General Flashcards
Mass Number
the total number of protons and neutrons in a nucleus
Atomic Number
the number of protons in the nucleus of an atom, which determines the chemical properties of an element and its place in the periodic table
Proton
a stable subatomic particle occurring in all atomic nuclei, with a positive electric charge equal in magnitude to that of an electron, but of opposite sign
Neutron
a subatomic particle of about the same mass as a proton but without an electric charge, present in all atomic nuclei except those of ordinary hydrogen
Electron
a stable subatomic particle with a charge of negative electricity, found in all atoms and acting as the primary carrier of electricity in solids
Isotope
each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties; in particular, a radioactive form of an element
Atom
the basic unit of a chemical element
Atomic Weight
The average mass of atoms of an element, calculated using the relative abundance of isotopes in a naturally-occurring element. It is the weighted average of the masses of naturally-occurring isotopes
Elements in the same column
group or family
Alkali Metals
Column A1
Alkaline Earth Metals
Column A2
Halogens/Halides
Column A7
Noble Gasses
Column A8
Transition Metals
Columns B1-B10
Electron Shell
a grouping of electrons surrounding the nucleus of an atom
Valence Electron
an electron in the outer shell of an atom which can combine with other atoms to form molecules
Valence Shell
the outermost shell of electrons in an atom; these electrons take part in bonding with other atoms
Core Shells
the shells of electrons within the valence shell
Nuclear Radiation
the process by which a nucleus of an unstable atom loses energy by emitting particles of ionizing radiation
Alpha Radiation
loss of 2 protons and 2 neutrons; ionizing radiation consisting of alpha particles, emitted by some substances undergoing radioactive decay;
Beta Radiation
loss of an electron and gain of a proton; radiation of beta particles during radioactive decay
Gama Radiation
emition of high energy light;
Half Life
the time taken for the radioactivity of a specified isotope to fall to half its original value
Octet Rule
each atom attempts to achieve 8 valence electrons with the exception of hydrogen, boron, and aluminum;
Ionic Bond
a chemical bond formed between two elements when the difference in their electronegativity is greater than 1.7; a chemical bond in which one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion; bonds formed primarily between elements from either side of the metaloid line; elements to the right gain one or more electrons and form anions with a negative charge; elements on the left lose one or more electrons to form cations with a positive charge; bonds between a metal and non-metal are ionic;
Covalent Bond
a chemical bond that involves sharing a pair of electrons between atoms in a molecule; bonds primarily between atoms on the same side of the metaliod line;
Salts
ionic compounds; compounds consisting of catons and anions through ionic bonds; usually disolve in water;
Single Bond; Double (Diative) Bond; Tripple Bond
a single covalent bond consisting of one set of electrons or one electron from each element; a pair of covalent bonds consisting of two sets of electrons or two electrons from each element; a triad of covalent bonds consisting of three sets of electrons or three electrons from each element;
Polar Covalent Bond
a bond formed between elements when the difference of their electronegativity is between 0.3 and 1.7; a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment; these molecules interact through dipole–dipole intermolecular forces and hydrogen bonds; it is dependent on the difference in electronegativity between atoms in a compound and the asymmetry of the compound’s structure; it underlies a number of physical properties including surface tension, solubility, and melting- and boiling-points;
Electronegativity
the tendency of an atom or radical to attract electrons in the formation of an ionic bond; flourine has the highest tendancy to atract an ionic bond; the closer an element is to flourine the higher it’s tendancy towards attracting an ionic bond is; the element with the higher tendancy has a slightly negative charge;
Non-Polar Covalent Bonds
bonds formed through the same element or between carbon and hydrogen;bonds between two elements when the difference of thier electronegativety is less than 0.3
Naming Ionic Compounds
name of cation - root of anion, add “ide”
NaCl is sodium - chlor - ide
MgI2 is magnesium - iod - ide
Physical States
solid (s) liquid (l) gass (g) aqueous (aq) (disolved in water)
A Balanced Equation
the expression of the ratio of molecules;
Molecular Measurement
number of molecules by weight based on the total atomic weight of avagadros number of each of the elements in the molecule;
Avagadro’s Number
6x1023
