Atomic Structure

Choose the highest energy involved when an electron makes a transition

• n = 4 to n = 3
  

• n = 2 to n = 1
  

• n = 4 to n = 2
  

• n = 3 to n = 1
  

Calculate the wavelength, ƴ, for the fourth line in Balmer series

• 432 nm

• 654 nm

• 410 nm

• 486 nm

The following statements are true, EXCEPT

• The energy of a photon is proportional to its wavelength

• A line spectrum is produced when light is emitted from an excited atom

• The region in which an electron is most likely to be found is called an orbital

• Light is composed of photons of discrete energy

Calculate energy required to excite an electron from n = 2 to n = 4

• $2.\ 05\ x\ 10^6\ J$

• $2.74\ x\ 10^6\ J$

• $4.09\ x\ 10^{-19}\ J$

• $5.45\ x\ 10^{-19}\ J$

The light emitted by a hydrogen atom with a wavelength of
 $434\ x\ 10^{-9}m,$  corresponds to a transition of its electron from

• n = 4 to n = 2
  

• n = 5 to n = 2

• n = 6 to n = 2

• n = 3 to n = 2

Which of the following represents an electron in 3p orbital?

• n = 3, l = 0, m = +1, s = +1/2

• n = 3, l = 2, m = +2, s = +1/2

• n = 3, l = 1, m = +1, s = +1/2

• n = 3, l = 0, m = 0 , s = +1/2

Electronic configuration of copper atom is  $1s^22s^22p^63s^23p^64s^13d^{10}$ .  Determine the number of electron in copper atom at its ground state if the azimuthal quantum number, l is 0

• 9

• 7

• 6

• 10

Maximum number of electron that can occupy 3d orbital is

• 2

• 6

• 8

• 10

The energy of the electron in a hydrogen atom is determined by ;

I. the principle quantum number

II. the magnetic quantum number

III. the electron spin quantum number

• I only

• I and II

• II and III

• I, II and III

Degenerate orbital have

I. the same value of the azimuthal quantum number, l

II. the same energy

III. the differences values of the s quantum number but the same set of quantum numbers, n, l and m

• I only

• I and II

• II and III

• I, II and III