Term
|
Definition
|
|
Term
|
Definition
| The smallest unit of matter that retains the properties of an element |
|
|
Term
|
Definition
| The total mass of an atom, which is the mass in grams of one mole of the atom, measured in daltons |
|
|
Term
|
Definition
| An atom's central core containing neutrons and protons closely packed together with electrons forming a cloud around the nucleus. |
|
|
Term
|
Definition
Number of protons, written as a subscript to the left of the symbol for an element.
2He (Helium 2 protons) |
|
|
Term
|
Definition
| An ion with a positive charge, produced by the loss of one or more electrons |
|
|
Term
|
Definition
| An attraction between two atoms, resulting from a sharing of otter-shell electrons or the presence of opposite charges on the atoms. The bonded atoms gain complete outer electron shells. |
|
|
Term
|
Definition
| In a reversible chemical reaction, the point at which the rate of the forward reaction equals the rate of the reverse reaction. |
|
|
Term
|
Definition
A process leading to chemical changes in matter; involves the making and/or breaking of chemical bonds.
A process in which atoms of the same or different elements rearrange themselves to form a new substance
|
|
|
Term
|
Definition
A substance consisting of two or more elements in a fixed ratio
Na + Cl = NaCl (1:1 ratio) |
|
|
Term
|
Definition
The bond formed by the sharing of a pair of valence electrons by two atoms
Hydrogen + Oxygen in Water = Methane
H + O = CH4
|
|
|
Term
|
Definition
John Dalton; English chemist
A measure of mass for atoms and subatomic particles |
|
|
Term
|
Definition
A type of chemical bond consisting of two covalent bonds linking two atoms in a molecule
H H
C=C
H H |
|
|
Term
|
Definition
A subatomic particle with a single negative charge, one or more move around the nucleus of an atom
|
|
|
Term
|
Definition
| An energy level represented as the distance of an electron from the nucleus of an atom. |
|
|
Term
|
Definition
| The attraction of an atom for the electrons of a covalent bond; non metals have a higher electronegativity |
|
|
Term
|
Definition
| Any substance that cannot be broken down to any other substances by chemical reaction; 92 elements occurring in nature |
|
|
Term
|
Definition
| the capacity to do work (to move matter against an opposing force |
|
|
Term
|
Definition
| Different states of potential energy for electrons in an atom; correlated with its average distance form the nucleus. |
|
|
Term
|
Definition
| A hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom; weak chem bond |
|
|
Term
|
Definition
| An atom that has gained or lost electrons, thus acquiring a charge |
|
|
Term
|
Definition
| A chemical bond resulting form the attraction between oppositely charged ions, high electronegativity difference |
|
|
Term
|
Definition
| A compound resulting from the formation of an ionic bond; also called a salt |
|
|
Term
|
Definition
| The atomic form of an element, containing a different number of neutrons and thus differing in atomic mass |
|
|
Term
|
Definition
| Number of protons + Number of electrons |
|
|
Term
|
Definition
| Anything that takes up space and has mass |
|
|
Term
|
Definition
A type of molecular notation indicating only the quantity of the essential atoms
H2 (molecule has 2 atoms of hydrogen) |
|
|
Term
|
Definition
| Two or more atoms held together by covalent bonds |
|
|
Term
|
Definition
| An electrically neutral particle (has no charge), found in the nucleus of an atom |
|
|
Term
|
Definition
| A type of covalent bond in which electrons are shared equally between two atoms of similar electronegativity |
|
|
Term
|
Definition
| The three-dimensional space where an electron is found 90% of the time. |
|
|
Term
| Periodic Table of Elements |
|
Definition
| A chart of the chemical elements, arranged in three rows, corresponding to the number of electron shells in their atoms. |
|
|
Term
|
Definition
| A covalent bond where one atom is more electronegative than the other; making one atom slightly negative and the other slightly positive. |
|
|
Term
|
Definition
| The energy stored by matter as a result of its location or spatial arrangement; measured in joules |
|
|
Term
|
Definition
An ending material in a chemical reaction
H + Cl = HCl (product) |
|
|
Term
|
Definition
| A subatomic particle with a single positive electrical charge found in the nucleus of an atom; atomic number on periodic table |
|
|
Term
|
Definition
An isotope (an atomic form of a chemical element) that is unstable; the nucleus decays spontaneously, giving off detectable particles of energy
NUCLEAR DECAY |
|
|
Term
|
Definition
A starting material in a chemical reaction
(reactant) H + Cl = HCl |
|
|
Term
|
Definition
A compound resulting from the formation of an ionic bond or ionic compound
Na + Cl = NaCl (sodium chloride) |
|
|
Term
|
Definition
| A covalent bond in which one electron pair is shared by two atoms |
|
|
Term
|
Definition
A type of molecular notation in which the essential atoms are joined by lines representing covalent bonds
[image] |
|
|
Term
|
Definition
| An element necessary for life but required in extremely minute amounts |
|
|
Term
|
Definition
| The bonding capacity of an atom, generally equal to the number of unpaired electrons in the outermost shell |
|
|
Term
|
Definition
| An electron in the outermost electron shell |
|
|
Term
|
Definition
| The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom |
|
|
Term
| Van der Waals Interactions |
|
Definition
Weak attractions between molecules or parts of molecules that are brought about by localized charge fluctuations
Electrons are constantly in motion and at any given instant changing "hot spots" of - or + charge may develop |
|
|
