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A typical electron configuration consists of numbers, letters, and superscripts with the following format: A number indicates the energy level (The number is called the principal quantum number.). A letter indicates the type of orbital; s, p, d, f. A superscript indicates the number of electrons in the orbital.
QUANTUM NUMBERS WORKSHEET. 1. State the four quantum numbers, then explain the possible values they may have and what they actually represent. n – Pricipal Quantum Number: represents the energy level the electron is in, linked to the periods of the periodic. Can be 1 to 7.
• The 2s2 means that the next 2 electrons go into the s orbital in the second energy level. • The 2p5 means that the next 5 electrons go into the p orbitals in the second energy level or second shell. Remember that 5 electrons cannot fit into one orbital. The p subshell actually contains 3 orbitals, which all together, could hold up to 6 ...
The electronic configuration of an atom provides information on which orbitals its electrons are in. The Periodic Table below shows how the orbitals occupied by the valence electrons. The number in front of the orbital (1s, 2s, 2p etc) gives the shell (the n quantum number). The letter (s, p, d etc) gives the subshell (the l quantum number).
The worksheets are available in the tutorials and form an integral part of the learning outcomes and experience for this unit. Model 1: Atomic Orbitals 1. s orbitals consist of a single lobe. p orbitals consist of two large lobes. d orbitals consist of four lobes. (The shape of 3 dz2 is a little different to that of the other 3 d orbitals. It ...
Orbitals and Quantum Numbers Practice Questions. 1. What are the shapes of s, p, and d orbitals respectively? s= spherical p = dumbbell d = cloverleaf. 2. How many 1s orbitals are there in an atom? 4p orbitals? 4d orbitals? 1s: 1 4p: 3 4d: 5. 3. What is the maximum number of orbitals with: n = 4 l = 1 3 (the 4p orbitals)
Worksheet #1: Atomic Spectra. 1. How did Bohr expand on Rutherford’s model of the atom? 2. Compare the energy of an electron in the ground state and an electron in the excited state. 3. When an electron falls from a higher energy level to a lower energy level, how is the energy released? 4.
