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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 = (_____)