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51 Cards in this Set

  • Front
  • Back
anion
a negative ion
halogens
the elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine)
alkaline-earth metals
the elements of Group 2 (beryllium, magnesium, calcium, strontium, barium, and radium)
periodic table
an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group
Henry Moseley
organized the periodic table by atomic number rather than atomic mass
isotope
an atom of the same element that has a different mass
John Dalton
in 1808, proposed the first comprehensive theory of the atom
noble gases
group 18 elements (helium, neon, argon, krypton, xenon, and radon)
electron configuration
the arrangement of electrons in an atom
orbital
a three-dimensional region around the nucleus that indicates the probable location of an electron
Niels Bohr
created a model of the atom in which the electrons were found at fixed orbits around the nucleus
frequency
the number of waves that pass a given point in a specific time, usually one second
molar mass
the mass of one mole of a pure substance
law of conservation of mass
mass is neither created nor destroyed
atomic number
the number of protons in the nucleus of each atom of that element
Ernest Rutherford
conducted the gold foil experiment that led to the discovery of the nucleus
atom
the smallest particle of an atom that retains the chemical properties of that element
covalent bonding
chemical bonding that results from the sharing of electron pairs between two atoms
molecule
a neutral group of atoms that are held together by covalent bonds
octet rule
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
valence electrons
electrons available to be lost, gained, or shared in an atom
metallic bonding
chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
malleability
ability to be hammered into thin sheets
intermolecular forces
forces of attraction between different molecules
polyatomic ion
a charged group of covalently bonded atoms
chemical bond
a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
ionic bonding
chemical bonding that results from the electrical attraction between larger numbers of cations and anions
polar
bonds that have an uneven distribution of charge
bond energy
energy required to break a chemical bond and form neutral isolated atoms
formula unit
simplest collection of atoms from which an ionic compound’s formula can be derived
ductility
ability to be extruded through a small opening and made into a wire
resonance
bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
VSEPR theory
repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible
Joseph John Thomson
conducted experiments cathode rays that led to the discovery of the electron
mass number
the total number of protons and neutrons in the nucleus of an isotope
mole
the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12
electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space
photoelectric effect
the emission of electrons from a metal when light shines on the metal
photon
a particle of electromagnetic radiation having zero rest mass and carrying a quantum of energy
ground state
the lowest energy state of an atom
Heisenberg uncertainty principle
it is impossible to determine simultaneously both the position and velocity of an electron or other particle
Aufbau principle
an electron occupies the lowest-energy orbital that can receive it
Hund’s rule
orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin
Demitri Mendeleev
credited with the creation of the modern periodic table
periodic law
the physical and chemical properties of the elements are periodic functions of their atomic numbers
alkali metals
the elements of Group 1 (lithium, sodium, potassium, rubidium, cesium, and francium)
transition elements
the d-block elements which are metals with typical metallic properties
cation
a positive ion
electronegativity
a measure of the ability of an atom in a chemical compound to attract electrons
lattice energy
the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
nuclear forces
short-range proton-proton, proton-neutron, and neutron-neutron forces that hold the nuclear particles together