2 e. 14 e. # e # orbitals. 10 e 5. sublevel. shape of orbital. Orbital Shapes. Notes Orbital Notation; e Config; NGN.
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1 How to build an atom: The bigger (more massive) the atom, the more protons (and neutrons) The bigger the atom, the more electrons Electrons fill lower energy levels first "Aufbau" Principle ("To build up") 7 energy levels 4 sublevels (s, p, d, f) s = holds 2 p = holds 6 d = holds 10 f = holds 14 Diagonal Rule Orbital Shapes sublevel s p d f # # orbitals 2 6 I shape of orbital 1
2 2
3 Bohr model Quantum mechanical model Quantum Mechanics for Dummies: Hund's Rule "Spread out before you fill up" When filling sublevels other than s, electrons are placed in individual orbitals before they are paired up. Pull X e? a.k.a., "Smelly Bus Rule" e "Mercedes convertible" e e 3
4 "Aufbau" (To build up) Electrons fill lower energy levels first "Hund's Rule" When filling sublevels other than s, electrons are placed in individual orbitals before they are paired up. "Pauli Exclusion Principle" F. Hund An orbital can hold 0, 1, or 2 electrons only, and if there are two electrons in the orbital, they must have opposite (paired) spins. Therefore, no two electrons in the same atom can have the same set of four "Quantum numbers". W. Pauli Orbital Notation How many electrons? Use boxes to represent orbitals Use arrows to represent electrons Use opposite arrows to represent "opposite spin" electrons H: He: Be: Mg: P: "Aufbau" (Diagonal Rule) "Hund's Rule" "Pauli Exclusion Principle" H/W: p.101 #1 4, 5b sublevel 2e 6e s p d 10e f 14e orbitals Be: Mg: P: 4
5 Orbital Notation Write the orbital notation for: (1) nitrogen (2) neon (3) aluminum (4) scandium Remember: "Aufbau" (Diagonal Rule) "Hund's Rule" "Pauli Exclusion Principle" s p d f N: Ne: Al: Sc: Write the orbital notation for: (1) oxygen (2) sulfur (3) selenium (4) tellurium (5) What similarities do the orbital notations for the above elements share? Highest E level O: S: Se: Te: # in Highest Level 2/14/14 s p d f 5
6 (Valence) Write the orbital notation for: (1) oxygen S: (2) sulfur (3) selenium Se: (4) tellurium (5) What similarities do the orbital notations for the above elements share? Highest E level O: S: Se: Te: s p d f Te: # in Highest Level O: Write the orbital notation for: (1) sodium (2) chlorine Warm up! (3) Circle the electron(s) in the metal orbitals that will be lost. (4) Circle the opening(s) in the nonmetal orbitals where the electron(s) from the metal will go. (5) Draw arrows indicating which electron(s) go where. 6
7 Draw orbital notation for: unstable Valence shell = Energy Level #3 Na: stable Na + Valence shell = Now Energy Level #2 : 11 Cl Cl - : 17 unstable stable Na atom 1 valence electron Choose: Steal 7 to make 8, OR lose 1 to make 8 Which is easier to do? circle that is lost circle where goes draw arrow to show where comes from, {& where it goes Valence shell = Energy Level #3 Valence shell = Still Energy Level #3 Cl atom 7 valence electrons Choose: Steal 1 to make 8, OR lose 7 to make 8 Which is easier to do? 6. Draw orbital notation for Be +2 : 7. Draw orbital notation for F - : Be +2 : 8. Which is more stable: Be or Be +2? F or F -? Explain using max = stable "valence electrons" in your explanation. Full. Stable. Happy! = "isoelectronic" with He" = "isoelectronic" with Ne" Energy Levels: #1 7 Sublevels: s,p,d,f 7
8 1. i.* Students know the experimental basis for the development of the quantum theory of atomic structure and the historical importance of the Bohr model of the atom. 1. j.* Students know that spectral lines are the result of transitions of electrons between energy levels and that these lines correspond to photons with a frequency related to the energy spacing between levels by using Planck s relationship E = hv. 8
9 Electron Configuration summary notation of the location of faster than orbital notation differences: no boxes, no arrows, put in order of energy levels Be: Mg: Orbital Notation Orbital Notation Electron Configuration Electron Configuration 7 N 10 Ne: Sc: 3s 3p 4s 3d s p d f 9
10 Electron Configuration Warm up! Write the electron configuration for: (1) nitrogen (2) neon (3) aluminum (4) scandium Electron Configuration Write the electron configuration for: (1) nitrogen (2) neon (3) aluminum (4) scandium 10
11 s p d f Write the orbital notation for: (1) vanadium Write the electron configuration for: (2) germanium (3) silver Warm up! (4) gold (5) What similarities do the electron configurations for silver and gold share? s p d f 11
12 (1) Write the electron configuration for fluorine (2) Write the electron configuration for calcium (3) For the ionic solid calcium fluoride: a) Give the formula b) Describe how many electrons are transferred c) Describe where they come from (which energy level, sublevel, and orbital) d) Describe where the electrons go (which energy level, sublevel, and orbital) (4) Write the electron configuration for cobalt (5) How many electrons in the 3rd energy level of Co? (6) How many valence electrons in Co? (1) Write the electron configuration for fluorine (2) Write the electron configuration for calcium (3) For the ionic solid calcium fluoride: a) Give the formula b) Describe how many electrons are transferred c) Describe where they come from (which energy level, sublevel, and orbital) d) Describe where the electrons go (which energy level, sublevel, and orbital) (4) Write the electron configuration for cobalt (5) How many electrons in the 3rd energy level of Co? (6) How many valence electrons in Co? Warm up! 12
13 Write the electron configuration for: the noble gases (He - Rn) He: Ne: Ar: Kr: Xe: Rn: 2e With which noble gas is the magnesium ion "isoelectronic"? With which noble gas is the fluoride ion "isoelectronic"? Electron Configuration summary notation of the location of faster than orbital notation differences: no boxes, no arrows, put in order of energy levels Noble gas notation substitute the configuration for a noble gas! Find the nearest noble gas, "without going over" Plug in the noble gas in brackets Add only the electrons that are left Write the noble gas notation for potassium: electron config. noble gas notation Li: 2 2s 1 Li: [ ] Mg: 2 2s 2 2p 6 3s 2 Mg: [ ] 13
14 Write noble gas notations for: l) sodium 2) Y 3) Rat poison (arsenic) (1) Write the orbital notation for Si (2) Write the electron configuration for Ge (3) Write the electron configuration for tin (4) Write the noble gas notation for #1-3. Si: Si: Ge: Sn: 14
15 (1) Write the orbital notation for Ca (2) Write the electron configuration for Y (3) Write the electron configuration for rat poison (arsenic) (4) Write the noble gas notation for #1-3 Ca: [ ] Y: [ ] As: [ ] 15
16 Using JUST your periodic table as reference, write the electron configurations for: 1) cobalt 2) cadmium And the noble gas notations for: 3) iodine 4) barium s orbitals d orbitals p orbitals Ca Co Kr Ag Cd I Ba At Ne? Ar? Kr? Xe? Q: How many electrons in the highest energy level of: f orbitals 16
17 Procedures: A. Record observations of high, medium and low energy waves produced in the slinky demonstration. Compare the effect on both wavelength and frequency as the energy of the wave increases. Draw a labeled sketch to compare the waves. ENERGY: WAVELENGTH: FREQUENCY: HIGH MEDIUM LOW WAVELENGTH 17
18 Write the orbital notation for: (1) sodium (2) chlorine (3) circle the electrons in the metal that will be lost when NaCl(s) dissociates into NaCl(aq) (4) circle the openings in the nonmetal orbitals where the electrons from the metal will go (5) draw arrows indicating which electrons go where Cl is "isoelectronic" with which element? (same e config.) Na + is "isoelectronic" with which element? 18
19 Noble gas notation substitute the config. for a noble gas: Na: Sr: Ni: 11 find nearest noble gas (without going over) Write the electron configuration for: (1) titanium (2) Mo (3) barium (4) Write the noble gas notation for #1-3. s p d f 19
20 Write the orbital notation for: (1) sodium (2) chlorine (3) circle the electrons in the metal that will be lost when NaCl(s) dissociates into NaCl(aq) (4) circle the openings in the nonmetal orbitals where the electrons from the metal will go (5) draw arrows indicating which electrons go where Write the electron configuration for: (6) sodium (7) chlorine (8) Write the electron configuration for Na+ (9) Write the electron configuration for Cl- (10) Write the noble gas notation for Cl- "isoelectronic" Na + is "" with Cl is "" with Draw the orbital notation for: Li Cr Draw the electron configuration for: Fe Sb Draw the noble gas notation for: Nb Re 20
21 Attachments photoelectric_en.jar
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