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Gen Chemistry Flashcards

1
Q

Branch of science that is concerned in the study of matter and changes it undergoes

A

Chemistry

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2
Q

Study of organic compounds (contains carbon)

A

Organic chemistry

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3
Q

Study of elements and compounds that is considered to be inorganic

A

Inorganic Chemistry

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4
Q

Study of chemistry of life

A

Biochemistry

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5
Q

Area of chemistry that is used in characterization of matter both quantitatively and qualitatively

A

Analytical chemistry

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6
Q

Study of macroscopic, and particulate phenomena in chemical systems in terms of the principles, practices, and concepts of physics such as motion, energy, force, time, thermodynamics, quantum chemistry, statistical mechanics, analytical dynamics and chemical equilibrium

A

physical chemistry

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7
Q

Study of energy, conversion of energy that in various forms and ability of energy to do work from the word ‘therme’ which means heat and ‘dynamis’ which means power or energy

A

Thermodynamics

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8
Q

Total amount of energy in an isolated system remains constant; it is said to be conserved over time energy is neither created nor destroyed, it can only be transformed or changed from one form to another

A

Law of Conservation of Energy (1st Law)

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9
Q

Energy inside the system

A

Internal energy

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10
Q

Thermodynamic property that is the measure of a system’s thermal energy per unit temperature that is unavailable for doing useful work.

Degree of disorderliness

A

Entropy

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11
Q

Law of disorderliness / Spontaneous Law. In relation of heat energy and entropy, it is impossible to obtain the process where the unique effect is the subtraction of positive heat from reservoir and the production of positive work states that the spontaneous natural processes increase entropy overall heat can spontaneously conducted or radiated only from higher temperature region to lower temperature region but not the other way around for natural spontaneous process the entropy increases, this can lead now to higher disorderliness for natural process

A

Law of Entropy

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12
Q

Entropy of perfect crystal is absolute zero is exactly equal to zero

A

solid entropy crystalline

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13
Q

All processes, temperature approaches absolute zero 2 bodies are in equilibrium with the 3rd body separately then it follows the 1st and 2nd body are also in thermal equilibrium.

A

Zeroth Law

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14
Q

Anything that occupies space and has mass (solid, liquid, gas). It has structure. It involves change. It requires energy for those changes and interaction

A

Matter

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15
Q

Matter possessing a definite and unvarying composition

A

Pure substance

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16
Q

Simplest form of substance that cannot be decomposed of a simple chemical reaction. 1 atom (+ or -)

A

Element

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17
Q

Substances composed of 2 or more elements united chemically in definite proportions

A

Compound

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18
Q

2 or more substances that retain its own characteristics

A

Mixture

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19
Q

Uniform throughout the mixture. No dissolved part particles

A

homogenous mixture

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20
Q

Composition is not uniform throughout the mixture, insoluble substance, 2 or more phases

A

heterogeneous mixture

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21
Q

Consist of positively charged core (atomic nucleus) which contains protons and neutrons

A

Atoms

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22
Q

Basic unit that made up all matter and basic unit of an element that can enter a chemical reaction.

A

Atoms

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23
Q
  • (Gold foil experiment)
  • Proton (+)
A

Ernest Rutherford

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24
Q

Electron (-)

A

JJ thompson

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25
Q

3 LAW PRINCIPLES

A
  • Definite proportions
    • Multiple proportions
    • Combining weights
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26
Q

aka Proust’s Law (Joseph-Louis Proust)

A

LAW OF DEFINITE PROPORTIONS

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27
Q

states that a chemical compound always contain exactly the same proportion of elements by mass

A

LAW OF DEFINITE PROPORTIONS

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28
Q

copper carbonate either made from the laboratory or obtained from natural resources are always compose of mass of 1.3 parts of copper ,1 part of carbon and 4 parts of oxygen

A

LAW OF DEFINITE PROPORTIONS

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29
Q

states that when 2 elements formed more than 1 compound between them then the ratios of the masses of 2nd element which combine with a fix mass of an element will be ratios of small whole number

A

LAW OF MULTIPLE PROPORTION

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30
Q

states that proportion by weight by chemical reactions take place can be express in terms of small integral multiple of fixed number could as combining weights of equivalent weight

A

LAW OF COMBINING WEIGHTS

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31
Q

“law of reciprocal proportions or law of equivalence”

A

Law of Combining weights

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32
Q

fundamental unit of structure of matter that can enter into a chemical reaction.

A

Atom

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33
Q

Diff elements, same atomic mass

A

Isobars

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34
Q

Atoms of different elements having the same number of neutrons

A

Isotone

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35
Q

Diff, structure, same molecule

A

Isomers

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36
Q

coined ‘’atomos’’ (tiny indivisible particles)

A

Democritus

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37
Q

considered to be 90% right

A

Democritus

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38
Q

atoms enter into a combination with other atoms to form compounds but it will remain unchanged during ordinary chemical reaction

A

John Dalton

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39
Q

atoms can combine in a simple numerical ratio

A

John Dalton

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40
Q

‘’Billiard ball model’’

A

John Dalton

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41
Q

atom is a hard indestructible sphere - Supports the law of definite proportion and law of multiple proportion

A

John Dalton

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42
Q

Thompson Model & Raisin bread model

A

JJ Thompson

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43
Q

Atom is a spherical mass containing electrons and that this spherical mass is positive but is made neutral by the electron embedded in it

A

JJ THOMPSON

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44
Q

Plum pudding (hollow but filled in structure)

A

Jj Thomspon

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45
Q

Negatively charged particles are embedded in the positively charged particles

Electrons are randomly spread throughout the clouds of massless positively charged material

A

Jj thompson

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46
Q

Gold film experiment

A

RUTHERFORD MODEL

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47
Q

Based on additional experimental evidence of ‘’alpha scattering experiments’’

A

RUTHERFORD MODEL

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48
Q

2 experiment in RUTHERFORD MODEL

A
  • Geiger Marsden experiment
    • Gold film foil experiment
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49
Q

To prove that atoms are in a really small space called atomic nucleus

A

Geiger Marsden experiment

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50
Q

Atom is mostly empty space and most of its mass and positively charged particles are concentrated in nucleus

A

Gold film foil experiment

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51
Q

Planetary Model

A

BOHR MODEL OF AN ATOM

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52
Q

Proton are in the nucleus and the electrons are in the orbital motion around the nucleus

A

BOHR MODEL OF AN ATOM

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53
Q

Electrons orbits the nucleus in a fix circular orbits

A

BOHR MODEL OF AN ATOM

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54
Q

Atoms are in elliptical orbits of increasing number

A

NEIL-BOHR MODEL

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55
Q

This principle states that simultaneous determination of the exact position and exact momentum of electron is impossible

A

HEISENBURG UNCERTAINTY PRINCIPLE

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56
Q

Aka Electron Cloud Model

A

WAVE MECHANICAL ATOM

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57
Q

The nucleus is a single cluster of particles at the center of the atom while the electrons are everywhere in rotating motion

A

WAVE MECHANICAL ATOM

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58
Q

What is the Model of Wave Mechanical atom?

A

Pauli’s Exclusion Model

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59
Q
  • Formulated by Wolfgand Pauli (1925)
    • No 2 electrons in an atom can have the same set of quantum numbers
A

Pauli’s Exclusion Model

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60
Q

This theory makes the assertion that electromagnetic radiation like X-rays, gamma rays, radio waves and light rays are made up of energy

A

SCHROEDINGER ‘’QUANTUM MODEL’’

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61
Q

Does not define the exact path of an electron but rather predicts the odds of the location of the electron

A

SCHROEDINGER ‘’QUANTUM MODEL’’

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62
Q

Nucleus surrounded by an electron cloud. Where the clouds are most dense, therefore the probability of finding the electron is quick and conversely the electron is like to be in less dense area of the cloud

A

SCHROEDINGER ‘’QUANTUM MODEL’’

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63
Q

This model introduces the concept of the subenergy levels

A

SCHROEDINGER ‘’QUANTUM MODEL’’

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64
Q

Known as Quantum Mechanical

A

Schroedinger

65
Q

He took the Bohr atom model one step further.

A

Erwin Schroedinger

66
Q

He uses mathematical equation to describe the likelihood of finding an electron in a certain position

A

Erwin Schroedinger

67
Q

Electron wave dimensions that is indicated by numbers

A

QUANTUM NUMBERS

68
Q

Determines the size of the particles and relates average distance of electrons from the nucleus in a particular orbital

A

PRINCIPAL QUANTUM NUMBER

69
Q

‘’n’’
Corresponds to the main energy level

A

PRINCIPAL QUANTUM NUMBER

70
Q

‘’l’’

A

AZIMUTHAL QUANTUM NUMBER

71
Q

Gives and measure the angular momentum of an electron in its motion about the nucleus

A

AZIMUTHAL QUANTUM NUMBER

72
Q

‘’m’’ and it indicates the behavior of electrons in the magnetic field and usually the range is from -1 to +1

A

MAGNETIC QUANTUM NUMBER

73
Q

‘’s’’ and it indicates the spin of an electron about in its own axis whether it will be clockwise of counter clockwise

A

SPIN QUANTUM NUMBER

74
Q

States that the number of orbital types in a given shell is equal to the shell number

A

ORBITAL THEORY

75
Q

Orbitals have the ___ dimensional region in space where the probability of finding the electron is greatest

A

3

76
Q

Atoms may be filled by progressively filling of the main energy levels, sublevels, and orbitals with electrons according to increasing sequence and the levels of lower energy are occupied first

A

AUFBAU PRINCIPLE

77
Q

Orbitals with same electron of same energy level must be filled in singly before pairing

A

HUND’S RULE OF MAXIMUM MULTIPLICITY

78
Q

Distribution of electrons in the different shells and subshells of orbitals within the atom

A

ELECTRONIC CONFIGURATION THEORY

79
Q

TYPES OF CHEMICAL BONDS

A
  1. IONIC BOND
  2. COVALENT BOND
  3. METALLIC BOND
  4. HYDROGEN BOND
  5. VANDERWAALS
80
Q

a connection between electrons and atoms. Forces that holds atoms together

A

Chemical bond

81
Q

2 or more atoms of an element is chemically joined together

A

Molecules

82
Q

Aggregates of at least 2 atoms in a definite arrangement held together by chemical forces

A

Molecules

83
Q

Smallest indivisible portion of a pure substance that has its unique set of chemical properties that is its potential to undergo a certain set of chemical reactions with other substances

A

Molecules

84
Q

positive (loss electron)

A

Cation

85
Q

negative (gain electron)

A

Anion

86
Q

Charged species, an atom or a molecule that has lost or gained one or more electrons

A

ION

87
Q

Total number of electrons is not equal to he total number of protons

A

ION

88
Q

Substances whose molecules are made up of 2 or more kinds of atoms combined in a definite proportion

A

COMPOUNDS

89
Q

TYPES OF COMPOUNDS

A

Ionic compounds and covalent compounds

90
Q

If compound is made from metal & nonmetal

A

Ionic

91
Q

Transfer of electrons
Attraction of + and – ion

A

Ionic

92
Q

2 nonmetal ions.

A

Covalent compound

93
Q

Sharing of electrons
Covalent bond (bond between 2 atoms shares electron)

A

Covalent compound

94
Q

Interaction between element which are metallic but the resulting compound behave just like an ordinary metal

A

Metallic compound

95
Q

Metal is always written ____ followed by nonmetal or polyatomic ion

A

First

96
Q

Color of Acids

A

litmus: Blue to red

97
Q

donates proton and accept electron

A

Acids

98
Q

contains hydrogen that is replaceable by a metal yields hydrogen ion is water

A

Acids

99
Q

TYPES OF INORGANIC COMPOUNDS

A

Acids,Bases,Salt, & Oxides

100
Q

most acid contains hydrogen atom that is bonded and ____ release to yield anion and cation in water

A

can’t

101
Q

accepts proton

A

Bases

102
Q

contained metal with hydroxyl group. It is sopay and slippery

A

Bases

103
Q

electrolyte that yields neither hydrogen and hydroxide from dissolve molecule

A

Salts

104
Q

formed by any positive and negative ions except hydrogen and hydroxyl ion

A

Salts

105
Q

oxygen is _____ reactive in nature

A

Highly

106
Q

consist of oxygen and other elements
binary compounds that are formed from the reaction of oxygen to other elements

A

Oxides

107
Q

Attractive forces between molecules specifically of polar substances

A

VAN DER WAALS

108
Q

Involves hydrogen ion in combination with other atoms in molecules

A

HYDROGEN BOND

109
Q

Electrostatic attraction of a positive and negative ions that holds the atoms together

A

METALLIC BOND

110
Q

Electrostatic attraction of a positive and negative ions that holds the atoms together

A

METALLIC BOND

111
Q

Attraction of 2 non polar molecules and weakest intermolecular force

A

LONDON/ DISPERSION FORCES

112
Q

3 types forces of VAN DER WAALS:

A
  • London/Dispersion Forces
    • Keesom Forces
    • Debye Forces
113
Q

AKA Induced dipole-induced dipole attraction

A

LONDON/ DISPERSION FORCES

114
Q

Temporary attractive force that results when the electrons in 2 adjacent atoms occupied positions that makes the atoms form temporary dipole

A

LONDON/ DISPERSION FORCES

115
Q

Dipole-dipole attraction. Attraction between 2 polar molecules

A

KEESOM FORCES

116
Q

Dipole-induced dipole. Between a polar and non-polar

A

DEBYE FORCES

117
Q

Dipole-dipole. Strong electronegative elements

A

HYDROGEN BONDS

118
Q

Weak attraction that results in the approach of an ion induces a dipole in an atom or non-polar molecule by disturbing the arrangement of electrons in the non-polar species

A

ION-INDUCED DIPOLE

119
Q

Tell which element is present and express in the simplest whole number ratio of their atoms

A

EMPIRICAL FORMULA

120
Q

shows the exact numbers of atoms of each element in the smallest unit of substances

base on the actual molecule

A

MOLECULAR FORMULA

121
Q

How the atoms are bonded to one another in a molecule

A

STRUCTURAL FORMULA

122
Q

How the atoms are bonded to one another in a molecule

A

STRUCTURAL FORMULA

123
Q

Relationship of volume and pressure

A

BOYLE’S LAW

124
Q

At constant temperature volume is inversely proportional to the pressure

A

BOYLE’S LAW

125
Q

Relationship of pressure and temperature

A

GAY-LUSSAC’S LAW OF COMBINING VOLUMES

126
Q

At constant volume and mass, it states that when measure at the same temperature and pressure the ratios of the volume of the reacting classes are small whole number

A

GAY-LUSSAC’S LAW OF COMBINING VOLUMES

127
Q

Combination of boyle’s and charles law. States that for a given mass of gas the volume is considered to be inversely proportional to the pressure and directly proportional to the absolute temperature

A

COMBINED GAS LAW

128
Q

States that the pressure, temp and volume of gas are related to each other
PV=nRT

A

IDEAL GAS LAW

129
Q

It states that equal volume of different gases having same temp and press will contain equal number of molecules

A

AVOGADRO’S LAW

130
Q

It states that a total pressure exerted by a mixture of gases is equal to the sum or partial pressure of all of the components of gases

A

DALTON’S LAW OF PARTIAL PRESSURE

131
Q

States that under the same conditions the ratio of diffusion of gas is inversely proportional to the square root of air molecular masses

A

GRAHAM’S LAW OF DIFFUSION

132
Q

Bases, it is a substance that dissociates in water to form hydroxide ion (OH-)

A

ARRHENIUS THEORY

133
Q

Base on aqueous solution wherein the acid is a substance that dissociates in water to form hydrogen ions (H+)

A

ARRHENIUS THEORY

134
Q

Theory that found by Svante Arrhenius

A

ARRHENIUS THEORY

135
Q

base on protonic nature that is based on the idea on the protonation of bases thru the deprotonation of acid. That tells us the ability of acid to donate hydrogen ions (protons) to bases

A

BRONSTED AND LOWRY THEORY

136
Q

the Danish chemist Johannes Nicolaus Brønsted and the English chemist Thomas Martin Lowry

A

BRONSTED AND LOWRY THEORY

137
Q

Based on electronic nature that defines the base (lewis base) can donate electron pair in an acid (lewis acid) and a compound can receive now the electron pair

A

LEWIS THEORY

138
Q

Gilbert N. Lewis

A

LEWIS THEORY

139
Q

Provide starting point for modern treatment for non-ideality of electrolytes solution

A

DEBYE-HUCKEL THEORY

140
Q

Based on electrolytes nature

A

DEBYE-HUCKEL THEORY

141
Q

Peter Debye and Erich Hückel

A

DEBYE-HUCKEL THEORY

142
Q

Based on an extremely simplified model of an electrolyte solution but nevertheless gave accurate prediction of main activity coefficient of ions in dilute solutions

A

DEBYE-HUCKEL THEORY

143
Q

representation of chemical reaction

A

Chemical equation

144
Q

Substances formed

A

Products

145
Q

substances that enter a chemical reaction

A

Reactants

146
Q

occurs when valence electrons around the nucleus interacts. This means removal of electrons and addition of electrons to a partly filled valence shell or sharing a pair of electrons

A

Chemical Reaction

147
Q

occurs when valence electrons around the nucleus interacts. This means removal of electrons and addition of electrons to a partly filled valence shell or sharing a pair of electrons

A

Chemical Reaction

148
Q

particles provide energy required to break bonds

A

COLLISION

149
Q

One compound decomposes to form two or more substance

A

DECOMPOSITION / ANALYSIS

150
Q

Involves the reaction of two or more substances react to form one compound

A

DIRECT UNION/ SYNTHESIS / COMPOSITION

151
Q

A change in the structure, properties, composition of the nucleus of an atom resulting in the transmutation of the element into another element.

A

NUCLEAR Change

152
Q

The _______ (greater/lower) the number of collision per unit time, the _____ (greater/lower) the conversion of initial substances into products per unit time that is, the greater the speed of reaction.

A

Greater
Greater

153
Q

minimum amount of energy required for successful collision

A

Activation energy

154
Q

Union of two light atoms to form a bigger molecule

A

Nuclear Fusion

155
Q

Splitting of heavy atoms / seen having nucleus
Mass number = ↑ 200

A

Nuclear Fission

156
Q

Splitting of heavy atoms / seen having nucleus
Mass number = ↑ 200

A

Nuclear Fission

157
Q

When stress is applied to a system in equilibrium, the equilibrium will shift in such a MANNER as to relieve or neutralize the stress.

A

Le Chatelier’s Principles

158
Q

The rate of chemical reaction is directly proportional to the concentrations of the reactants at a given temperature.

A

Law of Mass Action

159
Q

The equation that shows that the concentrations of reactants and products are raised to the power corresponding other coefficients in the balanced equation is equal to a constant

A

Law of Chemical Equilibrium

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