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Here are some useful chemistry terminologies
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Chemistry Terminologies
Chemistry
MatterProperty
Composition
Structure
Changes = Laws
Mass vs. Weight
• Unit of mass
• Amount of material in an object
• Constant
• Unit of force
• Force of gravity pulling on the object
• Depends on the location
Mass Weight
Temperaturehotness or coldness of
an object
Celsius vs. Fahrenheit vs. Kelvin
0C = (0F – 32)/ 1.8
0F = (1.8 X 0C) + 32
K = 0C + 273
0C 0F K
Normal body temperature
37 0C 98.6 0F ?
Boiling point 100 0C ? 373 K
Freezing point
? 32 0F 273 K
0C 0F K
Normal body temperature
37 0C 98.6 0F 310 K
Boiling point 100 0C 212 0F 373 K
Freezing point
0 0C 32 0F 273 K
Evaporation vs. Condensation
Evaporation vs. Condensation
Evaporation–Liquid to Gas
Condensation–Gas to Liquid
Sublimation vs. Condensation
Sublimation vs. Condensation
Sublimation–Solid to Gas
Condensation–Gas to Solid
Matter
Matter
Substance Mixture
Element
Compound
Homogenous
Heterogeneous
Solution
Suspension
Colloid
Matter
Space Mass
Pure Substance
Compose of the same kind of particles Has same color and taste Has definite properties and uniform
characteristics Has single phase
– Salt– Sugar– Pure water
Element
made up of only one kind of atoms having the same atomic number
cannot be further reduced to simpler substances by ordinary physical or chemical processes– Hydrogen– Oxygen
Compound
Formed by the combination two or more elements
Could not be separated into its constituents by mechanical or physical means
Properties of a compound differ entirely from those of its constituent elements
Mixture
Combination of two or more substances Each substance retains its own
properties– Air– Gasoline– Halo Halo– Fruit Salad
• Uniform characteristic
• Single phase
•Air
•Gasoline
• No uniform characteristic
• Two or more phase
•Fruit Salad
•Halo Halo
Homogenous Heterogeneous
Solution
Homogeneous mixture of two or more chemical substances
May be solid, liquid or gas– salt water (liquid solution)– air (gaseous solution)– alloy (solid solution)
Solute + Solvent = Solution
Suspension
Consists of particles of a solid suspended in a liquid medium
Has two distinct phases Particles of a suspension may not be visible
to the naked eye– Sand and water– Oil and water
Colloid
Represents an intermediate kind between true solution and suspension
Two-phase heterogeneous system – dispersed phase– dispersion medium
Dispersed phase = solute in a solution
Dispersed phase
Dispersed medium
Colloidal system
Examples
Solid Solid Solid solsColored glues, gem
stones, pearls,
Solid Liquid Sols Paints, starch,
Liquid Solid Gels cheese butter
Liquid Liquid Emulsion Milk, hair cream,
Solid Gas Aerosols of
solids Smoke, dust in air,
smog
Liquid Gas Aerosols of
Liquids Insecticide sprays
Gas Solid Solid foam Foam, Ice-cream,
Rubber
Gas Liquid Foam, Froth Soda water, whipped
cream froth
Matter
Substance Mixture
Element
Compound
Homogenous
Heterogeneous
Solution
Suspension
Colloid
Acid vs. Base
• Latin “acidus”
• Sour
• Proton donor
• Blue to red
• Bitter
• Slippery
• Proton acceptor
• Red to blue
Acid Base
• Fruits
• Citric Acid
• Vinegar
• Acetic Acid
• Soft drinks
• Carbonic Acid
• Milk
•Lactic Acid
• Vomit
•Hydrochloric Acid
• Lye
• Baking soda
• Milk of magnesia
• Antacid
Acid Base
Indicator
Exhibits specific color in the presence of acid or base
pH – measure of acidity or basicity
pH paper
pH meter
pH Reading
Values 1-14Less than 7 = acidicHigher than 7 = basicEqual to 7 = neutral
pH = 5
Acidic
pH = 4
Acidic
pH = 7
Neutral
pH = 6
Acidic
pH = 8
Basic
Strong or Weak
Acid + Base = Neutralization
Atom
Atom
Smallest particle of an atomJohn Dalton : indivisible
Parts of an Atom
Proton Electron Neutron
Charge + - No charge
Location • In the nucleus
• Surrounds proton and neutron
• Near protons•Holds the protons together
Nucleus = center = proton and neutron
Atomic Number vs. Atomic Mass
Atomic Number Atomic weight
• Equal to the number of protons
• Equal to mass number
• Equal to the no. of neutron + no. of proton
S
Ga Ba
Isotope vs. Isotone vs. Isobar
Isotope
Same elementDifferent atomic mass
C CMg Mg
Isotone
Same number of neutrons
Neutrons = A. Mass – A. No.
C NCa K
Isobar
Same atomic massDifferent elements
Ne NaAr K
Isotope vs. Isotone vs. Isobar
C N
Pb Pb
Na Mg
Alpha vs. Beta vs. Gamma
Radioactivity
process whereby unstable atomic nuclei release energetic subatomic particles
subatomic particles released during the process
Charge Penetrating
Power
Ionizing
Power
Alpha + Least Maximum
Beta - Less Less
Gamma No charge Maximum Least
Penetrating Power
If you have three radioactive cookies alpha beta and gamma, what will you
Eat?
Place in your pocket?
Hold by your hand?
If you have three radioactive cookies alpha beta and gamma, what will you
Eat? Gamma
Place in your pocket? Beta
Hold by your hand? Alpha
End