Introduction to Analytical Chemistry and Fundamental Concepts

This flashcard set covers the origins of atomic theory, basic subatomic physics, definitions and branches of analytical chemistry, types of chemical analysis, SI unit redefinitions (2019), and fundamental concepts of chemical equilibrium and concentration.

Thales (b. 626 BC)

Ancient Greek philosopher who proposed that water is the prime matter of everything.

Empedocles (b. 494 BC)

Philosopher who theorized that everything is made of four elements: water, earth, air, and fire.

Aristotle (b. 384 BC)

Philosopher who combined the four elements of Empedocles with four qualities: hot, cold, dry, and wet.

Democritus (b. 460 BC)

Theorized that everything we see is made of atoms.

Dalton (b. 1766)

Scientist who determined the relative weights of different types of atoms in 1804.

Prout (b. 1785)

Hypothesized in 1815 that all atoms consist of hydrogen atoms.

Gell-Mann & Zweig (1964)

Theorists who proposed the existence of the quark as the building block of protons and neutrons.

Baryon

A type of hadron made of 3 quarks.

Meson

A type of hadron made of 1 quark and 1 anti-quark.

Van Helmont’s Willow Tree Experiment

An experiment by Jan Baptist van Helmont (1580-1644) that theorized water turned into plant matter, as he did not yet know about photosynthesis.

Strong Nuclear Force

The force that holds protons and neutrons together in the nucleus, mediated by gluons.

Chemistry

The scientific study of the properties, composition, and structure of matter, the changes in structure and composition of matter, and accompanying energy changes according to the McGraw-Hill Dictionary of Scientific and Technical Terms.

Up Quark Charge

$$+2/3$$

Down Quark Charge

$$-1/3$$

Quark Content of a Proton

2 up quarks and 1 down quark, resulting in a net charge of $+1$ because $2 \times (+2/3) + 1 \times (-1/3) = 1$.

Quark Content of a Neutron

1 up quark and 2 down quarks, resulting in a net charge of $0$ because $1 \times (+2/3) + 2 \times (-1/3) = 0$.

Analytical Chemistry

A scientific discipline that develops and applies methods, instruments and strategies to obtain information on the composition and nature of matter in space and time.

Analyte

The specific substance or molecule being identified or measured in a sample.

LOD (Limit of Detection)

The smallest concentration of a target analyte that can be detected.

Sensitivity

The ability of an instrument to discriminate between a small difference in analyte concentration; defined as the detector signal per unit concentration of the analyte.

Population

The entire group being examined or characterized.

Sample

A portion taken from the population for analysis; it must be large enough to be representative.

Specimen

A fraction of a sample that is not necessarily representative of the whole population.

Matrix

Everything in a sample except for the target analyte.

Interference

A substance or condition present that has an effect on target analyte readings, such as baseline noise.

Chromatography

A pillar of modern analytical chemistry used to identify, separate, and quantify individual components of a complex chemical mixture.

Chemometrics

The application of mathematical and computer science techniques to chemical data.

Qualitative Analysis

The analysis of a sample to identify which elements, radicals, or compounds compose it; answers the question "What is it?"

Quantitative Analysis

The analysis of a sample to determine the precise percentage composition of its components; answers the question "How much is there?"

Preconcentration (Enrichment)

The process of increasing the concentration of an analyte so it reaches detectable levels for instruments.

Derivatization

The process of converting a target analyte into a new substance via chemical reaction to achieve more favorable chemical or physical properties.

Kilogram (2019 Definition)

The SI unit of mass defined by taking the fixed numerical value of the Planck constant $h$ to be $6.62607015 \times 10^{-34}$ when expressed in $J \, s$.

Mole (2019 Definition)

The SI unit of amount of substance which contains exactly $6.02214076 \times 10^{23}$ elementary entities.

Solute

The minor component(s) of a solution.

Solvent

The major component of a solution.

Molarity (M)

Concentration expressed as the number of moles of solute per liter of solution.

Molality (m)

Concentration expressed as the number of moles of solute per kilogram of solvent.

Equilibrium

A condition of balance between two opposing tendencies where the rate of the forward reaction equals the rate of the reverse reaction.

Law of Mass Action

A principle stating that for a general reaction $aA + bB \rightleftharpoons cC + dD$, the equilibrium constant is $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$.

Le Chatelier Principle

If a system in equilibrium is disturbed by an external force, the system proceeds to a new equilibrium such that the disturbance is partially offset.

Gibbs Free Energy Equation

$$\Delta G^\circ = -RT \ln K$$