Chemistry Chapter: Atomic Structure and Elements

A chemical compound formed from nonmetallic elements. Their bonds are typically covalent, meaning they share electrons.

A chemical compound formed when a metal reacts with a nonmetal. The metal typically loses electrons, forming a positive ion, and the nonmetal gains electrons, forming a negative ion.

A formula that indicates the kinds and relative numbers of atoms present in a molecule of a substance.

The simplest whole-number ratio of atoms of each element present in a compound.

A compound that contains carbon and hydrogen, often combined with other elements such as oxygen, nitrogen, sulfur, phosphorus, and halogens.

A compound that does not contain carbon.

A compound that contains a metal and a nonmetal. The metal typically forms a positive ion, and the nonmetal forms a negative ion.

A compound of oxygen with another element where oxygen is in -2 oxidation state.

A compound that contains hydrogen and oxygen.

A compound that dissolves in water to produce hydrogen ions (H+)

A set of three quantum numbers (n, l, ml) that uniquely describes the state of an electron in an atom.

The value 'n' of a quantum number set (n, l, ml) represents the principle quantum number.

The value 'l' of a quantum number set (n, l, ml) represents the angular momentum quantum number.

The value 'ml' of a quantum number set (n, l, ml) represents the magnetic quantum number.

The maximum number of electrons that can occupy a subshell is determined by the specific subshell.

The modern periodic table organizes elements by increasing atomic number.

Elements within the same group (vertical column) of the periodic table share similar chemical properties.

Atomic radius is the distance from the nucleus of an atom to its outermost electron.

Atomic radius generally increases moving down a group in the periodic table.

Atomic radius generally decreases across a period in the periodic table.

The ability of an atom in a gaseous state to lose an electron and become a positively charged ion. It is always endothermic - energy must be absorbed from the surroundings to remove the electron.

The energy required to remove one electron from a singly charged positive ion in its gaseous state.

A measure of the tendency of an atom to attract electrons to itself in a chemical bond.

The tendency of an element to lose electrons and form positive ions.

The principle stating that atoms tend to gain or lose electrons to achieve a stable electron configuration, usually with eight valence electrons like noble gases.

A representation of an atom's valence electrons using dots around its symbol.

A representation of a molecule showing the bonding and nonbonding electrons as dots or lines.

The electrons that occupy the outermost energy level of an atom and participate in chemical bonding.

A chemical bond formed by the sharing of electron pairs between atoms.

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

The center of an atom, containing protons and neutrons.

Potassium is a metal due to its tendency to lose electrons, while chlorine is a nonmetal due to its tendency to gain electrons.

Aluminum forms a +3 cation (Al3+) and sulfur forms a -2 anion (S2-), leading to the empirical formula Al2S3.

The correct name for SrO is strontium oxide, following the naming rules for ionic compounds.

PCl3 is named phosphorus trichloride, indicating three chlorine atoms bonded to a phosphorus atom.

Ammonium carbonate has the formula (NH4)2CO3, as ammonium is a polyatomic cation and carbonate is a polyatomic anion.

CrCl3 is named chromium (III) chloride, with the Roman numeral indicating chromium's +3 charge.

Electrons are the smallest and lightest subatomic particles, being negatively charged and orbiting the nucleus.

An atom of 40Ar has 18 electrons, 18 protons, and 22 neutrons (40 - 18 = 22).

Isotopes are atoms of the same element with the same number of protons but differing numbers of neutrons.