Principles of Chemistry CH401: Chapter 1 Review

A comprehensive set of flashcards covering qualitative vs. quantitative research, variables, hypotheses, theory, scientific method, measurements, SI units, density, temperature scales, scientific notation, accuracy/precision, dimensional analysis, ball-park estimates, chemical classification, and basic matter properties.

What is qualitative research?

Non-numerical data consisting of observations, words, and interviews; focuses on in-depth understanding of experiences, perspectives, and meanings rather than measuring data.

What is quantitative research?

Systematic investigation that uses numerical data and statistical techniques to quantify problems, test variables, and generalise results.

What is the Independent Variable (IV)?

The variable manipulated and/or changed in the experiment that affects the Dependent Variable (DV).

What is the Dependent Variable (DV)?

The variable measured and observed in response to the IV.

What is a hypothesis?

A testable and tentative statement proposing an explanation; should be clear, specific, and falsifiable, often following an if-then format.

What is a theory?

A well-known explanation that is repeatedly tested and observed; widely accepted yet testable and falsifiable, and can be revised or discarded if predictions fail.

What is the Scientific Method?

A systematic approach to research with steps such as Define the Problem, Experiment/Observe/Record Data, and Interpret/Explain.

What is a scientific law?

A concise statement, often mathematical, describing what always happens under certain conditions (e.g., Newton’s laws).

What role does the Higgs Boson play in mass?

The interaction of the Higgs Boson with the Higgs Field gives mass to fundamental particles.

What are macroscopic properties?

Properties determined directly, such as volume, temperature, mass, and length.

What are microscopic properties?

Properties that must be determined indirectly at atomic/molecular scales.

How many SI base units are there and what are they for Length?

7 base units; Length = meter (m).

How many SI base units are there and what are they for Mass?

7 base units; Mass = kilogram (kg).

How many SI base units are there and what are they for Time?

7 base units; Time = second (s).

How many SI base units are there and what are they for Electric Current?

7 base units; Electric Current = ampere (A).

How many SI base units are there and what are they for Temperature?

7 base units; Temperature = kelvin (K).

How many SI base units are there and what are they for Amount of Substance?

7 base units; Amount of Substance = mole (mol).

How many SI base units are there and what are they for Luminous Intensity?

7 base units; Luminous Intensity = candela (cd).

What units are commonly used for volume?

cubic centimeters (cm^3), cubic decimeters (dm^3), liters (L), and milliliters (mL).

What is the formula for density?

d = m / v; commonly in kg/m^3 or g/cm^3.

What are Fahrenheit’s freezing and boiling points?

Freezing point: 32°F; Boiling point: 212°F.

What are Celsius’s freezing and boiling points?

Freezing point: 0°C; Boiling point: 100°C.

What is Kelvin’s zero point and its sign restrictions?

0 K is the lowest possible temperature and cannot be negative.

What is the conversion from Celsius to Kelvin?

K = C + 273.15.

What is the conversion from Kelvin to Celsius?

C = K − 273.15.

What is the conversion from Fahrenheit to Celsius?

C = (F − 32) × 5/9.

What is the conversion from Celsius to Fahrenheit?

F = C × 9/5 + 32.

What is scientific notation (per the notes)?

Express numbers as N × 10^n, where N is a number from 1 to 10 and n is an integer.

How is a number like 568.762 written in scientific notation?

5.68762 × 10^2 (decimal moved left to make N between 1 and 10, n = 2).

How is 0.00000772 written in scientific notation?

7.72 × 10^−6.

What is the rule for adding/subtracting numbers in scientific notation?

Ensure all terms have the same exponent, then add or subtract like terms.

What is the rule for multiplying/dividing numbers in scientific notation?

Multiply/divide the coefficients and add/subtract the exponents accordingly.

What are significant figures (SF)?

Meaningful digits in a measured or calculated quantity.

Which digits are always significant?

Nonzero digits.

Are zeros between nonzero digits significant?

Yes, zeros between nonzero digits are significant.

Are leading zeros significant?

No, leading zeros are not significant.

Are trailing zeros significant?

Typically yes if the number has a decimal and the value is greater than 1; the notes provide examples like 2.0 mg = 2 SF and 40.062 mL = 5 SF.

What is dimensional analysis (factor-label method)?

A unit conversion technique using conversion factors to move from a given unit to a desired unit.

How is dimensional analysis applied in an example like 0.0833 lbs to mg?

Use: lbs → g → mg with conversions: 1 lb = 453.6 g and 1 g = 1000 mg; result ≈ 3.78 × 10^4 mg.

What is ball-park estimation?

Simple, quick estimates using educated guesses; formulate a plan, consider theory limitations, and acknowledge assumptions’ impact on accuracy.

What are the three states of matter and their basic definitions?

Solid—definite shape and volume; Liquid—definite volume, no definite shape; Gas—neither definite volume nor shape.

What are the common phase changes between solid, liquid, and gas?

Melting (solid to liquid), Fusion (solid to liquid), Sublimation (solid to gas), Boiling/Evaporation (liquid to gas), Condensation (gas to liquid), Deposition (gas to solid).

What is a substance in matter classification?

A form of matter with a constant composition and distinct properties.

What is a mixture, and how does it differ from a substance?

A combination of two or more substances that maintain their own identities; mixtures can be separated into pure components.

What is the difference between heterogeneous and homogeneous mixtures?

Heterogeneous: components are unevenly distributed and visible (e.g., sand and iron fillings); Homogeneous: components are evenly distributed and not visibly distinct (e.g., dissolved sugar in water).

What is an element?

A substance that cannot be broken down into chemically simpler components; there are 118 known elements.

What is a compound?

A substance composed of atoms of two or more different elements (e.g., H2O).

What are the basic subatomic particles and their properties?

Proton: +1.6×10^-19 C, mass ≈ 1.67×10^-27 kg, located in nucleus. Neutron: 0 C, mass ≈ 1.67×10^-27 kg, located in nucleus. Electron: −1.6×10^-19 C, mass ≈ 9.11×10^-31 kg, located in the electron cloud.

Where are protons, neutrons, and electrons located within an atom?

Protons and neutrons in the nucleus; electrons in the electron cloud surrounding the nucleus.

What are the three fundamental properties classifications?

Physical properties describe physical traits (qualitative: color, texture, odor, state; quantitative: density, boiling/melting point, viscosity, conductivity); Chemical properties describe a substance’s ability to change its chemical structure or composition (e.g., flammability, reactivity).

What is the distinction between extensive and intensive properties?

Extensive properties depend on the amount of matter (e.g., mass, volume); Intensive properties do not depend on amount (e.g., density, boiling point).