Mole Concept and Atomic Structure Flashcards

A comprehensive set of practice flashcards covering basic chemistry concepts, laws of chemical combination, and atomic structure based on the lecture notes.

Matter

Anything which has some mass and occupies some space.

Chemistry

The branch of science that studies the composition, structure, properties, and reactions of matter, often called the science of molecules and their transformations.

Alchemy and Iatrochemistry

The period (1300-1600 CE) from which modern chemistry developed, where researchers aimed to convert base metals into gold and discover the elixir of life.

Paramanu

The ancient Indian concept of the atom as an indivisible particle, proposed by Acharya Kanada around 600 BCE.

Cisplatin and Taxol

Two important life-saving drugs derived from chemical knowledge that are used in the treatment of cancer.

AZT (Azidothymidine)

An important drug used for helping victims of AIDS.

Pure Substances

Matter consisting of constituent particles that are all the same, categorized into elements (made of only one type of atom) and compounds (atoms of different elements combined).

Homogeneous Mixture

A type of mixture where the components are so thoroughly mixed that they cannot be differentiated by the naked eye.

Heterogeneous Mixture

A type of mixture where the constituent substances can be differentiated by the naked eye.

Precision

The closeness of various measurements for the same quantity to one another.

Accuracy

The closeness of a particular measurement to the true value of the result.

Law of Conservation of Mass

A law given by Antoine Lavoisier stating that mass is neither created nor destroyed during a chemical reaction.

Law of Definite Proportions

A law given by Joseph Proust stating that a given compound always contains elements in a fixed ratio by mass.

Law of Multiple Proportions

A law given by John Dalton stating that when elements combine in different ratios to form multiple compounds, they do so in simple whole number ratios.

Avogadro's Law

A law proposed by Amedeo Avogadro stating that equal volumes of gases at the same temperature and pressure contain an equal number of molecules.

Atomic Mass Unit (amu)

A mass exactly equal to $\frac{1}{12}$ the mass of one Carbon-12 atom, equivalent to approximately $1.66 \times 10^{-24}\,g$.

Avogadro Number ($N_A$)

The number of particles present in one mole of a substance, which is equal to $6.022 \times 10^{23}$.

Empirical Formula

The formula that represents the simplest whole number ratio of various atoms present in a compound.

Molecular Formula

The formula that expresses the actual number of atoms of each element present in one molecule of a compound.

Limiting Reagent

The reactant in a chemical reaction that is completely consumed first, thereby limiting the amount of product formed.

Molarity (M)

A temperature-dependent concentration unit defined as the number of moles of solute present in $1\,L$ of solution.

Molality (m)

A temperature-independent concentration unit defined as the number of moles of solute present in $1\,kg$ of solvent.

Isotopes

Atoms of the same element that have the same atomic number but different mass numbers, such as $^1H$, $^2H$, and $^3H$.

Isobars

Atoms that have the same mass number but different atomic numbers, such as $^{40}Ar$ and $^{40}Ca$.

Heisenberg Uncertainty Principle

The principle stating it is impossible to determine simultaneously the exact position and exact velocity (or momentum) of a sub-atomic particle.