chem chapter 3

Ionic Compounds

Compounds formed from the electrostatic attraction between oppositely charged ions.

Molecular Compounds

Compounds formed when two or more nonmetals share electrons to form covalent bonds.

Prefixes in Molecular Naming

Prefix used to indicate the number of atoms; for example, 'tri-' stands for three.

Binary Acids

Acids that consist of hydrogen and one other element, typically a nonmetal.

Oxoacids

Acids that contain hydrogen, oxygen, and another element, typically a polyatomic ion.

Hydroiodic Acid

The name for HI when it is dissolved in water, derived from iodine.

Phosphoric Acid

The acid derived from the phosphate ion, H3PO4.

Molar Mass

The mass of one mole of a substance, usually expressed in grams per mole.

Percentage Composition

The percentage by mass of each element in a compound.

Subscript in Chemical Formulas

Indicates the number of atoms of an element in a molecule.

Molecular Formula for Sodium Phosphate

Na3PO4, a compound that contains sodium, phosphorus, and oxygen.

Water's Chemical Name

H2O, commonly known as water, which is sometimes referred to in relation to acids as hydroxylic acid.

Carbonic Acid

The acid formed from carbon dioxide dissolved in water, represented as H2CO3.

Diatomic Molecule

A molecule composed of only two atoms, which can be of the same or different chemical elements.

Determining Grams from Moles

The process of converting moles of a compound to grams using its molar mass.

Acid Strength

Typically, the strength of an acid increases with the number of oxygen atoms in its structure.

Empirical Formula

A formula that shows the simplest whole-number ratio of elements in a compound.

Hydrochloric Acid

The name for HCl when it is dissolved in water.

Sulfate Ion

The polyatomic ion SO4^(2-), which is associated with sulfuric acid.

Covalent Bonds

Chemical bonds formed by the sharing of electron pairs between atoms.

Ionization Energy

The energy required to remove an electron from an atom or ion.

Electronegativity

A measure of an atom's ability to attract and hold onto electrons.

Polyatomic Ions

Ions that consist of two or more atoms bonded together, which carry a charge.

Sodium Chloride

An ionic compound commonly known as table salt, with the formula NaCl.

Hydrogen Bonding

A weak attraction between a hydrogen atom bonded to an electronegative atom and another electronegative atom.

Balancing Chemical Equations

The process of making sure that the number of atoms for each element is the same on both sides of a chemical equation.

Chemical Reaction Types

Different classifications of chemical reactions, including synthesis, decomposition, single-replacement, and double-replacement.

Phase Changes

Transitions between solid, liquid, and gas phases, such as melting, freezing, boiling, and condensation.

Molecular Geometry

The three-dimensional arrangement of atoms in a molecule, which affects its physical and chemical properties.

Crisscross Method

A technique used to determine the subscripts in a chemical formula by taking the charge of one ion as the subscript for the other.

Polyatomic Ions

Ions composed of two or more atoms, which can carry a charge.

Hydrate

A compound that includes water molecules within its structure.

Suffix Change to -ide

The change made to the name of a nonmetal after a compound forms; for example, nitrogen becomes nitride.

Common Denominator

A number that can be evenly divided by each of the subscripts in a chemical formula.

Roman Numerals in Naming

Indicate the charge of transition metals in compounds when they can have multiple oxidation states.

Nitrate

A polyatomic ion with the formula NO3-.

Calcium Hydroxide

A compound formed when calcium combines with hydroxide; often requires parentheses in its formula to denote the two hydroxide ions.

Chemical Formula for Hydrate

Typically written with a dot separating the compound from the water; representing water of crystallization.

Iron (II) Phosphate

A compound composed of iron with a +2 charge and phosphate (PO4) with a -3 charge.

Compound

A substance formed when two or more different elements are chemically bonded together.

Subscript

A number written below and to the right of a chemical symbol, indicating the number of atoms of that element in a molecule.

Atomic Element

An element that exists as single atoms.

Molecular Element

An element that does not exist as single atoms but as molecules, typically with two or more atoms.

Diatomic

A molecule composed of two atoms, which can be the same or different.

Allotropes

Different structural forms of the same element in the same physical state.

Ionic Compound

A compound formed between a metal and a nonmetal, involving the transfer of electrons.

Molecular Compound

A compound formed from nonmetals, where electrons are shared between atoms.

Molar Mass (MM)

The mass of one mole of a substance, usually expressed in grams per mole (g/mol).

Conversion between grams and moles

Using the molar mass to convert the mass of a substance to the amount in moles, and vice versa.

Chemical Bond

A lasting attraction between atoms that enables the formation of chemical compounds.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Polar Covalent Bond

A type of bond that occurs when two atoms share electrons unequally due to differences in electronegativity.

Nonpolar Covalent Bond

A bond formed when two atoms share electrons equally.

Polyatomic Ion

An ion made up of two or more atoms bonded together, which carries a net charge.

Solubility

The ability of a substance to dissolve in a solvent, typically measured in terms of concentration.

Oxidation State

A number that represents the total number of electrons an atom gains or loses to form a chemical bond.

Synthesis Reaction

A type of chemical reaction where two or more reactants combine to form a single product.

Decomposition Reaction

A reaction in which a single compound breaks down into two or more elements or new compounds.

Replacement Reaction

A reaction where one element replaces another in a compound, or when two compounds exchange components.

Balancing Chemical Equations

The process of ensuring that the number of atoms for each element is the same on both sides of a chemical equation.

Reactants

Substances that undergo a chemical change in a reaction, found on the left side of a chemical equation.

Products

Substances that are formed as a result of a chemical reaction, found on the right side of a chemical equation.

Coefficients

Numbers placed in front of the reactants or products in a chemical equation to balance the number of atoms.

Law of Conservation of Mass

A principle stating that mass is neither created nor destroyed in a chemical reaction; the mass of reactants equals the mass of products.

Steps to Balance Equations

1. Write the unbalanced equation; 2. Count the number of atoms of each element; 3. Adjust coefficients to balance the atoms; 4. Repeat until balanced.

Types of Chemical Reactions

The classification of reactions includes synthesis, decomposition, single replacement, and double replacement.

Stoichiometry

The calculation of reactants and products in chemical reactions based on balanced equations.

Milliliters

A unit of volume equivalent to one-thousandth of a liter.

Density

The mass of an object divided by its volume, typically expressed in g/mL or kg/m³.

Significant Figures

Digits in a number that contribute to its precision, including all non-zero digits, any zeros between significant digits, and trailing zeros only if there's a decimal point.

Atomic Number

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

Isotope

Atoms of the same element that have the same number of protons but different numbers of neutrons.

Avogadro's Number

The number of atoms or molecules in one mole of a substance, approximately 6.022 x 10²³.

Anion

A negatively charged ion that has gained one or more electrons.

Causality

The principle that everything has a cause and that cause must precede its effects.

Alkaline Earth Metals

Elements found in Group 2 of the periodic table, known for being reactive and typically forming +2 cations.

Grams to Moles Conversion

A calculation using the molar mass of a substance to convert its weight in grams to the amount in moles.

Proton Count

The number of protons in an atom's nucleus, which defines the element and determines its charge.

Krypton (Kr)

A noble gas with the atomic number 36, used in various lighting applications.

Mass Number

The total number of protons and neutrons in an atom's nucleus, used to identify isotopes.

Micrometers

A metric unit of length equal to one-millionth of a meter.

Halogens

Elements found in Group 17 of the periodic table, known for being highly reactive nonmetals.