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is the science that studies the properties, composition and structures of matter and the changes it undergoes.
Chemistry
Organic Chemistry
Inorganic Chemistry
Analytical Chemistry
Biochemistry
Branches of Chemistry: (O I A B)
Organic Chemistry
deals with the structure, properties, and reactions of compounds that contain carbon, hydrogen, oxygen, nitrogen and phosphorus.
Analytical Chemistry
study of qualitative and quantitative analysis of elements and compounds.
Biochemistry
study of chemical reactions that happen within the biological processes
Inorganic Chemistry
study of all elements and compounds that aren’t organic compounds
PROPERTIES OF MATTER: (P C I E)
Physical
Chemical
Intrinsic/Intensive
Extrinsic/Extensive
Physical Properties
those that a substance shows by itself, without changing or interacting with another substance, e.g. color, melting point, and density
Chemical Properties
those that a substance shows as it changes into or interacts with another substance, e.g. flammability, corrosiveness
Intrinsic/Intensive Properties
independent of the amount of material, e.g. solubility, boiling point, density
Extrinsic/Extensive Properties
dependent on the amount of material, e.g. mass, weight, volume
Physical
Chemical
Changes in Matter: (P C)
Physical change
occurs when a substance alters its physical form, NOT its composition (melting, sublimation, evaporation, condensation, freezing, deposition)
Chemical Change
occurs when a substance is converted into a different substance (chemical reactions such as burning and oxidation)
Solid
Liquid
Gas
States of Matter:
Solid
has a fixed shape with particles close together and organized
Gas
conforms to container shape but fills the entire container and with particles far apart and disorganized.
Liquid
conforms to the container’s shape but fills the container only to the extent of the liquid’s volume with particles which are close together but disorganized.
Substances
Pure matter; composition same throughout; single phase
Elements
Metals
Nonmetals
Metalloids
___substances made up of only one kind of atom
• ___ (electric conductors)
• ___ (non-conductors)
• ___ (semi-conductors)
Isotopes
elements w/ the same atomic number, different mass.
Noble Gases
All of them have completely filled electron shells. Since they have similar electronic structures, their chemical reactions are similar as well
Compounds
substances made up of two or more kinds of atoms; cannot be separated by physical means.
Mixtures
Heterogeneous
Homogenous
Colloids
Suspensions
_____ composed of two or more materials and can be separated by physical means
A. _____ mixture of substances of different phases
B. _____ composition is the same throughout
• ______ composed of two phases of matter (dispersed and continuous phase)
• ______ mixture of liquid and relatively large particles of solids.
Law of Definite
Composition states that a compound is formed by combining elements in ratios of simple whole numbers.
Law of Definite Proportion
states that every sample of a specific substance always contains the same proportion by mass of its components.
Law of Multiple Proportions
states that if two elements form multiple compounds, the ratios of the masses of the second element combining with a fixed mass of the first elements will be in ratios of small whole numbers.
Chemical formula
formula that gives the number of atoms of each type in a molecule.
Ions
Cations
Anions
_____ are atoms or groups of atoms that carry an electric charge. _____ carry positive charges while _____ carry negative charges. Charges are determined by the number of electrons relative to the number of protons in an atom or a group of atoms.
Electrically neutral
Electrically positive
Electrically negative
________ if the number of protons (or atomic number) is equal to its number of electrons (p + =e-
________ if the number of electrons is less than its number of protons (e- < p+)
________ if the number of electrons is greater than its number of protons (e- > p +)
mole
amount of substance that contains as many entities (atoms, molecules or other particles as 12 grams of pure carbon- 12 atoms)
6.022 x 1023 atoms (Avogadro's number)
1 mole =
Stoichiometry
determination or measurement of chemical quantities; often involves conversion processes (examples of conversion processes: Celsius to Fahrenheit, peso to dollar).
Electronic Configuration
Energy level
Sublevel
______ The arrangement of electrons of an atom in specific energy levels (shells) and orbitals (sublevels) around the nucleus.
______ region in space where certain electrons are most likely found
______ is a subdivision within an energy level that contains orbitals of the same type (s, p, d, or f) where electrons are located.
s (sharp)
p (principal)
d (diffuse)
f (fundamental)
____ max of 2 electrons (1 orbital)
____ max of 6 electrons (3 orbitals)
____ max of 10 electrons (5 orbitals)
____ max of 14 electrons (7 orbitals)
Pauli exclusion principle
Hund's rule
Aufbau principle
Rules for electron configuration: (P H A)
Pauli exclusion principle
no two electrons can have the same four quantum numbers
Hund's rule
Electrons occupy orbitals singly before pairing up
Aufbau principle
electrons assigned relative to atomic number with lower levels occupied first.
Kinetic Molecular Theory
- Gases consist of large numbers of molecules that are in continuous, random motion
- The volume of all the molecules of the gas is negligible compared to the total volume in which the gas is contained
- Attractive and repulsive forces between gas molecules is negligible
- The average kinetic energy of the molecules does not change with time (as long as the temperature of the gas remains constant)
- Energy can be transferred between molecules during collisions (but the collisions are perfectly elastic)
- The average kinetic energy of the molecules is proportional to absolute temperature.
Boyle’s Law
Temperature
If the volume increases, the pressure decreases.
_____ is constant
Charle’s Law
Pressure
if the temperature increases, the volume increases.
______ is constant
Gay-Lussacs’ law
Volume
if temperature increases, the pressure increases.
_____ is constant
Combination/Formation reaction
Decomposition
Single replacement
Double replacement/Double decomposition
Types of Chemical reactions:
Combination/Formation reaction
A + B -> AB
Decomposition
AB -> A + B
Single replacement
A + BX -> AX + B
Double replacement/Double decomposition
AX + BY -> AY + BX
Catalyst
a _____ speeds up the reaction but does not affect the amount of the reactants and/or the products.
Reactant
Product
Balancing chemical reactions:
In a balanced equation, each kind of atom has the same number of atoms for both sides of the equation → The left (____) side does not contain more than the right (the ____side); the right does not contain more than the left.
Sour
Corrosive
Ionize
Acid ionization
blue
red
Basic Characteristics of Acids:
- They have a taste and are highly __; they have a pH (power of Hydrogen) of 1≤acid< 7.0
- Strong acids completely ionize while the weak acid ionization is not complete.
- turns ___ litmus paper to __.
Bitter
Slippery
red
blue
Basic Characteristics of Bases:
- They have a ___ taste and feel ___; they have a pH (power of Hydrogen) of 7.0<base≤14.0
- turns ___ litmus paper to ___.
7.0
Neutral compounds have a pH value of ___.
pH scale
Logarithm of the reciprocal of the hydronium ion concentration
Lewis Acid-Base Concept
Lewis base
Lewis acid
_____ donates an electron pair in the covalent bonding.
_____ accepts the unshared electron pair.
Amphoteric compounds
substances that can act both as an acid and a base
Intramolecular forces
• Within each molecule
• Influence of chemical properties of the substance
• Bonding
Intermolecular forces
• Between molecules
• Influence of physical properties of the substance
• Nonbonding
Hydrocarbons
Alkanes
Alkenes
Alkynes
The most common organic compounds are _____ which mainly consist of hydrogen and carbon. These can be classified as ___, ___, and ___.
Meth
Eth
Prop
But
Pent
Hex
Hept
Oct
Non
Dec
Number of Carbons:
1-
2-
3-
4-
5-
6-
7-
8-
9-
10-
Alkanes
consist of single bonds.
These names of these organic compounds end in the suffix –ane.
Their molecular formulas follow the format CnH2n+2.
Ex. hexane, C6H14
Alkenes
have at least one double bond.
Their names of these end in –ene.
Their molecular formulas follow the format CnH2n.
Ex. propene, C3H6
Alkynes
have at least one triple bond.
Their names end in –yne.
Their molecular formulas follow the format CnH2n-2.
Ex. decyne, C10H18.
First Law of Thermodynamics
Heat flow
Work done
also known as Law of Conservation of Energy
states that energy cannot be created or destroyed in an isolated system.
All energy transfers can be described as either ____ or as ____ on or by a system.
Second law of thermodynamics
states that the entropy of any isolated system always increases.
Entropy
is a measure of the disorder or randomness of a system.
Third law of thermodynamics
states that the entropy of a perfect crystal at absolute zero temperature is exactly equal to zero.