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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.
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
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.
