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Karen Bright Saragih - Term 2 Science Mind Map - Coggle Diagram
Karen Bright Saragih
- Term 2 Science Mind Map
Acid, Base, and Salt
Examples
Acids
Acetic acid
Citric acid
Ascorbix acid
Sulfuric acid
Base
Ammonia
Sodium hydroxide
Potassium hydroxide
Sodium bicarbonate
Magnesium hydroxide
Salt
Sodium chromate
Sodium chloride
Nickle chloride
Copper sulfate
Magnesium sulfate
Neutralization
When acids and bases interact with each other, their opposing ionic compounds will react with each other in the form of NEUTRALIZATION by doing DOUBLE DISPLACEMENT
Properties
Base
Produce hydroxide ions when dissolved in water
Soapy/slippery
Bitter and chalky taste
Conducts electricity
Corrosive
Acid
A solution of hydrogen (H) ions
Sour
Conduct electricity
Corrosive
Some acids react strongly with metals
Produces hydrogen ions when dissolves in water
Salt
Transparent and colorless in crystalline form
Ionic compunds
Salty taste
Water-soluble although some are water-insoluble
Conduct electricity
Double Displayment
Double replacement reactions have two ionic compounds that are exchanging anions or cations.
pH Scale
An accurate way to express how ACIDIC or ALKALINE (base) a solution is. Ranges from 1 (Highly Acidic) to 14 (Highly Alkaline)
Atoms, Molecules, Ions, and such
History
Erwin Schrodinger
- He wasn't content with Niels Bohr's atomic model and soon discovered THE QUANTUM MECHANICAL MODEL OF THE ATOM by treating the atoms like waves and had made an equation to predict possible locations of electrons.
Niels Bohr
- Improved Ernest Rutherford's nuclear atomic model because he had discovered that atoms can have multiple "shells" instead of orbits. He named the atomic model THE PLANETARY ATOMIC MODEL
Ernest Rutherford
- Discovered the nucleus after conducting the gold foil experiment and using alpha particles to discover that alpha particles consist of mostly empty space. He made the NUCLEAR ATOMIC MODEL
JJ Thompson
- Discovered electrons and have made the PLUM PUDDING MODEL, where the electrons are inside and is surrounded by a "positively charged space" through the cathode ray experiment
John Dalton
- First concluded that atoms are just dense balls that make up matter and that atoms from 2 different elements are different while 2 atoms from the same element are identical and perfect to one another
Definitions
Atoms
Atoms are a single (or one piece)
Atomic Number - The number of protons in an atom
Atomic Mass - The number of protons and neutrons in the nucleus
Ions
Ions are the charge of atoms. It can be positive (Cations) and negative (Anions). It becomes negative if it GAINS an electron(s) and can be positive if it LOOSES an electron (s)
Molecules are a group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction (can be from different elements and from the same elements)
Radioactivity
(γ) Gamma rays - No charge and mass. Just like light!
(β) Beta particles - Attracted to positive electrodes because of their negative charge
(a) Alpha particles - Attracted to negative electrodes because of their positive charge
The Laws
Law of Constant Composition
The elemental composition of a pure substance never varies and the relative amounts of each element in a compound doesn't vary
Law of Conservation of Mass
The total mass of substances AFTER a chemical is equal to the mass of substances BEFORE a chemical process if there aren't any matters added or subtracted
Isotopes
Common isotopes is when a chemical has a different number of atomic mass but the same number of atomic number (which means it had gained a number of neutrons which don't affect the overall charge and atomic number of the element)
Subatomic Particles
Neutrons
The neutral charge (0) in an atom. Is found in the nucleus (the center of the atom that is where the mass if mostly from)
Has mass of 1 AMU (Atomic Mass Unit)
Electrons
The negative charge (-1) in an atom. Is found around the nucleus
It's mass is negligible because of how light it is.
Protons
The positive charge (+1) in an atom. Is found in the nucleus (the center of the atom that is where the mass is mostly from)
Has a mass of 1 AMU (Atomic Mass Unit)
Classifying/Identifying parts of shorthand notations
Orange : Atomic Mass
Red: Atomic Number
Green : Charge
