Significant Figures and Operations Quiz

Study Notes

Significant Figures and Calculations

Liters can be reported to the nearest significant figure, for instance, 152.82662 liters rounds to 152.83 liters.
Addition: Result is determined by the least precise decimal place.
Subtraction: Similar to addition, significant figures depend on precision of the decimal places.

Scientific Notation

In scientific notation, solve addition by converting both numbers to standard form.
Alternatively, adjust one number’s exponent for consistency before adding.

Multiplication and Division of Significant Figures

Result precision is limited by the number with the fewest significant figures.
Example: A number with 2 significant figures dictates the answer’s precision.

Unit Conversion

Factor-Label Method (Dimensional Analysis) aids in unit conversion using conversion factors.
Example: 1 gallon = 4 quarts allows conversion of 12 gallons to quarts.

Classification of Matter

Matter can be categorized by state (solid, liquid, gas) and composition (pure substances vs. mixtures).
Pure substance: One component; Mixture: Combination of two or more components retaining their identities.

States of Matter

Gas: Particles far apart with no definite shape or volume.
Liquid: Particles close yet no definite shape, maintains volume.
Solid: Particles tightly packed, maintains both shape and volume.

Composition of Matter

Elements: Pure substances that cannot be simplified chemically.
Compounds: Pure substances formed by the chemical combination of elements in fixed ratios.

Properties and Changes in Matter

Physical property: Observable without altering substance makeup (e.g., color, hardness).
Physical change: Alteration in state or appearance without changing composition.

Chemical Properties and Reactions

Chemical property: Observed only during a chemical reaction.
Chemical reaction: Transformation into different substances through atomic rearrangement.

Intensive vs. Extensive Properties

Intensive properties: Independent of quantity (e.g., color, boiling point).
Extensive properties: Dependent on amount of material present.

Energy

Defined as the ability to perform work; can be kinetic (energy of motion) or potential (stored energy).
Energy conversions are less than 100% efficient; reactions involve energy changes.

Units of Energy

Caloric measurement: 1 calorie = 4.184 joules; food Calories (kcal) measure energy in kilocalories.

Density and Concentration

Density: Mass-to-volume ratio, used for characterizing substances with unique values.
Common densities: Water at 1.000 g/mL, Mercury at 13.6 g/mL.
Concentration reflects the quantity or mass of a substance in a given volume.

Applications of Density

Calculation of density involves mass and volume; example: Aluminum density calculated as 2.70 g/mL.
Density can serve as a conversion factor for calculations involving mass and volume.

Example Density Values

Air: 0.00129 g/mL
Water: 1.000 g/mL (highest density at 4 degrees C)
Lead: 11.3 g/mL
Gasoline: 0.66 to 0.69 g/mL

Temperature Conversions

Convert between Fahrenheit and Celsius using established formulas.
Kelvin scale relates directly to molecular motion; important in thermodynamics.

These notes capture essential concepts from chemistry, focusing on measurement accuracy, states of matter, energy forms, properties of substances, and methods for conversion and computation.

Description

Test your knowledge of significant figures with this quiz focused on addition and subtraction. You will be required to report results properly to the correct number of significant figures. Ideal for students studying mathematics or scientific notation.