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IV. LESSON 4
Unit 1 – Lessons 1-6 “Describing Matter” (Pages 4-87)
A. Pure Substances and Mixtures
1. ALL matter is composed of particles called ATOMS
2. Atoms form ELEMENTS and come together in different ways to form COMPOUNDS and
MIXTURES
3. ATOM  SMALLEST unit of an ELEMENT and maintain the PROPERTIES of that element
4. MOLECULE  SMALLEST unit of a COMPOUND; maintaining PROPERTIES of the compound
5. ELEMENT  matter that is composed of one kind of ATOM (e.g. sulfur [S]; carbon [C])
a. each ELEMENT has its own CHARACTERISTIC, chemical, and PHYSICAL properties
*b. elements can NOT be BROKEN down into other substances by any CHEMICAL means
c. some MATTER exists in elemental form [(e.g.) gold [Au] = not chemically REACTIVE)]
*d. ELEMENTS individually or combined form everything in the universe including HUMANS
*1. Human body’s most abundant ELEMENTS: carbon [C], oxygen [O], hydrogen [H],
and nitrogen [N]; for teeth & BONES = calcium [Ca] and phosphorus [P]; for
taste buds = zinc [Zn]; for nervous system = copper [Cu]; for blood = iron [Fe]
*e. There are currently 118 known ELEMENTS and 92 are found in nature, while the others
are SYNTHETICALLY (man-made), but we only use between 30-40 elements daily
*1. The discovery of all the ELEMENTS to date has taken THOUSANDS of years
*2. In ancient times, it was believed there were “4” ELEMENTS: water, air, land, fire
*f. The chemical symbol of an ELEMENT  is a shorthand form of the element’s NAME
*1. The chemical SYMBOL always BEGINS with a CAPITAL letter, with any other
letter(s) written in their LOWER-CASE form
*a. (e.g.) sulfur [S]; iodine [I]; fluorine [F]; helium [He]; gallium [Ga]
*2. Some elements’ CHEMICAL symbols are based on their Latin, Greek or Arabic name
*a. (e.g.) gold [Au]; silver [Ag]; mercury [Hg]; tin [Sn]; lead [Pb]
6. COMPOUND  substance composed of two or more kinds of ATOM that has been CHEMICALLY
combined (e.g. sodium chloride [NaCl]; hydrogen peroxide [H2O2]; iron oxide [Fe2O3])
a. every COMPOUND has its own distinct PROPERTIES
1. the PROPERTIES of a compound differ from the PROPERTIES of the individual
ELEMENTS making up the COMPOUND
a. (e.g.) sodium [Na] and chlorine [Cl] individually have totally DIFFERENT
properties compared to the COMPOUND sodium chloride [NaCl]
b. MOST matter on Earth exists in the form of a COMPOUND
*c. When a COMPOUND forms, it ALWAYS contains the SAME elements and the SAME
number of atoms per ELEMENT in exactly the SAME ratio
*1. WATER = is always composed of the ELEMENTS hydrogen [H] and oxygen [O]
with a 2:1 ratio of atoms respectively  H2O
*2. HYDROGEN PEROXIDE = is always composed of the ELEMENTS hydrogen [H]
and oxygen [O] with a 2:2 ratio of atoms respectively  H2O2
*d. A chemical formula  is a chemical abbreviation for writing a COMPOUND
*1. A formula includes: CHEMICAL symbols of the ELEMENTS and numbers written
as subscripts to show the ratio of ATOMS per ELEMENT
*a. If an ELEMENT has NO subscript, the SUBSCRIPT is understood to be “1”
*b. (e.g.) carbon monoxide [CO]; carbon dioxide [CO2]; ammonia [NH3]
*e. Examples of COMPOUNDS:
*1. Table salt = NaCl [sodium, chlorine w/1:1 atom ratio]
*2. Sand = SiO2 [silicon, oxygen w/1:2 atom ratio]
*3. Table sugar = C12H22O11 [carbon, hydrogen, oxygen w/12:22:11 atom ratio]
*4. Glucose = C6H12O6 [carbon, hydrogen, oxygen w/6:12:6 atom ratio]
*5. Chalk = CaCO3 [calcium, carbon, oxygen w/1:1:3 atom ratio]
*6. Iron oxide (rust) = Fe2O3 [iron, oxygen w/2:3 atom ratio]
*7. Baking soda = NaHCO3 [sodium, hydrogen, carbon, oxygen w/1:1:1:3 atom ratio]
*f. COMPOUNDS CAN be broken down, but because the elements were CHEMICALLY joined
together, a CHEMICAL process is necessary to SEPARATE them
*1. Heating breaks down some COMPOUNDS: iron separated from oxygen
(e.g.) 2 Fe2O3 + 3 C (are heated)  4 Fe + 3 CO2 (the IRON [Fe] is SEPARATED)
*2. Electrolysis is an ELECTRIC current passed through some COMPOUNDS to break
them down: water is broken down into HYDROGEN gas [H2] and OXYGEN gas [O2]
(e.g.) 2 H2O (electricity is added)  2 H2 + O2 (the HYDROGEN [H] and OXYGEN [O]
are SEPARATED)
*3. Some COMPOUNDS are so UNSTABLE that they break down without the use of
HEAT or ELECTROLYSIS
*a. LIGHT acts as a catalyst (something that SPEEDS up a reaction) and is all that is
needed to break down an UNSTABLE compound: hydrogen peroxide [H2O2] is
broken down into WATER [H2O] and OXYGEN gas [O2]
(e.g.) 2 H2O2 (exposed to LIGHT)  2 H2O + O2 (DECOMPOSED into water and oxygen)
7. MIXTURE  is matter that has been MIXED or blended together PHYSICALLY, but NOT
___________________ combined
a. since MIXTURES are NOT ____________________ joined together, each substance retains its
__________________ and CHEMICAL properties
*b. MIXTURES, however, do _____ require a specific RATIO of substances
*1. Sugar water = is composed of the SOLUTE (substance being dissolved) sugar and the
SOLVENT (substance doing the dissolving) water
*a. Add more sugar (______________), the solution becomes CONCENTRATED
*b. Add LESS sugar (______________), the solution becomes DILUTED
B. Pure Substances: ELEMENTS and COMPOUNDS
1. Two types of PURE substances:
 __________________ (e.g.) potassium [__]; aluminum [___]; sodium [___]
 __________________ (e.g.) _____ [NaCl]; glucose [_______]; TABLE _______ [C12H22O11]
2. Pure substances have definite characteristic (INTRINSIC), physical, and chemical ______________
a. Properties of PURE substances remain consistent because the most basic particles (_______ and
_____________) making up each substance are IDENTICAL [(e.g.) copper [__]; water [____] ]
3. CHEMICAL bonds (ionic and covalent bonds) are FORCES that hold the __________ together that
form COMPOUNDS and can only be broken by a _______________ change (electrolysis, heat, light)
4. Classifications of PURE substances are according to their PROPERTIES
a. ELEMENTS are classified into 3 groups: __________, ______________ and METALLOIDS
*1. METALS (metallic) have the following PROPERTIES:
*a. LUSTER  the amount of __________ or brightness (e.g.) chromium [___]
*b. MALLEABLE  able to be hammered, rolled, or shaped without _____________
(e.g.) copper (___); gold [___]; aluminum [___]
*c. _________  able to be drawn into a WIRE (e.g.) tungsten [__]; platinum [___]
*d. Good CONDUCTORS of _______  items made from these elements heat quickly
and distribute the heat evenly (e.g.) iron [___]; aluminum [___]
*e. Good ______________ of ELECTRICITY  metals through which electrons move
freely forming ____________ currents (e.g.) gold [__]; copper [__]; tungsten [__]
*f. ______ of MATTER at room temperature (25o C)  most metals are a SOLID at
room temp; except mercury [___]; copernicium [___], which are ________ at 25o C
*g. Some METALS exist for a short period of time in pure form (e.g.) francium [___]
*2. NON-METALS (non-metallic) elements’ PROPERTIES:
*a. ________ of MATTER at room temperature (25o C)  nonmetals are a SOLID or
____ at room temperature, except bromine [__], only _________ non-metal at 25o C
*1. Nonmetals have “____________” properties of metals: low or no LUSTER,
poor conductors of HEAT /electricity, and not ductile or _______________
*3. METALLOIDS, the “6” elements that BORDER between the _______________ and
NONMETALS, having properties “___________” those of METALS and _____________
*a. Common metalloids:
*1. silicon [__] – combined with oxygen forming sand [_____], glass and cement
*2. boron [__] – is used in CLEANING solutions
*3. arsenic [__] – is a POISON
*b. Metalloids CONDUCT electricity LESS efficiently than ___________, but MORE
efficiently than _____________________
*1. silicon [__] and germanium [__] – are used as ______-CONDUCTORS to
make computer chips, transistors, and LASERS
*c. Two other METALLOIDS are: _______________ [Sb] and ______________ [Te]
*d. _______________ [Al] although it borders the line that SEPARATES the metallic
from the non-metallic ELEMENTS; it is definitely a ______________
*e. ____________ [At] and ___________ [Po] also border the zigzag line, but are still
being debated as to whether they are METALLOIDS
b. COMPOUNDS can be classified as a BASE, ________, or NEUTRAL substance based on their
“pH” value (determined using a LITMUS indicator):
 ACIDS have a pH value ________ “7”; (e.g.) vinegar [CH3COOH]; litmus turns RED
 BASES have a pH value _______ “7”; (e.g.) baking soda [NaHCO3]; litmus turns BLUE
 NEUTRAL substances’ ___ value is “_”; (e.g.) distilled water [____]; litmus NO change
c. COMPOUNDS can also be classified as ORGANIC or INORGANIC
1. ORGANIC compounds have chemical bonds between carbon [__] & hydrogen [__] atoms
a. ____________ compounds made from BIOTIC matter are called BIOCHEMICALS
1. Four categories of _____________________:
a. _______________________: a macronutrient and source of ENERGY
(e.g.) sugar, starch, fiber
b. ___________: a macronutrient that stores EXCESS energy and forms
CELL membranes (e.g.) FATS, oil, wax
c. ___________: a macronutrient that regulates body CHEMICAL
activities; builds and REPAIRS cellular structures
d. _________ ______: contain genetic information (e.g.) _____ and RNA;
build PROTEINS
C. Mixtures
1. MIXTURE  consists of TWO or more substances that are MIXED / BLENDED together, but do
NOT react ____________ to form a NEW substance, instead keeping their original PROPERTIES
2. Mixtures are not ______ substances (not an element or compound)
3. Components of a MIXTURE are NOT all IDENTICAL and do NOT have DEFINITE properties
because they do NOT have a defined __________________ makeup
4. Mixtures can be __________________ by PHYSICAL means which depends on their physical and
chemical PROPERTIES
*a. Methods used to separate the substances of MIXTURES are:
 ____________ separation the substances (e.g. remove mushroom topping from pizza)
 ___________________ various sized particles (e.g. sifting dirt particles)
 __________________ force of attraction or repulsion between MAGNETIC materials
*1. (e.g.) iron [Fe – most _____________ element ] nails from aluminum [___] nails)
 __________ (mass/volume) can separate substances NATURALLY (e.g. sand in water)
*1. CENTRIFUGE [e.g. separates parts of _______ (white, red blood cells; plasma)]
 DISTILLATION is the process of BOILING away water or letting water _____________
(the 2 forms of vaporization) from a SOLUTION, leaving the SOLID that was
DISSOLVED as a residue
5. MIXTURES are classified into two types: HOMOGENEOUS and HETEROGENEOUS
a. HOMOGENEOUS  the substances are EVENLY dispersed throughout the _______________
due to the __________________ (going from areas of HIGH concentration to areas of LOW
concentration) of the particles throughout the mixture
1. Particles are extremely SMALL; they will _____ settle out; ALWAYS stay ___________
2. SOLUTION  homogeneous mixture where one substance is _____________ in another
*a. Types of SOLUTIONS:
*1. the most common SOLUTION is a _________ dissolved in a LIQUID
*a. (e.g.) SUGAR (solute – the substance being dissolved) and water
(solvent – the substance that dissolves other materials)
*2. one LIQUID dissolved in another ____________
*a. (e.g.) Ethylene glycol (________) and WATER (__________) to make
ANTIFREEZE (FREEZING pt = -13o C; ___________ pt = 176 o C)
*3. a _______ dissolved in a LIQUID
*a. (e.g.) CARBON DIOXIDE gas (_________) and soda (_________) to
make a carbonated soft drink
*4. a ________ dissolved in another GAS
*a. (e.g.) _____ is a mixture of oxygen [__], argon [___] and carbon
dioxide [_____] (SOLUTES); nitrogen gas [N2] (______________)
*b. ALLOYS  (special solutions) are solid SOLUTIONS of metals ____________
in other metals and also non-metals ______________ in METALS
*1. Steel  is a SOLUTION of metal iron [__] and non-metal carbon [__];
making the steel alloy exceptionally strong
*2. Bronze  is a _______________ of metal copper [__] and metal tin [__];
bronze is the earliest of the _____________
*3. Brass  is a ______________ of metal copper [__] and metal zinc [__];
making the brass alloy very ______________ (bendable/shapeable)
*4. Sterling silver  is a ____________ of metal silver [__] and metal copper
[__]; harder and does NOT tarnish like pure silver [___]
*5. Solder  is a __________ of metal tin [__] and metal lead [__]; LOW
MELTING point and is used to join _____________ together
*6. Wood’s metal  is a __________ of metal bismuth [__], metal lead [__],
metal tin [__], and metal cadmium [__]; used in
sprinkler systems in buildings
*c. Concentration  is a way to describe a SOLUTION because different amounts
of _______________ can be DISSOLVED in different amounts of ___________
*1. DILUTE  are solutions with a __________ amount of SOLUTE
*a. (e.g.) “WEAK” tea (_____________ in color; __________ in taste)
*2. CONCENTRATED  are solutions with a LARGE amount of _________
*a. (e.g.) “STRONG” tea (darker in _________; stronger in ________)
*d. Solubility  is a MEASURE of how well a ___________ can ______________
in a SOLVENT at a given TEMPERATURE
*1. SOLUBLE  SOLUTES that WILL _______________ in a ___________
*2. INSOLUBLE  _____________ that will ____ dissolve in a SOLVENT
*3. SATURATED  are solutions with so much SOLUTE that NO _________
will DISSOLVE
*4. UNSATURATED  are solutions where ________ solute will CONTINUE
to _________________ when added to the SOLVENT
*5. SUPERSATURATED  are solutions containing more SOLUTE than the
SOLVENT at a given _________________ can DISSOLVE
*6. For many SOLIDS, solubility INCREASES as the temperatures __________,
because a solid’s particles move ____________ and spread _______________
apart allowing more room in the SOLVENT for ________ dissolved particles
*a. (e.g.) Potassium nitrate [__NO3] and ______________ chloride [KCl]
*7. For many GASES, an __________________ in temperature DECREASES the
solubility of a gas in a liquid, because the speed of the dissolved gas particles
INCREASES, causing the particles to gain energy and _______________ the
solution more readily.
*a. (e.g.) Bubbles of DISSOLVED air escape long before the water boils,
because water is able to hold ______ air in solution as its temperature
_________________
*e. Effects of Solutes on Solutions
*1. Lower the Freezing Points  Solutes LOWER the FREEZING point of a
___________, because the SOLUTE particles interfere with the SOLVENT’S
particles making it HARDER for the water molecules to form _____________
*a. (e.g.) A salt water SOLUTION – the temperature must drop lower
than ___C for water to ____________ and for a SOLID to form
*2. Higher Boiling Points  Solutes RAISE the BOILING point of a
___________, because the SOLUTE particles make it HARDER for the water
molecules to gain energy and _____________ into the air.
*a. (e.g.) A salt water SOLUTION – temperature must go higher than
____ C for the water to gain more ________ for the water to BOIL
*f. Water [H2O] is the UNIVERSAL solvent for _________________
*1. However, NOT all solutes _________________ in water
*a. (e.g.) oil-based paints require TURPENTINE as the _____________
b. HETEROGENEOUS  substances ______ evenly distributed throughout the MIXTURE
1. Particles are LARGER, can __________ in size and do NOT stay ____________
2. SUSPENSION  heterogeneous mixture where particles of one substance are
SCATTERED throughout another substance and WILL eventually ________ out
*3. Types of SUSPENSIONS:
*1. solid particles _________________ / SUSPENDED in a liquid
*a. (e.g.) sand in WATER; juices w/_________; Italian SALAD dressing
*2. solid particles _________________ / SUSPENDED in a gas
*a. (e.g.) dust or SMOKE particles in the ______
*3. gas molecules _________________ / SUSPENDED in a liquid
*a. (e.g.) AIR scattered in a “creamy” fluid to make shaving __________ and
________________ cream
*4. COLLOID  has MEDIUM - SIZED particles that remain MIXED in a gas, _______
or ____________
*a. Colloids appear to be SOLUTIONS, because their particles are well-mixed
and are too _________ to be SEEN because they are ___________________
evenly in another substance
*1. Colloids are HETEROGENEOUS, but have a homogeneous ______
*b. a COLLOID’s particles are large enough, however, to “______________”
or “SUSPEND” a beam of ____________, but a solution’s particles are NOT
*c. (e.g.) MILK, fog, ________________, gelatin and ________________
*d. SOLUTION versus ______________ (Tyndall effect):
*5. EMULSION  is a special type of COLLOID that consists of one liquid ___________
in another LIQUID
*a. Emulsions are well-mixed substances that have a homogeneous _________,
but are ______________________ mixtures
*b. (e.g.) mayonnaise is an EMULSION of vinegar (_________) SUSPENDED
in oil (_____________) and egg yolks (the emulsifier)
*c. EMULSIFIER  is a substance that keeps the particles in one LIQUID
MIXED in another __________
*1. (e.g.) in mayonnaise the ___________________ is the EGG YOLKS
*d. Many, but NOT all EMULSIONS have ____________________