Module 1.1: General Chemistry Flashcards
1
Q
It is anything that has mass and volume
A
Matter
2
Q
It is the amount of matter present in an object
A
Mass
3
Q
It is the amount of space occupied by an object
A
Volume
4
Q
It is the of
product of mass × by gravity (9.8m/s2)
A
Weight
5
Q
What are the properties of matter
A
Intensive or intrinsic
Extensive or extrinsic
6
Q
Properties that are independent on the amount of matter present
A
Intensive or intrinsic property
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
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
9
Q
Boiling point of water
A
100° c
10
Q
Properties that are dependent on the amount of matter present
A
Extensive or extrinsic property
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
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
13
Q
What are the changes of matter
A
Physical change
Chemical change
14
Q
It is observed or measured without changing the identity of matter
A
Physical change
15
Q
___ is a change in phase
A
Physical change
16
Q
Physically, MaVaSa ang LaVaVo
A
Physical change example melting point boiling point solubility viscosity length volume
17
Q
Describe the change or reaction a substance undergoes
A
Chemical change
18
Q
Change in both intrinsic and extrinsic properties
A
Chemical change
19
Q
Examples of chemical change
A
Flammability reactability formation of gas formation precipitate formation of odor change in color
20
Q
Fundamental states of matter
A
Solid
liquid
gas
Plasma
bose einstein condensate
21
Q
What is the molecular motion of solid liquid gas
A
solid- vibration
liquid- gliding
gas- random motion
22
Q
What is the shape of
solid
liquid
gas
A
solid- definite
liquid- indefinite
gas- indefinite
23
Q
What is the volume of
solid
liquid
gas
A
solid- definite
liquid- definite
gas- indefinite
24
Q
What is the ifa strength
solid
liquid
gas
A
solid- strongest
liquid- strong
gas- weakest
25
What is the compression of
solid
liquid
gas
solid- none
liquid- non or weak
gas- strongest
26
It is also known as plasma
Mesophase or liquid crystal
27
It is the fourth state of matter
Plasma
28
It has a solid and flow like properties
Plasma
29
Resembles those of a crystal in the formation of loosely ordered molecular arrays
Plasma
30
Ordered arrangement of atoms
Crystal lattice
31
Plasma is either
Smectic Nematic
32
Smectic is Nematic is
Smectic is a like or grease like
Nematic is thread like
33
What are the distinct crystal system
Cubic
Tetragonal
hexagonal
rhombic
orthoromobic
monoclinic triclinic
34
Shapes ?
Cubic
Tetragonal
hexagonal
rhombic
orthoromobic
monoclinic triclinic
Cubic - NaCl
Tetragonal- Urea
hexagonal- Iodoform
rhombic- Iodine
orthoromobic - Ritonavir II
monoclinic- Sucrose, Ritonavir I
triclinic- Boric acid
35
It is the degree of randomness
Entropy
36
It is the amount of heat present
Enthalpy
37
Plasma to gas
Decombination or deionization
38
Gas to plasma
Ionization
39
Gas to liquid
Condensation
40
Liquid to gas
Evaporation
41
Liquid to solid
Freezing or congealing
42
Solid to liquid
Melting point
43
Solid to gas
Sublimation
44
Gas to solid
Deposition
45
What are the laws of matter
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
45
The composition of a pure compound is always the same regardless of its source
Law of definite proportion or proust's law
46
In pure compounds the elements are always in the same proportion by mass
Law of definite proportion or proust's law
47
Atoms of two or more elements may combine in different ratios to produce more than one compound
Law of multiple proportion or dalton's law
48
No change is observed in the total mass of the substance involved in a chemical reaction
Law of conservation of mass
49
Energy is neither created or destroyed but it is conserved or transformed
Law of conservation of energy
50
Classification of matter
Pure and impure or mixture
51
What is the difference between pure and mixture or impure
Pure is chemically combined
Impure or mixture is not chemically combined but physically combined
And it can retain their individual properties
52
One kind of material atom is a theory of
Dalton's atomic theory
52
It is the simplest form of matter
Elements
53
Pure chemical substance
Elements
54
It cannot be decomposed by simple physical or chemical means into two or more different substances
Elements
55
Compose of two or more elements that unite chemically in different proportion
Compounds
56
Cannot be changed into simpler substances under normal laboratory condition
Compounds
57
True or false all molecules are considered compound
Because hydrogen gas is a molecule but not a compound
58
Classification of mixture
Nature of particles and particle size
59
Types of nature of particles in the classification of impure /mixture
Homogeneous and heterogeneous
60
What is the types of particle size in the context of classification of mixture
Solution
suspension
colloids
61
Consistent or uniform parts throughout
Homogeneous
62
Example is nacl dissolved in water, syrup, alloys
Homogeneous
63
Physically distinct parts
Heterogeneous
64
Example is sand and water mixture
Heterogeneous
65
True solution is __ mixture
Uniform
66
Atom or molecules and ions of the substance become dispersed
True solution
67
Contains particles bigger than those in solution but smaller than those in suspension
Colloids
68
Dividing line between solution and suspension
Colloids
69
Colloids particles of solid are broken down to the size of the molecule but are small enough in dispersed throughout the medium
Colloids
70
Example of colloids
Dust and mayonnaise
71
What are the properties of colloids
TBAC COL
Tyndall effect brownian movement
adsorption
charged electrically
72
Tyndall effect brownian movement
adsorption
charged electrically
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
73
Course mixture
Suspension
74
Finely divided solid materials distributed in liquid
Suspension
75
Factors affecting solubility
FAS NaTo Paster Paster Paster
Nature of solute and solvent
temperature
pressure
particle size
presence of salts
76
FAS NaTo Paster Paster Paster
Factors affecting solubility
Nature of solute and solvent
temperature
pressure
particle size
presence of salts
77
Refers to the maximum amount of solute expressed in grams that can be dissolved in 100 g of water
Solubility
78
Ability of one substance to mix with another substance
Miscibility
79
If temperature increases what happens to the solubility of solid in a liquid
Increases
If temperature increases it also increases the solubility of solid in a liquid
80
Temperature increases what happens to the solubility of a gas in a liquid
Decreases
If a temperature increases it decreases hindi solubility of a gas in a liquid
81
It absorbs heat and if temperature increases it also increases the solubility
Endothermic reaction
82
It releases heat and its temperature increases it decreases the solubility
Exothermic reaction
83
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
Henry's law of gas solubility
84
International system unit of pressure
Pascal
85
What happens to the solubility of gas if pressure increases
Increases
86
What happens to the surface area and solubility if particle size increases
Decreases
87
Presence of salt decrease as solubility
Salting out
88
Presence of salt increases solubility
Salting in
89
What are the types of solution
Saturated
unsaturated or diluted
super saturated or concentrated solution
90
Solution achieved the maximum solubility
Saturated solution
91
The solvent mar solute
Diluted or unsaturated
92
More solvent than solute
Supersaturated or concentrated
93
Interface to the limit before saturation in relation to ion
Solubility product constant
94
Q means
Degree of ion
95
Ion serves as an___ solubility product constant
Solute
96
Acid results to litmus paper
Blue to red
97
Base litmus test result
Red to blue
98
What is the taste of acid and base
Acid sour
Base is bitter
99
What are the theories in acid base equilibra
Arrhenius
Bronsted- Lowry
Lewis theory
100
What theory of acid base indicates that not hydroxyl group is base or basic because of ammonia
Arrhenius theory
101
Bro, acid ang PDos
Bronsted - Lowry theory
Acid: proton donor
Base : acceptor
102
What theory is that yields hydrogen and hydronium ion
Arrhenius theory: acid
103
What theory yield hydroxyl ion
Arrhenius theory: basic
104
What type of theory is an electron acceptor
Levi's theory : acid
105
It is formed from the neutralization reaction
Salts
106
Example of salts which are formed from the neutralization reaction
Strong acid + strong base
Strong acid + weak base
Weak acid + strong base
Weak acid + weak base
107
Identify their product
Strong acid + strong base
Strong acid + weak base
Weak acid + strong base
Weak acid + weak base
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
108
Acid + base=
Salt + h2o
109
Example of strong acids
HBCNIPS
Hydroboric acid
Hydrochloric acid
Nitric acid
Hydro ionic acid
Perchloric acid
Sulfuric acid
110
Examples of strong bases
Hydroxides
Group 1a and 2a
111
Ph is measured through
Sorensen's scale
112
General formula for Sorensen's scale
Ph + poh = 14
113
It measure the propensity of a larger object to separate or dissociate reversibly into smaller components
Dissociation constant
114
Ionic equilibra that completely dissociates
Strong acid base
115
Ionic equilibra that does not completely dissociate
Weak acid base
116
Ionic equilibrium that does not dissociate
Electrolytes
117
Example of strong acid base that completely dissociates
Sodium chloride
118
Example of weak acid that does not completely dissociates
Weak electrolytes such as buffer
119
Non electrolytes that does not dissociate example
Organic molecules such as glucose dextrose or other sugar
120
It gains or the need proton
Amphiprotic
121
Can neither gain or donate proton
Aprotic
122
It donates proton
Protogenic
123
Accepts proton
Protophilic
124
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
Buffer
125
What is the purpose of ph
It maintains neutrality
126
Buffer equation
Henderson hasselbalch equation
127
The magnitude of the resistance of a buffer to ph changes
Backer capacity
128
The ratio of the increment of strong base acids to the small changes in ph brought by this audition
Bakit capacity
129
Oil of vitreon is also known as
Sulfuric acid
130
What are the types of chemical reaction
Na CS si DanDan ng chemical reaction
Composition or synthesis or direct union
Decomposition or analysis
Single replacement
Double replacement
131
/It involves the formation of elements
/ it is a simple substance to complex substance
Composition , synthesis or direct union
132
/breakdown of compounds
/Complex substance to simpler substances
Decomposition or analysis
133
/defense on the activity series
/substitution
Single replacement
134
It is the most reactive element
Lithium
135
This the least reactive element
Silver
136
Acid + base--> salt + h2 O
Neutralization reaction
137
Folic acid + alkali -> soap
Saponification
138
Alcohol
Fermentation
139
Breakdown of bonds by the addition of H2O
Hydrolysis
140
Balance decreases and oxidation states decreases
Reduction
141
Red Cat Elect in
Reduction occurs in the cathode for electrons get in
142
Components within the nucleus
Nucleons : Protons and neutron s
143
What is the weight of electron in compared to proton
Electron has a negative charge and it is 1,836 x lighter than proton
144
The components within the nucleus is responsible for
Mass of an atom
145
He coined the term atom from the greek word atomos which means indivisible
Democritus
146
His model is billiard for model
John dalton
147
Hollow sphere
John dalton
148
May Billiard ball na si Dalton
The model of john dalton is billiard ball model
149
All matter are made up of atom
John dalton atomic theory
150
Each element has a different atoms
John dalton atomic theory
151
Atoms of an element are identical
John dalton atomic theory
152
atoms are rearranged in reaction
John dalton atomic theory
153
What is the model of jj thompson
Raisin bread or plum pudding model
154
Founded atoms could sometimes edject a far smaller negative particle called electron
Jj thompson
155
He founded electrons
Jj thompson
156
What is the model of ernest rutherford
Nuclear model
157
( 99% passed through but less than 1% deflected or blocked
Ernest rutherford
Gold film experiment
158
Discovery of proton
Ernest rutherford
159
Discovery of neutron
James Chadwick
160
It is the model of Neil Bohr
Planetary model
161
Redefined Rutherford first idea by adding that electrons were in orbitals like planets or orbiting the sun
Neil bohr
162
What is the model of erwin schrödinger
Quantum mechanical model
163
Quantum theory and wave theory
erwin schrödinger
164
The number of proton indicates the number of
Number of electron in neutral state
165
Atomic mass is also known as and its equation
Mass number is equal to p + n
166
Same elements in same number of protons but different number of neutrons
Isotope
167
It is the most abundant isotope of hydrogen
Protium
168
It is used as solvent for nmr studies
Heavy hydrogen or deuterium
169
Different elements and same number of mass number
isobar
170
Different elements same number of neutrons
Isotope
171
Different elements the same number of electrons
Isoelectronic
172
__ are different forms of an element
Allotropes
173
It is an atom of different element can link together in different ways the form substances with different properties
Allotropism
174
Example of an allotropism
Diamond
graphite
fullerene
These are allotropes of carbon
175
Who discovered the subatomic particle that is shown by the atomic number
Rutherford
176
It is a region in space where the probability of finding an electron is greatest
Orbitals
177
Are located in electron clouds or energy level
Electrons
178
One or more orbitals with of varying shape
Electron shell
179
Electrons occupying the outermost shell
Valence electrons
180
Group of numbers which shows the arrangement of electrons in an atom
Electron configuration
181
What are the electronic principle
Heisenberg uncertainty principle
Pauli's exclusion principle
Aufbau's binding
Hund's Rule
182
It is impossible to determine simultaneously the momentum and position of an electron
Heisenberg uncertainty principle
183
No 2 electrons can have the same exact set of quantum numbers
Pauli's exclusion principle
184
___; electrons are first placed on the subshell with a lower energy level
Aufbau's building: up principle
185
Electrons fill up orbitals singly first
Hands rule of pairing
186
Unpaired electrons are attracted to a magnet
Paramagnetism
187
Paired electrons repelled by a magnet
Diamagnetism
188
What are the two classification of hunds rule of pairing
Paramagnetism and diamagnetism
189
Principal quantum number symbol
n
190
It determines the main energy level or electron shell and the size of the orbital
Principal quantum number
191
It determines the shape and subshell
Azimuthal or angular quantum numbers
192
Azimuthal or angular quantum numbers symbol
l
193
194
KaAzi met ni SAS
Azimuthal or angular quantum number
It determines the angle, shape and subshell
195
What is the orbital number of
s
p
d
f
s-1
p-3
d-5
f-7
196
What is the maximum electron of
s
p
d
f
s-2
p-6
d-10
f-14
197
What is the azimuthal or angular quantum number
s
p
d
f
s-0
p-1
d-2
f-3
198
What is the shape of
s
p
d
f
s- sphere
p- dumbbell
d- clone/ double dumbbell
f- multiple lobes
199
Magnetic quantum numbers symbol
ml
200
It determines the special orientation
Magnetic quantum number
201
What is the values of Magnetic quantum number
-1 to + 1
202
What is the values of azimuthal or angular quantum number
0- (n-1)
203
What is the symbol of spin quantum numbers
ms
204
It describes the spin or rotation
Spin quantum number
205
Spin quantum number values
+ 1/2 or clockwise and
-1/2 counter clockwise
206
How many elements are there in periodic table
118
207
Horizontal in periodic table indicates the
7 periods from left to right homes
208
Vertical in periodic table indicates the
Group or family from top to bottom
209
Group a from periodic table is
Group B in periodic table is
Representative elements
S and I p block
Known oxidation state
Group b
Transition elements
D and F block
Transition oxidation state
210
Closely resembles the second number of an adjacent group to the right
Bridge element or diagonal element
211
Mg Li
Bo Si
Bridge element
Magnesium lithium
Boron silicon
212
Father of modern chemistry
Antoine laurent Lavoisier
213
Wrote the first extensive list of elements containing 33 elements
Antoine laurent Lavoisier
214
First true periodic table
Antoine laurent Lavoisier
215
Arrange the periodic table based on atomic mass
Meyer and Mendelev
216
Physical and chemical properties are periodic function of their atomic weight
Meyer and Mendelev
217
First true periodic law
Meyer and Mendelev
218
mu man Henry
Elements are arranged based on their atomic number: Henry moseley
219
Elements are arranged based on their atomic number:
Henry moseley
220
Modern periodic table
Henry moseley
221
Tri ta Johann
Introduce the law of triads according to physical properties: Johann dobereiner
222
Middle elements of a triad equal to the arithmic mean of atomic masses of other two elements
Johann dobereiner: law of triad
223
Introduce the law of triads according to physical properties:
Johann dobereiner
224
Every eight element is similar to the first element
Law of octa ves: john alexander newland
225
Law of john alexander newland
Law of octaves
226
Iron triad
Fe co Ni
227
Platinum triad
Ru Rh Rb
228
The property increases from right to left top to bottom
Metallic Radius
229
It is one of the distance between two nuclei
Atomic radius
230
The property increases from left to right bottom to top
Ionization energy anomaly INEA
231
Amount of energy required to remove an electron from a neutral atom to convert it to a positively charged ion
Ionization energy
232
The tendency of an atom to attract electrons itself
Electronegativity
233
Amount of energy released when a natural atom to convert it to negatively charged ion
Electron affinity
234
Intermediate between metals and metals
Metalloids
235
Example of metalloids
Si
Ge
Po
Sb
As
Te
B
236
It deals with the energy transformation
Thermodynam
237
Any part of the universe which isolated from the rest by a boundary on a wall
System
238
Everything outside the system
Surrounding
239
What are the types of thermodynamics
Open
closed
isolated
240
Types of isolated thermodynamics
Adiabatic
Diathermal
241
Allows the exchange of both matter and energy
Open thermodynamics
242
It allows the exchange of energy but not matter
Closed thermodynamics
243
It does not allow the exchange of both matter and energy
Isolated thermodynamics
244
Isolated thermodynamics it does not allow energy or heat flow
Adiabatic (isolated thermodynamics)
245
It allows energy and heat flow
Diathermal (isolated thermodynamic)
246
An energy transfer due to temperature difference
Heat (q)
247
Refers to the total in content
Enthalpy (H)
248
Measure of degree of randomness or disorderliness of a system
Entropy (S)
249
What are the thermodynamic functions
Heat
enthalpy
Entropy
250
What are the law of thermodynamics
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
Measure of spontaneity
Gibb's free energy
252
All of the atoms and molecules behave independently
Kinetic molecular theory of gases
253
No attractive or repulsive forces exist between atoms or molecules in a gas
Kinetic molecular theory of gases
254
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
Kinetic molecular theory of gases
255
The average kinetic energy of atoms or molecules increases
Kinetic molecular theory of gases
256
Boyle's law is also known as
Mariotte law
257
In boyle's law what is the relationship between pressure and volume
Pressure is inversely proportional to volume
258
What is constant in boyle's law
Temperature
259
What is constant in charles' law
Pressure
260
Pressure what is the relationship of volume and temperature in charles law
Directly proportional
261
Gay-lusacc's law is also known as
Amonton's law
262
What is constant in gay-lussac's law
Volume volume
263
What is the relationship of pressure and temperature in gay-lussac's law
Directly proportional
264
Equal volume of different gases have the same number of moles of at standard temperature and pressure
Avogadro's law
265
Avogadro's number
6.022x 10raised 23
266
Formula for avogadro's number
V1/n1 = V2/n2
267
Formula for combined gas law
P1V1/n1 = P2V2/n2
268
Provides convenient expression for performing gas law calculation involving the most common variable such as pressure volume and temperature
Combined gas law
269
Formula for ideal gas law
PV= nRT
P- 1atm
v- 22.4L
n - no. of mole
R- gas constant (0.08205L × atm / mol × K
T- 273.15 K
270
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
Dalton's law of partial pressure
271
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
Graham's law
272
Gradual mixing of molecules of one gas when the molecules of another gas
Diffusion
273
Passage of a gas under pressure through a small opening
Effusion
274
Change in structure properties composition of the nucleus of an atom resulting in the transformation of an element into another element
Nuclear change
275
Splitting of heavy atom
Nuclear fission
276
Union of two light atoms to form a bigger molecule
Nuclear fusion
277
It is a process of decomposition of unstable nuclei tumor stable or once
Radioactivity
278
Energy and particles release during the decomposition process
Radiation
279
What are the units of radioactivity
Non SI : Curie
SI: Becquerel (Bq)
280
Non SI : Curie = __ decays/sec
3.7 × 10 raised to 10
281
SI: Becquerel (Bq)= ___ decays/sec
1
282
What are the units of radiation damage
Roentgen's equivalent Man RE
283
What are the types of decay
Alpha
beta
gamma
284
Unit of amount of exposure to radiation
Rad/gray
285
What are the penetrating power of
Alpha
beta
gamma
Alpha- low
beta -; medium
gamma=high, which is dangerous
286
Alpha
beta
gamma
is blocked by
Alpha- paper
Beta- aluminum
gamma- lead
287
Refers to the study of rate for speed of chemical reaction
Chemical kinetic s
288
Finished reaction
Chemical reaction
289
Chemical reaction that shifts to the right
Forward reaction
290
Chemical reaction that shift to the left
Backward reaction
291
Collision theory
Increase in rate is equal to increase in collision
292
Should be overcome for the reaction to proceed
Activation energy
293
What is the proper orientation of the collision theory
It should be a lower activation energy for it to overcome
294
Reactants will undergo a transition state in order to produce products
Transition state theory
295
What are the factors affecting the rate of reaction
Particle size
concentration
nature of reactant
temperature
296
It states that narrate of forward reaction is equal to the rate of factor reaction
Chemical equilibrium
297
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
Le chatelier's principle
298
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
Law of mass action
299
Factors affecting the equilibrium
Concentration
pressure
temperature
300
Add A or b in concentration
Forward
300
Add C or D in concentration
Backward
301
Increase in pressure and decrease in volume is ___ number of moles
Less
302
Decrease in pressure and increase in volume is ___ number of moles
More
303
Reactant in factors affecting the equilibrium
Endothermic
304
Product in factors affecting the equilibrium
Exothermic
