NOTES: INTRODUCTION TO CHEMISTRY
INTRODUCTION TO CHEMISTRY - KEY
Chemistry- THE STUDY OF MATTER AND THE CHANGES MATTER UNDERGOES
Matter- ANYTHING THAT HAS VOLUME (TAKES UP SPACE) AND MASS
States of Matter:
SOLID, LIQUID, GAS & PLASMA
Types of Matter:
Element
MADE UP OF ONLY 1 TYPE OF ATOM
ONLY 1 CAPITAL LETTER IN THE SYMBOL OF AN ELEMENT (EX: H, C, O, Cl)
Compound
MADE UP OF 2 OR MORE ELEMENTS CHEMICALLY COMBINED
2 OR MORE CAPITAL LETTERS IN THE SYMBOL OF A COMPOUND (NaCl, H20, CO2)
Mixture
2 OR MORE SUBSTANCES PHYSICALLY COMBINED
Changes in Matter
Physical Change
DOES NOT CHANGE THE IDENTITY OF THE SUBSTANCE
KEY WORDS: MELT, FREEZE, EVAPORATE, DISSOLVE, CONDENSE, RIP/TEAR, BOIL, VAPORIZE
Chemical Change
PRODUCING SOMETHING NEW (CHANGED IDENTITY)
KEY WORDS: BURN, RUST, ROT, COOK/BAKE, REACT
MATTER, PHYSICAL /CHEMICAL PROPERTIES & CHANGE
States of Matter:
| |SOLID |LIQUID |GAS |PLASMA |
|SHAPE |DEFINITE SHAPE |TAKES SHAPE OF CONTAINER (NO DEF SHAPE) |TAKES SHAPE OF CONTAINER | |
| | | | | |
| | | | | |
| | | | | |
|VOLUME |DEFINITE VOLUME |DEFINITE VOLUME |FILLS THE CONTAINER (EXPANDS & COMPRESSES) | |
| | | | | |
| | | | | |
| | | | | |
|PARTICLES |TIGHTLY PACKED |CLOSE BUT CAN MOVE (FLOW) |SPREAD APART | |
| |STRONGEST ATTRACTION |MEDIUM ATTRACTION |NO ATTRACTION | |
| | | | | |
|MOTION |VIBRATE AROUND A FIXED POINT |SLIDE PAST EACH OTHER |RANDOM, RAPID MOTION | |
| | |MORE LOOSELY PACKED | | |
| | | | | |
Physical Property: CHARACTERISTIC THAT CAN BE OBSERVED WITHOUT CHANGING THE IDENTITY OF THE SUBSTANCE (EX: COLOR, FREEZE, MELT, BOIL, MASS, TEMPERATURE, DENSITY, TEXTURE, SHAPE, VOLUME)
Chemical Property: A DESCRIPTION OF HOW A SUBSTANCE REACTS OR CHANGES INTO SOMETHING ELSE (EX: REACTS, RUST)
Examples: the pigment is blue _______PHYSICAL PROPERTY_________________________
sodium reacts violently with water___CHEMICAL PROPERTY__________________
wax melts at 82°C____ PHYSICAL PROPERTY _______________________________
iron rusts when left out in the rain_ CHEMICAL PROPERTY______________________
oil floats on water ____ PHYSICAL PROPERTY _______________________________
Physical Change: PROCESS IN WHICH NO NEW SUBSTANCE FORMS
Chemical Change: PROCESS IN WHICH A NEW SUBSTANCE FORMS
Examples:
CO2 is released when alka seltzer is added to water _____CHEMICAL CHANGE___________
Salt dissolving in water ____PHYSICAL CHANGE____________
Baking cookies ___ CHEMICAL CHANGE _____________
Burning coal ___ CHEMICAL CHANGE _____________
PHYSICAL VS. CHEMICAL
Label each property below as physical (P) or chemical (C):
__P___ 1. moth balls vaporize in the closet __P___ 6. Butter melts at 30°C
__C___ 2. Hydrofluoric acid attacks glass __P___ 7. Sugar dissolves in water
__P___ 3. Chlorine gas liquefies at -35°C __C___ 8. Paint dissolves in acetone
__C___ 4. Hydrogen gas burns in chlorine gas __C___ 9. Baking soda fizzes with acid
__P___ 5. Hydrogen gas pours “up” because it is lighter than air
Determine whether each change below is physical (P) or chemical (C).
__P___ 1. Perfume evaporating on your skin _C____ 5. Wood rotting
__C___ 2. Autumn leaves changing color __P___ 6. Melting copper metal
__C___ 3. Burning sugar __C___7. Baking a cake
__P___ 4. Fogging a mirror with your breath __P___ 8. Slicing potatoes for fries
Classify each term below as physical (P) or chemical (C).
__P___ 1. Boil __P___ 6. Melt
__C___ 2. Burn (combustion) __C___ 7. Bake
__P___ 3. Evaporate __C___ 8. Tarnish
__P___ 4. Dissolve __C___ 9. React
__C___ 5. Rust __P___10. Freeze
Physical/Chemical Properties/Changes
CHEMISTRY: A Study of Matter
© 2004, GPB
2.4
I. Fill in the Blanks
__PHYSICAL__ properties can be observed without chemically changing matter.
___CHEMICAL_____ properties describe how a substance interacts with other
substances. __SOLIDS___ have definite shapes and definite volumes.
__LIQUIDS_____ have indefinite shapes and definiTe volumes. ___GASES______ have
indefinite shapes and indefinite volumes.
Phase changes are __PHYSICAL_______ changes. __FREEZING____ point is the
temperature at which a liquid turns to a solid. It is also equal to the
__MELTING____ point which is the temperature at which a __SOLID_____ turns
to a ___LIQUID____. ____BOILING__________ point is the temperature at which a liquid
turns to a gas, and __CONDENSATION_________ point is the temperature at which a gas turns
to a liquid. Occasionally, a solid turns directly into a gas without turning into a
liquid first. This is called _sublimation____.
II. Label these properties as chemical (C) or physical (P). Be certain to know the
definition of each of these properties.
_C____ combustibility _P____density __P___malleability
_C____tendency to corrode __C___failure to react __P___ melting point
_P____ ductility __P___ odor __P___ texture
_C____ flammability
III. Label these changes as chemical (C) or physical (P).
__C___ digestion of food __C___ explosions __P___ getting a haircut
__C___ lighting a candle __P___evaporation __C___ tarnishing silver
__P___ ice cube melting __C___ formation of acid rain
__P___ crushing rocks __P___ dissolving salt in water
CLASSIFICATION OF MATTER
TYPES OF MATTER:
pure substance – JUST ONE TYPE OF MATTER (ELEMENTS & COMPOUNDS)
mixture - 2 OR MORE TYPES OF MATTER THAT RETAIN THEIR PROPERTIES
|ELEMENT |COMPOUND |MIXTURE |
| | | |
|ONLY ONE SET OF PROPERTIES |2 OR MORE ELEMENTS JOINED BY A CHEMICAL BOND |2 OR MORE ELEMENTS OR COMPOUNDS PHYSICALLY |
| | |COMBINED |
|SIMPLEST TYPE OF MATTER |SEPARATED BY A CHEMICAL REACTION | |
| | |SEPARATED BASED ON PHYSICAL PROPERTIES |
|ONE TYPE OF ATOM ONLY (SMALLEST PARTICLE) |ONE SET OF PROPERTIES ONLY | |
| | |COMBINE IN ANY PROPORTION |
|CANT BE BROKEN DOWN IN A NORMAL CHEMICAL REACTION|ELEMENTS COMBINE IN A SPECIFIC PROPORTION | |
| | |HOMOGENEOUS – LOOKS PURE |
| | | |
| | |HETEROGENEOUS – CAN SEE DIFFERENT PARTS |
| | | |
| | |ALLOY – MELTED METALS TOGETHER (EX: BRONZE, |
| | |BRASS, STEEL) |
| | | |
| | | |
SEPARATION OF COMPOUNDS AND MIXTURES
1. sand, salt and water
FILTER OUT SAND, BOIL OUT WATER
2. water and rubbing alcohol
HEAT ( ALCOHOL BOILS OFF FIRST (DISTILLATION)
3. hydrogen and oxygen in water
4. salt and pepper (demonstration)
PHYSICAL MEANS (PEPPER IS LIGHT SO ATTRACTS TO STATIC)
5. C from H and O in sugar (demonstration)
CHEMICAL MEANS (REACTION BETWEEN SUGAR AND ACID)
SEPARATION OF MIXTURES VOCABULARY
1. filtration
- LIQUID/SOLID
- DOESN’T SEPARATE DISSOLVED SOLUTIONS
- EX: H20 & SAND
- CAN COLLECT THE LIQUID AND SOLID
2. crystallization
- LIQUID EVAPORATES
- SOLID REMAINS BEHIND
- CAN COLLECT JUST SOLID
3. chromatography
- SEPARATING COLORS (PIGMENTS) BASED ON SIZE
- SMALL PIGMENTS TRAVEL FARTHER/HIGHER
ON THE PAPER
4. distillation
- CAN SEPARATE DISSOLVED SOLID IN LIQUID
- CAN SEPARATE LIQUID/LIQUID (USING BOILING POINTS)
- CAN COLLECT LIQUID & SOLID / LIQUID & LIQUID
COMPARE & CONTRAST: sodium (Na), sodium chloride (NaCl) and salt water (NaCl & water)
ANSWERS TO WORKSHEET ON PAGE 8:
1A: SOLID/LIQUID, MIXTURE
1B: GAS, ELEMENT
1C: GAS, MIXTURE
1D: SOLID, COMPOUND
2A: SOLID, COMPOUND
2B: GAS, COMPOUND
2C: LIQUID, MIXTURE
2D: SOLID, ELEMENT
3A: GAS, COMPOUND
3B: SOLID, COMPOUND
3C: GAS, MIXTURE
3D: GAS, ELEMENT
4A: GAS, COMPOUND
4B: LIQUID/GAS, ELEMENT
4C: SOLID, COMPOUND
4D: GAS, MIXTURE
CLASSIFICATION OF MATTER
Determine whether each example or property below is a pure substance. Then label each as an “element” (E), “compound” (C), homogeneous mixture (HO) or Heterogeneous Mixture (HE). Use your own examples to complete the chart.
|Substance? |Example |E, C, HO or HE? |
|NO |1. sand |HE |
|YES |2. salt |C |
|YES |3. pure water |C |
|NO |4. tap water |HO |
|YES |5. aluminum |E |
|NO |6. gasoline |HO |
|NO |7. soda |HO / HE |
|NO |8. an egg |HE |
|YES |9. sugar |C |
|YES |10. copper |E |
|NO |11. steel |HO |
|YES |12. nitrogen |E |
|YES |13. air |HO |
|NO |14. particles combine in any proportion |HO / HE |
|NO |15. appears like one substance, but shows two different boiling points |HO |
|NO |16. only separable by a chemical reaction |C |
|NO |17. MILK |homogeneous mixture |
|YES |18. OXYGEN |element |
|YES |19. CARBON DIOXIDE |compound |
|NO |20. SALAD |Heterogeneous mixture |
MATTER & ENERGY
Energy: ABILITY TO DO WORK
potential energy: STORED ENERGY OR ENERGY OF POSITION (HAS CAPABILITY TO GIVE USABLE ENERGY BUT IS NOT RIGHT NOW)
examples: CHEMICAL BONDS, BATTERY, NUCLEAR ENERGY
kinetic energy: ENERGY OF MOTION
examples: ELECTRICITY, HEAT ENERGY, RIDING A BIKE
Units of Energy: JOULE OR CALORIE
Temperature: AVERAGE KINETIC ENERGY OF PARTICLES IN A SAMPLE
Units:
Celsius: °C BASED ON WATER (FREEZES AT 0, BOILS AT 100)
Kelvin: K BASED ON ABSOLUTE ZERO
Absolute zero: 0 K (ALL MOTION STOPS)
Law of Conservation of Energy:
ENERGY CANNOT BE CREATED OR DESTROYED BUT CAN BE CHANGED FROM ONE TYPE TO ANOTHER
EX) SOLAR ENERGY ( ELECTRIC ENERGY (SOLAR PANELS
HEAT/THERMAL ENERGY ( MECHANICAL ENERGY
[pic]
Law of Conservation of Matter/MASS: MATTER CANNOT BE CREATED OR DESTROYED
Example: Mg + Oxygen ( Ash
_____ + _____( ________
a. If 10.0g of magnesium metal burns in air, and reacts with 6.6g of oxygen, what mass of ash will form?
10g + 6.6g ( 16.6g
b. If 25g of magnesium metal burn in air, 41.5g of ash are formed. What mass of oxygen reacted with the magnesium?
25g + _____ ( 41.5 g 41.5g – 25g = 16.5g
Try: Sodium (Na) reacts with potassium chloride (KCl) to produce potassium (K) and sodium chloride (NaCl).
Na + KCl ( NaCl + K
_____ ______ ( ______ _______
If 20g of sodium (Na) reacts with 30.g of potassium chloride (KCl) and 15g of potassium (K) are produced, find the mass of sodium chloride (NaCl) also produced.
20g + 30g ( ____ + 15g
50g ( ____ + 15g
50g – 15g = 35g
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