Chemistry Fundamentals Quiz

Significant Figures

• All non-zero digits are significant, e.g., 23294 has five significant figures.
• All initial zeros are insignificant, e.g., 0.00231 has three significant figures.
• All zeros after a significant figure and after a decimal point are significant, e.g., 9.00 has three significant figures.
• All zeros between significant figures are significant, e.g., 303 has three significant figures.
• All zeros after a significant figure and before a decimal point are significant, e.g., 11,000. has five significant figures, while 11,000 has two significant figures.

Conversion of Units

• Milli (m) = -1000
• Centi (c) = -100
• Deci (d) = -10
• Base = 1
• Deca (D) = +10
• Hecto (H) = +100
• Kilo (K) = +1000
• Example: Convert 5 g/ml to kg/dL

Atoms

• The smallest unit of matter, consisting of protons, neutrons, and electrons.
• Atoms are arranged in periods in the periodic table.
• Each column is a group with similar properties and almost similar charges.
• Atoms react with each other to form molecules and new substances.
• Atoms have volume and mass, which are calculated using moles.
• Important atomic weights to memorize:
  • H = 1
  • C = 12
  • N = 14
  • O = 16
  • F = 19
  • Na = 23
  • Mg = 24.31
  • P = 30.97
  • S = 32.96
  • Cl = 35.45
  • K = 39.10
  • Ca = 40.08

Physical Pharmacy

• Application of physical and chemical principles and laws in the pharmaceutical sciences.
• Understanding and development of dosage forms and drug delivery systems.

Units and Dimensions

• Measuring physical quantities:
  • Quantity: length, mass, temperature, time, etc.
  • Dimension: L, M, Θ, T, etc.
  • SI Unit: meter, kilogram, kelvin, second, etc.
  • Symbol: m, kg, K, s, etc.
  • Formula: varies
• Base units:
  • Length: meter (m)
  • Mass: kilogram (kg)
  • Temperature: kelvin (K)
  • Time: second (s)
• Derived units:
  • Area: square meter (m2)
  • Volume: cubic meter (m3)
  • Velocity: meter per second (m/s)
  • Acceleration: meter per second squared (m/s2)
  • Density: kilogram per cubic meter (kg/m3)
  • Force: newton (N)
  • Pressure, Stress: pascal (Pa)
  • Energy: joule (J)
  • Quantity of heat: joule (J)
  • Work: joule (J)
  • Power: watt (W)
  • Viscosity, dynamic: pascal-second (Pa·s)
  • Viscosity, kinematic: square meter per second (m2/s)
  • Specific heat: joules per kilogram-kelvin (J/kg·K)

Temperature and Atmospheric Pressure

• These factors affect the physical properties of matter, so it's essential to record them in the laboratory before experimentation.

Milliequivalents

• An equivalent is the amount of a substance that will react with a certain number of hydrogen ions.
• A milliequivalent is one-thousandth of an equivalent.
• Formula: varies depending on the type of substance.

Osmolarity

• An osmole is an amount of a substance that contributes to the osmotic pressure of a solution.
• A milliosmole is one-thousandth of an osmole.
• Formula: varies depending on the type of substance.

Seatwork

• Examples of problems involving percentage concentration, e.g., finding the % concentration of 0.9g NaCl in 100ml solution.