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

0.0(0)
studied byStudied by 2 people
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
Card Sorting

1/107

flashcard set

Earn XP

Description and Tags

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

Study Analytics
Name
Mastery
Learn
Test
Matching
Spaced

No study sessions yet.

108 Terms

1
New cards

homogeneous mixture (solution)

A mixture that is uniform throughout at the molecular level.

2
New cards

heterogeneous mixture

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

3
New cards

suspensions

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

4
New cards

first characteristic of a solution

The distribution of particles in a solution is uniform.

5
New cards

second characteristic of a solution

The components of a solution do not separate on standing.

6
New cards

third characteristic of a solution

A solution cannot be separated into its components by filtration.

7
New cards

fourth characteristic of a solution

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

8
New cards

fifth characteristic of a solution

Solutions are almost always transparent.

9
New cards

sixth characteristic of a solution

Solutions can be separated into pure components.

10
New cards

solvent

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

11
New cards

solute

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

12
New cards

solution

Comprises of a solute and a solvent.

13
New cards

solubility

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

14
New cards

miscible

When liquids are completely soluble in other liquid solvents.

15
New cards

saturated

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

16
New cards

unsaturated

Any solution containing a lesser amount of solute.

17
New cards

supersaturated

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

18
New cards

seeding

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

19
New cards

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.

20
New cards

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.

21
New cards

concentration

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

22
New cards

nature of the solvent and solute

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

23
New cards

temperature

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

24
New cards

pressure

has little effect on the solubility of liquids or solids.

25
New cards

percent concentration

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

26
New cards

Molarity

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

27
New cards

dilution

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

28
New cards

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

A unit used to express concentration for very dilute solutions.

29
New cards

molality

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

30
New cards

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.

31
New cards

normality

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

32
New cards

aqueous solution

A solution in which water is the solvent.

33
New cards

non-aqueous solution

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

34
New cards

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.

35
New cards

anhydrous crystal

The crystal without its water of hydration.

36
New cards

hygroscopic

Some anhydrous crystals become hydrated upon standing in air.

37
New cards

electrolyte

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

38
New cards

non-electrolyte

A substance that does not conduct electricity.

39
New cards

strong electrolyte

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

40
New cards

weak electrolytes

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

41
New cards

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

2 basic characteristics of colloidal systems

42
New cards

Tyndall effect

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

43
New cards

Brownian motion

The random motion of colloid-size particles.

44
New cards

colligative property

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

45
New cards

Vapor-pressure lowering

boiling-point elevation

freezing-point depression

osmotic pressure

four colligative properties of solutions

46
New cards

vapor pressure lowering

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

47
New cards

boiling point

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

48
New cards

osmosis

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

49
New cards

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.

50
New cards

Osmolarity

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

51
New cards

isotonic solutions

Solutions with the same osmolarity.

52
New cards

hypotonic solution

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

53
New cards

hemolysis

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

54
New cards

hypertonic solution

A solution with higher osmolarity than red blood cells.

55
New cards

Arrhenius acid

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

56
New cards

Arrhenius base

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

57
New cards

Bronsted-Lowry acid

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

58
New cards

Bronsted-Lowry base

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

59
New cards

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.

60
New cards

Lewis theory acid

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

61
New cards

Lewis theory base

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

62
New cards

strong acid

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

63
New cards

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.

64
New cards

nuclear chemistry

The subfield of chemistry dealing with radioactivity and nuclear processes.

65
New cards

nuclear reaction

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

66
New cards

nuclide

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

67
New cards

radioactive nuclide (radionuclide)

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

68
New cards

radioactivity

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

69
New cards

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.

70
New cards

parent nuclide

Nuclide that undergoes decay.

71
New cards

daughter nuclide

Nuclide that is produced from the decay.

72
New cards

nuclear fission

The fragmentation of larger nuclei into smaller ones.

73
New cards

nuclear fusion

Two light nuclei merge to form a single heavier nucleus.

74
New cards

Henri Becquerel

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

75
New cards

Marie Curie

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

76
New cards

Earnest Rutherford

Discovered alpha, beta and gamma radiation.

77
New cards

Alpha radiation

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

78
New cards

Beta radiation

Slight penetrating power (stopped by clothing).

79
New cards

Gamma radiation

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

80
New cards

half-life of radioactive decay

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

81
New cards

What is nuclear medicine?

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

82
New cards

What is Transmutation?

Involves converting a chemical element into another less harmful one.

83
New cards

Raoult’s Law

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

84
New cards

Semi- permeable membrane

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

85
New cards

Conjugate Acid

It is the particle formed that has received the proton

86
New cards

Conjugate base

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

87
New cards

radiation

the penetrating rays and particles emitted by a radioactive source.

88
New cards

radioactivity

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

89
New cards

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.

90
New cards

Nuclear Equation

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

91
New cards

Alpha particles

Beta particles

Gamma rays

Types of radiation

92
New cards

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.

93
New cards

Neutron capture

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

94
New cards

Electron capture

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

95
New cards

Neutrino

it is emitted from the nucleus.

96
New cards

Intensity - energy flux

measures the number of particles of photons emerging per unit

97
New cards

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

98
New cards

Energy

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

99
New cards

Roentgens (R)

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

100
New cards

rads

measures of the radiation absorbed from a radiation course.