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attractive force that links atoms to form molecules and compounds

chemical bond resulting from the sharing of valence electrons between atoms

a covalent bond involving the sharing of a single pair of electrons

a covalent bond formed by the sharing of two pairs of electrons

a covalent bond in which three pairs of electrons are shared

diagram showing the locations of all the atoms and valence electrons in a molecule or ion

instead of being shared by just two oxygen atoms as part of a regular single bond or double bond

describes how strongly atoms of that element pull on electrons in chemical bonds

purely covalent bond formed between atoms with equal electronegativity, both atoms share their electrons equally, and the electrons are not pulled closer to one atom than to the other

covalent bond in which the more electronegative atom pulls the shared electrons toward itself

charge less than that of a proton or electron

has opposite partial charges on opposite ends of the molecule; one end of a polar molecule has a negative partial charge, and the other end has a positive partial charge. All polar molecules have at least one polar bond

ion formed from a group of atoms

combinations of chemical symbols and numbers showing the type and number of atoms in each compound

tells how many of each type of atom are in a molecule; covalent networks and ionic compounds do not have molecular formulas because they are not made of molecules

shows general arrangement of the atoms in a molecule

he name of the last element is changed to the end in -ide

prefixes are added to each lament indicating how many atoms are present

list the names of the ions with the cation listed first

he charges of the ions in an ionic compound must add to zero

when an element can form more than one monatomic cation, the charge of the ion is included as a Roman numeral

shows only the simplest ratio of atoms in a compound