Relative to electrons and electron states, what does each of the four quantum nu
ID: 476758 • Letter: R
Question
Relative to electrons and electron states, what does each of the four quantum numbers specify? Briefly cite the main differences between ionic, covalent, and metallic bonding. State the Pauli exclusion principle. With regard to electron configuration, what do all the elements in Group VIIA of the periodic table have in common? Give the electron configurations for the following: Fe and Fe^2+ Al and Al^3+, Cu and Cu^+, Ba and Ba^2+, Br and Br^-, O and O^2-. Determine whether each of the electron configurations given below is an inert gas. a halogen, an alkali metal, an alkaline earth metal, or a transition metal (without consulting related figures and tables). Justify your choices. 1s^22s^22p^63s^23p^63d^74s^2 1s^22s^22p^63s^23p^6 1s^22s^22p^5 1s^22s^22p^63s^2 1s^2s^22p^63s^23p^63d^24s^2 1s^22s^22p^43s^23p^64s^1Explanation / Answer
Quantum Number Name Waht it tells about electron Possible Values
n Principal Energy level or shell number 1, 2, 3, 4......
l Azimuthal It tells about the orbital type. 0 to (n-1)
0 for s orbital
1 for p orbital
2 for d orbital
3 for f orbital
m Magnetic Orbital sub-type -l to +l
s Spin Electron spin -1/2 or +1/2
Answer 2(a) Colvalent bond is formed when one or more elctron pair are shared between two atoms.
Ionic bonds are formed when one or more electroms are completely removed / accepted by atoms forming positive and negative ions completely.
Metallic bond are formed due to vander waals forces of attraction.
Answer 2 (b) : Pauli exclusion principal states that two electrons in an atom can not have all four quantum numbers same. This means that two electrons occuping same orbital must have opposite spins.
Answer (3) : Thier oute shell electronic configuration that is ns^2 np^5.
Problem (1) : Electronic configuration of Fe : [Ar] 3d6 4s2
Electronic configuration of Fe2+ : [Ar] 3d6
Electronic configuration of Al : [Ne] 3s2 3p2
Electronic configuration of Al3+ : [Ne]
Electronic configuration of Cu : [Ar] 3d10 4s1
Electronic configuration of Cu+ : [Ar] 3d10
Electronic configuration of Ba : [Xe 6s2
Electronic configuration of Ba2+ : [Xe]
Electronic configuration of Br : [Ar] 3d104s24p5
Electronic configuration of Br- : [Ar] 3d104s24p6
Electronic configuration of O: [He] 2s2 2p4
Electronic configuration of O: [He] 2s2 2p6
Problem (2) :
(a): Transition metal ( partially filled d orbitals)
(b): Inert gas ( completely filled s and p orbitals)
(c): Halogen ( ns2 np5 configuration)
(d): Alkaline earth metal ( ns2 configuration)
(e): Transition metal ( partially filled d orbitals)
(f): Alkaline metal ( ns1 configuration)