CHAPTER 9
ELEMENTS, COMPOUNDS, AND MIXTURES
OBJECTIVES
• SPI 0807.9.1 Recognize that all matter is made up of
atoms
• SPI 0807.9.3 Classify common substances as elements or
compounds based on their symbols or formulas.
I can:
1. Define all new vocabulary terms: element, pure
substance, metal, nonmetal, metalloid.
2. Describe the characteristics of elements, and give
examples.
3. Classify elements as metals, nonmetals, or metalloids.
4. Distinguish between metals, nonmetals, and metalloids.
ELEMENTS
I can describe the characteristics of elements, and give examples.
• A substance that cannot be separated or broken
down into simpler substances.
• Pure substance – only has one type of particle
(atoms).
• Every atom in a piece of gold is the same, no matter where
it is found.
• Every atom of iron is the same
• spoon, steel rod, meteorite
• Elements are found on the periodic table
• 111 elements known
I can describe the characteristics of elements, and give examples.
PROPERTIES OF ELEMENTS
I can describe the characteristics of elements, and give examples.
• Characteristic properties – do not depend on the
amt. of the element present.
• Boiling point, melting pt., density, reactivity with acid, color,
hardness, flammability
• Can be used to identify elements
• Identified by their physical and chemical properties
• Categorized by similar properties
• Metals, nonmetals, or metalloids
CLASSIFYING ELEMENTS
I can classify elements as metals, nonmetals, or metalloids.
1. Metals
• Shiny, conduct heat and electricity, malleable, ductile
• All are solid except mercury
• Examples: copper (Cu), tin (Sn), lead (Pb), iron (Fe), gold
(Au), mercury (Hg)
CLASSIFYING ELEMENTS
I can classify elements as metals, nonmetals, or metalloids.
2. Nonmetals
• Opposite of metals
• dull, poor conductors heat and electricity, brittle, not
malleable, not ductile
• Can be solid, liquid, or gas
• Examples: sulfur (S), iodine (I), neon (Ne), chlorine (Cl),
oxygen (O), hydrogen (H)
CLASSIFYING ELEMENTS
I can classify elements as metals, nonmetals, or metalloids.
3. Metalloids
• Properties of both metals and nonmetals
• Semi-conductors
• Some shiny, some dull, somewhat malleable and ductile,
some conduct heat and electricity
• Solids
• Examples: boron (B), silicon (Si), germanium (Ge), arsenic
(As), antimony (Sb), tellurium (Te)
I can distinguish between metals, nonmetals, and metalloids.
OBJECTIVES
• SPI 0807.9.1 Recognize that all matter is made up of
atoms
• SPI 0807.9.3 Classify common substances as elements or
compounds based on their symbols or formulas.
• SPI 0807.9.4 Differentiate between a mixture and a
compound.
• SPI 0807.9.6 Compare the particle arrangement and
type of particle motion associated with different states
of matter.
I can:
1. Identify examples of common compounds by their
chemical formula.
2. Explain how elements make up compounds.
3. Explain how compounds can be broken down.
4. Compare elements and compounds.
COMPOUNDS
I can identify examples of common compounds by their chemical formulas.
• Pure substance composed of two or more elements that are
chemically combined.
• Elements are rarely found alone in nature, so they combine with other
elements.
• Compounds form a particle called a molecule (two or more
atoms joined together).
• Found in a set ratio of elements
• Examples of common compounds:
•
•
•
•
•
•
•
Table Salt
Sugar
Water
Hydrogen Peroxide
Vinegar
Carbon Dioxide
Baking Soda
COMMON COMPOUNDS
I can identify examples of common compounds by their chemical formulas.
Compound
Elements Combined
Chemical
Formula
Table salt
Sodium(Na) and chlorine(Cl)
NaCl
Water
Hydrogen(H) and oxygen(O)
H2O
Hydrogen Peroxide
Hydrogen(H) and oxygen(O)
H2O2
Sugar
Hydrogen(H), carbon(C),
oxygen(O)
C12H22O11
Vinegar
Hydrogen(H), carbon(C), and
oxygen(O)
C2H4O2
Carbon dioxide
Carbon(C) and oxygen(O)
CO2
Baking Soda
Sodium(Na), hydrogen(H),
carbon(C), and oxygen(O)
NaHCO3
sugar
PROPERTIES OF COMPOUNDS
I can explain how elements make up compounds.
• Identified by physical and chemical properties
• Compounds have different properties than the
elements that form them.
• Forming Sodium chloride (NaCl)
Sodium is a soft,
silver white metal
that reacts
violently in water
Chlorine is a
poisonous,
greenish yellow
gas
Sodium Chloride is
a white solid. It
dissolves easily in
water and is safe to
eat.
SODIUM REACTING WITH WATER
BREAKING DOWN COMPOUNDS
I can explain how compounds can be broken down.
• Broken down by chemical changes
• Energy is needed to break down compounds
• Add heat or add electric current
1. Broken down into elements
• Water (H2O) → hydrogen(H) and oxygen(O).
• Table Salt (NaCl) → sodium (Na) and chlorine (Cl)
• Carbon Dioxide (CO2) → carbon (C) and oxygen(O)
2. Broken down in simpler compounds and then into
its elements
• Carbonic acid (H2CO3)→carbon dioxide (CO2) + water
(H2O)→carbon (C) + oxygen (O) + hydrogen (H)
OBJECTIVES
• SPI 0807.9.1 Recognize that all matter is made up of
atoms
• SPI 0807.9.4 Differentiate between a mixture and a
compound.
I can:
1. Define all new vocabulary terms: solution, solute,
solvent, concentration, solubility, suspension, colloid.
2. Describe three properties of mixtures.
3. Distinguish between a mixture and a compound.
4. Analyze a solution in terms of its solute and solvent.
5. Distinguish between a solution, a suspension, and a
colloid.
MIXTURES
I can describe three properties of mixtures.
• A combination of two or more substances that are
not chemically combined
• When mixed, the substances do not react
• No chemical change happens
• Each substance in the mixture keeps its identity
• Do not have a set ratio of components
• Separated through physical methods
1.
2.
3.
4.
Distillation – separates based on boiling points
Magnet - separates iron from other elements
Centrifuge – separates by densities
Filtration – separates by particle size
MIXTURES VS. COMPOUNDS
I can distinguish between a mixture and a compound.
Mixtures
Compounds
Made of elements, compounds, or
both
Made of elements
No change in original properties of
components
Change in original properties of
components
Separated by physical means
Separated by chemical means
Formed using any ratio of
components
Formed using a set ratio of
components
SOLUTIONS
I can distinguish between a solution, a suspension, and a colloid.
• A mixture that appears to be a single substance
• One substance is dissolved in another substance
•
•
•
•
•
Solute – substance that is dissolved
Solvent – substance in which the solute is dissolved
Soluble – able to dissolve
Insoluble – unable to dissolve
Examples of solutions:
•
•
•
•
•
•
•
Salt water
Sugar water
Gasoline
Soft drinks
Air
Brass
steel
SOLUTIONS
I can distinguish between a solution, a suspension, and a colloid.
States
Examples
Components
Gas in gas
Dry air
Oxygen in nitrogen
Gas in liquid
Soft drinks
Carbon dioxide in
water
Liquid in liquid
Antifreeze
Alcohol in water
Solid in liquid
Salt water
NaCl in water
Solid in solid
Brass
Zinc in copper
CONCENTRATION OF SOLUTIONS
I can analyze a solution in terms of its solute and solvent.
• Concentration – measure of the amount of solute
dissolved in a solvent
• Expressed in g/mL
• Concentration =
𝑔𝑟𝑎𝑚𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
𝑚𝐿 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡
• Concentrated solutions contain more solute per solvent
• Dissolving solids in liquids faster
1. Mixing or stirring
2. Heating
3. Crushing
SUSPENSIONS
I can distinguish between a solution, a suspension, and a colloid.
• Mixture in which particles of a material are
dispersed throughout a liquid or gas but large
enough to settle out
• Can be separated by filtration
• Examples:
•
•
•
•
•
Snow globe
Italian dressing
Paints
Medicines
Orange juice
COLLOIDS
I can distinguish between a solution, a suspension, and a colloid.
• Mixture in which the particles are dispersed
throughout but are not heavy enough to settle out
• Have properties of both solutions and suspensions
• Cannot be separated by filtration
• Examples:
•
•
•
•
•
•
Milk
Mayonnaise
Deodorant
Gelatin
Whipped cream
butter