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(SLU) PHARMA 113: Chem Lec > Introduction to Chemistry > Flashcards

Introduction to Chemistry Flashcards

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1
Q

Khemein or Khemia

A

“preparation of black powder”
from Greek

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2
Q

Chymist

A

“alchemist”
from French

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3
Q

anything that has mass and volume

A

matter

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4
Q

5 states of matter

A

solid
liquid
gas
plasma
bose-einstein condensate

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5
Q

describe solid

A
  • non-compressible
  • vibrates when collided
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6
Q

describe liquid

A
  • assumes the container’s shape
  • glides on solid surfaces
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7
Q

describe gas

A
  • compressible
  • neutrally charged (p+ & e-)
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8
Q

describe plasma

A
  • abundant protons and electrons (affects magnetic field)
  • most abundant state of matter (ionized neon lights, auroras, stars, sun)
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9
Q

INTERMOLECULAR FORCES OF ATTRACTION
highest to lowest attraction in order

A

solid
liquid
gas
plasma

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10
Q

ENTHALPY (HEAT/REACTION ENERGY)
highest to lowest attraction in order

A

plasma
gas
liquid
solid

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11
Q

saturated with p+ and e-

A

plasma

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12
Q

other names of MELTING

A

fusion
liquefaction
thawing

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13
Q

other name of VAPORIZATION

A

evaporation

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14
Q

other names of RECOMBINATION

A

de-ionization

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15
Q

melting

A

solid to liquid; caused by heating

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16
Q

freezing

A

liquid to solid, caused by cooling a liquid.

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17
Q

vaporization

A
  • liquid to gas (vapor) due to the escape of - - molecule from the surface.
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18
Q

condensation

A
  • gas to liquid
  • naturally caused by cooling.
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19
Q

sublimation

A
  • solid to gas
  • from solid to gaseous on heating, & from gaseous directly to solid on cooling.
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20
Q

deposition

A
  • gas to solid
  • direct transition from vapor state to the solid state
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21
Q

ionization

A

gas to plasma

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22
Q

recombination

A

plasma to gas

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23
Q

2 classifications of matter

A
  1. pure substance
  2. mixture
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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
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25
Q

what is mixture

A

2 or more substances wherein individual identities of the substances are retained

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26
Q

types of pure substance

A
  1. element
  2. compoundt
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27
Q

types of mixture

A
  1. homogenous
  2. heterogenous
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28
Q

element

A
  • 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
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29
Q

compound

A
  • 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
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30
Q

homogenous mixture

A

1 single phase (solution)

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31
Q

solution

A
  • uniform mixture
  • composed of solute and solvent
  • wherein atoms, molecules or ions of the substance becomes dispersed
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32
Q

heterogenous mixture

A

2 phases (suspension and colloids)

SUSPENSION

COLLOIDS

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33
Q
  • 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
A

SUSPENSION

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34
Q
  • 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
A

COLLOIDS

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35
Q

properties of colloids

A
  1. TYNDALL EFFECT
    - light-scattering effect
  2. BROWNIAN MOVEMENT
    - zig-zag movement of colloidal particles
  3. ELECTRICALLY CHARGED
  4. ADSORPTION
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36
Q

death of cells

A

necrosis

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37
Q
  • degree of messiness
  • measure of how disordered a system is
A

entropy

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38
Q

measure of energy in a thermodynamic system

A

enthalpy

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39
Q

CLASSIFICATION BASED ON DEPENDENCE TO THE AMOUNT OF MATTER PRESENT

A

extrinsic property
intrinsic property

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40
Q

describe extensive/extrinsic property

A
  • dependent on matter present
  • mostly depend also on external factors
41
Q

describe intensive/intrinsic property

A
  • 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
42
Q

examples of extrinsic property

A

length, mass/weight, volume, pressure, entropy, enthalpy, electrical substance

43
Q

examples of intrinsic property

A

density/specific gravity, viscosity, velocity, temperature, color, pH, concentration, boiling point, melting point, freezing point, sublimation temperature, optical activity

44
Q

what is chemistry?

A

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
Q

5 branches of chemistry

A

organic chemistry
inorganic chemistry
biochemistry
analytical chemistry
physical chemistry

46
Q

organic chemistry

A
  • chemistry of life
  • study of carbon-containing compounds
47
Q

inorganic chemistry

A

the study of inorganic compounds, or compounds that don’t contain the C-H bond

48
Q

biochemistry

A

study of chemical processes that occurs on living organisms

“chemistry in life”

49
Q

analytical chemistry

A

study of the chemistry of matter and the development of tools and measure their properties

QC/QA

50
Q

physical chemistry

A

branch of chemistry that applies physics (thermodynamics and quantum mechanics)

51
Q

what is matter? (3)

A
  • anything that occupies space and has mass
  • predominantly composed of atoms, molecules and ions
  • interconvertible with energy
52
Q

other names of plasma

A

mesophase or liquid crystals

53
Q

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

A

plasma

54
Q

solidification

A

liquid to solid
solid at room temperature and atmospheric pressure

55
Q

refers to the gaseous phase of a substance, which is normally liquid or solid at room temperature.

A

vapor

56
Q

boiling

A

liquid to gaseous (vapor)
at a temperature called boiling point

57
Q

Liquefaction

A
  • gas-liquid at a substance which is gas at room temperature & pressure.
  • It is caused by cooling & increasing pressure.
58
Q

classification of compounds

A
  • law of definite proportion
  • law of multiple proportion
59
Q

classification of homogenous

A

solution
suspension
colloids

60
Q

2 changes that matter undergoes

A

physical and chemical change

61
Q

physical change

A

change in phase

62
Q

chemical change

A

change in both extrinsic and intrinsic properties

63
Q

6 evidences of chemical change

A
  • evolution of gas
  • formation of precipitate
  • emission of light
  • generation of electricity
  • production of mechanical energy
  • adsorption/liberation of heat
64
Q

10 forms of energy

A

kinetic energy
potential
chemical
thermal
electromagnetic
electrical
nuclear
activation
bond
ionization

65
Q
  • energy of motion
  • related to their temperature; the higher the temperature, the more kinetic energy the molecules have.
A

kinetic energy

66
Q
  • stored energy, which can be due to the position of an object or its composition
  • often associated with the energy stored in chemical bonds.
A

potential energy

67
Q
  • form of potential energy stored in chemical bonds.
  • During chemical reactions, bonds are broken and formed, which can release or absorb energy.
A

chemical energy

68
Q
  • 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.
A

thermal energy

69
Q
  • 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.
A

electromagnetic energy

70
Q
  • energy associated with electric charges and their movement.
  • In electrochemistry, for example, electrical energy is essential for driving chemical reactions in batteries and electrolysis.
A

electrical energy

71
Q
  • 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.
A

nuclear energy

72
Q
  • minimum energy required to initiate a chemical reaction.
  • It’s the energy needed to reach the transition state from reactants to products.
A

activation energy

73
Q
  • energy required to break a chemical bond.
  • It’s a specific type of potential energy and is crucial in determining the stability of molecules.
A

bond energy

74
Q
  • 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.
A

ionization energy

75
Q

LAWS GOVERNING MATTER AND ENERGY

A
  1. Law of Conservation of Mass: matter is neither created nor destroyed.
  2. Law of Definite Proportions
  3. Law of Multiple Proportions
76
Q
  • This shows that both sides of the equation have the same number and type of elements.
  • states that matter cannot be created or destroyed.
A

Law of Conservation of Mass

77
Q
  • 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.
A

Law of Definite Proportions

78
Q
  • 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
A

Law of Multiple Proportions

79
Q

who created the law of conservation of mass/matter?

A

Antoine Lavoisier

80
Q

who created the law of definite/constant proportion?

A

Proust Law

81
Q

who created the law of multiple proportion?

A

John Dalton

82
Q

what is law of combining weights

A
  • proportions by weight when chemical reaction takes place
  • can be expressed in small integral units
83
Q

what is organic chemistry?

A

“chemistry OF life”

84
Q

what is biochemistry?

A
  • study of “chemistry IN life”
  • metabolism
85
Q

the lesser electrons….

A

the more stable

86
Q

halides are in group…

A

group VII

87
Q

biggest element

A

francium

88
Q

smallest element

A

helium

89
Q

stable elements are in group…

A

group VIII

90
Q

what are the alkali metal elements?

A

Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), Francium (Fr)

91
Q

what are the halogen/halide elements?

A

Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At), Tennessine (Ts)

92
Q

what are the noble gas elements?

A

Helium, Neon, Argon, Krypton, Xenon, Radon, Oganesson

93
Q

what are the non-metal elements?

A

Carbon, Nitrogen, Oxygen, Phosphorous, Sulfur, Selenium

94
Q

atomic mass of carbon

A

12

95
Q

atomic mass of nitrogen

A

14

96
Q

atomic mass of oxygen

A

16

97
Q

atomic mass of fluorine

A

18

98
Q

atomic mass of potassium

A

39

99
Q

atomic mass of iodine

A

127

(SLU) PHARMA 113: Chem Lec (10 decks)

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