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23 terms

Atoms, Molecules, Formulas, and Subatomic particles

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Atom
smallest particle of an element that can exist and still have the properties of the element
Atomic theory of matter
1) All mater is made up of small particles called atoms

2)All atoms of any given typer ar similar to one another and significantly different from all other types

3) The relative number and arrangement of different atoms in a pure substrance determine its identity.

4)Chemical change is a union separtaion, or rearrangement of atoms to give new substances

5) Only whole atoms can participate in or result from any chemical change, since atoms are considered indestructible during such changes
Molecule
two or more atoms tightly bound together that function as a unit
Diatomic molecule
Molecule that contains two atoms
Triatomic
Molecule that contains three atoms
Tetraatomic
Molecule that contains four atoms
Homoatomic
Molecule in which all atoms present are the same kind
Heteroatomic
Molecule in which two or more different kinds of atoms are present
Chemical Formula
a notation made up of the chemical symbols of the elements present in a compund and numerical subscript(located to the right of each chemical symbol) that indicate the number of atoms of each element present in a structural unit of the compound
Ionic Compounds
compounds that contain ions
no molecules
Subatomic particle
a very small particle that is a building block for atoms
ie proton, neutron, or, electron
Electron
subatomic particle with a negative charge
Proton
subatomic particle with a postive charge
neutron
subatomic particle with a neutral charge
Nucleus
small, dense, positively charged center of an atom
Nucleon
subatomic particle found in th nucleus of an atom
Atomic number
number of protons in the nucleus of an atom
Element
pure substance in which all atoms present have the same atomic number(sam number of protons)
mass number
sum of the neutron and protons in the nucleus
Isotope
atom with same number of protons and electrons but different number of neutrons
Percent abundance
percent of atoms in a natral sample of a pure element that are a particular isotope of the element
Isobars
atoms that have the same mass number but different atomic number
Atomic mass
relative mass of an average atom of an element on a scale using carbon 12/6Catom as the reference.
Unit is AMU