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Online Study Guide - Chem 1 - Electrons



Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 
 
Use the following figure to answer the questions below.
electrons_files/i0020000.jpg
 

 1. 

According to Bohr’s atomic model, which letter(s) in the figure represents a place where an electron cannot be?
a.
A
c.
A and D
b.
B, C and E
d.
D
 

 2. 

What can you conclude from the figure below?

  
electrons_files/i0040000.jpgelectrons_files/i0040001.jpgelectrons_files/i0040002.jpg
2p
 
electrons_files/i0040003.jpg
2s
 
electrons_files/i0040004.jpg
1s
  
a.
Hund’s rule has been violated.
b.
The Pauli exclusion principle has been violated.
c.
The Aufbau principle has been violated.
d.
This is a valid orbital diagram.
 

 3. 

What can you conclude from the figure below?

  
electrons_files/i0050000.jpgelectrons_files/i0050001.jpgelectrons_files/i0050002.jpgelectrons_files/i0050003.jpg
2p
 
electrons_files/i0050004.jpg
2s
 
electrons_files/i0050005.jpg
1s
  
a.
Hund’s rule has been violated.
b.
The Pauli exclusion principle has been violated.
c.
The Aufbau principle has been violated.
d.
This is a valid orbital diagram.
 

 4. 

Which of the following best describes the Heisenberg uncertainty principle?
a.
Light behaves like a particle and like a wave.
b.
The shorter the wavelength, the higher the frequency.
c.
It is impossible to know both the velocity and the position of a particle at the same time.
d.
You can measure an object without disturbing it.
 
 
Choose the letter of the choice that best completes the statement or answers the question. Use the periodic table in your textbook.
 

 5. 

Elements in the same group have the same ____.
a.
atomic radius.
c.
nuclear charge.
b.
energy level of outer electrons.
d.
number of valence electrons.
 

 6. 

Identify the period and group of the element that has the electron configuration [Ne]3s23p3.
a.
period 2, group 2A
c.
period 3, group 3A
b.
period 3, group 1A
d.
period 3, group 5A
 

 7. 

What is the electron configuration of the element in group 4A and period 4 of the periodic table?
a.
electrons_files/i0100000.jpg
c.
electrons_files/i0100001.jpg
b.
electrons_files/i0100002.jpg
d.
electrons_files/i0100003.jpg
 

 8. 

What is the trend in atomic radii as you move from left-to-right across a period?
a.
generally decreases
c.
remains the same
b.
generally increases
d.
varies randomly
 

 9. 

In which of the following pair is the second particle listed larger than the first?
a.
K, Ga
c.
Br, Br-
b.
Pb, C
d.
Li, Li+
 

 10. 

How many electrons does an atom generally need in its outer level to be the most stable?
a.
4
c.
10
b.
8
d.
12
 

 11. 

Elements in the same group have similar chemical properties because
a.
their atoms are about the same size.
b.
they have a similar atomic mass.
c.
they have the same number of valence elections.
d.
they have a diagonal relationship.
 

 12. 

The final electron in inner transition metals enters the
a.
p sublevel.
c.
d sublevel.
b.
s sublevel.
d.
f sublevel.
 

 13. 

The electrons in an atom’s outermost orbitals are called _____.
a.
electron dots.
c.
valence electrons.
b.
quantum electrons.
d.
noble-gas electrons.
 

 14. 

In an electron-dot structure, the element’s symbol represents the _____.
a.
nucleus of the noble gas closest to the atom in the periodic table.
b.
atom’s nucleus and inner-level electrons.
c.
atom’s valence electrons.
d.
electrons of the noble gas closest to the atom in the periodic table.
 

 15. 

How many valence electrons does a chlorine atom have if its electron configuration
is [Ne]3s23p5?
a.
3
c.
5
b.
21
d.
7
 

 16. 

Given boron’s electron configuration of [He]2s22p1, which of the following represents its electron-dot structure?
a.
electrons_files/i0190000.jpg
c.
electrons_files/i0190001.jpg
b.
electrons_files/i0190002.jpg
d.
electrons_files/i0190003.jpg
 

 17. 

Given beryllium’s electron configuration of 1s22s2, which of the following represents its electron-dot structure?
a.
electrons_files/i0200000.jpg
c.
electrons_files/i0200001.jpg
b.
electrons_files/i0200002.jpg
d.
electrons_files/i0200003.jpg
 

 18. 

Which electrons are represented by the dots in an electron-dot structure?
a.
valence electrons
c.
only s electrons
b.
inner-level electrons
d.
both a and c
 

 19. 

Which diagram best represents the group and period trends in atomic radii in the periodic table?
a.
electrons_files/i0220000.jpg
c.
electrons_files/i0220001.jpg
b.
electrons_files/i0220002.jpg
d.
electrons_files/i0220003.jpg
 

 20. 

The general trend in the radius of an atom moving down a group is partially accounted for by the_____.
a.
decrease in the mass of the nucleus.
b.
fewer number of filled orbitals.
c.
increase in the charge of the nucleus.
d.
shielding of the outer electrons by inner electrons.
 

 21. 

An atom becomes negatively charged by _____.
a.
gaining an electron.
c.
losing an electron.
b.
gaining a proton.
d.
losing a neutron.
 

 22. 

Which diagram best represents the relationship between the diameter of a sodium atom and the diameter of a positive sodium ion?
a.
electrons_files/i0250000.jpg
c.
electrons_files/i0250001.jpg
b.
electrons_files/i0250002.jpg
 

 23. 

How many valence electrons are present in silicon?
a.
One
c.
Four
b.
Two
d.
Six
 

 24. 

Which of the following elements is a metal?
a.
Boron
c.
Magnesium
b.
Nitrogen
d.
Carbon
 

 25. 

Which of the following is an alkaline earth metal?
a.
Sodium
c.
Iron
b.
Potassium
d.
Beryllium
 

 26. 

Which of the following groups consists of reactive p-block elements?
a.
Group 1A
c.
Group 8A
b.
Group 2A
d.
Group 3A
 

 27. 

Where does the final electron enter in an inner transition metal?
a.
s sublevel
c.
p sublevel
b.
d sublevel
d.
f sublevel
 

 28. 

At what sublevel does the final electron enter a transition metal?
a.
s sublevel
c.
d sublevel
b.
p sublevel
d.
f sublevel
 

Matching
 
 
Match the terms below with their correct definitions.
a.
alkali metals
h.
noble gases
b.
alkaline earth metals
i.
octet rule
c.
electronegativity
j.
periodic law
d.
halogens
k.
representative elements
e.
period
l.
transition elements
f.
ion
m.
group
g.
ionization energy
 

 29. 

Statement that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties
 

 30. 

Group A elements
 

 31. 

Group B elements
 

 32. 

Group 1A elements (except for hydrogen)
 

 33. 

Group 2A elements
 

 34. 

A column in the periodic table
 

 35. 

A row in the periodic table
 

 36. 

Group 7A elements
 

 37. 

Group 8A elements
 

 38. 

Atom or bonded group of atoms that has a positive or negative charge
 

 39. 

Energy required to remove an electron from a gaseous atom
 

 40. 

Statement that atoms tend to gain, lose, or share electrons to acquire a full set of eight valence electrons
 

 41. 

Indication of an atom’s ability to attract electrons in a chemical bond
 
 
Match the terms below with the correct definitions.
a.
Heisenberg uncertainty principle
c.
quantum mechanical model of the atom
b.
Schrödinger wave equation
d.
atomic orbital
 

 42. 

The modern model of the atom that treats electrons as waves
 

 43. 

States that it is impossible to know both the velocity and the position of a particle at the same time
 

 44. 

A three-dimensional region around the nucleus representing the probability of finding an electron
 

 45. 

Originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom
 
 
Match the terms below with their correct definitions.
a.
metals
d.
representative elements
b.
group
e.
transition elements
c.
period
 

 46. 

A column on the periodic table
 

 47. 

A row on the periodic table
 

 48. 

Group A elements
 

 49. 

Elements that are shiny and conduct electricity
 

 50. 

Group B elements
 



 
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