Solution, Colliods, Acids, Bases and Salts, and Nuclear Chemistry

Flashcards for reviewing solutions, colloids, acids, bases and salts, and nuclear chemistry concepts.

homogeneous mixture (solution)

A mixture that is uniform throughout at the molecular level.

heterogeneous mixture

A mixture in which the components are separated from each other by well-defined boundaries.

suspensions

Mixtures that may look homogeneous but do not have the transparency of air or seawater.

first characteristic of a solution

The distribution of particles in a solution is uniform.

second characteristic of a solution

The components of a solution do not separate on standing.

third characteristic of a solution

A solution cannot be separated into its components by filtration.

fourth characteristic of a solution

For any given solute and solvent, it is possible to make solutions of many different compositions.

fifth characteristic of a solution

Solutions are almost always transparent.

sixth characteristic of a solution

Solutions can be separated into pure components.

solvent

The fraction of a solution in which the other components are dissolved.

solute

A substance that is dissolved in a solvent to produce a solution.

solution

Comprises of a solute and a solvent.

solubility

The maximum amount of the solid that will dissolve in a given amount of a particular solvent at a given temperature.

miscible

When liquids are completely soluble in other liquid solvents.

saturated

When a solvent contains all the solute it can hold at a given temperature.

unsaturated

Any solution containing a lesser amount of solute.

supersaturated

A solution that contains more solute in the solvent than it can normally hold at a given temperature under equilibrium conditions.

seeding

Adding a crystal of the solute to crystallize the excess solute.

Henry's Law

Describes the solubility of a gas in a liquid, stating that the higher the pressure in a gas, the greater is the solubility of a gas in a liquid.

bends

A condition that occurs when divers come up and the pressure on their bodies decreases, causing the solubility of nitrogen in their blood to decrease, forming small bubbles.

concentration

The amount of a solute dissolved in a given quantity of solvent.

nature of the solvent and solute

follows the principle of 'like dissolves like'? polar solutes will dissolve in polar solvents and vice versa.

temperature

The solubility of solids in liquids generally increases as temperature increases.

pressure

has little effect on the solubility of liquids or solids.

percent concentration

the weight of solute per volume of solution? The number of grams of solute in 100 mL of solution.

Molarity

The number of moles of solute dissolved in 1 L of solution. The units are moles per liter.

dilution

A process where solutions are prepared by diluting concentrated solutions rather than by weighing out pure solute.

parts per million (PPM) and parts per billion (PPB)?

A unit used to express concentration for very dilute solutions.

molality

The number of moles of solute dissolved in 1000 g (1 kg) of solvent.

mole fraction

it is defined as the number of moles (n) of that component, divided by the total number of moles of all components in the solution.

normality

Defined as the number of grams equivalent weight of solute per liter of solution.

aqueous solution

A solution in which water is the solvent.

non-aqueous solution

A solution in which a substance other than water is the solvent.

water of hydration

The attraction between ions and water is so strong that for many solids, water molecules are a part of the crystal structure.

anhydrous crystal

The crystal without its water of hydration.

hygroscopic

Some anhydrous crystals become hydrated upon standing in air.

electrolyte

A substance that conducts electric current and separates into ions when dissolved in water.

non-electrolyte

A substance that does not conduct electricity.

strong electrolyte

A compound that dissociates completely to ions in an aqueous solution.

weak electrolytes

Compounds that only partially dissociate to ions in an aqueous solution.

They scatter light and therefore appear turbid, cloudy, or milky and form stable dispersions, they form stable dispersions

2 basic characteristics of colloidal systems

Tyndall effect

A phenomenon in which light passing through a colloid is scattered by colloidal-sized particles.

Brownian motion

The random motion of colloid-size particles.

colligative property

A physical property of a solution that depends only on the quantity of solute particles and not on their chemical identities.

Vapor-pressure lowering

boiling-point elevation

freezing-point depression

osmotic pressure

four colligative properties of solutions

vapor pressure lowering

The __________ of a solution of a nonvolatile nonelectrolyte is always lower than the vapor pressure of the pure solvent.

boiling point

The __________ of a substance is the temperature at which the vapor pressure of the substance equals atmospheric pressure.

osmosis

The passage of a solvent through a semipermeable membrane separating a dilute solution (or pure solvent) from a more concentrated solution.

osmotic pressure

The amount of external pressure that must be applied to the more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane.

Osmolarity

The molarity multiplied by the number of particles produced by each formula unit of solute.

isotonic solutions

Solutions with the same osmolarity.

hypotonic solution

A solution with lower osmolarity than blood plasma and red blood cells.

hemolysis

The swelling and bursting of red blood cells because they cannot resist the increase in osmotic pressure when put into a hypotonic solution.

hypertonic solution

A solution with higher osmolarity than red blood cells.

Arrhenius acid

An acid is a substance that yields hydrogen ions in aqueous solution.

Arrhenius base

A base is a substance that yields hydroxide ions in aqueous solution.

Bronsted-Lowry acid

An acid is a substance that donates protons (H+) to other substances.

Bronsted-Lowry base

A base is a substance that accepts protons from other substances.

Amphiprotic or Amphoteric Substance

A substance that can either donate or accept a proton and thus can function as either a Brønsted-Lowry acid or a Brønsted-Lowry base.

Lewis theory acid

An acid is any specie that is capable of accepting a pair of electrons to form a coordinate covalent bond.

Lewis theory base

A base is any specie that is capable of donating a pair of electrons to form a coordinate covalent bond.

strong acid

Transfers ~100% of its protons to water in an aqueous solution and yields a weak conjugate base.

weak acid

Transfers only a small % of its protons to water in an aqueous solution and the weaker the acid, the stronger its conjugate base.

nuclear chemistry

The subfield of chemistry dealing with radioactivity and nuclear processes.

nuclear reaction

A reaction in which changes occur in the nucleus of an atom.

nuclide

An atom with a specific atomic number and a specific mass number.

radioactive nuclide (radionuclide)

A nuclide with an unstable nucleus from which radiation is spontaneously emitted.

radioactivity

Spontaneous emission of particles from the decay of certain nuclides or due to an adjustment of their internal structure.

radioactive decay

Process in which a radionuclide is transformed into a nuclide of another element as a result of the emission of radiation from its nucleus.

parent nuclide

Nuclide that undergoes decay.

daughter nuclide

Nuclide that is produced from the decay.

nuclear fission

The fragmentation of larger nuclei into smaller ones.

nuclear fusion

Two light nuclei merge to form a single heavier nucleus.

Henri Becquerel

Discovered natural radioactivity in 1896 and that uranium salts gave off similar rays naturally on that of Roentgen.

Marie Curie

Coined ‘radioactivity’ and discovered radioactive elements: thorium, polonium, and radium.

Earnest Rutherford

Discovered alpha, beta and gamma radiation.

Alpha radiation

Low penetrating power (stopped by paper) and least penetrating but most ionizing.

Beta radiation

Slight penetrating power (stopped by clothing).

Gamma radiation

High-energy electromagnetic radiation and most penetrating radiation (pass through the body).

half-life of radioactive decay

The time it takes for half the nuclei present in a sample to decay.

What is nuclear medicine?

Use of radioactive isotopes as tools for both diagnosis and treatment of diseases.

What is Transmutation?

Involves converting a chemical element into another less harmful one.

Raoult’s Law

It states that the vapor pressure lowering is proportional to the mole fraction of the solute.

Semi- permeable membrane

a membrane that allows certain types of molecules to pass through it but prohibits the passage of other types of molecules.

Conjugate Acid

It is the particle formed that has received the proton

Conjugate base

is it the particle left from the acid once it has donated the proton.

radiation

the penetrating rays and particles emitted by a radioactive source.

radioactivity

the emission of particles caused by the spontaneous disintegration of atomic nuclei

Wilhelm Conrad Roentgen

(1895) He accidentally discovered an invisible radiation which is more penetrating than uv rays that it emits. He named it X-ray.

Nuclear Equation

is an equation in which the chemical symbols present represents atomic nuclei rather than atoms

Alpha particles

Beta particles

Gamma rays

Types of radiation

Positron decay

it is like a mirror image of beta decay. Something inside the nucleus of an atom breaks down, which causes a proton to became a neutron.

Neutron capture

it is a nuclear reaction in which an atomic nucleus and one more neutrons collide and merge to form heavier nucleus.

Electron capture

it is an electron from the closest energy levels falls into the nucleus which causes a proton to become a neutron.

Neutrino

it is emitted from the nucleus.

Intensity - energy flux

measures the number of particles of photons emerging per unit

Scintillation counters

contains a material called a phosphor that emits a unit of light for each alpha or beta particles or gamma rays that strikes it

Energy

The energies of different particles vary. the penetrating power of radiation depends on its energy and the mass of the particle.

Roentgens (R)

measures the energy delivered by a radiation source of the amount of exposure of radiation.

rads

measures of the radiation absorbed from a radiation course.