Unit 1 Vocab: Atomic Structure And Properties Flashcards
Molar Mass (g/mol)
The sum of the total mass in grams of all atoms that make up a mole of a substance
Fórmula Mass (amu)
The sum of average atomic masses of each atom represented in a chemical formula
Avogrados number
6.002x10^23 particles/mol. The number of atoms or molecules in one mole of a substance
Mass spectroscopy
An analytical tool useful for measuring the mass-to-charge ration (m/z) of one or more molecules present in a sample
Isotope
Atoms with the same number of protons but different number of neutrons in their nuclei. They have a different relative atomic mass but not chemical properties
Elemental composition
Specifies the identity, arrangement, and ratio of chemical elements making up a substance
Molecular formula
Tells which atoms and how many of each type of atom are present in a substance (actual ratio of elements)
Empirical formula
A chemical formula showing the simplest ratio of elements present in a compound (simplified subscripts)
Hydrate
A substance that contains water molecules within its structure
Ex: Na₂SO₄ • 10H₂O
Combustión
A type of chemical reaction in which a substance burns in the presence of oxygen giving off heat and light in the process
Ex: Fuel (CₓHᵧ) + O₂ (g) ➝ CO₂ (g) + H₂O (g)
Mixtures
A material made up of two or more different chemical substance which can be seperated by physical method
○ Homogenous mixtures and Heterogeneous mixtures
Puré substances
a unique form of matter with constant chemical composition and distinct chemical properties that cannot be broken down through physical methods.
○ Elements and Compounds
Electron configuration
the arrangement of electrons in orbitals around an atomic nucleus.
○ Full configuration of phosphorous is 1s² 2s² 2p⁶ 3s² 3p³
○ Noble gas abbreviation of phosphorus is [Ne] 3s² 3p³
Orbital diagrams
a type of notation which illustrates an atom’s electron distribution and electron spin within orbitals
Ground state
the lowest allowed energy state of an atom, molecule, or ion.
Excited state
when an electron temporarily occupies an energy state greater than its ground state.
Paired electron
two electrons that occupy the same
excited state
orbital but have opposite spins.
Unpaired electron
an electron that occupies an
orbital of an atom singly, rather than part of an electron pair.
Coulomb’s law
describes the strength of the electrostatic force (attraction or repulsion) between two charged objects.
Coulomb’s law
describes the strength of the electrostatic force (attraction or repulsion) between two charged objects.
Photoelectronic spectroscopy (PES)
the energy measurement of photoelectrons emitted from solids, liquids, or gases by the photoelectric effect.
Atomic radius
the total distance from an atom’s nucleus to the outermost shell of the atom.
Atomic radius
the total distance from an atom’s nucleus to the outermost shell of the atom.
Ionization energy
the amount of energy required to remove an electron from an isolated atom.
○ increases up and right
Electronegativity
the measure of the tendency of an atom to attract a bonding pair of electrons.
○ increases up and right
Electron affinity
the potential energy change of the atom when an electron is added to a neutral gaseous atom to form a negative ion.
○ increases up and right
Valence electrons
electrons in the outermost shell of an atom and that can participate in the formation of a chemical bond
Ion charges
the electrical charge of an ion, created by the gain (negative charge) or loss (positive charge) of one or more electrons.
Ion charges
the electrical charge of an ion, created by the gain (negative charge) or loss (positive charge) of one or more electrons.
Ionic compound
a type of chemical compound where the oppositely-charged ions of a metal and a nonmetal are attracted to each other to form an ionic bond.
