Introduction to Chemistry Flashcards
(99 cards)
1
Q
Khemein or Khemia
A
“preparation of black powder”
from Greek
2
Q
Chymist
A
“alchemist”
from French
3
Q
anything that has mass and volume
A
matter
4
Q
5 states of matter
A
solid
liquid
gas
plasma
bose-einstein condensate
5
Q
describe solid
A
- non-compressible
- vibrates when collided
6
Q
describe liquid
A
- assumes the container’s shape
- glides on solid surfaces
7
Q
describe gas
A
- compressible
- neutrally charged (p+ & e-)
8
Q
describe plasma
A
- abundant protons and electrons (affects magnetic field)
- most abundant state of matter (ionized neon lights, auroras, stars, sun)
9
Q
INTERMOLECULAR FORCES OF ATTRACTION
highest to lowest attraction in order
A
solid
liquid
gas
plasma
10
Q
ENTHALPY (HEAT/REACTION ENERGY)
highest to lowest attraction in order
A
plasma
gas
liquid
solid
11
Q
saturated with p+ and e-
A
plasma
12
Q
other names of MELTING
A
fusion
liquefaction
thawing
13
Q
other name of VAPORIZATION
A
evaporation
14
Q
other names of RECOMBINATION
A
de-ionization
15
Q
melting
A
solid to liquid; caused by heating
16
Q
freezing
A
liquid to solid, caused by cooling a liquid.
17
Q
vaporization
A
- liquid to gas (vapor) due to the escape of - - molecule from the surface.
18
Q
condensation
A
- gas to liquid
- naturally caused by cooling.
19
Q
sublimation
A
- solid to gas
- from solid to gaseous on heating, & from gaseous directly to solid on cooling.
20
Q
deposition
A
- gas to solid
- direct transition from vapor state to the solid state
21
Q
ionization
A
gas to plasma
22
Q
recombination
A
plasma to gas
23
Q
2 classifications of matter
A
- pure substance
- mixture
24
Q
what is pure substance
A
- it cannot be separated by any physical means
- has a definite and constant composition
- possesses distinct chemical properties
25
what is mixture
2 or more substances wherein individual identities of the substances are retained
26
types of pure substance
1. element
2. compoundt
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types of mixture
1. homogenous
2. heterogenous
28
element
- pure substance
- simplest form of matter
- 1 kind of material or atom
- has definite chemical composition
- cannot be decomposed by simple physical or chemical means into two or more different substances
29
compound
- elements chemically combined (must have chemical reaction)
- substance composed of two or more elements which combines chemically in definite proportion
- cannot be changed into simpler substances under normal laboratory conditions
30
homogenous mixture
1 single phase (solution)
31
solution
- uniform mixture
- composed of solute and solvent
- wherein atoms, molecules or ions of the substance becomes dispersed
32
heterogenous mixture
2 phases (suspension and colloids)
SUSPENSION
COLLOIDS
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- aka "coarse mixture"
- madali maexpire
- solid particles do not dissolve, they are clumped or suspended in a solution
- homogenous dispersion insoluble in a liquid
- finely divided solid materials distributed in liquid
SUSPENSION
34
- microscopically dispersed insoluble particles suspended in a solution
- contain particles bigger than those in solutions, but smaller than those in suspension
- particle of solute are not broken down to the size of the molecules but are dispersed throughout the medium
- exhibit the light scattering effect
COLLOIDS
35
properties of colloids
1. TYNDALL EFFECT
- light-scattering effect
2. BROWNIAN MOVEMENT
- zig-zag movement of colloidal particles
3. ELECTRICALLY CHARGED
4. ADSORPTION
36
death of cells
necrosis
37
- degree of messiness
- measure of how disordered a system is
entropy
38
measure of energy in a thermodynamic system
enthalpy
39
CLASSIFICATION BASED ON DEPENDENCE TO THE AMOUNT OF MATTER PRESENT
extrinsic property
intrinsic property
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describe extensive/extrinsic property
- dependent on matter present
- mostly depend also on external factors
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describe intensive/intrinsic property
- independent on matter presen
- constant
- characteristics of any sample of the substance regardless of the shape or size of the sample
- inherent to a sample
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examples of extrinsic property
length, mass/weight, volume, pressure, entropy, enthalpy, electrical substance
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examples of intrinsic property
density/specific gravity, viscosity, velocity, temperature, color, pH, concentration, boiling point, melting point, freezing point, sublimation temperature, optical activity
44
what is chemistry?
chemistry is the study of matter, its properties, how and why substances combine or separate to form other substances, and how substances interact with energy.
45
5 branches of chemistry
organic chemistry
inorganic chemistry
biochemistry
analytical chemistry
physical chemistry
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organic chemistry
- chemistry of life
- study of carbon-containing compounds
47
inorganic chemistry
the study of inorganic compounds, or compounds that don't contain the C-H bond
48
biochemistry
study of chemical processes that occurs on living organisms
"chemistry in life"
49
analytical chemistry
study of the chemistry of matter and the development of tools and measure their properties
QC/QA
50
physical chemistry
branch of chemistry that applies physics (thermodynamics and quantum mechanics)
51
what is matter? (3)
- anything that occupies space and has mass
- predominantly composed of atoms, molecules and ions
- interconvertible with energy
52
other names of plasma
mesophase or liquid crystals
53
resemble those of a crystal in the formation of loosely ordered molecular arrays similar to a regular crystalline lattice & anisotropic refraction of light
ex. lightning, aurora borealis
plasma
54
solidification
liquid to solid
solid at room temperature and atmospheric pressure
55
refers to the gaseous phase of a substance, which is normally liquid or solid at room temperature.
vapor
56
boiling
liquid to gaseous (vapor)
at a temperature called boiling point
57
Liquefaction
- gas-liquid at a substance which is gas at room temperature & pressure.
- It is caused by cooling & increasing pressure.
58
classification of compounds
- law of definite proportion
- law of multiple proportion
59
classification of homogenous
solution
suspension
colloids
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2 changes that matter undergoes
physical and chemical change
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physical change
change in phase
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chemical change
change in both extrinsic and intrinsic properties
63
6 evidences of chemical change
- evolution of gas
- formation of precipitate
- emission of light
- generation of electricity
- production of mechanical energy
- adsorption/liberation of heat
64
10 forms of energy
kinetic energy
potential
chemical
thermal
electromagnetic
electrical
nuclear
activation
bond
ionization
65
- energy of motion
- related to their temperature; the higher the temperature, the more kinetic energy the molecules have.
kinetic energy
66
- stored energy, which can be due to the position of an object or its composition
- often associated with the energy stored in chemical bonds.
potential energy
67
- form of potential energy stored in chemical bonds.
- During chemical reactions, bonds are broken and formed, which can release or absorb energy.
chemical energy
68
- total kinetic energy of all particles in a substance, related to temperature.
- It's a measure of the internal energy of a system due to its temperature.
thermal energy
69
- Also known as radiant energy, this includes energy from electromagnetic waves, such as light.
- In chemistry, this form of energy is crucial in processes like photosynthesis and spectroscopy.
electromagnetic energy
70
- energy associated with electric charges and their movement.
- In electrochemistry, for example, electrical energy is essential for driving chemical reactions in batteries and electrolysis.
electrical energy
71
- energy stored in the nucleus of an atom.
- can be released through nuclear reactions, such as fission or fusion, though this is more relevant to nuclear chemistry and physics.
nuclear energy
72
- minimum energy required to initiate a chemical reaction.
- It’s the energy needed to reach the transition state from reactants to products.
activation energy
73
- energy required to break a chemical bond.
- It's a specific type of potential energy and is crucial in determining the stability of molecules.
bond energy
74
- energy required to remove an electron from an atom or ion.
- It’s a key concept in atomic chemistry, influencing how atoms interact and form bonds.
ionization energy
75
LAWS GOVERNING MATTER AND ENERGY
1. Law of Conservation of Mass: matter is neither created nor destroyed.
2. Law of Definite Proportions
3. Law of Multiple Proportions
76
- This shows that both sides of the equation have the same number and type of elements.
- states that matter cannot be created or destroyed.
Law of Conservation of Mass
77
- a given compound always contains exactly the same proportion (ratio) of elements by mass.
- Any sample of pure water contains 11.19% Hydrogen and 88.81% Oxygen by mass, whether it comes from different source and preparation, the composition is fixed.
Law of Definite Proportions
78
- when two elements form a series of compounds, the ratios of the 2nd elements that combine with the first element can be reduced to small whole numbers
Law of Multiple Proportions
79
who created the law of conservation of mass/matter?
Antoine Lavoisier
80
who created the law of definite/constant proportion?
Proust Law
81
who created the law of multiple proportion?
John Dalton
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what is law of combining weights
- proportions by weight when chemical reaction takes place
- can be expressed in small integral units
83
what is organic chemistry?
"chemistry OF life"
84
what is biochemistry?
- study of "chemistry IN life"
- metabolism
85
the lesser electrons....
the more stable
86
halides are in group...
group VII
87
biggest element
francium
88
smallest element
helium
89
stable elements are in group...
group VIII
90
what are the alkali metal elements?
Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), Francium (Fr)
91
what are the halogen/halide elements?
Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At), Tennessine (Ts)
92
what are the noble gas elements?
Helium, Neon, Argon, Krypton, Xenon, Radon, Oganesson
93
what are the non-metal elements?
Carbon, Nitrogen, Oxygen, Phosphorous, Sulfur, Selenium
94
atomic mass of carbon
12
95
atomic mass of nitrogen
14
96
atomic mass of oxygen
16
97
atomic mass of fluorine
18
98
atomic mass of potassium
39
99
atomic mass of iodine
127
