Chemistry Fundamentals Quiz

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Questions and Answers

What is the number of significant figures in the number 9.34300?

four

six (correct)

five

seven

What is the conversion of 5 g/ml to kg/dL?

5 kg/dL

0.5 kg/dL

0.05 kg/dL

0.005 kg/dL (correct)

What is the atomic weight of Oxygen?

16 (correct)

What is the purpose of the periodic table?

To organize elements into periods and groups with similar properties Signup and view all the answers

What is the characteristic of atoms that makes them the smallest unit of matter?

They have volume and mass Signup and view all the answers

What is the unit used to calculate the quantity of atoms?

Moles Signup and view all the answers

What is the number of significant figures in the number 11,000.?

five Signup and view all the answers

What is the amount of a substance that will react with a certain number of hydrogen ions?

Equivalent Signup and view all the answers

What is one-thousandth of an osmole?

Milliosmole Signup and view all the answers

What is the unit of measurement for the amount of a substance that contributes to the osmotic pressure of a solution?

Osmole Signup and view all the answers

What is the percentage concentration (w/w, g/g) of 0.423 kg Atropine sulfate in cocoa butter making a total weight of 1.0 kg?

4.23 Signup and view all the answers

What is the percentage concentration (g/ml) of 0.9g NaCl in 100ml solution?

0.009 Signup and view all the answers

What is the formula to find the milliequivalent of a substance?

Not mentioned in the content Signup and view all the answers

What is the SI unit of length?

meter Signup and view all the answers

Which of the following is a derived unit of measurement?

Square meter Signup and view all the answers

What is the unit of energy in the SI system?

Joule Signup and view all the answers

What is the unit of density in the SI system?

Kilogram per cubic meter Signup and view all the answers

Why is it important to record temperature and pressure in the laboratory before experimentation?

To ensure accurate measurements of physical properties Signup and view all the answers

What is the unit of force in the SI system?

Newton Signup and view all the answers

What is the unit of power in the SI system?

Watt Signup and view all the answers

What is the unit of viscosity, dynamic in the SI system?

Pascal-second Signup and view all the answers

Study Notes

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.

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Description

Test your knowledge of basic chemistry concepts, including significant figures, unit conversions, atomic weights, and the periodic table.