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chem #1
electrons
Question | Answer |
---|---|
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 |