Term
| how to tell if an element is atomic or molecular |
|
Definition
Atomic = an element that does not exist in nature diatomically
molecular = an element that is diatomic in nature (Br, I, N, Cl, H, O, F) |
|
|
Term
| how to identify a molecular compound |
|
Definition
| has two or more covalently bonded nonmetals |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| HYDROGEN CARBONATE (BICARBONATE) |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| HYDROGEN SULFITE (BISULFITE) |
|
Definition
|
|
Term
|
Definition
|
|
Term
| HYDROGEN SULFATE (BISULFATE) |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| how to identify a OXYACID |
|
Definition
| contain hydrogen oxygen and some other nonmetal |
|
|
Term
| how to identify hydrocarbon |
|
Definition
| compound containing only carbon and hydrogen |
|
|
Term
| how to identify a functionalized hydrocarbon |
|
Definition
| contains on OH functional group |
|
|
Term
|
Definition
| mols of substance / liters of soln |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| What are the postulates of John Daltons atomic theory of matter |
|
Definition
1) all matter is composed of indivisible and indestructible atoms
2) an element is a type of matter composed of only one type of atom
3) a compound or molecule is a type of matter composed of two or more elements chemically combined in fixed proportions
4) A chemical reaction is where a substance is changed into a new substance |
|
|
Term
| what are the three temp scales measured relative too |
|
Definition
Fahrenheit - measured relative to salt water
Celsius - measured relative to pure water
Kelvin - absolute, measured relative to motion of atoms |
|
|
Term
| formula for Celsius to kelvin |
|
Definition
|
|
Term
| how to get to Fahrenheit from celcius |
|
Definition
|
|
Term
| the law of conservation of matter |
|
Definition
| matter is neither created nor destroyed |
|
|
Term
| the law of multiple proportions |
|
Definition
| elements can combine in more than one set of proportions, with each set of proportions corresponding to a diff compound |
|
|
Term
| the law of definite proportions |
|
Definition
| all samples of a given compound have the same proportions of their constituent elements |
|
|
Term
| what are cathode ray particles and who discovered them |
|
Definition
| electron streams, JJ Thompson |
|
|
Term
| what is the definition of wavelength |
|
Definition
| the distance between any adjacent identical points on a wave |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| the first law of thermodynamics |
|
Definition
| says that the total energy in the universe is constant |
|
|
Term
| energy is released in a chemical reaction when |
|
Definition
|
|
Term
| energy is consumed in during a chemical reaction when |
|
Definition
|
|
Term
| fuels always have what type of enthalpy |
|
Definition
| a negative enthalpy, ie negative delta H |
|
|
Term
| fuels are endo or exothermic |
|
Definition
|
|
Term
| standard state enthalpies are measured at what temp and pressure |
|
Definition
|
|
Term
|
Definition
| vertical height of a wave or depth of a trough |
|
|
Term
|
Definition
| the number of wave crests that pass a through a stationary point in a given period of time |
|
|
Term
| equation to find frequency (V) |
|
Definition
| frequency (v) = speed of light (c)/ wavelength (lambda) |
|
|
Term
| unit used to define frequency |
|
Definition
|
|
Term
| what is the photoelectric effect |
|
Definition
| the observation that many metals emit electrons when light shines upon them |
|
|
Term
| how to measure the energy of a photon |
|
Definition
| energy (E) = h(plancks constant)*v(frequency)/wavelength (lambda) |
|
|
Term
| Heisenberg's uncertainty principle |
|
Definition
| the more accurately you know the position of an electron the less accurately you know the position and vice versa |
|
|
Term
| principal quantum number (n) represents what |
|
Definition
| size and energy of the orbital (n can be 1-8) |
|
|
Term
| angualar momentum quantum number (L)represents what |
|
Definition
| shape of the orbital (n-1) |
|
|
Term
| magnetic quantum number (m sub L) represents what |
|
Definition
| orientation in space (-L through +L) |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| minimum energy required to completely remove an electron from a ground state atom In the gas phase |
|
|
Term
|
Definition
| every orbital in a subshell must be singly occupied before any one orbital is doubly occupied, all singly occupied must have same spin |
|
|
Term
| pauli exclusion principle |
|
Definition
| no two electrons in an atom can have the same four quantum numbers (must have opposite spin) |
|
|
Term
| how to know if something will interact with magnet |
|
Definition
full subshell = wont interact
not full subshell = will interact |
|
|
Term
| five basic shapes of VSEPR theory |
|
Definition
linear
bent
trigonal planar
trigonal pyramidal
tetrahedral |
|
|
Term
|
Definition
|
|
Term
| trigonal planar bond angle |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| trigonal pyramidal bond angle |
|
Definition
|
|
Term
| how to tell if a molecule is polar by looks |
|
Definition
| central atom has one or more lone pairs = polar |
|
|
Term
| how to tell if a molecule is non polar by looks |
|
Definition
| central atom has no lone pairs and all of the outer atoms are identical = non polar |
|
|
Term
| second way to tell if a molecule is polar by looks |
|
Definition
| central atom has no lone pairs and the outer atoms are not identical = polar |
|
|
Term
| how to tell if something will have a resonance hybrid |
|
Definition
| central atom bonded to more than one oxygen with double or triple bonds it is a tipoff |
|
|
Term
| what are the three postulates of kinetic molecular theory |
|
Definition
1) the size of a particle is negligibly small
2) the avg kinetic energy of a particle is proportional to them temp in K
3) the collisions between particles and their containers are elastic |
|
|
Term
| three types of intermolecular forces |
|
Definition
dispersion (London forces)
Dipole-Dipole forces
Hydrogen Bonding |
|
|
Term
| dispersion forces exist where |
|
Definition
|
|
Term
| dipole-dipole forces exist where |
|
Definition
|
|
Term
| hydrogen bonding forces exist where |
|
Definition
| in polar molecules where H atoms are bonded to FON, super dipole force |
|
|
Term
| how to change from liquid to gas |
|
Definition
| increase heat or reduce pressure |
|
|
Term
| gasses are least ideal when |
|
Definition
| high pressure and low temp |
|
|
Term
| a molecules weight relates to dispersion forces how |
|
Definition
| the heavier the molecule the higher the dispersion forces |
|
|
Term
| how does boiling point relate to intermolecular forces |
|
Definition
| higher boiling point = stronger IMF |
|
|
Term
| how do IMF relate to viscosity |
|
Definition
| high IMF = high viscosity |
|
|
Term
| boiling occurs when the pressure of the vapor... |
|
Definition
| when the pressure of the vapor equals the pressure being exerted from surroundings |
|
|
