PHA 317 Exam 1 | Questions and Answers (Complete Solutions)

PHA 317 Exam 1 | Questions and Answers (Complete Solutions) How closely a measured value is to the correct value is ___ Accuracy How closely individual measurements are relative to each other is ___ Precision Regarding ...

PHA 317 Exam 1 | Questions and Answers (Complete Solutions) How closely a measured value is to the correct value is ___ Accuracy How closely individual measurements are relative to each other is ___ Precision Regarding significant figures, ALL nonzero digits are ___ (i.e. - 12.768) Significant Regarding significant figures, a zero is ___ when followed by a nonzero number. (i.e. - 12.076) Significant Regarding significant figures, a zero after a decimal and before a nonzero number is ___ (i.e. - 0.02) not significant Regarding significant figures, a zero after a decimal and following a nonzero number is ___ (i.e. - 0.20) Significant Regarding significant figures, a zero before a decimal is ___ either significant or not significant depending on increments of the tool used for measuring (10 g increments vs 1 g increments on a scale) NLT means ___ not less than NMT means ___ no more than NLT and NMT are abbreviations used when talking about ___ USP monographs Rounding is ___ with USP monographs. not acceptable 89.9% can be equal to ___ but not ___ 90% ; 90.0% Mode is ___ most frequently occurring value Mean is ___ the average of all values Median is ___ the middle-most value Standard deviation is ___ A description of how much variation there is in a data set What mathematical method utilizes units and ratios between them to reach a desired quantity with a specific/ required unit? Dimensional analysis The three fundamental dimensions include ___ and this is called the ___ length, mass, and time ; cgs system The definite unit of length is ___ centimeters (cm) The definite unit of mass is ___ grams (g) The definite unit of time is ___ seconds (sec) An angstrom is equal to ___ and measures ___ 10^-10 meter ; microscopic distances The four derived dimensions typically discussed in pharmacy calculations include: 1. density and specific gravity, 2. force, 3. pressure, & 4. work, energy, and heat Density is equal to ___ mass / volume Specific gravity is equal to ___ density of a substance / density of water Units of density are written as ___ in the cgs system g/cm^3 (or g/cc) Units of density are written as ___ in the SI system Kg / m^3 Force is equal to ___ mass x acceleration Units for force are ___ dyne [ or (g*cm)/ sec^2 ] The force exerted on the body due to gravity is called ___ Weight With 1 gram of mass, weight is equal to ___ 981 dyne (g*cm/s^2) With 1 kilogram of mass, weight is equal to ___ 9.81 Newton (kg*m/sec^2) Pressure is equal to ___ force / area The unit for pressure is ___ dynes / cm^2 [ g / cm(sec^2) ] Work is equal to ___ force x distance The cgs unit for work is ___ which is equal to ___ ergs ; dyne*cm The SI unit of work is ___ which is equal to ___ joules (J) ; 10^7 ergs Energy is the ___ capacity to do work Heat is typically written in cgs units of ___ or ___ calorie or kilocalorie Heat and work are ___ forms of energy Equivalent Intravenous CSPs are typically allowed ___ variance ±5% Matter is anything with ___ mass and a volume The acceleration of matter is described by Newton's ___ law of motion, where F=m*a 2nd A greater mass will have a ___ acceleration for the same applied force Slower Molecules interact with each other via the forces of ___ and ___ attraction and repulsion What are the two types of attractive forces? cohesive and adhesive What are cohesive forces? forces of attraction between molecules of the same substance What are adhesive forces? forces of attraction between molecules of differing substance What are repulsive forces? forces that push molecules apart Attractive forces are inversely proportional to ___ the distance separating the molecules [ FA = 1 / (r^n) ] Repulsive forces are proportional to an exponential relationship with the ___ reciprocal of the distance separating molecules [FR = e ^(1/r) ] As repulsive forces increase, the potential energy becomes ___ increasingly positive What forces act over a longer distance than repulsive forces? attractive forces What is the distance where the attractive and repulsive forces balance with each other called? collision diameter Intramolecular bonds are forces of attraction between ___ atoms of an individual molecule (covalent bonds, ionic bonds) Intermolecular bonds are forces of attraction between ___ between a molecule and its neighbor molecule Intermolecular bonding is relatively ___ in nature Weak Dipoles can be ___ permanent or transient What kind of chemical bond formed through an electrostatic attraction between two oppositely charged ions? Ionic bond Ionic bonds are formed between a ___ and a ___ cation (typically metal) and anion (typically nonmetal) Ion-dipole bonds are formed between a ___ and a ___ a neutral molecule and a permanent dipole An example of an ion-dipole interaction is ___ NaCl dissolving in water Ion-dipole interactions are relatively ___ strong and insensitive to temperature/distance What forces originate from the interaction of permanent dipoles? Dipole-dipole forces Dipole-dipole forces are also called ___ Kescom forces The strongest type of Van der Waals forces are ___ dipole-dipole Dipole-induced dipole interactions are also called ___ Debye forces What forces include the interactions between atoms and molecules, even if they are neutral charge and don't have permanent dipoles? Dispersion forces Unusual properties of water, like high boiling point and solid ice occupying more space than liquid water, are due to ___ hydrogen bonding Dispersion forces are also called ___ and ___ Van der Waals forces ; London forces The cgs unit for a dipole is a debye, which is equivalent to ___ 10^-18 esu cm What is a measure of electrostatic charge required to repel a similar charge that is 1 cm away with a force of 1 dyne? An esu Abscissa is the ___ axis X Ordinate is the ___ axis Y Attractive forces ___ when the distance between two atoms decreases, therefore resulting in ___ potential energy increases ; decrease Molecules are more stable than atoms and their formation can be explained by what two theories? valence bond theory and molecular orbital theory If a dipole moment is ___, then the drug is more soluble in water Higher Hydrogen bonds have characteristics of both ___ and ___ forces ionic and dipolar Which type of solids will dissolve at a greater rate? Amorphous Sodium chloride is ___(-valent) Electrovalent Methane is ___ (-valent) Covalent The transition from the solid state to the liquid state is ___ Melting The transition from the liquid state to the gas state is ___ Vaporization The transition from the gas state to the solid state is ___ Deposition The transition from the solid state to the gas state is ___ Sublimation The transition from the gas state to the liquid state is ___ Condensation The transition from the liquid state to the solid state is ___ freezing or fusion Typically, a material must pass through the liquid state to go from a gas to a solid, however certain materials can change directly, such as the drug ___ Nitroglycerin Liquid crystals are a state of matter that has properties between those of ___ and those of a ___ conventional liquid and a solid crystal Supercritical fluids occur when a substance is at temperature and pressure above its ___ or at the ___ critical point ; triple point What is it called when all three phases are in equilibrium? Triple point The critical temperature for water is ___ 374 degrees Celsius The critical pressure for water is ___ 218 atm "Room temp" or "standard temp" is ___ 25 degrees Celsius What is the state in which the system has both properties of gas and liquid? supercritical fluid state Supercritical fluids are ___ to pharmaceuticals significantly important An example of supercritical fluid in pharmaceuticals includes: drug being suspended in a propellant which is gas at room temp but liquid under high pressure in a can What law describes the behavior of an ideal gas as a function of temperature, pressure, volume, and amount of gas? Ideal Gas Law Gay-Lussac's and Charle's Law Formula V/T = constant, k (when P is constant) Boyle's Law Formula PV = constant, k (when T is constant) Combing Boyle's, Gay-Lussac's, and Charle's Laws gives you the formula: (P1V1) / T1 = (P2V2) / T2 The formula for the Ideal Gas Law is PV = nRT The constant R in the ideal gas law is the molar gas constant, and is equal to ___ 8.314 J/K*mol 0.08206 Latm/Kmol 1.986 cal/K*mol For Ideal Gas Laws, the unit for temperature is always ___ Kelvin Henry's Law states that as pressure ___, the concentration of gas ___ increases ; also increases The pressure exerted by a vapor in equilibrium with a liquid at a given temperature in a closed system is called ___ vapor pressure degrees of freedom equation F = C - P + 2 (c is component, on a curve always =1) (p is number of phases) At the triple point, the degree of freedom is equal to ___ 0 What are the 2 types of solids? crystalline and amorphous Crystalline solids have ___ 3D structure a well-defined Amorphous solids have ___ 3D structure ambiguous, or poorly-defined