Presentation on theme: "Atomic Orbitals & Electron Configurations"— Presentation transcript:
1Atomic Orbitals & Electron Configurations Chemistry
2Atomic Orbitals & Electron Configurations 1. Identify the relationships among a hydrogen atom’s energy levels, sublevels, and atomic orbitals.2. Apply the Pauli exclusion principle, the aufbau principle, andHund’s rule to write electron configurations using orbitaldiagrams and electron configuration notation.3. Define valence electrons and draw electron-dot structuresrepresenting an atom’s valence electrons.For the Test:-be able to answer the objectives-know all vocabulary-be able to answer all review/practice questions-study your notes (anything can be asked from them)
3Atomic OrbitalsOrbitals do not have an exactly defined size, but are just unoccupied spaces available for electrons should the atom’s energy increase (or decrease)..As the energy level increases, the orbital becomes larger-n = 1, 2, … 7The shape of the orbital is represented by the sublevels in that orbital-s, p, d, & f
4Atomic Orbitals Each atomic orbital is designated by energy level and sublevel:1s represents ‘s’ orbital in the 1st energy leveleach suborbital holds 2 electrons, each withopposite spin~ s = 2~ p = 6, 3 suborbitals (2 per suborbital)~ d = 10, 5 suborbitals (2 per suborbital)~ f = 14, 7 suborbitals (2 per suborbital)
7Atomic Orbitals Review 1. Name the four orbital notations and give howmany suborbitals they have.2. What is an orbital?3. Carbon is located in the ____ orbital.4. What does the symbol 2p represent?5. What is special about the d and f orbitals whenrelated to the energy level?6. How many electrons are in each suborbital?Orbital?
8Electron Configurations electron configuration: arrangement of electrons in an atom.-electrons fill in so they have the lowest possibleenergy-there are three rules we follow1. Aufbau principle: each electron occupies the lowest energy orbital available-follows the aufbau diagram♦all orbitals in a sublevel are equal energy♦in multi-electron level, energy sublevels within aprinciple energy level have different energies
9♦in order of increasing energy, the sequence of energy sublevels within a principle energy level is s,p, d, and f♦orbitals related to energy sublevels within oneprinciple level can overlap orbitals related to energysublevels within another principle level; begins inn = 32. Pauli-exclusion principle: a maximum of 2electrons may occupy a single orbital, but only ifthey have opposite spins-arrows pointing up (↑)and down (↓) representelectron spins-paired electrons in same orbital: represented by ↑↓.
103. Hund’s rule: single electrons with the same spin must occupy each equal energy orbital beforeadditional electrons with opposite spins can occupythe same orbital-s sublevel: max 1 unpaired e-p sublevel: max 3 unpaired e-d sublevel: max 5 unpaired e-f sublevel: max 7 unpaired e-
11Electron Configurations Review 1 1. What does the Aufbau principle state?2. What does the Pauli-exclusion principle state?3. How do we represent electrons?4. What is the order the electrons fill the orbitals?5. What occurs at n=3 according to the Aufbau principle?
12Orbital Notation/Electron Configurations There are three ways to indicate electron configurations.1. orbital notation: an unoccupied orbital is represented by a line, ____, with the orbital’s principle quantum number and sublevel letter written underneath the line.___1s -an unpaired electron is shown as ____ and1spaired electrons as shown as ____ .
142. electron-configuration notation: eliminates the lines and arrows of orbital notation -the number of electrons in a sublevel is shown by adding a superscript to the sublevel designation;exs. H configuration is 1s1(1 electron on the 1s orbital)He is 1s2(2 electrons in the 1s orbital)-use the periodic table to write electron configurationnotation: s, p, d, and f block.-does not show orbital distributions of electrons
15Electron Configuration Notation Practice MgAlSiPSClArCrAsKr
16Noble Gas Notation3. noble-gas notation: shorthand notation using the noble gas elements-noble-gas configuration: outer main energy level fully occupied by eight electrons, except in He-ex: Na 1s22s22p63s1 is the electron-configurationnotation (long form)[Ne]3s1 is the noble gas notation (short form)because all orbitals are completely filledup to neon, who’s orbital notation is1s22s22p6-this notation is only used for elements above neon! (those in n = 3 and above)
18Exceptions Some transition metals do not follow this trend. -includes groups 6 and 11 (Cr and Cu groups)Cr [Ar]4s23d4 Cu [Ar]4s23d9Instead, we write it so that all s and d orbitals after the noble gas are half filled-increases stablity.Cr [Ar]4s13d5 Cu [Ar]4s13d10Practice with Exceptions:1. Mo2. Au
19Electron Configurations Review 2 1. According to Aufbau principle, does the 3d or 4s have more energy?2. How many electrons do each of the following element’s orbitals hold?a. Ne b. C3. List the Aufbau sequence of orbitals from 1s to 7p.4. Why do we write two electrons in the same orbital with opposite spins?5. How does noble gas notation shorten the process of writing electron configurations?6. Write the orbital notation, electron configuration and noble gas notation for:a. Sn b. Ag c. U7. Write electron configurations fora. Ni b. Pt
20More Electron Configuration Practice Draw orbital notations fora. In b. CeDraw electron configurations fora. Co b. RuDraw noble gas notation fora. W b. Po
21Valence ElectronsOnly certain electrons determine an element’s chemical properties-valence electrons: electron’s in the atom’s highest most energy level•sulfur has 16 electrons, but only 6 valence electronsValence electrons can be determined by writing electrons configurations:-S [Ne]3s23p4 6-Ga [Ar]4s23d104p1 3 (4th level highest)[Ar] 3d104s24p1
22Electron Dot Structures Chemists use valence electrons to show how atom’s are involved in bonding.-electron dot structure: consists of the element’ssymbol (which represents the nucleus and inner electrons) surrounded by dots (that represent thevalence electrons)•unpair the electrons first along the four sides of thesymbolS
23Oxidation NumbersWhen an atom bonds, it either gains or loses electrons, forming a charge on the atom-oxidation number: charge on an atom after bonding•metals lose to form a positive chargeCa+2 loses two electrons•nonmetals gain to form a negative chargeN gains three electronsLook at the electron dot structure to determine how many it will lose or gain.
24Valence Electrons Review 1. What are valence electrons?2. How many of magnesium’s electrons are valence electrons?3. What do we mean by oxidation number?4. Draw the electron dot structure for the following, then determine the oxidation number.a. C b. K c. Br