Sanitary Chemistry Lecture Notes

Flashcards relating to Sanitary Chemistry.

Acid Solution

A solution with added acid to lower the pH level.

Acid

The building blocks of chemistry, maintaining a balanced charge with positive and negative particles.

Proton

Positively charged particle found in the nucleus.

Neutron

Particle with no charge found in the nucleus.

Electron

Negatively charged particle.

Compound Law

The lightest number for a compound to obey this law.

Nucleus

Consists of protons and neutrons.

Modern Periodic Table

Arranged by atomic number.

Periodic Table Properties

Elements in a group have similar chemical properties, while elements in a period have different chemical properties.

Alkali Metals

Group 1A elements (except hydrogen).

Alkaline Earth Metals

Group 2A elements.

Boron Family

Group 3A elements.

Carbon Family

Group 4A elements.

Nitrogen Family

Group 5A elements.

Oxygen Family

Group 6A elements (Chalcogens).

Halogens

Group 7A elements.

Noble Gases

Group 0 or 8A elements.

Metals

Shiny solids at room temperature that conduct heat and electricity well and are malleable and ductile.

Nonmetals

Generally gases or dull, brittle solids at room temperature and conduct heat and electricity poorly.

Metalloids

Semi-metals.

Atomic Size

The size of the atoms; increases as the number of shells increases going down a group, generally decreases going across a period.

Ionization Energy

The amount of energy required to remove an electron from an atom; decreases down a group, increases across a period.

Electron Affinity

The amount of energy released when an electron is added to an atom; decreases down a group of non-metals, increases across a period.

Electronegativity

The tendency of an atom to attract electrons towards itself; decreases down a group, increases across a period.

Molecule

A structure consisting of two or more atoms that are bound chemically and behave as an independent unit.

C7H5N3O6

TNT

Ca(OH)2

Slaked lime.

CaO

Quicklime.

(NH4)2SO4

Ammonium Sulfate.

Ba3(PO4)2

Barium Phosphate.

SnO2

Stannic Oxide.

Equivalence

A measure of the combining power of an element or group expressed numerically by the number of hydrogen atoms it can displace or combine with.

Reducing Agent

Substance that donates electrons.

Oxidizing Agent

Substance that accepts electrons.

Molarity

The mass of solute per volume of solution.

Normality

The number of gram equivalent weights of solute per liter of solution.

Acid-Base Reactions (Neutralizations)

Acid added to water dissociates into hydrogen ions and anion radicals resulting in an acid solutions.

Gas Producing Reactions

Chemical processes involving the formation of gaseous product

Turbidity

Water that contains suspended matter that interferes with the passage of light through the water by scattering or absorbing rays or in which visual depth is restricted.

Turbidity

The cloudiness or haziness of a fluid caused by individual particles.

Boyle's Law

The volume of a gas varies inversely with its pressure at a constant temperature.

Charles Law

The volume of gas at constant pressure varies in direct proportion to the absolute temperature.

Generalized Gas Law

Law combining Boyle's and Charles' Laws for a given quantity of gas.

Dalton's Law of Partial Pressure

The partial pressure of each gas is proportional to the amount of gas in the mixture.

Raoult's Law

Deals with the vapor pressure of an ideal solution. The partial pressure of any component depends first on how volatile it is, and second, on how much of it is present in the solution.

Ideal Solution

Defined as one whose properties are a molar average of the corresponding properties of the components of that solution.

Henry's Law

The weight of any gas that will dissolve in a given volume of liquid at a constant temperature is directly proportional to the pressure that the gas exerts above the liquid.

Graham's Law

The rates of diffusion of gases are inversely proportional to the square root of their density.

Gay Lussac's Law of Combining Volume

The volumes of all gases that react and that are produced during the course of reaction are related numerically to one another as a group of small, whole numbers.

JTU or Jackson Turbidity Unit

Turbidity Unit, measured by means of Jackson tube turbid meter or Jackson Candle turbidimeter.

NTU

Nephelometric Turbidity Unit.

PH indicator

Indicators that exhibit significant color changes in a particular range involved.

pH

Measures the acidity and alkalinity condition of a solution.

pH

Mathematical system developed by Danish chemist Søren Sørenson as an abbreviation for potential of hydrogen.

Blue Litmus Paper

Turns red under acidic conditions and blue under basic conditions.

Red Litmus Paper

Turns blue under basic conditions and red under acidic conditions.

Alkalinity

A measurement of the capacity to neutralize acids.

Carbon Dioxide

Natural component of natural waters by absorption from atmosphere.

Algae

Effective agent in water having pH less than 4.

Carbon Dioxide

Effective agent in water having pH greater than 4.

Hydrocarbons

The simplest type of organic compound contain only H and C atoms.

Aliphatic compounds

Organic compounds formed in a chain

Aromatic compounds

Ring compounds are called

Alkanes

A hydrocarbon that contains only single bond.

Alkenes

Are also called ethylene (ethene) series.

Alkynes

Or called as acetylene series.

Alkanes

Are referred to as saturated hydrocarbons.

Paraffins

Longer aliphatic compounds in the form of waxes.

Methane CH4

Simplest hydrocarbon.

Olefins

Unsaturated Hydrocarbons - multiple bonds between some carbon atoms

Aromatic hydrocarbons

Contains one or more benzene rings

Alcohols

Hydrocarbons in which at least one or more hydrogen atom is substituted by a hydroxyl group.

Halogenated hydrocarbons

With at least one or more atom from the halogen group

Glycols and derivatives

Two hydrogen atoms substituted by a hydroxyl groups.

Carbonyl group

The C=O grouping of atoms.

Aldehyde

An organic compound that contains the carbonyl functional group in which the carbonyl C is also bonded to H.

Carboxylic acids

The highest state of oxidation that an organic radical can achieve.

Methane

Simplest hydrocarbon.

Alkane

Type of Compound: Saturated hydrocarbon, Proper name ending: -ane

Alkene

Type of Compound: Olefin, Proper name ending: -ene

Alkyne

Type of Compound: Acetylene, Proper name ending: -yne

Aldehyde

Type of Compound: Aldehyde, Proper name ending: -al

Ketone

Type of Compound: Ketone, Proper name ending: -one

Carboxylic acid

Type of Compound: Carboxylic acid, Proper name ending: -oic acid

Acid

Added to lessen the pH level.

Nucleus

Consists of proton and neutrons.

NOTE

Elements in a group have similar chemical properties and elements in a period have different chemical properties.

Element Group

Elements in a group have similar chemical properties.

Element Period

Elements in a period have different chemical properties.

METALS

Shiny solids at room temperature that conduct heat and electricity well and are malleable and ductile.

NONMETALS

Generally gases or dull, brittle solids at room temperature and conduct heat and electricity poorly.

METALLOIDS

Semi-metals.

Atomic Size

The size of the atoms become bigger as the number of shells increases.

Atomic Size (Group Trend)

Going down any group in the table there is a large increase in atomic size.

Atomic Size (Period Trend)

Going across any period, there is a small but rather general decrease in size of atomic radius.

Ionization energy

The amount of energy required to remove an electron from an atom.

Electron affinity

The amount of energy released when an electron is added to an atom.

Electronegativity

Defined as the tendency of that atom to attract electrons towards itself.

Molecule

A structure consisting of two or more atoms that are bound chemically and behave as an independent unit.

TURBIDITY

Water that contain suspended matter that interfere with the passage of light through the water by scattering or absorbing rays or in which visual depth is restricted.