The possible orbitals in an atom should be determined. Concept Introduction: The distribution of electrons in an atom is described by the use of quantum numbers used by the Bohr model one-dimensional model. The most important information that is the size of the atom is determined by the principal quantum number denoted by symbol n . Other quantum numbers are angular and magnetic quantum numbers which describes shape and orientation in the space of the orbitals of the atom. The forth quantum number is spin quantum number which is denoted by symbol s and determined the spin of the electron if it is clockwise or anticlockwise. The all four quantum numbers are explained in detail as follows: Principal quantum number (n) determines the size of the orbital. The orbital with principal quantum number 2 is larger than the value 1. This also determines the energy of the orbital, as the value of n increases the energy of the orbital increases as its distance from the nucleus increases. Angular quantum number (l) determined the shape of the orbital. For l = 0 , the shape of the orbital is sphere, for l = 1 , the shape of orbital is polar and that for l = 2 is cloverleaf. The rules for the allowed quantum numbers combinations are as follows: All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers. The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on. The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2. The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2 For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell. Here, for s orbital value of l = 0 , for p orbital it is l = 1 , for d orbital it is l = 2 and for f it is 3.

Question

Want to see the full answer?

Answer 1

Question

Chapter 5, Problem 5.91AQAP

Interpretation Introduction

Interpretation:

The possible orbitals in an atom should be determined.

Concept Introduction:

The distribution of electrons in an atom is described by the use of quantum numbers used by the Bohr model one-dimensional model. The most important information that is the size of the atom is determined by the principal quantum number denoted by symbol n . Other quantum numbers are angular and magnetic quantum numbers which describes shape and orientation in the space of the orbitals of the atom.

The forth quantum number is spin quantum number which is denoted by symbol s and determined the spin of the electron if it is clockwise or anticlockwise.

The all four quantum numbers are explained in detail as follows:

Principal quantum number (n) determines the size of the orbital. The orbital with principal quantum number 2 is larger than the value 1. This also determines the energy of the orbital, as the value of n increases the energy of the orbital increases as its distance from the nucleus increases.

Angular quantum number (l) determined the shape of the orbital. For l=0 , the shape of the orbital is sphere, for l=1 , the shape of orbital is polar and that for l=2 is cloverleaf.

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.
Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Arrange the solutions in order of increasing acidity. (Note that K (HF) = 6.8 x 10 and K (NH3) = 1.8 × 10-5) Rank solutions from least acidity to greatest acidity. To rank items as equivalent, overlap them. ▸ View Available Hint(s) Least acidity NH&F NaBr NaOH NH,Br NaCIO Reset Greatest acidity

1. Consider the following molecular-level diagrams of a titration. O-HA molecule -Aion °° о ° (a) о (b) (c) (d) a. Which diagram best illustrates the microscopic representation for the EQUIVALENCE POINT in a titration of a weak acid (HA) with sodium. hydroxide? (e)

Answers to the remaining 6 questions will be hand-drawn on paper and submitted as a single file upload below: Review of this week's reaction: H₂NCN (cyanamide) + CH3NHCH2COOH (sarcosine) + NaCl, NH4OH, H₂O ---> H₂NC(=NH)N(CH3)CH2COOH (creatine) Q7. Draw by hand the reaction of creatine synthesis listed above using line structures without showing the Cs and some of the Hs, but include the lone pairs of electrons wherever they apply. (4 pts) Q8. Considering the Zwitterion form of an amino acid, draw the Zwitterion form of Creatine. (2 pts) Q9. Explain with drawing why the C-N bond shown in creatine structure below can or cannot rotate. (3 pts) NH2(C=NH)-N(CH)CH2COOH This bond Q10. Draw two tautomers of creatine using line structures. (Note: this question is valid because problem Q9 is valid). (4 pts) Q11. Mechanism. After seeing and understanding the mechanism of creatine synthesis, students should be ready to understand the first half of one of the Grignard reactions presented in a past…