

A specific arrangement of electrons in different energy levels within an atom, represented by a sequence of numbers and letters.

The outermost shell of an atom that contains electrons involved in chemical bonding. These electrons are the most reactive and determine how an atom will bond with other atoms.

It's a weighted average of the masses of all the isotopes of an element, taking into account their relative abundance.

When excited electrons in an atom return to their ground state, they release energy in the form of light, creating a unique spectral pattern for each element.

A system for naming chemical compounds based on their composition and oxidation states. It involves determining the oxidation numbers of the elements and writing a formula that reflects the compound's structure.

A diagram that shows the arrangement of valence electrons in a molecule. Valence electrons are represented by dots around the symbol of each atom.

A strong covalent network structure where each carbon atom is bonded to four other carbon atoms in a three-dimensional arrangement. This results in high hardness, high melting point, and poor electrical conductivity.

A layered structure held together by weak intermolecular forces. Each layer consists of carbon atoms bonded in hexagonal rings. This arrangement results in high electrical conductivity and slipperiness.

A regular, repeating arrangement of ions in a solid crystal structure. The positive and negative ions are held together by electrostatic attraction.

The tendency of metals to lose electrons due to their low electronegativity. This characteristic leads to the formation of positively charged ions (cations) and contributes to their ability to conduct electricity.

A type of intermolecular force that occurs when a hydrogen atom is bonded to a highly electronegative atom (like F, O, or N) and is attracted to an electron pair on another nearby atom.

The ability of an atom to attract electrons towards itself in a chemical bond. Higher electronegativity means a stronger pull.

Dalton proposed that atoms are the fundamental, indivisible building blocks of matter. He suggested that atoms of a given element are identical and that chemical reactions involve the rearrangement of atoms.

Thomson discovered electrons using cathode ray experiments. He envisioned a model where electrons are embedded within a positively charged sphere, similar to plums within a pudding.

Rutherford conducted the gold foil experiment, which involved firing alpha particles at a thin gold foil. Most particles passed through, but some were deflected, revealing a dense, positively charged nucleus at the atom's center.

Chadwick discovered neutrons, which are neutral particles residing in the atom's nucleus. This discovery refined our understanding of atomic structure, adding neutrons alongside protons.

Millikan's oil drop experiment determined the charge of an electron, a fundamental discovery in understanding the electrical nature of matter. It established the electron's charge as a fundamental unit.