final exam reviewer Flashcards
The branch of chemistry focused on the qualitative and quantitative analysis of matter to identify substances and determine their amounts.
Analytical Chemistry
The process of identifying the components or types of substances present in a sample.
Qualitative Analysis
The determination of the amount or concentration of a substance in a sample.
Quantitative Analysis
The specific substances being measured or analyzed in a sample.
Analytes
An analytical method based on the measurement of mass to determine the quantity of analytes.
Gravimetric Method
An analytical method that uses the measurement of liquid volumes to determine analyte concentrations.
Volumetric Method
A method that uses electrical properties of a substance, such as current or voltage, to analyze its composition.
Electroanalytical Method
A technique involving the interaction of electromagnetic radiation with matter to measure analytes.
Spectroscopy Method
A mixture in which the composition is not uniform throughout.
Heterogeneous
A test or analysis to determine the presence, amount, or functional activity of a substance.
Assay
The process of collecting a portion of material to represent the whole for analysis.
Sampling
Repeated measurements or samples analyzed under the same conditions to assess precision.
Replicates
Substances that hinder the accurate measurement of an analyte by affecting the analysis.
Interferences
The components of a sample other than the analyte of interest.
Matrix
Methods that measure only the analyte of interest, even in complex mixtures.
Specific Techniques
Methods that target specific analytes but may include minor contributions from other substances.
Selective Techniques
The process of relating the response of an instrument to known quantities of analyte.
Calibration
The number of particles in one mole of a substance.
6.022×10^23; Avogadro’s Number
The mass of one mole of a substance, typically expressed in grams per mole.
Molar Mass
The average mass of an atom of an element, considering all its isotopes.
Atomic Mass
Atoms of the same element with different numbers of neutrons and, therefore, different masses.
Isotope
A measure of concentration expressed as moles of solute per liter of solution.
Molarity
The calculation of reactants and products in a chemical reaction based on balanced equations.
Stoichiometry
A measure of concentration expressed as moles of solute per kilogram of solvent.
Molality
The percentage of a component’s mass relative to the total mass of the mixture or solution.
Weight Percent
The percentage of a component’s volume relative to the total volume of the mixture.
Volume Percent
The percentage of a solute’s mass relative to the solution’s total volume.
Weight/Volume Percent
a unit of concentration equal to 1 part in 1,000 parts.
Parts per thousand (PPTh)
a unit of concentration equal to 1 part in 1,000,000 parts.
parts per million (PPM)
a unit of concentration equal to 1 part in 1,000,000,000 parts.
Parts per billion (PPB)
a unit of concentration equal to 1 part in 1,000,000,000,000 parts
Parts per trillion (PPTr)
The measured amount of product obtained from a reaction.
Actual Yield
The calculated amount of product expected based on the stoichiometry of the reaction.
Theoretical Yield
proton donors
Acid
proton acceptors
base
The species formed when an acid donates a proton.
Conjugate Base
The species formed when a base accepts a proton.
Conjugate Acid
The closeness of a measurement to the true or accepted value.
Accuracy
The consistency or repeatability of a set of measurements.
Precision
Consistent and predictable error affecting all measurements in the same way.
Systematic Error
Unpredictable variations in measurements caused by uncontrollable factors.
Random Error
A homogeneous mixture of two or more substances.
Solution
The process of converting a measurement from one unit to another using dimensional analysis.
Unit Conversion
Adjusting the coefficients in a chemical equation to satisfy the law of conservation of mass.
Balancing a Chemical Reaction
A unit representing
6.022×10^23 entities of a substance.
Mole
Absorption of UV/visible light by molecules corresponding to electronic transitions.
UV-Vis Spectroscopy
Absorption of IR radiation causes molecular bond vibrations; it detects and measures these absorptions.
FTIR Spectroscopy
Measures light absorption by free atoms in a gaseous state at specific wavelengths.
Atomic Absorption Spectroscopy
Uses a graphite furnace to atomize the sample, providing greater sensitivity than flame AAS.
Graphite Furnace AAS (GFAAS)
Excited atoms emit light at characteristic wavelengths; emissions are measured for analysis.
Atomic Emission Spectroscopy (AES)
Separates ions based on mass-to-charge ratio (m/z), providing molecular weight and structure.
Mass Spectroscopy (MS)
Generates and manipulates electron beams using electric/magnetic fields; historically used in displays and oscilloscopes.
Cathode Ray Tube
a laboratory procedure used to determine the presence, amount, or concentration of a substance in a sample
assay
unit of weight
N
unit of mass
kg
It refers to the amount of a substance (solute) dissolved in a given volume of solvent or solution. It is commonly expressed in units such as molarity (moles per liter), molality (moles per kilogram), weight percent, or parts per million (PPM).
concentration
It have the same number of protons but a different number of neutrons, which results in different atomic masses.
isotopes
