Structure 1.3.5—Each orbital has a defined energy state for a given electron configuration and chemical environment, and can hold two electrons of opposite spin. Sublevels contain a fixed number of orbitals, regions of space where there is a high probability of finding an electron. Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to deduce electron configurations for atoms and ions up to Z = 36.
Description
[N/A]Directly related questions
-
19M.1A.SL.TZ1.4:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.4:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.4:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.4:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ1.6:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ1.6:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.6:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.6:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.6:
What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?
A. [Ar]3d6
B. [Ar]4s23d4
C. [Ar]4s13d5
D. [Ar]4s24p4
-
19M.1A.SL.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ1.7:
Which describes an atom of bismuth, Bi (Z = 83)?
-
19M.1A.SL.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?
A. Highest energy levels occupied
B. Energy sub-levels occupied
C. Orbitals occupied
D. Valence electrons
-
19M.1A.SL.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?
A. Highest energy levels occupied
B. Energy sub-levels occupied
C. Orbitals occupied
D. Valence electrons
-
19M.1A.SL.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?
A. Highest energy levels occupied
B. Energy sub-levels occupied
C. Orbitals occupied
D. Valence electrons
-
19M.1A.SL.TZ2.7:
Which of the following would have the same numerical value for all elements in the same period?
A. Highest energy levels occupied
B. Energy sub-levels occupied
C. Orbitals occupied
D. Valence electrons
-
21M.2.SL.TZ1.1d(iii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.1d(iii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.d(iii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.1d(iii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.1d(iii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.d(iii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.1c(ii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.1c(ii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.c(ii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.1c(ii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.1c(ii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ1.c(ii):
State the full electron configuration of the sulfide ion.
-
21M.2.SL.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3+.
-
21M.2.SL.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3+.
-
21M.2.SL.TZ2.b(i):
State the condensed electron configurations for Cr and Cr3+.
-
21M.2.SL.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3+.
-
21M.2.SL.TZ2.2b(i):
State the condensed electron configurations for Cr and Cr3+.
-
21M.2.SL.TZ2.b(i):
State the condensed electron configurations for Cr and Cr3+.
- 21N.1A.SL.TZ0.6: How many p-orbitals are occupied in a phosphorus atom? A. 2 B. 3 C. 5 D. 6
- 21N.1A.SL.TZ0.6: How many p-orbitals are occupied in a phosphorus atom? A. 2 B. 3 C. 5 D. 6
- 21N.1A.SL.TZ0.6: How many p-orbitals are occupied in a phosphorus atom? A. 2 B. 3 C. 5 D. 6
- 21N.1A.SL.TZ0.6: How many p-orbitals are occupied in a phosphorus atom? A. 2 B. 3 C. 5 D. 6
-
21N.2.SL.TZ0.9b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.9b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.9b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.9b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.8b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.8b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.8b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.8b(ii):
State the electron configuration of copper.
-
21N.2.SL.TZ0.b(ii):
State the electron configuration of copper.
-
22M.1A.SL.TZ1.6:
What is the maximum number of electrons that can occupy a p-orbital?
A. 2
B. 3
C. 6
D. 8
-
22M.1A.SL.TZ1.6:
What is the maximum number of electrons that can occupy a p-orbital?
A. 2
B. 3
C. 6
D. 8
-
22M.1A.SL.TZ1.6:
What is the maximum number of electrons that can occupy a p-orbital?
A. 2
B. 3
C. 6
D. 8
-
22M.1A.SL.TZ1.6:
What is the maximum number of electrons that can occupy a p-orbital?
A. 2
B. 3
C. 6
D. 8
- 22M.2.SL.TZ1.6a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
- 22M.2.SL.TZ1.6a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
- 22M.2.SL.TZ1.a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
- 22M.2.SL.TZ1.6a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
- 22M.2.SL.TZ1.6a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
- 22M.2.SL.TZ1.a(i): Draw arrows in the boxes to represent the electron configuration of a nitrogen atom.
-
22M.2.SL.TZ2.5a(i):
State the full electronic configuration of Fe2+.
-
22M.2.SL.TZ2.5a(i):
State the full electronic configuration of Fe2+.
-
22M.2.SL.TZ2.a(i):
State the full electronic configuration of Fe2+.
-
22M.2.SL.TZ2.5a(i):
State the full electronic configuration of Fe2+.
-
22M.2.SL.TZ2.5a(i):
State the full electronic configuration of Fe2+.
-
22M.2.SL.TZ2.a(i):
State the full electronic configuration of Fe2+.
-
22M.2.SL.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
-
22M.2.SL.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
-
22M.2.SL.TZ1.e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
-
22M.2.SL.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
-
22M.2.SL.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
-
22M.2.SL.TZ1.e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.