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TCEP Review > Module 1.1: General Chemistry > Flashcards

Module 1.1: General Chemistry Flashcards

1
Q

It is anything that has mass and volume

A

Matter

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2
Q

It is the amount of matter present in an object

A

Mass

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3
Q

It is the amount of space occupied by an object

A

Volume

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4
Q

It is the of
product of mass × by gravity (9.8m/s2)

A

Weight

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5
Q

What are the properties of matter

A

Intensive or intrinsic
Extensive or extrinsic

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6
Q

Properties that are independent on the amount of matter present

A

Intensive or intrinsic property

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7
Q

Intensive or intrinsic property is independent on the amount of matter present in

A

Intan DeS BOM
Density specific gravity boiling point organoleptic properties melting point

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8
Q

Intan DeS BOM

A

Intensive or intrinsic property is independent on the amount of matter present in

Intan DeS BOM
Density specific gravity boiling point organoleptic properties melting point

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9
Q

Boiling point of water

A

100° c

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10
Q

Properties that are dependent on the amount of matter present

A

Extensive or extrinsic property

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11
Q

Extensive or extrinsic property is dependent on the amount of matter present in

A

Ex kun Vom PHire
Volume
mass
pressure
heat content

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12
Q

Ex kun Vom PHire

A

Extensive or extrinsic property is dependent on the amount of matter present in

Ex kun Vom PHire
Volume
mass
pressure
heat content

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13
Q

What are the changes of matter

A

Physical change
Chemical change

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14
Q

It is observed or measured without changing the identity of matter

A

Physical change

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15
Q

___ is a change in phase

A

Physical change

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16
Q

Physically, MaVaSa ang LaVaVo

A

Physical change example melting point boiling point solubility viscosity length volume

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17
Q

Describe the change or reaction a substance undergoes

A

Chemical change

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18
Q

Change in both intrinsic and extrinsic properties

A

Chemical change

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19
Q

Examples of chemical change

A

Flammability reactability formation of gas formation precipitate formation of odor change in color

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20
Q

Fundamental states of matter

A

Solid
liquid
gas
Plasma
bose einstein condensate

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21
Q

What is the molecular motion of solid liquid gas

A

solid- vibration
liquid- gliding
gas- random motion

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22
Q

What is the shape of
solid
liquid
gas

A

solid- definite
liquid- indefinite
gas- indefinite

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23
Q

What is the volume of
solid
liquid
gas

A

solid- definite
liquid- definite
gas- indefinite

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24
Q

What is the ifa strength
solid
liquid
gas

A

solid- strongest
liquid- strong
gas- weakest

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25
Q

What is the compression of
solid
liquid
gas

A

solid- none
liquid- non or weak
gas- strongest

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26
Q

It is also known as plasma

A

Mesophase or liquid crystal

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27
Q

It is the fourth state of matter

A

Plasma

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28
Q

It has a solid and flow like properties

A

Plasma

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29
Q

Resembles those of a crystal in the formation of loosely ordered molecular arrays

A

Plasma

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30
Q

Ordered arrangement of atoms

A

Crystal lattice

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31
Q

Plasma is either

A

Smectic Nematic

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32
Q

Smectic is Nematic is

A

Smectic is a like or grease like

Nematic is thread like

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33
Q

What are the distinct crystal system

A

Cubic
Tetragonal
hexagonal
rhombic
orthoromobic
monoclinic triclinic

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34
Q

Shapes ?
Cubic
Tetragonal
hexagonal
rhombic
orthoromobic
monoclinic triclinic

A

Cubic - NaCl

Tetragonal- Urea

hexagonal- Iodoform

rhombic- Iodine

orthoromobic - Ritonavir II

monoclinic- Sucrose, Ritonavir I

triclinic- Boric acid

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35
Q

It is the degree of randomness

A

Entropy

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36
Q

It is the amount of heat present

A

Enthalpy

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37
Q

Plasma to gas

A

Decombination or deionization

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38
Q

Gas to plasma

A

Ionization

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39
Q

Gas to liquid

A

Condensation

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40
Q

Liquid to gas

A

Evaporation

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41
Q

Liquid to solid

A

Freezing or congealing

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42
Q

Solid to liquid

A

Melting point

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43
Q

Solid to gas

A

Sublimation

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44
Q

Gas to solid

A

Deposition

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45
Q

What are the laws of matter

A

Law of definite proportion or proust’s law

Law of multiple proportion or dalton’s law

Law of conservation of mass

Law of conservation of energy

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45
Q

The composition of a pure compound is always the same regardless of its source

A

Law of definite proportion or proust’s law

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46
Q

In pure compounds the elements are always in the same proportion by mass

A

Law of definite proportion or proust’s law

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47
Q

Atoms of two or more elements may combine in different ratios to produce more than one compound

A

Law of multiple proportion or dalton’s law

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48
Q

No change is observed in the total mass of the substance involved in a chemical reaction

A

Law of conservation of mass

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49
Q

Energy is neither created or destroyed but it is conserved or transformed

A

Law of conservation of energy

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50
Q

Classification of matter

A

Pure and impure or mixture

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51
Q

What is the difference between pure and mixture or impure

A

Pure is chemically combined

Impure or mixture is not chemically combined but physically combined
And it can retain their individual properties

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52
Q

One kind of material atom is a theory of

A

Dalton’s atomic theory

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52
Q

It is the simplest form of matter

A

Elements

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53
Q

Pure chemical substance

A

Elements

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54
Q

It cannot be decomposed by simple physical or chemical means into two or more different substances

A

Elements

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55
Q

Compose of two or more elements that unite chemically in different proportion

A

Compounds

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56
Q

Cannot be changed into simpler substances under normal laboratory condition

A

Compounds

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57
Q

True or false all molecules are considered compound

A

Because hydrogen gas is a molecule but not a compound

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58
Q

Classification of mixture

A

Nature of particles and particle size

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59
Q

Types of nature of particles in the classification of impure /mixture

A

Homogeneous and heterogeneous

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60
Q

What is the types of particle size in the context of classification of mixture

A

Solution
suspension
colloids

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61
Q

Consistent or uniform parts throughout

A

Homogeneous

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62
Q

Example is nacl dissolved in water, syrup, alloys

A

Homogeneous

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63
Q

Physically distinct parts

A

Heterogeneous

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64
Q

Example is sand and water mixture

A

Heterogeneous

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65
Q

True solution is __ mixture

A

Uniform

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66
Q

Atom or molecules and ions of the substance become dispersed

A

True solution

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67
Q

Contains particles bigger than those in solution but smaller than those in suspension

A

Colloids

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68
Q

Dividing line between solution and suspension

A

Colloids

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69
Q

Colloids particles of solid are broken down to the size of the molecule but are small enough in dispersed throughout the medium

A

Colloids

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70
Q

Example of colloids

A

Dust and mayonnaise

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71
Q

What are the properties of colloids

A

TBAC COL
Tyndall effect brownian movement
adsorption
charged electrically

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72
Q

Tyndall effect brownian movement
adsorption
charged electrically

A

Tyndall effect - light scattering effect TINDAHAN MALIWANAG

brownian movement- zigzag movement of colloidal particles

adsorption- capacity to adhere or stick to the surface
AD AD

charged electrically- Nernst/Zeta potential

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73
Q

Course mixture

A

Suspension

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74
Q

Finely divided solid materials distributed in liquid

A

Suspension

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75
Q

Factors affecting solubility

A

FAS NaTo Paster Paster Paster

Nature of solute and solvent
temperature
pressure
particle size
presence of salts

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76
Q

FAS NaTo Paster Paster Paster

A

Factors affecting solubility

Nature of solute and solvent
temperature
pressure
particle size
presence of salts

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77
Q

Refers to the maximum amount of solute expressed in grams that can be dissolved in 100 g of water

A

Solubility

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78
Q

Ability of one substance to mix with another substance

A

Miscibility

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79
Q

If temperature increases what happens to the solubility of solid in a liquid

A

Increases
If temperature increases it also increases the solubility of solid in a liquid

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80
Q

Temperature increases what happens to the solubility of a gas in a liquid

A

Decreases
If a temperature increases it decreases hindi solubility of a gas in a liquid

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81
Q

It absorbs heat and if temperature increases it also increases the solubility

A

Endothermic reaction

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82
Q

It releases heat and its temperature increases it decreases the solubility

A

Exothermic reaction

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83
Q

It states that at constant temperature the solubility of gas in a liquid is directly proportional to the pressure of the gas above the liquid

A

Henry’s law of gas solubility

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84
Q

International system unit of pressure

A

Pascal

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85
Q

What happens to the solubility of gas if pressure increases

A

Increases

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86
Q

What happens to the surface area and solubility if particle size increases

A

Decreases

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87
Q

Presence of salt decrease as solubility

A

Salting out

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88
Q

Presence of salt increases solubility

A

Salting in

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89
Q

What are the types of solution

A

Saturated

unsaturated or diluted

super saturated or concentrated solution

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90
Q

Solution achieved the maximum solubility

A

Saturated solution

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91
Q

The solvent mar solute

A

Diluted or unsaturated

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92
Q

More solvent than solute

A

Supersaturated or concentrated

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93
Q

Interface to the limit before saturation in relation to ion

A

Solubility product constant

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94
Q

Q means

A

Degree of ion

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95
Q

Ion serves as an___ solubility product constant

A

Solute

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96
Q

Acid results to litmus paper

A

Blue to red

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97
Q

Base litmus test result

A

Red to blue

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98
Q

What is the taste of acid and base

A

Acid sour
Base is bitter

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99
Q

What are the theories in acid base equilibra

A

Arrhenius
Bronsted- Lowry
Lewis theory

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100
Q

What theory of acid base indicates that not hydroxyl group is base or basic because of ammonia

A

Arrhenius theory

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101
Q

Bro, acid ang PDos

A

Bronsted - Lowry theory
Acid: proton donor
Base : acceptor

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102
Q

What theory is that yields hydrogen and hydronium ion

A

Arrhenius theory: acid

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103
Q

What theory yield hydroxyl ion

A

Arrhenius theory: basic

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104
Q

What type of theory is an electron acceptor

A

Levi’s theory : acid

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105
Q

It is formed from the neutralization reaction

A

Salts

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106
Q

Example of salts which are formed from the neutralization reaction

A

Strong acid + strong base
Strong acid + weak base
Weak acid + strong base
Weak acid + weak base

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107
Q

Identify their product

Strong acid + strong base
Strong acid + weak base
Weak acid + strong base
Weak acid + weak base

A

Strong acid + strong base - neutral salt

Strong acid + weak base = acidic salt

Weak acid + strong base= basic salt

Weak acid + weak base= no salt formed

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108
Q

Acid + base=

A

Salt + h2o

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109
Q

Example of strong acids

A

HBCNIPS
Hydroboric acid
Hydrochloric acid
Nitric acid
Hydro ionic acid
Perchloric acid
Sulfuric acid

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110
Q

Examples of strong bases

A

Hydroxides
Group 1a and 2a

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111
Q

Ph is measured through

A

Sorensen’s scale

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112
Q

General formula for Sorensen’s scale

A

Ph + poh = 14

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113
Q

It measure the propensity of a larger object to separate or dissociate reversibly into smaller components

A

Dissociation constant

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114
Q

Ionic equilibra that completely dissociates

A

Strong acid base

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115
Q

Ionic equilibra that does not completely dissociate

A

Weak acid base

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116
Q

Ionic equilibrium that does not dissociate

A

Electrolytes

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117
Q

Example of strong acid base that completely dissociates

A

Sodium chloride

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118
Q

Example of weak acid that does not completely dissociates

A

Weak electrolytes such as buffer

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119
Q

Non electrolytes that does not dissociate example

A

Organic molecules such as glucose dextrose or other sugar

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120
Q

It gains or the need proton

A

Amphiprotic

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121
Q

Can neither gain or donate proton

A

Aprotic

122
Q

It donates proton

A

Protogenic

123
Q

Accepts proton

A

Protophilic

124
Q

It is a combination of because in conjugate base or a weak base and its conjugate acid that resist changes in ph upon the addition of small quantities of acid or alkali

A

Buffer

125
Q

What is the purpose of ph

A

It maintains neutrality

126
Q

Buffer equation

A

Henderson hasselbalch equation

127
Q

The magnitude of the resistance of a buffer to ph changes

A

Backer capacity

128
Q

The ratio of the increment of strong base acids to the small changes in ph brought by this audition

A

Bakit capacity

129
Q

Oil of vitreon is also known as

A

Sulfuric acid

130
Q

What are the types of chemical reaction

A

Na CS si DanDan ng chemical reaction

Composition or synthesis or direct union

Decomposition or analysis

Single replacement

Double replacement

131
Q

/It involves the formation of elements
/ it is a simple substance to complex substance

A

Composition , synthesis or direct union

132
Q

/breakdown of compounds
/Complex substance to simpler substances

A

Decomposition or analysis

133
Q

/defense on the activity series
/substitution

A

Single replacement

134
Q

It is the most reactive element

A

Lithium

135
Q

This the least reactive element

A

Silver

136
Q

Acid + base–> salt + h2 O

A

Neutralization reaction

137
Q

Folic acid + alkali -> soap

A

Saponification

138
Q

Alcohol

A

Fermentation

139
Q

Breakdown of bonds by the addition of H2O

A

Hydrolysis

140
Q

Balance decreases and oxidation states decreases

A

Reduction

141
Q

Red Cat Elect in

A

Reduction occurs in the cathode for electrons get in

142
Q

Components within the nucleus

A

Nucleons : Protons and neutron s

143
Q

What is the weight of electron in compared to proton

A

Electron has a negative charge and it is 1,836 x lighter than proton

144
Q

The components within the nucleus is responsible for

A

Mass of an atom

145
Q

He coined the term atom from the greek word atomos which means indivisible

A

Democritus

146
Q

His model is billiard for model

A

John dalton

147
Q

Hollow sphere

A

John dalton

148
Q

May Billiard ball na si Dalton

A

The model of john dalton is billiard ball model

149
Q

All matter are made up of atom

A

John dalton atomic theory

150
Q

Each element has a different atoms

A

John dalton atomic theory

151
Q

Atoms of an element are identical

A

John dalton atomic theory

152
Q

atoms are rearranged in reaction

A

John dalton atomic theory

153
Q

What is the model of jj thompson

A

Raisin bread or plum pudding model

154
Q

Founded atoms could sometimes edject a far smaller negative particle called electron

A

Jj thompson

155
Q

He founded electrons

A

Jj thompson

156
Q

What is the model of ernest rutherford

A

Nuclear model

157
Q

( 99% passed through but less than 1% deflected or blocked

A

Ernest rutherford
Gold film experiment

158
Q

Discovery of proton

A

Ernest rutherford

159
Q

Discovery of neutron

A

James Chadwick

160
Q

It is the model of Neil Bohr

A

Planetary model

161
Q

Redefined Rutherford first idea by adding that electrons were in orbitals like planets or orbiting the sun

A

Neil bohr

162
Q

What is the model of erwin schrödinger

A

Quantum mechanical model

163
Q

Quantum theory and wave theory

A

erwin schrödinger

164
Q

The number of proton indicates the number of

A

Number of electron in neutral state

165
Q

Atomic mass is also known as and its equation

A

Mass number is equal to p + n

166
Q

Same elements in same number of protons but different number of neutrons

A

Isotope

167
Q

It is the most abundant isotope of hydrogen

A

Protium

168
Q

It is used as solvent for nmr studies

A

Heavy hydrogen or deuterium

169
Q

Different elements and same number of mass number

A

isobar

170
Q

Different elements same number of neutrons

A

Isotope

171
Q

Different elements the same number of electrons

A

Isoelectronic

172
Q

__ are different forms of an element

A

Allotropes

173
Q

It is an atom of different element can link together in different ways the form substances with different properties

A

Allotropism

174
Q

Example of an allotropism

A

Diamond
graphite
fullerene

These are allotropes of carbon

175
Q

Who discovered the subatomic particle that is shown by the atomic number

A

Rutherford

176
Q

It is a region in space where the probability of finding an electron is greatest

A

Orbitals

177
Q

Are located in electron clouds or energy level

A

Electrons

178
Q

One or more orbitals with of varying shape

A

Electron shell

179
Q

Electrons occupying the outermost shell

A

Valence electrons

180
Q

Group of numbers which shows the arrangement of electrons in an atom

A

Electron configuration

181
Q

What are the electronic principle

A

Heisenberg uncertainty principle

Pauli’s exclusion principle

Aufbau’s binding

Hund’s Rule

182
Q

It is impossible to determine simultaneously the momentum and position of an electron

A

Heisenberg uncertainty principle

183
Q

No 2 electrons can have the same exact set of quantum numbers

A

Pauli’s exclusion principle

184
Q

___; electrons are first placed on the subshell with a lower energy level

A

Aufbau’s building: up principle

185
Q

Electrons fill up orbitals singly first

A

Hands rule of pairing

186
Q

Unpaired electrons are attracted to a magnet

A

Paramagnetism

187
Q

Paired electrons repelled by a magnet

A

Diamagnetism

188
Q

What are the two classification of hunds rule of pairing

A

Paramagnetism and diamagnetism

189
Q

Principal quantum number symbol

A

n

190
Q

It determines the main energy level or electron shell and the size of the orbital

A

Principal quantum number

191
Q

It determines the shape and subshell

A

Azimuthal or angular quantum numbers

192
Q

Azimuthal or angular quantum numbers symbol

A

l

193
Q
A
194
Q

KaAzi met ni SAS

A

Azimuthal or angular quantum number
It determines the angle, shape and subshell

195
Q

What is the orbital number of
s
p
d
f

A

s-1
p-3
d-5
f-7

196
Q

What is the maximum electron of
s
p
d
f

A

s-2
p-6
d-10
f-14

197
Q

What is the azimuthal or angular quantum number
s
p
d
f

A

s-0
p-1
d-2
f-3

198
Q

What is the shape of
s
p
d
f

A

s- sphere
p- dumbbell
d- clone/ double dumbbell
f- multiple lobes

199
Q

Magnetic quantum numbers symbol

A

ml

200
Q

It determines the special orientation

A

Magnetic quantum number

201
Q

What is the values of Magnetic quantum number

A

-1 to + 1

202
Q

What is the values of azimuthal or angular quantum number

A

0- (n-1)

203
Q

What is the symbol of spin quantum numbers

A

ms

204
Q

It describes the spin or rotation

A

Spin quantum number

205
Q

Spin quantum number values

A

+ 1/2 or clockwise and
-1/2 counter clockwise

206
Q

How many elements are there in periodic table

A

118

207
Q

Horizontal in periodic table indicates the

A

7 periods from left to right homes

208
Q

Vertical in periodic table indicates the

A

Group or family from top to bottom

209
Q

Group a from periodic table is

Group B in periodic table is

A

Representative elements
S and I p block
Known oxidation state

Group b
Transition elements
D and F block
Transition oxidation state

210
Q

Closely resembles the second number of an adjacent group to the right

A

Bridge element or diagonal element

211
Q

Mg Li
Bo Si

A

Bridge element
Magnesium lithium

Boron silicon

212
Q

Father of modern chemistry

A

Antoine laurent Lavoisier

213
Q

Wrote the first extensive list of elements containing 33 elements

A

Antoine laurent Lavoisier

214
Q

First true periodic table

A

Antoine laurent Lavoisier

215
Q

Arrange the periodic table based on atomic mass

A

Meyer and Mendelev

216
Q

Physical and chemical properties are periodic function of their atomic weight

A

Meyer and Mendelev

217
Q

First true periodic law

A

Meyer and Mendelev

218
Q

mu man Henry

A

Elements are arranged based on their atomic number: Henry moseley

219
Q

Elements are arranged based on their atomic number:

A

Henry moseley

220
Q

Modern periodic table

A

Henry moseley

221
Q

Tri ta Johann

A

Introduce the law of triads according to physical properties: Johann dobereiner

222
Q

Middle elements of a triad equal to the arithmic mean of atomic masses of other two elements

A

Johann dobereiner: law of triad

223
Q

Introduce the law of triads according to physical properties:

A

Johann dobereiner

224
Q

Every eight element is similar to the first element

A

Law of octa ves: john alexander newland

225
Q

Law of john alexander newland

A

Law of octaves

226
Q

Iron triad

A

Fe co Ni

227
Q

Platinum triad

A

Ru Rh Rb

228
Q

The property increases from right to left top to bottom

A

Metallic Radius

229
Q

It is one of the distance between two nuclei

A

Atomic radius

230
Q

The property increases from left to right bottom to top

A

Ionization energy anomaly INEA

231
Q

Amount of energy required to remove an electron from a neutral atom to convert it to a positively charged ion

A

Ionization energy

232
Q

The tendency of an atom to attract electrons itself

A

Electronegativity

233
Q

Amount of energy released when a natural atom to convert it to negatively charged ion

A

Electron affinity

234
Q

Intermediate between metals and metals

A

Metalloids

235
Q

Example of metalloids

A

Si
Ge
Po
Sb
As
Te
B

236
Q

It deals with the energy transformation

A

Thermodynam

237
Q

Any part of the universe which isolated from the rest by a boundary on a wall

A

System

238
Q

Everything outside the system

A

Surrounding

239
Q

What are the types of thermodynamics

A

Open
closed
isolated

240
Q

Types of isolated thermodynamics

A

Adiabatic
Diathermal

241
Q

Allows the exchange of both matter and energy

A

Open thermodynamics

242
Q

It allows the exchange of energy but not matter

A

Closed thermodynamics

243
Q

It does not allow the exchange of both matter and energy

A

Isolated thermodynamics

244
Q

Isolated thermodynamics it does not allow energy or heat flow

A

Adiabatic (isolated thermodynamics)

245
Q

It allows energy and heat flow

A

Diathermal (isolated thermodynamic)

246
Q

An energy transfer due to temperature difference

A

Heat (q)

247
Q

Refers to the total in content

A

Enthalpy (H)

248
Q

Measure of degree of randomness or disorderliness of a system

A

Entropy (S)

249
Q

What are the thermodynamic functions

A

Heat
enthalpy
Entropy

250
Q

What are the law of thermodynamics

A

1st law: law of conservation of energy

2nd law: spontaneous law

3rd law: the entropy of a pure crystalline solid at a zero kelvin is zero

4th law: states that if two bodies are each in thermal equilibrium with some third body then they also equilibrium with each other

251
Q

Measure of spontaneity

A

Gibb’s free energy

252
Q

All of the atoms and molecules behave independently

A

Kinetic molecular theory of gases

253
Q

No attractive or repulsive forces exist between atoms or molecules in a gas

A

Kinetic molecular theory of gases

254
Q

Atoms and molecules collide with each other and with the walls of the container without losing energy. The energy is transferred from one atom or molecule to another

A

Kinetic molecular theory of gases

255
Q

The average kinetic energy of atoms or molecules increases

A

Kinetic molecular theory of gases

256
Q

Boyle’s law is also known as

A

Mariotte law

257
Q

In boyle’s law what is the relationship between pressure and volume

A

Pressure is inversely proportional to volume

258
Q

What is constant in boyle’s law

A

Temperature

259
Q

What is constant in charles’ law

A

Pressure

260
Q

Pressure what is the relationship of volume and temperature in charles law

A

Directly proportional

261
Q

Gay-lusacc’s law is also known as

A

Amonton’s law

262
Q

What is constant in gay-lussac’s law

A

Volume volume

263
Q

What is the relationship of pressure and temperature in gay-lussac’s law

A

Directly proportional

264
Q

Equal volume of different gases have the same number of moles of at standard temperature and pressure

A

Avogadro’s law

265
Q

Avogadro’s number

A

6.022x 10raised 23

266
Q

Formula for avogadro’s number

A

V1/n1 = V2/n2

267
Q

Formula for combined gas law

A

P1V1/n1 = P2V2/n2

268
Q

Provides convenient expression for performing gas law calculation involving the most common variable such as pressure volume and temperature

A

Combined gas law

269
Q

Formula for ideal gas law

A

PV= nRT
P- 1atm
v- 22.4L
n - no. of mole
R- gas constant (0.08205L × atm / mol × K
T- 273.15 K

270
Q

States that the pressure exerted by a mixture of gases or non reacting gases is the sum of partial pressure that each has in the mixture exert individually

A

Dalton’s law of partial pressure

271
Q

The rate of the effusion of two gases and diffusion are inversely proportional to the square root of there densities providing the temperature and pressure are the same for two gases

A

Graham’s law

272
Q

Gradual mixing of molecules of one gas when the molecules of another gas

A

Diffusion

273
Q

Passage of a gas under pressure through a small opening

A

Effusion

274
Q

Change in structure properties composition of the nucleus of an atom resulting in the transformation of an element into another element

A

Nuclear change

275
Q

Splitting of heavy atom

A

Nuclear fission

276
Q

Union of two light atoms to form a bigger molecule

A

Nuclear fusion

277
Q

It is a process of decomposition of unstable nuclei tumor stable or once

A

Radioactivity

278
Q

Energy and particles release during the decomposition process

A

Radiation

279
Q

What are the units of radioactivity

A

Non SI : Curie
SI: Becquerel (Bq)

280
Q

Non SI : Curie = __ decays/sec

A

3.7 × 10 raised to 10

281
Q

SI: Becquerel (Bq)= ___ decays/sec

A

1

282
Q

What are the units of radiation damage

A

Roentgen’s equivalent Man RE

283
Q

What are the types of decay

A

Alpha
beta
gamma

284
Q

Unit of amount of exposure to radiation

A

Rad/gray

285
Q

What are the penetrating power of
Alpha
beta
gamma

A

Alpha- low
beta -; medium
gamma=high, which is dangerous

286
Q

Alpha
beta
gamma
is blocked by

A

Alpha- paper
Beta- aluminum
gamma- lead

287
Q

Refers to the study of rate for speed of chemical reaction

A

Chemical kinetic s

288
Q

Finished reaction

A

Chemical reaction

289
Q

Chemical reaction that shifts to the right

A

Forward reaction

290
Q

Chemical reaction that shift to the left

A

Backward reaction

291
Q

Collision theory

A

Increase in rate is equal to increase in collision

292
Q

Should be overcome for the reaction to proceed

A

Activation energy

293
Q

What is the proper orientation of the collision theory

A

It should be a lower activation energy for it to overcome

294
Q

Reactants will undergo a transition state in order to produce products

A

Transition state theory

295
Q

What are the factors affecting the rate of reaction

A

Particle size
concentration
nature of reactant
temperature

296
Q

It states that narrate of forward reaction is equal to the rate of factor reaction

A

Chemical equilibrium

297
Q

If stress is applied or applied are placed on an equilibrium system, the system will respond by altering the equipment in such way as to minimize stress

A

Le chatelier’s principle

298
Q

States that the rate of the reaction is proportional to the product of the concentration of the reactants to the power of its coefficient in a balanced equation

A

Law of mass action

299
Q

Factors affecting the equilibrium

A

Concentration
pressure
temperature

300
Q

Add A or b in concentration

A

Forward

300
Q

Add C or D in concentration

A

Backward

301
Q

Increase in pressure and decrease in volume is ___ number of moles

A

Less

302
Q

Decrease in pressure and increase in volume is ___ number of moles

A

More

303
Q

Reactant in factors affecting the equilibrium

A

Endothermic

304
Q

Product in factors affecting the equilibrium

A

Exothermic

TCEP Review (6 decks)

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