Download 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
FOUND ON THE PERIODIC TABLE
Compound
MADE UP OF 2 OR MORE ELEMENTS CHEMICALLY BONDED
Mixture
NOT CHEMICALLY COMBINED
Changes in Matter
Physical Change
NOTHING NEW IS MADE
Chemical Change
MAKING SOMETHING NEW
MATTER, PHYSICAL /CHEMICAL PROPERTIES & CHANGE
States of Matter:
SOLID
PARTICLES CLOSE AND
ORGANIZED
LIQUID
CLOSE AND
UNORGANIZED
GAS
FAR APART
PLASMA
+ IONS &
ELECTRONS – FAR
APART
DENSITY
HIGH
HIGH
LOW
LOW
VOLUME
DEFINITE
DEFINITE
HAS VOLUME OF
ITS CONTAINER
HAS VOLUME OF
ITS CONTAINER
SHAPE
DEFINITE
SHAPE
TAKES SHAPE OF
CONTAINER
TAKES SHAPE OF
CONTAINER
TAKES SHAPE OF
CONTAINER
Physical Property: SOMETHING YOU CAN OBSERVABLE AND MEASURABLE WITHOUT
CHANGING THE SUBSTANCE (EX: COLOR, FREEZE, MELT, BOIL, MASS, TEMPERATURE,
DENSITY, TEXTURE, SHAPE)
Chemical Property: YOU MUST CHANGE THE SUBSTANCE IN ORDER TO OBSERVE THE (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:
NOTHING NEW IS MADE
EXAMPLE: RIP PAPER, MELT, FREEZE, BOIL, CONDENSE
Chemical Change:
SOMETHING NEW IS MADE
EXAMPLE: “REACTS WITH”, RUST, BURN, TARNISH
EVIDENCE: BUBBLES/FOAM, COLOR CHANGE, ODOR, TEMP. CHANGE, LIGHT,
SMOKE
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 _____________
Compare & Contrast: ice and water
SIMILARITY: H20
DIFFERENCES: SOLID VS. LIQUID
DEFINITE SHAPE VS. SHAPE OF CONTAINER
LOWER DENSITY VS. HIGHER DENSITY
ORGANIZED PARTICLES VS. UNORGANIZED PARTICLES
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/ PLASMA______ have indefinite shapes and indefinite volumes.
__SOLIDS_______ and __LIQUIDS____ cannot be easily compressed. (squeezing particles
together)
__MELTING____ have a low density.
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
__C___ 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 – MADE UP OF 1 KIND OF PARTICLE (ELEMENTS & COMPOUNDS)
mixture – MADE UP OF MORE THAN 1 KIND OF PARTICLE
ELEMENT
EX) COPPER, ZINC,
HYDROGEN, OXYGEN
COMPOUND
EX) GLUCOSE, WATER,
CARBON DIOXIDE, SALT
MIXTURE
EX) SALT WATER, DIRT,
CEMENT, AIR
SMALLEST PARTICLE =
ATOM
SMALLEST PARTICLE =
MOLECULE
PARTICLES ARE NOT
CHEMICALLY COMBINED
IN THE MOLECULE,
ATOMS ARE
CHEMICALLY COMBINED
SEPARATE PARTICLES
WITH A PHYSICAL
CHANGE (CLUE FOR A
MIXTURE)
SEPARATE ATOMS IN A
MOLECULE W/ A
CHEMICAL CHANGE
COMBINE IN ANY
PROPORTION
ALLOY – MELT METALS
TOGETHER (EX: BRONZE,
BRASS, 14 CARAT GOLD)
HETEROGENEOUS MIXTURE – CAN SEE DIFFERENT PARTS (EX: SALT AND PEPPER,
BLOOD, MILK)
HOMOGENEOUS MIXTURE – CANNOT SEE DIFFERENT PARTS (EX: SALT WATER)
ATOMS ARE ALWAYS IN A
SPECIFIC PROPORTION
SEPARATION OF COMPOUNDS AND MIXTURES
1. sand, salt and water
PHYSICAL CHANGE (EVAPORATE AND FILTER/SIFT)
2. water and rubbing alcohol
PHYSICAL CHANGE (DISTILLATION)
3. hydrogen and oxygen in water
CHEMICAL CHANGE
4. salt and pepper (demonstration)
PHYSICAL CHANGE
5. C from H and O in sugar (demonstration)
CHEMICAL CHANGE
SEPARATION OF MIXTURES (PHYSICAL CHANGES) VOCABULARY
1. filtration
- ONLY WORKS ON HETEROGENEOUS MIXTURES
- SOLID GETS TRAPPED IN SOLID
2. crystallization
- SOLID DISSOLVED IN WATER
- EVAPORATE WATER
- CAN BE USED FOR HOMOGENEOUS MIXTURE
3. Chromatography
- CHROMO = COLOR
- SEPARATE COLORS
- COLORS HAVE DIFFERENT DENSITIES
- CAN BE USED ON HOMOGENEOUS MIXTURES
4. distillation
- CAN SEPARATE LIQUIDS WITH DIFFERENT BOILING POINTS
COMPARE & CONTRAST: sodium (Na), sodium chloride (NaCl) and salt water (NaCl & water)
SIMILARITY: Na (SODIUM) IN ALL 3
DIFFERENCES: Na IS AN ELEMENT, NaCl IS A COMPOUNT, NaCl AND WATER IS A
HOMOGENEOUS MIXTURE
MATTER & ENERGY
Energy: ABILITY TO DO WORK OR PRODUCE HEAT
potential energy: STORED ENERGY
examples: FAT, FOOD, GAS, BATTERY(FOOD AND GAS – CHEMICAL – NEED TO
BREAK BONDS TO GET THE ENERGY OUT)
kinetic energy: ENERGY THAT’S BEING USED IN THE FORM OF MOTION/MOVEMENT
examples: BITING AN APPLE, CAR MOVING, TEMPERATURE
Units of Energy: JOULE (SI UNIT), CALORIE (ENGLISH SYSTEM)
Temperature: MEASURE OF KINETIC ENERGY (MEASURES HOW FAST PARTICLES VIBRATE)
Units:
Celsius:
Kelvin:
Absolute zero:
Law of Conservation of Energy:
Law of Conservation of Matter:
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?
b. If 25g of magnesium metal burn in air, 41.5g of ash are formed. What mass of oxygen reacted with the
magnesium?
Try: Sodium (Na) reacts with potassium chloride (KCl)
chloride (NaCl).
Na
_____
+
KCl

NaCl +
K
______

______
_______
to produce potassium (K) and sodium
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.
KELVIN AND CELCIUS TEMPERATURE SCALES
Celsius temperature scale: 0°C = WATER FREEZES
100°C = WATER BOILS
**BASED AROUND WATER
Kelvin temperature scale: 0 K (NO NEGATIVE #S)
Absolute zero: WHERE EVERYTHING STOPS MOVING/VIBRATING
COLDEST TEMPERATURE = 0 K
K = ºC + 273
Make the following temperature conversions:
a. 25ºC to Kelvin
CK
25 + 273 = 298 K
ºC = K – 273
d. 355K to Celsius
KC
355 – 273 = 82 °C
b. 149 ºC to Kelvin
e. 408K to Celsius
c. -55 ºC to Kelvin
f. 135K to Celsius
Temperature facts:
1. The highest recorded temperature in the world was recorded in El Azizia, Libya, in September, 1922. The
recorded temperature was 136ºF, or 58ºC. Report this temperature in Kelvin.
2. The lowest recorded temperature in the world was recorded in Vostock, Antartica in July, 1983. The
recorded temperature was -129ºF, or -89ºC. Report this temperature in Kelvin.
ON YOUR OWN
Make the following temperature conversions:
a.
55ºC = _________ K
e. 125ºC = __________K
b. _______ K = 33ºC
f. ________K = -40ºC
c. _______ K = -95ºC
g.
380K = __________ºC
d. _______ ºC = 423 K
h.
120K = _________ºC