Chem - Chapter 1 Notes: Scientific Measurements and Uncertainty

Vocabulary flashcards covering fundamental chemistry terminology, SI base units, temperature conversion, density equations, measurement uncertainty, and significant figure rules based on chapter 1 notes.

Chemistry

The study of matter and the changes it undergoes.

Matter

Anything that has mass and occupies space.

Scientific method

A systematic process of inquiry that progresses from method to hypothesis, experiment, experiment, and theory.

SI Base units

The revised metric system base units consisting of length ($\text{m}$), mass ($\text{kg}$), time ($\text{s}$), electric current ($\text{A}$, ampere), temperature ($\text{K}$, kelvin), and amount of substance ($\text{mol}$).

Kelvin temperature conversion

The formula $K = {}^\circ\text{C} + 273.15$, which defines the temperature scale relative to absolute zero.

Density

The quantitative relationship defined as $\text{density} = \frac{\text{mass}}{\text{volume}}$, typically expressed in units of $\text{g/mL}$ or $\text{g/cm}^3$.

Exact numbers

Quantities that are counted or derived from defined precise measurements (for example, $1\,\text{m} = 100\,\text{cm}$).

Inexact numbers

Values obtained through measurement that contain uncertainty, encompassing all non-exact values.

Uncertain digit

The last reported digit in a measured quantity, reflecting the precision limit expressed as $\pm 0.01$ or $\pm 0.001$.

Exponential notation for significant figures

The method of writing numbers with trailing zeros using scientific notation ($\text{sig fig} \times 10^x$) to unambiguously indicate significant figures; for example, $100$ expressed as $1 \times 10^2$ has $1$ sig fig, $1.0 \times 10^2$ has $2$ sig figs, and $1.00 \times 10^2$ has $3$ sig figs.