Download NAME PRACTICE: QUANTUM CONFIGURATIONS 1) Each of the

NAME ___________________________________
PRACTICE: QUANTUM CONFIGURATIONS
1) Each of the following electron configurations represents the valence electron configuration for an atom of an
element in the periodic table. For, each, what is the element, what is its group number, and what is its
period?
Valence Configuration
4s24p2
3d64s2
6s1
2s22p5
3d104s2
Period
*4
*4
*6
*2
*4
Group
*14
*8
*1
*7
*12
Name of Element
*germanium
*iron
*cesium
*fluorine
*zinc
___2) What is the energy of radiation that has a frequency of 9.00 x1011 Hz?
1) 1.66 x 10-5J
2) 5.97 x 10-22J
3) 4.99 x 10-27J
4) 5.00 x 10-22J
___3) Atoms of which element has the electron configuration of: 1s22s22p63s23p63d44s2
1) chromium
2) manganese
3) nickel
4) iron
___4) The energy of a photon of light is __________proportional to its frequency and __________
proportional to its wavelength.
1) directly, directly
2) inversely, inversely
3) inversely, directly
4) directly, inversely
___5) What is the frequency of light (s -1) that has a wavelength of 1.23 x 10-6 cm __________?
1) 3.00 x 108
2).2.44 x 1016
3) 4.10 x 10-17
4) 9.62 x 1012
___6) With what noble gas is an ion of S2- isoelectronic? __________________
___7) Which what species is an ion of S2- isoelectronic?
1) O2-
2) K1+
3) Br1-
4) Ca0
___8) A sodium ion differs from a sodium atom in that the sodium ion
1) has fewer electrons
2) is an isotope of sodium
3) exists only in aqueous solution
4) has a negative nuclear charge
___9) The maximum number of electrons that can occupy an orbital labeled dxy is
1) 1
2) 2
3) 3
4) 4
___10) Which species has the ground-state electron configuration of 1s22s22p63s23p63d10
1) Ni
2) Ni2+
3) Zn
4) Zn2+
___11) What is the valence electron configuration for the element in Period 5, Group 13?
1) 5s25p1
2) 5s25p3
3) 3s23p3
4) 3s23p5
___12) Helium, 42He, has two electrons in the 1s orbital. When it becomes ionized, forming He+,
1)
2)
3)
4)
its spectrum resembles that of the hydrogen spectrum
the remaining electron is easier to remove
the nuclear charge of has decreased by one
it has lost one atomic mass unit
___13) Which of these species is/are paramagnetic?
1)
2)
3)
4)
Fe2+, Zn0, Ti4+
Fe2+, only
Ti4+ and Fe2+, only
Zn0, only
Fe2+ and Zn0, only
___14) An atom of Fe has two 4s electrons and six 3d electrons. How many unpaired electrons would there be
in the Fe+2 ion?
1) 1
2) 2
3) 3
4) 4
___15) An argon atom is isoelectronic with
1) Cl
2) Ca
3) Ti4+
4) N3-
Use the following answers for questions 16-18
(1) F
(2) S
(3) Mg
(4) Ar
(5) Mn
___16) Forms monatomic ions with 2+ charge in solutions
___17) Forms a compound having the formula KXO4 (Could be quite tricky …you need to pull together a fair amount)
___18) Forms oxides that are common air pollutants and that yield acidic solution in water
Use these answers for questions 19-22.
(1) 1s2 2s22p5 3s23p5
(2) 1s2 2s22p6 3s23p6
(3) 1s2 2s22p62d10 3s23p6
(4) 1s2 2s22p6 3s23p63d5
(5) 1s2 2s22p6 3s23p63d3 4s2
___19) An impossible electronic configuration
___20) The ground-state configuration for the atoms of a transition element
___21) The ground-state configuration of a negative ion of a halogen
___22) The ground-state configuration of a common ion of an alkaline earth element
Use these answers for questions 23-25.
(1) Heisenberg uncertainty principle
(2) Pauli exclusion principle
(3) Hund's rule (principle of maximum multiplicity)
(4) Shielding effect
___23)
___24)
___25)
___26)
Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic
Helps to explain the lesser effect of coulombic forces of attraction on valence electrons
Explains that no two electrons can have the same 4 quantum numbers
Predicts that it is impossible to determine simultaneously the exact position and the exact velocity
of an electron
___27) Given: Ca, V, Co, Zn, As
Gaseous atoms of which of the elements above are paramagnetic?
1) Ca and As only
2) Zn and As only
3) Ca, V, and Co only
4) V, Co, and As only
5) V, Co, and Zn only
___28) Most members of the lanthanide series have the same number of:
1)
2)
3)
4)
5)
4s and 6s electrons but a different number of 4f electrons
4s and 6s electrons but a different number of 5s electrons
4f and 6s electrons but a different number of 5f electrons
4f and 5s electrons but a different number of 6s electrons
5s electrons but different numbers of 6s and 4f electrons
___29) How does a phosphorus atom differ from a phosphide ion?
I) The phosphide ion has more electrons
II) The phosphorus atom has more unpaired electrons
III) The phosphide ion has more kernel electrons
1) I only
2) I and II only
3) I and III only
4) II and III only
5) I, II and III
___30) The electron configuration of atoms of element X is show [Ar] 4s2 3d10. Which is the most likely
formula for the compound of this element, with oxygen?
1) XO
2) X2O
3) XO2
4) X2O3
5) X2O5
___31) N2 molecules absorb ultraviolet light but not visible light. I2 molecules absorb both visible and
ultraviolet light. Which of the following statements explains the observations?
1) More energy is required to make N2 molecules vibrate than is required to make I2 molecules vibrate
2) More energy is required to remove an electron from an I2 molecule than is required to remove an
electron from a N2 molecule
3) Visible light does not produce transitions between electronic energy levels in the N2 molecule, but
does produce transitions in the I2 molecule.
4) The molecular mass of I2 is greater than the molecular mass of N2
Questions 32 – 35 refer to atoms for which the occupied atomic orbitals are shown below:
2s ↑
1)
1s
2)
1s ↑↓ 2s ↑↓
3)
1s ↑↓
4)
1s ↑↓ 2s ↑↓
5)
[Ar] 4s ↑↓
2s ↑↓
2p
↑
↑
2p ↑↓
3d ↑↓
↑↓
↑
↑
↑↓
↑
↑
32) Represents an atom that is chemically unreactive
33) Represents an atom in an excited state
34) Represents an atom that has four valence electrons.
35) Represents an atom of a transition metal.
36) Passing an electrical charge through argon gas contained in a partially evacuated vessel yields which of
the following?
1) a continuous spectrum
2) a line spectrum
3) white light
4) no visible change
37) In the photoelectric effect, for an electron to be released from the surface of a clean metal, which one of the
following conditions must exist?
1) The metal must have a high temperature
2) The kinetic energy of photons striking the metal’s surface must equal that of the emitted electron.
3) The kinetic energy of photons striking the metal’s surface must be less than that of the
emitted electrons
4) The kinetic energy of photons striking the metal’s surface must be greater than or equal to that of
the emitted electrons plus the binding energy holding the electron in the metal.
38) Which of the following is NOT TRUE about the principal quantum number, n?
1)
2)
3)
4)
It is related to the spin of an electron.
It is related to the energy of an electron.
The larger the n value of an electron, the higher the energy.
The larger the n value of an electron, the larger the value of its Bohr radius
39) Which of the following describes a position around the nucleus, in which there is NO electron electron
density?
1)
2)
3)
4)
principal energy level
node
sublevel
orbital
Answers: 1) highlight and check
13) 1
14) 4
15) 3
26) 1
27) 4
28) 1
38) 1
39) 2
2) 2
3) 1
16) 3
29)
2
4) 4
17) 5
30) 1
5) 2
18) 2
31) 3
6) argon
19) 3
7) 2
20) 5
32) D
21) 2
33) A
8) 1
22) 2
34) C
9) 2
10) 4
23) 3
35) E
11) 2
24) 4
36) 2
12) 1
25) 2
37) 4