Gen Chemistry Flashcards
1
Q
Branch of science that is concerned in the study of matter and changes it undergoes
A
Chemistry
2
Q
Study of organic compounds (contains carbon)
A
Organic chemistry
3
Q
Study of elements and compounds that is considered to be inorganic
A
Inorganic Chemistry
4
Q
Study of chemistry of life
A
Biochemistry
5
Q
Area of chemistry that is used in characterization of matter both quantitatively and qualitatively
A
Analytical chemistry
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
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
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)
9
Q
Energy inside the system
A
Internal energy
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
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
12
Q
Entropy of perfect crystal is absolute zero is exactly equal to zero
A
solid entropy crystalline
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
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
15
Q
Matter possessing a definite and unvarying composition
A
Pure substance
16
Q
Simplest form of substance that cannot be decomposed of a simple chemical reaction. 1 atom (+ or -)
A
Element
17
Q
Substances composed of 2 or more elements united chemically in definite proportions
A
Compound
18
Q
2 or more substances that retain its own characteristics
A
Mixture
19
Q
Uniform throughout the mixture. No dissolved part particles
A
homogenous mixture
20
Q
Composition is not uniform throughout the mixture, insoluble substance, 2 or more phases
A
heterogeneous mixture
21
Q
Consist of positively charged core (atomic nucleus) which contains protons and neutrons
A
Atoms
22
Q
Basic unit that made up all matter and basic unit of an element that can enter a chemical reaction.
A
Atoms
23
Q
- (Gold foil experiment)
- Proton (+)
A
Ernest Rutherford
24
Q
Electron (-)
A
JJ thompson
25
3 LAW PRINCIPLES
- Definite proportions
- Multiple proportions
- Combining weights
26
aka Proust’s Law (Joseph-Louis Proust)
LAW OF DEFINITE PROPORTIONS
27
states that a chemical compound always contain exactly the same proportion of elements by mass
LAW OF DEFINITE PROPORTIONS
28
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
LAW OF DEFINITE PROPORTIONS
29
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
LAW OF MULTIPLE PROPORTION
30
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
LAW OF COMBINING WEIGHTS
31
“law of reciprocal proportions or law of equivalence”
Law of Combining weights
32
fundamental unit of structure of matter that can enter into a chemical reaction.
Atom
33
Diff elements, same atomic mass
Isobars
34
Atoms of different elements having the same number of neutrons
Isotone
35
Diff, structure, same molecule
Isomers
36
coined ‘’atomos’’ (tiny indivisible particles)
Democritus
37
considered to be 90% right
Democritus
38
atoms enter into a combination with other atoms to form compounds but it will remain unchanged during ordinary chemical reaction
John Dalton
39
atoms can combine in a simple numerical ratio
John Dalton
40
‘’Billiard ball model’’
John Dalton
41
atom is a hard indestructible sphere - Supports the law of definite proportion and law of multiple proportion
John Dalton
42
Thompson Model & Raisin bread model
JJ Thompson
43
Atom is a spherical mass containing electrons and that this spherical mass is positive but is made neutral by the electron embedded in it
JJ THOMPSON
44
Plum pudding (hollow but filled in structure)
Jj Thomspon
45
Negatively charged particles are embedded in the positively charged particles
Electrons are randomly spread throughout the clouds of massless positively charged material
Jj thompson
46
Gold film experiment
RUTHERFORD MODEL
47
Based on additional experimental evidence of ‘’alpha scattering experiments’’
RUTHERFORD MODEL
48
2 experiment in RUTHERFORD MODEL
- Geiger Marsden experiment
- Gold film foil experiment
49
To prove that atoms are in a really small space called atomic nucleus
Geiger Marsden experiment
50
Atom is mostly empty space and most of its mass and positively charged particles are concentrated in nucleus
Gold film foil experiment
51
Planetary Model
BOHR MODEL OF AN ATOM
52
Proton are in the nucleus and the electrons are in the orbital motion around the nucleus
BOHR MODEL OF AN ATOM
53
Electrons orbits the nucleus in a fix circular orbits
BOHR MODEL OF AN ATOM
54
Atoms are in elliptical orbits of increasing number
NEIL-BOHR MODEL
55
This principle states that simultaneous determination of the exact position and exact momentum of electron is impossible
HEISENBURG UNCERTAINTY PRINCIPLE
56
Aka Electron Cloud Model
WAVE MECHANICAL ATOM
57
The nucleus is a single cluster of particles at the center of the atom while the electrons are everywhere in rotating motion
WAVE MECHANICAL ATOM
58
What is the Model of Wave Mechanical atom?
Pauli's Exclusion Model
59
- Formulated by Wolfgand Pauli (1925)
- No 2 electrons in an atom can have the same set of quantum numbers
Pauli’s Exclusion Model
60
This theory makes the assertion that electromagnetic radiation like X-rays, gamma rays, radio waves and light rays are made up of energy
SCHROEDINGER ‘’QUANTUM MODEL’’
61
Does not define the exact path of an electron but rather predicts the odds of the location of the electron
SCHROEDINGER ‘’QUANTUM MODEL’’
62
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
SCHROEDINGER ‘’QUANTUM MODEL’’
63
This model introduces the concept of the subenergy levels
SCHROEDINGER ‘’QUANTUM MODEL’’
64
Known as Quantum Mechanical
Schroedinger
65
He took the Bohr atom model one step further.
Erwin Schroedinger
66
He uses mathematical equation to describe the likelihood of finding an electron in a certain position
Erwin Schroedinger
67
Electron wave dimensions that is indicated by numbers
QUANTUM NUMBERS
68
Determines the size of the particles and relates average distance of electrons from the nucleus in a particular orbital
PRINCIPAL QUANTUM NUMBER
69
‘’n’’
Corresponds to the main energy level
PRINCIPAL QUANTUM NUMBER
70
‘’l’’
AZIMUTHAL QUANTUM NUMBER
71
Gives and measure the angular momentum of an electron in its motion about the nucleus
AZIMUTHAL QUANTUM NUMBER
72
‘’m’’ and it indicates the behavior of electrons in the magnetic field and usually the range is from -1 to +1
MAGNETIC QUANTUM NUMBER
73
‘’s’’ and it indicates the spin of an electron about in its own axis whether it will be clockwise of counter clockwise
SPIN QUANTUM NUMBER
74
States that the number of orbital types in a given shell is equal to the shell number
ORBITAL THEORY
75
Orbitals have the ___ dimensional region in space where the probability of finding the electron is greatest
3
76
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
AUFBAU PRINCIPLE
77
Orbitals with same electron of same energy level must be filled in singly before pairing
HUND’S RULE OF MAXIMUM MULTIPLICITY
78
Distribution of electrons in the different shells and subshells of orbitals within the atom
ELECTRONIC CONFIGURATION THEORY
79
TYPES OF CHEMICAL BONDS
1. IONIC BOND
2. COVALENT BOND
3. METALLIC BOND
4. HYDROGEN BOND
5. VANDERWAALS
80
a connection between electrons and atoms. Forces that holds atoms together
Chemical bond
81
2 or more atoms of an element is chemically joined together
Molecules
82
Aggregates of at least 2 atoms in a definite arrangement held together by chemical forces
Molecules
83
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
Molecules
84
positive (loss electron)
Cation
85
negative (gain electron)
Anion
86
Charged species, an atom or a molecule that has lost or gained one or more electrons
ION
87
Total number of electrons is not equal to he total number of protons
ION
88
Substances whose molecules are made up of 2 or more kinds of atoms combined in a definite proportion
COMPOUNDS
89
TYPES OF COMPOUNDS
Ionic compounds and covalent compounds
90
If compound is made from metal & nonmetal
Ionic
91
Transfer of electrons
Attraction of + and – ion
Ionic
92
2 nonmetal ions.
Covalent compound
93
Sharing of electrons
Covalent bond (bond between 2 atoms shares electron)
Covalent compound
94
Interaction between element which are metallic but the resulting compound behave just like an ordinary metal
Metallic compound
95
Metal is always written ____ followed by nonmetal or polyatomic ion
First
96
Color of Acids
litmus: Blue to red
97
donates proton and accept electron
Acids
98
contains hydrogen that is replaceable by a metal yields hydrogen ion is water
Acids
99
TYPES OF INORGANIC COMPOUNDS
Acids,Bases,Salt, & Oxides
100
most acid contains hydrogen atom that is bonded and ____ release to yield anion and cation in water
can't
101
accepts proton
Bases
102
contained metal with hydroxyl group. It is sopay and slippery
Bases
103
electrolyte that yields neither hydrogen and hydroxide from dissolve molecule
Salts
104
formed by any positive and negative ions except hydrogen and hydroxyl ion
Salts
105
oxygen is _____ reactive in nature
Highly
106
consist of oxygen and other elements
binary compounds that are formed from the reaction of oxygen to other elements
Oxides
107
Attractive forces between molecules specifically of polar substances
VAN DER WAALS
108
Involves hydrogen ion in combination with other atoms in molecules
HYDROGEN BOND
109
Electrostatic attraction of a positive and negative ions that holds the atoms together
METALLIC BOND
110
Electrostatic attraction of a positive and negative ions that holds the atoms together
METALLIC BOND
111
Attraction of 2 non polar molecules and weakest intermolecular force
LONDON/ DISPERSION FORCES
112
3 types forces of VAN DER WAALS:
- London/Dispersion Forces
- Keesom Forces
- Debye Forces
113
AKA Induced dipole-induced dipole attraction
LONDON/ DISPERSION FORCES
114
Temporary attractive force that results when the electrons in 2 adjacent atoms occupied positions that makes the atoms form temporary dipole
LONDON/ DISPERSION FORCES
115
Dipole-dipole attraction. Attraction between 2 polar molecules
KEESOM FORCES
116
Dipole-induced dipole. Between a polar and non-polar
DEBYE FORCES
117
Dipole-dipole. Strong electronegative elements
HYDROGEN BONDS
118
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
ION-INDUCED DIPOLE
119
Tell which element is present and express in the simplest whole number ratio of their atoms
EMPIRICAL FORMULA
120
shows the exact numbers of atoms of each element in the smallest unit of substances
base on the actual molecule
MOLECULAR FORMULA
121
How the atoms are bonded to one another in a molecule
STRUCTURAL FORMULA
122
How the atoms are bonded to one another in a molecule
STRUCTURAL FORMULA
123
Relationship of volume and pressure
BOYLE’S LAW
124
At constant temperature volume is inversely proportional to the pressure
BOYLE’S LAW
125
Relationship of pressure and temperature
GAY-LUSSAC’S LAW OF COMBINING VOLUMES
126
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
GAY-LUSSAC’S LAW OF COMBINING VOLUMES
127
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
COMBINED GAS LAW
128
States that the pressure, temp and volume of gas are related to each other
PV=nRT
IDEAL GAS LAW
129
It states that equal volume of different gases having same temp and press will contain equal number of molecules
AVOGADRO’S LAW
130
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
DALTON’S LAW OF PARTIAL PRESSURE
131
States that under the same conditions the ratio of diffusion of gas is inversely proportional to the square root of air molecular masses
GRAHAM'S LAW OF DIFFUSION
132
Bases, it is a substance that dissociates in water to form hydroxide ion (OH-)
ARRHENIUS THEORY
133
Base on aqueous solution wherein the acid is a substance that dissociates in water to form hydrogen ions (H+)
ARRHENIUS THEORY
134
Theory that found by Svante Arrhenius
ARRHENIUS THEORY
135
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
BRONSTED AND LOWRY THEORY
136
the Danish chemist Johannes Nicolaus Brønsted and the English chemist Thomas Martin Lowry
BRONSTED AND LOWRY THEORY
137
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
LEWIS THEORY
138
Gilbert N. Lewis
LEWIS THEORY
139
Provide starting point for modern treatment for non-ideality of electrolytes solution
DEBYE-HUCKEL THEORY
140
Based on electrolytes nature
DEBYE-HUCKEL THEORY
141
Peter Debye and Erich Hückel
DEBYE-HUCKEL THEORY
142
Based on an extremely simplified model of an electrolyte solution but nevertheless gave accurate prediction of main activity coefficient of ions in dilute solutions
DEBYE-HUCKEL THEORY
143
representation of chemical reaction
Chemical equation
144
Substances formed
Products
145
substances that enter a chemical reaction
Reactants
146
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
Chemical Reaction
147
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
Chemical Reaction
148
particles provide energy required to break bonds
COLLISION
149
One compound decomposes to form two or more substance
DECOMPOSITION / ANALYSIS
150
Involves the reaction of two or more substances react to form one compound
DIRECT UNION/ SYNTHESIS / COMPOSITION
151
A change in the structure, properties, composition of the nucleus of an atom resulting in the transmutation of the element into another element.
NUCLEAR Change
152
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.
Greater
Greater
153
minimum amount of energy required for successful collision
Activation energy
154
Union of two light atoms to form a bigger molecule
Nuclear Fusion
155
Splitting of heavy atoms / seen having nucleus
Mass number = ↑ 200
Nuclear Fission
156
Splitting of heavy atoms / seen having nucleus
Mass number = ↑ 200
Nuclear Fission
157
When stress is applied to a system in equilibrium, the equilibrium will shift in such a MANNER as to relieve or neutralize the stress.
Le Chatelier's Principles
158
The rate of chemical reaction is directly proportional to the concentrations of the reactants at a given temperature.
Law of Mass Action
159
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
Law of Chemical Equilibrium
