Matter and Energy Name ______
Applied Chemistry
Date: ______Period: ______
I. The UNIVERSE is made of ______and ______.
II. Energy
A. Definition: Energy is the capacity to do ______or to produce ______.
1. Common Unit: ______abbreviated ______.
2. SI Unit: ______abbreviated ______.
B. Forms
1. Radiant Energy is energy transferred ______.
Example: ______
2. Kinetic Energy is the energy of ______.
Examples: ______
______
______
3. Potential Energy is energy of ______or ______.
Examples: ______
______
C. Law of Conservation of Energy
1. Energy is neither ______nor ______.
2. Energy can change from one ______to another.
III. Matter
A. Definition: Matter is anything that has ______and ______.
B. States of Matter
1. Identification Table
NAME
/ABBREV
/SHAPE
/VOLUME
/DENSITY
2. Change in state is also known as a ______.
(See next page for changes between states.)
C. Properties or Characteristics of Matter
1. A physical property is a property ______or ______without changing the material.
Examples: ______
______
2. A chemical property is a property that refers to the ability of a material to undergo a ______that alters its structure.
Examples: ______
______
D. Changes
1. All changes involve a change in ______.
2. Physical Changes: Do NOT change the ______of a substance.
Examples: ______
______
3. Chemical Changes: ______the identity of a substance.
Examples: ______
______
4. Signs of a Chemical Change:
______, ______,
______, ______,
or ______.
a. Chemical Equation – a shorthand way to write a ______.
· Starting materials are called ______.
· Newly formed materials are called ______.
Reactants ® Products
Yield
Iron + Oxygen ® Rust (Iron(II) oxide)
E. Law of Conservation of Matter
1. Matter is neither ______nor ______. It only changes ______.
2. Shown by the French chemist Antoine Lavoisier in the 1700s. He is known as the Father of ______.
mass of the ______= mass of the ______
F. Classification of Matter
1. Pure substances
a. Elements
· Contain only ______.
· ______be broken down by ordinary methods. (chemical/physical)
· Ancient Greeks believed in only ______elements (______, ______, ______, ______)
· _____ naturally occurring elements. Others are short-lived, man-made elements.
· A ______is a shorthand way of writing the name of an element.
· Represents 1 ______of an element.
1. Consists of 1 or 2 letters
2. 1st letter is ALWAYS capitalized.
3. Subsequent letter is lower case.
4. 3-letter symbols are temporary designations assigned by IUPAC.
Ex. Hydrogen ______Carbon ______
Helium ______Chlorine ______
# of elements as a Solid, Liquid, or Gas at room temperature
______Liquids ______Gases All others are solids.
b. Compounds
· Contain ______that are chemically combined.
· Can be broken down by chemical processes, such as ______.
· Smallest particle of a compound is a .
· A ______is a shorthand way of writing the name of a compound. It shows:
1. Which elements are present
2. The ratio of the elements present.
Example: H2O - the 2 is called a ______that tells you that ______of hydrogen combine with ______of oxygen to form ______of water.
Example: 3 H2O is read as 3 ______of water. The 3 is called a ______. There are ______hydrogen atoms and ______oxygen atoms.
Element or Compound?
Co ______CO ______
CS ______Mg ______
How many atoms are in Na2SO4? ______
How many atoms are in Ca(OH)2? ______
How many atoms are in 3Fe2(SO3)3? ______
2. Mixtures contain ______that are mixed together but ______chemically joined.
A. Homogeneous Mixture or Solution
· ______throughout
· Not visibly different
· Examples:
______
______
B. Heterogeneous Mixture or Mechanical Mixture
· Not ______throughout
· Visibly different (layers)
· Examples:
______
______
IV. Separation Techniques
A. Heterogeneous Mixtures
1. Filtration
· Separate ______from a clear liquid by pouring through a
______, ______, or ______.
· filtrate:
· residue:
· Examples: ______
2. Magnetic Method
· Separate ______substances from ______substances.
· Examples: ______
3. Decanting
· Separate ______due to a difference in ______.
· Example: ______
B. Homogenous Mixtures:
1. Chromatography
· Separate ______of ink using strips of paper.
· Examples: ______
2. Distillation
· Separate solution by a difference in ______. The liquids will evaporate and then ______back to a liquid.
· Example: ______
3. Crystallization
· Separate a solution by ______the liquid and the solid will ______.
· Examples: ______
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