Notes in Chemistry

To Subscribe, use this Key

Status	Last Update	Fields
Published	11/14/2024	{{c1::Pure substances}} contain only one chemical species, either an element or a compound.
Published	11/14/2024	An {{c1::element}} cannot be separated into simpler substances by chemical means.
Published	11/14/2024	{{c1::Compounds}} consist of two or more chemically bonded elements that can be separated by chemical means.
Published	11/14/2024	Atoms consist of a nucleus with positively charged {{c1::protons}} and neutral {{c1::neutrons}} surrounded by negatively charged {{c1::electrons}}.
Published	11/14/2024	The number of {{c1::protons}} in the nucleus defines the elemental identity of the atom.
Published	11/14/2024	Atoms of the same element can have different numbers of {{c1::neutrons}}, forming isotopes.
Published	11/14/2024	The atomic number refers to the number of {{c1::protons}} in an atom's nucleus.
Published	11/14/2024	The mass number of an atom is the sum of the {{c1::protons}} and {{c1::neutrons}} in the nucleus.
Published	11/14/2024	An atom is electrically neutral when the number of protons equals the number of {{c1::electrons}}.
Published	11/14/2024	Atoms that gain electrons form {{c1::negatively charged ions}}.
Published	11/14/2024	Atoms that lose electrons form {{c1::positively charged ions}}.
Published	11/14/2024	{{c1::Isotopes}} are atoms of the same element that have different numbers of neutrons in their nuclei.
Published	11/14/2024	Isotopes are identified by their {{c1::mass number}}, which is the sum of protons and neutrons.
Published	11/14/2024	The {{c1::natural abundance}} of each isotope is the percentage of that isotope found in an average sample of the element.
Published	11/14/2024	The distribution of isotopes can be determined using {{c1::mass spectrometry}}.
Published	11/14/2024	Isotopes of the same element have nearly identical {{c1::chemical properties}} because they share the same electron configuration.
Published	11/14/2024	Lab measurements use atomic mass, which is {{c1::an average of isotope masses weighted by their natural abundance}}.
Published	11/14/2024	The atomic mass of this element is {{c1::65.38}}
Published	11/14/2024	The {{c1::strong nuclear force}} holds nucleons (protons and neutrons) together in the nucleus.
Published	11/14/2024	The {{c1::n/p ratio}} determines the stability of a nucleus, and a stable nucleus typically has a ratio close to 1.
Published	11/14/2024	During {{c1::alpha decay}}, a nucleus ejects a particle made of 2 protons and 2 neutrons.
Published	11/14/2024	After alpha decay, the new nucleus has an atomic number that is {{c1::2 units less}} than the original nucleus.
Published	11/14/2024	{{c1::Alpha particles}} are the least energetic and most massive type of radioactive emission.
Published	11/14/2024	In beta decay, the {{c1::mass number}} remains unchanged, but the {{c1::atomic number}} either increases or decreases by 1.
Published	11/14/2024	In {{c1::β⁻ decay}}, a neutron converts to a proton and ejects a high-speed electron and an antineutrino.
Published	11/14/2024	In {{c1::positron emission (β⁺ decay)}}, a proton converts to a neutron and ejects a positron and a neutrino.
Published	11/14/2024	In β⁺ decay, the atomic number {{c1::decreases by 1 unit}}, while the mass number {{c1::remains the same}}.
Published	11/14/2024	In {{c1::electron capture}}, a proton captures an orbiting electron and converts into a neutron.
Published	11/14/2024	Electron capture {{c1::decreases::decreases/increases}} the atomic number by {{c1::1 unit}} while the {{c1::mass number}} remains unchanged.
Published	11/14/2024	During {{c1::gamma decay}}, an unstable nucleus releases excess energy in the form of a gamma ray.
Published	11/14/2024	In gamma emission, the number of protons and neutrons in the nucleus {{c1::remains unchanged}}.
Published	11/14/2024	The {{c1::half-life}} of a radioisotope is the time required for half of a sample to decay.
Published	11/14/2024	The fraction of radioisotope remaining after n half-lives is calculated as {{c1::1/2ⁿ}}.
Published	11/14/2024	The {{c1::activity}} of a radioisotope refers to the number of decay events per unit of time and can be calculated as {{c1::1/2ⁿ × Initial activi…
Published	11/14/2024	The SI unit for measuring radioactive activity is the {{c1::becquerel (Bq)}}, defined as {{c1::1 decay per second}}.
Published	11/14/2024	Electrons are organized within {{c1::specific shells and subshells}} according to their energy levels.
Published	11/14/2024	In the Bohr model, electrons move around the nucleus in {{c1::fixed circular orbits}} or shells.
Published	11/14/2024	In the Bohr model, electrons farther from the nucleus have {{c1::higher::lower/higher}} energy compared to those closer to the nucleus.
Published	11/14/2024	In the Bohr model, electrons can move to higher orbits by {{c1::absorbing energy}}, such as heat or light.
Published	11/14/2024	In the Bohr model, electrons return to a lower orbit by {{c1::emitting energy in the form of a photon}}.
Published	11/14/2024	In the Bohr model, the energy absorbed or emitted by an electron must {{c1::match the energy difference between two orbits}}.
Published	11/14/2024	Electromagnetic radiation consists of {{c1::photons}}, which are discrete packets of energy.
Published	11/14/2024	The energy of a photon (E) is directly proportional to its {{c1::frequency (v)}} and inversely proportional to its {{c1::wavelength (λ)}}.
Published	11/14/2024	Longer wavelengths correspond to {{c1::lower::lower/higher}} frequencies and {{c1::lower::lower/higher}} energy.
Published	11/14/2024	Only photons with certain {{c1::specific wavelengths}} are absorbed or emitted by atoms.
Published	11/14/2024	Electrons around an atom typically exist in the {{c1::ground state}}, the lowest allowed energy level.
Published	11/14/2024	An electron transitions to an {{c1::excited}} state by absorbing a photon of energy.
Published	11/14/2024	The Bohr model did not fully describe the behavior of atoms with more than {{c1::one electron}} because it did not account for {{c1::electron repulsio…
Published	11/14/2024	The {{c1::Heisenberg uncertainty principle}} states that it is impossible to know both the position and momentum of an electron at the same time.
Published	11/14/2024	The uncertainties in position and momentum are {{c1::inversely proportional}}
Published	11/14/2024	The allowed values for the principal quantum number (n) are {{c1::1, 2, 3, 4…}}.
Published	11/14/2024	The angular momentum quantum number (ℓ) can have values from {{c1::0}} to {{c1::n - 1}}.
Published	11/14/2024	The magnetic quantum number (mₗ) can have values between {{c1::-ℓ}} and {{c1::+ℓ}}.
Published	11/14/2024	The allowed values for the spin quantum number (mₛ) are {{c1::+½}} or {{c1::-½}}.
Published	11/14/2024	The angular momentum quantum number (ℓ) for a p orbital is {{c1::1}} and corresponds to a {{c1::dumbbell-shaped}} orbital.
Published	11/14/2024	A d subshell (ℓ = 2) contains {{c1::5}} orbitals and can hold a maximum of {{c1::10}} electrons.
Published	11/14/2024	The maximum number of electrons in a shell is given by the equation {{c1::2n²}}.
Published	11/14/2024	The {{c1::principal (n)}} quantum number  describes the main energy level (shell) of an electron and its most probable distance from the nucleus.
Published	11/14/2024	The {{c1::angular momentum (ℓ)}} quantum number corresponds to the subshell type (s, p, d, f) and determines the orbital shape.
Published	11/14/2024	The {{c1::magnetic (mₗ)}} quantum number  specifies the three-dimensional orientation of an orbital within a subshell.
Published	11/14/2024	The {{c1::electron spin (mₛ)}} quantum number  describes the intrinsic angular momentum (spin) of an electron, with possible values of +½ (spin u…
Published	11/14/2024	An s subshell contains {{c1::1}} orbital that can hold a maximum of {{c1::2}} electrons.
Published	11/14/2024	The {{c1::Pauli exclusion principle}} states that no two electrons in an atom can have the same set of four quantum numbers.
Published	11/14/2024	According to the Pauli exclusion principle, each orbital can hold a maximum of {{c1::two electrons}} with {{c1::opposite spins}}.
Published	11/14/2024	The {{c1::Aufbau principle}} states that electrons fill lower energy levels before occupying higher ones.
Published	11/14/2024	In electron configurations, the outermost shell with the highest {{c1::principal quantum number (n)}} contains the valence electrons.
Published	11/14/2024	Elements in the same column of the periodic table have the same number of {{c1::valence electrons}}, which determine their {{c1::chemical properties}}…
Published	11/14/2024	Half-filled and completely filled orbitals are more {{c1::stable}} than unevenly filled orbitals.
Published	11/14/2024	What is the electron configuration of Selenium and how many valence electrons does it have? 1s22s22p63s23p64s2{{c1::3d104p4}} It has {{c1::6}} valence…
Published	11/14/2024	What is the electron configuration of Cr? 1s22s22p63s23p6{{c1::4s13d5}}
Published	11/14/2024	What is the electron configuration of Cu? 1s22s22p63s23p6{{c1::4s13d10}}
Published	11/14/2024	Electron configuration of Se2-? 1s22s22p63s23p64s2{{c1::3d104p6}}
Published	11/14/2024	According to {{c1::Hund's rule}}, electrons fill orbitals to maximize the number of unpaired electrons within a sublevel.
Published	11/14/2024	If an atom has all paired electrons, it is classified as {{c1::diamagnetic}} and is {{c1::repelled}} by an external magnetic field.
Published	11/14/2024	If an atom has unpaired electrons, it is classified as {{c1::paramagnetic}} and is {{c1::attracted}} to an external magnetic field.
Published	11/14/2024	Metals are located to the {{c1::left::left/right}} of the zigzag line on the periodic table, and nonmetals are located to the {{c1::right::left/right}…
Published	11/14/2024	Metals are generally {{c1::shiny, ductile, and good conductors}} of heat and electricity.
Published	11/14/2024	Nonmetals are generally {{c1::dull, brittle, and poor}} electrical conductors.
Published	11/14/2024	{{c1::Metalloids}} share properties of both metals and nonmetals and are often {{c1::semiconductors}}.
Published	11/14/2024	The {{c1::representative elements}} include Groups 1-2 and Groups 13-18 and are located in the {{c1::s-block and p-block}}.
Published	11/14/2024	The {{c1::transition metals}} include Groups 3-12 and occupy the {{c1::d-block}} of the periodic table.
Published	11/14/2024	Seven elements exist as diatomic molecules in their standard state: {{c1::H₂, N₂, O₂, F₂, Cl₂, Br₂, and I₂}}.
Published	11/14/2024	At room temperature, {{c1::bromine}} is a liquid and {{c1::iodine}} is a solid, while the {{c1::other}} diatomic elements are gases.
Published	11/14/2024	{{c1::Alkali metals}} are highly reactive and easily donate their single valence electron to form strong ionic bonds.
Published	11/14/2024	{{c1::Alkaline-earth metals}} (Group 2) have two valence electrons (ns²) and form cations with a +2 charge.
Published	11/14/2024	{{c1::Transition metals}} (Groups 3-12) can lose varying numbers of valence electrons from their {{c1::s and d}} orbitals to form cations wi…
Published	11/14/2024	Transition metals often form compounds that produce {{c1::colorful}} solutions.
Published	11/14/2024	{{c1::Chalcogens}} (Group 16) have six valence electrons (ns²np⁴) and tend to gain two electrons, forming an anion with a −2 charge.
Published	11/14/2024	{{c1::Halogens}} (Group 17) have seven valence electrons (ns²np⁵) and tend to gain one electron, forming an anion with a −1 charge.
Published	11/14/2024	{{c1::Noble gases}} (Group 18) have full s and p orbitals (ns²np⁶) in their valence shell and are {{c1::inert}}.
Published	11/14/2024	Electron configuration of Ga3+? 1s22s22p63s23p6{{c1::3d10}}. Given, the electron configuration of Ga is 1s22s22p63s23p64s2d104p1.
Published	11/14/2024	Core electrons introduce a {{c1::shielding constant (S)}} that reduces the attraction of the nuclear charge on valence electrons.
Published	11/14/2024	Due to the shielding effect of core electrons, valence electrons experience an effective nuclear charge (Zeff) that is {{c1::less::less/more}} than th…
Published	11/14/2024	Effective nuclear charge Zeff {{c1::increases::decreases/increases}} across a period (left to right).
Published	11/14/2024	Down a group, Zeff generally {{c1::increases slightly::decreases/increases}}.
Published	11/14/2024	The atomic radius {{c1::increases::decreases/increases}} down a group.
Published	11/14/2024	The atomic radius {{c1::decreases::decreases/increases}} across a period.
Published	11/14/2024	The {{c1::ionic radius}} measures the size of atoms that have gained or lost electrons and acquired a net charge.
Published	11/14/2024	Compared to a neutral atom, a cation is {{c1::smaller::smaller/larger}} because it often loses its outer shell and experiences less electron repulsion…
Published	11/14/2024	Compared to a neutral atom, an anion is {{c1::larger::smaller/larger}} because adding electrons increases repulsion and pushes electrons farther from …
Published	11/14/2024	Isoelectronic ions have the same number of electrons but different {{c1::numbers of protons}}, resulting in different {{c1::effective nuclear charges}…
Published	11/14/2024	In an isoelectronic series, ionic radii {{c1::decreases::decreases/increases}} as atomic number increases due to increasing effective nuclear charge (…
Published	11/14/2024	{{c1::Electronegativity}} measures how strongly an atom attracts valence electrons within a chemical bond.
Published	11/14/2024	Electronegativity {{c1::increases::decreases/increases}} from left to right across a period and from {{c1::decreases::decreases/increases}} top to bot…
Published	11/14/2024	Electronegativity values are typically reported on the Pauling scale, which ranges from {{c1::0 to 4}}.
Published	11/14/2024	{{c1::Electron affinity}} measures how readily a neutral atom accepts an additional electron.
Published	11/14/2024	When a stable anion is formed, electron affinity is {{c1::negative}} because energy is released (exothermic).
Published	11/14/2024	If an unstable anion is formed, electron affinity is {{c1::positive}} because energy is required (endothermic) to add an electron.
Published	11/14/2024	Electron affinity becomes {{c1::more negative}} from left to right across a period, with some exceptions.
Published	11/14/2024	Electron affinity becomes {{c1::less negative}} down a group because added electrons experience {{c1::weaker nuclear attraction}}.
Published	11/14/2024	Small atoms like oxygen and fluorine have greater electron-electron repulsion, which makes adding another electron {{c1::less::less/more}} favorable.
Published	11/14/2024	Noble gases (Group 18) have {{c1::nearly zero}} electron affinity because {{c1::they already have a full valence shell}}.
Published	11/14/2024	{{c1::Ionization energy}} is the minimum energy required to remove an electron from a neutral atom or ion in the gas state.
Published	11/14/2024	The {{c1::first ionization energy}} refers to the removal of the most loosely bound valence electron to form a +1 cation.
Published	11/14/2024	Ionization energy {{c1::increases::decreases/increases}} with greater effective nuclear charge (Zeff) because the electrostatic force pulls electrons …
Published	11/14/2024	Ionization energy {{c1::decreases::decreases/increases}} as atomic radius increases because electrons farther from the nucleus are held less tightly.
Published	11/14/2024	The first ionization energy generally {{c1::increases::decreases/increases}} across a period and {{c1::decreases::decreases/increases}} down a gr…
Published	11/14/2024	The prefix kilo (k) corresponds to 10^{{c1::3}}.
Published	11/14/2024	The prefix milli (m) corresponds to 10^{{c1::-3}}.
Published	11/14/2024	The prefix micro (μ) corresponds to 10^{{c1::-6}}.
Published	11/14/2024	The prefix nano (n) corresponds to 10^{{c1::-9}}.
Published	11/14/2024	The prefix pico (p) corresponds to 10^{{c1::-12}}.
Published	11/14/2024	The SI unit for length is the {{c1::meter}} ({{c1::m}}).
Published	11/14/2024	The SI unit for mass is the {{c1::kilogram}} ({{c1::kg}}).
Published	11/14/2024	The SI unit for time is the {{c1::second}} ({{c1::s}}).
Published	11/14/2024	The SI unit for temperature is the {{c1::kelvin}} ({{c1::K}}).
Published	11/14/2024	The SI unit for electric current is the {{c1::ampere}} ({{c1::A}}).
Published	11/14/2024	The SI unit for the amount of substance is the {{c1::mole}} ({{c1::mol}}).
Published	11/14/2024	The SI unit for luminous intensity is the {{c1::candela}} ({{c1::cd}}).
Published	11/14/2024	The equation for density is density ρ of a substance is defined as the {{c1::mass m it contains per unit of volume V}}. The SI unit of density is {{c…
Published	11/14/2024	the composition of a mixture can be expressed in terms of its molarity, which has the equation {{c1::M = mol/L}}.
Published	11/14/2024	The density (ρ) of a substance is defined as the {{c1::mass}} (m) per unit of {{c1::volume}} (V) it occupies.
Published	11/14/2024	Density can vary slightly with {{c1::temperature}} because materials tend to expand when heated and contract when cooled.
Published	11/14/2024	if a sample contains 2.0 mol of H3PO4, how many moles of H are in the sample? {{c1::6}}
Published	11/14/2024	The law of definite proportions states that the {{c1::mass ratio}} of atoms in a compound is {{c1::constant}} regardless of how the compound is obtain…
Published	11/14/2024	An {{c1::empirical formula}} gives the lowest whole-number ratio of atoms of each unique element in a compound.
Published	11/14/2024	A {{c1::molecular formula}} lists the actual number of atoms of each element in one molecule of a compound.
Published	11/14/2024	The mass of a single atom in amu numerically matches its {{c1::molar mass}} in grams per mole (g/mol).
Published	11/14/2024	Lewis symbols use dots around an element’s chemical symbol to represent its {{c1::valence electrons}}.
Published	11/14/2024	The octet rule states that atoms react by gaining, losing, or sharing electrons to achieve a {{c1::full outer shell}} of electrons.
Published	11/14/2024	A large difference in electronegativity between two atoms results in the formation of an {{c1::ionic}} bond.
Published	11/14/2024	A small or moderate difference in electronegativity between atoms leads to the formation of a {{c1::covalent}} bond.
Published	11/14/2024	{{c1::Hydrogen}} and {{c1::helium}} are exceptions to the octet rule because they can have a full outer shell with only 2 electrons.
Published	11/14/2024	Electron-deficient species like {{c1::beryllium}} and {{c1::boron}} can form stable compounds with fewer than 8 valence electrons.
Published	11/14/2024	Atoms in Period 3 and beyond can be {{c1::hypervalent}} and have more than 8 electrons in their valence shell.
Published	11/14/2024	Species with an {{c1::odd}} number of electrons, such as free radicals, cannot follow the octet rule.
Published	11/14/2024	Atoms that lose electrons form {{c1::cations}} (positively charged ions), and atoms that gain electrons form {{c1::anions}} (negatively charged ions).
Published	11/14/2024	In ionic bonds, the oppositely charged ions assemble in ratios that give a formula unit with a {{c1::net charge of zero}}.
Published	11/14/2024	Ionic bond lengths can be estimated as the sum of the {{c1::ionic radii}} of the joined ions.
Published	11/14/2024	Dissolved {{c1::ionic}} compounds conduct electricity because they dissociate into freely moving, charged ions, making them {{c1::electrolytes}}.
Published	11/14/2024	A {{c1::covalent bond}} is formed when two atoms share two or more valence electrons to achieve full valence shells.
Published	11/14/2024	Covalent bonds are formed because nonmetal atoms are energetically {{c1::unfavorable to lose electrons}} and have a small difference in {{c1::electron…
Published	11/14/2024	The shared pair of electrons between two atoms in a covalent bond is called {{c1::bonding electrons}}.
Published	11/14/2024	Covalent bond lengths can be approximated as the sum of the {{c1::atomic radii}} of the bonded atoms.
Published	11/14/2024	Molecular compounds are typically not electrically conductive in water because the molecules are {{c1::uncharged}} and the bonding electrons are {{c1:…
Published	11/14/2024	Covalent bonds formed by the end-to-end overlap of atomic orbitals are called {{c1::sigma (σ) bonds}}.
Published	11/14/2024	Covalent bonds formed by the side-to-side overlap of p orbitals are called {{c1::pi (π) bonds}}.
Published	11/14/2024	Pi (π) bonds are {{c1::more::less/more}} rigid than sigma (σ) bonds due to the lack of free rotation.
Published	11/14/2024	Bond length decreases as {{c1::bond order}} increases because more bonds pull the atoms closer together.
Published	11/14/2024	Bond dissociation energy is the amount of energy required to {{c1::break a covalent bond}} and separate the bonded atoms.
Published	11/14/2024	Pi (π) bonds require {{c1::less::less/more}} energy to break than sigma (σ) bonds because their {{c1::side-to-side overlap}} is less efficient.
Published	11/14/2024	Increasing the {{c1::bond order}} (number of bonds) increases the bond dissociation energy.
Published	11/14/2024	A coordinate covalent bond is formed when a pair of nonbonding electrons from a {{c1::ligand}} is shared with a {{c1::metal cation}}.
Published	11/14/2024	The ensemble of a metal cation and its associated ligands is called a {{c1::coordination complex}}.
Published	11/14/2024	In a coordinate covalent bond, the electrons are {{c1::donated}} by the ligand but shared with the {{c1::metal cation}}.
Published	11/14/2024	The process in which a ligand and its electrons "unplug" from a coordination complex and are replaced by another ligand is called {{c1::liga…
Published	11/14/2024	The coordination number of a coordination complex is the number of {{c1::coordinate covalent bonds formed between the central metal ion and its neighb…
Published	11/14/2024	A ligand that forms two or more coordinate covalent bonds is called a {{c1::chelate}}.
Published	11/14/2024	{{c1::Denticity}} refers to how many atoms in a ligand can "bite" the metal cation (eg, a bidentate ligand forms two bonds).
Published	11/14/2024	The net charge of a coordination complex is equal to the sum of the charges of the {{c1::cation}} and its {{c1::ligands}}.
Published	11/14/2024	When the ligands in a coordination complex are neutral or don't fully counter the charge of the cation, the complex is called a {{c1::complex ion}}.
Published	11/14/2024	Lewis structures use dots to represent {{c1::covalent bonds}} and the bonding configuration of atoms in a molecule.
Published	11/14/2024	The sum of the {{c1::formal charges}} in a Lewis structure must equal the {{c1::net charge}} of the chemical formula.
Published	11/14/2024	Polyatomic ions are groups of two or more covalently bonded atoms that have a {{c1::net charge}}.
Published	11/14/2024	{{c1::Resonance}} occurs when some electrons in a molecule can adopt more than one valid bonding configuration, making the structure delocalized.
Published	11/14/2024	The most stable resonance contributor has the fewest {{c1::formal charges}} and places any negative charges on the {{c1::more electronegative atoms}}.
Published	11/14/2024	{{c1::Conjugation}} refers to a sequence of three or more adjacent {{c1::p orbitals}} that function as a single, continuous network for delocalized el…
Published	11/14/2024	The formula for {{c1::dimercury}} is {{c2::Hg₂²⁺}}.
Published	11/14/2024	The formula for {{c1::ammonium}} is {{c2::NH₄⁺}}.
Published	11/14/2024	The formula for {{c1::acetate}} is {{c2::CH₃COO⁻}}.
Published	11/14/2024	The formula for {{c1::bromate}} is {{c2::BrO₃⁻}}.
Published	11/14/2024	The formula for {{c1::hydroxide}} is {{c2::OH⁻}}.
Published	11/14/2024	The formula for {{c1::cyanide}} is {{c2::CN⁻}}.
Published	11/14/2024	The formula for {{c1::thiocyanate}} is {{c2::SCN⁻}}.
Published	11/14/2024	The formula for {{c1::permanganate}} is {{c2::MnO₄⁻}}.
Published	11/14/2024	The formula for {{c1::perchlorate}} is {{c2::ClO₄⁻}}.
Published	11/14/2024	The formula for {{c1::chlorate}} is {{c2::ClO₃⁻}}.
Published	11/14/2024	The formula for {{c1::chlorite}} is {{c2::ClO₂⁻}}.
Published	11/14/2024	The formula for {{c1::hypochlorite}} is {{c2::ClO⁻}}.
Published	11/14/2024	The formula for {{c1::dihydrogen phosphate}} is {{c2::H₂PO₄⁻}}.
Published	11/14/2024	The formula for {{c1::hydrogen carbonate}} is {{c2::HCO₃⁻}}.
Published	11/14/2024	The formula for {{c1::hydrogen sulfate}} is {{c2::HSO₄⁻}}.
Published	11/14/2024	The formula for {{c1::nitrate}} is {{c2::NO₃⁻}}.
Published	11/14/2024	The formula for {{c1::nitrite}} is {{c2::NO₂⁻}}.
Published	11/14/2024	The formula for {{c1::hydrogen phosphate}} is {{c2::HPO₄²⁻}}.
Published	11/14/2024	The formula for {{c1::carbonate}} is {{c2::CO₃²⁻}}.
Published	11/14/2024	The formula for {{c1::sulfate}} is {{c2::SO₄²⁻}}.
Published	11/14/2024	The formula for {{c1::sulfite}} is {{c2::SO₃²⁻}}.
Published	11/14/2024	The formula for {{c1::dichromate}} is {{c2::Cr₂O₇²⁻}}.
Published	11/14/2024	The formula for {{c1::phosphate}} is {{c2::PO₄³⁻}}.
Status	Last Update	Fields