CHEM
Study of matter and the changes it undergoes. (physical and chemical)
Chemistry
Cleaning purposes
Ammonia
Neutralize soil acidity
Calcium hydroxide
An antacid active ingredient, baking
Sodium bicarbonate
Good rust and stain remover and used in commercial cleaning
Oxalic Acid
Gives sour milk it's sharp taste; responsible for muscle fatigue
Lactic acid
Food preservative and food additive
Ascetic acid
Made up of two or more pure substances that are physically combined
Mixture
Observed and measured without changing the composition or identity
Physical Property
Observed only if it will undergo chemical change. Forms new substance
Chemical property
First organic compound that is derived from inorganic (French Wohler-Father of Organic Chemistry)
Urea
Father of Organic Chemistry
Friedreich Wohler
Lipids serving as energy storage and structural components of cell membranes
Fats and oils
Macromolecule carrying genetic information in living organisms
DNA Deoxyribunucleic acid
Simple sugar and essential energy source for living organisms
Glucose C6H12O6
Alcohol used in beverages and as fuel
Ethanol C2H5OH
The force that acts on the surface of a liquid
Surface tension
Organic compounds are generally poor conductors of electricity
Electrical conductivity
Ability of a substance to exist in different crystalline forms
Polymorphism
Types of intermolecular bonding
Ionic bonding, hydrogen bonding, dipole-dipole interaction, van Der waals interactions
Strongest bonding /weakest bonding
Ionic/van Der waals
French chemist who defined element as any substance that could not be decomposed into simpler substances.
Antoine Lavoiser (1743-1994)
study of compounds that do not contain carbon as a central element. It is the study of feature and characteristics of metals and minerals
Inorganic Chemistry
deals with the chemical compounds and reactions that occur in living organisms. It is where chemistry and biology meet
Biochemistry
Father of Analytical Chemistry
Izaak Maurits Kolthoff
most fundamental and applies the theories of physics (specially thermodynamics) to the study of chemical systems in general
Physical Chemistry
describes an entity that occupies space, contains various particles, has different size and mass, and exhibits inertia
Matter
Energy In / particles move away / absorbs heat and energy
Endothermic
Energy Out / particles are closer / Releases energy or heat
Exothermic
He named the Proton
Ernest Rutherford
Negatively charged particles discovered by John Joseph Thompson in 1897
Electrons
uncharged paprticles
discovered by James Chadwick in 1932.
Neutrons
atoms that have the same atomic number but different mass numbers.
Isotopes
Isotopes of elements are identified by their mass numbers
an arrangement of chemical elements that is very helpful tool for determining their chemical properties. This summarizes the relationship between elements.
Periodic table
States that the physical and chemical characteristics of the elements are periodic functions of thir atomic numbers
Modern Periodic Law
columns of elements
Group/Family
majority of the elements in the periodic table; Left side of the periodic table are called
Metals
zigzag/staircase pattern on the periodic table; same physical appearance as metals but behaves chemically like non-metals
Metalloids
Semi metals elements are
B, Si, Ge, As, Sb, Te, Po
groups designated by a numeral and the letters B
Transition elements
a representation of the arrangement of atom and its distribution. It denotes how the electrons are distributed among the various atomic orbitals, in order to understand electronic behavior
Electron Configuration
Atoms that have a charge, meaning the number of protons is not equal to the number of electrons, giving the atom positive o negative net charge
Ions
an electrically neutral particle composed of two or more atoms chemically bonded. They can be a combination of atoms of the same element or different elements
Molecule
there are 7 common elements that exist as atomic molecules. Their atoms are too reactive to exist as independent ndividuals
H2,N2,O2,2,Cl2,Br2,I2
Have No Fear Of Ice Cold Beer
depends on how much matter a sample contains
Extensive Properties
Do not depend on the amount of matter in the sample
Intensive Properties
unique state of matter that occurs when the temperatures closed to zero
Boise-Einstein Condensate
Measurement of how tightly a material is packed together.
Mass per unit volume
Density
solid to liquid
melting
liquid to solid
Freezing
liquid to gas
vaporization
gas to liquid
Condensation
gas to solid
Deposition
solid t gas
sublimation
plasma to gas
recombination
gas to plasma
Ionization
carbon-containing compound
Organic compound
compounds that do not contain carbon
Inorganic compound
atoms that are bonded share electrons rather than transfer electrons from one to the other and formed when two non-metals bond to each other
Covalent compound
same throughout/one phase.
can be separated by physical methods (evaporation and filtration). Uniform compositio
also called solutions
Homogenous
homogenous mixture composed of two or more substances
Solution
branch of chemistry that deals with the calculation of quantities of substances involved in chemical reactionss
Stoichiometry
types and number of atoms in a compound
chemical formula
a small number written above and to the right of an element symbol, often indicating the charge of an ion
superscript
substance that undergo a chemical change
reactants
result of a chemical reaction
Products
a compound breaks down into simpler substances
Decomposition
One element replaces another in a compound
Single replacement (Displacement)
exchange of ions between two compounds, leading to the formation of two new compounds
Double replacement
loss of electrons
Oxidation
gain of electrons
Reduction
a substance that causes oxidation in another substance by accepting electrons
Oxidizing agent
causes reduction in another substance by donating electrons
Reducing agent