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chem #1


Explains how electrons exist in atoms and how those electrons affect the chemical and physical properties of elements. Bohr model and quantum-mechanical model
A type f energy that travels through space at a constant speed of 3.0x10^8 m/s (186,000 mi/s) electromagnetic radiation
What determines the color of light wavelength
The number of cycles or crests that pass through a stationary point in one second. frequency
Produced by the sun, by stars and by certain unstable atomic nuclei on Earth. gamma rays
A released photon of light containing the precise amount of energy that corresponds to the energy difference between the two orbits. quantum
represents the probability maps that show a statistical distribution of where the electron is likely to be found. orbitals
Represented by letters s, p, d, and f, and specifies its shape. subshell
Lowest energy state ground state
High energy state of an atom excited state
Electrons in the outermost principal shell valence electrons
The energy required to remove an electron from the atom in the gaseous state. ionization energy
models that predict how atoms bond together to form molecules bonding theories
the sharing or transfer of electrons to attain stable electron configurations for bonding atoms. Chemical bond
the transferring of electrons ionic bond
only shared electrons covalent bond
used to predict the shapes of molecules VSEPR theory
the geometrical arrangement of the atoms molecular geometry
the geometrical arrangement of the electron groups electron geometry
the result of an uneven electron sharing, a separation of charge within a bond dipole moment
covalent bonds that have a dipole moment polar covalent bonds
electrons shared equally nonpolar- pure covalent bond
electrons shared unequally polar covalent
a simple model for understanding the behavior of gases kinetic molecular theory
the result of the constant collision s between the atoms or molecules in a gas and the surfaces around them pressure
pressure and volume P1V1=P2V2 Boyle's law
volume and temperature V1/T1=V2/T2 Charle's law
volume and moles V1/n1=V2/n2 Avogadro's law
the interaction between the molecules in coffee that taste bitter and the taste receptors on the tongue: attractive forces that exist between molecules intermolecular forces
the tendency of liquids to minimize their surface area surface tension
liquids that evaporate easily volatile
at the point where the rates of condensation and evaporation become equal dynamic equilibrium
the temperature at which the vapor pressure of a liquid is equal to the pressure above it boiling point
the default intermolecular force, present in all molecules and atoms dispersion force
a type of intermolecular force resulting from transient shifts in electron density within an atom or molecule instantaneous dipole
a separation of charge resulting form the unequal sharing of electrons between atoms permanent dipole
its ability to mix without separating into two phases miscibility
solids whose composite units are molecules molecular solids
solids whose composite units are individual atoms Atomic solids
an atomic solid, sucas iron, which is held together by metallic bonds that, in the simplest model, consist of positively charged ions in a sea of electrons metallic atomic solid
an atomic solid such as diamond, that is held together by covalent bonds covalent atomic solid
is a physical change in which a substance changes from its slid state directly to its gaseous state sublimation
Created by: mistyharrison17