Download Atoms and Electrons Name: Practice H

Atoms and Electrons
Practice
Name: ______________________
1. The person who first postulated the concept of the nuclear
atom was
A) Bohr
C) Moseley
E) Avogadro
7. Which electron transition absorbs the most energy?
B) Dalton
D) Rutherford
2. Rutherford discussed experiments providing evidence that
atomic nuclei are
A)
B)
C)
D)
E)
positively charged and close together
negatively charged and close together
positively charged and far apart
negatively charged and far apart
neutral and close together
A)
B)
C)
D)
E)
3. The values for the emission spectrum of hydrogen was first
explained by
A)
B)
C)
D)
E)
8. Which of the following statements are true?
the Aufbau principle
Rutherford's empty space theory
Hund's Rule
the Heisenberg uncertainty principle
the Bohr model of the atom
I. The energy of electromagnetic radiation increases as its
frequency increases.
II. The energy of an atom is increased as it emits
electromagnetic radiation.
III. An excited atom returns to its ground state by absorbing
electromagnetic radiation.
IV. The frequency and wavelength of electromagnetic
radiation are inversely proportional.
V. An electron in the n = 3 state in the hydrogen atom can go
to the n = 1 state by emitting electromagnetic radiation at the
appropriate frequency.
4. According to the Bohr model of the atom, atoms can only
absorb energy at certain wavelengths because
A) Atoms of different elements contain different numbers of
protons
B) Electrons can only exist in certain energy levels
C) Most of the atom contains empty space
D) Atoms of different elements contain different numbers of
electrons
E) None of the above
5. What is the shell configuration of electrons for neutral atoms
of nickel, 28Ni, in the ground state?
A) 2–8–16–2
C) 2–8–8–10
E) 2–8–16–28
A) II, III, and V only
C) I, II, and III only
E) II, III, and V only
A)
B)
C)
D)
E)
B) 2–8–10–8
D) 2–18–8–0
pulls a proton out of the nucleus
pulls a neutron out of the nucleus
is changes from a particle to a wave
moves from a higher to a lower energy level
moves from a lower to a higher energy level
H-Chemistry
B) III and IV only
D) I, IV, and V only
9. The light from fluorescent lights, when analyzed in a
spectrometer, exhibit the same lines in the yellow, green and
blue spectral regions. This is evidence that
6. A single burst of light is released from an atom. A likely
explanation of this observation would be that an electron
A)
B)
C)
D)
E)
A
B
C
D
This diagram does not give enough information to tell.
fluorescent lights contain fluorine gas
air is present in all fluorescent lights
there are no gases present in fluorescent lights
the same element is present in all the fluorescent lights
different elements are present in each fluorescent light
10. Sunlight, when viewed through a prism or a diffraction
grating, shows all of the colors of visible light. This is an
example of a
A) bright line spectrum
C) infrared spectrum
E) ultraviolet spectrum
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B) continuous spectrum
D) visible spectrum
Dr. Powell
11. Movement of an electron from the 5 th to the 1st energy level
in an atom is:
A)
B)
C)
D)
E)
17. Which of the following explains why the electron
configuration below cannot exist?
exothermic and absorbs energy.
exothermic and evolves energy.
endothermic and absorbs energy.
endothermic and evolves energy.
neither exothermic nor endothermic.
A)
B)
C)
D)
E)
12. How many energy levels are shown in the electron
configuration?
1s2 2s22p6 3s23p63d10 4s24p3
A) 3
B) 4
C) 8
D) 18
E) 33
18. Which of the following could not represent the electron
configuration of a neutral atom in the ground state?
13. Which is the shape of a p–orbital?
A) spherical
C) clover leaf
E) pointed
A) 1s2 2s2 2p6 3s23p4
C) 1s2 2s2 2p6 3s33p4
E) 1s2 2s2 2p6 3s1
B) propeller
D) dumbbell
14. Which of the following scientists proposed the theory that it
is impossible to simultaneously determine the exact
momentum and position of particle
A) Niels Bohr
C) Werner Heisenberg
E) Josiah Gibbs
Hund's Rule
Pauli exclusion principle
Heisenberg uncertainty principle
Rutherford's empty space model
It can exist
B) 1s2 2s2 2p2
D) 1s2 2s2 2p6 3s2
19. The ground state electronic configuration for an atom of
neon, 2010Ne, is
A) 1s2 2s2
C) 1s2 2s2 2p6 3s1
E) ls2 2s4 2p4
B) Dmitri Mendeleev
D) Wolfgang Pauli
B) ls2 2s2 2p6
D) ls2 2s2 2p6 3s2 3p6
20. Consider the orbital diagram.
15. Which of the following explains why the electron
configuration below cannot exist?
The species that has this orbital configuration is
A)
B)
C)
D)
E)
Hund's rule
Pauli exclusion principle
Heisenberg uncertainty principle
Bohr's model of the atom
it can exist
A) 137N
C) 2713Al3+
E) None of the above
B)
D)
2713Al
3115P3-
21. Consider the orbital diagram
16. Which of the following explains why the electron
configuration below cannot exist?
The species that does not have this orbital
occupancy pattern is
A)
A)
B)
C)
D)
E)
Hund's rule
Pauli exclusion principle
Heisenberg uncertainty principle
Bohr's model of the atom
It can exist
H-Chemistry
4018Ar
B)
3416S
C)
3717Cl-
D)
3919K+
E)
3216S2–
22. Which electronic configuration is most characteristic of a
nonmetallic element?
A) 1s22s22p63s1
C) 1s22s22p63s2
E) 1s22s22p63s23p5
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B) 1s22s22p63p1
D) 1s22s22p63s23p1
Dr. Powell
23. The atomic number of an electrically neutral element with an
electron configuration 1s22s22p1 is
A) 1
B) 2
C) 3
D) 4
32. Which group is arranged correctly in order of increasing
energy for electrons in an element?
E) 5
A) 2s, 4p, 3d
C) 3p, 4s, 3d
E) 3p, 4s, 4d
24. In the excited state, a possible electron configuration of
aluminum, 13Al, is
A)
B)
C)
D)
E)
33. How many electrons are in each orbital of a completed
2p–sublevel?
1s 22s 22p 63s 3
1s 22s 22p 63s 23d 1
1s 22s 22p 63s 23p 1
1s 22s 22p 63s 23d 64s 24p 1
1s 22s 22p 63s 23p 2
A) 1
A) zinc
C) nickel
E) chlorine
1s22s22p63s23p63d74s2
B) 2
C) 3
D) 7
E) 9
A) 3
1s22s22p63s23p63d74s2
B) 7
C) 12
D) 15
E) 27
C) 12
D) 15
E) 27
A)
B)
C)
D)
E)
29. How many electron–pairs are there in neutral atoms of
cobalt, 27Co?
B) 11
C) 12
D) 13
A) [Ar]
C) [Ar] 3d84s3
E) [Ar] 3d94s2
H-Chemistry
B) n2
3d64s5
B) [Ar]
D) [Ar] 3d104s1
C) 2n
D) 6
E) 7
D) 2n2
mass
atomic mass
nuclear mass
number of valence electrons
physical properties
A) 8
B) 14
C) 10
D) 18
E) 2
39. How many valence electrons are in an arsenic atom with the
electron structure
[Ar] 3d104s24p3
A) 2
31. Which general expression is used to find the maximum
number of electrons which exist in a given shell?
A) n
C) 5
38. The number of valence shell electrons in a calcium atom,
20Ca, is
E) 27
30. What is the correct electron configuration for element 29, Cu,
in the ground state?
3d94s2
B) 4
37. The chemical properties of an atom depends primarily upon
the atom’s
1s22s22p63s23p6
1s22s22p63s23p63d104s04p1
1s22s22p93s23p63d104s24p2
1s22s22p63s23p63d104s24p3
1s22s22p63s23p4
A) 10
B) copper
D) chromium
a spherical shell containing electrons
a cloud which is always perfectly circular
a cloud with hundreds of electrons in it
the figure formed by the extremely rapid motion of
electrons
E) a probability function
28. Which is an ‘impossible’ configuration?
A)
B)
C)
D)
E)
E) 6
A)
B)
C)
D)
1s22s22p63s23p63d74s2
B) 7
D) 4
36. An electron orbital is best described as
27. How many orbitals are in neutral atoms of this element?
A) 4
C) 3
35. How many valence electrons does oxygen have?
26. How many subshells are shown in this configuration?
A) 4
B) 2
34. Which neutral element has the electron configuration
1s2 2s22p63s23p63d54s1?
25. How many unpaired electrons are in this atom?
A) 0
B) 3s, 3d, 3p
D) 2p, 2s, 1s
B) 3
C) 5
D) 10
E) 15
E) 2n – 2
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Dr. Powell
45. I. An atom of 23Na has 23 electrons
40. The electron dot symbol for nitrogen is.
BECAUSE
The element represented by an identical
electron dot arrangement is
A)
105B
B)
3115P
C)
3216S
D)
4020Ca
II. the number of protons equals the number of electrons in a
neutral atom.
E)
168O
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
41. What is the Lewis electron–dot diagram for neutral atoms of
element 12?
A)
B)
C)
D)
46. I. A sodium atom becomes a positive ion when it loses an
electron
E)
BECAUSE
42. In order for electrons to occupy the same orbital, they must
have
A)
B)
C)
D)
E)
II. electrons have a positive charge.
different magnetic quantum numbers
different azimuthal quantum numbers
the same spin
opposite spins
two electrons cannot occupy the same orbital
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
43. I. Isotopes of the same element have the same electron
configuration
47. I. An element with a mass number of 20 has 20 electrons
when it forms a 1+ ion
BECAUSE
BECAUSE
II. only their number of neutrons differ.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
44. I. The electron configuration of Cr is [Ar]3d54s1
BECAUSE
II. ions are formed to complete the outer valence shell.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
II. all sublevels in the 3rd principal energy level are half-filled
before the next principal energy level is filled.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
H-Chemistry
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Dr. Powell
48. I. An element with an atomic number of 19 has 20 electrons
when it forms a 1+ ion
50. I. Two electrons filling the same orbital in a given sublevel of
an atom must have opposite spins
BECAUSE
BECAUSE
II. positive ions are formed by losing electrons.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
49. I. Na+ is a positively charged ion
II. Hund’s Rule states that when electrons occupy orbitals of
equal energy, one electron occupies each orbital in a given
sublevel before there is any pairing.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
BECAUSE
II. it has less electrons than protons.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
H-Chemistry
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Dr. Powell