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SRS Study Cards > CHEMISTRY REVIEW > Flashcards

CHEMISTRY REVIEW Flashcards

REVIEW

1
Q

Matter

A

anything that has mass and takes up space

takes up space means volume

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2
Q

Mass

A

the amount of material in a substance, the amount of stuff that’s present and takes up the space

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3
Q

describe matter as a solid

A

has definite shape and definite volume

particles are closely packed and rigidly held in fixed positions

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4
Q

describe matter as a liquid

A

has no definite shape, but has a definite volume

the particles are not bound in fixed positions and can slide past and around each other

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5
Q

describe matter as a gas or vapor

A

has no definite shape and no definite volume

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6
Q

occurs when somethin in solid form changes into liquid

A

melting

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7
Q

melting point

A

the temperature at which matter changes from a solid to a liquid

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8
Q

the change from liquid to solid

A

freezing

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9
Q

the temperature at which a liquid changes into a solid

A

freezing point

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10
Q

boiling

A

the change from liquid to gas (vapor) at the boiling point

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11
Q

evaporation

A

the change from liquid to gas (vapor) below the boiling point

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12
Q

the term that describes the change from gas (vapor) to liquid

A

condensation

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13
Q

when a liquid, gas, or solid is cooled the molecules

A

lose kinetic energy and slow down

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14
Q

increases of kinetic energy and speeds up molecules

A

when a solid, liquid, or gas is heated

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15
Q

sublimation

A

the change from a solid directly to a gas (vapor)

dry ice is frozen carbon dioxide

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16
Q

Examples of physical properties

A

density, specific gravity, shape, hardness, odor, color, solubility, melting point, and boiling point

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17
Q

chemical properties

A

characteristics of matter that allow it to combine or react with other matter

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18
Q

Matter can not be created or destroyed

A

Law of Conservation of Mass/Energy

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19
Q

two or more pure substances that are physically combined in variable proportions

A

Mixture

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20
Q

solution

A

homogeneous mixtures

molecules of the two bonded substances intermix evenly but are not bound together by intermolecular bonds

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21
Q

solute

A

the substance in a solution that is dissolved into another substance
ie sugar in water and oxygen in our atmosphere

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22
Q

the solution that dissolves the other substance

ie water in our sugar water and nitrogen in our atmosphere

A

solvent

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23
Q

solubility

A

refers to how easily a substance will or will not dissolve readily it is said to be soluble.

salt and sugar are soluble in water
silicon dioxide (sand) is insoluble in water

Soluble is means that the compound is able to break apart into fragments too small to be caught by any filter

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24
Q

homogeneous sample of matter that has the same composition and properties, whatever its source

A

pure substance

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25
Q

compound

A

pure substances composed of two or more different elements chemically combined in fixed proportions

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26
Q

two or more atoms chemically bonded together

the smallest piece of a compound that can exist and keep its properties

A

molecule

molecules of an element (diatomic)

molecules of an compound

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27
Q

the higher the atomic number the more energy levels the atom has, the electrons are further from the nucleus, and more reactive the atom

A

How the atomic number influences the chemical properties of an atom

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28
Q

protons

A

carries a positive electrical charge in the nucleus

is about 1 amu

give atoms their identity, identifies the element

atomic number

the periodic table is arranged the order of increasing atomic number

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29
Q

The two regions of an atom

A

the nucleus and the electron cloud

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30
Q

subatomic particles that reside in the nucleus along with the proton

neutral charge

1amu

A

neutrons

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31
Q

atomic mass number

A

sum of protons and neutrons in the nucleus

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32
Q

Isotopes

A

Atoms with the same number of protons but different number of neutrons

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33
Q

negatively charged subatomic particle

makes up an elements volume through the electron cloud

.0055amu

A

electron

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34
Q

Reactivity for columns 1 and 2
Reactivity for columns 16 and 17
Reactivity for column 18

A

Increases as you go down the column
Increases as you go up the column
Are unreactive because their valence shell is full

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35
Q

valence electron
valence shell

A

electrons in the highest energy level or electrons in the outermost shell

the outermost shell or the highest energy level

the most chemically active electrons

can also mean ionic charge

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36
Q

Why does bonding happen on the outer most electrons

A

the elements strive to achieve an outer shell that is full of electrons

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37
Q

ionization

A

occurs when electrons are gained or lost by an atom or compound

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38
Q

anion

A

negatively charged ions formed when the atom gains electrons

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39
Q

cation

A

positively charged ions formed when the atom losses electrons

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40
Q

period

A

each row on a periodic table

all the elements have same number of energy shells

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41
Q

groups

A

the columns on a periodic table

they contain the same number of electrons on the valence shell

valence shells have the same electron configuration

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42
Q

Number of electrons per shell

A

The inner or first shell needs 2 electrons to be full
The rest of the shells want 8 electrons

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43
Q

The stair step on the periodic table is the ____

These elements have characteristics of metals and non-metals depending on the conditions

Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, and Polonium

A

Metalloids

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44
Q

Unreactive gasses because their valence shell is full

A

Inert or Noble Gases

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45
Q

In groups one and two the reactive increases going _____ the column

A

Down

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46
Q

First write out chemical notation (think isotopes)

What does he large X represent

A

The element’s symbol

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47
Q

First write out chemical notation (think isotopes)

What does the Z represent

A

The atomic number and the number of protons

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48
Q

First write out chemical notation (think isotopes)

What letter represents the mass number

A

A is the mass number and tells us the number of protons and neutrons

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49
Q

First write out chemical notation (think isotopes)

What does the + or - represent

A

The + or - denotes ionic charge. Charge is based on excess (-) or deficiency (+) of electrons.

50
Q

First write out chemical notation (think isotopes)

How do we denote the number of atoms in the molecule?

A

The n on the right bottom

51
Q

Atomic weight

A

the weighted average of the masses of all of the an element’s naturally occurring isotopes

52
Q

the sum of the atomic weights of all the atoms in the molecule

A

molecular weight

53
Q

The mole

A

is a counting term we use, represents 6.022 x 10^23

54
Q

Gram atomic weight (gaw)

A

mass (weight) in grams of a mole of atoms

55
Q

formed when electrons are gained and lost

A

ionic bonds

56
Q

the electrostatic attraction between oppositely charged particles

A

the force that holds ionic bonds

57
Q

covalent bonding

A

two atoms share electrons in order to fill their outer shells

58
Q

the force that holds together covalent bonds

A

are the overlapping (intertwined) electrons clouds of the atoms

59
Q

the bonding in which each atom contributes its valence electrons, these electrons are delocalized, and the valence electrons are shared by many atoms

A

metallic bonding

60
Q

the purpose of a balanced equation

A

tells us the amounts of reactants and products involved, number of atoms and molecules, number of moles and mole ratios, or masses

61
Q

the quantity of heat released or absorbed during a chemical reaction

A

heat of a reaction or delta H

62
Q

exothermic reaction

A

is when energy is given off or released an example is a burning candle

63
Q

endothermic reaction

A

when energy is absorbed and example is cooking an egg, baking bread, water evaporation, and melting ice cubes.

64
Q

the minimum amount of energy required to start a chemical reaction

A

activation energy

65
Q

how rapidly a chemical reaction progresses, and whether the reaction is speeding up or slowing down as it progresses

A

reaction rate

66
Q

factors that affect reation rate

A

nature of the reactant- how reactive the react is
surface area- when solids react the chemical reaction takes place on the surface of the solid
concentration- is a measure of how many atoms ore molecules or ions are contained in a given volume of material
temperature
catalyst

67
Q

catalyst

A

substance that changes the rate of a chemical reaction but doesn’t get permanently consumed during the reaction

68
Q

reversible reaction

A

a reaction in which the products can react to re-form the reactants

69
Q

chemical equilibrium

A

the state in which the rate of the forward and reverse reauctions are exactly equal

70
Q

shifting the equilibrium

A

means the reaction is shifted to favor either the forward or the reverse reaction. By adjusting the reaction conditions and quantities of materials, we can shift the equilibrium to reach a more desired state.

71
Q

the state of a solution when it holds the maximum amount of a dissolved substance at a given temperature.

A

saturation

72
Q

a solution that contains the maximum amount of dissolved solute

A

saturated solution

73
Q

super saturated solution

A

a solution that contains more dissolved solute than a saturated solution under the same conditions

74
Q

chemical concentration

concentration in context of a chemical reaction

A

is a measurement of the amount of solute present in a given amount of solvent or solution.

The total mass of reactants in a given volume of material

75
Q

a solution with a relatively small amount of solute as compared to the amount of solvent

A

dilute solution

76
Q

the process by which the concentration of solution is increased

A

concentration process

77
Q

the process by which the concentration of a solution is decreased

A

dilution process

78
Q

electrolytes

A

substances that form ions when they dissolve in water

ionic compounds composed of both negative and positive ions

79
Q

compounds that dissolve in water to produce hydrogen ions

A

acids

80
Q

neutralization

A

the reaction of hydrogen ions and hydroxide ions to form a salt and water

81
Q

the negative logarithm of the hydrogen ion concentration of a solution

A

pH

82
Q

pH of a solution grater than 7

A

basic

83
Q

the pH of a solution is less than 7

A

acid

84
Q

the pH is equal to 7

A

neutral

85
Q

Three reasons we treat water

A

to minimize corrosion
to minimize radiation
to minimize fouling of heat transfer surfaces

86
Q

What happens to corrosion rates of metals when there is impurities

A

The corrosion rate of metals is increased by impurities. High corrosion rates can lead to the failure of components or systems

87
Q

mixed resin beds filter ___

A

all dissolved solids

88
Q

IT is important to maintain the proper pH of a water-based system in order to

A

control the rate of corrosion

89
Q

Deaeration
filtration
ion exchange

A

Methods to filter water

90
Q

Deaeration

A

method used to remove or strip dissolved gases from water and vent them into the atmosphere

91
Q

Cation and Anion resin beds can control pH by

A

cation resin releasing hydrogen ions increasing the pH

anion resin releasing hydroxide ions decreasing the pH

92
Q

Sand
Activated charcoal (treated to increase absorptive power)
anthracite
diatomaceous earth
ion exchanger resin

A

five common filtration media

93
Q

Agitators are used in ion exchangers

A

during initial resin loading, after resin replacement, and during resin generation

94
Q

water flows what direction through the ion exchanger (IX)

A

From top to bottom

95
Q

The bottom port of the Ion Exchanger is used to _____

A

remove resin beads

96
Q

influent water

A

waste water, makeup water, water to be filtered

97
Q

pure water, filtered water

A

effluent water

98
Q

Resin channeling

A

A condition in which the resin allows a direct flow of water through the ion exchange. Flow channels are established from the inlet to the outlet of the ion exchanger, which allows water to flow essentially unrestricted through the resin via these paths.

99
Q

small particles that may clog the retention elements in the ion exchanger reducing ion exchanger flow

A

resin fines

100
Q

oxidation-reduction reactions

A

chemical change that electrons are gained or lost

101
Q

Reduction

A

is when a chemical gains one or more electrons

102
Q

when a chemical loses one or more electrons

A

oxidation

103
Q

the surface of a metal undergoes a slow, relatively uniform deterioration and removal of metal

A

general corrosion

104
Q

the mechanism by which general corrosion occurs is

A

the metal ionizes, dissolves into solution, and may form other compounds such as metal oxides

105
Q

As temperature changes corrosion changes

A

As temperature increases corrosion increases

As temperature decreases corrosion decreases

106
Q

Oxygen causes corrosion to

A

as oxygen increases corrosion increases

as oxygen decreases corrosion decreases

107
Q

metal surface, condition, and composition effect corrosion

A

Deposits of insoluble impurities and irregular metal surfaces create areas where local corrosion can initiate and proceed at a faster than normal rate. A pitted, uneven surface where these impurities can deposit is more susceptible to corrosion that a polished, flat surface.

108
Q

Protective layer, passivity, and corrosion

A

Removal of the protective layers will increase the rate of corrosion.

109
Q

Commonly used technique to prevent or slow corrosion

A

Separate the metal from water in the environment. This can be accomplished by painting the surface or applying a protective coating to the metal surface.

110
Q

The process in which an oxide layer to form between the metal and the environment. This process results in the metal being separated from its environment.

A

Passivity

111
Q

Iron corrosion can be slowed by two factors

A

pH and oxygen. If possible, systems containing iron should be operated in the pH range (4-10) that promotes the lowest corrosion rate.

112
Q

Galvanic corrosion

A

when two dissimilar metals with different potentials are placed in electrical contact in an electrolyte (an electricity conducting fluid)

113
Q

a metal that is more easily oxidized than the metal to be protected (higher on the electromotive series table)

a metal that is more easily oxidized than the metal to be protected

A

sacrificial anode

114
Q

pitting corrosion

A

occurs where the corrosion site becomes fixed in a small area and the formation of holes takes place in an otherwise unaffected area.

115
Q

a type of pitting corrosion that occurs specifically within the low flow region of a crevice

A

crevice corrosion

116
Q

stress corrosion cracking (SCC)

A

a form of corrosion that can produce spontaneous failure of metals as the result of the combined action of a corrosive environment and tensile (pulling apart) stress

117
Q

Two main ways to reduce stress corrosion cracking

A

to reduce tensile stresses

to eliminate or reduce severity of the corrosive environment

118
Q

Why is using alternate materials not a great option for reducing stress corrosion cracking

A

The cost or fabrication difficulties eliminates this option for most applications

119
Q

Tensile stress

A

type of stress that occurs when a material is being pulled apart, stretched, or elongated

120
Q

the reverse of tensile stress, occurs when a material is being pressed together, compacted or squeezed

A

compressive

121
Q

exists when two parts of a material are loaded causing them to tend to slide across each other

A

shear stress

SRS Study Cards (3 decks)

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