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Chapter 4: Problem 32

The atomic number of an element is 35 . What is the total number of electrons present in all the p-orbitals of the ground state atom of that element? (a) 17 (b) 11 (c) 23 (d) 6

Short Answer

Expert verified
(a) 17

Step by step solution

01

Understand Atomic Number

The atomic number of an element tells us the number of protons present in an atom of that element. Since atoms are neutral, the number of electrons equals the number of protons. Thus, an element with an atomic number of 35 has 35 electrons.
02

Identify Electron Configuration Pattern

Electron configurations distribute electrons among orbitals. The pattern is 1s, 2s, 2p, 3s, 3p, 4s, 3d, and 4p. We fill from lower to higher energy orbitals.
03

Fill Electron Configuration

Fill the first few orbitals to account for all 35 electrons: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦�. Each numeral and letter represent orbitals, with superscripts indicating the number of electrons in each.
04

Count Electrons in P-Orbitals

Identify electrons in the p-orbitals: - 2p has 6 electrons - 3p has 6 electrons - 4p has 5 electrons Add these: 6 + 6 + 5 = 17 electrons in the p-orbitals.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Atomic Number
The atomic number is a fundamental concept to understand when exploring elements. It represents the number of protons found in the nucleus of an atom. For example, an atomic number of 35 indicates that the element contains 35 protons. This number is unique to each element and defines the identity of the element on the periodic table.

In a neutral atom, the number of electrons is equal to the number of protons. Thus, for an element with an atomic number 35, there are 35 electrons. These electrons are what define the electron configuration and determine the chemical properties of the element.

Knowing the atomic number is the first step in figuring out how the electrons are distributed across different orbitals in an atom.
P-Orbitals
Electrons are arranged in different energy levels and subshells within an atom, with p-orbitals being one type of subshell. P-orbitals can hold up to 6 electrons and exist in the second energy level and higher.

The electron configuration of an atom describes how these electrons are distributed among its orbitals. For a total atomic number of 35, electrons occupy all available lower energy orbitals first鈥攂efore filling the p-orbitals.
  • The 2p orbital contains 6 electrons.
  • The 3p orbital contains 6 electrons.
  • The 4p orbital contains 5 electrons.
Summing these gives a total of 17 electrons in p-orbitals. With these electrons, p-orbitals play a significant role in determining the chemical and physical properties of the element.
Ground State Atom
The ground state of an atom is its lowest energy state in which the electrons are in the most stable configuration. In this state, electrons fill the orbitals in order of increasing energy, following the Aufbau principle.

For the element with an atomic number of 35, the ground state configuration is found by filling up orbitals from the lowest energy level. This specific arrangement ensures that the atom is as stable as possible:
  • Electrons first fill the 1s, 2s, and 2p orbitals.
  • Next, electrons move to 3s and 3p, followed by 4s.
  • Subsequently, the 3d orbital is filled, then the 4p orbital.
In the ground state, all 35 electrons are arranged as: - 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦�.
This distribution of electrons in the ground state governs the chemical behavior and reactivity of the atom.

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Most popular questions from this chapter

In which of the following pairs are both the ions coloured in aqueous solution? (a) \(\mathrm{Sc}^{3+}, \mathrm{Co}^{2+}\) (b) \(\mathrm{Ni}^{2+}, \mathrm{Cu}^{+}\) (c) \(\mathrm{Ni}^{2+}, \mathrm{Ti}^{3+}\) (d) \(\mathrm{Sc}^{3+}, \mathrm{Ti}^{3+}\) (At. no. \(\mathrm{Sc}=21, \mathrm{Ti}=22, \mathrm{Ni}=28, \mathrm{Cu}=29, \mathrm{Co}=27\) )

The value of Planck constant is \(6.63 \times 10^{-34} \mathrm{Js}\). he velocity of light is \(3.0 \times 10^{8} \mathrm{~m} \mathrm{~s}^{-1} .\) which value is closest to the wavelength in nanometres of a quantum of light with frequency of \(8 \times 10^{15} \mathrm{~s}^{-1}\) ? (a) \(4 \times 10^{1}\) (b) \(3 \times 10^{7}\) (c) \(2 \times 10^{-25}\) (d) \(5 \times 10^{-18}\)

The electronic configuration of an element is \(1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2}\) \(2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}\). This represents (a) excited state (b) ground state (c) cationic form (d) anionic form

The quantum number 'm' of a free gaseous atom is associated with (a) the effective volume of the orbital (b) the shape of the orbital (c) the spatial orientation of the orbital (d) the energy of the orbital in the absence of a magnetic field

The energy of second Bohr orbit of the hydrogen atom is \(-328 \mathrm{~kJ} \mathrm{~mol}^{-1}\), hence the energy of fourth bohr orbit would be (a) \(-164 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (b) \(-41 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (c) \(-82 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (d) \(-1312 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
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