General Chemistry I: Chemistry and Measurement Flashcards

Flashcards covering general chemistry concepts including matter classification, the scientific method, SI prefixes, temperature scales, properties of matter, and significant figures.

Chemistry

The study of matter and how it changes.

Matter

Anything that takes up space and has mass.

Observation

A component of the scientific method that is natural and measurable.

Hypothesis

An educated guess used in the scientific method.

Experiment

A test of a hypothesis that measures one variable at a time.

Theory

A component of the scientific method that explains and supports a hypothesis and predicts related observations.

Law

A statement supporting observations within the scientific method.

Solid

A phase of matter with fixed volume and shape, high intermolecular force of attraction, and low kinetic energy where particles vibrate in a fixed position.

Liquid

A phase of matter with fixed volume that takes the shape of its container, having medium intermolecular force of attraction and moderate kinetic energy allowing particles to flow past each other.

Gas

A phase of matter where volume and shape are determined by the container, characterized by low intermolecular force of attraction and high kinetic energy with constantly moving particles.

Pure substance

Matter that has a definite composition and distinct properties.

Element

A substance comprised of the same atoms that cannot be separated into simpler substances through chemical means; examples include iron, oxygen, and carbon.

Compound

A substance comprised of two or more different atoms of different elements that can be separated through chemical means such as decomposition.

Mixture

A physical blend of two or more substances that retain their own distinct properties.

Homogeneous mixture

A mixture with a uniform composition throughout, also referred to as a solution.

Heterogeneous mixture

A mixture with inconsistent composition; if layers form, it can be called a suspension.

Area SI Unit

$$m^2$$

Volume SI Unit

$$m^3$$

Density SI Unit

$$kg/m^3$$

Concentration SI Unit

$$mol/m^3$$

Peta- (P)

SI prefix for the multiplication factor $10^{15}$.

Tera- (T)

SI prefix for the multiplication factor $10^{12}$.

Giga- (G)

SI prefix for the multiplication factor $10^9$.

Mega- (M)

SI prefix for the multiplication factor $10^6$.

Kilo- (k)

SI prefix for the multiplication factor $10^3$.

Deci- (d)

SI prefix for the multiplication factor $10^{-1}$.

Centi- (c)

SI prefix for the multiplication factor $10^{-2}$.

Milli- (m)

SI prefix for the multiplication factor $10^{-3}$.

Micro- (\mu)

SI prefix for the multiplication factor $10^{-6}$.

Nano- (n)

SI prefix for the multiplication factor $10^{-9}$.

Pico- (p)

SI prefix for the multiplication factor $10^{-12}$.

Femto- (f)

SI prefix for the multiplication factor $10^{-15}$.

Mass

The amount of matter in a substance.

Temperature

The average kinetic energy of a substance.

Fahrenheit conversion formula

$$\text{℉} = (\frac{9\text{℉}}{5\text{℃}} \times \text{℃}) + 32\text{℉}$$

Celsius conversion formula

$$\text{℃} = (\text{℉} - 32\text{℉}) \times \frac{5\text{℃}}{9\text{℉}}$$

Kelvin scale

The absolute temperature scale where the lowest possible temperature is zero kelvins; $K = \text{°C} + 273.15 \, \text{K/°C}$.

Density formula

$d = \frac{m}{V}$ (mass divided by volume).

Physical properties

Characteristics that can be observed without changing the identity of a substance, such as length, texture, or color.

Chemical properties

Characteristics only observable as a substance undergoes a chemical change, such as combustibility or reactivity.

Physical changes

Events where external properties change but chemical composition remains the same, such as melting or ripping.

Chemical changes

Events where chemical composition is altered, resulting in a new substance with different properties; indicators include color changes or gas formation.

Quantitative properties

Properties measured with a tool and represented with a numerical value, such as mass or volume.

Qualitative properties

Properties observed without the explicit need for a tool, such as color or texture.

Extensive properties

Properties that depend on the amount of matter present rather than its identity, such as mass or length.

Intensive properties

Properties that depend on the identity of the substance rather than the amount of matter, such as density or boiling point.

Exact numbers

Counting numbers or defined values like conversion factors that do not require rules for uncertainty.

Inexact numbers

Measured numbers (other than counting or defined) that must be rounded to indicate uncertainty.

Significant figures

The meaningful digits in a measured number.

Scientific Notation

A method to represent numbers to clarify significant figures by moving decimal places to create a number between 1 and 9 multiplied by an exponent of 10.

Accuracy

How close a measurement is to a true value.

Precision

How close multiple measurements are with respect to each other.

Dimensional analysis

A problem-solving method using conversion factors as ratios to cancel out units.