N 4 how many subshells

Download APP. About SnapSolve. Join Now. Question Chemistry Class Hint: A subshell is a group of orbitals. These are the collections of orbitals which share the same principal quantum number and angular momentum quantum number which is denoted by the letters s, p, d, f and so on.

The electrons in an atom are arranged in shells that surround the nucleus. Complete step by step answer:The angular momentum quantum number l, can have any integer value from to. This quantum number describes the shape or type of the orbital. Orbitals with the same principal quantum number and the same l value belong to the same subshell. The value of n determines the possible values for l. For any given shell, the number of subshells can be found by l.

The fourth shell has 4 subshells, i. The s subshell, which has 1 orbital with 2 electrons, the p subshell, which has 3 orbitals with 6 electrons, the d subshell, which has 5 orbitals with 10 electrons, and the f subshell, which has7 orbitals with 14 electrons.

For total there are 16 orbitals and 32 electrons. The s subshell is the lowest energy subshell and the f subshell is the highest energy subshellAnd according to Pauli's Exclusion principle no two electrons can have the same set of quantum numbers, that is no two electrons can be in the same state.

This exclusion limits the number of electrons in atomic shells and subshells. Hence, option A is correct. A thermodynamic state function is a quantity i used to determine heat changes ii whose value is independent of path iii used to determine pressure volume work iv whose value depends on temperature only. The equilibrium constant for a reaction is A sample of HI g is placed in flask at a pressure of 0.

At equilibrium the partial pressure of HI g is 0. What is K p for the given equilibrium? Q1 i Calculate the number of electrons which will together weigh one gram. Q2 i Calculate the total number of electrons present in one mole of methane. Q3 How many neutrons and protons are there in the following nuclei?

Q7 Calculate the wavelength, frequency and wave number of a light wave whose period is 2. Q8 What is the number of photons of light with a wavelength of pm that provide 1 J of energy? Q10 Electromagnetic radiation of wavelength nm is just sufficient to ionise the sodium atom. Calculate the ionisa Q11 A 25 watt bulb emits monochromatic yellow light of wavelength of 0.

Calculate the rate of emission of qua Q12 Electrons are emitted with zero velocity from a metal surface when it is exposed to radiation of wavelength Q13 What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy Compare your answer with the Q16 i The energy associated with the first orbit in the hydrogen atom is —2. Q17 Calculate the wave number for the longest wavelength transition in the Balmer series of atomic hydrogen.

Q18 What is the energy in joules, required to shift the electron of the hydrogen atom from the first Bohr orbit to th Calculate the energ Q20 Calculate the wavelength of an electron moving with a velocity of 2. Q21 The mass of an electron is 9. Q22 Which of the following are isoelectronic species i. Q24 What is the lowest value of n that allows g orbitals to exist? Q25 An electron is in one of the 3d orbitals. Give the possible values of n, l and ml for this electron Q26 An atom of an element contains 29 electrons and 35 neutrons.

Deduce i the number of protons and ii the elect Q27 Give the number of electrons in the species , H2 and Q29 Using s, p, d notations, describe the orbital with the following quantum numbers. Q30 Explain, giving reasons, which of the following sets of quantum numbers are not possible.

Q31 How many electrons in an atom may have the following quantum numbers? Q32 Show that the circumference of the Bohr orbit for the hydrogen atom is an integral multiple of the de Broglie wav Q34 Calculate the energy required for the process The ionization energy for the H atom in the ground state is Each shell must be full before the next starts to fill. There are 4 subshells, s, p, d, and f.

Each subshell can hold a different number of electrons. SubShell Electrons s 2 p 6 d 10 f The n number determines how many of the subshells make up the shell. For example, the 1st shell is made up of 1 subshell, s. It can therefore contain only 2 electrons.