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Note Taking Guide: Episode 301 Name___________________ Model: A __________ idea used to explain __________ facts __________ in __________. Theory: An __________ of __________ facts and __________. To remain valid, models and theories must: • • __________ all known __________ enable __________ to make correct __________ Democritus: • proposed the __________ of an __________ • word comes from the __________ word __________ which means __________ __________ __________ or “indivisible” Aristotle • __________ the __________ of the __________ • said __________ could be __________ __________ Dalton’s • • • • • theory proposed that atoms: are __________ __________ of __________ are __________ of the __________ __________ are __________ of __________ __________ are __________ __________ in __________, __________ __________ ratios to form __________ J.J. Thomson • credited with __________ of __________: a blow to __________ __________ atom • proposed the __________ __________ model of the __________: __________ charged __________ embedded in a ball of __________ __________ CHEMISTRY: A Study of Matter © 2004, GPB 3.1 Rutherford’s Gold-foil Experiment: • aimed __________ __________ at __________ __________ • __________ passed __________ • a __________ particles were __________ • __________ particles even __________ __________ Conclusions of Rutherford's experiment: • __________ of the __________ is __________ __________ • __________ ____________ charged __________ The Chemistry Quiz CR1._____ CR2._____ 3._____ 1._____ 4._____ CHEMISTRY: A Study of Matter © 2004, GPB 3.2 2._____ 5._____ Worksheet: Development of Atomic Theory Name___________________ True-False: place a "+" in the blank if the statement is true, and a "O" in the blank if the statement is false. 1. Dalton's atomic theory stated: a. atoms are indivisible. b. all atoms of the same element are alike. c. atoms unite in small, whole number ratios to form compounds. _____ _____ _____ 2. The Greek philosopher Democritus was one of the first to suggest the existence of atoms. _____ 3. The word "atom" means invisible. _____ 4. A theory is an explanation of observable facts and phenomena. _____ 5. Aristotle supported the idea of the atom. _____ 6. From the "gold-foil" experiment it was concluded that the atom is mostly empty space. _____ Short Answer and Fill in the Blanks: 1. What must models and theories do in order to remain valid? a. b. 2. The "gold-foil" experiment had the following results: ____________ of the alpha particles were deflected, ______________ of the alpha particles were reflected, and _____________ of the alpha particles passed through the gold foil. CHEMISTRY: A Study of Matter © 2004, GPB 3.3 Note Taking Guide: Episode 302 Name___________________ Nucleons- __________ in the __________ of __________ • __________ • __________ Atomic Number- __________ of __________ in the __________ of an __________ Neutral atom- # of __________ (+) = # of __________ (-) Isotope- __________ of an __________ that have __________ __________ of __________. Isotopes of Hydrogen Hydrogen-1 _______ proton and _______ neutrons Hydrogen-2 _______ proton and _______ neutrons Hydrogen-3 _______ proton and _______ neutrons Mass Number- __________ number of __________ and __________ in an __________. Example: Carbon-14 _________________ Neon-20 _________________ Particle Proton Charge Mass Location Neutron Electron Atomic Mass- __________ of the __________ of all the element’s __________ CHEMISTRY: A Study of Matter © 2004, GPB 3.4 Subatomic Particles # of protons =__________ __________ # of electrons = __________ __________ # of neutrons = __________ __________ - __________ __________ 26 Fe iron: 55.8 __________ protons __________ electrons __________ neutrons 8 oxygen-17: O 15.994 __________ protons __________ electrons __________ neutrons 4 2 He __________ protons __________ electrons __________ neutrons The Chemistry Quiz CR1._____ CR2._____ 3._____ 1._____ 4._____ CHEMISTRY: A Study of Matter © 2004, GPB 3.5 2._____ 5._____ Worksheet: Atomic Structure Name___________________ Use your notes from the Atomic Structure program to answer the following questions. 1. The atomic number tells the number of positively charged ________ in the nucleus of an atom. The atom is __________ because this is also the number of __________ charged __________ in the atom. 2. The mass number tells the total number of________ and _________ in the nucleus of an atom. These particles collectively are called ___________ since both are located in the nucleus. 3. Isotopes are atoms of the same element with different numbers of _________ which results in different _______ numbers. 4. Write the hyphen notation of the three isotopes of hydrogen: a. b. c. 5. Fill in the following chart (Hint: Isotopes may have different masses than the periodic table lists!): Symbol Atomic # Mass # Hg 80 201 Mo 42 96 # of protons # of electrons # of neutrons 29 35 29 C 14 15 Pb Na 31 208 82 11 13 CHEMISTRY: A Study of Matter © 2004, GPB 3.6 Lab: Atoms and Eggs—Datasheet Name___________________ Inside the nucleus of an atom are ______________ and _______________. The __________ ______________ of an atom is the sum of these two particles. The atomic number is equal to the number of __________________ present in the nucleus of the atom, and because the atom is neutral, the atomic number is also the number of ________________ outside the nucleus of the atom. Procedure: In this activity an “egg” will represent the nucleus of an atom and different colors of candy will represent the subatomic particles within the nucleus. Write the description of the candy used to represent the subatomic particles based on your teacher’s instructions below: Particle Description __________________ ________________________________ __________________ ________________________________ The “atoms” have been numbered. In the data table, write the number of the “atom”, the number of each subatomic particle present, the mass number, and the nuclear symbol for the element represented by the “atom” as well as the hyphen notation for that atom. # of Atom # of protons # of neutrons Mass number Nuclear Symbol CHEMISTRY: A Study of Matter © 2004, GPB 3.7 Hyphen Notation Lab: Isotopes—Datasheet Name______________ Purpose: A new element has been discovered and it is your responsibility to learn the following about the element: • the number of naturally occurring isotopes present in the element • the percentage of each isotope present in your sample of the element • the atomic mass of the element Procedure: 1. Obtain a sample of the element from your teacher and record its ID number above the chart. 2. Count the total number of atoms in your sample and record in the space labeled as such beside the blank for the ID#. 3. Separate the element into its different isotopes. Assign each isotope a letter to identify it and record this letter in the first column of the chart. 4. Count the number of atoms of each isotope and record in the second column of the chart. 5. Calculate the percentage of each isotope present in your element (# of atoms of isotope/total # of atoms in sample) and record in the last column of the chart. 6. Mass each isotope group of atoms and record in the third column under "Mass of Isotope Group”. 7. Calculate the average mass of one atom of that isotope (Mass of Isotope Group/ # of atoms of that isotope) and record under "Average Mass of Isotope Group." ID #______________ Total # of Atoms in Sample ________ Isotope # of atoms in Isotope Group Mass of Isotope Group Average Mass of Isotope Group Percentage of Isotope Group 8. On the back of this worksheet, determine the average atomic mass of your element using this equation: Be sure to show your work! Average atomic mass = (avg. mass of isotope)(%) + (avg. mass of isotope)(%) + ... (Remember that % means "per 100". In a calculation, 50% becomes 50/100 or 0.50.) 9. Give your element a name and symbol and record the information here. Remember that this is a new element so you, as a scientist, get to name this element whatever you want! Element Name:______________ Symbol_____ Atomic Mass_________ CHEMISTRY: A Study of Matter © 2004, GPB 3.8 Worksheet: Isotope Problems Name___________________ 1. A student looked up the naturally occurring isotopes of bromine and found the following information: 50.54% of the naturally occurring isotopes of bromine have an atomic mass of 78.92 u while 49.46% of the naturally occurring isotopes of bromine have an atomic mass of 80.92 u. Calculate the average atomic mass of bromine, showing all work: 2. Using the following data, calculate the average atomic mass of magnesium (give your answer to the nearest .01 u) : Show all work! Isotope: Percent abundance: 78.70% 25 Isotope: 12 Mg Percent abundance: 10.13% 26 Isotope: 12 Mg Percent abundance: 11.17% 24 12 Mg 3. Using the periodic table, What is the average atomic mass of bromine? ____________ What is the average atomic mass of magnesium? __________ How do your calculated answers in #1 and #2 compare to those on the periodic table? ________________________________________ CHEMISTRY: A Study of Matter © 2004, GPB 3.9 Note Taking Guide: Episode 303 Name___________________ Bohr's Energy Levels • Electrons in __________ __________ __________ • __________ energy levels: __________ to __________ • __________ energy levels: __________ from __________ • Ground State: __________ in __________ __________ __________ possible Excited Atom • Atom has __________ __________. • __________ state is __________. • __________ soon __________ same amount of __________ __________. • __________ seen as __________ __________. Wave Description of Light Wavelength (_____): __________ between __________ __________ on __________ waves Frequency (_____): the __________ of __________ passing a given __________ in a given __________ c = __________ c = _______________ : speed of ___________ Sample problem #1: What is the frequency of light if the wavelength is 6.0 x 10 -7 m? CHEMISTRY: A Study of Matter © 2004, GPB 3.10 Sample problem #2: What is the wavelength of light if its frequency is 5.0 x 1014 Hz? Particle Description of Light __________ exists as __________ called __________ E = ____________ • • The Modern View of Light __________ has a __________ __________. Light may __________ as a __________. Light may __________ as a __________ of __________ called __________ or __________. Spectroscopy • __________ lines represent __________ __________ as __________ returns to __________ __________ __________. • __________ lines __________ an __________. • Called the __________ __________ ____________ of an __________. Orbital __________ of __________ where an __________ is __________ to be __________ The Chemistry Quiz CR1._____ CR2._____ 3._____ 1._____ 4._____ © 2004, GPB 3.11 2._____ 5._____ Worksheet: Electrons in Atoms I. Name___________________ Fill in the blanks with the most appropriate term: In Bohr’s model of the atom, electrons are in certain ___________ levels, with the levels closest to the nucleus of __________ energy than those farther from the nucleus. In the _____________ state of the atom, the electrons are in the lowest _____________ level possible. When an atom absorbs energy, it is said to be in the _______________ state, which is unstable. The atom will soon _______ the same amount of energy absorbed which may be seen as visible light. In the study of ________________, this visible light is seen as the ________ __________ spectrum of an element, which is also called an element’s “fingerprints”. The modern view of light is that it has a _____________ nature. In other words, light may behave as a stream of particles called ____________ or ___________, or light may behave as a ______________. Modern scientists suggest that the nature of light depends on the experiment! In the wave view of light, the wave equation is often used to determine a wave’s frequency or wavelength. The ____________ is the distance between corresponding points on adjacent waves while the _______________ is the number of waves passing a given point in a given time. The wave equation is: ____________ II. 1. Use the wave equation to solve the following: What is the frequency of light with a wavelength of 1.87 x 10-14 m? 2. What is the wavelength of light with a frequency of 5.6 x 1014 Hz? III. 1. Short Answer: According to Planck’s equation, E = hf , what is the relationship between the frequency and the energy of light? 2. According to the wave equation, ________________, what is the relationship between the frequency and wavelength of light? CHEMISTRY: A Study of Matter © 2004, GPB 3.12 Note Taking Guide: Episode 304 Name___________________ Quantum Numbers • ___________________________________ • Used to __________ an __________ in an __________ n • • __________ __________ __________ Represents __________ energy level of __________ __________ # of __________ in an __________ __________ = __________ Example: What is the maximum number of electrons that can be in the _____ main energy level? l • • • The __________ __________ __________ Describes the __________ __________ within an __________ __________ __________ of orbital __________ possible in __________ __________ = __________ Orbital Shapes designated __________________ • level 1: __________ • level 2: __________ • level 3: __________ • level 4: __________ How many electrons can each sublevel hold? s = 1 orbital x 2 e-/orbital = _______ep = 3 orbitals x 2 e-/orbital = _______ed = 5 orbitals x 2 e-/orbital = _______ef = 7 orbitals x 2 e-/orbital = _______e- CHEMISTRY: A Study of Matter © 2004, GPB 3.13 m • • s • • The __________ __________ __________ describes __________ of __________ in __________ The __________ __________ __________ describes __________ of __________ in __________ Ground State: __________ energy arrangement of __________ Diagonal Rule Examples— hydrogen _______________ lithium_________________ nitrogen ________________ Orbital Notation Examples— hydrogen nitrogen CHEMISTRY: A Study of Matter © 2004, GPB 3.14 Hund's Rule: __________ of __________ __________ are each __________ by one __________ before any __________ is occupied by a __________ __________. Pauli Exclusion Principle: No two __________ in the __________ __________ can have the __________ __________ of __________ __________ __________. The Chemistry Quiz CR1._____ CR2._____ 3._____ 1._____ 4._____ CHEMISTRY: A Study of Matter © 2004, GPB 3.15 2._____ 5._____ Worksheet: Energy Levels, Sublevels, Orbitals Name___________________ Energy Level n # of e- in Sublevel E Sublevel (type of orbital) # of Orbitals in Sublevel 1 2 3 4 CHEMISTRY: A Study of Matter © 2004, GPB 3.16 Total # of ein E level (2n2) Worksheet: The Diagonal Rule To determine the order in which electrons will fill orbitals in an atom, use the diagonal rule below. Start at the top 1s and when you reach the end of one arrow, return to the next, working your way down. 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f CHEMISTRY: A Study of Matter © 2004, GPB 3.17 Worksheet: Electron Distributions Name___________________ 1. There are four types of orbitals: s : shaped like a ___________ An E level can contain only _____ s orbital, making up the “s sublevel”. p : shaped like ____________ An E level can contain _____ p orbitals, making up the “p sublevel”. d: shaped like double dumbbells An E level can contain _____ d orbitals, making up the “d sublevel”. f: too complex to draw or describe An E level can contain _____ f orbitals, making up the “f sublevel”. 2. Each orbital can hold a maximum of _____ electrons. Since both electrons have a __________ charge, they __________. What keeps them from flying apart? Each electron _______ on its axis. One spins __________ and the other spins _____________. When charged particles spin, they act like tiny magnets. Since the two electrons spin in ___________ directions, one acts like the north pole of a magnet and the other acts like the south pole. This makes the electrons _____________ . 3. Since each orbital can hold _____ electrons: The “s sublevel” can hold ______ electrons. The “p sublevel” can hold ______ electrons. The “d sublevel” can hold ______ electrons. The “f sublevel” can hold ______ electrons. We use this notation to describe an electron: main _______ level 3p5 # of e- in __________ __________ How are electrons distributed within a sublevel? According to Hund’s Rule, each __________ within a sublevel is half-filled before any is __________. CHEMISTRY: A Study of Matter © 2004, GPB 3.18 We draw orbital diagrams to show the distribution of electrons in a sublevel. Circles are used to represent the individual ________. __________ are used to represent electrons in the orbital. The first electron in an orbital is represented by a ! and the second by a ! . A set of four ______________ numbers is assigned to each __________ to describe its energy and location within the atom. The quantum numbers use the symbols _______, _______, _______, and _______. _______ is the principle quantum number and represents the ________ level of the electron. _______ represents the sublevel of the electron, which depends on the type of _____________. Pauli’s Exclusion Principle states that within an atom, no two electrons can have the same set of _____________ _____________. If two electrons have the same n, l, and m numbers, they are in the same _______ level, the same ___________, and the same _____________. They must then have ____________spins! So, the s quantum numbers must be different. Practice: Write electron distributions and do the orbital notation for the following: 1. P: 2. Ca: Only do the electron distributions for the following: 1. Co: 2. Eu: 3. Tc: CHEMISTRY: A Study of Matter © 2004, GPB 3.19 Worksheet: Electron Distributions Review Name___________________ I. Fill in the blanks: 1. The orbital shaped like a "dumb-bell" is the _____ orbital, while the orbital shaped spherically is the ______ orbital. 2. How many sublevels are present in the third main energy level?_____ 3. What is the maximum number of orbitals in the "d" sublevel?_____ 4. The maximum number of electrons that can occupy an orbital is _____, provided they have ____________ _________. 5. The maximum number of electrons that can occupy an energy level is represented by the formula _________. 6. The highly probable location of an electron within the atom is a(n) _________. II. Write the electron configuration for the following: 1. Mg:______________________________ 2. As:______________________________ III. In the space below, show the orbital notation for Mg: CHEMISTRY: A Study of Matter © 2004, GPB 3.20 Review Sheet: Unit 3 Name___________________ I. Short Answer and Fill in the Blanks: 1. _____________ are a familiar idea used to explain unfamiliar facts observed in nature while a ______________ is an explanation of observable facts and phenomena. To remain valid, models and theories must: a. b. The existence of the atom was proposed by the Greek philosopher ______________. The word “atom” comes from the Greek word “atomos” which means ________________. ____________ was a Greek philosopher who rejected the idea of the atom. __________ __________ was an English schoolmaster who explained the Law of Conservation of Mass, the Law of Definite Proportions, and the Law of Multiple Proportions using an atomic theory. His theory proposed that atoms: a. b. c. d. e. The discovery of the atom’s nucleus can be credited to __________, whose _______-foil experiment provided experimental detail about the atom’s structure. In his experiment, Rutherford aimed _______ particles at a piece of _______ foil. _________ of the particles passed through the foil, but a few were ___________, and some even bounced back (were reflected). He concluded that most of the atom is _________ __________. He also concluded that the atom has a dense, ____________ charged core we call the nucleus. The particles that make up the nucleus of the atom are called ____________ and are comprised of the __________ and ____________ in an atom. Atoms are ___________ because the number of _________ charged protons equals the number of ___________ charged electrons. 2. 3. 4. 5. 6. 7. 8. CHEMISTRY: A Study of Matter © 2004, GPB 3.21 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. __________ are atoms of an element that have different numbers of neutrons, and consequently, different atomic ___________. The _________ _________ of an atom is the sum of all the nucleons of an atom. Rutherford’s planetary model of the atom faced a major problem. Classical physics predicted that the electron, as it circled the nucleus, would ________ energy so eventually the atom would collapse! Bohr placed e- in _________ levels, assuming that the electron won’t lose energy as long as it stays in the allowed level. Bohr suggested that electrons can ________ a quantum or ________ of energy, and then jump to a __________ energy level. This is called the ____________ state. This is an unstable state, and the atom soon gives off the same amount of energy absorbed. Some of this energy is in the form of __________ light. The science of studying visible light through the use of a spectroscope is called _______________. The ___________ lines identify an element and are called the element’s __________ _________ spectrum. The modern view of light is that it has a ___________ nature, behaving as both a ___________ and a stream of ___________. It simply depends on the experiment! Four _________ ___________ are used to describe the location of an electron in an atom. They are _____, _____, ____, and ____. The principal quantum number, _____, represents the main ________ level of the electron. The maximum number of electrons in this level is found using the formula: ________. The second quantum number, _____, describes the _________ shape. In the electron distribution 1s2, the “1” represents the ________ _________ level, the “s” represents the __________, and the “2” represents the number of __________ in the ___________. _________ Rule states that orbitals of equal energy are each occupied by _________ electron before any orbital is occupied by a __________ electron. The _____________ Exclusion Principle states that no two electrons in the ________ atom can have the ________ set of four ________ ________________. CHEMISTRY: A Study of Matter © 2004, GPB 3.22 II. 1. Charts and Problems: Show all work if applicable. Complete the following table: Hyphen Notation Nuclear Symbol Carbon - 12 Atomic Number Mass Number # of Protons # of Electrons # of Neutrons 6 40 19 K 5 2. 6 The relative abundance of the isotopes of oxygen are: Oxygen-16: 99.760% Oxygen-17: 0.037% Oxygen-18: Calculate the average atomic mass of oxygen: 0.204% 3. In a bright-line spectrum, the wavelength of a particular line is 6.0 x 10-7m. What is the frequency of this color of light? 4. The maximum number of electrons in a main energy level is calculated using the formula ___________. Therefore, the maximum number of electrons in the 5th main energy level is: 5. How many sublevels are present in the 4th main energy level?_____ What are they?_______________ 6. The maximum number of electrons that can occupy an orbital is ____, if they have __________ ____________. 7. Do the electron distribution and the orbital notation for: Li: O: CHEMISTRY: A Study of Matter © 2004, GPB 3.23