English-Vietnamese Bilingual Chemistry Lecture Notes

Comprehensive vocabulary flashcards covering mathematical operations, laboratory equipment, chemical reaction types, and fundamental concepts in inorganic and organic chemistry as presented in the bilingual teaching initiative.

Addition

The mathematical operation represented by $3 + 5 = 8$ (Three plus five equals to eight).

Substraction

The mathematical operation represented by $10 - 7 = 3$ (Ten minus seven equals to three).

Multiplication

The mathematical operation represented by $3 \times 5 = 15$ (Three times five equals fifteen).

Division

The mathematical operation represented by $21 : 3 = 7$ (Twenty-one divided by three equals seven).

Atomic number

The number of protons in an atom, used to identify an element as seen in the periodic table (Symbol: $Z$).

Relative atomic mass

The average mass of an atom of an element, such as $1.008$ for Hydrogen or $16.00$ for Oxygen.

Hydrochloric acid

An aqueous acid with the chemical formula $HCl(aq)$, whose corresponding anion is the chloride ion ($Cl^-$).

Nitric acid

A strong acid with the formula $HNO_3$, frequently used in redox reactions to produce Nitrogen oxides.

Burette

A graduated glass tube with a tap at one end, for delivering known volumes of a liquid, especially in titrations.

Erlenmeyer flask

A conical-shaped laboratory flask used to mix chemicals or hold solutions.

Distillation

A laboratory process (Chưng cất) used to separate components of a mixture based on differences in boiling points.

Pyrolysis

The chemical decomposition of a substance through the application of heat (Phân hủy).

Downward delivery

A method used to collect gases that are soluble in water and denser than air, such as Chlorine ($Cl_2$) and Hydrogen chloride ($HCl$).

Upward delivery

A method used to collect gases that are soluble in water and less dense than air, such as Ammonia ($NH_3$).

Displacement of water

A method suitable for collecting gases that are insoluble or slightly soluble in water, such as $CO_2$, $H_2$, or $O_2$.

Combination reaction

A type of chemical reaction where two or more reactants join to form a single product.

Displacement reaction

A chemical reaction in which one element replaces another in a compound.

Oxidation Reduction Reactions (Redox Reactions)

Reactions involving the transfer of electrons, characterized by changes in the oxidation numbers of elements.

Exothermic reaction

A chemical reaction that releases heat to its surroundings, indicated by a negative enthalpy change ($\Delta H < 0$).

Endothermic reaction

A reaction that absorbs energy from the surroundings, indicated by a positive enthalpy change ($\Delta H > 0$).

Net ionic equation

A chemical equation that shows only the species that actually participate in the reaction, omitting spectator ions.

Acid-base indicators

Substances such as litmus or phenolphthalein that change color depending on the pH of a solution.

STP

Standard Temperature and Pressure ($0^{\circ} C$ and $1\,atm$), where one mole of an ideal gas occupies $22.4\,liters$.

Molar concentration (Molarity)

The number of moles of solute per liter of solution ($mol/L$ or $M$).

Saturated solution

A solution in which no more solute can be dissolved at a given temperature.

Solubility

The maximum amount of a substance that can dissolve in a specific amount of solvent at a specific temperature.

Isotope

Atoms of the same element that have the same number of protons but different numbers of neutrons (e.g., $^{35}Cl$ and $^{37}Cl$).

Electronegativity

A measure of the tendency of an atom to attract a shared pair of electrons in a chemical bond.

Octet rule

The tendency of atoms to prefer to have eight electrons in their valence shell.

Crystal

A solid material whose constituents are arranged in a highly ordered microscopic structure (e.g., atomic, molecular, or ionic crystals).

Dynamic equilibrium

A state in a reversible reaction where the rate of the forward reaction equals the rate of the backward reaction.

Catalyst

A substance that speeds up a chemical reaction but is not consumed by it.

Efficiency (Yield)

The ratio of the actual amount of product obtained from a reaction to the theoretical maximum amount.

Alkali metals

The series of reactive metals in Group 1 of the periodic table, such as Sodium ($Na$) and Potassium ($K$).

Halogens

The reactive nonmetal elements in Group 17, including Fluorine, Chlorine, Bromine, and Iodine.

Noble gases

The chemically unreactive (inert) gases in Group 18 of the periodic table.

Dissociation

The process in which an ionic compound or a polar molecule separates into ions when dissolved in a solvent like water.

Electrolyte

A substance that produces an electrically conducting solution when dissolved in water.

Urea

A specific organic compound with the formula $(NH_2)_2CO$, often used as a nitrogen fertilizer.

Allotropes

Different physical forms in which an element can exist, such as diamond and graphite for Carbon.

Homologous series

A series of organic compounds with the same functional group and similar chemical properties (e.g., alkanes).

Isomers

Compounds with the same molecular formula but different structural arrangements or spatial orientations.