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Unit 3 – Lessons 1-4 “ATOMS and the PERIODIC TABLE” (Pages 153-208)
I. LESSON 1
A. The Atom
1. The basic UNIT of all MATTER is the __________
2. ATOM  is the SMALLEST particle of an ___________ retaining all the chemical _____________
of that ELEMENT
3. Democritus’s GREEK term “____________,” which means “not able to be divided,” is the ORIGIN
of the word, ___________
*4. Individual ATOMS are so __________ they can only be seen using a scanning tunneling
MICROSCOPE (STM), a special type of ELECTRON microscope
*a. Due to their __________ size, huge numbers of ATOMS are used in the composition of very
small substances
*b. The average DIAMETER (distance across) of an __________ is about ________________ m
or 2 x 10-9 m (scientific notation) or [2 nm (nanometers)]
*5. Scientific notation  is a system of writing NUMBERS with a LARGE number of place value
positions containing zeroes
*a. SCIENTIFIC NOTATION is a ________________ written as a product with two FACTORS
1. The 1st FACTOR is a single digit whole number greater than ___, but less than __
2. The 2nd FACTOR is a ____________ of 10 in exponential form [(e.g.) “105” ]
*b. Steps for writing a NUMBER in a SCIENTIFIC NOTATION format:
1. Move the decimal ______ until the first NUMBER is “1” or between “1-10” but not __
a. The first factor may be a _________-___________ (e.g. 1.8 or 3.22)
2. Count the number of PLACE VALUE positions moved and express that total as an
__________________
a. When you move the ____________ point to the left, the EXPONENT will be
expressed as a POSITIVE number
b. When you move the DECIMAL point to the ________, the ______________
will be expressed as a ___________________ number
3.(e.g.) Speed of light  30, 000,000,000 cm/sec = __ x 10 __ cm/sec
Mass of a dust particle  0.000000000753 kg = _____ x 10 __ kg
*c. A neutron’s mass is 168 hundred-octillionths of a kg
*1. (e.g.) Standard format: 0.00000000000000000000000000168 kg
Scientific notation: ______________________
*d. An electron’s mass is 9,109,822 hundred-undecillionths of a kg
*1. (e.g.) Standard format: 0.0000000000000000000000000000009109822 kg
Scientific notation: ______________________
*e. The Earth’s circumference is 40 million meters
*1. (e.g.) Scientific notation: 40,000,000 = ________________
f. A penny contains about “20” sextillion ____________ of COPPER [___] and ZINC [___]
1. (e.g.) Scientific notation: 20,000,000,000,000,000,000,000 = _____________
B. Atomic Theory
1. Dalton’s _________________ of the ATOM having certain characteristics, form the BASIS of our
understanding of ____________ today
a. All MATTER is composed of _____________
b. Atoms can NOT be ________________, DIVIDED or _________________
c. All the _____________ of a specific ELEMENT are IDENTICAL
1. Explains why an ELEMENT always has the same _________________
d. Atoms of two or more ELEMENTS can COMBINE to form _______ substances
*e. Atoms of each ELEMENT have a unique MASS
*1. The number of PROTONS plus _____________ in the _____________ give an atom its
characteristic atomic MASS
*f. The MASSES of the ELEMENTS in a COMPOUND are ALWAYS in the same RATIO
*1. Since compounds have a specific chemical ______________, the ELEMENT(S) and the
number (or RATIO) of ATOMS per ELEMENT are always the ________. Therefore,
the RATIO of the MASS of each ________________ is also always the ___________
*a. (e.g.) calcium oxide [Ca5O2] = 5 (Ca amu) + 2 (O amu) = ______ amu
5 ( ___ amu) + 2 ( ___ amu)
( ____ amu) + ( ____ amu)
2. Thomson provided evidence of ATOMS having ______________ charged particles = ELECTRONS
3. Rutherford’s experiments provided evidence that the ATOM contained a DENSE, central core called
a _____________, composed of POSITIVELY charged, SUBATOMIC particles called __________
4. Chadwick discovered that the ATOM contained UNCHARGED particles called ________________
5. Bohr’s observations provided ATOM behavior based on ELECTRON movement around the
_______________ on circular _____________ paths (ENERGY levels)
6. Today:
a. ELECTRON CLOUDS  the area around the NUCLEUS where ___________________ move
*b. QUARKS  the sub-subatomic particles that make up _____________ and _______________
C. Parts of an Atom
1. Within the NUCLEUS:
a. NUCLEUS:
 refers to the dense, inner most _____________ of an __________ containing the PROTONS
(__________ charged particles) and the _____________ (particles that have NO CHARGE)
*1. the NUCLEUS is the most _______________ part of an ATOM
b. PROTON:
 ________________ electrical CHARGE
*1. written as: one proton = 1+; atom with “14” PROTONS = ______

this MASSIVE subatomic particle along with the ____________ count gives an ATOM its
atomic ______ number (measured in “____” units or UNIFIED atomic mass units “__”)
*1. mass of a PROTON = 0.0000000000000000000000000017 u = 17 ten-octillionths
u = ____________ u (in SCIENTIFIC NOTATION)

number of ____________ (atomic number) determines the _________________ of the
ELEMENT
*1. ATOMIC number  is the ____________ count; unique for each ELEMENT
*2. (e.g.) atomic number = 5; ___________ count = ____; element = __________ [B]

proton COUNT can _____ change for an ELEMENT or you have a different __________
*1. (e.g.) PROTON count = 10; element = ___________ [Ne]
“1” less proton than neon = 9; element = _________________ [F]
“1” more proton than neon = 11; element = _____________ [___]
c. NEUTRON:
 ____ electrical CHARGE
*1. (e.g.) beryllium [__]: 4 protons = “___” and 5 NEUTRONS = “___” NET charge

this MASSIVE subatomic particle along with the ___________ count gives an ATOM its
atomic _______ number (measured in “_____” units or ____________ atomic mass “u”)
*1. mass of a NEUTRON = slightly more than a _____________
*2. (e.g.) beryllium [__]: 4 protons = “__” and 5 NEUTRONS = “__” u (or “__” amu)

neutron COUNT _____ change for an ELEMENT forming _____________
*1. Steps to finding the NEUTRON count from a _______________ table
*a. Find the atomic number (____________ count)
*b. Find the average atomic _____ number (mixed decimal on Periodic Table)
*c. __________ the average atomic mass number to the nearest whole number
*d. _____________ the atomic number from the atomic mass number
*e. (e.g.) manganese [___]  atomic number = ____
average atomic mass # = _______ ~ ____ (atomic mass #)
manganese [___] = “___” neutrons
*2. ISOTOPE  atoms of the same ELEMENT with the same ___________ count
(atomic number), but have a DIFFERENT number of ____________
and therefore have a DIFFERENT atomic ________ number
*a. hydrogen (protium) [__]  proton = ___; neutron = __; __ amu
*b. hydrogen (deuterium) [__]  proton = ___; neutron = __; __ amu (isotope)
*c. hydrogen (tritium) [__]  proton = ____; neutron = __; __ amu (isotope)
2. Outside the NUCLEUS:
a. ELECTRON:
 ______________ electrical CHARGE
*1. written as: one electron = 1-; atom with “14” ELECTRONS = “____”
2. the charges of PROTONS and ELECTRONS are OPPOSITE but ___________,
which makes the ATOM electrically ________________ (NET charge = “__”)
*3. (e.g.) beryllium [__]: 4 protons = “__” + “4-” ______________ = “__” net charge

has relatively NO _________; the ELECTRONS are ___________ used to determine the
atomic ___________ of an ELEMENT
*1. ________ of an ELECTRON is 1,860 times _____ than a _________ or NEUTRON
*2. (e.g.) lithium [__]: protons = 3+; electrons = 3-; neutrons = 4 = __ u (or __ amu)

are in constant MOTION around the _________ of the nucleus within the electron CLOUD
*1. HEISENBERG RULE  states that it is NOT possible to determine the exact
LOCATION and SPEED of an _______________ simultaneously
*2. ELECTRON models show their movement on paths called energy _____________
(or energy LEVELS or energy SHELLS)

electron COUNT _____ change for an ELEMENT when forming _______ bonds by
transferring (giving up or taking on) _________________, producing IONS
*1. ION  an electrically charged _________ (having a “+” or “-” charge) due to
ELECTRONS being _____________________ (gained or lost)
*2. IONIC bond  the FORCE that attracts ________________ charged IONS and
CHEMICALLY holds them together
*a. sodium [___] will lose “1” ______________ to become stable = “___”
*b. chlorine [____] will gain “1” _____________ to become stable = “___”
*3. STABLE  the outer-most, VALENCE energy _______________ contains the
MAXIMUM number of valence _________________
*a. helium [__] = 1st energy ORBITAL contains “__” electrons (maximum)
*b. krypton [__] = 4th energy __________ contains “__” electrons (maximum)
D. Atomic Number verses Atomic Mass Number
1. Different COMBINATIONS of ____________, ___________ and _____________ produce ATOMS
with different PROPERTIES (ELEMENTS)
a. These different ATOMS chemically COMBINE to form different, _______ substances
(COMPOUNDS)
2. The number of ______________ distinguishes each ATOM from the other 118 ______________
3. ATOMIC NUMBER  the number of ______________ in the NUCLEUS of an ATOM
a. (e.g.) iron [__] atomic number = 26; proton count = ____
tin [___] atomic number = ___; proton count = 50+
mercury [___] (a ___________ metal) atomic number = ___; proton count = ____
bromine [___] (only liquid __________) atomic number = ___; proton count = ___
californium [___] (period 7; actinides) atomic number = ___; proton count = ____
4. The ATOM of a specific ELEMENT always has the ________ number of PROTONS, but it does
______ always have the same number of NEUTRONS
a. (e.g.) chlorine [__] ALWAYS has 17+ __________, but it could have 18 or 20 ___________
b. chlorine-35 [__] with 17+ ____________ and 18 ____________ = ISOTOPE of CHLORINE
chlorine-37 [__] with ___+ ___________ and 20 ____________ = __________ of CHLORINE
5. Atomic MASS NUMBER  is TOTAL number of _____________ plus ______________ in the
NUCLEUS of a specific ATOM
a. (e.g.) silver [__] (period 5; group 11) proton count = ____; neutron count = 61 = _____ u
argon [__] (period 3; group 18) proton count = ____; neutron count = 22 = _____ u
arsenic [__] (period 4; group 15) proton count = ___; neutron count = 42 = _____ u
lead [__] (period 6; group 14) proton count = ____; neutron count = 125 = _____ u
uranium [___] (period 7; actinides) proton count = ___; neutron count = 146 = ____ u
*6. AVERAGE ATOMIC MASS  is the weighted average of the MASSES of all the naturally
occurring ISOTOPES of an _________________
*a. generally ___________ decimals on the Periodic Table
*1. Exception: RADIOACTIVE elements’ most common ____________ (whole numbers)
b. (e.g.) potassium [__] (period 4; group 1) average atomic mass = ________
phosphorus [__] (period 3; group 15) average atomic mass = ___________
gold [___] (period 6; group 11) average atomic mass = _____________
praseodymium [___] (period 6; lanthanides) average atomic mass = __________
mendelevium [___] (period 7; actinides) average atomic mass = (_____)