general chemistry chapter 2 definitions left click your mouse to continue
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ALLOTROPIC MODIFICATIONS (ALLOTROPES)
Different forms of the same element in the same physical state
ATOM
• The smallest particle of an element that maintains its chemical identity through all chemical and physical changes.
• Fundamentally consists of: electrons, protons and neutrons
• Atom contains equal numbers of protons and electrons
• Atoms are components of molecules
ATOMIC MASS UNIT (AMU)
One twelfth of the mass of an atom of the carbon-12 isotope; a unit used for stating atomic and formula weights
ATOMIC NUMBER
• The number of protons in the nucleus of an atom.
• An atom contains an equal number of electrons and protons.
ATOMIC WEIGHT
Weighted average of the masses of the constituent isotopes of an element; the relative mass of atoms of different
elements.
COMPOSITION STOICHIOMETRY
Describes the quantitative (mass) relationships among elements in
compounds.
EMPIRICAL FORMULA
The smallest whole-number ratio of atoms present in a compound;
Also known as the simplest formula
FORMULA WEIGHT
The mass, in atomic mass units, of one formula unit of substance.
Numerically equal to the mass, in grams, of one mole of the substance. This number is obtained by adding
the atomic weights of the atoms specified in the formula.
HYDRATE
A crystalline sample that contains water and another compound in a
fixed mole ratio.
Ex: CuCO4.5H2O
ION
• An atom or group of atoms that carries an electrical charge.
• A positive ion is a cation; a negative ion is an anion
• Ions are formed when neutral atoms lose or gain electrons
LAWS OF CONSTANT COMPOSITION
Different samples of a pure compound always contain the same elements in the same proportions by mass; this corresponds to atoms of these elements in fixed numerical ratios.
Also known the Law of Definite Proportions
LAW OF MULTIPLE PROPORTIONS
When two elements, A and B, form more than one compound, the ratio of the masses of element B that combine
with a given mass of element A in each of the compounds can be
expressed by small whole numbers.
MOLAR MASS
The mass of substance in one mole of the substance; numerically equal to the formula weight of the substance
Units= g/mol
MOLE
6.02 x 1023 formula units (or molecules, for a molecular substance)
of the substance under discussion. The mass of one mole, in grams, is numerically equal to the formula
(molecular) weight of the substance.
MOLECULAR FORMULA
A formula that indicates the actual number of atoms present in a
molecule of a molecular substance.
MOLECULE
• The smallest particle of an element or compound that can have a stable independent existence.
• Atoms are components of molecules, and molecules are the components of many elements and most compounds
MOLECULAR WEIGHT
The mass, in atomic mass units, of one molecule of a nonionic
(molecular) substance. Numerically equal to the mass, in grams, of one
mole of such a substance. This number is obtained by adding the
atomic weights of the atoms specified in the formula.
MONATOMIC
Consisting of a single atom. The noble gases exist as monatomic molecules. Chlorine gas is not
monatomic Cl2
POLYATOMIC
Consisting of more than one atom. Elements such as Cl2, P4 and S8 exist as polyatomic molecules. Examples of polyatomic ions are ammonium
ion, NH4+, and sulfate ion, SO4
-2
STOICHIOMETRY
Description of the quantitative relationships among elements in
compounds and among substances as they undergo chemical changes
DALTON’S ATOMIC THEORY1. An element is composed if extremely small indivisible
particles called atoms.
2. All atoms of a given element have identical properties, which differ from those of other elements.
3. Atoms cannot be created, destroyed, or transformed into atoms of another element.
4. Compounds are formed when atoms of different elements combine with each other in small whole-number ratios.
5. The relative numbers and kinds of atoms are constant in a given compound.