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WorksheetsREVISION ATOMIC STRUCTURE
Total questions: 34
Worksheet time: 15mins
Ground state means that an electron is...
at its lowest possible potential energy
in the first shell of an atom
laying low for the weekend
removed from an atom
When an electron returns to ground state from an excited state, the atom will
emit energy
absorb energy
rotate
wiggle
Which electronic transition would result in ultraviolet region?
n=3 to n=2
n=4 to n=1
n=4 to n=3
n=6 to n=4
The principal quantum number, n, represents the
spin value
suborbital value
energy level
magnetic value
A transition of electron from a higher energy level to energy level of n = 5 formed a photon. Which of the following series belongs to this transition?
Balmer
Pfund
Brackett
Lyman
Paschen
The impossibility to know simultaneously the exact position and momentum of a particle is called the
de Broglie's Uncertainty Principle
Moseley's Uncertainty Principle
Heisenberg's Uncertainty Principle
Bohr's Uncertainty Principle
Ionisation energy is ___________.
maximum energy required to remove 1 electron from 1 mol of gaseous atoms.
minimum energy required to remove 1 mol of electrons from 1 mol of gaseous atoms/ions.
first ionisation energy for a mol of gaseous atoms.
second ionisation energy for 1 mol of gaseous ions.
Which equation show the relationship among wavelength, frequency, and speed of light/radiation?
ΔE =λhc
ΔE=hv
λ = vc
En=− RH (n21)
Which formula is used to calculate energy of an electron in a given energy state of the H atom?
ΔE =λhc
ΔE=hv
λ = vc
En=− RH (n21)
Which number of line spectrum formed when electron falls down from n=5 to n =3 in Paschen series?
3rd line
1st line
2nd line
4th line
The following are weaknesses of Bohr’s postulate EXCEPT
Unable to explain the extra lines formed in the hydrogen spectrum
Unable to explain the dual nature of electrons
Unable to calculate the energy at specific energy level
Unable to explain the line spectrum of atoms or ions that contain more than one electron
Which principle or rule state that an electron will occupies the lowest energy orbital that can receive it?
Hund’s rule
Pauli exclusion principle
Bohr model of the atom
Aufbau principle
Which principle or rule state that all orbitals of equal energy (degenerate orbitals) are occupied by one electron before any single orbital is occupied by a second electron?
Aufbau principle
Pauli exclusion principle
Hund’s rule
Core Notation
Which principle or rule state that no two electrons in the same atom can have the same four quantum numbers?
Aufbau principle
Pauli exclusion principle
Hund’s rule
Noble gas notation
What are the shapes of p orbitals ?
cloverleaf
spherical
dumbbell
complex
What is the shape of the s orbital?
dumb bell
spherical
cloverleaf
flat
What is the shape of the d orbital?
flat shape
spherical shape
dumb bell shape
cloverleaf shape
What does the 1 in "1s" stand for?
energy level
s orbitals
p orbitals
the number of electrons
How many electrons are in 1s2 2s2 2p4?
5
6
8
13
For each of the following sublevels, which is lowest in energy?
4s
3d
4p
5s
Maximum number of electrons that can be placed in 2s are ..
2
6
10
14
The maximum number of electrons that can be placed in 2p are
2
6
10
14
The maximum number of electrons that can be placed in n = 3 with ℓ = 2 are ..
2
6
10
14
Which of the following is the shape of 2px orbital?
Choose the shape dx2-y2 orbital.
Which element has anomalous electronic configuration?
Cr
Cl
C
Ca
4 electrons are added to 2p orbitals in order of..
Electrons are filled in orbitals according to the following order
1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p
1s, 2s, 2p, 3s, 4s, 3p, 3d, 4p
1s, 2s, 3s, 4s, 2p, 3p, 4p, 3d
Why the elements Cu and Cr have anomalous electronic configuration?
due to lack of available orbital to be occupied by electrons.
due to the fact that these elements are from period 3 and above.
due to stability of electronic configuration for the ions of these elements.
due to half-filled and fully-filled 3d orbital are more stable than partially-filled filled 3d orbital.
Which shape represented by angular momentum quantum number, ℓ = 0
Which orbital represented by angular momentum quantum number, ℓ = 2
s
p
d
f
Which of the following sets of quantum numbers is NOT allowed?
(n=1, ℓ= 0, m= 0, s= +½ )
(n=7, ℓ= 3, m= 0, s= −½ ),
(n=3, ℓ= 1, m= +2, s= +½ )
(n=4, ℓ= 3, m= +2, s= +½ )
The orientation of orbital in the space
around the nucleus is indicated by
Principal quantum number (n)
Angular momentum quantum number (ℓ)
Magnetic quantum number (m)
Spin quantum number (s)
State the orbitals corresponding to these sets of quantum numbers, (n=2, ℓ= 0, m= 0, s= +½ ), (n=3, ℓ= 2, m= 0, s= +½ ), (n=3, ℓ= 1, m= 0, s= +½ )
2p, 3s, 3p
2s, 3f, 3p
2s, 3d, 3p
2p, 3d, 3f
