The physical and chemical properties of the elements are periodic functions of their atomic numbers.
An arrangement of the elements in order of their atomic numbers so that the elements with similar properties fall in the same column or group.
The 14 elements with the atomic numbers 58-71.
The 14 elements with the atomic numbers 90-103.
The elements of group 1 of the periodic table.
The elements of group 2 of the periodic table.
The d-block elements are metals with typical metallic properties.
The p-block elements together with the s-block elements.
The elements of group 17 of the periodic table.
1/2 the distance between the nuclei of identical atoms that are bonded together.
An atom or group of bonded atoms that has a positive or negative charge.
Any process that results in the formation of an ion.
The energy required to remove one electron from a neutral atom of an element.
The energy change that occurs when an electron is acquired by a neutral atom.
a positive ion
a negative ion
The electrons available to be lost, gained, or shared in the formation of chemical compounds.
A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.
a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
chemical bonding that results from the electrical attraction between cations and anions
results from the sharing of electron pairs between two atoms
a covalent bond in which the bonding electrons are shared equally by the bonded atoms resulting in a balanced distribution of electrical charge
have an uneven distribution of charge
covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
energy required to break a chemical bond and form neutral isolated atoms
the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms
indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
a molecule containing only two atoms
a covalent bond in which two pairs of electrons are shared between two atoms
an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the elements symbol
formulas in which atomic symbols represent nuclei and inner-shell electrons, dot pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons
pair of electrons that is not involved in bonding and that belongs exclusively to one atom
a chemical compound whose simplest units are molecules
shows the types and numbers of atoms combined in a single molecule of a molecular compound
a neutral group of atoms that are held together by covalent bonds
double and triple bonds are referred
chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level
bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
is a covalent bond in which one pair of electrons is shared between two atoms
indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in molecule
covalent bond in which 3 pairs of electrons are shared between two atoms
a pair of electrons that is not involved in bonding and that belongs exclusively to one atom
the simplest collection of atoms from which ionic compound's formula can be established
composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
a charged group of covalently bonded atoms
ability of a substance ti be drawn, pulled or extruded through a small opening to produce wire
the ability of a substance to be hammered or beaten into thin sheets
chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons