UNIT 2 PART 1: ELECTRONS
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1 UNIT 2 PART 1: ELECTRONS
2 Electrons in an Atom Bohr s Model: Electrons resided in an allowed orbit. Quantum Mechanics Model: Probability of finding an electron in an area around the nucleus. This area around the nucleus is called an orbital.
3 Energy of Orbitals Orbitals can be described using a few important symbold. 1. n, principal quantum number relative size and energy of atomic orbitals. Bigger n = bigger orbital. The principal quantum number specifies the atom s major energy levels, which are called principal energy levels. The lowest principal energy level is assigned a n of 1.
4 Energy of Orbitals 2. Sublevels Principal energy levels contain energy sublevels. Each principal energy level contains a set number of sublevels. The sublevels are labeled as s, p, d or f. Each sublevel has a different shape. Each sublevel is related to a specific number of orbitals.
5 Energy of Orbitals 2. Sublevels Sublevels have different energies. s(lowest energy) < p < d < f (highest energy) Generally, electrons prefer to be in the lowest energy level, sublevel, and orbital as possible.
6 3. Orbitals In each sublevel, there are a certain number of orbitals. Orbitals are where electrons can be found. s sublevel: orbital p sublevel: orbitals d sublevel: orbitals f sublevel: orbitals Each orbital can hold only up to two electrons. Each orbital in the same subshell has the same energy.
7 Orbitals Electrons occupy a certain orbital at any given instant. When an electron occupies the lowest energy orbitals, the electron is said to be in its ground state. Electrons can be excited to a higher-energy orbital by absorption of a photon (= a packet of light) of appropriate energy.
8 Energy of Orbitals Summary: Fill out table Principal energy level Number of sublevels Sublevel name Number of orbitals in each sublevel
9 Energy of Orbitals Summary: Fill out table Principal energy level Number of sublevels Sublevel name Number of orbitals in each sublevel n=1 1 1s 1s: one orbital n=2 2 2s, 2p 2s: one orbital 2p: three orbitals n=3 3 3s, 3p, 3d 3s: one orbital 3p: three orbitals 3d: five orbitals n=4 4 4s, 4p, 4d, 4f 4s: one orbital 4p: three orbitals 4d: five orbitals 4f: seven orbitals
10 Shells and Subshells All orbitals in the same main energy level (ie. same n) is said to be in the same electron shell. Eg. The set of orbitals in the same main energy level (ie. same n) AND in the same sublevel (ie. the same shape of orbital) is called a subshell. Eg.
11 Shapes of Orbitals s orbital
12 Shapes of Orbitals p orbitals
13 Shapes of Orbitals d orbitals
14 Shapes of Orbitals f orbitals
15 Orbitals
16 Electron Configurations The arrangement of electrons around a nucleus for a particular atom is called the atom s electron configuration. There are three rules you must follow when you write an electron configuration for any atom. 1. Aufbau Principle 2. Pauli Exclusion Principle 3. Hund s Rule
17 Electron Configurations 1. Aufbau Principle: Electrons occupy the lowest energy orbital available first. 2. Pauli Exclusion Principle: Only two electrons can occupy any orbital at a time. 3. Hund s rule: Electrons occupy all the unoccupied orbitals of the same energy subshell first, before pairing up and filling the orbitals. Eg. Carbon, Nitrogen, Oxygen
18 Electron Configurations There are two ways you can write the electron configuration for any atom. 1. Orbital Diagram eg. 2. Electron Configuration Notation eg.
19 Electron Configurations Noble gas configurations/condensed electron configuration: Shortened form. Noble gas of the closest lower atomic number given in square brackets: Eg. Neon Sodium Magnesium Argon Potassium
20 Electron Configurations Textbook pg. 160 Q p.167 Q 77, 85
21 Valence Electrons Recall that electron shells are all orbitals of the same principal quantum number. Valence electrons, also called outer-shell electrons, are all electrons in the atom s outermost shell. Eg. Sulfur Silicon Fluorine
22 Valence Electrons Because valence electrons are involved in chemical reactions, electron-dot structures are drawn, which only show the atom s valence electrons. Dots representing valence electrons are drawn around the chemical symbol for the atom. Eg. Draw the dot structures for period 2. Textbook p.162 Q 26-28
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